{"id":381,"date":"2017-12-14T21:34:43","date_gmt":"2017-12-14T21:34:43","guid":{"rendered":"https:\/\/courses.lumenlearning.com\/suny-mcc-introductorychemistry\/chapter\/lewis-electron-dot-diagrams\/"},"modified":"2023-04-26T16:01:10","modified_gmt":"2023-04-26T16:01:10","slug":"lewis-electron-dot-diagrams","status":"publish","type":"chapter","link":"https:\/\/courses.lumenlearning.com\/suny-mcc-introductorychemistry\/chapter\/lewis-electron-dot-diagrams\/","title":{"raw":"6.1 Lewis Electron Dot Symbols","rendered":"6.1 Lewis Electron Dot Symbols"},"content":{"raw":"<div>\r\n<div id=\"ball-ch09_s01\" class=\"section\" lang=\"en\">\r\n<div class=\"textbox learning-objectives\">\r\n<h3>Learning Objectives<\/h3>\r\nBy the end of this section, you will be able to:\r\n<ul>\r\n \t<li>Write Lewis symbols for neutral atoms and ions<\/li>\r\n<\/ul>\r\n<\/div>\r\n<h2>Lewis Symbols of Monoatomic Elements<\/h2>\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 symbol<\/a> (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.)\r\n\r\nFor example, the Lewis electron dot symbol for calcium is simply\r\n\r\n<img class=\"aligncenter\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/887\/2015\/04\/23211351\/CNX_Chem_07_03_Lewisstruct1_img1.jpg\" alt=\"A Lewis structure of calcium is shown. A lone pair of electrons are shown to the right of the symbol.\" width=\"325\" height=\"34\" \/>\r\n\r\nFigure 1 shows the Lewis symbols for the elements of the third period of the periodic table.\r\n\r\n[caption id=\"\" align=\"aligncenter\" width=\"881\"]<img src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/887\/2015\/04\/23211352\/CNX_Chem_07_03_3rowLewis1.jpg\" alt=\"A table is shown that has three columns and nine rows. The header row reads \u201cAtoms,\u201d \u201cElectronic Configuration,\u201d and \u201cLewis Symbol.\u201d The first column contains the words \u201csodium,\u201d \u201cmagnesium,\u201d \u201caluminum,\u201d \u201csilicon,\u201d \u201cphosphorus,\u201d \u201csulfur,\u201d \u201cchlorine,\u201d and \u201cargon.\u201d The second column contains the symbols and numbers \u201c[ N e ] 3 s superscript 2,\u201d \u201c[ N e ] 3 s superscript 2, 3 p superscript 1,\u201d \u201c[ N e ] 3 s superscript 2, 3 p superscript 2,\u201d \u201c[ N e ] 3 s superscript 2, 3 p superscript 3,\u201d \u201c[ N e ] 3 s superscript 2, 3 p superscript 4,\u201d \u201c[ N e ] 3 s superscript 2, 3 p superscript 5,\u201d and \u201c[ N e ] 3 s superscript 2, 3 p superscript 6.\u201d The third column contains Lewis structures for N a with one dot, M g with two dots, A l with three dots, Si with four dots, P with five dots, S with six dots, C l with seven dots, and A r with eight dots.\" width=\"881\" height=\"416\" \/> Figure 1. Lewis symbols illustrating the number of valence electrons for each element in the third period of the periodic table.[\/caption]<\/div>\r\n<div lang=\"en\"><\/div>\r\n<div class=\"section\" lang=\"en\">\r\n\r\nLewis symbols can also be used to illustrate the formation of cations from atoms, as shown here for sodium and calcium:<img class=\"aligncenter\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/887\/2015\/04\/23211353\/CNX_Chem_07_03_NaCa_img1.jpg\" alt=\"Two diagrams are shown. The left diagram shows a Lewis dot structure of sodium with one dot, then a right-facing arrow leading to a sodium symbol with a superscripted plus sign, a plus sign, and the letter \u201ce\u201d with a superscripted negative sign. The terms below this diagram read \u201cSodium atom\u201d and \u201cSodium cation.\u201d The right diagram shows a Lewis dot structure of calcium with two dots, then a right-facing arrow leading to a calcium symbol with a superscripted two and a plus sign, a plus sign, and the value \u201c2e\u201d with a superscripted negative sign. The terms below this diagram read \u201cCalcium atom\u201d and \u201cCalcium cation.\u201d\" width=\"885\" height=\"81\" \/>Likewise, they can be used to show the formation of anions from atoms, as shown below for chlorine and sulfur:<img class=\"aligncenter\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/887\/2015\/04\/23211355\/CNX_Chem_07_03_ClS_img1.jpg\" alt=\"Two diagrams are shown. The left diagram shows a Lewis dot structure of chlorine with seven dots and the letter \u201ce\u201d with a superscripted negative sign, then a right-facing arrow leading to a chlorine symbol with eight dots and a superscripted negative sign. The terms below this diagram read, \u201cChlorine atom,\u201d and, \u201cChlorine anion.\u201d The right diagram shows a Lewis dot structure of sulfur with six dots and the symbol \u201c2e\u201d with a superscripted negative sign, then a right-facing arrow leading to a sulfur symbol with eight dots and a superscripted two and negative sign. The terms below this diagram read, \u201cSulfur atom,\u201d and, \u201cSulfur anion.