{"id":841,"date":"2021-07-23T09:20:51","date_gmt":"2021-07-23T13:20:51","guid":{"rendered":"https:\/\/pressbooks.bccampus.ca\/aperrott\/chapter\/lewis-acids-and-bases\/"},"modified":"2022-06-23T09:22:26","modified_gmt":"2022-06-23T13:22:26","slug":"lewis-acids-and-bases","status":"publish","type":"chapter","link":"https:\/\/pressbooks.bccampus.ca\/aperrott\/chapter\/lewis-acids-and-bases\/","title":{"raw":"15.2 Lewis Acids and Bases","rendered":"15.2 Lewis Acids and Bases"},"content":{"raw":"&nbsp;\r\n<div class=\"textbox textbox--learning-objectives\">\r\n<h3><strong>Learning Objectives<\/strong><\/h3>\r\nBy the end of this section, you will be able to:\r\n<ul>\r\n \t<li>Explain the Lewis model of acid-base chemistry<\/li>\r\n<\/ul>\r\n<\/div>\r\n<p id=\"fs-idp51077712\">In 1923, G. N. <span class=\"no-emphasis\" data-type=\"term\">Lewis<\/span> proposed a generalized definition of acid-base behavior in which acids and bases are identified by their ability to accept or to donate a pair of electrons and form a coordinate covalent bond.<\/p>\r\n<p id=\"fs-idp107912128\">A <span data-type=\"term\">coordinate covalent bond<\/span> (or dative bond) occurs when one of the atoms in the bond provides both bonding electrons. For example, a coordinate covalent bond occurs when a water molecule combines with a hydrogen ion to form a hydronium ion. A coordinate covalent bond also results when an ammonia molecule combines with a hydrogen ion to form an ammonium ion. Both of these equations are shown here.<\/p>\r\n<span id=\"fs-idm2583104\" class=\"scaled-down\" data-type=\"media\" data-alt=\"This figure shows two reactions represented with Lewis structures. The first shows an O atom bonded to two H atoms. The O atom has two lone pairs of electrons. There is a plus sign and then an H atom with a superscript positive sign followed by a right-facing arrow. The next Lewis structure is in brackets and shows an O atom bonded to three H atoms. There is one lone pair of electrons on the O atom. Outside of the brackets is a superscript positive sign. The second reaction shows an N atom bonded to three H atoms. The N atom has one lone pair of electrons. There is a plus sign and then an H superscript positive sign. After the H superscript positive sign is a right-facing arrow. The next Lewis structure is in brackets. It shows an N atom bonded to four H atoms. There is a superscript positive sign outside the brackets.\"><img src=\"https:\/\/pressbooks.bccampus.ca\/aperrott\/wp-content\/uploads\/sites\/1463\/2021\/07\/CNX_Chem_15_03_hydronium_img-1.jpg\" alt=\"This figure shows two reactions represented with Lewis structures. The first shows an O atom bonded to two H atoms. The O atom has two lone pairs of electrons. There is a plus sign and then an H atom with a superscript positive sign followed by a right-facing arrow. The next Lewis structure is in brackets and shows an O atom bonded to three H atoms. There is one lone pair of electrons on the O atom. Outside of the brackets is a superscript positive sign. The second reaction shows an N atom bonded to three H atoms. The N atom has one lone pair of electrons. There is a plus sign and then an H superscript positive sign. After the H superscript positive sign is a right-facing arrow. The next Lewis structure is in brackets. It shows an N atom bonded to four H atoms. There is a superscript positive sign outside the brackets.\" data-media-type=\"image\/jpeg\" \/><\/span>\r\n<p id=\"fs-idp133241888\">Reactions involving the formation of coordinate covalent bonds are classified as <strong>Lewis acid-base chemistry<\/strong>. The species donating the electron pair that compose the bond is a <strong>Lewis base<\/strong>, the species accepting the electron pair is a <strong>Lewis acid<\/strong>, and the product of the reaction is a <span data-type=\"term\">Lewis acid-base adduct<\/span>. As the two examples above illustrate, Br\u00f8nsted-Lowry acid-base reactions represent a subcategory of Lewis acid reactions, specifically, those in which the acid species is H<sup>+<\/sup>. A few examples involving other Lewis acids and bases are described below.