{"id":1353,"date":"2018-04-11T22:51:30","date_gmt":"2018-04-12T02:51:30","guid":{"rendered":"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/chapter\/2-7-chemical-nomenclature\/"},"modified":"2019-06-11T17:50:45","modified_gmt":"2019-06-11T21:50:45","slug":"2-7-chemical-nomenclature","status":"publish","type":"chapter","link":"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/chapter\/2-7-chemical-nomenclature\/","title":{"raw":"4.3 Nomenclature of Simple Ionic and Molecular Compounds","rendered":"4.3 Nomenclature of Simple Ionic and Molecular Compounds"},"content":{"raw":"<div class=\"bcc-box bcc-highlight\">\r\n<h3>Learning Objectives<\/h3>\r\nBy the end of this module, you will be able to:\r\n<ul>\r\n \t<li>Derive names for common types of inorganic compounds and simple molecular compounds using a systematic approach<\/li>\r\n<\/ul>\r\n<\/div>\r\n<p id=\"fs-idp268117168\"><strong>Nomenclature<\/strong>, a collection of rules for naming things, is important in science and in many other situations. This module describes an approach that is used to name simple ionic and molecular compounds, such as NaCl, CaCO<sub>3<\/sub>, and N<sub>2<\/sub>O<sub>4<\/sub>. The simplest of these are <strong>binary compounds<\/strong>, those containing only two elements, but we will also consider how to name ionic compounds containing polyatomic ions, and one specific, very important class of compounds known as <strong class=\"no-emphasis\">acids<\/strong>\u00a0- subsequent chapters in this text will focus on these compounds in great detail. We will limit our attention here to inorganic compounds, compounds that are composed principally of elements other than carbon, and will follow the nomenclature guidelines proposed by IUPAC. The rules for organic compounds, in which carbon is the principle element, will be treated in a later chapter on organic chemistry.<\/p>\r\n\r\n<section id=\"fs-idp268266480\">\r\n<h2>Nomenclature of Ionic Compounds<\/h2>\r\n<p id=\"fs-idp268131792\">To name an inorganic compound, we need to consider the answers to several questions. First, is the compound ionic or molecular? If the compound is ionic, does the metal form ions of only one type (fixed charge) or more than one type (variable charge)? Are the ions monatomic or polyatomic? If the compound is molecular, does it contain hydrogen? If so, does it also contain oxygen? From the answers we derive, we place the compound in an appropriate category and then name it accordingly.<\/p>\r\n\r\n<section id=\"fs-idm335792\">\r\n<h2>Compounds Containing Only Monatomic Ions<\/h2>\r\n<p id=\"fs-idp279143120\">The name of a binary compound containing monatomic ions consists of the name of the cation (the name of the metal) followed by the name of the anion (the name of the nonmetallic element with its ending replaced by the suffix \u2013<em>ide<\/em>). Some examples are given in <a class=\"autogenerated-content\" href=\"#fs-idp282234816\">Table 1<\/a>.<\/p>\r\n\r\n<table id=\"fs-idp282234816\" summary=\"The examples of ionic compounds shown in this table are N a C l sodium chloride, K B r potassium bromide, C a I subscript 2 calcium iodide, C s F cesium fluoride, L i C l lithium chloride, N a subscript 2 O sodium oxide, C d S cadmium sulfide, M g subscript 3 N subscript 2 magnesium nitride, C a subscript 3 P subscript 2 calcium phosphide, and A l subscript 4 C subscript 3 aluminum carbide.\">\r\n<tbody>\r\n<tr>\r\n<td>NaCl, sodium chloride<\/td>\r\n<td>Na<sub>2<\/sub>O, sodium oxide<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>KBr, potassium bromide<\/td>\r\n<td>CdS, cadmium sulfide<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>CaI<sub>2<\/sub>, calcium iodide<\/td>\r\n<td>Mg<sub>3<\/sub>N<sub>2<\/sub>, magnesium nitride<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>CsF, cesium fluoride<\/td>\r\n<td>Ca<sub>3<\/sub>P<sub>2<\/sub>, calcium phosphide<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>LiCl, lithium chloride<\/td>\r\n<td>Al<sub>4<\/sub>C<sub>3<\/sub>, aluminum carbide<\/td>\r\n<\/tr>\r\n<tr>\r\n<td colspan=\"2\"><strong>Table 1.<\/strong> Names of Some Ionic Compounds<\/td>\r\n<\/tr>\r\n<\/tbody>\r\n<\/table>\r\n<\/section><section id=\"fs-idp279293712\">\r\n<h2>Compounds Containing Polyatomic Ions<\/h2>\r\n<p id=\"fs-idp282236928\">Compounds containing polyatomic ions are named similarly to those containing only monatomic ions, except there is no need to change to an \u2013<em>ide<\/em> ending, since the suffix is already present in the name of the anion. Examples are shown in <a class=\"autogenerated-content\" href=\"#fs-idp279316112\">Table 2<\/a>. \u00a0See <a class=\"autogenerated-content\" href=\"https:\/\/opentextbc.ca\/chemistry\/chapter\/2-6-molecular-and-ionic-compounds\/#CNX_Chem_02_06_IonCharges\" target=\"_blank\" rel=\"noopener\">Table 1 in Chapter 4.2 Ionic and Molecular Compounds<\/a>\u00a0for the list of common polyatomic ions.<\/p>\r\n\r\n<table id=\"fs-idp279316112\" class=\"span-all\" summary=\"The examples of polyatomic ionic compounds shown in this table are K C subscript 2 H subscript 3 O subscript 2 potassium acetate, N a H C O subscript 3 sodium bicarbonate, A l subscript 2 ( C O subscript 3 ) subscript 3 aluminum carbonate, (N H subscript 4) CL, ammonium chloride, C a S O subscript 4 calcium sulfate, and M g subscript 3 ( P O subscript 4 ) subscript 2 magnesium phosphate.\">\r\n<tbody>\r\n<tr>\r\n<td>KC<sub>2<\/sub>H<sub>3<\/sub>O<sub>2<\/sub>, potassium acetate<\/td>\r\n<td>(NH<sub>4<\/sub>)Cl, ammonium chloride<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>NaHCO<sub>3<\/sub>, sodium bicarbonate<\/td>\r\n<td>CaSO<sub>4<\/sub>, calcium sulfate<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Al<sub>2<\/sub>(CO<sub>3<\/sub>)<sub>3<\/sub>, aluminum carbonate<\/td>\r\n<td>Mg<sub>3<\/sub>(PO<sub>4<\/sub>)<sub>2<\/sub>, magnesium phosphate<\/td>\r\n<\/tr>\r\n<tr>\r\n<td colspan=\"3\"><strong>Table 2.<\/strong> Names of Some Polyatomic Ionic Compounds<\/td>\r\n<\/tr>\r\n<\/tbody>\r\n<\/table>\r\n<\/section><\/section>\r\n<div>\r\n<div class=\"textbox shaded\">\r\n<h3 class=\"title\">Example 1<\/h3>\r\n<h3 class=\"title\"><span style=\"font-family: Tinos, Georgia, serif;font-size: 1em;font-weight: normal\">Name the following ionic compounds:<\/span><\/h3>\r\n<h3 class=\"title\"><span lang=\"ES-MX\" style=\"font-family: Tinos, Georgia, serif;font-size: 1em;font-weight: normal\">a)\u00a0 NaCl\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 b)\u00a0AlBr<sub>3<\/sub>\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 c)\u00a0 BaH<sub>2<\/sub><\/span><\/h3>\r\n<p class=\"Solution\"><strong>Solution\u00a0\u00a0 <\/strong><\/p>\r\n<p class=\"Indentpoints\">a)<span>\u00a0 <\/span>Identify the cation and anion.\r\nNa is a Group 1 metal, and thus it forms the cation Na<sup>+<\/sup>, called \u201csodium\u201d ion.\r\nCl is a nonmetal, and forms the anion Cl<sup>-<\/sup>, chloride.<span>\u00a0 <\/span>Thus, NaCl = sodium chloride.<\/p>\r\n<p class=\"Indentpoints\">b)<span>\u00a0 <\/span>AlBr<sub>3\u00a0<\/sub>consists of aluminum and bromine; we call it aluminum bromide.<\/p>\r\n<p class=\"Indentpoints\">c)<span>\u00a0 <\/span>BaH<sub>2<\/sub>is called barium hydride.<\/p>\r\n&nbsp;\r\n<p class=\"SelfTest\"><em><strong>Test Yourself<\/strong><\/em><\/p>\r\n<p class=\"Indent\">Name the following ionic compounds:<\/p>\r\n<p class=\"Indent\"><span>\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span>a)<span>\u00a0 <\/span>Al<sub>2<\/sub>S<sub>3<\/sub><span>\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span>b)<span>\u00a0<\/span>ZnS<span>\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span>c)<span>\u00a0 <\/span>MgI<sub>2<\/sub><\/p>\r\n&nbsp;\r\n<p class=\"Answers\"><span lang=\"PT-BR\"><em><strong>Answers<\/strong><\/em><\/span><\/p>\r\n<p class=\"Answers\"><span lang=\"PT-BR\">a) aluminum sulfide \u00a0 \u00a0 \u00a0 \u00a0\u00a0b) zinc sulfide \u00a0 \u00a0 \u00a0 \u00a0\u00a0c) magnesium iodide<\/span><\/p>\r\n\r\n<\/div>\r\n<\/div>\r\n<section id=\"fs-idp268266480\"><section id=\"fs-idp282353488\">\r\n<h2>Compounds Containing a Metal Ion with a Variable Charge<\/h2>\r\n<p id=\"fs-idp282354128\">Most of the transition metals can form two or more cations with different charges. Compounds of these metals with nonmetals are named with the same method as compounds in the first category, except the charge of the metal ion is specified by a Roman numeral in parentheses after the name of the metal. The charge of the metal ion is determined from the formula of the compound and the charge of the anion. For example, consider binary ionic compounds of iron and chlorine. Iron typically exhibits a charge of either 2+ or 3+ (see <a class=\"autogenerated-content\" href=\"https:\/\/opentextbc.ca\/chemistry\/chapter\/2-6-molecular-and-ionic-compounds\/#CNX_Chem_02_06_IonCharges\" target=\"_blank\" rel=\"noopener\">Figure 2 in Chapter 4.2 Ionic and Molecular Compounds<\/a>), and the two corresponding compound formulas are FeCl<sub>2<\/sub> and FeCl<sub>3<\/sub>. The simplest name, \u201ciron chloride,\u201d will, in this case, be ambiguous, as it does not distinguish between these two compounds. In cases like this, the charge of the metal ion is included as a Roman numeral in parentheses immediately following the metal name. These two compounds are then unambiguously named iron(II) chloride and iron(III) chloride, respectively. Other examples are provided in <a class=\"autogenerated-content\" href=\"#fs-idp282283328\">Table 4<\/a>.<\/p>\r\n\r\n<table id=\"fs-idp282283328\" class=\"span-all\" summary=\"The transition metal ionic compound examples included in this table are F e C L subscript 3 or iron three chloride, H g subscript 2 O or mercury one oxide, H g O or mercury two oxide, and C u subscript 3 ( P O subscript 4 ) subscript 2 or copper two phosphate.\">\r\n<thead>\r\n<tr>\r\n<th>Transition Metal Ionic Compound<\/th>\r\n<th>Name<\/th>\r\n<\/tr>\r\n<\/thead>\r\n<tbody>\r\n<tr>\r\n<td>FeCl<sub>3<\/sub><\/td>\r\n<td>iron(III) chloride<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Hg<sub>2<\/sub>O<\/td>\r\n<td>mercury(I) oxide<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>HgO<\/td>\r\n<td>mercury(II) oxide<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Cu<sub>3<\/sub>(PO<sub>4<\/sub>)<sub>2<\/sub><\/td>\r\n<td>copper(II) phosphate<\/td>\r\n<\/tr>\r\n<tr>\r\n<td colspan=\"2\"><strong>Table 4.<\/strong> Names of Some Transition Metal Ionic Compounds<\/td>\r\n<\/tr>\r\n<\/tbody>\r\n<\/table>\r\n<p id=\"fs-idp268391888\">An old naming convention used the suffixes \u2013<em>ic<\/em> and \u2013<em>ous<\/em> to designate metals with higher and lower charges, respectively: Iron(III) chloride, FeCl<sub>3<\/sub>, can be called called ferric chloride, and iron(II) chloride, FeCl<sub>2<\/sub>, is also known as ferrous chloride. \u00a0This older naming convention remains in use by some segments of industry. For example, you may see the words <em>stannous fluoride<\/em> on a tube of toothpaste. This represents the formula SnF<sub>2<\/sub>, which is also named tin(II) fluoride following the more current convention. The other fluoride of tin is SnF<sub>4<\/sub>, is now named tin(IV) fluoride but is still often referred to as stannic fluoride. \u00a0Knowing both convention remains important.<\/p>\r\n\r\n<table id=\"fs-idp268340336\" class=\"span-all\" style=\"height: 240px\" summary=\"This table has three columns labeled \u201cformula\u201d, \u201canion name\u201d, and \u201cacid name\u201d. H C subscript 2 H subscript 3 O subscript 2 is named acetate or acetic acid. H N O subscript 3 is named nitrate or nitric acid. H N O subscript 2 is named nitrite or nitrous acid, H C l O subscript 4 is named perchlorate or perchloric acid. H subscript 2 C O subscript 3 is named carbonate or carbonic acid. H subscript 2 S O subscript 4 is named sulfate or sulfuric acid. H subscript 2 S O subscript 3 is named sulfite or sulfurous acid. H subscript 3 P O subscript 4 is named phosphate or phosphoric acid.\">\r\n<thead>\r\n<tr style=\"height: 24px\">\r\n<th style=\"height: 24px;width: 83px\">Element<\/th>\r\n<th style=\"height: 24px;width: 137px\">Common Ions<\/th>\r\n<th style=\"height: 24px;width: 238px\">Common Names for Ions<\/th>\r\n<\/tr>\r\n<\/thead>\r\n<tbody>\r\n<tr style=\"height: 24px\">\r\n<td style=\"height: 24px;width: 83px\">Cu<\/td>\r\n<td style=\"height: 24px;width: 137px\">Cu<sup>+<\/sup>\/Cu<sup>2+<\/sup><\/td>\r\n<td style=\"height: 24px;width: 238px\">cuprous\/cupric<\/td>\r\n<\/tr>\r\n<tr style=\"height: 24px\">\r\n<td style=\"height: 24px;width: 83px\">Fe<\/td>\r\n<td style=\"height: 24px;width: 137px\">Fe<sup>2+<\/sup>\/Fe<sup>3+<\/sup><\/td>\r\n<td style=\"height: 24px;width: 238px\">ferrous\/ferric<\/td>\r\n<\/tr>\r\n<tr style=\"height: 24px\">\r\n<td style=\"height: 24px;width: 83px\">Co<\/td>\r\n<td style=\"height: 24px;width: 137px\">Co<sup>2+<\/sup>\/Co<sup>3+<\/sup><\/td>\r\n<td style=\"height: 24px;width: 238px\">cobaltous\/cobaltic<\/td>\r\n<\/tr>\r\n<tr>\r\n<td style=\"width: 83px\">Cr<\/td>\r\n<td style=\"width: 137px\">Cr<sup>2+<\/sup>\/Cr<sup>3+<\/sup><\/td>\r\n<td style=\"width: 238px\">chromous\/chromic<\/td>\r\n<\/tr>\r\n<tr style=\"height: 24px\">\r\n<td style=\"height: 24px;width: 83px\">Sn<\/td>\r\n<td style=\"height: 24px;width: 137px\">Sn<sup>2+<\/sup>\/Sn<sup>4+<\/sup><\/td>\r\n<td style=\"height: 24px;width: 238px\">stannous\/stannic<\/td>\r\n<\/tr>\r\n<tr style=\"height: 24px\">\r\n<td style=\"height: 24px;width: 83px\">Pb<\/td>\r\n<td style=\"height: 24px;width: 137px\">Pb<sup>2+<\/sup>\/Pb<sup>4+<\/sup><\/td>\r\n<td style=\"height: 24px;width: 238px\">plumbous\/plumbic<\/td>\r\n<\/tr>\r\n<tr style=\"height: 24px\">\r\n<td style=\"height: 24px;width: 83px\">Hg<\/td>\r\n<td style=\"height: 24px;width: 137px\">Hg<sub>2<\/sub><sup>2+<\/sup>\/Hg<sup>2+<\/sup><\/td>\r\n<td style=\"height: 24px;width: 238px\">mercurous\/mercuric<\/td>\r\n<\/tr>\r\n<tr style=\"height: 24px\">\r\n<td style=\"height: 24px;width: 458px\" colspan=\"3\"><strong>Table 5.<\/strong>\u00a0Common Names for Some Metal Ions with Variable Charges<\/td>\r\n<\/tr>\r\n<\/tbody>\r\n<\/table>\r\n<div class=\"textbox shaded\">\r\n<h3 class=\"title\">Example 2<\/h3>\r\n<p id=\"ball-ch03_s04_p07\" class=\"para\">Name each species.<\/p>\r\n<p class=\"para\">a) O<sup class=\"superscript\">2\u2212 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup>b) Co \u00a0 \u00a0 \u00a0 \u00a0 c)\u00a0Co<sup class=\"superscript\">2+<\/sup><\/p>\r\n&nbsp;\r\n<p class=\"simpara\"><strong>Solution<\/strong><\/p>\r\n<p class=\"simpara\">a) This species has a 2\u2212 charge on it, so it is an anion. Anions are named using the stem of the element name with the suffix <em class=\"emphasis\">-ide<\/em> added. This is the oxide anion.<\/p>\r\n<p class=\"simpara\">b) Because this species has no charge, it is an atom in its elemental form. This is cobalt.<\/p>\r\n<p class=\"simpara\">c) In this case, there is a 2+\u00a0charge on the atom, so it is a cation. We note from <a class=\"autogenerated-content\" href=\"https:\/\/opentextbc.ca\/chemistry\/chapter\/2-6-molecular-and-ionic-compounds\/#CNX_Chem_02_06_IonCharges\" target=\"_blank\" rel=\"noopener\">Figure 2 in Chapter 4.2 Ionic and Molecular Compounds<\/a>),\u00a0that cobalt cations can have two possible charges, so the name of the ion must specify which charge the ion has. This is the cobalt(II) cation.<\/p>\r\n&nbsp;\r\n<p class=\"simpara\"><strong><em class=\"emphasis bolditalic\">Test Yourself<\/em><\/strong><\/p>\r\n<p id=\"ball-ch03_s04_p08\" class=\"para\">Name each species:\u00a0P<sup class=\"superscript\">3\u2212 \u00a0<\/sup>and Sr<sup class=\"superscript\">2+<\/sup><\/p>\r\n&nbsp;\r\n<p class=\"simpara\"><strong><em class=\"emphasis\">Answers<\/em><\/strong><\/p>\r\n<p class=\"simpara\">the phosphide anion and\u00a0the strontium cation<\/p>\r\n\r\n<\/div>\r\n<div class=\"textbox shaded\">\r\n<h3 class=\"title\">Example 3<\/h3>\r\n<p class=\"Indent\">Name the following ionic compounds:<\/p>\r\n<p class=\"Indent\"><span>\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span><span lang=\"ES-MX\">a)<span>\u00a0 <\/span>SnBr<sub>4<\/sub><span>\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span>b)<span>\u00a0<\/span>CoCl<sub>3<\/sub><span>\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span>c)<span>\u00a0 <\/span>Fe<sub>2<\/sub>O<sub>3<\/sub><\/span><\/p>\r\n&nbsp;\r\n<p class=\"Solution\"><strong>Solution\u00a0\u00a0 <\/strong><\/p>\r\n<p class=\"Indentpoints\">a)<span>\u00a0\u00a0 <\/span>First, identify the charge on the cation (Sn).<\/p>\r\n<p class=\"Indentpoints\">Because Br has a charge of \u20131, we know that Sn must have a charge of +4.<\/p>\r\n<p class=\"Indentpoints\"><span>\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span>0 = 1(x) + 4(-1)<span>\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span>x = +4 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<span><\/span>Therefore SnBr<sub>4<\/sub>=<span>\u00a0 <\/span>tin(IV) bromide<\/p>\r\n<p class=\"Indentpoints\">b)<span>\u00a0 <\/span>Cl adopts a charge of \u20131<\/p>\r\n<p class=\"Indentpoints\"><span>\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span>0 = 1(x) + 3(-1)<span>\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span>x = +3 \u00a0 \u00a0 \u00a0 \u00a0\u00a0Therefore CoCl<sub>3<\/sub>= cobalt(III) chloride<\/p>\r\n<p class=\"Indentpoints\">c)<span>\u00a0 <\/span>O adopts a charge of \u20132<\/p>\r\n<p class=\"Indentpoints\"><span>\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span>0 = 2(x) + 3(-2)<span>\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span>x = +3 \u00a0 \u00a0 \u00a0 \u00a0\u00a0Therefore Fe<sub>2<\/sub>O<sub>3<\/sub>= iron(III) oxide<\/p>\r\n&nbsp;\r\n<p class=\"SelfTest\"><em><strong>Test Yourself<\/strong><\/em><\/p>\r\n<p class=\"Indent\">Name the following ionic compounds:<\/p>\r\n<p class=\"Indent\"><span>\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span>a)<span>\u00a0 <\/span>HgO<span>\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span>b)<span>\u00a0 <\/span>PbCl<sub>4<\/sub><span>\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span>c) PbS \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 d) Sc<sub class=\"subscript\">2<\/sub>O<sub class=\"subscript\">3<\/sub> \u00a0 \u00a0 \u00a0 \u00a0 e)\u00a0AgCl<\/p>\r\n&nbsp;\r\n<p class=\"Answers\"><em><strong>Answers<\/strong><\/em><\/p>\r\n<p class=\"Answers\">a) mercury(II) oxide \u00a0 \u00a0 \u00a0 \u00a0 b) lead(IV) chloride \u00a0 \u00a0 \u00a0 \u00a0\u00a0c) lead(II) sulphide<\/p>\r\n<p class=\"Answers\">d) scandium oxide \u00a0 \u00a0 \u00a0 \u00a0 e)\u00a0silver chloride<\/p>\r\n\r\n<\/div>\r\n<div class=\"textbox shaded\" id=\"fs-idm194224\">\r\n<h3>Example 4<\/h3>\r\n<p id=\"fs-idm193552\">Name the following ionic compounds:<\/p>\r\n<p id=\"fs-idm193056\">a) Fe<sub>2<\/sub>S<sub>3 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sub>b) CuSe \u00a0 \u00a0 \u00a0 \u00a0\u00a0c) GaN \u00a0 \u00a0 \u00a0 \u00a0\u00a0d) CrCl<sub>3 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sub>e) Ti<sub>2<\/sub>(SO<sub>4<\/sub>)<sub>3 \u00a0 \u00a0 \u00a0<\/sub> \u00a0\u00a0f) Co<sub class=\"subscript\">2<\/sub>O<sub class=\"subscript\">3<\/sub>\u00a0 \u00a0 \u00a0 \u00a0 \u00a0g)\u00a0CaCl<sub class=\"subscript\">2<\/sub>\u00a0 \u00a0 \u00a0 \u00a0 \u00a0h) AlF<sub class=\"subscript\">3<\/sub><\/p>\r\n&nbsp;\r\n<p id=\"fs-idp282326320\"><strong>Solution<\/strong>\r\nThe anions in these compounds have a fixed negative charge (S<sup>2\u2212<\/sup>, Se<sup>2\u2212 <\/sup>, N<sup>3\u2212<\/sup>, Cl<sup>\u2212<\/sup>, SO<sub>4<\/sub><sup>2\u2212<\/sup>,\u00a0O<sup>\u22122<\/sup>, and F<sup>\u2212<\/sup>), and the compounds must be neutral. Because the metal ions in questions a) to f) have a variable charge, we must figure out the charge of the metal ion by ensuring that the total number of positive charges in each compound must equal the total number of negative charges. \u00a0Therefore the positive ions must be Fe<sup>3+<\/sup>, Cu<sup>2+<\/sup>, Ga<sup>3+<\/sup>, Cr<sup>3+<\/sup>, Ti<sup>3+<\/sup>\u00a0and Co<sup>3+<\/sup>. These charges are used in the names of the metal ions:<\/p>\r\n<p id=\"fs-idm104688\">a) iron(III) sulfide \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 b) copper(II) selenide \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 c) gallium(III) nitride<\/p>\r\nd) chromium(III) chloride \u00a0 \u00a0 \u00a0 \u00a0\u00a0e) titanium(III) sulfate \u00a0 \u00a0 \u00a0 \u00a0 \u00a0f)\u00a0cobalt(III) oxide\r\n\r\nIn questions g) and h) the metal ions do not have a variable charge, therefore\r\n<p class=\"simpara\">g) Using the names of the ions, this ionic compound is named calcium chloride. <em class=\"emphasis\">It is not calcium(II) chloride<\/em> because calcium forms only one cation when it forms an ion, and it has a characteristic charge of 2+.