\u201d\" width=\"883\" height=\"89\" \/>Figure 2 demonstrates the use of Lewis symbols to show the transfer of electrons during the formation of ionic compounds.\r\n\r\n[caption id=\"\" align=\"aligncenter\" width=\"884\"]<img src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/887\/2015\/04\/23211357\/CNX_Chem_07_03_IonLewis1.jpg\" alt=\"A table is shown with four rows. The header row reads \u201cMetal,\u201d \u201cNonmetal,\u201d and \u201cIonic Compound.\u201d The second row shows the Lewis structures of a reaction. A sodium symbol with one dot, a plus sign, and a chlorine symbol with seven dots lie to the left of a right-facing arrow. To the right of the arrow a sodium symbol with a superscripted plus sign is drawn next to a chlorine symbol with eight dots surrounded by brackets with a superscripted negative sign. One of the dots on the C l atom is red. The terms \u201csodium atom,\u201d \u201cchlorine atom,\u201d and \u201csodium chloride ( sodium ion and chloride ion )\u201d are written under the reaction. The third row shows the Lewis structures of a reaction. A magnesium symbol with two red dots, a plus sign, and an oxygen symbol with six dots lie to the left of a right-facing arrow. To the right of the arrow a magnesium symbol with a superscripted two and a plus sign is drawn next to an oxygen symbol with eight dots, two of which are red, surrounded by brackets with a superscripted two a and a negative sign. The terms \u201cmagnesium atom,\u201d \u201coxygen atom,\u201d and \u201cmagnesium oxide ( magnesium ion and oxide ion )\u201d are written under the reaction. The fourth row shows the Lewis structures of a reaction. A calcium symbol with two red dots, a plus sign, and a fluorine symbol with a coefficient of two and seven dots lie to the left of a right-facing arrow. To the right of the arrow a calcium symbol with a superscripted two and a plus sign is drawn next to a fluorine symbol with eight dots, one of which is red, surrounded by brackets with a superscripted negative sign and a subscripted two. The terms \u201ccalcium atom,\u201d \u201cfluorine atoms,\u201d and \u201ccalcium fluoride ( calcium ion and two fluoride ions )\u201d are written under the reaction.\" width=\"884\" height=\"457\" \/> Figure 2. Cations are formed when atoms lose electrons, represented by fewer Lewis dots, whereas anions are formed by atoms gaining electrons. The total number of electrons does not change.[\/caption]\r\n\r\n<div class=\"informalfigure large block\">\r\n<div class=\"informalfigure large block\">\r\n<div class=\"informalfigure large block\">\r\n<div class=\"informalfigure large block\">\r\n<div class=\"informalfigure large block\">\r\n<div class=\"informalfigure large block\">\r\n<div class=\"informalfigure large block\">\r\n<div class=\"informalfigure large block\">\r\n<div class=\"informalfigure large block\">\r\n<div class=\"informalfigure large block\">\r\n<div class=\"textbox examples\">\r\n<h3>Example 1: <strong>Writing Lewis DoT SYmbols of Elements\r\n<\/strong><\/h3>\r\n<p id=\"ball-ch09_s01_p14\" class=\"para\">What is the Lewis electron dot symbol for each element?<\/p>\r\n\r\n<ol id=\"ball-ch09_s01_l02\" class=\"orderedlist\">\r\n \t<li>aluminum<\/li>\r\n \t<li>selenium<\/li>\r\n<\/ol>\r\n[reveal-answer q=\"3675621\"]Show Answer[\/reveal-answer]\r\n[hidden-answer a=\"3675621\"]\r\n<ol id=\"ball-ch09_s01_l03\" class=\"orderedlist\">\r\n \t<li>\r\n<p class=\"para\">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 (or three single dots around the atom):<\/p>\r\n<a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Aluminium.png\"><img class=\"alignnone wp-image-4354\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/2835\/2017\/12\/14213413\/Aluminium-1.png\" alt=\"Aluminium\" width=\"400\" height=\"49\" \/><\/a><\/li>\r\n \t<li>\r\n<p class=\"para\">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:<\/p>\r\n<a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Selenium.png\"><img class=\"alignnone wp-image-4374\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/2835\/2017\/12\/14213415\/Selenium-1.png\" alt=\"Selenium\" width=\"400\" height=\"49\" \/><\/a><\/li>\r\n<\/ol>\r\n[\/hidden-answer]\r\n<h4><strong>Check Your Learning<\/strong><\/h4>\r\n<p id=\"ball-ch09_s01_p15\" class=\"para\">What is the Lewis electron dot symbol for each element?