<\/p>\r\n<p id=\"fs-idm91313680\">The boron atom in boron trifluoride, BF<sub>3<\/sub>, has only six electrons in its valence shell. Being short of the preferred octet, BF<sub>3<\/sub> is a very good Lewis acid and reacts with many Lewis bases; a fluoride ion is the Lewis base in this reaction, donating one of its lone pairs:<\/p>\r\n<span id=\"fs-idp160186064\" class=\"scaled-down\" data-type=\"media\" data-alt=\"This figure illustrates a chemical reaction using structural formulas. On the left, an F atom is surrounded by four electron dot pairs and has a superscript negative symbol. This structure is labeled below as \u201cLewis base.\u201d Following a plus sign is another structure which has a B atom at the center and three F atoms single bonded above, right, and below. Each F atom has three pairs of electron dots. This structure is labeled below as \u201cLewis acid.\u201d Following a right pointing arrow is a structure in brackets that has a central B atom to which 4 F atoms are connected with single bonds above, below, to the left, and to the right. Each F atom in this structure has three pairs of electron dots. Outside the brackets is a superscript negative symbol. This structure is labeled below as \u201cAcid-base adduct.\u201d\"><img src=\"https:\/\/pressbooks.bccampus.ca\/aperrott\/wp-content\/uploads\/sites\/1463\/2021\/07\/CNX_Chem_15_02_BF3-LA_img-1.jpg\" alt=\"This figure illustrates a chemical reaction using structural formulas. On the left, an F atom is surrounded by four electron dot pairs and has a superscript negative symbol. This structure is labeled below as \u201cLewis base.\u201d Following a plus sign is another structure which has a B atom at the center and three F atoms single bonded above, right, and below. Each F atom has three pairs of electron dots. This structure is labeled below as \u201cLewis acid.\u201d Following a right pointing arrow is a structure in brackets that has a central B atom to which 4 F atoms are connected with single bonds above, below, to the left, and to the right. Each F atom in this structure has three pairs of electron dots. Outside the brackets is a superscript negative symbol. This structure is labeled below as \u201cAcid-base adduct.\u201d\" data-media-type=\"image\/jpeg\" \/><\/span>\r\n<p id=\"fs-idp34388288\">In the following reaction, each of two ammonia molecules, Lewis bases, donates a pair of electrons to a silver ion, the Lewis acid:<\/p>\r\n<span id=\"fs-idp134365040\" class=\"scaled-down\" data-type=\"media\" data-alt=\"This figure illustrates a chemical reaction using structural formulas. On the left side, a 2 preceeds an N atom which has H atoms single bonded above, to the left, and below. A single electron dot pair is on the right side of the N atom. This structure is labeled below as \u201cLewis base.\u201d Following a plus sign is an A g atom which has a superscript plus symbol. Following a right pointing arrow is a structure in brackets that has a central A g atom to which N atoms are connected with single bonds to the left and to the right. Each of these N atoms has H atoms bonded above, below, and to the outside of the structure. Outside the brackets is a superscript plus symbol. This structure is labeled below as \u201cAcid-base adduct.\u201d\"><img src=\"https:\/\/pressbooks.bccampus.ca\/aperrott\/wp-content\/uploads\/sites\/1463\/2021\/07\/CNX_Chem_15_02_NH3-LBase_img-1.jpg\" alt=\"This figure illustrates a chemical reaction using structural formulas. On the left side, a 2 preceeds an N atom which has H atoms single bonded above, to the left, and below. A single electron dot pair is on the right side of the N atom. This structure is labeled below as \u201cLewis base.