{"id":2429,"date":"2018-04-11T23:52:51","date_gmt":"2018-04-12T03:52:51","guid":{"rendered":"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/chapter\/lewis-electron-dot-diagrams\/"},"modified":"2018-06-23T00:04:24","modified_gmt":"2018-06-23T04:04:24","slug":"lewis-electron-dot-diagrams","status":"publish","type":"chapter","link":"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/chapter\/lewis-electron-dot-diagrams\/","title":{"raw":"9.3 Lewis Electron Dot Diagrams","rendered":"9.3 Lewis Electron Dot Diagrams"},"content":{"raw":"<div class=\"section\" id=\"ball-ch09_s01\" lang=\"en\">\r\n<div class=\"learning_objectives editable block\" id=\"ball-ch09_s01_n01\">\r\n<div class=\"bcc-box bcc-highlight\">\r\n<h3>Learning Objective<\/h3>\r\nBy the end of this section, you will be able to:\r\n<ul>\r\n \t<li>Draw a Lewis electron dot diagram for an atom or a monatomic ion.<\/li>\r\n<\/ul>\r\n<\/div>\r\n<\/div>\r\n<p id=\"ball-ch09_s01_p01\" class=\"para editable block\">In almost all cases, chemical bonds are formed by interactions of valence electrons in atoms. To facilitate our understanding of how valence electrons interact, a simple way of representing those valence electrons would be useful.<\/p>\r\nA <a class=\"glossterm\">Lewis electron dot diagram<\/a>\u00a0(or electron dot diagram or a Lewis diagram or a Lewis structure) is a representation of the valence electrons of an atom that uses dots around the symbol of the element. The number of dots equals the number of valence electrons in the atom. These dots are arranged to the right and left and above and below the symbol, with no more than two dots on a side. (It does not matter what order the positions are used.) For example, the Lewis electron dot diagram for hydrogen is simply<a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Hydrogen.png\"><img src=\"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/Hydrogen-1.png\" alt=\"Hydrogen\" width=\"400\" height=\"49\" class=\"wp-image-4361 aligncenter\" \/><\/a>Because the side is not important, the Lewis electron dot diagram could also be drawn as follows:\r\n<div class=\"informalfigure large block\">\r\n<p id=\"ball-ch09_s01_p03\" class=\"para editable block\"><a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Hydrogen-Sides.png\"><img src=\"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/Hydrogen-Sides-1.png\" alt=\"Hydrogen-Sides\" width=\"400\" height=\"49\" class=\"wp-image-4362 aligncenter\" \/><\/a>The electron dot diagram for helium, with two valence electrons, is as follows:<\/p>\r\n\r\n<div class=\"informalfigure large block\">\r\n<p class=\"para editable block\"><a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Helium.png\"><img src=\"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/Helium-1.png\" alt=\"Helium\" width=\"400\" height=\"49\" class=\"wp-image-4360 aligncenter\" \/><\/a>By putting the two electrons together on the same side, we emphasize the fact that these two electrons are both in the 1<em class=\"emphasis\">s<\/em> subshell; this is the common convention we will adopt, although there will be exceptions later. The next atom, lithium, has an electron configuration of 1<em class=\"emphasis\">s<\/em><sup class=\"superscript\">2<\/sup>2<em class=\"emphasis\">s<\/em><sup class=\"superscript\">1<\/sup>, so it has only one electron in its valence shell. Its electron dot diagram resembles that of hydrogen, except the symbol for lithium is used:<\/p>\r\n\r\n<div class=\"informalfigure large block\">\r\n<p class=\"para editable block\"><a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Lithium.png\"><img src=\"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/Lithium-1.png\" alt=\"Lithium\" width=\"400\" height=\"49\" class=\"wp-image-4367 aligncenter\" \/><\/a>Beryllium has two valence electrons in its 2<em class=\"emphasis\">s<\/em> shell, so its electron dot diagram is like that of helium:<\/p>\r\n\r\n<div class=\"informalfigure large block\">\r\n<p class=\"para editable block\"><a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Beryllium.png\"><img src=\"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/Beryllium-1.png\" alt=\"Beryllium\" width=\"400\" height=\"49\" class=\"wp-image-4355 aligncenter\" \/><\/a>The next atom is boron. Its valence electron shell is 2<em class=\"emphasis\">s<\/em><sup class=\"superscript\">2<\/sup>2<em class=\"emphasis\">p<\/em><sup class=\"superscript\">1<\/sup>, so it has three valence electrons. The third electron will go on another side of the symbol:<\/p>\r\n\r\n<div class=\"informalfigure large block\">\r\n<p class=\"para editable block\"><a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Boron.png\"><img src=\"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/Boron-1.png\" alt=\"Boron\" width=\"400\" height=\"49\" class=\"wp-image-4356 aligncenter\" \/><\/a>Again, it does not matter on which sides of the symbol the electron dots are positioned.