{"id":3068,"date":"2016-08-25T17:18:09","date_gmt":"2016-08-25T17:18:09","guid":{"rendered":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/?post_type=chapter&#038;p=3068"},"modified":"2016-08-26T02:17:08","modified_gmt":"2016-08-26T02:17:08","slug":"bond-polarity","status":"publish","type":"chapter","link":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/chapter\/bond-polarity\/","title":{"raw":"Bond Polarity","rendered":"Bond Polarity"},"content":{"raw":"<div class=\"x-ck12-data-objectives\">\r\n<div class=\"textbox learning-objectives\">\r\n<h3>Learning Objectives<\/h3>\r\n<ul>\r\n \t<li>Define electronegativity.<\/li>\r\n \t<li>Use electronegativity values to determine bond type.<\/li>\r\n<\/ul>\r\n<\/div>\r\n<\/div>\r\n<div class=\"textbox examples\">\r\n<h3><strong style=\"line-height: 1.5;\">What makes people share?<\/strong><\/h3>\r\n<p id=\"x-ck12-YzY2MGUxOTE3N2Y2MmE3MTFhYjAwY2RiMDNkYzFkMWU.-djn\"><img class=\"alignright size-medium wp-image-3140\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/515\/2016\/08\/25170122\/people-coffee-tea-meeting-300x200.jpg\" alt=\"four people meeting around a table\" width=\"300\" height=\"200\" \/>Have you ever spent time with someone you really didn\u2019t like?\u00a0 You had nothing in common with them and did not want to have anything to do with them.\u00a0 On the other hand, there are people you enjoy being with.\u00a0 You have a lot in common and like to share with them.\u00a0 Atoms work the same way.\u00a0 If there are strong differences in their attraction of electrons, one atoms gets the electrons and the other atom loses them.\u00a0 If they are similar, they share the electrons to form a covalent bond.<\/p>\r\n\r\n<\/div>\r\n<p id=\"x-ck12-YjdlNjg1NDgwNGJmMGJhMTZjMzQ0MDEzZDcwYjllNTg.-4p6\"><strong> Electronegativity <\/strong> is defined as the ability of an atom to attract electrons when the atoms are in a compound.\u00a0 Electronegativities of elements are shown in the periodic table below.<\/p>\r\n\r\n<div id=\"x-ck12-Mzc0YWUwZDFhYzA4NmJhMzUzZjRlYjBjMDMwZDIzOWI.-ywe\" class=\"x-ck12-img-postcard x-ck12-nofloat\">\r\n\r\n[caption id=\"\" align=\"aligncenter\" width=\"500\"]<img id=\"x-ck12-OTgwNDUtMTM2MTg1OTc5MC00MS01LUltYWdlLS0tMTk.\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/53\/2014\/08\/19211522\/20140811155256944281.png\" alt=\"Electronegativity values of elements in the periodic table\" width=\"500\" height=\"241\" longdesc=\"Electronegativities%20of%20elements.\" \/> Figure 1.\u00a0Electronegativities of elements.[\/caption]\r\n\r\n<\/div>\r\n<div id=\"x-ck12-MmZjYjU2MmRlN2FkMGVhMzQ5ZTI1ZGEyZTFkOTU0ZDg.-9df\" class=\"x-ck12-img-postcard x-ck12-nofloat\">\r\n\r\n[caption id=\"\" align=\"alignright\" width=\"313\"]<img id=\"x-ck12-OTgwNDUtMTM2MTg1OTg0Mi03Mi0zMC1JbWFnZS0tLTIw\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/53\/2014\/08\/19211523\/20140811155257031327.png\" alt=\"Electronegativity difference and whether the bond is covalent, polar covalent, or ionic. Bond type is predicated on the difference in electronegativity of the two elements involved in the bond.\" width=\"313\" height=\"500\" \/> Figure 2.\u00a0Bond type is predicated on the difference in electronegativity of the two elements involved in the bond.[\/caption]\r\n\r\n<\/div>\r\n<p id=\"x-ck12-MDRlNjA0YzM1Zjg0NDdjYTUzNTc3MTUwYjdmODQ0ZTI.-sxz\">The degree to which a given bond is ionic or covalent is determined by calculating the difference in electronegativity between the two atoms involved in the bond.<\/p>\r\n<p id=\"x-ck12-MmEwMDYyMGNhNTJlMWYyYjNhODE3ZjYyNTljZDM2YzI.