<\/p>\r\n<p class=\"simpara\">h)The name of this ionic compound is aluminum fluoride.<\/p>\r\n&nbsp;\r\n<p id=\"fs-idp283458192\"><b><i>Test Yourself<\/i><\/b><\/p>\r\nWrite the formulas of the following ionic compounds:\r\n<p id=\"fs-idp283458864\">a) chromium(III) phosphide \u00a0 \u00a0 \u00a0 \u00a0b) mercury(II) sulfide \u00a0 \u00a0 \u00a0 \u00a0\u00a0c) manganese(II) phosphate<\/p>\r\n<p id=\"fs-idp268147248\">d) copper(I) oxide \u00a0 \u00a0 \u00a0 \u00a0\u00a0e) chromium(VI) fluoride<\/p>\r\n&nbsp;\r\n\r\n<em><strong>Answers<\/strong><\/em>\r\n\r\na) CrP \u00a0 \u00a0 \u00a0 \u00a0 b) HgS \u00a0 \u00a0 \u00a0 \u00a0c) Mn<sub>3<\/sub>(PO<sub>4<\/sub>)<sub>2 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sub>d) Cu<sub>2<\/sub>O \u00a0 \u00a0 \u00a0 \u00a0 e) CrF<sub>6<\/sub>\r\n\r\n<\/div>\r\n<\/section><section id=\"fs-idp282353488\">\r\n<div class=\"textbox shaded\" id=\"fs-idm8768\">\r\n<h3 class=\"title\">Erin Brockovich and Chromium Contamination<\/h3>\r\n<p id=\"fs-idm7968\">In the early 1990s, legal file clerk Erin Brockovich (<a class=\"autogenerated-content\" href=\"#CNX_Chem_02_07_ErinBrocko\">Figure 1<\/a>) discovered a high rate of serious illnesses in the small town of Hinckley, California. Her investigation eventually linked the illnesses to groundwater contaminated by Cr(VI) used by Pacific Gas &amp; Electric (PG&amp;E) to fight corrosion in a nearby natural gas pipeline. As dramatized in the film <em>Erin Brokovich<\/em> (for which Julia Roberts won an Oscar), Erin and lawyer Edward Masry sued PG&amp;E for contaminating the water near Hinckley in 1993. The settlement they won in 1996\u2014$333 million\u2014was the largest amount ever awarded for a direct-action lawsuit in the US at that time.<\/p>\r\n\r\n<figure id=\"CNX_Chem_02_07_ErinBrocko\">\r\n\r\n[caption id=\"\" align=\"aligncenter\" width=\"1200\"]<a href=\"https:\/\/opentextbc.ca\/chemistry\/wp-content\/uploads\/sites\/150\/2016\/05\/CNX_Chem_02_07_ErinBrocko.jpg\"><img width=\"1200\" height=\"447\" alt=\"Figure A shows a photo of Erin Brockovich. Figure B shows a 3-D ball-and-stick model of chromate. Chromate has a chromium atom at its center that forms bonds with four oxygen atoms each. Two of the oxygen atoms form single bonds with the chromium atom while the other two form double bonds each. The structure of dichromate consists of two chromate ions that are bonded and share one of their oxygen atoms to which each chromate atom has a single bond.\" src=\"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/CNX_Chem_02_07_ErinBrocko-2.jpg\" \/><\/a> <strong>Figure 1.<\/strong> (a) Erin Brockovich found that Cr(VI), used by PG&amp;E, had contaminated the Hinckley, California, water supply. (b) The Cr(VI) ion is often present in water as the polyatomic ions chromate, CrO<sub>4<\/sub><sup>2\u2212<\/sup> (left), and dichromate, Cr<sub>2<\/sub>O<sub>7<\/sub><sup>2\u2212<\/sup> (right).[\/caption]<\/figure>\r\n<p id=\"fs-idp279149248\">Chromium compounds are widely used in industry, such as for chrome plating, in dye-making, as preservatives, and to prevent corrosion in cooling tower water, as occurred near Hinckley. In the environment, chromium exists primarily in either the Cr(III) or Cr(VI) forms. Cr(III), an ingredient of many vitamin and nutritional supplements, forms compounds that are not very soluble in water, and it has low toxicity. But Cr(VI) is much more toxic and forms compounds that are reasonably soluble in water. Exposure to small amounts of Cr(VI) can lead to damage of the respiratory, gastrointestinal, and immune systems, as well as the kidneys, liver, blood, and skin.<\/p>\r\n<p id=\"fs-idp279150320\">Despite cleanup efforts, Cr(VI) groundwater contamination remains a problem in Hinckley and other locations across the globe. A 2010 study by the Environmental Working Group found that of 35 US cities tested, 31 had higher levels of Cr(VI) in their tap water than the public health goal of 0.02 parts per billion set by the California Environmental Protection Agency.<\/p>\r\n\r\n<\/div>\r\n<\/section><\/section><section id=\"fs-idp279151472\">\r\n<div class=\"textbox shaded\">\r\n<h3 class=\"title\">Example 5<\/h3>\r\n<p id=\"ball-ch03_s04_p23\" class=\"para\">Write the proper formula and give the proper name for each ionic compound formed between the two listed ions.<\/p>\r\n<p class=\"para\">a) NH<sub class=\"subscript\">4<\/sub><sup class=\"superscript\">+<\/sup> and S<sup class=\"superscript\">2\u2212 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0<\/sup>b) Al<sup class=\"superscript\">3+<\/sup> and PO<sub class=\"subscript\">4<\/sub><sup class=\"superscript\">3\u2212 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0<\/sup>c) Fe<sup class=\"superscript\">2+<\/sup> and PO<sub class=\"subscript\">4<\/sub><sup class=\"superscript\">3\u2212<\/sup><\/p>\r\n&nbsp;\r\n<p class=\"simpara\"><strong>Solution<\/strong><\/p>\r\n<p class=\"simpara\">a) Because the ammonium ion has a 1+\u00a0charge and the sulfide ion has a 2\u2212 charge, we need two ammonium ions to balance the charge on a single sulfide ion. Enclosing the formula for the ammonium ion in parentheses, we have (NH<sub class=\"subscript\">4<\/sub>)<sub class=\"subscript\">2<\/sub>S. The compound\u2019s name is ammonium sulfide.<\/p>\r\n<p class=\"simpara\">b) Because the ions have the same magnitude of charge, we need only one of each to balance the charges. The formula is AlPO<sub class=\"subscript\">4<\/sub>, and the name of the compound is aluminum phosphate.<\/p>\r\n<p class=\"simpara\">c) Neither charge is an exact multiple of the other, so we have to go to the least common multiple of 6. To get 6+, we need three iron(II) ions, and to get 6\u2212, we need two phosphate ions. The proper formula is Fe<sub class=\"subscript\">3<\/sub>(PO<sub class=\"subscript\">4<\/sub>)<sub class=\"subscript\">2<\/sub>, and the compound\u2019s name is iron(II) phosphate.<\/p>\r\n&nbsp;\r\n<p class=\"simpara\"><strong><em class=\"emphasis bolditalic\">Test Yourself<\/em><\/strong><\/p>\r\n<p id=\"ball-ch03_s04_p24\" class=\"para\">Write the proper formula and give the proper name for each ionic compound formed between the two listed ions.<\/p>\r\n<p class=\"para\">a) NH<sub class=\"subscript\">4<\/sub><sup class=\"superscript\">+<\/sup> and PO<sub class=\"subscript\">4<\/sub><sup class=\"superscript\">3\u2212 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0<\/sup>b) Co<sup class=\"superscript\">3+<\/sup> and NO<sub class=\"subscript\">2<\/sub><sup class=\"superscript\">\u2212<\/sup><\/p>\r\n&nbsp;\r\n<p class=\"simpara\"><strong><em class=\"emphasis\">Answers<\/em><\/strong><\/p>\r\n<p class=\"simpara\">a) (NH<sub class=\"subscript\">4<\/sub>)<sub class=\"subscript\">3<\/sub>PO<sub class=\"subscript\">4<\/sub>, ammonium phosphate \u00a0 \u00a0 \u00a0 \u00a0 \u00a0b)\u00a0Co(NO<sub class=\"subscript\">2<\/sub>)<sub class=\"subscript\">3<\/sub>, cobalt(III) nitrite<\/p>\r\n\r\n<\/div>\r\n<section id=\"fs-idp268266480\"><section id=\"fs-idp279293712\">\r\n<div class=\"textbox shaded\" id=\"fs-idm337456\">\r\n<h3 class=\"title\">Ionic Compounds in Your Cabinets<\/h3>\r\n<p id=\"fs-idm70496\">Every day you encounter and use a large number of ionic compounds. Some of these compounds, where they are found, and what they are used for are listed in <a class=\"autogenerated-content\" href=\"#fs-idp268265360\">Table 3<\/a>. Look at the label or ingredients list on the various products that you use during the next few days, and see if you run into any of those in this table, or find other ionic compounds that you could now name or write as a formula.<\/p>\r\n\r\n<table id=\"fs-idp268265360\" class=\"span-all\" summary=\"The everyday ionic compound examples included in this table are: N a C L sodium chloride, or ordinary table salt, K I potassium iodide which is added to iodized salt, N a F, sodium fluoride which is an ingredient in toothpaste, N a H C O subscript 3 sodium bicarbonate which is baking soda, used in cooking and as an antacid, N a subscript 2 C O subscript 3 sodium carbonate which is washing soda and is used in cleaning agents, N a O C l sodium hypochlorite which is the active ingredient in household bleach, C a C O subscript 3 calcium carbonate which is an ingredient of antacids, M g ( O H ) subscript 2, magnesium hydroxide which is also an ingredient of antacids, A l ( O H ) subscript 3 aluminum hydroxide which is also an ingredient in antacids, N a O H sodium hydroxide which is lye and is used as a drain cleaner, K subscript 3 P O subscript 4 potassium phosphate which is a food additive, M g S O subscript 4 magneisum sulfate which is added to purified water, N a subscript 2 H P O subscript 4 sodium hydrogen phosphate which is an anti-caking agent and is used in powdered products, and N a subscript 2 S O subscript 3 sodium sulfite which is a preservative.\">\r\n<thead>\r\n<tr>\r\n<th>Ionic Compound<\/th>\r\n<th>Use<\/th>\r\n<\/tr>\r\n<\/thead>\r\n<tbody>\r\n<tr>\r\n<td>NaCl, sodium chloride<\/td>\r\n<td>ordinary table salt<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>KI, potassium iodide<\/td>\r\n<td>added to \u201ciodized\u201d salt for thyroid health<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>NaF, sodium fluoride<\/td>\r\n<td>ingredient in toothpaste<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>NaHCO<sub>3<\/sub>, sodium bicarbonate<\/td>\r\n<td>baking soda; used in cooking (and as antacid)<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Na<sub>2<\/sub>CO<sub>3<\/sub>, sodium carbonate<\/td>\r\n<td>washing soda; used in cleaning agents<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>NaOCl, sodium hypochlorite<\/td>\r\n<td>active ingredient in household bleach<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>CaCO<sub>3<\/sub> calcium carbonate<\/td>\r\n<td>ingredient in antacids<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Mg(OH)<sub>2<\/sub>, magnesium hydroxide<\/td>\r\n<td>ingredient in antacids<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Al(OH)<sub>3<\/sub>, aluminum hydroxide<\/td>\r\n<td>ingredient in antacids<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>NaOH, sodium hydroxide<\/td>\r\n<td>lye; used as drain cleaner<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>K<sub>3<\/sub>PO<sub>4<\/sub>, potassium phosphate<\/td>\r\n<td>food additive (many purposes)<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>MgSO<sub>4<\/sub>, magnesium sulfate<\/td>\r\n<td>added to purified water<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Na<sub>2<\/sub>HPO<sub>4<\/sub>, sodium hydrogen phosphate<\/td>\r\n<td>anti-caking agent; used in powdered products<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Na<sub>2<\/sub>SO<sub>3<\/sub>, sodium sulfite<\/td>\r\n<td>preservative<\/td>\r\n<\/tr>\r\n<tr>\r\n<td colspan=\"2\"><strong>Table 3.<\/strong> Everyday Ionic Compounds<\/td>\r\n<\/tr>\r\n<\/tbody>\r\n<\/table>\r\n&nbsp;\r\n\r\n<\/div>\r\n<\/section><\/section>\r\n<h2>Nomenclature of Molecular (Covalent) Compounds<\/h2>\r\n<p id=\"fs-idp268164784\">The bonding characteristics of inorganic molecular compounds are different from ionic compounds, and they are named using a different system as well. The charges of cations and anions dictate their ratios in ionic compounds, so specifying the names of the ions provides sufficient information to determine chemical formulas. However, because covalent bonding allows for significant variation in the combination ratios of the atoms in a molecule, the names for molecular compounds must explicitly identify these ratios.<\/p>\r\n\r\n<section id=\"fs-idp268165696\">\r\n<h2>Compounds Composed of Two Elements<\/h2>\r\n<p id=\"fs-idp268166336\">When two nonmetallic elements form a molecular compound, several combination ratios are often possible. For example, carbon and oxygen can form the compounds CO and CO<sub>2<\/sub>. Since these are different substances with different properties, they cannot both have the same name (they cannot both be called carbon oxide). To deal with this situation, we use a naming method that is somewhat similar to that used for ionic compounds, but with added prefixes to specify the numbers of atoms of each element. The name of the more metallic element (the one farther to the left and\/or bottom of the periodic table) is first, followed by the name of the more nonmetallic element (the one farther to the right and\/or top) with its ending changed to the suffix \u2013<em>ide<\/em>. The numbers of atoms of each element are designated by the Greek prefixes shown in <a class=\"autogenerated-content\" href=\"#fs-idp268400368\">Table 6<\/a>.<\/p>\r\n\r\n<table id=\"fs-idp268400368\" class=\"span-all\" summary=\"This table has two columns labeled \u201cprefix\u201d and \u201cnumber\u201d. Mono is associated with one although this prefix is sometimes omitted. Di is associated with two. Tri is associated with three. Tetra is associated with four. Penta is associated with five. Hexa is associated with six. Hepta is associated with seven. Octa is associated with eight. Nona is associated with nine. Deca is associated with ten.\">\r\n<thead>\r\n<tr>\r\n<th>Number<\/th>\r\n<th>Prefix<\/th>\r\n<th>Number<\/th>\r\n<th>Prefix<\/th>\r\n<\/tr>\r\n<\/thead>\r\n<tbody>\r\n<tr>\r\n<td>1 (sometimes omitted)<\/td>\r\n<td>mono-<\/td>\r\n<td>6<\/td>\r\n<td>hexa-<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>2<\/td>\r\n<td>di-<\/td>\r\n<td>7<\/td>\r\n<td>hepta-<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>3<\/td>\r\n<td>tri-<\/td>\r\n<td>8<\/td>\r\n<td>octa-<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>4<\/td>\r\n<td>tetra-<\/td>\r\n<td>9<\/td>\r\n<td>nona-<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>5<\/td>\r\n<td>penta-<\/td>\r\n<td>10<\/td>\r\n<td>deca-<\/td>\r\n<\/tr>\r\n<tr>\r\n<td colspan=\"4\"><strong>Table 6.<\/strong> Nomenclature Prefixes<\/td>\r\n<\/tr>\r\n<\/tbody>\r\n<\/table>\r\n<p id=\"fs-idm325632\">When only one atom of the first element is present, the prefix <em>mono<\/em>- is usually deleted from that part. Thus, CO is named carbon monoxide, and CO<sub>2<\/sub> is called carbon dioxide. When two vowels are adjacent, the <em>a<\/em> in the Greek prefix is usually dropped. Some other examples are shown in <a class=\"autogenerated-content\" href=\"#fs-idp269568176\">Table 7<\/a>.<\/p>\r\n\r\n<table id=\"fs-idp269568176\" class=\"span-all\" summary=\"A two column table is shown. The left column is titled \u201cCompound\u201d and the right column is titled \u201cName.\u201d From left to right, the first row reads \u201cS O subscript 2\u201d and \u201csulfur dioxide.\u201d The second row reads \u201cS O subscript 3\u201d and \u201csulfur trioxide.\u201d The third row reads \u201cN O subscript 2\u201d and \u201cnitrogen dioxide.\u201d The fourth row reads \u201cN subscript 2 O subscript 4\u201d and \u201cdinitrogen tetroxide.\u201d The fifth row reads \u201cN subscript 2 O subscript 5\u201d and \u201cdinitrogen pentoxide.\u201d The sixth row reads \u201cB C l subscript 3\u201d and \u201cboron trichloride.\u201d The seventh row reads \u201cS F subscript 6\u201d and \u201csulfur hexafluoride.\u201d The eighth row reads \u201cP F subscript 5\u201d and \u201cphosphorus pentafluoride.\u201d The ninth row reads \u201cP subscript 4 O subscript 10\u201d and \u201ctetraphosphorus decaoxide.\u201d The tenth row reads \u201cI F subscript 7\u201d and \u201ciodine heptafluoride.\u201d\">\r\n<thead>\r\n<tr>\r\n<th>Compound<\/th>\r\n<th>Name<\/th>\r\n<th>Compound<\/th>\r\n<th>Name<\/th>\r\n<\/tr>\r\n<\/thead>\r\n<tbody>\r\n<tr>\r\n<td>SO<sub>2<\/sub><\/td>\r\n<td>sulfur dioxide<\/td>\r\n<td>BCl<sub>3<\/sub><\/td>\r\n<td>boron trichloride<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>SO<sub>3<\/sub><\/td>\r\n<td>sulfur trioxide<\/td>\r\n<td>SF<sub>6<\/sub><\/td>\r\n<td>sulfur hexafluoride<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>NO<sub>2<\/sub><\/td>\r\n<td>nitrogen dioxide<\/td>\r\n<td>PF<sub>5<\/sub><\/td>\r\n<td>phosphorus pentafluoride<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>N<sub>2<\/sub>O<sub>4<\/sub><\/td>\r\n<td>dinitrogen tetroxide<\/td>\r\n<td>P<sub>4<\/sub>O<sub>10<\/sub><\/td>\r\n<td>tetraphosphorus decaoxide<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>N<sub>2<\/sub>O<sub>5<\/sub><\/td>\r\n<td>dinitrogen pentoxide<\/td>\r\n<td>IF<sub>7<\/sub><\/td>\r\n<td>iodine heptafluoride<\/td>\r\n<\/tr>\r\n<tr>\r\n<td colspan=\"4\"><strong>Table 7.<\/strong> Names of Some Molecular Compounds Composed of Two Elements<\/td>\r\n<\/tr>\r\n<\/tbody>\r\n<\/table>\r\n<p id=\"fs-idm207744\">There are a few common names that you will encounter as you continue your study of chemistry. For example, although NO is often called nitric oxide, its proper name is nitrogen monoxide. Similarly, N<sub>2<\/sub>O is known as nitrous oxide even though our rules would specify the name dinitrogen monoxide. (And H<sub>2<\/sub>O is usually called water, not dihydrogen monoxide.) You should commit to memory the common names of compounds as you encounter them.