<\/p>\r\n\r\n<div class=\"informalfigure large block\">\r\n<p id=\"ball-ch09_s01_p09\" class=\"para editable block\">For carbon, there are four valence electrons, two in the 2<em class=\"emphasis\">s<\/em> subshell and two in the 2<em class=\"emphasis\">p<\/em> subshell. As usual, we will draw two dots together on one side, to represent the 2<em class=\"emphasis\">s<\/em> electrons. However, conventionally, we draw the dots for the two <em class=\"emphasis\">p<\/em> electrons on different sides. As such, the electron dot diagram for carbon is as follows:<a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Carbon.png\"><img src=\"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/Carbon-1.png\" alt=\"Carbon\" width=\"400\" height=\"49\" class=\"wp-image-4357 aligncenter\" \/><\/a>With nitrogen, which has three <em class=\"emphasis\">p<\/em> electrons, we put a single dot on each of the three remaining sides:<\/p>\r\n\r\n<div class=\"informalfigure large block\">\r\n<p class=\"para editable block\"><a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Nitrogen.png\"><img src=\"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/Nitrogen-1.png\" alt=\"Nitrogen\" width=\"400\" height=\"49\" class=\"wp-image-4368 aligncenter\" \/><\/a>For oxygen, which has four <em class=\"emphasis\">p<\/em> electrons, we now have to start doubling up on the dots on one other side of the symbol. When doubling up electrons, make sure that a side has no more than two electrons.<\/p>\r\n\r\n<div class=\"informalfigure large block\">\r\n<p class=\"para editable block\"><a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Oxygen.png\"><img src=\"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/Oxygen-1.png\" alt=\"Oxygen\" width=\"400\" height=\"49\" class=\"wp-image-4370 aligncenter\" \/><\/a>Fluorine and neon have seven and eight dots, respectively:<\/p>\r\n\r\n<div class=\"informalfigure large block\">\r\n<p class=\"para editable block\"><a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Fluoride-Neon.png\"><img src=\"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/Fluoride-Neon-1.png\" alt=\"Fluoride-Neon\" width=\"400\" height=\"49\" class=\"wp-image-4359 aligncenter\" \/><\/a>With the next element, sodium, the process starts over with a single electron because sodium has a single electron in its highest-numbered shell, the <em class=\"emphasis\">n<\/em> = 3 shell. By going through the periodic table, we see that the Lewis electron dot diagrams of atoms will never have more than eight dots around the atomic symbol.<\/p>\r\n\r\n<\/div>\r\n<div class=\"textbox shaded\">\r\n<h3 class=\"title\">Example 1<\/h3>\r\n<p id=\"ball-ch09_s01_p14\" class=\"para\">What is the Lewis electron dot diagram for each element? \u00a0 \u00a0 \u00a0a)\u00a0aluminum \u00a0 \u00a0 \u00a0 \u00a0 b)\u00a0selenium<\/p>\r\n&nbsp;\r\n<p class=\"simpara\"><strong>Solution<\/strong><\/p>\r\n<p class=\"simpara\">a) The valence electron configuration for aluminum is 3<em class=\"emphasis\">s<\/em><sup class=\"superscript\">2<\/sup>3<em class=\"emphasis\">p<\/em><sup class=\"superscript\">1<\/sup>. So it would have three dots around the symbol for aluminum, two of them paired to represent the 3<em class=\"emphasis\">s<\/em> electrons:<a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Aluminium.png\"><img src=\"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/Aluminium-1.png\" alt=\"Aluminium\" width=\"400\" height=\"49\" class=\"wp-image-4354 aligncenter\" \/><\/a>b) The valence electron configuration for selenium is 4<em class=\"emphasis\">s<\/em><sup class=\"superscript\">2<\/sup>4<em class=\"emphasis\">p<\/em><sup class=\"superscript\">4<\/sup>. In the highest-numbered shell, the <em class=\"emphasis\">n<\/em> = 4 shell, there are six electrons. Its electron dot diagram is as follows:<a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Selenium.png\"><img src=\"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/Selenium-1.png\" alt=\"Selenium\" width=\"400\" height=\"49\" class=\"wp-image-4374 aligncenter\" \/><\/a><\/p>\r\n\r\n<div class=\"informalfigure large\"><\/div>\r\n<p class=\"simpara\"><strong><em class=\"emphasis bolditalic\">Test Yourself<\/em><\/strong><\/p>\r\n<p id=\"ball-ch09_s01_p15\" class=\"para\">What is the Lewis electron dot diagram for each element? \u00a0a)\u00a0phosphorus \u00a0 \u00a0 \u00a0 \u00a0 \u00a0b)\u00a0argon<\/p>\r\n&nbsp;\r\n<p class=\"simpara\"><strong><em class=\"emphasis\">Answer<\/em><\/strong><a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Phosphorus-Argon.png\"><img src=\"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/Phosphorus-Argon-1.png\" alt=\"Phosphorus-Argon\" width=\"400\" height=\"49\" class=\"wp-image-4373 