-kz8\">As an example, consider the bond that occurs between an atom of potassium and an atom of fluorine.\u00a0 Using the table, the difference in electronegativity is equal to 4.0\u00a0-\u00a00.8\u00a0=\u00a03.2.<\/p>\r\nSince the difference in electronegativity is relatively large, the bond between the two atoms is ionic.\u00a0 Since the fluorine atom has a much larger attraction for electrons than the potassium atom does, the valence electron from the potassium atom is completely transferred to the fluorine atom.\u00a0 The diagram below\u00a0shows how difference in electronegativity relates to the ionic or covalent character of a chemical bond.\r\n<h2>Nonpolar Covalent Bonds<\/h2>\r\n<p id=\"x-ck12-NTNiYmRlMTI3Yjk2YWM3NjY5YjhmMjQ0MDljZjMxODI.-fjd\">A bond in which the electronegativity difference is less than 1.7 is considered to be mostly covalent in character. However, at this point we need to distinguish between two general types of covalent bonds.<\/p>\r\nA <strong> nonpolar covalent bond <\/strong> is a covalent bond in which the bonding electrons are shared equally between the two atoms. In a nonpolar covalent bond, the distribution of electrical charge is balanced between the two atoms.\r\n\r\n[caption id=\"\" align=\"aligncenter\" width=\"500\"]<img id=\"x-ck12-OTgwNDUtMTM2MTg1OTk2Ny0xMS0xMC1JbWFnZS0tLTIx\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/53\/2014\/08\/19211524\/20140811155257109593.png\" alt=\"A nonpolar covalent bond is one in which the distribution of electron density between the two atoms is equal.\" width=\"500\" height=\"310\" \/> Figure 3.\u00a0A nonpolar covalent bond is one in which the distribution of electron density between the two atoms is equal.[\/caption]\r\n<p id=\"x-ck12-M2FhMzI1MTgwMzBiMjU3OTAzNTZhYzRiOGM1NzhjZGY.-nxm\">The two chlorine atoms share the pair of electrons in the single covalent bond equally, and the electron density surrounding the Cl<sub>2 <\/sub> molecule is symmetrical.\u00a0 Also note that molecules in which the electronegativity difference is very small (&lt;0.4) are also considered nonpolar covalent.\u00a0 An example would be a bond between chlorine and bromine <img id=\"x-ck12-MTQwMDUxODI3MDM2Nw..\" class=\"x-ck12-math\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/53\/2014\/08\/19211526\/495e087690890785c303ba6dc63e1006.png\" alt=\"(Delta EN = 3.0 - 2.8 = 0.2)\" width=\"197\" height=\"18\" \/> .<\/p>\r\n\r\n<h2>Polar Covalent Bonds<\/h2>\r\n[caption id=\"\" align=\"aligncenter\" width=\"192\"]<img id=\"x-ck12-OTgwNDUtMTM2MTg2MDAzNy04Mi0zOC1JbWFnZS0tLTIy\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/53\/2014\/08\/19211526\/20140811155257200024.png\" alt=\"In the polar covalent bond of HF the electron density is unevenly distributed. There is a higher density red near the fluorine atom and a lower density blue near the hydrogen atom.\" width=\"192\" height=\"154\" \/> Figure 4.\u00a0In the polar covalent bond of HF, the electron density is unevenly distributed. There is a higher density (red) near the fluorine atom, and a lower density (blue) near the hydrogen atom.[\/caption]\r\n\r\nA bond in which the electronegativity difference between the atoms is between 0.4 and 1.7 is called a polar covalent bond.\r\n\r\nA <strong> polar covalent bond <\/strong> is a covalent bond in which the atoms have an unequal attraction for electrons and so the sharing is unequal.\u00a0 In a polar covalent bond, sometimes simply called a polar bond, the distribution of electrons around the molecule is no longer symmetrical.