\u201d Following a plus sign is an A g atom which has a superscript plus symbol. Following a right pointing arrow is a structure in brackets that has a central A g atom to which N atoms are connected with single bonds to the left and to the right. Each of these N atoms has H atoms bonded above, below, and to the outside of the structure. Outside the brackets is a superscript plus symbol. This structure is labeled below as \u201cAcid-base adduct.\u201d\" data-media-type=\"image\/jpeg\" \/><\/span>\r\n<p id=\"fs-idm82519616\">Nonmetal oxides act as Lewis acids and react with oxide ions, Lewis bases, to form oxyanions:<\/p>\r\n<span id=\"fs-idm21887312\" class=\"scaled-down\" data-type=\"media\" data-alt=\"This figure illustrates a chemical reaction using structural formulas. On the left, an O atom is surrounded by four electron dot pairs and has a superscript 2 negative. This structure is labeled below as \u201cLewis base.\u201d Following a plus sign is another structure which has an S atom at the center. O atoms are single bonded above and below. These O atoms have three electron dot pairs each. To the right of the S atom is a double bonded O atom which has two pairs of electron dots. This structure is labeled below as \u201cLewis acid.\u201d Following a right pointing arrow is a structure in brackets that has a central S atom to which 4 O atoms are connected with single bonds above, below, to the left, and to the right. Each of the O atoms has three pairs of electron dots. Outside the brackets is a superscript 2 negative. This structure is labeled below as \u201cAcid-base adduct.\u201d\"><img src=\"https:\/\/pressbooks.bccampus.ca\/aperrott\/wp-content\/uploads\/sites\/1463\/2021\/07\/CNX_Chem_15_02_NonmetalOx_img-1.jpg\" alt=\"This figure illustrates a chemical reaction using structural formulas. On the left, an O atom is surrounded by four electron dot pairs and has a superscript 2 negative. This structure is labeled below as \u201cLewis base.\u201d Following a plus sign is another structure which has an S atom at the center. O atoms are single bonded above and below. These O atoms have three electron dot pairs each. To the right of the S atom is a double bonded O atom which has two pairs of electron dots. This structure is labeled below as \u201cLewis acid.\u201d Following a right pointing arrow is a structure in brackets that has a central S atom to which 4 O atoms are connected with single bonds above, below, to the left, and to the right. Each of the O atoms has three pairs of electron dots. Outside the brackets is a superscript 2 negative. This structure is labeled below as \u201cAcid-base adduct.\u201d\" data-media-type=\"image\/jpeg\" \/><\/span>\r\n<p id=\"fs-idm28146992\">Another type of Lewis acid-base chemistry involves the formation of a complex ion (or a coordination complex) comprising a central atom, typically a transition metal cation, surrounded by ions or molecules called <strong>ligands<\/strong>. These ligands can be neutral molecules like H<sub>2<\/sub>O or NH<sub>3<\/sub>, or ions such as CN<sup>\u2013<\/sup> or OH<sup>\u2013<\/sup>. Often, the ligands act as Lewis bases, donating a pair of electrons to the central atom. These types of Lewis acid-base reactions are examples of a broad subdiscipline called <em data-effect=\"italics\">coordination chemistry.<\/em><\/p>\r\n\r\n<div id=\"fs-idp45945376\" class=\"summary\" data-depth=\"1\">\r\n<h3 data-type=\"title\"><strong>Key Concepts and Summary<\/strong><\/h3>\r\n<p id=\"fs-idm14023472\">A Lewis acid is a species that can accept an electron pair, whereas a Lewis base has an electron pair available for donation to a Lewis acid. Complex ions are examples of Lewis acid-base adducts and comprise central metal atoms or ions acting as Lewis acids bonded to molecules or ions called ligands that act as Lewis bases.