aligncenter\" \/><\/a><\/p>\r\n\r\n<\/div>\r\n<\/div>\r\n<\/div>\r\n<p id=\"ball-ch09_s01_p16\" class=\"para editable block\">For atoms with partially filled <em class=\"emphasis\">d<\/em> or <em class=\"emphasis\">f<\/em> subshells, these electrons are typically omitted from Lewis electron dot diagrams. For example, the electron dot diagram for iron (valence shell configuration 4<em class=\"emphasis\">s<\/em><sup class=\"superscript\">2<\/sup>3<em class=\"emphasis\">d<\/em><sup class=\"superscript\">6<\/sup>) is as follows:<a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Iron.png\"><img src=\"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/Iron-1.png\" alt=\"Iron\" width=\"400\" height=\"49\" class=\"wp-image-4363 aligncenter\" \/><\/a>Elements in the same column of the periodic table have similar Lewis electron dot diagrams because they have the same valence shell electron configuration. Thus the electron dot diagrams for the first column of elements are as follows:<\/p>\r\n\r\n<div class=\"informalfigure large block\">\r\n<p class=\"para editable block\"><a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/First-Column.png\"><img src=\"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/First-Column-1.png\" alt=\"First-Column\" width=\"400\" height=\"49\" class=\"wp-image-4358 aligncenter\" \/><\/a>Monatomic ions are atoms that have either lost (for cations) or gained (for anions) electrons. Electron dot diagrams for ions are the same as for atoms, except that some electrons have been removed for cations, while some electrons have been added for anions. Thus in comparing the electron configurations and electron dot diagrams for the Na atom and the Na<sup class=\"superscript\">+<\/sup> ion, we note that the Na atom has a single valence electron in its Lewis diagram, while the Na<sup class=\"superscript\">+<\/sup> ion has lost that one valence electron:<\/p>\r\n\r\n<div class=\"informalfigure large block\">\r\n<p class=\"para editable block\"><a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Lewis-Dot-Sodium.png\"><img src=\"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/Lewis-Dot-Sodium-1.png\" alt=\"Lewis-Dot-Sodium\" width=\"400\" height=\"80\" class=\"wp-image-4366 aligncenter\" \/><\/a>Technically, the valence shell of the Na<sup class=\"superscript\">+<\/sup> ion is now the <em class=\"emphasis\">n<\/em> = 2 shell, which has eight electrons in it. So why do we not put eight dots around Na<sup class=\"superscript\">+<\/sup>? Conventionally, when we show electron dot diagrams for ions, we show the original valence shell of the atom, which in this case is the <em class=\"emphasis\">n<\/em> = 3 shell and empty in the Na<sup class=\"superscript\">+<\/sup> ion.<\/p>\r\n\r\n<div class=\"informalfigure large block\">\r\n<p id=\"ball-ch09_s01_p20\" class=\"para editable block\">In making cations, electrons are first lost from the <em class=\"emphasis\">highest numbered shell<\/em>, not necessarily the last subshell filled. For example, in going from the neutral Fe atom to the Fe<sup class=\"superscript\">2+<\/sup> ion, the Fe atom loses its two 4<em class=\"emphasis\">s<\/em> electrons first, not its 3<em class=\"emphasis\">d<\/em> electrons, despite the fact that the 3<em class=\"emphasis\">d<\/em> subshell is the last subshell being filled. Thus we have<a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Lewis-Dot-Iron.png\"><img src=\"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/Lewis-Dot-Iron-1.png\" alt=\"Lewis-Dot-Iron\" width=\"400\" height=\"80\" class=\"wp-image-4365 aligncenter\" \/><\/a>Anions have extra electrons when compared to the original atom. Here is a comparison of the Cl atom with the Cl<sup class=\"superscript\">\u2212<\/sup> ion:<\/p>\r\n\r\n<div class=\"informalfigure large block\">\r\n<p class=\"para editable block\"><a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Lewis-Dot-Chlorine.png\"><img src=\"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/Lewis-Dot-Chlorine-1.png\" alt=\"Lewis-Dot-Chlorine\" width=\"400\" height=\"80\" class=\"wp-image-4364 aligncenter\" \/><\/a><\/p>\r\n\r\n<div class=\"textbox shaded\">\r\n<h3 class=\"title\">Example 2<\/h3>\r\n<p id=\"ball-ch09_s01_p22\" class=\"para\">What is the Lewis electron dot diagram for each ion? \u00a0 a)\u00a0Ca<sup class=\"superscript\">2+ \u00a0 \u00a0 \u00a0 \u00a0 <\/sup>b) O<sup class=\"superscript\">2\u2212<\/sup><\/p>\r\n&nbsp;\r\n<p class=\"simpara\"><strong>Solution<\/strong><\/p>\r\n<p class=\"simpara\">a) Having lost its two original valence electrons, the Lewis electron dot diagram is just Ca<sup class=\"superscript\">2+<\/sup>.