<\/p>\r\n\r\n<ol id=\"ball-ch09_s01_l04\" class=\"orderedlist\">\r\n \t<li>phosphorus<\/li>\r\n \t<li>argon<\/li>\r\n<\/ol>\r\n[reveal-answer q=\"6525751\"]Show Answer[\/reveal-answer]\r\n[hidden-answer a=\"6525751\"] <a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Phosphorus-Argon.png\"><img class=\"alignnone wp-image-4373\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/2835\/2017\/12\/14213417\/Phosphorus-Argon-1.png\" alt=\"Phosphorus-Argon\" width=\"400\" height=\"49\" \/><\/a> [\/hidden-answer]\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 class=\"informalfigure large block\">\r\n<div class=\"textbox examples\">\r\n<h3>Example 2: <strong>Writing Lewis DoT SYmbols of Ions\r\n<\/strong><\/h3>\r\n<p id=\"ball-ch09_s01_p22\" class=\"para\">What is the Lewis electron dot symbol for each ion?<\/p>\r\n\r\n<ol id=\"ball-ch09_s01_l05\" class=\"orderedlist\">\r\n \t<li>Ca<sup class=\"superscript\">2+<\/sup><\/li>\r\n \t<li>O<sup class=\"superscript\">2\u2212<\/sup><\/li>\r\n<\/ol>\r\n[reveal-answer q=\"36756212\"]Show Answer[\/reveal-answer]\r\n[hidden-answer a=\"36756212\"]\r\n<ol id=\"ball-ch09_s01_l06\" class=\"orderedlist\">\r\n \t<li>\r\n<p class=\"para\">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><\/li>\r\n \t<li>\r\n<p class=\"para\">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:<\/p>\r\n<a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Oxygen-Ion.png\"><img class=\"alignnone wp-image-4371\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/2835\/2017\/12\/14213428\/Oxygen-Ion-1.png\" alt=\"Oxygen-Ion\" width=\"400\" height=\"49\" \/><\/a><\/li>\r\n<\/ol>\r\n[\/hidden-answer]\r\n<h4><strong>Check Your Learning<\/strong><\/h4>\r\nThe 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?\r\n[reveal-answer q=\"65257512\"]Show Answer[\/reveal-answer]\r\n[hidden-answer a=\"65257512\"]\u00a0<a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Thallium-Ion.png\"><img class=\"alignnone wp-image-4378\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/2835\/2017\/12\/14213430\/Thallium-Ion-1.png\" alt=\"Thallium-Ion\" width=\"400\" height=\"49\" \/><\/a> [\/hidden-answer]\r\n\r\n<\/div>\r\n<\/div>\r\n<div id=\"ball-ch09_s01_n04\" class=\"key_takeaways editable block\">\r\n<div class=\"bcc-box bcc-success\">\r\n<h3>Key Takeaways<\/h3>\r\n<ul id=\"ball-ch09_s01_l07\" class=\"itemizedlist\">\r\n \t<li>Lewis electron dot diagrams use dots to represent valence electrons around an atomic symbol.<\/li>\r\n \t<li>Lewis electron dot diagrams for ions have fewer (for cations) or more (for anions) dots than the corresponding atom.<\/li>\r\n<\/ul>\r\n<\/div>\r\n<\/div>\r\n<div id=\"ball-ch09_s01_qs01\" class=\"qandaset block\">\r\n<div class=\"bcc-box bcc-info\">\r\n<h3>Exercises<\/h3>\r\n<div class=\"question\">\r\n<p id=\"ball-ch09_s01_qs01_p01\" class=\"para\">1.\u00a0 Explain why the first two dots in a Lewis electron dot symbol are drawn on the same side of the atomic symbol.<\/p>\r\n\r\n<\/div>\r\n<div class=\"question\">\r\n<p id=\"ball-ch09_s01_qs01_p03\" class=\"para\">2.\u00a0 Is it necessary for the first dot around an atomic symbol to go on a particular side of the atomic symbol?<\/p>\r\n\r\n<\/div>\r\n<div class=\"question\">\r\n<p id=\"ball-ch09_s01_qs01_p05\" class=\"para\">3.\u00a0 What column of the periodic table has Lewis electron dot symbol with two electrons?<\/p>\r\n\r\n<\/div>\r\n<div class=\"question\">\r\n<p id=\"ball-ch09_s01_qs01_p07\" class=\"para\">4.\u00a0 What column of the periodic table has Lewis electron dot symbol that have six electrons in them?<\/p>\r\n\r\n<\/div>\r\n<div class=\"question\">\r\n<p id=\"ball-ch09_s01_qs01_p09\" class=\"para\">5.\u00a0 Draw the Lewis electron dot symbol for each element.<\/p>\r\n\r\n<\/div>\r\n<p style=\"padding-left: 30px;\">a) \u00a0strontium<\/p>\r\n<p style=\"padding-left: 30px;\">b) \u00a0silicon<\/p>\r\n\r\n<div class=\"question\">\r\n<p id=\"ball-ch09_s01_qs01_p10\" class=\"para\">6. \u00a0Draw the Lewis electron dot symbol for each element.<\/p>\r\n<p style=\"padding-left: 30px;\">a) \u00a0krypton<\/p>\r\n<p style=\"padding-left: 30px;\">b) \u00a0sulfur<\/p>\r\n\r\n<\/div>\r\n<div class=\"question\">\r\n<p id=\"ball-ch09_s01_qs01_p11\" class=\"para\">7. \u00a0Draw the Lewis electron dot symbol for each element.<\/p>\r\n<p style=\"padding-left: 30px;\">a) \u00a0titanium<\/p>\r\n<p style=\"padding-left: 30px;\">b) \u00a0phosphorus<\/p>\r\n\r\n<\/div>\r\n<div class=\"question\">\r\n<p id=\"ball-ch09_s01_qs01_p12\" class=\"para\">8. \u00a0Draw the Lewis electron dot symbol for each element.<\/p>\r\n<p style=\"padding-left: 30px;\">a) \u00a0bromine<\/p>\r\n<p style=\"padding-left: 30px;\">b) \u00a0gallium<\/p>\r\n\r\n<\/div>\r\n<div class=\"question\">\r\n<p id=\"ball-ch09_s01_qs01_p13\" class=\"para\">9. \u00a0Draw the Lewis electron dot symbol for each ion.