<\/p>\r\n\r\n<div class=\"textbox shaded\" id=\"fs-idm206240\">\r\n<h3>Example 6<\/h3>\r\n<p id=\"fs-idm205600\">Name the following covalent compounds:<\/p>\r\n<p id=\"fs-idm205216\">a) SF<sub>6 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sub>b) N<sub>2<\/sub>O<sub>3 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sub>c) Cl<sub>2<\/sub>O<sub>7 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sub>d) P<sub>4<\/sub>O<sub>6<\/sub> \u00a0 \u00a0 \u00a0 \u00a0\u00a0e) PF<sub class=\"subscript\">3<\/sub> \u00a0 \u00a0 \u00a0 \u00a0 f)\u00a0CO \u00a0 \u00a0 \u00a0 \u00a0 g)\u00a0Se<sub class=\"subscript\">2<\/sub>Br<sub class=\"subscript\">2<\/sub><\/p>\r\n&nbsp;\r\n<p id=\"fs-idp268181136\"><strong>Solution<\/strong>\r\nBecause these compounds consist solely of nonmetals, they are molecular compounds, therefore according to the rules, we use prefixes to designate the number of atoms of each element:<\/p>\r\n<p id=\"fs-idm335200\">a) sulfur hexafluoride \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0b) dinitrogen trioxide \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0c) dichloride heptoxide<\/p>\r\nd) tetraphosphorus hexoxide \u00a0 \u00a0 \u00a0 \u00a0 e) phosphorus trifluoride \u00a0 \u00a0 \u00a0 \u00a0 f) carbon monoxide (not carbon monooxide)\r\n\r\ng)\u00a0diselenium dibromide\r\n\r\n&nbsp;\r\n<p id=\"fs-idm333600\"><em><strong>Test Yourself<\/strong><\/em>\r\nWrite the formulas for the following compounds:<\/p>\r\n<p id=\"fs-idm332928\">a) phosphorus pentachloride \u00a0 \u00a0 \u00a0 \u00a0 \u00a0b) dinitrogen monoxide \u00a0 \u00a0 \u00a0 \u00a0\u00a0c) iodine heptafluoride<\/p>\r\nd) carbon tetrachloride \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 e)\u00a0disulfur difluoride \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0f)\u00a0iodine pentabromide\r\n\r\n&nbsp;\r\n\r\n<em><strong>Answers<\/strong><\/em>\r\n\r\na) PCl<sub>5 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sub>b) N<sub>2<\/sub>O \u00a0 \u00a0 \u00a0 \u00a0 c) IF<sub>7 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sub>d) CCl<sub>4<\/sub> \u00a0 \u00a0 \u00a0e)\u00a0S<sub class=\"subscript\">2<\/sub>F<sub class=\"subscript\">2 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sub>f) IBr<sub class=\"subscript\">5<\/sub>\r\n\r\n<\/div>\r\n<div class=\"textbox shaded\" id=\"fs-idp283404080\">\r\n\r\n<img width=\"108\" height=\"67\" class=\"alignleft\" alt=\"\u00a0\" src=\"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/OSC_Interactive_200-4-2.png\" \/>\r\n<p id=\"fs-idp268192304\">The following <a href=\"http:\/\/openstaxcollege.org\/l\/16chemcompname\">website<\/a> provides practice with naming chemical compounds and writing chemical formulas. You can choose binary, polyatomic, and variable charge ionic compounds, as well as molecular compounds.<\/p>\r\n\r\n<\/div>\r\n<\/section><section id=\"fs-idp268193776\">\r\n<h2>Binary Acids<\/h2>\r\n<p id=\"fs-idp282238096\">Some compounds containing hydrogen are members of an important class of substances known as acids, and these compounds have interesting chemical properties. The chemistry of these compounds is explored in more detail in later chapters of this text, but for now, it will suffice to note that many acids release hydrogen ions, H<sup>+<\/sup>, when dissolved in water. \u00a0To indicate that something is dissolved in water, we will use the phase label (aq) next to a chemical formula (where aq stands for \u201caqueous,\u201d a word that describes something dissolved in water). \u00a0To denote this distinct chemical property, a mixture of water with an acid is given a name derived from the compound\u2019s name. If the compound is a <strong>binary acid<\/strong> (comprised of hydrogen and one other nonmetallic element):<\/p>\r\n\r\n<ol id=\"fs-idp282239904\">\r\n \t<li>The word \u201chydrogen\u201d is changed to the prefix <em>hydro-<\/em><\/li>\r\n \t<li>The other nonmetallic element name is modified by adding the suffix -<em>ic<\/em><\/li>\r\n \t<li>The word \u201cacid\u201d is added as a second word<\/li>\r\n<\/ol>\r\n<p id=\"fs-idm109568\">For example, when the gas HCl (hydrogen chloride) is dissolved in water, the solution is called <em>hydrochloric acid<\/em>. Several other examples of this nomenclature are shown in <a class=\"autogenerated-content\" href=\"#fs-idp272649888\">Table 8<\/a>.<\/p>\r\n\r\n<table id=\"fs-idp272649888\" class=\"span-all\" summary=\"The names of simple acids included in this table are: H F gas, which is hydrogen fluoride, H C l gas which is hydrogen chloride, H B r gas which is hydrogen bromide, H I gas which is hydrogen iodide, H subscript 2 S gas which is hydrogen sulfide, H F aqueous which is hydrofluoric acid, H C l aqueous which is hydrochloric acid, H B r aqueous which is hydrobromic acid, H I aqueous which is hydroiodic acid, and H subscript 2 S aqueous which is hydrosulfuric acid.\">\r\n<thead>\r\n<tr>\r\n<th>Name of Gas<\/th>\r\n<th>Name of Acid<\/th>\r\n<\/tr>\r\n<\/thead>\r\n<tbody>\r\n<tr>\r\n<td>HF(<em>g<\/em>), hydrogen fluoride<\/td>\r\n<td>HF(<em>aq<\/em>), hydrofluoric acid<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>HCl(<em>g<\/em>), hydrogen chloride<\/td>\r\n<td>HCl(<em>aq<\/em>), hydrochloric acid<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>HBr(<em>g<\/em>), hydrogen bromide<\/td>\r\n<td>HBr(<em>aq<\/em>), hydrobromic acid<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>HI(<em>g<\/em>), hydrogen iodide<\/td>\r\n<td>HI(<em>aq<\/em>), hydroiodic acid<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>H<sub>2<\/sub>S(<em>g<\/em>), hydrogen sulfide<\/td>\r\n<td>H<sub>2<\/sub>S(<em>aq<\/em>), hydrosulfuric acid<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>HCN(<em>g<\/em>), hydrogen cyanide<\/td>\r\n<td>HCN(<em>aq<\/em>), hydrocyanic acid<\/td>\r\n<\/tr>\r\n<tr>\r\n<td colspan=\"2\"><strong>Table 8.<\/strong> Names of Some Simple Acids<\/td>\r\n<\/tr>\r\n<\/tbody>\r\n<\/table>\r\n<\/section><section id=\"fs-idp268349296\">\r\n<h2>Oxyacids<\/h2>\r\n<p id=\"fs-idp279162704\">Many compounds containing three or more elements (such as organic compounds or coordination compounds) are subject to specialized nomenclature rules that you will learn later. However, we will briefly discuss the important compounds known as <strong>oxyacids<\/strong>, compounds that contain hydrogen, oxygen, and at least one other element, and are bonded in such a way as to impart acidic properties to the compound (you will learn the details of this in a later chapter). Typical oxyacids consist of hydrogen combined with a polyatomic, oxygen-containing ion. To name oxyacids:<\/p>\r\n\r\n<ol id=\"fs-idp279164064\">\r\n \t<li>Omit \u201chydrogen\u201d<\/li>\r\n \t<li>Start with the root name of the anion<\/li>\r\n \t<li>Replace \u2013<em>ate<\/em> with \u2013<em>ic<\/em>, or \u2013<em>ite<\/em> with \u2013<em>ous<\/em><\/li>\r\n \t<li>Add \u201cacid\u201d<\/li>\r\n<\/ol>\r\n<p id=\"fs-idp282461232\">For example, consider H<sub>2<\/sub>CO<sub>3<\/sub> (which you might be tempted to call \u201chydrogen carbonate\u201d). To name this correctly, \u201chydrogen\u201d is omitted; the \u2013<em>ate<\/em> of carbonate is replace with \u2013<em>ic<\/em>; and acid is added\u2014so its name is carbonic acid. Other examples are given in <a class=\"autogenerated-content\" href=\"#fs-idp268340336\">Table 9<\/a>. There are some exceptions to the general naming method (e.g., H<sub>2<\/sub>SO<sub>4<\/sub> is called sulfuric acid, not sulfic acid, and H<sub>2<\/sub>SO<sub>3<\/sub> is sulfurous, not sulfous, acid).<\/p>\r\n\r\n<table id=\"fs-idp268340336\" class=\"span-all\" summary=\"This table has three columns labeled \u201cformula\u201d, \u201canion name\u201d, and \u201cacid name\u201d. H C subscript 2 H subscript 3 O subscript 2 is named acetate or acetic acid. H N O subscript 3 is named nitrate or nitric acid. H N O subscript 2 is named nitrite or nitrous acid, H C l O subscript 4 is named perchlorate or perchloric acid. H subscript 2 C O subscript 3 is named carbonate or carbonic acid. H subscript 2 S O subscript 4 is named sulfate or sulfuric acid. H subscript 2 S O subscript 3 is named sulfite or sulfurous acid. H subscript 3 P O subscript 4 is named phosphate or phosphoric acid.\">\r\n<thead>\r\n<tr>\r\n<th>Formula<\/th>\r\n<th>Anion Name<\/th>\r\n<th>Acid Name<\/th>\r\n<\/tr>\r\n<\/thead>\r\n<tbody>\r\n<tr>\r\n<td>HC<sub>2<\/sub>H<sub>3<\/sub>O<sub>2<\/sub><\/td>\r\n<td>acetate<\/td>\r\n<td>acetic acid<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>HNO<sub>3<\/sub><\/td>\r\n<td>nitrate<\/td>\r\n<td>nitric acid<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>HNO<sub>2<\/sub><\/td>\r\n<td>nitrite<\/td>\r\n<td>nitrous acid<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>HClO<sub>4<\/sub><\/td>\r\n<td>perchlorate<\/td>\r\n<td>perchloric acid<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>HClO<sub><span style=\"font-size: small\">3<\/span><\/sub><\/td>\r\n<td>chlorate<\/td>\r\n<td>chloric acid<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>HClO<sub><span style=\"font-size: small\">2<\/span><\/sub><\/td>\r\n<td>chlorite<\/td>\r\n<td>chlorous acid<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>HClO<\/td>\r\n<td>hypochlorite<\/td>\r\n<td>hypochlorous acid<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>H<sub>2<\/sub>CO<sub>3<\/sub><\/td>\r\n<td>carbonate<\/td>\r\n<td>carbonic acid<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>H<sub>2<\/sub>SO<sub>4<\/sub><\/td>\r\n<td>sulfate<\/td>\r\n<td>sulfuric acid<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>H<sub>2<\/sub>SO<sub>3<\/sub><\/td>\r\n<td>sulfite<\/td>\r\n<td>sulfurous acid<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>H<sub>3<\/sub>PO<sub>4<\/sub><\/td>\r\n<td>phosphate<\/td>\r\n<td>phosphoric acid<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>H<sub>3<\/sub>PO<sub>3<\/sub><\/td>\r\n<td>phosphite<\/td>\r\n<td>phosphorous acid<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>H<sub>2<\/sub>CrO<sub>4<\/sub><\/td>\r\n<td>chromate<\/td>\r\n<td>chromic acid<\/td>\r\n<\/tr>\r\n<tr>\r\n<td colspan=\"3\"><strong>Table 9.<\/strong> Names of Common Oxyacids<\/td>\r\n<\/tr>\r\n<\/tbody>\r\n<\/table>\r\n<\/section><\/section><section id=\"fs-idp282340144\" class=\"summary\">\r\n<div class=\"textbox shaded\">\r\n<h3 class=\"title\">Example 7<\/h3>\r\n<p id=\"ball-ch03_s05_p04\" class=\"para\">Name each acid without consulting the tables.<\/p>\r\n<p class=\"para\">a) HBr(aq) \u00a0 \u00a0 \u00a0 \u00a0 b)\u00a0H<sub class=\"subscript\">2<\/sub>SO<sub class=\"subscript\">4 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sub><span>c)\u00a0 HF(g)\u00a0 \u00a0 \u00a0 \u00a0 \u00a0d)\u00a0 HCN(aq) \u00a0 \u00a0\u00a0\u00a0\u00a0\u00a0 e) H<sub>2<\/sub>S(aq)<\/span><\/p>\r\n&nbsp;\r\n<p class=\"simpara\"><strong>Solution<\/strong><\/p>\r\n<p class=\"simpara\">a) As an aqueous binary acid, the acid\u2019s name is <em class=\"emphasis\">hydro-<\/em> +\u00a0stem name +\u00a0<em class=\"emphasis\">-ic acid<\/em>. Because this acid contains a bromine atom, the name is hydrobromic acid.<\/p>\r\n<p class=\"simpara\">b) Because this acid is derived from the sulfate ion, the name of the acid is the stem of the anion name +\u00a0<em class=\"emphasis\">-ic acid<\/em>. The name of this acid is sulfuric acid.<\/p>\r\n<p class=\"simpara\">c) Because HF<span>(g)<\/span><span>\u00a0is in gaseous form, we name it hydrogen fluoride<\/span>.<\/p>\r\n<p class=\"Indentpoints\">d)<span>\u00a0 <\/span>HCN<span>(aq)<\/span><span>\u00a0<\/span>contains the polyatomic ion cyanide. The root is \u201ccyan\u201d, thus HCN<span>(aq)<\/span><span>\u00a0<\/span>= hydrocyanic acid.<\/p>\r\n<p class=\"Indentpoints\">e)<span>\u00a0 <\/span>H<sub>2<\/sub>S<span>(aq)<\/span><span>\u00a0<\/span>contains the ion sulfide. In this case, however, the root takes a slightly different form of \u201csulfur\u201d (the same as the element name). Thus H<sub>2<\/sub>S<span>(aq)<\/span><span>\u00a0<\/span>= hydrosulfuric acid.<\/p>\r\n&nbsp;\r\n<p class=\"simpara\"><strong><em class=\"emphasis bolditalic\">Test Yourself<\/em><\/strong><\/p>\r\n<p id=\"ball-ch03_s05_p05\" class=\"para\">Name each acid.<\/p>\r\n<p class=\"para\">a) HF(aq) \u00a0 \u00a0 \u00a0 \u00a0 b)\u00a0HNO<sub class=\"subscript\">2 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sub>c)<span>\u00a0<\/span>HClO<sub>4<\/sub><span>\u00a0 \u00a0 \u00a0 \u00a0<\/span>d)<span>\u00a0<\/span>H<sub>2<\/sub>SO<sub>4 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sub>e)<span>\u00a0<\/span>H<sub>2<\/sub>CrO<sub>4<\/sub><span>(aq)<\/span><span>\u00a0 \u00a0 \u00a0 \u00a0 \u00a0 f<\/span>)<span>\u00a0 <\/span>H<sub>3<\/sub>PO<sub>4<\/sub><span>(aq)<\/span><span>\u00a0 \u00a0 \u00a0\u00a0<\/span>g) HClO<span>(aq)<\/span><\/p>\r\n&nbsp;\r\n<p class=\"simpara\"><strong><em class=\"emphasis\">Answers<\/em><\/strong><\/p>\r\n<p class=\"simpara\">a) hydrofluoric acid \u00a0 \u00a0 \u00a0 \u00a0\u00a0b) nitrous acid \u00a0 \u00a0 \u00a0 \u00a0 c) perchloric acid \u00a0 \u00a0 \u00a0 \u00a0 d) sulphuric acid \u00a0 \u00a0 \u00a0 \u00a0 e) chromic acid<\/p>\r\nf) phosphoric acid \u00a0 \u00a0 \u00a0 \u00a0 g) hypochlorous acid\r\n\r\n<\/div>\r\n<p id=\"ball-ch03_s05_p06\" class=\"para editable block\">All acids have some similar properties. For example, acids have a sour taste; in fact, the sour taste of some of our foods, such as citrus fruits and vinegar, is caused by the presence of acids in food. Many acids react with some metallic elements to form metal ions and elemental hydrogen. Acids make certain plant pigments change colors; indeed, the ripening of some fruits and vegetables is caused by the formation or destruction of excess acid in the plant. In a later chapter, we will explore the chemical behaviour of acids.<\/p>\r\n<p id=\"ball-ch03_s05_p07\" class=\"para editable block\">Acids are very prevalent in the world around us. We have already mentioned that citrus fruits contain acid; among other compounds, they contain citric acid, H<sub class=\"subscript\">3<\/sub>C<sub class=\"subscript\">6<\/sub>H<sub class=\"subscript\">5<\/sub>O<sub class=\"subscript\">7<\/sub>(aq). Oxalic acid, H<sub class=\"subscript\">2<\/sub>C<sub class=\"subscript\">2<\/sub>O<sub class=\"subscript\">4<\/sub>(aq), is found in spinach and other green leafy vegetables. Hydrochloric acid not only is found in the stomach (stomach acid) but also can be bought in hardware stores as a cleaner for concrete and masonry. Phosphoric acid is an ingredient in some soft drinks.<\/p>\r\n\r\n<div class=\"textbox shaded\">\r\n<h3 class=\"title\">Sodium in Your Food<\/h3>\r\n<p id=\"ball-ch03_s04_p25\" class=\"para\">The element sodium, at least in its ionic form as Na<sup class=\"superscript\">+<\/sup>, is a necessary nutrient for humans to live. In fact, the human body is approximately 0.15% sodium, with the average person having one-twentieth to one-tenth of a kilogram in their body at any given time, mostly in fluids outside cells and in other bodily fluids.<\/p>\r\n<p id=\"ball-ch03_s04_p26\" class=\"para\">Sodium is also present in our diet. The common table salt we use on our foods is an ionic sodium compound. Many processed foods also contain significant amounts of sodium added to them as a variety of ionic compounds. Why are sodium compounds used so much? Usually sodium compounds are inexpensive, but, more importantly, most ionic sodium compounds dissolve easily. This allows processed food manufacturers to add sodium-containing substances to food mixtures and know that the compound will dissolve and distribute evenly throughout the food. Simple ionic compounds such as sodium nitrite (NaNO<sub class=\"subscript\">2<\/sub>) are added to cured meats, such as bacon and deli-style meats, while a compound called sodium benzoate is added to many packaged foods as a preservative. <a class=\"xref\" href=\"#ball-ch03_s04_t03\">Table 10 \"Some Sodium Compounds Added to Food\"<\/a> is a partial list of some sodium additives used in food. Some of them you may recognize after reading this chapter. Others you may not recognize, but they are all ionic sodium compounds with some negatively charged ion also present.<\/p>\r\n\r\n<div class=\"table\" id=\"ball-ch03_s04_t03\">\r\n<table style=\"border-spacing: 0px\" cellpadding=\"0\">\r\n<thead>\r\n<tr>\r\n<th>Sodium Compound<\/th>\r\n<th>Use in Food<\/th>\r\n<\/tr>\r\n<\/thead>\r\n<tbody>\r\n<tr>\r\n<td>Sodium acetate<\/td>\r\n<td>preservative, acidity regulator<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Sodium adipate<\/td>\r\n<td>food acid<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Sodium alginate<\/td>\r\n<td>thickener, vegetable gum, stabilizer, gelling agent, emulsifier<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Sodium aluminum phosphate<\/td>\r\n<td>acidity regulator, emulsifier<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Sodium aluminosilicate<\/td>\r\n<td>anticaking agent<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Sodium ascorbate<\/td>\r\n<td>antioxidant<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Sodium benzoate<\/td>\r\n<td>preservative<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Sodium bicarbonate<\/td>\r\n<td>mineral salt<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Sodium bisulfite<\/td>\r\n<td>preservative, antioxidant<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Sodium carbonate<\/td>\r\n<td>mineral salt<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Sodium carboxymethylcellulose<\/td>\r\n<td>emulsifier<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Sodium citrates<\/td>\r\n<td>food acid<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Sodium dehydroacetate<\/td>\r\n<td>preservative<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Sodium erythorbate<\/td>\r\n<td>antioxidant<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Sodium erythorbin<\/td>\r\n<td>antioxidant<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Sodium ethyl para-hydroxybenzoate<\/td>\r\n<td>preservative<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Sodium ferrocyanide<\/td>\r\n<td>anticaking agent<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Sodium formate<\/td>\r\n<td>preservative<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Sodium fumarate<\/td>\r\n<td>food acid<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Sodium gluconate<\/td>\r\n<td>stabilizer<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Sodium hydrogen acetate<\/td>\r\n<td>preservative, acidity regulator<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Sodium hydroxide<\/td>\r\n<td>mineral salt<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Sodium lactate<\/td>\r\n<td>food acid<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Sodium malate<\/td>\r\n<td>food acid<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Sodium metabisulfite<\/td>\r\n<td>preservative, antioxidant, bleaching agent<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Sodium methyl para-hydroxybenzoate<\/td>\r\n<td>preservative<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Sodium nitrate<\/td>\r\n<td>preservative, color fixative<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Sodium nitrite<\/td>\r\n<td>preservative, color fixative<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Sodium orthophenyl phenol<\/td>\r\n<td>preservative<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Sodium propionate<\/td>\r\n<td>preservative<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Sodium propyl para-hydroxybenzoate<\/td>\r\n<td>preservative<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Sodium sorbate<\/td>\r\n<td>preservative<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Sodium stearoyl lactylate<\/td>\r\n<td>emulsifier<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Sodium succinates<\/td>\r\n<td>acidity regulator, flavour enhancer<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Sodium salts of fatty acids<\/td>\r\n<td>emulsifier, stabilizer, anticaking agent<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Sodium sulfite<\/td>\r\n<td>mineral salt, preservative, antioxidant<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Sodium sulfite<\/td>\r\n<td>preservative, antioxidant<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Sodium tartrate<\/td>\r\n<td>food acid<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Sodium tetraborate<\/td>\r\n<td>preservative<\/td>\r\n<\/tr>\r\n<\/tbody>\r\n<\/table>\r\n<\/div>\r\n<strong><span class=\"title-prefix\">Table 10.