<\/p>\r\n<span class=\"informalequation\"><span class=\"mathphrase\">Ca<sup class=\"superscript\">2+<\/sup><\/span><\/span>\r\n\r\nb) The O<sup class=\"superscript\">2\u2212<\/sup> ion has gained two electrons in its valence shell, so its Lewis electron dot diagram is as follows:<a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Oxygen-Ion.png\"><img src=\"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/Oxygen-Ion-1.png\" alt=\"Oxygen-Ion\" width=\"400\" height=\"49\" class=\"wp-image-4371 aligncenter\" \/><\/a>\r\n<div class=\"informalfigure large\"><\/div>\r\n<p class=\"simpara\"><strong><em class=\"emphasis bolditalic\">Test Yourself<\/em><\/strong><\/p>\r\n<p id=\"ball-ch09_s01_p23\" class=\"para\">The valence electron configuration of thallium, whose symbol is Tl, is 6<em class=\"emphasis\">s<\/em><sup class=\"superscript\">2<\/sup>5<em class=\"emphasis\">d<\/em><sup class=\"superscript\">10<\/sup>6<em class=\"emphasis\">p<\/em><sup class=\"superscript\">1<\/sup>. What is the Lewis electron dot diagram for the Tl<sup class=\"superscript\">+<\/sup> ion?<\/p>\r\n&nbsp;\r\n<p class=\"simpara\"><strong><em class=\"emphasis\">Answer<\/em><\/strong><a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Thallium-Ion.png\"><img src=\"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/Thallium-Ion-1.png\" alt=\"Thallium-Ion\" width=\"400\" height=\"49\" class=\"wp-image-4378 aligncenter\" \/><\/a><\/p>\r\n\r\n<\/div>\r\n<h2>Key Concepts and Summary<\/h2>\r\nLewis electron dot diagrams use dots to represent valence electrons around an atomic symbol. \u00a0\u00a0Lewis electron dot diagrams for ions have fewer (for cations) or more (for anions) dots than the corresponding atom.\r\n<div class=\"textbox exercises\">\r\n<h3 itemprop=\"educationalUse\">Exercises<\/h3>\r\n<div class=\"question\">\r\n\r\n1. Explain why the first two dots in a Lewis electron dot diagram are drawn on the same side of the atomic symbol.\r\n\r\n<span style=\"font-size: 1em\">2. What column of the periodic table has Lewis electron dot diagrams with two electrons?<\/span>\r\n\r\n<span style=\"font-size: 1em\">3. Draw the Lewis electron dot diagram for each element. \u00a0\u00a0<\/span><span style=\"font-size: 1em\">a) \u00a0strontium \u00a0 \u00a0 \u00a0<\/span><span style=\"font-size: 1em\">b) \u00a0silicon<\/span>\r\n\r\n<span style=\"font-size: 1em\">4. Draw the Lewis electron dot diagram for each element. \u00a0\u00a0<\/span><span style=\"font-size: 1em\">a) \u00a0titanium \u00a0 \u00a0 \u00a0 \u00a0<\/span><span style=\"font-size: 1em\">b) \u00a0phosphorus<\/span>\r\n\r\n<span style=\"font-size: 1em\">5. Draw the Lewis electron dot diagram for each ion. \u00a0<\/span><span style=\"font-size: 1em\">a) \u00a0Mg<\/span><sup class=\"superscript\">2+ \u00a0\u00a0<\/sup><span style=\"font-size: 1em\">b) \u00a0S<\/span><sup class=\"superscript\">2\u2212<\/sup>\r\n\r\n<span style=\"font-size: 1em\">6. Draw the Lewis electron dot diagram for each ion. \u00a0<\/span><span style=\"font-size: 1em\">a) \u00a0Fe<\/span><sup class=\"superscript\">2+ \u00a0 \u00a0\u00a0<\/sup><span style=\"font-size: 1em\">b) \u00a0N<\/span><sup class=\"superscript\">3\u2212<\/sup>\r\n\r\n<\/div>\r\n<div class=\"question\"><\/div>\r\n<b>Answers<\/b>\r\n\r\n1.\u00a0The first two electrons in a valence shell are <em class=\"emphasis\">s<\/em> electrons, which are paired.\r\n\r\n2. the second column of the periodic table\r\n\r\n3. a) \u00a0\u00a0<a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Strontium.png\"><img src=\"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/Strontium-1.png\" alt=\"Strontium\" width=\"400\" height=\"81\" class=\"alignnone wp-image-4376\" \/><\/a>\r\n\r\nb) \u00a0\u00a0<a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Silicone.png\"><img src=\"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/Silicone-1.png\" alt=\"Silicone\" width=\"400\" height=\"81\" class=\"alignnone wp-image-4375\" \/><\/a>\r\n\r\n4. a) \u00a0\u00a0<a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Titanium.png\"><img src=\"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/Titanium-1.png\" alt=\"Titanium\" width=\"400\" height=\"81\" class=\"alignnone wp-image-4379\" \/><\/a>\r\n\r\nb) \u00a0\u00a0<a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Phosphorus.png\"><img src=\"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/Phosphorus-1.png\" alt=\"Phosphorus\" width=\"400\" height=\"81\" class=\"alignnone wp-image-4372\" \/><\/a>\r\n\r\n5. a) \u00a0\u00a0Mg<sup class=\"superscript\">2+<\/sup>\r\n\r\nb) \u00a0\u00a0<a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Sulfur-Ion.png\"><img src=\"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/Sulfur-Ion-1.png\" alt=\"Sulfur-Ion\" width=\"400\" height=\"81\" class=\"alignnone wp-image-4377\" \/><\/a>\r\n\r\n6. a) \u00a0Fe<sup