<\/p>\r\n<p style=\"padding-left: 30px;\">a) \u00a0Mg<sup class=\"superscript\">2+<\/sup><\/p>\r\n<p style=\"padding-left: 30px;\">b) \u00a0S<sup class=\"superscript\">2\u2212<\/sup><\/p>\r\n\r\n<\/div>\r\n<div class=\"question\">\r\n<p id=\"ball-ch09_s01_qs01_p14\" class=\"para\">10. \u00a0Draw the Lewis electron dot symbol for each ion.<\/p>\r\n<p style=\"padding-left: 30px;\">a) \u00a0In<sup class=\"superscript\">+<\/sup><\/p>\r\n<p style=\"padding-left: 30px;\">b) \u00a0Br<sup class=\"superscript\">\u2212<\/sup><\/p>\r\n\r\n<\/div>\r\n<div class=\"question\">\r\n<p id=\"ball-ch09_s01_qs01_p15\" class=\"para\">11. \u00a0Draw the Lewis electron dot symbol for each ion.<\/p>\r\n<p style=\"padding-left: 30px;\">a) \u00a0Fe<sup class=\"superscript\">2+<\/sup><\/p>\r\n<p style=\"padding-left: 30px;\">b) \u00a0N<sup class=\"superscript\">3\u2212<\/sup><\/p>\r\n\r\n<\/div>\r\n<div class=\"question\">\r\n<p id=\"ball-ch09_s01_qs01_p16\" class=\"para\">12. \u00a0Draw the Lewis electron dot symbol for each ion.<\/p>\r\n<p style=\"padding-left: 30px;\">a) \u00a0H<sup class=\"superscript\">+<\/sup><\/p>\r\n<p style=\"padding-left: 30px;\">b) \u00a0H<sup class=\"superscript\">\u2212<\/sup><\/p>\r\n\r\n<\/div>\r\n[reveal-answer q=\"652575123\"]Show Select Answer[\/reveal-answer]\r\n[hidden-answer a=\"652575123\"]\r\n\r\n<strong>1. <\/strong>The first two electrons in a valence shell are <em class=\"emphasis\">s<\/em> electrons, which are paired.\r\n\r\n<strong>3. <\/strong>The second column of the periodic table\r\n\r\n<strong>5.<\/strong>\r\n<p style=\"padding-left: 30px;\">a) \u00a0\u00a0<a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Strontium.png\"><img class=\"alignnone wp-image-4376\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/2835\/2017\/12\/14213432\/Strontium-1.png\" alt=\"Strontium\" width=\"400\" height=\"81\" \/><\/a><\/p>\r\n<p style=\"padding-left: 30px;\">b) \u00a0\u00a0<a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Silicone.png\"><img class=\"alignnone wp-image-4375\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/2835\/2017\/12\/14213434\/Silicone-1.png\" alt=\"Silicone\" width=\"400\" height=\"81\" \/><\/a><\/p>\r\n<strong>7.<\/strong>\r\n<p style=\"padding-left: 30px;\">a) \u00a0\u00a0<a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Titanium.png\"><img class=\"alignnone wp-image-4379\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/2835\/2017\/12\/14213436\/Titanium-1.png\" alt=\"Titanium\" width=\"400\" height=\"81\" \/><\/a><\/p>\r\n<p style=\"padding-left: 30px;\">b) \u00a0\u00a0<a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Phosphorus.png\"><img class=\"alignnone wp-image-4372\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/2835\/2017\/12\/14213438\/Phosphorus-1.png\" alt=\"Phosphorus\" width=\"400\" height=\"81\" \/><\/a><\/p>\r\n<strong>9.<\/strong>\r\n<p style=\"padding-left: 30px;\">a) \u00a0\u00a0Mg<sup class=\"superscript\">2+<\/sup><\/p>\r\n<p style=\"padding-left: 30px;\">b) \u00a0\u00a0<a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Sulfur-Ion.png\"><img class=\"alignnone wp-image-4377\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/2835\/2017\/12\/14213440\/Sulfur-Ion-1.png\" alt=\"Sulfur-Ion\" width=\"400\" height=\"81\" \/><\/a><\/p>\r\n<strong>11.<\/strong>\r\n<p style=\"padding-left: 30px;\">a) \u00a0Fe<sup class=\"superscript\">2+<\/sup><\/p>\r\n<p style=\"padding-left: 30px;\">b) \u00a0\u00a0<a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Nitrogen-Ion.png\"><img class=\"alignnone wp-image-4369\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/2835\/2017\/12\/14213441\/Nitrogen-Ion-1.png\" alt=\"Nitrogen-Ion\" width=\"400\" height=\"81\" \/><\/a><\/p>\r\n[\/hidden-answer]\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>","rendered":"<div>\n<div id=\"ball-ch09_s01\" class=\"section\" lang=\"en\">\n<div class=\"textbox learning-objectives\">\n<h3>Learning Objectives<\/h3>\n<p>By the end of this section, you will be able to:<\/p>\n<ul>\n<li>Write Lewis symbols for neutral atoms and ions<\/li>\n<\/ul>\n<\/div>\n<h2>Lewis Symbols of Monoatomic Elements<\/h2>\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 symbol<\/a> (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.)<\/p>\n<p>For example, the Lewis electron dot symbol for calcium is simply<\/p>\n<p><img loading=\"lazy\" decoding=\"async\" class=\"aligncenter\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/887\/2015\/04\/23211351\/CNX_Chem_07_03_Lewisstruct1_img1.jpg\" alt=\"A Lewis structure of calcium is shown. A lone pair of electrons are shown to the right of the symbol.\" width=\"325\" height=\"34\" \/><\/p>\n<p>Figure 1 shows the Lewis symbols for the elements of the third period of the periodic table.