<\/p>\r\n\r\n<\/div>\r\n<div class=\"textbox shaded\" data-type=\"glossary\">\r\n<h3 data-type=\"glossary-title\"><strong>Glossary<\/strong><\/h3>\r\n<dl id=\"fs-idm90510160\">\r\n \t<dt>complex ion<\/dt>\r\n \t<dd id=\"fs-idm90509776\">ion consisting of a central atom surrounding molecules or ions called ligands via coordinate covalent bonds<\/dd>\r\n<\/dl>\r\n<dl id=\"fs-idp1460096\">\r\n \t<dt>coordinate covalent bond<\/dt>\r\n \t<dd id=\"fs-idp143749120\">(also, dative bond) covalent bond in which both electrons originated from the same atom<\/dd>\r\n<\/dl>\r\n<dl id=\"fs-idp11302544\">\r\n \t<dt>Lewis acid<\/dt>\r\n \t<dd id=\"fs-idp11302928\">any species that can accept a pair of electrons and form a coordinate covalent bond<\/dd>\r\n<\/dl>\r\n<dl id=\"fs-idm26641568\">\r\n \t<dt>Lewis acid-base adduct<\/dt>\r\n \t<dd id=\"fs-idm26641184\">compound or ion that contains a coordinate covalent bond between a Lewis acid and a Lewis base<\/dd>\r\n<\/dl>\r\n<dl id=\"fs-idm465112896\">\r\n \t<dt>Lewis acid-base chemistry<\/dt>\r\n \t<dd id=\"fs-idm101700960a\">reactions involving the formation of coordinate covalent bonds<\/dd>\r\n<\/dl>\r\n<dl id=\"fs-idp29842512\">\r\n \t<dt>Lewis base<\/dt>\r\n \t<dd id=\"fs-idm101700960\">any species that can donate a pair of electrons and form a coordinate covalent bond<\/dd>\r\n<\/dl>\r\n<dl id=\"fs-idm101700576\">\r\n \t<dt>ligand<\/dt>\r\n \t<dd id=\"fs-idp77291984\">molecule or ion acting as a Lewis base in complex ion formation; bonds to the central atom of the complex<\/dd>\r\n<\/dl>\r\n<\/div>","rendered":"<p>&nbsp;<\/p>\n<div class=\"textbox textbox--learning-objectives\">\n<h3><strong>Learning Objectives<\/strong><\/h3>\n<p>By the end of this section, you will be able to:<\/p>\n<ul>\n<li>Explain the Lewis model of acid-base chemistry<\/li>\n<\/ul>\n<\/div>\n<p id=\"fs-idp51077712\">In 1923, G. N. <span class=\"no-emphasis\" data-type=\"term\">Lewis<\/span> proposed a generalized definition of acid-base behavior in which acids and bases are identified by their ability to accept or to donate a pair of electrons and form a coordinate covalent bond.<\/p>\n<p id=\"fs-idp107912128\">A <span data-type=\"term\">coordinate covalent bond<\/span> (or dative bond) occurs when one of the atoms in the bond provides both bonding electrons. For example, a coordinate covalent bond occurs when a water molecule combines with a hydrogen ion to form a hydronium ion. A coordinate covalent bond also results when an ammonia molecule combines with a hydrogen ion to form an ammonium ion. Both of these equations are shown here.<\/p>\n<p><span id=\"fs-idm2583104\" class=\"scaled-down\" data-type=\"media\" data-alt=\"This figure shows two reactions represented with Lewis structures. The first shows an O atom bonded to two H atoms. The O atom has two lone pairs of electrons. There is a plus sign and then an H atom with a superscript positive sign followed by a right-facing arrow. The next Lewis structure is in brackets and shows an O atom bonded to three H atoms. There is one lone pair of electrons on the O atom. Outside of the brackets is a superscript positive sign. The second reaction shows an N atom bonded to three H atoms. The N atom has one lone pair of electrons. There is a plus sign and then an H superscript positive sign. After the H superscript positive sign is a right-facing arrow. The next Lewis structure is in brackets. It shows an N atom bonded to four H atoms. There is a superscript positive sign outside the brackets.\"><img decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/aperrott\/wp-content\/uploads\/sites\/1463\/2021\/07\/CNX_Chem_15_03_hydronium_img-1.jpg\" alt=\"This figure shows two reactions represented with Lewis structures. The first shows an O atom bonded to two H atoms. The O atom has two lone pairs of electrons. There is a plus sign and then an H atom with a superscript positive sign followed by a right-facing arrow. The next Lewis structure is in brackets and shows an O atom bonded to three H atoms. There is one lone pair of electrons on the O atom. Outside of the brackets is a superscript positive sign. The second reaction shows an N atom bonded to three H atoms. The N atom has one lone pair of electrons. There is a plus sign and then an H superscript positive sign. After the H superscript positive sign is a right-facing arrow. The next Lewis structure is in brackets. It shows an N atom bonded to four H atoms. There is a superscript positive sign outside the brackets.