\r\n<p id=\"x-ck12-Y2I4MzgxOWQxMWQ0NGVlMzYyOWEwMWRjYjU0NzE3MmI.-igp\">An easy way to illustrate the uneven electron distribution in a polar covalent bond is to use the Greek letter delta (<em>\u03b4<\/em>).<\/p>\r\n\r\n\r\n[caption id=\"\" align=\"aligncenter\" width=\"192\"]<img id=\"x-ck12-OTgwNDUtMTM2MTg2MDA5NS00My01NS1JbWFnZS0tLTIz\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/53\/2014\/08\/19211527\/20140811155257330982.png\" alt=\"Delta symbols can be used to indicate polarity\" width=\"192\" height=\"151\" \/> Figure 5.\u00a0Use of \u03b4 to indicate partial charge.[\/caption]\r\n<p id=\"x-ck12-NDkzMThhZGQ3ODM4OTc1MTIyNDlhNDRjZTZkYzg2Mzg.-5el\">The atom with the greater electronegativity acquires a partial negative charge, while the atom with the lesser electronegativity acquires a partial positive charge.\u00a0 The delta symbol is used to indicate that the quantity of charge is less than one.\u00a0 A crossed arrow can also be used to indicate the direction of greater electron density.<\/p>\r\n\r\n\r\n[caption id=\"\" align=\"aligncenter\" width=\"192\"]<img id=\"x-ck12-OTgwNDUtMTM2MTg2MDEyOC0yOS0xNC1JbWFnZS0tLTI0\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/53\/2014\/08\/19211528\/20140811155257526819.png\" alt=\"A crossed\u00a0arrow\u00a0can be used to indicate polarity\" width=\"192\" height=\"139\" \/> Figure 6.\u00a0Use of crossed arrow to indicate polarity.[\/caption]\r\n\r\n<div class=\"textbox key-takeaways\">\r\n<h3>Summary<\/h3>\r\n<ul id=\"x-ck12-YmFjMTcyZWVjODNlZmZmZjYxZjZmZmEyOWZmZDA0ZmY.-gq2\">\r\n \t<li>The electronegativity of an atom determines how strongly it attracts electrons to itself.<\/li>\r\n \t<li>The polarity of a bond is affected by the electronegativity values of the two atoms involved in that bond.<\/li>\r\n<\/ul>\r\n<\/div>\r\n<div class=\"textbox exercises\">\r\n<h3>Practice<\/h3>\r\n<p id=\"x-ck12-MDBhOGMyMjE2YTQ4NTEwN2FmOGI1NDkxNWE4MGU0YTE.-jrx\">Take the quiz on the right-hand side of this page:<\/p>\r\n<p id=\"x-ck12-NDZlMTQxNThlNDA0OGRmOGFmN2ExMGUwNDc0MjRjYmU.-5qf\"><a href=\"http:\/\/www.sophia.org\/determining-bond-polarity\/determining-bond-polarity-tutorial\"> http:\/\/www.sophia.org\/determining-bond-polarity\/determining-bond-polarity-tutorial<\/a><\/p>\r\n\r\n<\/div>\r\n<div class=\"textbox exercises\">\r\n<h3>Review<\/h3>\r\n<ol id=\"x-ck12-NGI0YjU1Mjg3MzQ2OTllZjE5MDgyY2U1MDcxZmZlODE.-bkp\">\r\n \t<li>What is the bond type of a bond with a difference of 1.9?<\/li>\r\n \t<li>What would be he bond type for BH<sub>2 <\/sub> ?<\/li>\r\n \t<li>Your friend tells you that the LiF bond is covalent. What do you say?<\/li>\r\n<\/ol>\r\n<\/div>\r\n<h2>\u00a0Glossary<\/h2>\r\n<div class=\"x-ck12-data-vocabulary\">\r\n<ul id=\"x-ck12-NDExY2EwMTVmODZmYmQ5NDE4MjM5YjU0YzgyZTRjZTM.-sfk\">\r\n \t<li><strong> electronegativity: <\/strong> The ability of an atom to attract electrons when the atoms are in a compound.<\/li>\r\n \t<li><strong> nonpolar covalent bond: <\/strong> A covalent bond in which the bonding electrons are shared equally between the two atoms.<\/li>\r\n \t<li><strong> polar covalent bond: <\/strong> A covalent bond in which the atoms have an unequal attraction for electrons and so the sharing is unequal.<\/li>\r\n<\/ul>\r\n<\/div>","rendered":"<div class=\"x-ck12-data-objectives\">\n<div class=\"textbox learning-objectives\">\n<h3>Learning Objectives<\/h3>\n<ul>\n<li>Define electronegativity.<\/li>\n<li>Use electronegativity values to determine bond type.<\/li>\n<\/ul>\n<\/div>\n<\/div>\n<div class=\"textbox examples\">\n<h3><strong style=\"line-height: 1.5;\">What makes people share?