<\/p>\n<div style=\"width: 891px\" class=\"wp-caption aligncenter\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/887\/2015\/04\/23211352\/CNX_Chem_07_03_3rowLewis1.jpg\" alt=\"A table is shown that has three columns and nine rows. The header row reads \u201cAtoms,\u201d \u201cElectronic Configuration,\u201d and \u201cLewis Symbol.\u201d The first column contains the words \u201csodium,\u201d \u201cmagnesium,\u201d \u201caluminum,\u201d \u201csilicon,\u201d \u201cphosphorus,\u201d \u201csulfur,\u201d \u201cchlorine,\u201d and \u201cargon.\u201d The second column contains the symbols and numbers \u201c[ N e ] 3 s superscript 2,\u201d \u201c[ N e ] 3 s superscript 2, 3 p superscript 1,\u201d \u201c[ N e ] 3 s superscript 2, 3 p superscript 2,\u201d \u201c[ N e ] 3 s superscript 2, 3 p superscript 3,\u201d \u201c[ N e ] 3 s superscript 2, 3 p superscript 4,\u201d \u201c[ N e ] 3 s superscript 2, 3 p superscript 5,\u201d and \u201c[ N e ] 3 s superscript 2, 3 p superscript 6.\u201d The third column contains Lewis structures for N a with one dot, M g with two dots, A l with three dots, Si with four dots, P with five dots, S with six dots, C l with seven dots, and A r with eight dots.\" width=\"881\" height=\"416\" \/><\/p>\n<p class=\"wp-caption-text\">Figure 1. Lewis symbols illustrating the number of valence electrons for each element in the third period of the periodic table.<\/p>\n<\/div>\n<\/div>\n<div lang=\"en\"><\/div>\n<div class=\"section\" lang=\"en\">\n<p>Lewis symbols can also be used to illustrate the formation of cations from atoms, as shown here for sodium and calcium:<img loading=\"lazy\" decoding=\"async\" class=\"aligncenter\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/887\/2015\/04\/23211353\/CNX_Chem_07_03_NaCa_img1.jpg\" alt=\"Two diagrams are shown. The left diagram shows a Lewis dot structure of sodium with one dot, then a right-facing arrow leading to a sodium symbol with a superscripted plus sign, a plus sign, and the letter \u201ce\u201d with a superscripted negative sign. The terms below this diagram read \u201cSodium atom\u201d and \u201cSodium cation.\u201d The right diagram shows a Lewis dot structure of calcium with two dots, then a right-facing arrow leading to a calcium symbol with a superscripted two and a plus sign, a plus sign, and the value \u201c2e\u201d with a superscripted negative sign. The terms below this diagram read \u201cCalcium atom\u201d and \u201cCalcium cation.\u201d\" width=\"885\" height=\"81\" \/>Likewise, they can be used to show the formation of anions from atoms, as shown below for chlorine and sulfur:<img loading=\"lazy\" decoding=\"async\" class=\"aligncenter\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/887\/2015\/04\/23211355\/CNX_Chem_07_03_ClS_img1.jpg\" alt=\"Two diagrams are shown. The left diagram shows a Lewis dot structure of chlorine with seven dots and the letter \u201ce\u201d with a superscripted negative sign, then a right-facing arrow leading to a chlorine symbol with eight dots and a superscripted negative sign. The terms below this diagram read, \u201cChlorine atom,\u201d and, \u201cChlorine anion.\u201d The right diagram shows a Lewis dot structure of sulfur with six dots and the symbol \u201c2e\u201d with a superscripted negative sign, then a right-facing arrow leading to a sulfur symbol with eight dots and a superscripted two and negative sign. The terms below this diagram read, \u201cSulfur atom,\u201d and, \u201cSulfur anion.\u201d\" width=\"883\" height=\"89\" \/>Figure 2 demonstrates the use of Lewis symbols to show the transfer of electrons during the formation of ionic compounds.<\/p>\n<div style=\"width: 894px\" class=\"wp-caption aligncenter\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/887\/2015\/04\/23211357\/CNX_Chem_07_03_IonLewis1.jpg\" alt=\"A table is shown with four rows. The header row reads \u201cMetal,\u201d \u201cNonmetal,\u201d and \u201cIonic Compound.\u201d The second row shows the Lewis structures of a reaction. A sodium symbol with one dot, a plus sign, and a chlorine symbol with seven dots lie to the left of a right-facing arrow. To the right of the arrow a sodium symbol with a superscripted plus sign is drawn next to a chlorine symbol with eight dots surrounded by brackets with a superscripted negative sign. One of the dots on the C l atom is red. The terms \u201csodium atom,\u201d \u201cchlorine atom,\u201d and \u201csodium chloride ( sodium ion and chloride ion )\u201d are written under the reaction. The third row shows the Lewis structures of a reaction. A magnesium symbol with two red dots, a plus sign, and an oxygen symbol with six dots lie to the left of a right-facing arrow. To the right of the arrow a magnesium symbol with a superscripted two and a plus sign is drawn next to an oxygen symbol with eight dots, two of which are red, surrounded by brackets with