<\/span><\/strong> Some Sodium Compounds Added to Food\r\n\r\nThe use of so many sodium compounds in prepared and processed foods has alarmed some physicians and nutritionists. They argue that the average person consumes too much sodium from his or her diet. The average person needs only about 500 mg of sodium every day; most people consume more than this\u2014up to 10 times as much. Some studies have implicated increased sodium intake with high blood pressure; newer studies suggest that the link is questionable. However, there has been a push to reduce the amount of sodium most people ingest every day: avoid processed and manufactured foods, read labels on packaged foods (which include an indication of the sodium content), don\u2019t oversalt foods, and use other herbs and spices besides salt in cooking.\r\n\r\n<\/div>\r\n<h2>Key Concepts and Summary<\/h2>\r\n<p id=\"fs-idp282340912\">Chemists use nomenclature rules to clearly name compounds. Ionic and molecular compounds are named using somewhat-different methods. Binary ionic compounds typically consist of a metal and a nonmetal. The name of the metal is written first, followed by the name of the nonmetal with its ending changed to \u2013<em>ide<\/em>. For example, K<sub>2<\/sub>O is called potassium oxide. If the metal can form ions with different charges, a Roman numeral in parentheses follows the name of the metal to specify its charge. Thus, FeCl<sub>2<\/sub> is iron(II) chloride and FeCl<sub>3<\/sub> is iron(III) chloride. Some compounds contain polyatomic ions; the names of common polyatomic ions should be memorized. Molecular compounds can form compounds with different ratios of their elements, so prefixes are used to specify the numbers of atoms of each element in a molecule of the compound. Examples include SF<sub>6<\/sub>, sulfur hexafluoride, and N<sub>2<\/sub>O<sub>4<\/sub>, dinitrogen tetroxide. Acids are an important class of compounds containing hydrogen and having special nomenclature rules. Binary acids are named using the prefix <em>hydro-<\/em>, changing the \u2013<em>ide<\/em> suffix to \u2013<em>ic<\/em>, and adding \u201cacid;\u201d HCl is hydrochloric acid. Oxyacids are named by changing the ending of the anion to \u2013<em>ic<\/em>, and adding \u201cacid;\u201d H<sub>2<\/sub>CO<sub>3<\/sub> is carbonic acid.<\/p>\r\n&nbsp;\r\n\r\n<\/section><a href=\"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/Flowchart.jpg\"><img width=\"916\" height=\"1190\" class=\"aligncenter wp-image-3484 size-full\" alt=\"\" src=\"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/Flowchart.jpg\" \/><\/a>\r\n\r\n<strong>Figure 3.<\/strong> Flowchart illustrating the thought process involved in naming simple ionic and covalent compounds and the rules needed to follow.\r\n<div class=\"textbox examples\">\r\n<h3 itemprop=\"educationalUse\">Activity<\/h3>\r\nMake yourself a stack of small sized Qcards. \u00a0On one side have the name of an ionic compound (e.g. sodium hydroxide) and on the other side have its chemical formula (e.g. NaOH). \u00a0Use every example found in this chapter - including those in the exercises. \u00a0Then use these Qcards to quiz yourself.\r\n\r\n<\/div>\r\n<section id=\"fs-idp282340144\" class=\"summary\">\r\n<div class=\"bcc-box bcc-info\">\r\n<h3>Exercises<\/h3>\r\n<div class=\"qandaset block\" id=\"ball-ch03_s02_qs01\">\r\n<div class=\"question\">\r\n<div class=\"qandaset block\" id=\"ball-ch03_s04_qs01\">\r\n\r\n<span style=\"font-size: 1em\">1. \u00a0Give the formula and name for each ionic compound formed between the two listed ions.<\/span>\r\n<div class=\"question\">\r\n\r\na) \u00a0Mg<sup class=\"superscript\">2+<\/sup> and Cl<sup class=\"superscript\">\u2212 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup>b) \u00a0Fe<sup class=\"superscript\">2+<\/sup> and O<sup class=\"superscript\">2\u2212 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup>c) \u00a0Fe<sup class=\"superscript\">3+<\/sup> and O<sup class=\"superscript\">2\u2212<\/sup>\r\n\r\n<\/div>\r\n2<span style=\"font-size: 1em\">. \u00a0Give the formula and name for each ionic compound formed between the two listed ions.<\/span>\r\n<div class=\"question\"><\/div>\r\n<div class=\"question\">\r\n\r\na) \u00a0Cu<sup class=\"superscript\">2+<\/sup> and F<sup class=\"superscript\">\u2212 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup>b) \u00a0Ca<sup class=\"superscript\">2+<\/sup> and O<sup class=\"superscript\">2\u2212 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup>c) \u00a0K<sup class=\"superscript\">+<\/sup> and P<sup class=\"superscript\">3\u2212<\/sup>\r\n\r\n<\/div>\r\n<span style=\"font-size: 1em\">3. \u00a0Give the formula and name for each ionic compound formed between the two listed ions.<\/span>\r\n<div class=\"question\">\r\n\r\na) \u00a0K<sup class=\"superscript\">+<\/sup> and SO<sub class=\"subscript\">4<\/sub><sup class=\"superscript\">2\u2212 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup>b) \u00a0NH<sub class=\"subscript\">4<\/sub><sup class=\"superscript\">+<\/sup> and S<sup class=\"superscript\">2\u2212 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup>c) \u00a0NH<sub class=\"subscript\">4<\/sub><sup class=\"superscript\">+<\/sup> and PO<sub class=\"subscript\">4<\/sub><sup class=\"superscript\">3\u2212<\/sup>\r\n\r\n<\/div>\r\n<span style=\"font-size: 1em\">4. \u00a0Give the formula and name for each ionic compound formed between the two listed ions.<\/span>\r\n<div class=\"question\"><\/div>\r\n<div class=\"question\">\r\n\r\na) \u00a0Pb<sup class=\"superscript\">4+<\/sup> and SO<sub class=\"subscript\">4<\/sub><sup class=\"superscript\">2\u2212 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup>b) \u00a0Na<sup class=\"superscript\">+<\/sup> and I<sub class=\"subscript\">3<\/sub><sup class=\"superscript\">\u2212 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup>c) \u00a0Li<sup class=\"superscript\">+<\/sup> and Cr<sub class=\"subscript\">2<\/sub>O<sub class=\"subscript\">7<\/sub><sup class=\"superscript\">2\u2212<\/sup>\r\n\r\n<\/div>\r\n5<span style=\"font-size: 1em\">. \u00a0Give the formula and name for each ionic compound formed between the two listed ions.<\/span>\r\n<div class=\"question\">\r\n\r\na) \u00a0Ag<sup class=\"superscript\">+<\/sup> and SO<sub class=\"subscript\">3<\/sub><sup class=\"superscript\">2\u2212 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup>b) \u00a0Na<sup class=\"superscript\">+<\/sup> and HCO<sub class=\"subscript\">3<\/sub><sup class=\"superscript\">\u2212 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup>c) \u00a0Fe<sup class=\"superscript\">3+<\/sup> and ClO<sub class=\"subscript\">3<\/sub><sup class=\"superscript\">\u2212<\/sup>\r\n\r\n<\/div>\r\n<span style=\"font-size: 1em\">6. .Which of these formulas represent molecules? State how many atoms are in each molecule.<\/span>\r\n\r\na) \u00a0Fe<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup>b) \u00a0PCl<sub class=\"subscript\">3<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup><\/sub>c) \u00a0P<sub class=\"subscript\">4<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup><\/sub>d) \u00a0Ar\r\n\r\n<span style=\"font-size: 1em\">7. \u00a0What is the difference between CO and Co?<\/span>\r\n\r\n<span style=\"font-size: 1em\">8. \u00a0Give the proper formula for each diatomic element.<\/span>\r\n\r\n<span style=\"font-size: 1em\">9. \u00a0What is the stem of fluorine used in molecule names? CF<\/span><sub class=\"subscript\">4<\/sub><span style=\"font-size: 1em\"> is one example.<\/span>\r\n\r\n<span style=\"font-size: 1em\">10. \u00a0Give the proper name for each molecule.<\/span>\r\n<div class=\"question\">\r\n\r\na) \u00a0PF<sub class=\"subscript\">3<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup><\/sub>b) \u00a0TeCl<sub class=\"subscript\">2<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup><\/sub>c) \u00a0N<sub class=\"subscript\">2<\/sub>O<sub class=\"subscript\">3<\/sub>\r\n\r\n<\/div>\r\n<div class=\"question\">\r\n<p id=\"ball-ch03_s02_qs01_p17\" class=\"para\">11. \u00a0Give the proper name for each molecule.<\/p>\r\na) \u00a0XeF<sub class=\"subscript\">2<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup><\/sub>b) \u00a0O<sub class=\"subscript\">2<\/sub>F<sub class=\"subscript\">2<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup><\/sub>c) \u00a0SF<sub class=\"subscript\">6<\/sub>\r\n\r\n<\/div>\r\n<div class=\"question\">\r\n<p id=\"ball-ch03_s02_qs01_p19\" class=\"para\">12. \u00a0Give the proper name for each molecule.<\/p>\r\na) \u00a0N<sub class=\"subscript\">2<\/sub>O<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup>b) \u00a0N<sub class=\"subscript\">2<\/sub>O<sub class=\"subscript\">4<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup><\/sub>c) \u00a0N<sub class=\"subscript\">2<\/sub>O<sub class=\"subscript\">5<\/sub>\r\n\r\n<\/div>\r\n<div class=\"question\">\r\n<p id=\"ball-ch03_s02_qs01_p21\" class=\"para\">13. \u00a0Give the proper formula for each name.<\/p>\r\na) \u00a0dinitrogen pentoxide<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup>b) \u00a0tetraboron tricarbide<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup>c) \u00a0phosphorus pentachloride\r\n\r\n<\/div>\r\n<span style=\"font-size: 1em\">14. \u00a0Give the proper formula for each name.<\/span>\r\n<div class=\"question\">\r\n\r\na) \u00a0dioxygen dichloride<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup>b) \u00a0dinitrogen trisulfide<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup>c) \u00a0xenon tetrafluoride\r\n\r\n<\/div>\r\n<span style=\"font-size: 1em\">15. \u00a0Give the proper formula for each name.<\/span>\r\n<div class=\"question\">\r\n\r\na) \u00a0iodine trifluoride<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup>b) \u00a0xenon trioxide<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup>c) \u00a0disulfur decafluoride\r\n\r\n<span style=\"font-size: 1em\">16. Give the formula for each acid.<\/span>\r\n\r\n<\/div>\r\n<div class=\"qandaset block\" id=\"ball-ch03_s05_qs01\">\r\n\r\na) \u00a0perchloric acid \u00a0 \u00a0 \u00a0 \u00a0\u00a0b) \u00a0hydroiodic acid\r\n<div class=\"question\">\r\n<p id=\"ball-ch03_s05_qs01_p3\" class=\"para\">17. Name each acid.<\/p>\r\na) \u00a0HF(aq) \u00a0 \u00a0 \u00a0 \u00a0\u00a0b) \u00a0HNO<sub class=\"subscript\">3<\/sub>(aq) \u00a0 \u00a0 \u00a0 \u00a0\u00a0c) \u00a0H<sub class=\"subscript\">2<\/sub>C<sub class=\"subscript\">2<\/sub>O<sub class=\"subscript\">4<\/sub>(aq)\r\n\r\n<span style=\"font-size: 1em\">18. Name the following compounds:<\/span>\r\n\r\n<\/div>\r\n<p id=\"fs-idp282298368\">a) CsCl \u00a0 \u00a0 \u00a0 \u00a0\u00a0b) BaO \u00a0 \u00a0 \u00a0 \u00a0\u00a0c) K<sub>2<\/sub>S \u00a0 \u00a0 \u00a0 \u00a0\u00a0d) BeCl<sub>2 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sub>e) HBr \u00a0 \u00a0 \u00a0 \u00a0\u00a0f) AlF<sub>3<\/sub><\/p>\r\n19. Write the formulas of the following compounds:\r\n<p id=\"fs-idm306848\">a) rubidium bromide \u00a0 \u00a0 \u00a0 \u00a0\u00a0b) magnesium selenide \u00a0 \u00a0 \u00a0 \u00a0\u00a0c) sodium oxide \u00a0 \u00a0 \u00a0 \u00a0\u00a0d) calcium chloride<\/p>\r\n<p id=\"fs-idm305184\">e) hydrogen fluoride \u00a0 \u00a0 \u00a0 \u00a0\u00a0f) gallium phosphide \u00a0 \u00a0 \u00a0 \u00a0\u00a0g) aluminum bromide \u00a0 \u00a0 \u00a0 \u00a0\u00a0h) ammonium sulfate<\/p>\r\n20. Write the formulas of the following compounds:\r\n<p id=\"fs-idp268322592\">a) chlorine dioxide \u00a0 \u00a0 \u00a0 \u00a0\u00a0b) dinitrogen tetraoxide \u00a0 \u00a0 \u00a0 \u00a0\u00a0c) potassium phosphide<\/p>\r\n<p id=\"fs-idp268323808\">d) silver(I) sulfide \u00a0 \u00a0 \u00a0 \u00a0\u00a0e) aluminum nitride \u00a0 \u00a0 \u00a0 \u00a0\u00a0f) silicon dioxide<\/p>\r\n21. Each of the following compounds contains a metal that can exhibit more than one ionic charge. Name these compounds:\r\n<p id=\"fs-idp279516416\">a) Cr<sub>2<\/sub>O<sub>3 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sub>b) FeCl<sub>2 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sub>c) CrO<sub>3 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sub>d) TiCl<sub>4 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sub>e) CoO \u00a0 \u00a0 \u00a0 \u00a0\u00a0f) MoS<sub>2<\/sub><\/p>\r\n22. The following ionic compounds are found in common household products. Write the formulas for each compound:\r\n<p id=\"fs-idp268366192\">a) potassium phosphate \u00a0 \u00a0 \u00a0 \u00a0\u00a0b) copper(II) sulfate \u00a0 \u00a0 \u00a0 \u00a0\u00a0c) calcium chloride<\/p>\r\n<p id=\"fs-idp282328976\">d) titanium dioxide \u00a0 \u00a0 \u00a0 \u00a0\u00a0e) ammonium nitrate<\/p>\r\nf) sodium bisulfate (the common name for sodium hydrogen sulfate)\r\n\r\n23. What are the IUPAC names of the following compounds?\r\n<p id=\"fs-idp268311808\">a) manganese dioxide \u00a0 \u00a0 \u00a0 \u00a0\u00a0b) mercurous chloride (Hg<sub>2<\/sub>Cl<sub>2<\/sub>) \u00a0 \u00a0 \u00a0 \u00a0\u00a0c) ferric nitrate [Fe(NO<sub>3<\/sub>)<sub>3<\/sub>]<\/p>\r\n<p id=\"fs-idp282287056\">d) titanium tetrachloride \u00a0 \u00a0 \u00a0 \u00a0\u00a0e) cupric bromide (CuBr<sub>2<\/sub>)<\/p>\r\n\r\n<\/div>\r\n&nbsp;\r\n\r\n<\/div>\r\n<b>Answers<\/b>\r\n\r\n1. a) \u00a0magnesium chloride, MgCl<sub class=\"subscript\">2<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup><\/sub>b) \u00a0iron(II) oxide, FeO<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup>c) \u00a0iron(III) oxide, Fe<sub class=\"subscript\">2<\/sub>O<sub class=\"subscript\">3<\/sub>\r\n\r\n2.\u00a0a) \u00a0copper(II) fluoride, CuF<sub class=\"subscript\">2<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup><\/sub>b) \u00a0calcium oxide, CaO<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup>c) \u00a0potassium phosphide, K<sub class=\"subscript\">3<\/sub>P\r\n\r\n3.\u00a0a) \u00a0potassium sulfate, K<sub class=\"subscript\">2<\/sub>SO<sub class=\"subscript\">4<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup><\/sub>b) \u00a0ammonium sulfide, (NH<sub class=\"subscript\">4<\/sub>)<sub class=\"subscript\">2<\/sub>S<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup>c) \u00a0ammonium phosphate, (NH<sub class=\"subscript\">4<\/sub>)<sub class=\"subscript\">3<\/sub>PO<sub class=\"subscript\">4<\/sub>\r\n\r\n4.\u00a0a) \u00a0lead(IV) sulfate, Pb(SO<sub class=\"subscript\">4<\/sub>)<sub class=\"subscript\">2<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup><\/sub>b) \u00a0sodium triiodide, NaI<sub class=\"subscript\">3<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup><\/sub>c) \u00a0lithium dichromate, Li<sub class=\"subscript\">2<\/sub>Cr<sub class=\"subscript\">2<\/sub>O<sub class=\"subscript\">7<\/sub>\r\n\r\n5.\u00a0a) \u00a0silver sulfite, Ag<sub class=\"subscript\">2<\/sub>SO<sub class=\"subscript\">3<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup><\/sub>b) \u00a0sodium hydrogen carbonate, NaHCO<sub class=\"subscript\">3<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup><\/sub>c) \u00a0iron(III) chlorate, Fe(ClO<sub class=\"subscript\">3<\/sub>)<sub class=\"subscript\">3<\/sub>\r\n\r\n6. a) \u00a0not a molecule<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup>b) \u00a0a molecule; four atoms total<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup>c) \u00a0a molecule; four atoms total\r\n\r\nd) \u00a0not a molecule\r\n\r\n<span style=\"font-size: 1em\">7.\u00a0CO is a compound of carbon and oxygen; Co is the element cobalt.<\/span>\r\n\r\n8.\u00a0H<sub class=\"subscript\">2<\/sub>, O<sub class=\"subscript\">2<\/sub>, N<sub class=\"subscript\">2<\/sub>, F<sub class=\"subscript\">2<\/sub>, Cl<sub class=\"subscript\">2<\/sub>, Br<sub class=\"subscript\">2<\/sub>, I<sub class=\"subscript\">2<\/sub>\r\n\r\n9. \u00a0<em class=\"emphasis\">fluor-<\/em>\r\n\r\n10.\u00a0a) \u00a0phosphorus trifluoride<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup>b) \u00a0tellurium dichloride<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup>c) \u00a0dinitrogen trioxide\r\n\r\n11.\u00a0a) \u00a0xenon difluoride<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup>b) \u00a0dioxygen difluoride<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup>c) \u00a0sulfur hexafluoride\r\n\r\n12.\u00a0a) \u00a0dinitrogen monoxide<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup>b) \u00a0dinitrogen tetroxide<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup>c) \u00a0dinitrogen pentoxide\r\n\r\n13.\u00a0a) \u00a0N<sub class=\"subscript\">2<\/sub>O<sub class=\"subscript\">5<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup><\/sub>b) \u00a0B<sub class=\"subscript\">4<\/sub>C<sub class=\"subscript\">3<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup><\/sub>c) \u00a0PCl<sub class=\"subscript\">5<\/sub>\r\n\r\n14.\u00a0a) \u00a0O<sub class=\"subscript\">2<\/sub>Cl<sub class=\"subscript\">2<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup><\/sub>b) \u00a0N<sub class=\"subscript\">2<\/sub>S<sub class=\"subscript\">3<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup><\/sub>c) \u00a0XeF<sub class=\"subscript\">4<\/sub>\r\n\r\n15.\u00a0a) \u00a0IF<sub class=\"subscript\">3<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup><\/sub>b) \u00a0XeO<sub class=\"subscript\">3<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup><\/sub>c) \u00a0S<sub class=\"subscript\">2<\/sub>F<sub class=\"subscript\">10<\/sub>\r\n\r\n<\/div>\r\n16.\u00a0<span style=\"font-size: 1em\">a) \u00a0HClO<\/span><sub class=\"subscript\">4<\/sub><span style=\"font-size: 1em\">(aq) \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/span><span style=\"font-size: 1em\">b) \u00a0HI(aq)<\/span>\r\n\r\n<\/div>\r\n17.\u00a0a) \u00a0hydrofluoric acid \u00a0 \u00a0 \u00a0 \u00a0\u00a0b) \u00a0nitric acid \u00a0 \u00a0 \u00a0 \u00a0\u00a0c) \u00a0oxalic acid\r\n<p id=\"fs-idp283374992\">18. a) cesium chloride \u00a0 \u00a0 \u00a0 \u00a0 b) barium oxide \u00a0 \u00a0 \u00a0 \u00a0 c) potassium sulfide<\/p>\r\nd) beryllium chloride \u00a0 \u00a0 \u00a0 \u00a0 e) hydrogen bromide \u00a0 \u00a0 \u00a0 \u00a0 f) aluminum fluoride\r\n<p id=\"fs-idm303264\">19. a) RbBr \u00a0 \u00a0 \u00a0 \u00a0 b) MgSe \u00a0 \u00a0 \u00a0 \u00a0 c) Na<sub>2<\/sub>O \u00a0 \u00a0 \u00a0 \u00a0 d) CaCl<sub>2 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sub>e) HF \u00a0 \u00a0 \u00a0 \u00a0 f) GaP \u00a0 \u00a0 \u00a0 \u00a0 g) AlBr<sub>3 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sub>h) (NH<sub>4<\/sub>)<sub>2<\/sub>SO<sub>4<\/sub><\/p>\r\n<p id=\"fs-idp268325312\">20. a) ClO<sub>2 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sub>b) N<sub>2<\/sub>O<sub>4 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sub>c) K<sub>3<\/sub>P \u00a0 \u00a0 \u00a0 \u00a0 d) Ag<sub>2<\/sub>S \u00a0 \u00a0 \u00a0 \u00a0 e) AlN \u00a0 \u00a0 \u00a0 \u00a0 f) SiO<sub>2<\/sub><\/p>\r\n<p id=\"fs-idp268274112\">21. a) chromium(III) oxide \u00a0 \u00a0 \u00a0 \u00a0 b) iron(II) chloride \u00a0 \u00a0 \u00a0 \u00a0 c) chromium(VI) oxide<\/p>\r\nd) titanium(IV) chloride \u00a0 \u00a0 \u00a0 \u00a0 e) cobalt(II) oxide \u00a0 \u00a0 \u00a0 \u00a0 f) molybdenum(IV) sulfide\r\n<p id=\"fs-idp282330448\">22. a) K<sub>3<\/sub>PO<sub>4 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sub>b) CuSO<sub>4 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sub>c) CaCl<sub>2 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sub>d) TiO<sub>2 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sub>e) NH<sub>4<\/sub>NO<sub>3 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sub>f) NaHSO<sub>4<\/sub><\/p>\r\n<p id=\"fs-idp282288464\">23. a) manganese(IV) oxide \u00a0 \u00a0 \u00a0 \u00a0 b) mercury(I) chloride \u00a0 \u00a0 \u00a0 \u00a0 c) iron(III) nitrate<\/p>\r\nd) titanium(IV) chloride \u00a0 \u00a0 \u00a0 \u00a0 e) copper(II) bromide\r\n\r\n<\/div>\r\n<\/section>\r\n<div>\r\n<h2>Glossary<\/h2>\r\n<strong>binary acid:\u00a0<\/strong>compound that contains hydrogen and one other element, bonded in a way that imparts acidic properties to the compound (ability to release H<sup>+<\/sup> ions when dissolved in water)\r\n\r\n<strong>binary compound:\u00a0<\/strong>compound containing two different elements.