<\/strong><\/h3>\n<p id=\"x-ck12-YzY2MGUxOTE3N2Y2MmE3MTFhYjAwY2RiMDNkYzFkMWU.-djn\"><img loading=\"lazy\" decoding=\"async\" class=\"alignright size-medium wp-image-3140\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/515\/2016\/08\/25170122\/people-coffee-tea-meeting-300x200.jpg\" alt=\"four people meeting around a table\" width=\"300\" height=\"200\" \/>Have you ever spent time with someone you really didn\u2019t like?\u00a0 You had nothing in common with them and did not want to have anything to do with them.\u00a0 On the other hand, there are people you enjoy being with.\u00a0 You have a lot in common and like to share with them.\u00a0 Atoms work the same way.\u00a0 If there are strong differences in their attraction of electrons, one atoms gets the electrons and the other atom loses them.\u00a0 If they are similar, they share the electrons to form a covalent bond.<\/p>\n<\/div>\n<p id=\"x-ck12-YjdlNjg1NDgwNGJmMGJhMTZjMzQ0MDEzZDcwYjllNTg.-4p6\"><strong> Electronegativity <\/strong> is defined as the ability of an atom to attract electrons when the atoms are in a compound.\u00a0 Electronegativities of elements are shown in the periodic table below.<\/p>\n<div id=\"x-ck12-Mzc0YWUwZDFhYzA4NmJhMzUzZjRlYjBjMDMwZDIzOWI.-ywe\" class=\"x-ck12-img-postcard x-ck12-nofloat\">\n<div style=\"width: 510px\" class=\"wp-caption aligncenter\"><img loading=\"lazy\" decoding=\"async\" id=\"x-ck12-OTgwNDUtMTM2MTg1OTc5MC00MS01LUltYWdlLS0tMTk.\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/53\/2014\/08\/19211522\/20140811155256944281.png\" alt=\"Electronegativity values of elements in the periodic table\" width=\"500\" height=\"241\" longdesc=\"Electronegativities%20of%20elements.\" \/><\/p>\n<p class=\"wp-caption-text\">Figure 1.\u00a0Electronegativities of elements.<\/p>\n<\/div>\n<\/div>\n<div id=\"x-ck12-MmZjYjU2MmRlN2FkMGVhMzQ5ZTI1ZGEyZTFkOTU0ZDg.-9df\" class=\"x-ck12-img-postcard x-ck12-nofloat\">\n<div style=\"width: 323px\" class=\"wp-caption alignright\"><img loading=\"lazy\" decoding=\"async\" id=\"x-ck12-OTgwNDUtMTM2MTg1OTg0Mi03Mi0zMC1JbWFnZS0tLTIw\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/53\/2014\/08\/19211523\/20140811155257031327.png\" alt=\"Electronegativity difference and whether the bond is covalent, polar covalent, or ionic. Bond type is predicated on the difference in electronegativity of the two elements involved in the bond.\" width=\"313\" height=\"500\" \/><\/p>\n<p class=\"wp-caption-text\">Figure 2.\u00a0Bond type is predicated on the difference in electronegativity of the two elements involved in the bond.<\/p>\n<\/div>\n<\/div>\n<p id=\"x-ck12-MDRlNjA0YzM1Zjg0NDdjYTUzNTc3MTUwYjdmODQ0ZTI.-sxz\">The degree to which a given bond is ionic or covalent is determined by calculating the difference in electronegativity between the two atoms involved in the bond.<\/p>\n<p id=\"x-ck12-MmEwMDYyMGNhNTJlMWYyYjNhODE3ZjYyNTljZDM2YzI.-kz8\">As an example, consider the bond that occurs between an atom of potassium and an atom of fluorine.\u00a0 Using the table, the difference in electronegativity is equal to 4.0\u00a0&#8211;\u00a00.8\u00a0=\u00a03.2.<\/p>\n<p>Since the difference in electronegativity is relatively large, the bond between the two atoms is ionic.\u00a0 Since the fluorine atom has a much larger attraction for electrons than the potassium atom does, the valence electron from the potassium atom is completely transferred to the fluorine atom.\u00a0 The diagram below\u00a0shows how difference in electronegativity relates to the ionic or covalent character of a chemical bond.