a superscripted two a and a negative sign. The terms \u201cmagnesium atom,\u201d \u201coxygen atom,\u201d and \u201cmagnesium oxide ( magnesium ion and oxide ion )\u201d are written under the reaction. The fourth row shows the Lewis structures of a reaction. A calcium symbol with two red dots, a plus sign, and a fluorine symbol with a coefficient of two and seven dots lie to the left of a right-facing arrow. To the right of the arrow a calcium symbol with a superscripted two and a plus sign is drawn next to a fluorine symbol with eight dots, one of which is red, surrounded by brackets with a superscripted negative sign and a subscripted two. The terms \u201ccalcium atom,\u201d \u201cfluorine atoms,\u201d and \u201ccalcium fluoride ( calcium ion and two fluoride ions )\u201d are written under the reaction.\" width=\"884\" height=\"457\" \/><\/p>\n<p class=\"wp-caption-text\">Figure 2. Cations are formed when atoms lose electrons, represented by fewer Lewis dots, whereas anions are formed by atoms gaining electrons. The total number of electrons does not change.<\/p>\n<\/div>\n<div class=\"informalfigure large block\">\n<div class=\"informalfigure large block\">\n<div class=\"informalfigure large block\">\n<div class=\"informalfigure large block\">\n<div class=\"informalfigure large block\">\n<div class=\"informalfigure large block\">\n<div class=\"informalfigure large block\">\n<div class=\"informalfigure large block\">\n<div class=\"informalfigure large block\">\n<div class=\"informalfigure large block\">\n<div class=\"textbox examples\">\n<h3>Example 1: <strong>Writing Lewis DoT SYmbols of Elements<br \/>\n<\/strong><\/h3>\n<p id=\"ball-ch09_s01_p14\" class=\"para\">What is the Lewis electron dot symbol for each element?<\/p>\n<ol id=\"ball-ch09_s01_l02\" class=\"orderedlist\">\n<li>aluminum<\/li>\n<li>selenium<\/li>\n<\/ol>\n<div class=\"qa-wrapper\" style=\"display: block\"><span class=\"show-answer collapsed\" style=\"cursor: pointer\" data-target=\"q3675621\">Show Answer<\/span><\/p>\n<div id=\"q3675621\" class=\"hidden-answer\" style=\"display: none\">\n<ol id=\"ball-ch09_s01_l03\" class=\"orderedlist\">\n<li>\n<p class=\"para\">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 (or three single dots around the atom):<\/p>\n<p><a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Aluminium.png\"><img loading=\"lazy\" decoding=\"async\" class=\"alignnone wp-image-4354\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/2835\/2017\/12\/14213413\/Aluminium-1.png\" alt=\"Aluminium\" width=\"400\" height=\"49\" \/><\/a><\/li>\n<li>\n<p class=\"para\">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:<\/p>\n<p><a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Selenium.png\"><img loading=\"lazy\" decoding=\"async\" class=\"alignnone wp-image-4374\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/2835\/2017\/12\/14213415\/Selenium-1.png\" alt=\"Selenium\" width=\"400\" height=\"49\" \/><\/a><\/li>\n<\/ol>\n<\/div>\n<\/div>\n<h4><strong>Check Your Learning<\/strong><\/h4>\n<p id=\"ball-ch09_s01_p15\" class=\"para\">What is the Lewis electron dot symbol for each element?<\/p>\n<ol id=\"ball-ch09_s01_l04\" class=\"orderedlist\">\n<li>phosphorus<\/li>\n<li>argon<\/li>\n<\/ol>\n<div class=\"qa-wrapper\" style=\"display: block\"><span class=\"show-answer collapsed\" style=\"cursor: pointer\" data-target=\"q6525751\">Show Answer<\/span><\/p>\n<div id=\"q6525751\" class=\"hidden-answer\" style=\"display: none\"> <a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Phosphorus-Argon.png\"><img loading=\"lazy\" decoding=\"async\" class=\"alignnone wp-image-4373\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/2835\/2017\/12\/14213417\/Phosphorus-Argon-1.png\" alt=\"Phosphorus-Argon\" width=\"400\" height=\"49\" \/><\/a> <\/div>\n<\/div>\n<\/div>\n<\/div>\n<\/div>\n<\/div>\n<\/div>\n<\/div>\n<\/div>\n<div class=\"informalfigure large block\">\n<div class=\"textbox examples\">\n<h3>Example 2: <strong>Writing Lewis DoT SYmbols of Ions<br \/>\n<\/strong><\/h3>\n<p id=\"ball-ch09_s01_p22\" class=\"para\">What is the Lewis electron dot symbol for each ion?