class=\"superscript\">2+<\/sup>\r\n\r\nb) \u00a0\u00a0<a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Nitrogen-Ion.png\"><img src=\"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/Nitrogen-Ion-1.png\" alt=\"Nitrogen-Ion\" width=\"400\" height=\"81\" class=\"alignnone wp-image-4369\" \/><\/a>\r\n\r\n<\/div>\r\n<\/div>\r\n<\/div>\r\n<\/div>\r\n<\/div>\r\n<\/div>\r\n<\/div>\r\n<\/div>\r\n<\/div>\r\n<\/div>\r\n<\/div>\r\n<\/div>","rendered":"<div class=\"section\" id=\"ball-ch09_s01\" lang=\"en\">\n<div class=\"learning_objectives editable block\" id=\"ball-ch09_s01_n01\">\n<div class=\"bcc-box bcc-highlight\">\n<h3>Learning Objective<\/h3>\n<p>By the end of this section, you will be able to:<\/p>\n<ul>\n<li>Draw a Lewis electron dot diagram for an atom or a monatomic ion.<\/li>\n<\/ul>\n<\/div>\n<\/div>\n<p id=\"ball-ch09_s01_p01\" class=\"para editable block\">In almost all cases, chemical bonds are formed by interactions of valence electrons in atoms. To facilitate our understanding of how valence electrons interact, a simple way of representing those valence electrons would be useful.<\/p>\n<p>A <a class=\"glossterm\">Lewis electron dot diagram<\/a>\u00a0(or electron dot diagram or a Lewis diagram or a Lewis structure) is a representation of the valence electrons of an atom that uses dots around the symbol of the element. The number of dots equals the number of valence electrons in the atom. These dots are arranged to the right and left and above and below the symbol, with no more than two dots on a side. (It does not matter what order the positions are used.) For example, the Lewis electron dot diagram for hydrogen is simply<a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Hydrogen.png\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/Hydrogen-1.png\" alt=\"Hydrogen\" width=\"400\" height=\"49\" class=\"wp-image-4361 aligncenter\" \/><\/a>Because the side is not important, the Lewis electron dot diagram could also be drawn as follows:<\/p>\n<div class=\"informalfigure large block\">\n<p id=\"ball-ch09_s01_p03\" class=\"para editable block\"><a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Hydrogen-Sides.png\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/Hydrogen-Sides-1.png\" alt=\"Hydrogen-Sides\" width=\"400\" height=\"49\" class=\"wp-image-4362 aligncenter\" \/><\/a>The electron dot diagram for helium, with two valence electrons, is as follows:<\/p>\n<div class=\"informalfigure large block\">\n<p class=\"para editable block\"><a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Helium.png\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/Helium-1.png\" alt=\"Helium\" width=\"400\" height=\"49\" class=\"wp-image-4360 aligncenter\" \/><\/a>By putting the two electrons together on the same side, we emphasize the fact that these two electrons are both in the 1<em class=\"emphasis\">s<\/em> subshell; this is the common convention we will adopt, although there will be exceptions later. The next atom, lithium, has an electron configuration of 1<em class=\"emphasis\">s<\/em><sup class=\"superscript\">2<\/sup>2<em class=\"emphasis\">s<\/em><sup class=\"superscript\">1<\/sup>, so it has only one electron in its valence shell. Its electron dot diagram resembles that of hydrogen, except the symbol for lithium is used:<\/p>\n<div class=\"informalfigure large block\">\n<p class=\"para editable block\"><a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Lithium.png\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/Lithium-1.png\" alt=\"Lithium\" width=\"400\" height=\"49\" class=\"wp-image-4367 aligncenter\" \/><\/a>Beryllium has two valence electrons in its 2<em class=\"emphasis\">s<\/em> shell, so its electron dot diagram is like that of helium:<\/p>\n<div class=\"informalfigure large block\">\n<p class=\"para editable block\"><a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Beryllium.png\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/Beryllium-1.png\" alt=\"Beryllium\" width=\"400\" height=\"49\" class=\"wp-image-4355 aligncenter\" \/><\/a>The next atom is boron. Its valence electron shell is 2<em class=\"emphasis\">s<\/em><sup class=\"superscript\">2<\/sup>2<em class=\"emphasis\">p<\/em><sup class=\"superscript\">1<\/sup>, so it has three valence electrons. The third electron will go on another side of the symbol:<\/p>\n<div class=\"informalfigure large block\">\n<p class=\"para editable block\"><a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Boron.png\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/Boron-1.png\" alt=\"Boron\" width=\"400\" height=\"49\" class=\"wp-image-4356 aligncenter\" \/><\/a>Again, it does not matter on which sides of the symbol the electron dots are positioned.