<\/p>\n<h2>Nonpolar Covalent Bonds<\/h2>\n<p id=\"x-ck12-NTNiYmRlMTI3Yjk2YWM3NjY5YjhmMjQ0MDljZjMxODI.-fjd\">A bond in which the electronegativity difference is less than 1.7 is considered to be mostly covalent in character. However, at this point we need to distinguish between two general types of covalent bonds.<\/p>\n<p>A <strong> nonpolar covalent bond <\/strong> is a covalent bond in which the bonding electrons are shared equally between the two atoms. In a nonpolar covalent bond, the distribution of electrical charge is balanced between the two atoms.<\/p>\n<div style=\"width: 510px\" class=\"wp-caption aligncenter\"><img loading=\"lazy\" decoding=\"async\" id=\"x-ck12-OTgwNDUtMTM2MTg1OTk2Ny0xMS0xMC1JbWFnZS0tLTIx\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/53\/2014\/08\/19211524\/20140811155257109593.png\" alt=\"A nonpolar covalent bond is one in which the distribution of electron density between the two atoms is equal.\" width=\"500\" height=\"310\" \/><\/p>\n<p class=\"wp-caption-text\">Figure 3.\u00a0A nonpolar covalent bond is one in which the distribution of electron density between the two atoms is equal.<\/p>\n<\/div>\n<p id=\"x-ck12-M2FhMzI1MTgwMzBiMjU3OTAzNTZhYzRiOGM1NzhjZGY.-nxm\">The two chlorine atoms share the pair of electrons in the single covalent bond equally, and the electron density surrounding the Cl<sub>2 <\/sub> molecule is symmetrical.\u00a0 Also note that molecules in which the electronegativity difference is very small (&lt;0.4) are also considered nonpolar covalent.\u00a0 An example would be a bond between chlorine and bromine <img loading=\"lazy\" decoding=\"async\" id=\"x-ck12-MTQwMDUxODI3MDM2Nw..\" class=\"x-ck12-math\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/53\/2014\/08\/19211526\/495e087690890785c303ba6dc63e1006.png\" alt=\"(Delta EN = 3.0 - 2.8 = 0.2)\" width=\"197\" height=\"18\" \/> .<\/p>\n<h2>Polar Covalent Bonds<\/h2>\n<div style=\"width: 202px\" class=\"wp-caption aligncenter\"><img loading=\"lazy\" decoding=\"async\" id=\"x-ck12-OTgwNDUtMTM2MTg2MDAzNy04Mi0zOC1JbWFnZS0tLTIy\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/53\/2014\/08\/19211526\/20140811155257200024.png\" alt=\"In the polar covalent bond of HF the electron density is unevenly distributed. There is a higher density red near the fluorine atom and a lower density blue near the hydrogen atom.\" width=\"192\" height=\"154\" \/><\/p>\n<p class=\"wp-caption-text\">Figure 4.\u00a0In the polar covalent bond of HF, the electron density is unevenly distributed. There is a higher density (red) near the fluorine atom, and a lower density (blue) near the hydrogen atom.<\/p>\n<\/div>\n<p>A bond in which the electronegativity difference between the atoms is between 0.4 and 1.7 is called a polar covalent bond.<\/p>\n<p>A <strong> polar covalent bond <\/strong> is a covalent bond in which the atoms have an unequal attraction for electrons and so the sharing is unequal.\u00a0 In a polar covalent bond, sometimes simply called a polar bond, the distribution of electrons around the molecule is no longer symmetrical.<\/p>\n<p id=\"x-ck12-Y2I4MzgxOWQxMWQ0NGVlMzYyOWEwMWRjYjU0NzE3MmI.-igp\">An easy way to illustrate the uneven electron distribution in a polar covalent bond is to use the Greek letter delta (<em>\u03b4<\/em>).<\/p>\n<div style=\"width: 202px\" class=\"wp-caption aligncenter\"><img loading=\"lazy\" decoding=\"async\" id=\"x-ck12-OTgwNDUtMTM2MTg2MDA5NS00My01NS1JbWFnZS0tLTIz\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/53\/2014\/08\/19211527\/20140811155257330982.png\" alt=\"Delta symbols can be used to indicate polarity\" width=\"192\" height=\"151\" \/><\/p>\n<p class=\"wp-caption-text\">Figure 5.