<\/p>\n<ol id=\"ball-ch09_s01_l05\" class=\"orderedlist\">\n<li>Ca<sup class=\"superscript\">2+<\/sup><\/li>\n<li>O<sup class=\"superscript\">2\u2212<\/sup><\/li>\n<\/ol>\n<div class=\"qa-wrapper\" style=\"display: block\"><span class=\"show-answer collapsed\" style=\"cursor: pointer\" data-target=\"q36756212\">Show Answer<\/span><\/p>\n<div id=\"q36756212\" class=\"hidden-answer\" style=\"display: none\">\n<ol id=\"ball-ch09_s01_l06\" class=\"orderedlist\">\n<li>\n<p class=\"para\">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><\/li>\n<li>\n<p class=\"para\">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:<\/p>\n<p><a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Oxygen-Ion.png\"><img loading=\"lazy\" decoding=\"async\" class=\"alignnone wp-image-4371\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/2835\/2017\/12\/14213428\/Oxygen-Ion-1.png\" alt=\"Oxygen-Ion\" width=\"400\" height=\"49\" \/><\/a><\/li>\n<\/ol>\n<\/div>\n<\/div>\n<h4><strong>Check Your Learning<\/strong><\/h4>\n<p>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<div class=\"qa-wrapper\" style=\"display: block\"><span class=\"show-answer collapsed\" style=\"cursor: pointer\" data-target=\"q65257512\">Show Answer<\/span><\/p>\n<div id=\"q65257512\" class=\"hidden-answer\" style=\"display: none\">\u00a0<a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Thallium-Ion.png\"><img loading=\"lazy\" decoding=\"async\" class=\"alignnone wp-image-4378\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/2835\/2017\/12\/14213430\/Thallium-Ion-1.png\" alt=\"Thallium-Ion\" width=\"400\" height=\"49\" \/><\/a> <\/div>\n<\/div>\n<\/div>\n<\/div>\n<div id=\"ball-ch09_s01_n04\" class=\"key_takeaways editable block\">\n<div class=\"bcc-box bcc-success\">\n<h3>Key Takeaways<\/h3>\n<ul id=\"ball-ch09_s01_l07\" class=\"itemizedlist\">\n<li>Lewis electron dot diagrams use dots to represent valence electrons around an atomic symbol.<\/li>\n<li>Lewis electron dot diagrams for ions have fewer (for cations) or more (for anions) dots than the corresponding atom.<\/li>\n<\/ul>\n<\/div>\n<\/div>\n<div id=\"ball-ch09_s01_qs01\" class=\"qandaset block\">\n<div class=\"bcc-box bcc-info\">\n<h3>Exercises<\/h3>\n<div class=\"question\">\n<p id=\"ball-ch09_s01_qs01_p01\" class=\"para\">1.\u00a0 Explain why the first two dots in a Lewis electron dot symbol are drawn on the same side of the atomic symbol.<\/p>\n<\/div>\n<div class=\"question\">\n<p id=\"ball-ch09_s01_qs01_p03\" class=\"para\">2.\u00a0 Is it necessary for the first dot around an atomic symbol to go on a particular side of the atomic symbol?<\/p>\n<\/div>\n<div class=\"question\">\n<p id=\"ball-ch09_s01_qs01_p05\" class=\"para\">3.\u00a0 What column of the periodic table has Lewis electron dot symbol with two electrons?<\/p>\n<\/div>\n<div class=\"question\">\n<p id=\"ball-ch09_s01_qs01_p07\" class=\"para\">4.\u00a0 What column of the periodic table has Lewis electron dot symbol that have six electrons in them?<\/p>\n<\/div>\n<div class=\"question\">\n<p id=\"ball-ch09_s01_qs01_p09\" class=\"para\">5.\u00a0 Draw the Lewis electron dot symbol for each element.<\/p>\n<\/div>\n<p style=\"padding-left: 30px;\">a) \u00a0strontium<\/p>\n<p style=\"padding-left: 30px;\">b) \u00a0silicon<\/p>\n<div class=\"question\">\n<p id=\"ball-ch09_s01_qs01_p10\" class=\"para\">6. \u00a0Draw the Lewis electron dot symbol for each element.<\/p>\n<p style=\"padding-left: 30px;\">a) \u00a0krypton<\/p>\n<p style=\"padding-left: 30px;\">b) \u00a0sulfur<\/p>\n<\/div>\n<div class=\"question\">\n<p id=\"ball-ch09_s01_qs01_p11\" class=\"para\">7. \u00a0Draw the Lewis electron dot symbol for each element.<\/p>\n<p style=\"padding-left: 30px;\">a) \u00a0titanium<\/p>\n<p style=\"padding-left: 30px;\">b) \u00a0phosphorus<\/p>\n<\/div>\n<div class=\"question\">\n<p id=\"ball-ch09_s01_qs01_p12\" class=\"para\">8. \u00a0Draw the Lewis electron dot symbol for each element.<\/p>\n<p style=\"padding-left: 30px;\">a) \u00a0bromine<\/p>\n<p style=\"padding-left: 30px;\">b) \u00a0gallium<\/p>\n<\/div>\n<div class=\"question\">\n<p id=\"ball-ch09_s01_qs01_p13\" class=\"para\">9. \u00a0Draw the Lewis electron dot symbol for each ion.<\/p>\n<p style=\"padding-left: 30px;\">a) \u00a0Mg<sup class=\"superscript\">2+<\/sup><\/p>\n<p style=\"padding-left: 30px;\">b) \u00a0S<sup class=\"superscript\">2\u2212<\/sup><\/p>\n<\/div>\n<div class=\"question\">\n<p id=\"ball-ch09_s01_qs01_p14\" class=\"para\">10. \u00a0Draw the Lewis electron dot symbol for each ion.<\/p>\n<p style=\"padding-left: 30px;\">a) \u00a0In<sup class=\"superscript\">+<\/sup><\/p>\n<p style=\"padding-left: 30px;\">b) \u00a0Br<sup class=\"superscript\">\u2212<\/sup><\/p>\n<\/div>\n<div class=\"question\">\n<p id=\"ball-ch09_s01_qs01_p15\" class=\"para\">11. \u00a0Draw the Lewis electron dot symbol for each ion.<\/p>\n<p style=\"padding-left: 30px;\">a) \u00a0Fe<sup class=\"superscript\">2+<\/sup><\/p>\n<p style=\"padding-left: 30px;\">b) \u00a0N<sup class=\"superscript\">3\u2212<\/sup><\/p>\n<\/div>\n<div class=\"question\">\n<p id=\"ball-ch09_s01_qs01_p16\" class=\"para\">12. \u00a0Draw the Lewis electron dot symbol for each ion.