<\/p>\n<div class=\"informalfigure large block\">\n<p id=\"ball-ch09_s01_p09\" class=\"para editable block\">For carbon, there are four valence electrons, two in the 2<em class=\"emphasis\">s<\/em> subshell and two in the 2<em class=\"emphasis\">p<\/em> subshell. As usual, we will draw two dots together on one side, to represent the 2<em class=\"emphasis\">s<\/em> electrons. However, conventionally, we draw the dots for the two <em class=\"emphasis\">p<\/em> electrons on different sides. As such, the electron dot diagram for carbon is as follows:<a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Carbon.png\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/Carbon-1.png\" alt=\"Carbon\" width=\"400\" height=\"49\" class=\"wp-image-4357 aligncenter\" \/><\/a>With nitrogen, which has three <em class=\"emphasis\">p<\/em> electrons, we put a single dot on each of the three remaining sides:<\/p>\n<div class=\"informalfigure large block\">\n<p class=\"para editable block\"><a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Nitrogen.png\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/Nitrogen-1.png\" alt=\"Nitrogen\" width=\"400\" height=\"49\" class=\"wp-image-4368 aligncenter\" \/><\/a>For oxygen, which has four <em class=\"emphasis\">p<\/em> electrons, we now have to start doubling up on the dots on one other side of the symbol. When doubling up electrons, make sure that a side has no more than two electrons.<\/p>\n<div class=\"informalfigure large block\">\n<p class=\"para editable block\"><a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Oxygen.png\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/Oxygen-1.png\" alt=\"Oxygen\" width=\"400\" height=\"49\" class=\"wp-image-4370 aligncenter\" \/><\/a>Fluorine and neon have seven and eight dots, respectively:<\/p>\n<div class=\"informalfigure large block\">\n<p class=\"para editable block\"><a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Fluoride-Neon.png\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/Fluoride-Neon-1.png\" alt=\"Fluoride-Neon\" width=\"400\" height=\"49\" class=\"wp-image-4359 aligncenter\" \/><\/a>With the next element, sodium, the process starts over with a single electron because sodium has a single electron in its highest-numbered shell, the <em class=\"emphasis\">n<\/em> = 3 shell. By going through the periodic table, we see that the Lewis electron dot diagrams of atoms will never have more than eight dots around the atomic symbol.<\/p>\n<\/div>\n<div class=\"textbox shaded\">\n<h3 class=\"title\">Example 1<\/h3>\n<p id=\"ball-ch09_s01_p14\" class=\"para\">What is the Lewis electron dot diagram for each element? \u00a0 \u00a0 \u00a0a)\u00a0aluminum \u00a0 \u00a0 \u00a0 \u00a0 b)\u00a0selenium<\/p>\n<p>&nbsp;<\/p>\n<p class=\"simpara\"><strong>Solution<\/strong><\/p>\n<p class=\"simpara\">a) The valence electron configuration for aluminum is 3<em class=\"emphasis\">s<\/em><sup class=\"superscript\">2<\/sup>3<em class=\"emphasis\">p<\/em><sup class=\"superscript\">1<\/sup>. So it would have three dots around the symbol for aluminum, two of them paired to represent the 3<em class=\"emphasis\">s<\/em> electrons:<a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Aluminium.png\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/Aluminium-1.png\" alt=\"Aluminium\" width=\"400\" height=\"49\" class=\"wp-image-4354 aligncenter\" \/><\/a>b) The valence electron configuration for selenium is 4<em class=\"emphasis\">s<\/em><sup class=\"superscript\">2<\/sup>4<em class=\"emphasis\">p<\/em><sup class=\"superscript\">4<\/sup>. In the highest-numbered shell, the <em class=\"emphasis\">n<\/em> = 4 shell, there are six electrons. Its electron dot diagram is as follows:<a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Selenium.png\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/Selenium-1.png\" alt=\"Selenium\" width=\"400\" height=\"49\" class=\"wp-image-4374 aligncenter\" \/><\/a><\/p>\n<div class=\"informalfigure large\"><\/div>\n<p class=\"simpara\"><strong><em class=\"emphasis bolditalic\">Test Yourself<\/em><\/strong><\/p>\n<p id=\"ball-ch09_s01_p15\" class=\"para\">What is the Lewis electron dot diagram for each element? \u00a0a)\u00a0phosphorus \u00a0 \u00a0 \u00a0 \u00a0 \u00a0b)\u00a0argon<\/p>\n<p>&nbsp;<\/p>\n<p class=\"simpara\"><strong><em class=\"emphasis\">Answer<\/em><\/strong><a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Phosphorus-Argon.png\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/Phosphorus-Argon-1.png\" alt=\"Phosphorus-Argon\" width=\"400\" height=\"49\" class=\"wp-image-4373 aligncenter\" \/><\/a><\/p>\n<\/div>\n<\/div>\n<\/div>\n<p id=\"ball-ch09_s01_p16\" class=\"para editable block\">For atoms with partially filled <em class=\"emphasis\">d<\/em> or <em class=\"emphasis\">f<\/em> subshells, these electrons are typically omitted from Lewis electron dot diagrams. For example, the electron dot diagram