\u00a0Use of \u03b4 to indicate partial charge.<\/p>\n<\/div>\n<p id=\"x-ck12-NDkzMThhZGQ3ODM4OTc1MTIyNDlhNDRjZTZkYzg2Mzg.-5el\">The atom with the greater electronegativity acquires a partial negative charge, while the atom with the lesser electronegativity acquires a partial positive charge.\u00a0 The delta symbol is used to indicate that the quantity of charge is less than one.\u00a0 A crossed arrow can also be used to indicate the direction of greater electron density.<\/p>\n<div style=\"width: 202px\" class=\"wp-caption aligncenter\"><img loading=\"lazy\" decoding=\"async\" id=\"x-ck12-OTgwNDUtMTM2MTg2MDEyOC0yOS0xNC1JbWFnZS0tLTI0\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/53\/2014\/08\/19211528\/20140811155257526819.png\" alt=\"A crossed\u00a0arrow\u00a0can be used to indicate polarity\" width=\"192\" height=\"139\" \/><\/p>\n<p class=\"wp-caption-text\">Figure 6.\u00a0Use of crossed arrow to indicate polarity.<\/p>\n<\/div>\n<div class=\"textbox key-takeaways\">\n<h3>Summary<\/h3>\n<ul id=\"x-ck12-YmFjMTcyZWVjODNlZmZmZjYxZjZmZmEyOWZmZDA0ZmY.-gq2\">\n<li>The electronegativity of an atom determines how strongly it attracts electrons to itself.<\/li>\n<li>The polarity of a bond is affected by the electronegativity values of the two atoms involved in that bond.<\/li>\n<\/ul>\n<\/div>\n<div class=\"textbox exercises\">\n<h3>Practice<\/h3>\n<p id=\"x-ck12-MDBhOGMyMjE2YTQ4NTEwN2FmOGI1NDkxNWE4MGU0YTE.-jrx\">Take the quiz on the right-hand side of this page:<\/p>\n<p id=\"x-ck12-NDZlMTQxNThlNDA0OGRmOGFmN2ExMGUwNDc0MjRjYmU.-5qf\"><a href=\"http:\/\/www.sophia.org\/determining-bond-polarity\/determining-bond-polarity-tutorial\"> http:\/\/www.sophia.org\/determining-bond-polarity\/determining-bond-polarity-tutorial<\/a><\/p>\n<\/div>\n<div class=\"textbox exercises\">\n<h3>Review<\/h3>\n<ol id=\"x-ck12-NGI0YjU1Mjg3MzQ2OTllZjE5MDgyY2U1MDcxZmZlODE.-bkp\">\n<li>What is the bond type of a bond with a difference of 1.9?<\/li>\n<li>What would be he bond type for BH<sub>2 <\/sub> ?<\/li>\n<li>Your friend tells you that the LiF bond is covalent. What do you say?<\/li>\n<\/ol>\n<\/div>\n<h2>\u00a0Glossary<\/h2>\n<div class=\"x-ck12-data-vocabulary\">\n<ul id=\"x-ck12-NDExY2EwMTVmODZmYmQ5NDE4MjM5YjU0YzgyZTRjZTM.-sfk\">\n<li><strong> electronegativity: <\/strong> The ability of an atom to attract electrons when the atoms are in a compound.<\/li>\n<li><strong> nonpolar covalent bond: <\/strong> A covalent bond in which the bonding electrons are shared equally between the two atoms.<\/li>\n<li><strong> polar covalent bond: <\/strong> A covalent bond in which the atoms have an unequal attraction for electrons and so the sharing is unequal.<\/li>\n<\/ul>\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-3068\">\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>Chemistry Concepts Intermediate. <strong>Authored by<\/strong>: Calbreath, Baxter, et al.. <strong>Provided by<\/strong>: CK12.org. <strong>Located at<\/strong>: <a target=\"_blank\" href=\"http:\/\/www.ck12.org\/book\/CK-12-Chemistry-Concepts-Intermediate\/\">http:\/\/www.ck12.org\/book\/CK-12-Chemistry-Concepts-Intermediate\/<\/a>. <strong>License<\/strong>: <em><a target=\"_blank\" rel=\"license\" href=\"https:\/\/creativecommons.org\/licenses\/by-nc\/4.0\/\">CC BY-NC: Attribution-NonCommercial<\/a><\/em><\/li><li>waterstreet coffee bar. <strong>Provided by<\/strong>: Startup Stock Photos. <strong>Located