\" data-media-type=\"image\/jpeg\" \/><\/span><\/p>\n<p id=\"fs-idp133241888\">Reactions involving the formation of coordinate covalent bonds are classified as <strong>Lewis acid-base chemistry<\/strong>. The species donating the electron pair that compose the bond is a <strong>Lewis base<\/strong>, the species accepting the electron pair is a <strong>Lewis acid<\/strong>, and the product of the reaction is a <span data-type=\"term\">Lewis acid-base adduct<\/span>. As the two examples above illustrate, Br\u00f8nsted-Lowry acid-base reactions represent a subcategory of Lewis acid reactions, specifically, those in which the acid species is H<sup>+<\/sup>. A few examples involving other Lewis acids and bases are described below.<\/p>\n<p id=\"fs-idm91313680\">The boron atom in boron trifluoride, BF<sub>3<\/sub>, has only six electrons in its valence shell. Being short of the preferred octet, BF<sub>3<\/sub> is a very good Lewis acid and reacts with many Lewis bases; a fluoride ion is the Lewis base in this reaction, donating one of its lone pairs:<\/p>\n<p><span id=\"fs-idp160186064\" class=\"scaled-down\" data-type=\"media\" data-alt=\"This figure illustrates a chemical reaction using structural formulas. On the left, an F atom is surrounded by four electron dot pairs and has a superscript negative symbol. This structure is labeled below as \u201cLewis base.\u201d Following a plus sign is another structure which has a B atom at the center and three F atoms single bonded above, right, and below. Each F atom has three pairs of electron dots. This structure is labeled below as \u201cLewis acid.\u201d Following a right pointing arrow is a structure in brackets that has a central B atom to which 4 F atoms are connected with single bonds above, below, to the left, and to the right. Each F atom in this structure has three pairs of electron dots. Outside the brackets is a superscript negative symbol. This structure is labeled below as \u201cAcid-base adduct.\u201d\"><img decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/aperrott\/wp-content\/uploads\/sites\/1463\/2021\/07\/CNX_Chem_15_02_BF3-LA_img-1.jpg\" alt=\"This figure illustrates a chemical reaction using structural formulas. On the left, an F atom is surrounded by four electron dot pairs and has a superscript negative symbol. This structure is labeled below as \u201cLewis base.\u201d Following a plus sign is another structure which has a B atom at the center and three F atoms single bonded above, right, and below. Each F atom has three pairs of electron dots. This structure is labeled below as \u201cLewis acid.\u201d Following a right pointing arrow is a structure in brackets that has a central B atom to which 4 F atoms are connected with single bonds above, below, to the left, and to the right. Each F atom in this structure has three pairs of electron dots. Outside the brackets is a superscript negative symbol. This structure is labeled below as \u201cAcid-base adduct.\u201d\" data-media-type=\"image\/jpeg\" \/><\/span><\/p>\n<p id=\"fs-idp34388288\">In the following reaction, each of two ammonia molecules, Lewis bases, donates a pair of electrons to a silver ion, the Lewis acid:<\/p>\n<p><span id=\"fs-idp134365040\" class=\"scaled-down\" data-type=\"media\" data-alt=\"This figure illustrates a chemical reaction using structural formulas. On the left side, a 2 preceeds an N atom which has H atoms single bonded above, to the left, and below. A single electron dot pair is on the right side of the N atom. This structure is labeled below as \u201cLewis base.