\r\n\r\n<strong>nomenclature:\u00a0<\/strong>system of rules for naming objects of interest\r\n\r\n<strong>oxyacid:\u00a0<\/strong>compound that contains hydrogen, oxygen, and one other element, bonded in a way that imparts acidic properties to the compound (ability to release H<sup>+<\/sup> ions when dissolved in water)\r\n\r\n<\/div>","rendered":"<div class=\"bcc-box bcc-highlight\">\n<h3>Learning Objectives<\/h3>\n<p>By the end of this module, you will be able to:<\/p>\n<ul>\n<li>Derive names for common types of inorganic compounds and simple molecular compounds using a systematic approach<\/li>\n<\/ul>\n<\/div>\n<p id=\"fs-idp268117168\"><strong>Nomenclature<\/strong>, a collection of rules for naming things, is important in science and in many other situations. This module describes an approach that is used to name simple ionic and molecular compounds, such as NaCl, CaCO<sub>3<\/sub>, and N<sub>2<\/sub>O<sub>4<\/sub>. The simplest of these are <strong>binary compounds<\/strong>, those containing only two elements, but we will also consider how to name ionic compounds containing polyatomic ions, and one specific, very important class of compounds known as <strong class=\"no-emphasis\">acids<\/strong>\u00a0&#8211; subsequent chapters in this text will focus on these compounds in great detail. We will limit our attention here to inorganic compounds, compounds that are composed principally of elements other than carbon, and will follow the nomenclature guidelines proposed by IUPAC. The rules for organic compounds, in which carbon is the principle element, will be treated in a later chapter on organic chemistry.<\/p>\n<section id=\"fs-idp268266480\">\n<h2>Nomenclature of Ionic Compounds<\/h2>\n<p id=\"fs-idp268131792\">To name an inorganic compound, we need to consider the answers to several questions. First, is the compound ionic or molecular? If the compound is ionic, does the metal form ions of only one type (fixed charge) or more than one type (variable charge)? Are the ions monatomic or polyatomic? If the compound is molecular, does it contain hydrogen? If so, does it also contain oxygen? From the answers we derive, we place the compound in an appropriate category and then name it accordingly.<\/p>\n<section id=\"fs-idm335792\">\n<h2>Compounds Containing Only Monatomic Ions<\/h2>\n<p id=\"fs-idp279143120\">The name of a binary compound containing monatomic ions consists of the name of the cation (the name of the metal) followed by the name of the anion (the name of the nonmetallic element with its ending replaced by the suffix \u2013<em>ide<\/em>). Some examples are given in <a class=\"autogenerated-content\" href=\"#fs-idp282234816\">Table 1<\/a>.<\/p>\n<table id=\"fs-idp282234816\" summary=\"The examples of ionic compounds shown in this table are N a C l sodium chloride, K B r potassium bromide, C a I subscript 2 calcium iodide, C s F cesium fluoride, L i C l lithium chloride, N a subscript 2 O sodium oxide, C d S cadmium sulfide, M g subscript 3 N subscript 2 magnesium nitride, C a subscript 3 P subscript 2 calcium phosphide, and A l subscript 4 C subscript 3 aluminum carbide.\">\n<tbody>\n<tr>\n<td>NaCl, sodium chloride<\/td>\n<td>Na<sub>2<\/sub>O, sodium oxide<\/td>\n<\/tr>\n<tr>\n<td>KBr, potassium bromide<\/td>\n<td>CdS, cadmium sulfide<\/td>\n<\/tr>\n<tr>\n<td>CaI<sub>2<\/sub>, calcium iodide<\/td>\n<td>Mg<sub>3<\/sub>N<sub>2<\/sub>, magnesium nitride<\/td>\n<\/tr>\n<tr>\n<td>CsF, cesium fluoride<\/td>\n<td>Ca<sub>3<\/sub>P<sub>2<\/sub>, calcium phosphide<\/td>\n<\/tr>\n<tr>\n<td>LiCl, lithium chloride<\/td>\n<td>Al<sub>4<\/sub>C<sub>3<\/sub>, aluminum carbide<\/td>\n<\/tr>\n<tr>\n<td colspan=\"2\"><strong>Table 1.<\/strong> Names of Some Ionic Compounds<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<\/section>\n<section id=\"fs-idp279293712\">\n<h2>Compounds Containing Polyatomic Ions<\/h2>\n<p id=\"fs-idp282236928\">Compounds containing polyatomic ions are named similarly to those containing only monatomic ions, except there is no need to change to an \u2013<em>ide<\/em> ending, since the suffix is already present in the name of the anion. Examples are shown in <a class=\"autogenerated-content\" href=\"#fs-idp279316112\">Table 2<\/a>. \u00a0See <a class=\"autogenerated-content\" href=\"https:\/\/opentextbc.ca\/chemistry\/chapter\/2-6-molecular-and-ionic-compounds\/#CNX_Chem_02_06_IonCharges\" target=\"_blank\" rel=\"noopener\">Table 1 in Chapter 4.2 Ionic and Molecular Compounds<\/a>\u00a0for the list of common polyatomic ions.<\/p>\n<table id=\"fs-idp279316112\" class=\"span-all\" summary=\"The examples of polyatomic ionic compounds shown in this table are K C subscript 2 H subscript 3 O subscript 2 potassium acetate, N a H C O subscript 3 sodium bicarbonate, A l subscript 2 ( C O subscript 3 ) subscript 3 aluminum carbonate, (N H subscript 4) CL, ammonium chloride, C a S O subscript 4 calcium sulfate, and M g subscript 3 ( P O subscript 4 ) subscript 2 magnesium phosphate.\">\n<tbody>\n<tr>\n<td>KC<sub>2<\/sub>H<sub>3<\/sub>O<sub>2<\/sub>, potassium acetate<\/td>\n<td>(NH<sub>4<\/sub>)Cl, ammonium chloride<\/td>\n<\/tr>\n<tr>\n<td>NaHCO<sub>3<\/sub>, sodium bicarbonate<\/td>\n<td>CaSO<sub>4<\/sub>, calcium sulfate<\/td>\n<\/tr>\n<tr>\n<td>Al<sub>2<\/sub>(CO<sub>3<\/sub>)<sub>3<\/sub>, aluminum carbonate<\/td>\n<td>Mg<sub>3<\/sub>(PO<sub>4<\/sub>)<sub>2<\/sub>, magnesium phosphate<\/td>\n<\/tr>\n<tr>\n<td colspan=\"3\"><strong>Table 2.<\/strong> Names of Some Polyatomic Ionic Compounds<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<\/section>\n<\/section>\n<div>\n<div class=\"textbox shaded\">\n<h3 class=\"title\">Example 1<\/h3>\n<h3 class=\"title\"><span style=\"font-family: Tinos, Georgia, serif;font-size: 1em;font-weight: normal\">Name the following ionic compounds:<\/span><\/h3>\n<h3 class=\"title\"><span lang=\"ES-MX\" style=\"font-family: Tinos, Georgia, serif;font-size: 1em;font-weight: normal\">a)\u00a0 NaCl\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 b)\u00a0AlBr<sub>3<\/sub>\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 c)\u00a0 BaH<sub>2<\/sub><\/span><\/h3>\n<p class=\"Solution\"><strong>Solution\u00a0\u00a0 <\/strong><\/p>\n<p class=\"Indentpoints\">a)<span>\u00a0 <\/span>Identify the cation and anion.<br \/>\nNa is a Group 1 metal, and thus it forms the cation Na<sup>+<\/sup>, called \u201csodium\u201d ion.<br \/>\nCl is a nonmetal, and forms the anion Cl<sup>&#8211;<\/sup>, chloride.<span>\u00a0 <\/span>Thus, NaCl = sodium chloride.<\/p>\n<p class=\"Indentpoints\">b)<span>\u00a0 <\/span>AlBr<sub>3\u00a0<\/sub>consists of aluminum and bromine; we call it aluminum bromide.<\/p>\n<p class=\"Indentpoints\">c)<span>\u00a0 <\/span>BaH<sub>2<\/sub>is called barium hydride.<\/p>\n<p>&nbsp;<\/p>\n<p class=\"SelfTest\"><em><strong>Test Yourself<\/strong><\/em><\/p>\n<p class=\"Indent\">Name the following ionic compounds:<\/p>\n<p class=\"Indent\"><span>\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span>a)<span>\u00a0 <\/span>Al<sub>2<\/sub>S<sub>3<\/sub><span>\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span>b)<span>\u00a0<\/span>ZnS<span>\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span>c)<span>\u00a0 <\/span>MgI<sub>2<\/sub><\/p>\n<p>&nbsp;<\/p>\n<p class=\"Answers\"><span lang=\"PT-BR\"><em><strong>Answers<\/strong><\/em><\/span><\/p>\n<p class=\"Answers\"><span lang=\"PT-BR\">a) aluminum sulfide \u00a0 \u00a0 \u00a0 \u00a0\u00a0b) zinc sulfide \u00a0 \u00a0 \u00a0 \u00a0\u00a0c) magnesium iodide<\/span><\/p>\n<\/div>\n<\/div>\n<section id=\"fs-idp268266480\">\n<section id=\"fs-idp282353488\">\n<h2>Compounds Containing a Metal Ion with a Variable Charge<\/h2>\n<p id=\"fs-idp282354128\">Most of the transition metals can form two or more cations with different charges. Compounds of these metals with nonmetals are named with the same method as compounds in the first category, except the charge of the metal ion is specified by a Roman numeral in parentheses after the name of the metal. The charge of the metal ion is determined from the formula of the compound and the charge of the anion. For example, consider binary ionic compounds of iron and chlorine. Iron typically exhibits a charge of either 2+ or 3+ (see <a class=\"autogenerated-content\" href=\"https:\/\/opentextbc.ca\/chemistry\/chapter\/2-6-molecular-and-ionic-compounds\/#CNX_Chem_02_06_IonCharges\" target=\"_blank\" rel=\"noopener\">Figure 2 in Chapter 4.2 Ionic and Molecular Compounds<\/a>), and the two corresponding compound formulas are FeCl<sub>2<\/sub> and FeCl<sub>3<\/sub>. The simplest name, \u201ciron chloride,\u201d will, in this case, be ambiguous, as it does not distinguish between these two compounds. In cases like this, the charge of the metal ion is included as a Roman numeral in parentheses immediately following the metal name. These two compounds are then unambiguously named iron(II) chloride and iron(III) chloride, respectively. Other examples are provided in <a class=\"autogenerated-content\" href=\"#fs-idp282283328\">Table 4<\/a>.<\/p>\n<table id=\"fs-idp282283328\" class=\"span-all\" summary=\"The transition metal ionic compound examples included in this table are F e C L subscript 3 or iron three chloride, H g subscript 2 O or mercury one oxide, H g O or mercury two oxide, and C u subscript 3 ( P O subscript 4 ) subscript 2 or copper two phosphate.\">\n<thead>\n<tr>\n<th>Transition Metal Ionic Compound<\/th>\n<th>Name<\/th>\n<\/tr>\n<\/thead>\n<tbody>\n<tr>\n<td>FeCl<sub>3<\/sub><\/td>\n<td>iron(III) chloride<\/td>\n<\/tr>\n<tr>\n<td>Hg<sub>2<\/sub>O<\/td>\n<td>mercury(I) oxide<\/td>\n<\/tr>\n<tr>\n<td>HgO<\/td>\n<td>mercury(II) oxide<\/td>\n<\/tr>\n<tr>\n<td>Cu<sub>3<\/sub>(PO<sub>4<\/sub>)<sub>2<\/sub><\/td>\n<td>copper(II) phosphate<\/td>\n<\/tr>\n<tr>\n<td colspan=\"2\"><strong>Table 4.<\/strong> Names of Some Transition Metal Ionic Compounds<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<p id=\"fs-idp268391888\">An old naming convention used the suffixes \u2013<em>ic<\/em> and \u2013<em>ous<\/em> to designate metals with higher and lower charges, respectively: Iron(III) chloride, FeCl<sub>3<\/sub>, can be called called ferric chloride, and iron(II) chloride, FeCl<sub>2<\/sub>, is also known as ferrous chloride. \u00a0This older naming convention remains in use by some segments of industry. For example, you may see the words <em>stannous fluoride<\/em> on a tube of toothpaste. This represents the formula SnF<sub>2<\/sub>, which is also named tin(II) fluoride following the more current convention. The other fluoride of tin is SnF<sub>4<\/sub>, is now named tin(IV) fluoride but is still often referred to as stannic fluoride. \u00a0Knowing both convention remains important.<\/p>\n<table id=\"fs-idp268340336\" class=\"span-all\" style=\"height: 240px\" summary=\"This table has three columns labeled \u201cformula\u201d, \u201canion name\u201d, and \u201cacid name\u201d. H C subscript 2 H subscript 3 O subscript 2 is named acetate or acetic acid. H N O subscript 3 is named nitrate or nitric acid. H N O subscript 2 is named nitrite or nitrous acid, H C l O subscript 4 is named perchlorate or perchloric acid. H subscript 2 C O subscript 3 is named carbonate or carbonic acid. H subscript 2 S O subscript 4 is named sulfate or sulfuric acid. H subscript 2 S O subscript 3 is named sulfite or sulfurous acid. H subscript 3 P O subscript 4 is named phosphate or phosphoric acid.\">\n<thead>\n<tr style=\"height: 24px\">\n<th style=\"height: 24px;width: 83px\">Element<\/th>\n<th style=\"height: 24px;width: 137px\">Common Ions<\/th>\n<th style=\"height: 24px;width: 238px\">Common Names for Ions<\/th>\n<\/tr>\n<\/thead>\n<tbody>\n<tr style=\"height: 24px\">\n<td style=\"height: 24px;width: 83px\">Cu<\/td>\n<td style=\"height: 24px;width: 137px\">Cu<sup>+<\/sup>\/Cu<sup>2+<\/sup><\/td>\n<td style=\"height: 24px;width: 238px\">cuprous\/cupric<\/td>\n<\/tr>\n<tr style=\"height: 24px\">\n<td style=\"height: 24px;width: 83px\">Fe<\/td>\n<td style=\"height: 24px;width: 137px\">Fe<sup>2+<\/sup>\/Fe<sup>3+<\/sup><\/td>\n<td style=\"height: 24px;width: 238px\">ferrous\/ferric<\/td>\n<\/tr>\n<tr style=\"height: 24px\">\n<td style=\"height: 24px;width: 83px\">Co<\/td>\n<td style=\"height: 24px;width: 137px\">Co<sup>2+<\/sup>\/Co<sup>3+<\/sup><\/td>\n<td style=\"height: 24px;width: 238px\">cobaltous\/cobaltic<\/td>\n<\/tr>\n<tr>\n<td style=\"width: 83px\">Cr<\/td>\n<td style=\"width: 137px\">Cr<sup>2+<\/sup>\/Cr<sup>3+<\/sup><\/td>\n<td style=\"width: 238px\">chromous\/chromic<\/td>\n<\/tr>\n<tr style=\"height: 24px\">\n<td style=\"height: 24px;width: 83px\">Sn<\/td>\n<td style=\"height: 24px;width: 137px\">Sn<sup>2+<\/sup>\/Sn<sup>4+<\/sup><\/td>\n<td style=\"height: 24px;width: 238px\">stannous\/stannic<\/td>\n<\/tr>\n<tr style=\"height: 24px\">\n<td style=\"height: 24px;width: 83px\">Pb<\/td>\n<td style=\"height: 24px;width: 137px\">Pb<sup>2+<\/sup>\/Pb<sup>4+<\/sup><\/td>\n<td style=\"height: 24px;width: 238px\">plumbous\/plumbic<\/td>\n<\/tr>\n<tr style=\"height: 24px\">\n<td style=\"height: 24px;width: 83px\">Hg<\/td>\n<td style=\"height: 24px;width: 137px\">Hg<sub>2<\/sub><sup>2+<\/sup>\/Hg<sup>2+<\/sup><\/td>\n<td style=\"height: 24px;width: 238px\">mercurous\/mercuric<\/td>\n<\/tr>\n<tr style=\"height: 24px\">\n<td style=\"height: 24px;width: 458px\" colspan=\"3\"><strong>Table 5.<\/strong>\u00a0Common Names for Some Metal Ions with Variable Charges<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<div class=\"textbox shaded\">\n<h3 class=\"title\">Example 2<\/h3>\n<p id=\"ball-ch03_s04_p07\" class=\"para\">Name each species.<\/p>\n<p class=\"para\">a) O<sup class=\"superscript\">2\u2212 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup>b) Co \u00a0 \u00a0 \u00a0 \u00a0 c)\u00a0Co<sup class=\"superscript\">2+<\/sup><\/p>\n<p>&nbsp;<\/p>\n<p class=\"simpara\"><strong>Solution<\/strong><\/p>\n<p class=\"simpara\">a) This species has a 2\u2212 charge on it, so it is an anion. Anions are named using the stem of the element name with the suffix <em class=\"emphasis\">-ide<\/em> added. This is the oxide anion.<\/p>\n<p class=\"simpara\">b) Because this species has no charge, it is an atom in its elemental form. This is cobalt.<\/p>\n<p class=\"simpara\">c) In this case, there is a 2+\u00a0charge on the atom, so it is a cation. We note from <a class=\"autogenerated-content\" href=\"https:\/\/opentextbc.ca\/chemistry\/chapter\/2-6-molecular-and-ionic-compounds\/#CNX_Chem_02_06_IonCharges\" target=\"_blank\" rel=\"noopener\">Figure 2 in Chapter 4.2 Ionic and Molecular Compounds<\/a>),\u00a0that cobalt cations can have two possible charges, so the name of the ion must specify which charge the ion has. This is the cobalt(II) cation.<\/p>\n<p>&nbsp;<\/p>\n<p class=\"simpara\"><strong><em class=\"emphasis bolditalic\">Test Yourself<\/em><\/strong><\/p>\n<p id=\"ball-ch03_s04_p08\" class=\"para\">Name each species:\u00a0P<sup class=\"superscript\">3\u2212 \u00a0<\/sup>and Sr<sup class=\"superscript\">2+<\/sup><\/p>\n<p>&nbsp;<\/p>\n<p class=\"simpara\"><strong><em class=\"emphasis\">Answers<\/em><\/strong><\/p>\n<p class=\"simpara\">the phosphide anion and\u00a0the strontium cation<\/p>\n<\/div>\n<div class=\"textbox shaded\">\n<h3 class=\"title\">Example 3<\/h3>\n<p class=\"Indent\">Name the following ionic compounds:<\/p>\n<p class=\"Indent\"><span>\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span><span lang=\"ES-MX\">a)<span>\u00a0 <\/span>SnBr<sub>4<\/sub><span>\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span>b)<span>\u00a0<\/span>CoCl<sub>3<\/sub><span>\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span>c)<span>\u00a0 <\/span>Fe<sub>2<\/sub>O<sub>3<\/sub><\/span><\/p>\n<p>&nbsp;<\/p>\n<p class=\"Solution\"><strong>Solution\u00a0\u00a0 <\/strong><\/p>\n<p class=\"Indentpoints\">a)<span>\u00a0\u00a0 <\/span>First, identify the charge on the cation (Sn).<\/p>\n<p class=\"Indentpoints\">Because Br has a charge of \u20131, we know that Sn must have a charge of +4.<\/p>\n<p class=\"Indentpoints\"><span>\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span>0 = 1(x) + 4(-1)<span>\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span>x = +4 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<span><\/span>Therefore SnBr<sub>4<\/sub>=<span>\u00a0 <\/span>tin(IV) bromide<\/p>\n<p class=\"Indentpoints\">b)<span>\u00a0 <\/span>Cl adopts a charge of \u20131<\/p>\n<p class=\"Indentpoints\"><span>\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span>0 = 1(x) + 3(-1)<span>\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span>x = +3 \u00a0 \u00a0 \u00a0 \u00a0\u00a0Therefore CoCl<sub>3<\/sub>= cobalt(III) chloride<\/p>\n<p class=\"Indentpoints\">c)<span>\u00a0 <\/span>O adopts a charge of \u20132<\/p>\n<p class=\"Indentpoints\"><span>\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span>0 = 2(x) + 3(-2)<span>\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span>x = +3 \u00a0 \u00a0 \u00a0 \u00a0\u00a0Therefore Fe<sub>2<\/sub>O<sub>3<\/sub>= iron(III) oxide<\/p>\n<p>&nbsp;<\/p>\n<p class=\"SelfTest\"><em><strong>Test Yourself<\/strong><\/em><\/p>\n<p class=\"Indent\">Name the following ionic compounds:<\/p>\n<p class=\"Indent\"><span>\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span>a)<span>\u00a0 <\/span>HgO<span>\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span>b)<span>\u00a0 <\/span>PbCl<sub>4<\/sub><span>\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span>c) PbS \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 d) Sc<sub class=\"subscript\">2<\/sub>O<sub class=\"subscript\">3<\/sub> \u00a0 \u00a0 \u00a0 \u00a0 e)\u00a0AgCl<\/p>\n<p>&nbsp;<\/p>\n<p class=\"Answers\"><em><strong>Answers<\/strong><\/em><\/p>\n<p class=\"Answers\">a) mercury(II) oxide \u00a0 \u00a0 \u00a0 \u00a0 b) lead(IV) chloride \u00a0 \u00a0 \u00a0 \u00a0\u00a0c) lead(II) sulphide<\/p>\n<p class=\"Answers\">d) scandium oxide \u00a0 \u00a0 \u00a0 \u00a0 e)\u00a0silver chloride<\/p>\n<\/div>\n<div class=\"textbox shaded\" id=\"fs-idm194224\">\n<h3>Example 4<\/h3>\n<p id=\"fs-idm193552\">Name the following ionic compounds:<\/p>\n<p id=\"fs-idm193056\">a) Fe<sub>2<\/sub>S<sub>3 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sub>b) CuSe \u00a0 \u00a0 \u00a0 \u00a0\u00a0c) GaN \u00a0 \u00a0 \u00a0 \u00a0\u00a0d) CrCl<sub>3 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sub>e) Ti<sub>2<\/sub>(SO<sub>4<\/sub>)<sub>3 \u00a0 \u00a0 \u00a0<\/sub> \u00a0\u00a0f) Co<sub class=\"subscript\">2<\/sub>O<sub class=\"subscript\">3<\/sub>\u00a0 \u00a0 \u00a0 \u00a0 \u00a0g)\u00a0CaCl<sub class=\"subscript\">2<\/sub>\u00a0 \u00a0 \u00a0 \u00a0 \u00a0h) AlF<sub class=\"subscript\">3<\/sub><\/p>\n<p>&nbsp;<\/p>\n<p id=\"fs-idp282326320\"><strong>Solution<\/strong><br \/>\nThe anions in these compounds have a fixed negative charge (S<sup>2\u2212<\/sup>, Se<sup>2\u2212 <\/sup>, N<sup>3\u2212<\/sup>, Cl<sup>\u2212<\/sup>, SO<sub>4<\/sub><sup>2\u2212<\/sup>,\u00a0O<sup>\u22122<\/sup>, and F<sup>\u2212<\/sup>), and the compounds must be neutral. Because the metal ions in questions a) to f) have a variable charge, we must figure out the charge of the metal ion by ensuring that the total number of positive charges in each compound must equal the total number of negative charges. \u00a0Therefore the positive ions must be Fe<sup>3+<\/sup>, Cu<sup>2+<\/sup>, Ga<sup>3+<\/sup>, Cr<sup>3+<\/sup>, Ti<sup>3+<\/sup>\u00a0and Co<sup>3+<\/sup>. These charges are used in the names of the metal ions:<\/p>\n<p id=\"fs-idm104688\">a) iron(III) sulfide \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 b) copper(II) selenide \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 c) gallium(III) nitride<\/p>\n<p>d) chromium(III) chloride \u00a0 \u00a0 \u00a0 \u00a0\u00a0e) titanium(III) sulfate \u00a0 \u00a0 \u00a0 \u00a0 \u00a0f)\u00a0cobalt(III) oxide<\/p>\n<p>In questions g) and h) the metal ions do not have a variable charge, therefore<\/p>\n<p class=\"simpara\">g) Using the names of the ions, this ionic compound is named calcium chloride. <em class=\"emphasis\">It is not calcium(II) chloride<\/em> because calcium forms only one cation when it forms an ion, and it has a characteristic charge of 2+.