for iron (valence shell configuration 4<em class=\"emphasis\">s<\/em><sup class=\"superscript\">2<\/sup>3<em class=\"emphasis\">d<\/em><sup class=\"superscript\">6<\/sup>) is as follows:<a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Iron.png\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/Iron-1.png\" alt=\"Iron\" width=\"400\" height=\"49\" class=\"wp-image-4363 aligncenter\" \/><\/a>Elements in the same column of the periodic table have similar Lewis electron dot diagrams because they have the same valence shell electron configuration. Thus the electron dot diagrams for the first column of elements are as follows:<\/p>\n<div class=\"informalfigure large block\">\n<p class=\"para editable block\"><a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/First-Column.png\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/First-Column-1.png\" alt=\"First-Column\" width=\"400\" height=\"49\" class=\"wp-image-4358 aligncenter\" \/><\/a>Monatomic ions are atoms that have either lost (for cations) or gained (for anions) electrons. Electron dot diagrams for ions are the same as for atoms, except that some electrons have been removed for cations, while some electrons have been added for anions. Thus in comparing the electron configurations and electron dot diagrams for the Na atom and the Na<sup class=\"superscript\">+<\/sup> ion, we note that the Na atom has a single valence electron in its Lewis diagram, while the Na<sup class=\"superscript\">+<\/sup> ion has lost that one valence electron:<\/p>\n<div class=\"informalfigure large block\">\n<p class=\"para editable block\"><a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Lewis-Dot-Sodium.png\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/Lewis-Dot-Sodium-1.png\" alt=\"Lewis-Dot-Sodium\" width=\"400\" height=\"80\" class=\"wp-image-4366 aligncenter\" \/><\/a>Technically, the valence shell of the Na<sup class=\"superscript\">+<\/sup> ion is now the <em class=\"emphasis\">n<\/em> = 2 shell, which has eight electrons in it. So why do we not put eight dots around Na<sup class=\"superscript\">+<\/sup>? Conventionally, when we show electron dot diagrams for ions, we show the original valence shell of the atom, which in this case is the <em class=\"emphasis\">n<\/em> = 3 shell and empty in the Na<sup class=\"superscript\">+<\/sup> ion.<\/p>\n<div class=\"informalfigure large block\">\n<p id=\"ball-ch09_s01_p20\" class=\"para editable block\">In making cations, electrons are first lost from the <em class=\"emphasis\">highest numbered shell<\/em>, not necessarily the last subshell filled. For example, in going from the neutral Fe atom to the Fe<sup class=\"superscript\">2+<\/sup> ion, the Fe atom loses its two 4<em class=\"emphasis\">s<\/em> electrons first, not its 3<em class=\"emphasis\">d<\/em> electrons, despite the fact that the 3<em class=\"emphasis\">d<\/em> subshell is the last subshell being filled. Thus we have<a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Lewis-Dot-Iron.png\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/Lewis-Dot-Iron-1.png\" alt=\"Lewis-Dot-Iron\" width=\"400\" height=\"80\" class=\"wp-image-4365 aligncenter\" \/><\/a>Anions have extra electrons when compared to the original atom. Here is a comparison of the Cl atom with the Cl<sup class=\"superscript\">\u2212<\/sup> ion:<\/p>\n<div class=\"informalfigure large block\">\n<p class=\"para editable block\"><a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Lewis-Dot-Chlorine.png\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/Lewis-Dot-Chlorine-1.png\" alt=\"Lewis-Dot-Chlorine\" width=\"400\" height=\"80\" class=\"wp-image-4364 aligncenter\" \/><\/a><\/p>\n<div class=\"textbox shaded\">\n<h3 class=\"title\">Example 2<\/h3>\n<p id=\"ball-ch09_s01_p22\" class=\"para\">What is the Lewis electron dot diagram for each ion? \u00a0 a)\u00a0Ca<sup class=\"superscript\">2+ \u00a0 \u00a0 \u00a0 \u00a0 <\/sup>b) O<sup class=\"superscript\">2\u2212<\/sup><\/p>\n<p>&nbsp;<\/p>\n<p class=\"simpara\"><strong>Solution<\/strong><\/p>\n<p class=\"simpara\">a) Having lost its two original valence electrons, the Lewis electron dot diagram is just Ca<sup class=\"superscript\">2+<\/sup>.<\/p>\n<p><span class=\"informalequation\"><span class=\"mathphrase\">Ca<sup class=\"superscript\">2+<\/sup><\/span><\/span><\/p>\n<p>b) The O<sup class=\"superscript\">2\u2212<\/sup> ion has gained two electrons in its valence shell, so its Lewis electron dot diagram is as follows:<a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Oxygen-Ion.png\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/Oxygen-Ion-1.png\" alt=\"Oxygen-Ion\" width=\"400\" height=\"49\" class=\"wp-image-4371 aligncenter\" \/><\/a><\/p>\n<div class=\"informalfigure large\"><\/div>\n<p class=\"simpara\"><strong><em class=\"emphasis bolditalic\">Test Yourself<\/em><\/strong><\/p>\n<p id=\"ball-ch09_s01_p23\" class=\"para\">The valence electron configuration of thallium, whose symbol is Tl, is 6<em class=\"emphasis\">s<\/em><sup class=\"superscript\">2<\/sup>5<em class=\"emphasis\">d<\/em><sup class=\"superscript\">10<\/sup>6<em class=\"emphasis\">p<\/em><sup class=\"superscript\">1<\/sup>. What is the Lewis electron dot diagram for the Tl<sup class=\"superscript\">+<\/sup> ion?