\u201d Following a plus sign is an A g atom which has a superscript plus symbol. Following a right pointing arrow is a structure in brackets that has a central A g atom to which N atoms are connected with single bonds to the left and to the right. Each of these N atoms has H atoms bonded above, below, and to the outside of the structure. Outside the brackets is a superscript plus symbol. This structure is labeled below as \u201cAcid-base adduct.\u201d\"><img decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/aperrott\/wp-content\/uploads\/sites\/1463\/2021\/07\/CNX_Chem_15_02_NH3-LBase_img-1.jpg\" alt=\"This figure illustrates a chemical reaction using structural formulas. On the left side, a 2 preceeds an N atom which has H atoms single bonded above, to the left, and below. A single electron dot pair is on the right side of the N atom. This structure is labeled below as \u201cLewis base.\u201d Following a plus sign is an A g atom which has a superscript plus symbol. Following a right pointing arrow is a structure in brackets that has a central A g atom to which N atoms are connected with single bonds to the left and to the right. Each of these N atoms has H atoms bonded above, below, and to the outside of the structure. Outside the brackets is a superscript plus symbol. This structure is labeled below as \u201cAcid-base adduct.\u201d\" data-media-type=\"image\/jpeg\" \/><\/span><\/p>\n<p id=\"fs-idm82519616\">Nonmetal oxides act as Lewis acids and react with oxide ions, Lewis bases, to form oxyanions:<\/p>\n<p><span id=\"fs-idm21887312\" class=\"scaled-down\" data-type=\"media\" data-alt=\"This figure illustrates a chemical reaction using structural formulas. On the left, an O atom is surrounded by four electron dot pairs and has a superscript 2 negative. This structure is labeled below as \u201cLewis base.\u201d Following a plus sign is another structure which has an S atom at the center. O atoms are single bonded above and below. These O atoms have three electron dot pairs each. To the right of the S atom is a double bonded O atom which has two pairs of electron dots. This structure is labeled below as \u201cLewis acid.\u201d Following a right pointing arrow is a structure in brackets that has a central S atom to which 4 O atoms are connected with single bonds above, below, to the left, and to the right. Each of the O atoms has three pairs of electron dots. Outside the brackets is a superscript 2 negative. This structure is labeled below as \u201cAcid-base adduct.\u201d\"><img decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/aperrott\/wp-content\/uploads\/sites\/1463\/2021\/07\/CNX_Chem_15_02_NonmetalOx_img-1.jpg\" alt=\"This figure illustrates a chemical reaction using structural formulas. On the left, an O atom is surrounded by four electron dot pairs and has a superscript 2 negative. This structure is labeled below as \u201cLewis base.\u201d Following a plus sign is another structure which has an S atom at the center. O atoms are single bonded above and below. These O atoms have three electron dot pairs each. To the right of the S atom is a double bonded O atom which has two pairs of electron dots. This structure is labeled below as \u201cLewis acid.\u201d Following a right pointing arrow is a structure in brackets that has a central S atom to which 4 O atoms are connected with single bonds above, below, to the left, and to the right. Each of the O atoms has three pairs of electron dots. Outside the brackets is a superscript 2 negative. This structure is labeled below as \u201cAcid-base adduct.\u201d\" data-media-type=\"image\/jpeg\" \/><\/span><\/p>\n<p id=\"fs-idm28146992\">Another type of Lewis acid-base chemistry involves the formation of a complex ion (or a coordination complex) comprising a central atom, typically a transition metal cation, surrounded by ions or molecules called <strong>ligands<\/strong>. These ligands can be neutral molecules like H<sub>2<\/sub>O or NH<sub>3<\/sub>, or ions such as CN<sup>\u2013<\/sup> or OH<sup>\u2013<\/sup>. Often, the ligands act as Lewis bases, donating a pair of electrons to the central atom. These types of Lewis acid-base reactions are examples of a broad subdiscipline called <em data-effect=\"italics\">coordination chemistry.