<\/p>\n<p class=\"simpara\">h)The name of this ionic compound is aluminum fluoride.<\/p>\n<p>&nbsp;<\/p>\n<p id=\"fs-idp283458192\"><b><i>Test Yourself<\/i><\/b><\/p>\n<p>Write the formulas of the following ionic compounds:<\/p>\n<p id=\"fs-idp283458864\">a) chromium(III) phosphide \u00a0 \u00a0 \u00a0 \u00a0b) mercury(II) sulfide \u00a0 \u00a0 \u00a0 \u00a0\u00a0c) manganese(II) phosphate<\/p>\n<p id=\"fs-idp268147248\">d) copper(I) oxide \u00a0 \u00a0 \u00a0 \u00a0\u00a0e) chromium(VI) fluoride<\/p>\n<p>&nbsp;<\/p>\n<p><em><strong>Answers<\/strong><\/em><\/p>\n<p>a) CrP \u00a0 \u00a0 \u00a0 \u00a0 b) HgS \u00a0 \u00a0 \u00a0 \u00a0c) Mn<sub>3<\/sub>(PO<sub>4<\/sub>)<sub>2 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sub>d) Cu<sub>2<\/sub>O \u00a0 \u00a0 \u00a0 \u00a0 e) CrF<sub>6<\/sub><\/p>\n<\/div>\n<\/section>\n<section id=\"fs-idp282353488\">\n<div class=\"textbox shaded\" id=\"fs-idm8768\">\n<h3 class=\"title\">Erin Brockovich and Chromium Contamination<\/h3>\n<p id=\"fs-idm7968\">In the early 1990s, legal file clerk Erin Brockovich (<a class=\"autogenerated-content\" href=\"#CNX_Chem_02_07_ErinBrocko\">Figure 1<\/a>) discovered a high rate of serious illnesses in the small town of Hinckley, California. Her investigation eventually linked the illnesses to groundwater contaminated by Cr(VI) used by Pacific Gas &amp; Electric (PG&amp;E) to fight corrosion in a nearby natural gas pipeline. As dramatized in the film <em>Erin Brokovich<\/em> (for which Julia Roberts won an Oscar), Erin and lawyer Edward Masry sued PG&amp;E for contaminating the water near Hinckley in 1993. The settlement they won in 1996\u2014$333 million\u2014was the largest amount ever awarded for a direct-action lawsuit in the US at that time.<\/p>\n<figure id=\"CNX_Chem_02_07_ErinBrocko\">\n<figure style=\"width: 1200px\" class=\"wp-caption aligncenter\"><a href=\"https:\/\/opentextbc.ca\/chemistry\/wp-content\/uploads\/sites\/150\/2016\/05\/CNX_Chem_02_07_ErinBrocko.jpg\"><img loading=\"lazy\" decoding=\"async\" width=\"1200\" height=\"447\" alt=\"Figure A shows a photo of Erin Brockovich. Figure B shows a 3-D ball-and-stick model of chromate. Chromate has a chromium atom at its center that forms bonds with four oxygen atoms each. Two of the oxygen atoms form single bonds with the chromium atom while the other two form double bonds each. The structure of dichromate consists of two chromate ions that are bonded and share one of their oxygen atoms to which each chromate atom has a single bond.\" src=\"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/CNX_Chem_02_07_ErinBrocko-2.jpg\" \/><\/a><figcaption class=\"wp-caption-text\"><strong>Figure 1.<\/strong> (a) Erin Brockovich found that Cr(VI), used by PG&amp;E, had contaminated the Hinckley, California, water supply. (b) The Cr(VI) ion is often present in water as the polyatomic ions chromate, CrO<sub>4<\/sub><sup>2\u2212<\/sup> (left), and dichromate, Cr<sub>2<\/sub>O<sub>7<\/sub><sup>2\u2212<\/sup> (right).<\/figcaption><\/figure>\n<\/figure>\n<p id=\"fs-idp279149248\">Chromium compounds are widely used in industry, such as for chrome plating, in dye-making, as preservatives, and to prevent corrosion in cooling tower water, as occurred near Hinckley. In the environment, chromium exists primarily in either the Cr(III) or Cr(VI) forms. Cr(III), an ingredient of many vitamin and nutritional supplements, forms compounds that are not very soluble in water, and it has low toxicity. But Cr(VI) is much more toxic and forms compounds that are reasonably soluble in water. Exposure to small amounts of Cr(VI) can lead to damage of the respiratory, gastrointestinal, and immune systems, as well as the kidneys, liver, blood, and skin.<\/p>\n<p id=\"fs-idp279150320\">Despite cleanup efforts, Cr(VI) groundwater contamination remains a problem in Hinckley and other locations across the globe. A 2010 study by the Environmental Working Group found that of 35 US cities tested, 31 had higher levels of Cr(VI) in their tap water than the public health goal of 0.02 parts per billion set by the California Environmental Protection Agency.<\/p>\n<\/div>\n<\/section>\n<\/section>\n<section id=\"fs-idp279151472\">\n<div class=\"textbox shaded\">\n<h3 class=\"title\">Example 5<\/h3>\n<p id=\"ball-ch03_s04_p23\" class=\"para\">Write the proper formula and give the proper name for each ionic compound formed between the two listed ions.<\/p>\n<p class=\"para\">a) NH<sub class=\"subscript\">4<\/sub><sup class=\"superscript\">+<\/sup> and S<sup class=\"superscript\">2\u2212 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0<\/sup>b) Al<sup class=\"superscript\">3+<\/sup> and PO<sub class=\"subscript\">4<\/sub><sup class=\"superscript\">3\u2212 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0<\/sup>c) Fe<sup class=\"superscript\">2+<\/sup> and PO<sub class=\"subscript\">4<\/sub><sup class=\"superscript\">3\u2212<\/sup><\/p>\n<p>&nbsp;<\/p>\n<p class=\"simpara\"><strong>Solution<\/strong><\/p>\n<p class=\"simpara\">a) Because the ammonium ion has a 1+\u00a0charge and the sulfide ion has a 2\u2212 charge, we need two ammonium ions to balance the charge on a single sulfide ion. Enclosing the formula for the ammonium ion in parentheses, we have (NH<sub class=\"subscript\">4<\/sub>)<sub class=\"subscript\">2<\/sub>S. The compound\u2019s name is ammonium sulfide.<\/p>\n<p class=\"simpara\">b) Because the ions have the same magnitude of charge, we need only one of each to balance the charges. The formula is AlPO<sub class=\"subscript\">4<\/sub>, and the name of the compound is aluminum phosphate.<\/p>\n<p class=\"simpara\">c) Neither charge is an exact multiple of the other, so we have to go to the least common multiple of 6. To get 6+, we need three iron(II) ions, and to get 6\u2212, we need two phosphate ions. The proper formula is Fe<sub class=\"subscript\">3<\/sub>(PO<sub class=\"subscript\">4<\/sub>)<sub class=\"subscript\">2<\/sub>, and the compound\u2019s name is iron(II) phosphate.<\/p>\n<p>&nbsp;<\/p>\n<p class=\"simpara\"><strong><em class=\"emphasis bolditalic\">Test Yourself<\/em><\/strong><\/p>\n<p id=\"ball-ch03_s04_p24\" class=\"para\">Write the proper formula and give the proper name for each ionic compound formed between the two listed ions.<\/p>\n<p class=\"para\">a) NH<sub class=\"subscript\">4<\/sub><sup class=\"superscript\">+<\/sup> and PO<sub class=\"subscript\">4<\/sub><sup class=\"superscript\">3\u2212 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0<\/sup>b) Co<sup class=\"superscript\">3+<\/sup> and NO<sub class=\"subscript\">2<\/sub><sup class=\"superscript\">\u2212<\/sup><\/p>\n<p>&nbsp;<\/p>\n<p class=\"simpara\"><strong><em class=\"emphasis\">Answers<\/em><\/strong><\/p>\n<p class=\"simpara\">a) (NH<sub class=\"subscript\">4<\/sub>)<sub class=\"subscript\">3<\/sub>PO<sub class=\"subscript\">4<\/sub>, ammonium phosphate \u00a0 \u00a0 \u00a0 \u00a0 \u00a0b)\u00a0Co(NO<sub class=\"subscript\">2<\/sub>)<sub class=\"subscript\">3<\/sub>, cobalt(III) nitrite<\/p>\n<\/div>\n<section id=\"fs-idp268266480\">\n<section id=\"fs-idp279293712\">\n<div class=\"textbox shaded\" id=\"fs-idm337456\">\n<h3 class=\"title\">Ionic Compounds in Your Cabinets<\/h3>\n<p id=\"fs-idm70496\">Every day you encounter and use a large number of ionic compounds. Some of these compounds, where they are found, and what they are used for are listed in <a class=\"autogenerated-content\" href=\"#fs-idp268265360\">Table 3<\/a>. Look at the label or ingredients list on the various products that you use during the next few days, and see if you run into any of those in this table, or find other ionic compounds that you could now name or write as a formula.<\/p>\n<table id=\"fs-idp268265360\" class=\"span-all\" summary=\"The everyday ionic compound examples included in this table are: N a C L sodium chloride, or ordinary table salt, K I potassium iodide which is added to iodized salt, N a F, sodium fluoride which is an ingredient in toothpaste, N a H C O subscript 3 sodium bicarbonate which is baking soda, used in cooking and as an antacid, N a subscript 2 C O subscript 3 sodium carbonate which is washing soda and is used in cleaning agents, N a O C l sodium hypochlorite which is the active ingredient in household bleach, C a C O subscript 3 calcium carbonate which is an ingredient of antacids, M g ( O H ) subscript 2, magnesium hydroxide which is also an ingredient of antacids, A l ( O H ) subscript 3 aluminum hydroxide which is also an ingredient in antacids, N a O H sodium hydroxide which is lye and is used as a drain cleaner, K subscript 3 P O subscript 4 potassium phosphate which is a food additive, M g S O subscript 4 magneisum sulfate which is added to purified water, N a subscript 2 H P O subscript 4 sodium hydrogen phosphate which is an anti-caking agent and is used in powdered products, and N a subscript 2 S O subscript 3 sodium sulfite which is a preservative.\">\n<thead>\n<tr>\n<th>Ionic Compound<\/th>\n<th>Use<\/th>\n<\/tr>\n<\/thead>\n<tbody>\n<tr>\n<td>NaCl, sodium chloride<\/td>\n<td>ordinary table salt<\/td>\n<\/tr>\n<tr>\n<td>KI, potassium iodide<\/td>\n<td>added to \u201ciodized\u201d salt for thyroid health<\/td>\n<\/tr>\n<tr>\n<td>NaF, sodium fluoride<\/td>\n<td>ingredient in toothpaste<\/td>\n<\/tr>\n<tr>\n<td>NaHCO<sub>3<\/sub>, sodium bicarbonate<\/td>\n<td>baking soda; used in cooking (and as antacid)<\/td>\n<\/tr>\n<tr>\n<td>Na<sub>2<\/sub>CO<sub>3<\/sub>, sodium carbonate<\/td>\n<td>washing soda; used in cleaning agents<\/td>\n<\/tr>\n<tr>\n<td>NaOCl, sodium hypochlorite<\/td>\n<td>active ingredient in household bleach<\/td>\n<\/tr>\n<tr>\n<td>CaCO<sub>3<\/sub> calcium carbonate<\/td>\n<td>ingredient in antacids<\/td>\n<\/tr>\n<tr>\n<td>Mg(OH)<sub>2<\/sub>, magnesium hydroxide<\/td>\n<td>ingredient in antacids<\/td>\n<\/tr>\n<tr>\n<td>Al(OH)<sub>3<\/sub>, aluminum hydroxide<\/td>\n<td>ingredient in antacids<\/td>\n<\/tr>\n<tr>\n<td>NaOH, sodium hydroxide<\/td>\n<td>lye; used as drain cleaner<\/td>\n<\/tr>\n<tr>\n<td>K<sub>3<\/sub>PO<sub>4<\/sub>, potassium phosphate<\/td>\n<td>food additive (many purposes)<\/td>\n<\/tr>\n<tr>\n<td>MgSO<sub>4<\/sub>, magnesium sulfate<\/td>\n<td>added to purified water<\/td>\n<\/tr>\n<tr>\n<td>Na<sub>2<\/sub>HPO<sub>4<\/sub>, sodium hydrogen phosphate<\/td>\n<td>anti-caking agent; used in powdered products<\/td>\n<\/tr>\n<tr>\n<td>Na<sub>2<\/sub>SO<sub>3<\/sub>, sodium sulfite<\/td>\n<td>preservative<\/td>\n<\/tr>\n<tr>\n<td colspan=\"2\"><strong>Table 3.<\/strong> Everyday Ionic Compounds<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<p>&nbsp;<\/p>\n<\/div>\n<\/section>\n<\/section>\n<h2>Nomenclature of Molecular (Covalent) Compounds<\/h2>\n<p id=\"fs-idp268164784\">The bonding characteristics of inorganic molecular compounds are different from ionic compounds, and they are named using a different system as well. The charges of cations and anions dictate their ratios in ionic compounds, so specifying the names of the ions provides sufficient information to determine chemical formulas. However, because covalent bonding allows for significant variation in the combination ratios of the atoms in a molecule, the names for molecular compounds must explicitly identify these ratios.<\/p>\n<section id=\"fs-idp268165696\">\n<h2>Compounds Composed of Two Elements<\/h2>\n<p id=\"fs-idp268166336\">When two nonmetallic elements form a molecular compound, several combination ratios are often possible. For example, carbon and oxygen can form the compounds CO and CO<sub>2<\/sub>. Since these are different substances with different properties, they cannot both have the same name (they cannot both be called carbon oxide). To deal with this situation, we use a naming method that is somewhat similar to that used for ionic compounds, but with added prefixes to specify the numbers of atoms of each element. The name of the more metallic element (the one farther to the left and\/or bottom of the periodic table) is first, followed by the name of the more nonmetallic element (the one farther to the right and\/or top) with its ending changed to the suffix \u2013<em>ide<\/em>. The numbers of atoms of each element are designated by the Greek prefixes shown in <a class=\"autogenerated-content\" href=\"#fs-idp268400368\">Table 6<\/a>.<\/p>\n<table id=\"fs-idp268400368\" class=\"span-all\" summary=\"This table has two columns labeled \u201cprefix\u201d and \u201cnumber\u201d. Mono is associated with one although this prefix is sometimes omitted. Di is associated with two. Tri is associated with three. Tetra is associated with four. Penta is associated with five. Hexa is associated with six. Hepta is associated with seven. Octa is associated with eight. Nona is associated with nine. Deca is associated with ten.\">\n<thead>\n<tr>\n<th>Number<\/th>\n<th>Prefix<\/th>\n<th>Number<\/th>\n<th>Prefix<\/th>\n<\/tr>\n<\/thead>\n<tbody>\n<tr>\n<td>1 (sometimes omitted)<\/td>\n<td>mono-<\/td>\n<td>6<\/td>\n<td>hexa-<\/td>\n<\/tr>\n<tr>\n<td>2<\/td>\n<td>di-<\/td>\n<td>7<\/td>\n<td>hepta-<\/td>\n<\/tr>\n<tr>\n<td>3<\/td>\n<td>tri-<\/td>\n<td>8<\/td>\n<td>octa-<\/td>\n<\/tr>\n<tr>\n<td>4<\/td>\n<td>tetra-<\/td>\n<td>9<\/td>\n<td>nona-<\/td>\n<\/tr>\n<tr>\n<td>5<\/td>\n<td>penta-<\/td>\n<td>10<\/td>\n<td>deca-<\/td>\n<\/tr>\n<tr>\n<td colspan=\"4\"><strong>Table 6.<\/strong> Nomenclature Prefixes<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<p id=\"fs-idm325632\">When only one atom of the first element is present, the prefix <em>mono<\/em>&#8211; is usually deleted from that part. Thus, CO is named carbon monoxide, and CO<sub>2<\/sub> is called carbon dioxide. When two vowels are adjacent, the <em>a<\/em> in the Greek prefix is usually dropped. Some other examples are shown in <a class=\"autogenerated-content\" href=\"#fs-idp269568176\">Table 7<\/a>.<\/p>\n<table id=\"fs-idp269568176\" class=\"span-all\" summary=\"A two column table is shown. The left column is titled \u201cCompound\u201d and the right column is titled \u201cName.\u201d From left to right, the first row reads \u201cS O subscript 2\u201d and \u201csulfur dioxide.\u201d The second row reads \u201cS O subscript 3\u201d and \u201csulfur trioxide.\u201d The third row reads \u201cN O subscript 2\u201d and \u201cnitrogen dioxide.\u201d The fourth row reads \u201cN subscript 2 O subscript 4\u201d and \u201cdinitrogen tetroxide.\u201d The fifth row reads \u201cN subscript 2 O subscript 5\u201d and \u201cdinitrogen pentoxide.\u201d The sixth row reads \u201cB C l subscript 3\u201d and \u201cboron trichloride.\u201d The seventh row reads \u201cS F subscript 6\u201d and \u201csulfur hexafluoride.\u201d The eighth row reads \u201cP F subscript 5\u201d and \u201cphosphorus pentafluoride.\u201d The ninth row reads \u201cP subscript 4 O subscript 10\u201d and \u201ctetraphosphorus decaoxide.\u201d The tenth row reads \u201cI F subscript 7\u201d and \u201ciodine heptafluoride.\u201d\">\n<thead>\n<tr>\n<th>Compound<\/th>\n<th>Name<\/th>\n<th>Compound<\/th>\n<th>Name<\/th>\n<\/tr>\n<\/thead>\n<tbody>\n<tr>\n<td>SO<sub>2<\/sub><\/td>\n<td>sulfur dioxide<\/td>\n<td>BCl<sub>3<\/sub><\/td>\n<td>boron trichloride<\/td>\n<\/tr>\n<tr>\n<td>SO<sub>3<\/sub><\/td>\n<td>sulfur trioxide<\/td>\n<td>SF<sub>6<\/sub><\/td>\n<td>sulfur hexafluoride<\/td>\n<\/tr>\n<tr>\n<td>NO<sub>2<\/sub><\/td>\n<td>nitrogen dioxide<\/td>\n<td>PF<sub>5<\/sub><\/td>\n<td>phosphorus pentafluoride<\/td>\n<\/tr>\n<tr>\n<td>N<sub>2<\/sub>O<sub>4<\/sub><\/td>\n<td>dinitrogen tetroxide<\/td>\n<td>P<sub>4<\/sub>O<sub>10<\/sub><\/td>\n<td>tetraphosphorus decaoxide<\/td>\n<\/tr>\n<tr>\n<td>N<sub>2<\/sub>O<sub>5<\/sub><\/td>\n<td>dinitrogen pentoxide<\/td>\n<td>IF<sub>7<\/sub><\/td>\n<td>iodine heptafluoride<\/td>\n<\/tr>\n<tr>\n<td colspan=\"4\"><strong>Table 7.<\/strong> Names of Some Molecular Compounds Composed of Two Elements<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<p id=\"fs-idm207744\">There are a few common names that you will encounter as you continue your study of chemistry. For example, although NO is often called nitric oxide, its proper name is nitrogen monoxide. Similarly, N<sub>2<\/sub>O is known as nitrous oxide even though our rules would specify the name dinitrogen monoxide. (And H<sub>2<\/sub>O is usually called water, not dihydrogen monoxide.) You should commit to memory the common names of compounds as you encounter them.