<\/p>\n<p>&nbsp;<\/p>\n<p class=\"simpara\"><strong><em class=\"emphasis\">Answer<\/em><\/strong><a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Thallium-Ion.png\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/Thallium-Ion-1.png\" alt=\"Thallium-Ion\" width=\"400\" height=\"49\" class=\"wp-image-4378 aligncenter\" \/><\/a><\/p>\n<\/div>\n<h2>Key Concepts and Summary<\/h2>\n<p>Lewis electron dot diagrams use dots to represent valence electrons around an atomic symbol. \u00a0\u00a0Lewis electron dot diagrams for ions have fewer (for cations) or more (for anions) dots than the corresponding atom.<\/p>\n<div class=\"textbox exercises\">\n<h3 itemprop=\"educationalUse\">Exercises<\/h3>\n<div class=\"question\">\n<p>1. Explain why the first two dots in a Lewis electron dot diagram are drawn on the same side of the atomic symbol.<\/p>\n<p><span style=\"font-size: 1em\">2. What column of the periodic table has Lewis electron dot diagrams with two electrons?<\/span><\/p>\n<p><span style=\"font-size: 1em\">3. Draw the Lewis electron dot diagram for each element. \u00a0\u00a0<\/span><span style=\"font-size: 1em\">a) \u00a0strontium \u00a0 \u00a0 \u00a0<\/span><span style=\"font-size: 1em\">b) \u00a0silicon<\/span><\/p>\n<p><span style=\"font-size: 1em\">4. Draw the Lewis electron dot diagram for each element. \u00a0\u00a0<\/span><span style=\"font-size: 1em\">a) \u00a0titanium \u00a0 \u00a0 \u00a0 \u00a0<\/span><span style=\"font-size: 1em\">b) \u00a0phosphorus<\/span><\/p>\n<p><span style=\"font-size: 1em\">5. Draw the Lewis electron dot diagram for each ion. \u00a0<\/span><span style=\"font-size: 1em\">a) \u00a0Mg<\/span><sup class=\"superscript\">2+ \u00a0\u00a0<\/sup><span style=\"font-size: 1em\">b) \u00a0S<\/span><sup class=\"superscript\">2\u2212<\/sup><\/p>\n<p><span style=\"font-size: 1em\">6. Draw the Lewis electron dot diagram for each ion. \u00a0<\/span><span style=\"font-size: 1em\">a) \u00a0Fe<\/span><sup class=\"superscript\">2+ \u00a0 \u00a0\u00a0<\/sup><span style=\"font-size: 1em\">b) \u00a0N<\/span><sup class=\"superscript\">3\u2212<\/sup><\/p>\n<\/div>\n<div class=\"question\"><\/div>\n<p><b>Answers<\/b><\/p>\n<p>1.\u00a0The first two electrons in a valence shell are <em class=\"emphasis\">s<\/em> electrons, which are paired.<\/p>\n<p>2. the second column of the periodic table<\/p>\n<p>3. a) \u00a0\u00a0<a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Strontium.png\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/Strontium-1.png\" alt=\"Strontium\" width=\"400\" height=\"81\" class=\"alignnone wp-image-4376\" \/><\/a><\/p>\n<p>b) \u00a0\u00a0<a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Silicone.png\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/Silicone-1.png\" alt=\"Silicone\" width=\"400\" height=\"81\" class=\"alignnone wp-image-4375\" \/><\/a><\/p>\n<p>4. a) \u00a0\u00a0<a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Titanium.png\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/Titanium-1.png\" alt=\"Titanium\" width=\"400\" height=\"81\" class=\"alignnone wp-image-4379\" \/><\/a><\/p>\n<p>b) \u00a0\u00a0<a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Phosphorus.png\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/Phosphorus-1.png\" alt=\"Phosphorus\" width=\"400\" height=\"81\" class=\"alignnone wp-image-4372\" \/><\/a><\/p>\n<p>5. a) \u00a0\u00a0Mg<sup class=\"superscript\">2+<\/sup><\/p>\n<p>b) \u00a0\u00a0<a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Sulfur-Ion.png\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/Sulfur-Ion-1.png\" alt=\"Sulfur-Ion\" width=\"400\" height=\"81\" class=\"alignnone wp-image-4377\" \/><\/a><\/p>\n<p>6. a) \u00a0Fe<sup class=\"superscript\">2+<\/sup><\/p>\n<p>b) \u00a0\u00a0<a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Nitrogen-Ion.png\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-content\/uploads\/sites\/387\/2018\/04\/Nitrogen-Ion-1.png\" alt=\"Nitrogen-Ion\" width=\"400\" height=\"81\" class=\"alignnone wp-image-4369\" \/><\/a><\/p>\n<\/div>\n<\/div>\n<\/div>\n<\/div>\n<\/div>\n<\/div>\n<\/div>\n<\/div>\n<\/div>\n<\/div>\n<\/div>\n<\/div>\n","protected":false},"author":330,"menu_order":4,"template":"","meta":{"pb_show_title":"on","pb_short_title":"9.3 Lewis Electron Dot 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