<\/em><\/p>\n<div id=\"fs-idp45945376\" class=\"summary\" data-depth=\"1\">\n<h3 data-type=\"title\"><strong>Key Concepts and Summary<\/strong><\/h3>\n<p id=\"fs-idm14023472\">A Lewis acid is a species that can accept an electron pair, whereas a Lewis base has an electron pair available for donation to a Lewis acid. Complex ions are examples of Lewis acid-base adducts and comprise central metal atoms or ions acting as Lewis acids bonded to molecules or ions called ligands that act as Lewis bases.<\/p>\n<\/div>\n<div class=\"textbox shaded\" data-type=\"glossary\">\n<h3 data-type=\"glossary-title\"><strong>Glossary<\/strong><\/h3>\n<dl id=\"fs-idm90510160\">\n<dt>complex ion<\/dt>\n<dd id=\"fs-idm90509776\">ion consisting of a central atom surrounding molecules or ions called ligands via coordinate covalent bonds<\/dd>\n<\/dl>\n<dl id=\"fs-idp1460096\">\n<dt>coordinate covalent bond<\/dt>\n<dd id=\"fs-idp143749120\">(also, dative bond) covalent bond in which both electrons originated from the same atom<\/dd>\n<\/dl>\n<dl id=\"fs-idp11302544\">\n<dt>Lewis acid<\/dt>\n<dd id=\"fs-idp11302928\">any species that can accept a pair of electrons and form a coordinate covalent bond<\/dd>\n<\/dl>\n<dl id=\"fs-idm26641568\">\n<dt>Lewis acid-base adduct<\/dt>\n<dd id=\"fs-idm26641184\">compound or ion that contains a coordinate covalent bond between a Lewis acid and a Lewis base<\/dd>\n<\/dl>\n<dl id=\"fs-idm465112896\">\n<dt>Lewis acid-base chemistry<\/dt>\n<dd id=\"fs-idm101700960a\">reactions involving the formation of coordinate covalent bonds<\/dd>\n<\/dl>\n<dl id=\"fs-idp29842512\">\n<dt>Lewis base<\/dt>\n<dd id=\"fs-idm101700960\">any species that can donate a pair of electrons and form a coordinate covalent bond<\/dd>\n<\/dl>\n<dl id=\"fs-idm101700576\">\n<dt>ligand<\/dt>\n<dd id=\"fs-idp77291984\">molecule or ion acting as a Lewis base in complex ion formation; bonds to the central atom of the complex<\/dd>\n<\/dl>\n<\/div>\n","protected":false},"author":1392,"menu_order":3,"template":"","meta":{"pb_show_title":"on","pb_short_title":"","pb_subtitle":"","pb_authors":[],"pb_section_license":""},"chapter-type":[48],"contributor":[],"license":[],"class_list":["post-841","chapter","type-chapter","status-publish","hentry","chapter-type-numberless"],"part":811,"_links":{"self":[{"href":"https:\/\/pressbooks.bccampus.ca\/aperrott\/wp-json\/pressbooks\/v2\/chapters\/841","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/pressbooks.bccampus.ca\/aperrott\/wp-json\/pressbooks\/v2\/chapters"}],"about":[{"href":"https:\/\/pressbooks.bccampus.ca\/aperrott\/wp-json\/wp\/v2\/types\/chapter"}],"author":[{"embeddable":true,"href":"https:\/\/pressbooks.bccampus.ca\/aperrott\/wp-json\/wp\/v2\/users\/1392"}],"version-history":[{"count":2,"href":"https:\/\/pressbooks.bccampus.ca\/aperrott\/wp-json\/pressbooks\/v2\/chapters\/841\/revisions"}],"predecessor-version":[{"id":2178,"href":"https:\/\/pressbooks.bccampus.ca\/aperrott\/wp-json\/pressbooks\/v2\/chapters\/841\/revisions\/2178"}],"part":[{"href":"https:\/\/pressbooks.bccampus.ca\/aperrott\/wp-json\/pressbooks\/v2\/parts\/811"}],"metadata":[{"href":"https:\/\/pressbooks.bccampus.ca\/aperrott\/wp-json\/pressbooks\/v2\/chapters\/841\/metadata\/"}],"wp:attachment":[{"href":"https:\/\/pressbooks.bccampus.ca\/aperrott\/wp-json\/wp\/v2\/media?parent=841"}],"wp:term":[{"taxonomy":"chapter-type","embeddable":true,"href":"https:\/\/pressbooks.bccampus.ca\/aperrott\/wp-json\/pressbooks\/v2\/chapter-type?post=841"},{"taxonomy":"contributor","embeddable":true,"href":"https:\/\/pressbooks.bccampus.ca\/aperrott\/wp-json\/wp\/v2\/contributor?post=841"},{"taxonomy":"license","embeddable":true,"href":"https:\/\/pressbooks.bccampus.ca\/aperrott\/wp-json\/wp\/v2\/license?post=841"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}