<\/p>\n<div class=\"textbox shaded\" id=\"fs-idm206240\">\n<h3>Example 6<\/h3>\n<p id=\"fs-idm205600\">Name the following covalent compounds:<\/p>\n<p id=\"fs-idm205216\">a) SF<sub>6 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sub>b) N<sub>2<\/sub>O<sub>3 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sub>c) Cl<sub>2<\/sub>O<sub>7 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sub>d) P<sub>4<\/sub>O<sub>6<\/sub> \u00a0 \u00a0 \u00a0 \u00a0\u00a0e) PF<sub class=\"subscript\">3<\/sub> \u00a0 \u00a0 \u00a0 \u00a0 f)\u00a0CO \u00a0 \u00a0 \u00a0 \u00a0 g)\u00a0Se<sub class=\"subscript\">2<\/sub>Br<sub class=\"subscript\">2<\/sub><\/p>\n<p>&nbsp;<\/p>\n<p id=\"fs-idp268181136\"><strong>Solution<\/strong><br \/>\nBecause these compounds consist solely of nonmetals, they are molecular compounds, therefore according to the rules, we use prefixes to designate the number of atoms of each element:<\/p>\n<p id=\"fs-idm335200\">a) sulfur hexafluoride \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0b) dinitrogen trioxide \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0c) dichloride heptoxide<\/p>\n<p>d) tetraphosphorus hexoxide \u00a0 \u00a0 \u00a0 \u00a0 e) phosphorus trifluoride \u00a0 \u00a0 \u00a0 \u00a0 f) carbon monoxide (not carbon monooxide)<\/p>\n<p>g)\u00a0diselenium dibromide<\/p>\n<p>&nbsp;<\/p>\n<p id=\"fs-idm333600\"><em><strong>Test Yourself<\/strong><\/em><br \/>\nWrite the formulas for the following compounds:<\/p>\n<p id=\"fs-idm332928\">a) phosphorus pentachloride \u00a0 \u00a0 \u00a0 \u00a0 \u00a0b) dinitrogen monoxide \u00a0 \u00a0 \u00a0 \u00a0\u00a0c) iodine heptafluoride<\/p>\n<p>d) carbon tetrachloride \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 e)\u00a0disulfur difluoride \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0f)\u00a0iodine pentabromide<\/p>\n<p>&nbsp;<\/p>\n<p><em><strong>Answers<\/strong><\/em><\/p>\n<p>a) PCl<sub>5 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sub>b) N<sub>2<\/sub>O \u00a0 \u00a0 \u00a0 \u00a0 c) IF<sub>7 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sub>d) CCl<sub>4<\/sub> \u00a0 \u00a0 \u00a0e)\u00a0S<sub class=\"subscript\">2<\/sub>F<sub class=\"subscript\">2 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sub>f) IBr<sub class=\"subscript\">5<\/sub><\/p>\n<\/div>\n<div class=\"textbox shaded\" id=\"fs-idp283404080\">\n<p><img loading=\"lazy\" decoding=\"async\" width=\"108\" height=\"67\" class=\"alignleft\" alt=\"\u00a0\" src=\"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/OSC_Interactive_200-4-2.png\" \/><\/p>\n<p id=\"fs-idp268192304\">The following <a href=\"http:\/\/openstaxcollege.org\/l\/16chemcompname\">website<\/a> provides practice with naming chemical compounds and writing chemical formulas. You can choose binary, polyatomic, and variable charge ionic compounds, as well as molecular compounds.<\/p>\n<\/div>\n<\/section>\n<section id=\"fs-idp268193776\">\n<h2>Binary Acids<\/h2>\n<p id=\"fs-idp282238096\">Some compounds containing hydrogen are members of an important class of substances known as acids, and these compounds have interesting chemical properties. The chemistry of these compounds is explored in more detail in later chapters of this text, but for now, it will suffice to note that many acids release hydrogen ions, H<sup>+<\/sup>, when dissolved in water. \u00a0To indicate that something is dissolved in water, we will use the phase label (aq) next to a chemical formula (where aq stands for \u201caqueous,\u201d a word that describes something dissolved in water). \u00a0To denote this distinct chemical property, a mixture of water with an acid is given a name derived from the compound\u2019s name. If the compound is a <strong>binary acid<\/strong> (comprised of hydrogen and one other nonmetallic element):<\/p>\n<ol id=\"fs-idp282239904\">\n<li>The word \u201chydrogen\u201d is changed to the prefix <em>hydro-<\/em><\/li>\n<li>The other nonmetallic element name is modified by adding the suffix &#8211;<em>ic<\/em><\/li>\n<li>The word \u201cacid\u201d is added as a second word<\/li>\n<\/ol>\n<p id=\"fs-idm109568\">For example, when the gas HCl (hydrogen chloride) is dissolved in water, the solution is called <em>hydrochloric acid<\/em>. Several other examples of this nomenclature are shown in <a class=\"autogenerated-content\" href=\"#fs-idp272649888\">Table 8<\/a>.<\/p>\n<table id=\"fs-idp272649888\" class=\"span-all\" summary=\"The names of simple acids included in this table are: H F gas, which is hydrogen fluoride, H C l gas which is hydrogen chloride, H B r gas which is hydrogen bromide, H I gas which is hydrogen iodide, H subscript 2 S gas which is hydrogen sulfide, H F aqueous which is hydrofluoric acid, H C l aqueous which is hydrochloric acid, H B r aqueous which is hydrobromic acid, H I aqueous which is hydroiodic acid, and H subscript 2 S aqueous which is hydrosulfuric acid.\">\n<thead>\n<tr>\n<th>Name of Gas<\/th>\n<th>Name of Acid<\/th>\n<\/tr>\n<\/thead>\n<tbody>\n<tr>\n<td>HF(<em>g<\/em>), hydrogen fluoride<\/td>\n<td>HF(<em>aq<\/em>), hydrofluoric acid<\/td>\n<\/tr>\n<tr>\n<td>HCl(<em>g<\/em>), hydrogen chloride<\/td>\n<td>HCl(<em>aq<\/em>), hydrochloric acid<\/td>\n<\/tr>\n<tr>\n<td>HBr(<em>g<\/em>), hydrogen bromide<\/td>\n<td>HBr(<em>aq<\/em>), hydrobromic acid<\/td>\n<\/tr>\n<tr>\n<td>HI(<em>g<\/em>), hydrogen iodide<\/td>\n<td>HI(<em>aq<\/em>), hydroiodic acid<\/td>\n<\/tr>\n<tr>\n<td>H<sub>2<\/sub>S(<em>g<\/em>), hydrogen sulfide<\/td>\n<td>H<sub>2<\/sub>S(<em>aq<\/em>), hydrosulfuric acid<\/td>\n<\/tr>\n<tr>\n<td>HCN(<em>g<\/em>), hydrogen cyanide<\/td>\n<td>HCN(<em>aq<\/em>), hydrocyanic acid<\/td>\n<\/tr>\n<tr>\n<td colspan=\"2\"><strong>Table 8.<\/strong> Names of Some Simple Acids<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<\/section>\n<section id=\"fs-idp268349296\">\n<h2>Oxyacids<\/h2>\n<p id=\"fs-idp279162704\">Many compounds containing three or more elements (such as organic compounds or coordination compounds) are subject to specialized nomenclature rules that you will learn later. However, we will briefly discuss the important compounds known as <strong>oxyacids<\/strong>, compounds that contain hydrogen, oxygen, and at least one other element, and are bonded in such a way as to impart acidic properties to the compound (you will learn the details of this in a later chapter). Typical oxyacids consist of hydrogen combined with a polyatomic, oxygen-containing ion. To name oxyacids:<\/p>\n<ol id=\"fs-idp279164064\">\n<li>Omit \u201chydrogen\u201d<\/li>\n<li>Start with the root name of the anion<\/li>\n<li>Replace \u2013<em>ate<\/em> with \u2013<em>ic<\/em>, or \u2013<em>ite<\/em> with \u2013<em>ous<\/em><\/li>\n<li>Add \u201cacid\u201d<\/li>\n<\/ol>\n<p id=\"fs-idp282461232\">For example, consider H<sub>2<\/sub>CO<sub>3<\/sub> (which you might be tempted to call \u201chydrogen carbonate\u201d). To name this correctly, \u201chydrogen\u201d is omitted; the \u2013<em>ate<\/em> of carbonate is replace with \u2013<em>ic<\/em>; and acid is added\u2014so its name is carbonic acid. Other examples are given in <a class=\"autogenerated-content\" href=\"#fs-idp268340336\">Table 9<\/a>. There are some exceptions to the general naming method (e.g., H<sub>2<\/sub>SO<sub>4<\/sub> is called sulfuric acid, not sulfic acid, and H<sub>2<\/sub>SO<sub>3<\/sub> is sulfurous, not sulfous, acid).<\/p>\n<table id=\"fs-idp268340336\" class=\"span-all\" summary=\"This table has three columns labeled \u201cformula\u201d, \u201canion name\u201d, and \u201cacid name\u201d. H C subscript 2 H subscript 3 O subscript 2 is named acetate or acetic acid. H N O subscript 3 is named nitrate or nitric acid. H N O subscript 2 is named nitrite or nitrous acid, H C l O subscript 4 is named perchlorate or perchloric acid. H subscript 2 C O subscript 3 is named carbonate or carbonic acid. H subscript 2 S O subscript 4 is named sulfate or sulfuric acid. H subscript 2 S O subscript 3 is named sulfite or sulfurous acid. H subscript 3 P O subscript 4 is named phosphate or phosphoric acid.\">\n<thead>\n<tr>\n<th>Formula<\/th>\n<th>Anion Name<\/th>\n<th>Acid Name<\/th>\n<\/tr>\n<\/thead>\n<tbody>\n<tr>\n<td>HC<sub>2<\/sub>H<sub>3<\/sub>O<sub>2<\/sub><\/td>\n<td>acetate<\/td>\n<td>acetic acid<\/td>\n<\/tr>\n<tr>\n<td>HNO<sub>3<\/sub><\/td>\n<td>nitrate<\/td>\n<td>nitric acid<\/td>\n<\/tr>\n<tr>\n<td>HNO<sub>2<\/sub><\/td>\n<td>nitrite<\/td>\n<td>nitrous acid<\/td>\n<\/tr>\n<tr>\n<td>HClO<sub>4<\/sub><\/td>\n<td>perchlorate<\/td>\n<td>perchloric acid<\/td>\n<\/tr>\n<tr>\n<td>HClO<sub><span style=\"font-size: small\">3<\/span><\/sub><\/td>\n<td>chlorate<\/td>\n<td>chloric acid<\/td>\n<\/tr>\n<tr>\n<td>HClO<sub><span style=\"font-size: small\">2<\/span><\/sub><\/td>\n<td>chlorite<\/td>\n<td>chlorous acid<\/td>\n<\/tr>\n<tr>\n<td>HClO<\/td>\n<td>hypochlorite<\/td>\n<td>hypochlorous acid<\/td>\n<\/tr>\n<tr>\n<td>H<sub>2<\/sub>CO<sub>3<\/sub><\/td>\n<td>carbonate<\/td>\n<td>carbonic acid<\/td>\n<\/tr>\n<tr>\n<td>H<sub>2<\/sub>SO<sub>4<\/sub><\/td>\n<td>sulfate<\/td>\n<td>sulfuric acid<\/td>\n<\/tr>\n<tr>\n<td>H<sub>2<\/sub>SO<sub>3<\/sub><\/td>\n<td>sulfite<\/td>\n<td>sulfurous acid<\/td>\n<\/tr>\n<tr>\n<td>H<sub>3<\/sub>PO<sub>4<\/sub><\/td>\n<td>phosphate<\/td>\n<td>phosphoric acid<\/td>\n<\/tr>\n<tr>\n<td>H<sub>3<\/sub>PO<sub>3<\/sub><\/td>\n<td>phosphite<\/td>\n<td>phosphorous acid<\/td>\n<\/tr>\n<tr>\n<td>H<sub>2<\/sub>CrO<sub>4<\/sub><\/td>\n<td>chromate<\/td>\n<td>chromic acid<\/td>\n<\/tr>\n<tr>\n<td colspan=\"3\"><strong>Table 9.<\/strong> Names of Common Oxyacids<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<\/section>\n<\/section>\n<section id=\"fs-idp282340144\" class=\"summary\">\n<div class=\"textbox shaded\">\n<h3 class=\"title\">Example 7<\/h3>\n<p id=\"ball-ch03_s05_p04\" class=\"para\">Name each acid without consulting the tables.<\/p>\n<p class=\"para\">a) HBr(aq) \u00a0 \u00a0 \u00a0 \u00a0 b)\u00a0H<sub class=\"subscript\">2<\/sub>SO<sub class=\"subscript\">4 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sub><span>c)\u00a0 HF(g)\u00a0 \u00a0 \u00a0 \u00a0 \u00a0d)\u00a0 HCN(aq) \u00a0 \u00a0\u00a0\u00a0\u00a0\u00a0 e) H<sub>2<\/sub>S(aq)<\/span><\/p>\n<p>&nbsp;<\/p>\n<p class=\"simpara\"><strong>Solution<\/strong><\/p>\n<p class=\"simpara\">a) As an aqueous binary acid, the acid\u2019s name is <em class=\"emphasis\">hydro-<\/em> +\u00a0stem name +\u00a0<em class=\"emphasis\">-ic acid<\/em>. Because this acid contains a bromine atom, the name is hydrobromic acid.<\/p>\n<p class=\"simpara\">b) Because this acid is derived from the sulfate ion, the name of the acid is the stem of the anion name +\u00a0<em class=\"emphasis\">-ic acid<\/em>. The name of this acid is sulfuric acid.<\/p>\n<p class=\"simpara\">c) Because HF<span>(g)<\/span><span>\u00a0is in gaseous form, we name it hydrogen fluoride<\/span>.<\/p>\n<p class=\"Indentpoints\">d)<span>\u00a0 <\/span>HCN<span>(aq)<\/span><span>\u00a0<\/span>contains the polyatomic ion cyanide. The root is \u201ccyan\u201d, thus HCN<span>(aq)<\/span><span>\u00a0<\/span>= hydrocyanic acid.<\/p>\n<p class=\"Indentpoints\">e)<span>\u00a0 <\/span>H<sub>2<\/sub>S<span>(aq)<\/span><span>\u00a0<\/span>contains the ion sulfide. In this case, however, the root takes a slightly different form of \u201csulfur\u201d (the same as the element name). Thus H<sub>2<\/sub>S<span>(aq)<\/span><span>\u00a0<\/span>= hydrosulfuric acid.<\/p>\n<p>&nbsp;<\/p>\n<p class=\"simpara\"><strong><em class=\"emphasis bolditalic\">Test Yourself<\/em><\/strong><\/p>\n<p id=\"ball-ch03_s05_p05\" class=\"para\">Name each acid.<\/p>\n<p class=\"para\">a) HF(aq) \u00a0 \u00a0 \u00a0 \u00a0 b)\u00a0HNO<sub class=\"subscript\">2 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sub>c)<span>\u00a0<\/span>HClO<sub>4<\/sub><span>\u00a0 \u00a0 \u00a0 \u00a0<\/span>d)<span>\u00a0<\/span>H<sub>2<\/sub>SO<sub>4 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sub>e)<span>\u00a0<\/span>H<sub>2<\/sub>CrO<sub>4<\/sub><span>(aq)<\/span><span>\u00a0 \u00a0 \u00a0 \u00a0 \u00a0 f<\/span>)<span>\u00a0 <\/span>H<sub>3<\/sub>PO<sub>4<\/sub><span>(aq)<\/span><span>\u00a0 \u00a0 \u00a0\u00a0<\/span>g) HClO<span>(aq)<\/span><\/p>\n<p>&nbsp;<\/p>\n<p class=\"simpara\"><strong><em class=\"emphasis\">Answers<\/em><\/strong><\/p>\n<p class=\"simpara\">a) hydrofluoric acid \u00a0 \u00a0 \u00a0 \u00a0\u00a0b) nitrous acid \u00a0 \u00a0 \u00a0 \u00a0 c) perchloric acid \u00a0 \u00a0 \u00a0 \u00a0 d) sulphuric acid \u00a0 \u00a0 \u00a0 \u00a0 e) chromic acid<\/p>\n<p>f) phosphoric acid \u00a0 \u00a0 \u00a0 \u00a0 g) hypochlorous acid<\/p>\n<\/div>\n<p id=\"ball-ch03_s05_p06\" class=\"para editable block\">All acids have some similar properties. For example, acids have a sour taste; in fact, the sour taste of some of our foods, such as citrus fruits and vinegar, is caused by the presence of acids in food. Many acids react with some metallic elements to form metal ions and elemental hydrogen. Acids make certain plant pigments change colors; indeed, the ripening of some fruits and vegetables is caused by the formation or destruction of excess acid in the plant. In a later chapter, we will explore the chemical behaviour of acids.<\/p>\n<p id=\"ball-ch03_s05_p07\" class=\"para editable block\">Acids are very prevalent in the world around us. We have already mentioned that citrus fruits contain acid; among other compounds, they contain citric acid, H<sub class=\"subscript\">3<\/sub>C<sub class=\"subscript\">6<\/sub>H<sub class=\"subscript\">5<\/sub>O<sub class=\"subscript\">7<\/sub>(aq). Oxalic acid, H<sub class=\"subscript\">2<\/sub>C<sub class=\"subscript\">2<\/sub>O<sub class=\"subscript\">4<\/sub>(aq), is found in spinach and other green leafy vegetables. Hydrochloric acid not only is found in the stomach (stomach acid) but also can be bought in hardware stores as a cleaner for concrete and masonry. Phosphoric acid is an ingredient in some soft drinks.<\/p>\n<div class=\"textbox shaded\">\n<h3 class=\"title\">Sodium in Your Food<\/h3>\n<p id=\"ball-ch03_s04_p25\" class=\"para\">The element sodium, at least in its ionic form as Na<sup class=\"superscript\">+<\/sup>, is a necessary nutrient for humans to live. In fact, the human body is approximately 0.15% sodium, with the average person having one-twentieth to one-tenth of a kilogram in their body at any given time, mostly in fluids outside cells and in other bodily fluids.<\/p>\n<p id=\"ball-ch03_s04_p26\" class=\"para\">Sodium is also present in our diet. The common table salt we use on our foods is an ionic sodium compound. Many processed foods also contain significant amounts of sodium added to them as a variety of ionic compounds. Why are sodium compounds used so much? Usually sodium compounds are inexpensive, but, more importantly, most ionic sodium compounds dissolve easily. This allows processed food manufacturers to add sodium-containing substances to food mixtures and know that the compound will dissolve and distribute evenly throughout the food. Simple ionic compounds such as sodium nitrite (NaNO<sub class=\"subscript\">2<\/sub>) are added to cured meats, such as bacon and deli-style meats, while a compound called sodium benzoate is added to many packaged foods as a preservative. <a class=\"xref\" href=\"#ball-ch03_s04_t03\">Table 10 &#8220;Some Sodium Compounds Added to Food&#8221;<\/a> is a partial list of some sodium additives used in food. Some of them you may recognize after reading this chapter. Others you may not recognize, but they are all ionic sodium compounds with some negatively charged ion also present.<\/p>\n<div class=\"table\" id=\"ball-ch03_s04_t03\">\n<table style=\"border-spacing: 0px\" cellpadding=\"0\">\n<thead>\n<tr>\n<th>Sodium Compound<\/th>\n<th>Use in Food<\/th>\n<\/tr>\n<\/thead>\n<tbody>\n<tr>\n<td>Sodium acetate<\/td>\n<td>preservative, acidity regulator<\/td>\n<\/tr>\n<tr>\n<td>Sodium adipate<\/td>\n<td>food acid<\/td>\n<\/tr>\n<tr>\n<td>Sodium alginate<\/td>\n<td>thickener, vegetable gum, stabilizer, gelling agent, emulsifier<\/td>\n<\/tr>\n<tr>\n<td>Sodium aluminum phosphate<\/td>\n<td>acidity regulator, emulsifier<\/td>\n<\/tr>\n<tr>\n<td>Sodium aluminosilicate<\/td>\n<td>anticaking agent<\/td>\n<\/tr>\n<tr>\n<td>Sodium ascorbate<\/td>\n<td>antioxidant<\/td>\n<\/tr>\n<tr>\n<td>Sodium benzoate<\/td>\n<td>preservative<\/td>\n<\/tr>\n<tr>\n<td>Sodium bicarbonate<\/td>\n<td>mineral salt<\/td>\n<\/tr>\n<tr>\n<td>Sodium bisulfite<\/td>\n<td>preservative, antioxidant<\/td>\n<\/tr>\n<tr>\n<td>Sodium carbonate<\/td>\n<td>mineral salt<\/td>\n<\/tr>\n<tr>\n<td>Sodium carboxymethylcellulose<\/td>\n<td>emulsifier<\/td>\n<\/tr>\n<tr>\n<td>Sodium citrates<\/td>\n<td>food acid<\/td>\n<\/tr>\n<tr>\n<td>Sodium dehydroacetate<\/td>\n<td>preservative<\/td>\n<\/tr>\n<tr>\n<td>Sodium erythorbate<\/td>\n<td>antioxidant<\/td>\n<\/tr>\n<tr>\n<td>Sodium erythorbin<\/td>\n<td>antioxidant<\/td>\n<\/tr>\n<tr>\n<td>Sodium ethyl para-hydroxybenzoate<\/td>\n<td>preservative<\/td>\n<\/tr>\n<tr>\n<td>Sodium ferrocyanide<\/td>\n<td>anticaking agent<\/td>\n<\/tr>\n<tr>\n<td>Sodium formate<\/td>\n<td>preservative<\/td>\n<\/tr>\n<tr>\n<td>Sodium fumarate<\/td>\n<td>food acid<\/td>\n<\/tr>\n<tr>\n<td>Sodium gluconate<\/td>\n<td>stabilizer<\/td>\n<\/tr>\n<tr>\n<td>Sodium hydrogen acetate<\/td>\n<td>preservative, acidity regulator<\/td>\n<\/tr>\n<tr>\n<td>Sodium hydroxide<\/td>\n<td>mineral salt<\/td>\n<\/tr>\n<tr>\n<td>Sodium lactate<\/td>\n<td>food acid<\/td>\n<\/tr>\n<tr>\n<td>Sodium malate<\/td>\n<td>food acid<\/td>\n<\/tr>\n<tr>\n<td>Sodium metabisulfite<\/td>\n<td>preservative, antioxidant, bleaching agent<\/td>\n<\/tr>\n<tr>\n<td>Sodium methyl para-hydroxybenzoate<\/td>\n<td>preservative<\/td>\n<\/tr>\n<tr>\n<td>Sodium nitrate<\/td>\n<td>preservative, color fixative<\/td>\n<\/tr>\n<tr>\n<td>Sodium nitrite<\/td>\n<td>preservative, color fixative<\/td>\n<\/tr>\n<tr>\n<td>Sodium orthophenyl phenol<\/td>\n<td>preservative<\/td>\n<\/tr>\n<tr>\n<td>Sodium propionate<\/td>\n<td>preservative<\/td>\n<\/tr>\n<tr>\n<td>Sodium propyl para-hydroxybenzoate<\/td>\n<td>preservative<\/td>\n<\/tr>\n<tr>\n<td>Sodium sorbate<\/td>\n<td>preservative<\/td>\n<\/tr>\n<tr>\n<td>Sodium stearoyl lactylate<\/td>\n<td>emulsifier<\/td>\n<\/tr>\n<tr>\n<td>Sodium succinates<\/td>\n<td>acidity regulator, flavour enhancer<\/td>\n<\/tr>\n<tr>\n<td>Sodium salts of fatty acids<\/td>\n<td>emulsifier, stabilizer, anticaking agent<\/td>\n<\/tr>\n<tr>\n<td>Sodium sulfite<\/td>\n<td>mineral salt, preservative, antioxidant<\/td>\n<\/tr>\n<tr>\n<td>Sodium sulfite<\/td>\n<td>preservative, antioxidant<\/td>\n<\/tr>\n<tr>\n<td>Sodium tartrate<\/td>\n<td>food acid<\/td>\n<\/tr>\n<tr>\n<td>Sodium tetraborate<\/td>\n<td>preservative<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<\/div>\n<p><strong><span class=\"title-prefix\">Table 10.<\/span><\/strong> Some Sodium Compounds Added to Food<\/p>\n<p>The use of so many sodium compounds in prepared and processed foods has alarmed some physicians and nutritionists. They argue that the average person consumes too much sodium from his or her diet. The average person needs only about 500 mg of sodium every day; most people consume more than this\u2014up to 10 times as much. Some studies have implicated increased sodium intake with high blood pressure; newer studies suggest that the link is questionable. However, there has been a push to reduce the amount of sodium most people ingest every day: avoid processed and manufactured foods, read labels on packaged foods (which include an indication of the sodium content), don\u2019t oversalt foods, and use other herbs and spices besides salt in cooking.<\/p>\n<\/div>\n<h2>Key Concepts and Summary<\/h2>\n<p id=\"fs-idp282340912\">Chemists use nomenclature rules to clearly name compounds. Ionic and molecular compounds are named using somewhat-different methods. Binary ionic compounds typically consist of a metal and a nonmetal. The name of the metal is written first, followed by the name of the nonmetal with its ending changed to \u2013<em>ide<\/em>. For example, K<sub>2<\/sub>O is called potassium oxide. If the metal can form ions with different charges, a Roman numeral in parentheses follows the name of the metal to specify its charge. Thus, FeCl<sub>2<\/sub> is iron(II) chloride and FeCl<sub>3<\/sub> is iron(III) chloride. Some compounds contain polyatomic ions; the names of common polyatomic ions should be memorized. Molecular compounds can form compounds with different ratios of their elements, so prefixes are used to specify the numbers of atoms of each element in a molecule of the compound. Examples include SF<sub>6<\/sub>, sulfur hexafluoride, and N<sub>2<\/sub>O<sub>4<\/sub>, dinitrogen tetroxide. Acids are an important class of compounds containing hydrogen and having special nomenclature rules. Binary acids are named using the prefix <em>hydro-<\/em>, changing the \u2013<em>ide<\/em> suffix to \u2013<em>ic<\/em>, and adding \u201cacid;\u201d HCl is hydrochloric acid. Oxyacids are named by changing the ending of the anion to \u2013<em>ic<\/em>, and adding \u201cacid;\u201d H<sub>2<\/sub>CO<sub>3<\/sub> is carbonic acid.