<\/p>\n<p style=\"padding-left: 30px;\">a) \u00a0H<sup class=\"superscript\">+<\/sup><\/p>\n<p style=\"padding-left: 30px;\">b) \u00a0H<sup class=\"superscript\">\u2212<\/sup><\/p>\n<\/div>\n<div class=\"qa-wrapper\" style=\"display: block\"><span class=\"show-answer collapsed\" style=\"cursor: pointer\" data-target=\"q652575123\">Show Select Answer<\/span><\/p>\n<div id=\"q652575123\" class=\"hidden-answer\" style=\"display: none\">\n<p><strong>1. <\/strong>The first two electrons in a valence shell are <em class=\"emphasis\">s<\/em> electrons, which are paired.<\/p>\n<p><strong>3. <\/strong>The second column of the periodic table<\/p>\n<p><strong>5.<\/strong><\/p>\n<p style=\"padding-left: 30px;\">a) \u00a0\u00a0<a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Strontium.png\"><img loading=\"lazy\" decoding=\"async\" class=\"alignnone wp-image-4376\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/2835\/2017\/12\/14213432\/Strontium-1.png\" alt=\"Strontium\" width=\"400\" height=\"81\" \/><\/a><\/p>\n<p style=\"padding-left: 30px;\">b) \u00a0\u00a0<a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Silicone.png\"><img loading=\"lazy\" decoding=\"async\" class=\"alignnone wp-image-4375\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/2835\/2017\/12\/14213434\/Silicone-1.png\" alt=\"Silicone\" width=\"400\" height=\"81\" \/><\/a><\/p>\n<p><strong>7.<\/strong><\/p>\n<p style=\"padding-left: 30px;\">a) \u00a0\u00a0<a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Titanium.png\"><img loading=\"lazy\" decoding=\"async\" class=\"alignnone wp-image-4379\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/2835\/2017\/12\/14213436\/Titanium-1.png\" alt=\"Titanium\" width=\"400\" height=\"81\" \/><\/a><\/p>\n<p style=\"padding-left: 30px;\">b) \u00a0\u00a0<a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Phosphorus.png\"><img loading=\"lazy\" decoding=\"async\" class=\"alignnone wp-image-4372\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/2835\/2017\/12\/14213438\/Phosphorus-1.png\" alt=\"Phosphorus\" width=\"400\" height=\"81\" \/><\/a><\/p>\n<p><strong>9.<\/strong><\/p>\n<p style=\"padding-left: 30px;\">a) \u00a0\u00a0Mg<sup class=\"superscript\">2+<\/sup><\/p>\n<p style=\"padding-left: 30px;\">b) \u00a0\u00a0<a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Sulfur-Ion.png\"><img loading=\"lazy\" decoding=\"async\" class=\"alignnone wp-image-4377\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/2835\/2017\/12\/14213440\/Sulfur-Ion-1.png\" alt=\"Sulfur-Ion\" width=\"400\" height=\"81\" \/><\/a><\/p>\n<p><strong>11.<\/strong><\/p>\n<p style=\"padding-left: 30px;\">a) \u00a0Fe<sup class=\"superscript\">2+<\/sup><\/p>\n<p style=\"padding-left: 30px;\">b) \u00a0\u00a0<a href=\"http:\/\/opentextbc.ca\/introductorychemistry\/wp-content\/uploads\/sites\/17\/2014\/09\/Nitrogen-Ion.png\"><img loading=\"lazy\" decoding=\"async\" class=\"alignnone wp-image-4369\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/2835\/2017\/12\/14213441\/Nitrogen-Ion-1.png\" alt=\"Nitrogen-Ion\" width=\"400\" height=\"81\" \/><\/a><\/p>\n<\/div>\n<\/div>\n<\/div>\n<\/div>\n<\/div>\n<\/div>\n<\/div>\n<\/div>\n<\/div>\n<\/div>\n\n\t\t\t <section class=\"citations-section\" role=\"contentinfo\">\n\t\t\t <h3>Candela Citations<\/h3>\n\t\t\t\t\t <div>\n\t\t\t\t\t\t <div id=\"citation-list-381\">\n\t\t\t\t\t\t\t <div class=\"licensing\"><div class=\"license-attribution-dropdown-subheading\">CC licensed content, Shared previously<\/div><ul class=\"citation-list\"><li>Introductory Chemistry- 1st Canadian Edition . <strong>Authored by<\/strong>: Jessie A. Key and David W. Ball. <strong>Provided by<\/strong>: BCCampus. <strong>Located at<\/strong>: <a target=\"_blank\" href=\"https:\/\/opentextbc.ca\/introductorychemistry\/\">https:\/\/opentextbc.ca\/introductorychemistry\/<\/a>. <strong>License<\/strong>: <em><a target=\"_blank\" rel=\"license\" href=\"https:\/\/creativecommons.org\/licenses\/by-nc-sa\/4.0\/\">CC BY-NC-SA: Attribution-NonCommercial-ShareAlike<\/a><\/em>. <strong>License Terms<\/strong>: Download this book for free at http:\/\/open.bccampus.ca<\/li><li>Chemistry. <strong>Provided by<\/strong>: OpenStaxCollege. <strong>Located at<\/strong>: <a target=\"_blank\" href=\"http:\/\/openstaxcollege.org\">http:\/\/openstaxcollege.org<\/a>. <strong>License<\/strong>: <em><a target=\"_blank\" rel=\"license\" href=\"https:\/\/creativecommons.org\/licenses\/by\/4.0\/\">CC BY: Attribution<\/a><\/em>. <strong>License Terms<\/strong>: Download for free at https:\/\/openstaxcollege.org\/textbooks\/chemistry\/get<\/li><\/ul><\/div>\n\t\t\t\t\t\t <\/div>\n\t\t\t\t\t <\/div>\n\t\t\t <\/section>","protected":false},"author":23485,"menu_order":1,"template":"","meta":{"_candela_citation":"[{\"type\":\"cc\",\"description\":\"Introductory Chemistry- 1st Canadian Edition \",\"author\":\"Jessie A. 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