at<\/strong>: <a target=\"_blank\" href=\"http:\/\/startupstockphotos.com\/post\/94180886521\/waterstreet-coffee-bar-on-location-for-a\">http:\/\/startupstockphotos.com\/post\/94180886521\/waterstreet-coffee-bar-on-location-for-a<\/a>. <strong>License<\/strong>: <em><a target=\"_blank\" rel=\"license\" href=\"https:\/\/creativecommons.org\/about\/cc0\">CC0: No Rights Reserved<\/a><\/em><\/li><\/ul><div class=\"license-attribution-dropdown-subheading\">Public domain content<\/div><ul class=\"citation-list\"><li>Hydrogen fluoride. <strong>Authored by<\/strong>: Ben Mills. <strong>Located at<\/strong>: <a target=\"_blank\" href=\"https:\/\/commons.wikimedia.org\/wiki\/File:Hydrogen-fluoride-elpot-transparent-3D-balls.png\">https:\/\/commons.wikimedia.org\/wiki\/File:Hydrogen-fluoride-elpot-transparent-3D-balls.png<\/a>. <strong>License<\/strong>: <em><a target=\"_blank\" rel=\"license\" href=\"https:\/\/creativecommons.org\/about\/pdm\">Public Domain: No Known Copyright<\/a><\/em><\/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":17,"menu_order":13,"template":"","meta":{"_candela_citation":"[{\"type\":\"cc\",\"description\":\"Chemistry Concepts Intermediate\",\"author\":\"Calbreath, Baxter, et al.\",\"organization\":\"CK12.org\",\"url\":\"http:\/\/www.ck12.org\/book\/CK-12-Chemistry-Concepts-Intermediate\/\",\"project\":\"\",\"license\":\"cc-by-nc\",\"license_terms\":\"\"},{\"type\":\"cc\",\"description\":\"waterstreet coffee bar\",\"author\":\"\",\"organization\":\"Startup Stock Photos\",\"url\":\"http:\/\/startupstockphotos.com\/post\/94180886521\/waterstreet-coffee-bar-on-location-for-a\",\"project\":\"\",\"license\":\"cc0\",\"license_terms\":\"\"},{\"type\":\"pd\",\"description\":\"Hydrogen fluoride\",\"author\":\"Ben Mills\",\"organization\":\"\",\"url\":\"https:\/\/commons.wikimedia.org\/wiki\/File:Hydrogen-fluoride-elpot-transparent-3D-balls.png\",\"project\":\"\",\"license\":\"pd\",\"license_terms\":\"\"}]","CANDELA_OUTCOMES_GUID":"","pb_show_title":"on","pb_short_title":"","pb_subtitle":"","pb_authors":[],"pb_section_license":""},"chapter-type":[],"contributor":[],"license":[],"class_list":["post-3068","chapter","type-chapter","status-publish","hentry"],"part":2330,"_links":{"self":[{"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/pressbooks\/v2\/chapters\/3068","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/pressbooks\/v2\/chapters"}],"about":[{"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/wp\/v2\/types\/chapter"}],"author":[{"embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/wp\/v2\/users\/17"}],"version-history":[{"count":5,"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/pressbooks\/v2\/chapters\/3068\/revisions"}],"predecessor-version":[{"id":3302,"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/pressbooks\/v2\/chapters\/3068\/revisions\/3302"}],"part":[{"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/pressbooks\/v2\/parts\/2330"}],"metadata":[{"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/pressbooks\/v2\/chapters\/3068\/metadata\/"}],"wp:attachment":[{"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/wp\/v2\/media?parent=3068"}],"wp:term":[{"taxonomy":"chapter-type","embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/pressbooks\/v2\/chapter-type?post=3068"},{"taxonomy":"contributor","embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/wp\/v2\/contributor?post=3068"},{"taxonomy":"license","embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/wp\/v2\/license?post=3068"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}