<\/p>\n<p>&nbsp;<\/p>\n<\/section>\n<p><a href=\"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/Flowchart.jpg\"><img loading=\"lazy\" decoding=\"async\" width=\"916\" height=\"1190\" class=\"aligncenter wp-image-3484 size-full\" alt=\"\" src=\"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/Flowchart.jpg\" srcset=\"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/Flowchart.jpg 916w, https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/Flowchart-231x300.jpg 231w, https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/Flowchart-768x998.jpg 768w, https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/Flowchart-788x1024.jpg 788w, https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/Flowchart-65x84.jpg 65w, https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/Flowchart-225x292.jpg 225w, https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/Flowchart-350x455.jpg 350w\" sizes=\"auto, (max-width: 916px) 100vw, 916px\" \/><\/a><\/p>\n<p><strong>Figure 3.<\/strong> Flowchart illustrating the thought process involved in naming simple ionic and covalent compounds and the rules needed to follow.<\/p>\n<div class=\"textbox examples\">\n<h3 itemprop=\"educationalUse\">Activity<\/h3>\n<p>Make yourself a stack of small sized Qcards. \u00a0On one side have the name of an ionic compound (e.g. sodium hydroxide) and on the other side have its chemical formula (e.g. NaOH). \u00a0Use every example found in this chapter &#8211; including those in the exercises. \u00a0Then use these Qcards to quiz yourself.<\/p>\n<\/div>\n<section id=\"fs-idp282340144\" class=\"summary\">\n<div class=\"bcc-box bcc-info\">\n<h3>Exercises<\/h3>\n<div class=\"qandaset block\" id=\"ball-ch03_s02_qs01\">\n<div class=\"question\">\n<div class=\"qandaset block\" id=\"ball-ch03_s04_qs01\">\n<p><span style=\"font-size: 1em\">1. \u00a0Give the formula and name for each ionic compound formed between the two listed ions.<\/span><\/p>\n<div class=\"question\">\n<p>a) \u00a0Mg<sup class=\"superscript\">2+<\/sup> and Cl<sup class=\"superscript\">\u2212 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup>b) \u00a0Fe<sup class=\"superscript\">2+<\/sup> and O<sup class=\"superscript\">2\u2212 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup>c) \u00a0Fe<sup class=\"superscript\">3+<\/sup> and O<sup class=\"superscript\">2\u2212<\/sup><\/p>\n<\/div>\n<p>2<span style=\"font-size: 1em\">. \u00a0Give the formula and name for each ionic compound formed between the two listed ions.<\/span><\/p>\n<div class=\"question\"><\/div>\n<div class=\"question\">\n<p>a) \u00a0Cu<sup class=\"superscript\">2+<\/sup> and F<sup class=\"superscript\">\u2212 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup>b) \u00a0Ca<sup class=\"superscript\">2+<\/sup> and O<sup class=\"superscript\">2\u2212 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup>c) \u00a0K<sup class=\"superscript\">+<\/sup> and P<sup class=\"superscript\">3\u2212<\/sup><\/p>\n<\/div>\n<p><span style=\"font-size: 1em\">3. \u00a0Give the formula and name for each ionic compound formed between the two listed ions.<\/span><\/p>\n<div class=\"question\">\n<p>a) \u00a0K<sup class=\"superscript\">+<\/sup> and SO<sub class=\"subscript\">4<\/sub><sup class=\"superscript\">2\u2212 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup>b) \u00a0NH<sub class=\"subscript\">4<\/sub><sup class=\"superscript\">+<\/sup> and S<sup class=\"superscript\">2\u2212 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup>c) \u00a0NH<sub class=\"subscript\">4<\/sub><sup class=\"superscript\">+<\/sup> and PO<sub class=\"subscript\">4<\/sub><sup class=\"superscript\">3\u2212<\/sup><\/p>\n<\/div>\n<p><span style=\"font-size: 1em\">4. \u00a0Give the formula and name for each ionic compound formed between the two listed ions.<\/span><\/p>\n<div class=\"question\"><\/div>\n<div class=\"question\">\n<p>a) \u00a0Pb<sup class=\"superscript\">4+<\/sup> and SO<sub class=\"subscript\">4<\/sub><sup class=\"superscript\">2\u2212 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup>b) \u00a0Na<sup class=\"superscript\">+<\/sup> and I<sub class=\"subscript\">3<\/sub><sup class=\"superscript\">\u2212 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup>c) \u00a0Li<sup class=\"superscript\">+<\/sup> and Cr<sub class=\"subscript\">2<\/sub>O<sub class=\"subscript\">7<\/sub><sup class=\"superscript\">2\u2212<\/sup><\/p>\n<\/div>\n<p>5<span style=\"font-size: 1em\">. \u00a0Give the formula and name for each ionic compound formed between the two listed ions.<\/span><\/p>\n<div class=\"question\">\n<p>a) \u00a0Ag<sup class=\"superscript\">+<\/sup> and SO<sub class=\"subscript\">3<\/sub><sup class=\"superscript\">2\u2212 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup>b) \u00a0Na<sup class=\"superscript\">+<\/sup> and HCO<sub class=\"subscript\">3<\/sub><sup class=\"superscript\">\u2212 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup>c) \u00a0Fe<sup class=\"superscript\">3+<\/sup> and ClO<sub class=\"subscript\">3<\/sub><sup class=\"superscript\">\u2212<\/sup><\/p>\n<\/div>\n<p><span style=\"font-size: 1em\">6. .Which of these formulas represent molecules? State how many atoms are in each molecule.<\/span><\/p>\n<p>a) \u00a0Fe<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup>b) \u00a0PCl<sub class=\"subscript\">3<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup><\/sub>c) \u00a0P<sub class=\"subscript\">4<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup><\/sub>d) \u00a0Ar<\/p>\n<p><span style=\"font-size: 1em\">7. \u00a0What is the difference between CO and Co?<\/span><\/p>\n<p><span style=\"font-size: 1em\">8. \u00a0Give the proper formula for each diatomic element.<\/span><\/p>\n<p><span style=\"font-size: 1em\">9. \u00a0What is the stem of fluorine used in molecule names? CF<\/span><sub class=\"subscript\">4<\/sub><span style=\"font-size: 1em\"> is one example.<\/span><\/p>\n<p><span style=\"font-size: 1em\">10. \u00a0Give the proper name for each molecule.<\/span><\/p>\n<div class=\"question\">\n<p>a) \u00a0PF<sub class=\"subscript\">3<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup><\/sub>b) \u00a0TeCl<sub class=\"subscript\">2<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup><\/sub>c) \u00a0N<sub class=\"subscript\">2<\/sub>O<sub class=\"subscript\">3<\/sub><\/p>\n<\/div>\n<div class=\"question\">\n<p id=\"ball-ch03_s02_qs01_p17\" class=\"para\">11. \u00a0Give the proper name for each molecule.<\/p>\n<p>a) \u00a0XeF<sub class=\"subscript\">2<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup><\/sub>b) \u00a0O<sub class=\"subscript\">2<\/sub>F<sub class=\"subscript\">2<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup><\/sub>c) \u00a0SF<sub class=\"subscript\">6<\/sub><\/p>\n<\/div>\n<div class=\"question\">\n<p id=\"ball-ch03_s02_qs01_p19\" class=\"para\">12. \u00a0Give the proper name for each molecule.<\/p>\n<p>a) \u00a0N<sub class=\"subscript\">2<\/sub>O<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup>b) \u00a0N<sub class=\"subscript\">2<\/sub>O<sub class=\"subscript\">4<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup><\/sub>c) \u00a0N<sub class=\"subscript\">2<\/sub>O<sub class=\"subscript\">5<\/sub><\/p>\n<\/div>\n<div class=\"question\">\n<p id=\"ball-ch03_s02_qs01_p21\" class=\"para\">13. \u00a0Give the proper formula for each name.<\/p>\n<p>a) \u00a0dinitrogen pentoxide<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup>b) \u00a0tetraboron tricarbide<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup>c) \u00a0phosphorus pentachloride<\/p>\n<\/div>\n<p><span style=\"font-size: 1em\">14. \u00a0Give the proper formula for each name.<\/span><\/p>\n<div class=\"question\">\n<p>a) \u00a0dioxygen dichloride<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup>b) \u00a0dinitrogen trisulfide<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup>c) \u00a0xenon tetrafluoride<\/p>\n<\/div>\n<p><span style=\"font-size: 1em\">15. \u00a0Give the proper formula for each name.<\/span><\/p>\n<div class=\"question\">\n<p>a) \u00a0iodine trifluoride<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup>b) \u00a0xenon trioxide<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup>c) \u00a0disulfur decafluoride<\/p>\n<p><span style=\"font-size: 1em\">16. Give the formula for each acid.<\/span><\/p>\n<\/div>\n<div class=\"qandaset block\" id=\"ball-ch03_s05_qs01\">\n<p>a) \u00a0perchloric acid \u00a0 \u00a0 \u00a0 \u00a0\u00a0b) \u00a0hydroiodic acid<\/p>\n<div class=\"question\">\n<p id=\"ball-ch03_s05_qs01_p3\" class=\"para\">17. Name each acid.<\/p>\n<p>a) \u00a0HF(aq) \u00a0 \u00a0 \u00a0 \u00a0\u00a0b) \u00a0HNO<sub class=\"subscript\">3<\/sub>(aq) \u00a0 \u00a0 \u00a0 \u00a0\u00a0c) \u00a0H<sub class=\"subscript\">2<\/sub>C<sub class=\"subscript\">2<\/sub>O<sub class=\"subscript\">4<\/sub>(aq)<\/p>\n<p><span style=\"font-size: 1em\">18. Name the following compounds:<\/span><\/p>\n<\/div>\n<p id=\"fs-idp282298368\">a) CsCl \u00a0 \u00a0 \u00a0 \u00a0\u00a0b) BaO \u00a0 \u00a0 \u00a0 \u00a0\u00a0c) K<sub>2<\/sub>S \u00a0 \u00a0 \u00a0 \u00a0\u00a0d) BeCl<sub>2 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sub>e) HBr \u00a0 \u00a0 \u00a0 \u00a0\u00a0f) AlF<sub>3<\/sub><\/p>\n<p>19. Write the formulas of the following compounds:<\/p>\n<p id=\"fs-idm306848\">a) rubidium bromide \u00a0 \u00a0 \u00a0 \u00a0\u00a0b) magnesium selenide \u00a0 \u00a0 \u00a0 \u00a0\u00a0c) sodium oxide \u00a0 \u00a0 \u00a0 \u00a0\u00a0d) calcium chloride<\/p>\n<p id=\"fs-idm305184\">e) hydrogen fluoride \u00a0 \u00a0 \u00a0 \u00a0\u00a0f) gallium phosphide \u00a0 \u00a0 \u00a0 \u00a0\u00a0g) aluminum bromide \u00a0 \u00a0 \u00a0 \u00a0\u00a0h) ammonium sulfate<\/p>\n<p>20. Write the formulas of the following compounds:<\/p>\n<p id=\"fs-idp268322592\">a) chlorine dioxide \u00a0 \u00a0 \u00a0 \u00a0\u00a0b) dinitrogen tetraoxide \u00a0 \u00a0 \u00a0 \u00a0\u00a0c) potassium phosphide<\/p>\n<p id=\"fs-idp268323808\">d) silver(I) sulfide \u00a0 \u00a0 \u00a0 \u00a0\u00a0e) aluminum nitride \u00a0 \u00a0 \u00a0 \u00a0\u00a0f) silicon dioxide<\/p>\n<p>21. Each of the following compounds contains a metal that can exhibit more than one ionic charge. Name these compounds:<\/p>\n<p id=\"fs-idp279516416\">a) Cr<sub>2<\/sub>O<sub>3 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sub>b) FeCl<sub>2 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sub>c) CrO<sub>3 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sub>d) TiCl<sub>4 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sub>e) CoO \u00a0 \u00a0 \u00a0 \u00a0\u00a0f) MoS<sub>2<\/sub><\/p>\n<p>22. The following ionic compounds are found in common household products. Write the formulas for each compound:<\/p>\n<p id=\"fs-idp268366192\">a) potassium phosphate \u00a0 \u00a0 \u00a0 \u00a0\u00a0b) copper(II) sulfate \u00a0 \u00a0 \u00a0 \u00a0\u00a0c) calcium chloride<\/p>\n<p id=\"fs-idp282328976\">d) titanium dioxide \u00a0 \u00a0 \u00a0 \u00a0\u00a0e) ammonium nitrate<\/p>\n<p>f) sodium bisulfate (the common name for sodium hydrogen sulfate)<\/p>\n<p>23. What are the IUPAC names of the following compounds?<\/p>\n<p id=\"fs-idp268311808\">a) manganese dioxide \u00a0 \u00a0 \u00a0 \u00a0\u00a0b) mercurous chloride (Hg<sub>2<\/sub>Cl<sub>2<\/sub>) \u00a0 \u00a0 \u00a0 \u00a0\u00a0c) ferric nitrate [Fe(NO<sub>3<\/sub>)<sub>3<\/sub>]<\/p>\n<p id=\"fs-idp282287056\">d) titanium tetrachloride \u00a0 \u00a0 \u00a0 \u00a0\u00a0e) cupric bromide (CuBr<sub>2<\/sub>)<\/p>\n<\/div>\n<p>&nbsp;<\/p>\n<\/div>\n<p><b>Answers<\/b><\/p>\n<p>1. a) \u00a0magnesium chloride, MgCl<sub class=\"subscript\">2<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup><\/sub>b) \u00a0iron(II) oxide, FeO<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup>c) \u00a0iron(III) oxide, Fe<sub class=\"subscript\">2<\/sub>O<sub class=\"subscript\">3<\/sub><\/p>\n<p>2.\u00a0a) \u00a0copper(II) fluoride, CuF<sub class=\"subscript\">2<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup><\/sub>b) \u00a0calcium oxide, CaO<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup>c) \u00a0potassium phosphide, K<sub class=\"subscript\">3<\/sub>P<\/p>\n<p>3.\u00a0a) \u00a0potassium sulfate, K<sub class=\"subscript\">2<\/sub>SO<sub class=\"subscript\">4<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup><\/sub>b) \u00a0ammonium sulfide, (NH<sub class=\"subscript\">4<\/sub>)<sub class=\"subscript\">2<\/sub>S<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup>c) \u00a0ammonium phosphate, (NH<sub class=\"subscript\">4<\/sub>)<sub class=\"subscript\">3<\/sub>PO<sub class=\"subscript\">4<\/sub><\/p>\n<p>4.\u00a0a) \u00a0lead(IV) sulfate, Pb(SO<sub class=\"subscript\">4<\/sub>)<sub class=\"subscript\">2<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup><\/sub>b) \u00a0sodium triiodide, NaI<sub class=\"subscript\">3<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup><\/sub>c) \u00a0lithium dichromate, Li<sub class=\"subscript\">2<\/sub>Cr<sub class=\"subscript\">2<\/sub>O<sub class=\"subscript\">7<\/sub><\/p>\n<p>5.\u00a0a) \u00a0silver sulfite, Ag<sub class=\"subscript\">2<\/sub>SO<sub class=\"subscript\">3<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup><\/sub>b) \u00a0sodium hydrogen carbonate, NaHCO<sub class=\"subscript\">3<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup><\/sub>c) \u00a0iron(III) chlorate, Fe(ClO<sub class=\"subscript\">3<\/sub>)<sub class=\"subscript\">3<\/sub><\/p>\n<p>6. a) \u00a0not a molecule<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup>b) \u00a0a molecule; four atoms total<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup>c) \u00a0a molecule; four atoms total<\/p>\n<p>d) \u00a0not a molecule<\/p>\n<p><span style=\"font-size: 1em\">7.\u00a0CO is a compound of carbon and oxygen; Co is the element cobalt.<\/span><\/p>\n<p>8.\u00a0H<sub class=\"subscript\">2<\/sub>, O<sub class=\"subscript\">2<\/sub>, N<sub class=\"subscript\">2<\/sub>, F<sub class=\"subscript\">2<\/sub>, Cl<sub class=\"subscript\">2<\/sub>, Br<sub class=\"subscript\">2<\/sub>, I<sub class=\"subscript\">2<\/sub><\/p>\n<p>9. \u00a0<em class=\"emphasis\">fluor-<\/em><\/p>\n<p>10.\u00a0a) \u00a0phosphorus trifluoride<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup>b) \u00a0tellurium dichloride<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup>c) \u00a0dinitrogen trioxide<\/p>\n<p>11.\u00a0a) \u00a0xenon difluoride<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup>b) \u00a0dioxygen difluoride<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup>c) \u00a0sulfur hexafluoride<\/p>\n<p>12.\u00a0a) \u00a0dinitrogen monoxide<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup>b) \u00a0dinitrogen tetroxide<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup>c) \u00a0dinitrogen pentoxide<\/p>\n<p>13.\u00a0a) \u00a0N<sub class=\"subscript\">2<\/sub>O<sub class=\"subscript\">5<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup><\/sub>b) \u00a0B<sub class=\"subscript\">4<\/sub>C<sub class=\"subscript\">3<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup><\/sub>c) \u00a0PCl<sub class=\"subscript\">5<\/sub><\/p>\n<p>14.\u00a0a) \u00a0O<sub class=\"subscript\">2<\/sub>Cl<sub class=\"subscript\">2<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup><\/sub>b) \u00a0N<sub class=\"subscript\">2<\/sub>S<sub class=\"subscript\">3<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup><\/sub>c) \u00a0XeF<sub class=\"subscript\">4<\/sub><\/p>\n<p>15.\u00a0a) \u00a0IF<sub class=\"subscript\">3<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup><\/sub>b) \u00a0XeO<sub class=\"subscript\">3<sup class=\"superscript\"> \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup><\/sub>c) \u00a0S<sub class=\"subscript\">2<\/sub>F<sub class=\"subscript\">10<\/sub><\/p>\n<\/div>\n<p>16.\u00a0<span style=\"font-size: 1em\">a) \u00a0HClO<\/span><sub class=\"subscript\">4<\/sub><span style=\"font-size: 1em\">(aq) \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/span><span style=\"font-size: 1em\">b) \u00a0HI(aq)<\/span><\/p>\n<\/div>\n<p>17.\u00a0a) \u00a0hydrofluoric acid \u00a0 \u00a0 \u00a0 \u00a0\u00a0b) \u00a0nitric acid \u00a0 \u00a0 \u00a0 \u00a0\u00a0c) \u00a0oxalic acid<\/p>\n<p id=\"fs-idp283374992\">18. a) cesium chloride \u00a0 \u00a0 \u00a0 \u00a0 b) barium oxide \u00a0 \u00a0 \u00a0 \u00a0 c) potassium sulfide<\/p>\n<p>d) beryllium chloride \u00a0 \u00a0 \u00a0 \u00a0 e) hydrogen bromide \u00a0 \u00a0 \u00a0 \u00a0 f) aluminum fluoride<\/p>\n<p id=\"fs-idm303264\">19. a) RbBr \u00a0 \u00a0 \u00a0 \u00a0 b) MgSe \u00a0 \u00a0 \u00a0 \u00a0 c) Na<sub>2<\/sub>O \u00a0 \u00a0 \u00a0 \u00a0 d) CaCl<sub>2 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sub>e) HF \u00a0 \u00a0 \u00a0 \u00a0 f) GaP \u00a0 \u00a0 \u00a0 \u00a0 g) AlBr<sub>3 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sub>h) (NH<sub>4<\/sub>)<sub>2<\/sub>SO<sub>4<\/sub><\/p>\n<p id=\"fs-idp268325312\">20. a) ClO<sub>2 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sub>b) N<sub>2<\/sub>O<sub>4 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sub>c) K<sub>3<\/sub>P \u00a0 \u00a0 \u00a0 \u00a0 d) Ag<sub>2<\/sub>S \u00a0 \u00a0 \u00a0 \u00a0 e) AlN \u00a0 \u00a0 \u00a0 \u00a0 f) SiO<sub>2<\/sub><\/p>\n<p id=\"fs-idp268274112\">21. a) chromium(III) oxide \u00a0 \u00a0 \u00a0 \u00a0 b) iron(II) chloride \u00a0 \u00a0 \u00a0 \u00a0 c) chromium(VI) oxide<\/p>\n<p>d) titanium(IV) chloride \u00a0 \u00a0 \u00a0 \u00a0 e) cobalt(II) oxide \u00a0 \u00a0 \u00a0 \u00a0 f) molybdenum(IV) sulfide<\/p>\n<p id=\"fs-idp282330448\">22. a) K<sub>3<\/sub>PO<sub>4 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sub>b) CuSO<sub>4 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sub>c) CaCl<sub>2 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sub>d) TiO<sub>2 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sub>e) NH<sub>4<\/sub>NO<sub>3 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sub>f) NaHSO<sub>4<\/sub><\/p>\n<p id=\"fs-idp282288464\">23. a) manganese(IV) oxide \u00a0 \u00a0 \u00a0 \u00a0 b) mercury(I) chloride \u00a0 \u00a0 \u00a0 \u00a0 c) iron(III) nitrate<\/p>\n<p>d) titanium(IV) chloride \u00a0 \u00a0 \u00a0 \u00a0 e) copper(II) bromide<\/p>\n<\/div>\n<\/section>\n<div>\n<h2>Glossary<\/h2>\n<p><strong>binary acid:\u00a0<\/strong>compound that contains hydrogen and one other element, bonded in a way that imparts acidic properties to the compound (ability to release H<sup>+<\/sup> ions when dissolved in water)<\/p>\n<p><strong>binary compound:\u00a0<\/strong>compound containing two different elements.<\/p>\n<p><strong>nomenclature:\u00a0<\/strong>system of rules for naming objects of interest<\/p>\n<p><strong>oxyacid:\u00a0<\/strong>compound that contains hydrogen, oxygen, and one other element, bonded in a way that imparts acidic properties to the compound (ability to release H<sup>+<\/sup> ions when dissolved in water)<\/p>\n<\/div>\n","protected":false},"author":330,"menu_order":4,"template":"","meta":{"pb_show_title":"on","pb_short_title":"4.3 Nomenclature of Simple Ionic and Molecular 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