{"id":3071,"date":"2016-08-26T02:39:02","date_gmt":"2016-08-26T02:39:02","guid":{"rendered":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/?post_type=chapter&#038;p=3071"},"modified":"2017-08-29T20:24:55","modified_gmt":"2017-08-29T20:24:55","slug":"hydrogen-bonding","status":"publish","type":"chapter","link":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/chapter\/hydrogen-bonding\/","title":{"raw":"Hydrogen Bonding","rendered":"Hydrogen Bonding"},"content":{"raw":"<div class=\"x-ck12-data-objectives\">\r\n<div class=\"textbox learning-objectives\">\r\n<h3>Learning Objectives<\/h3>\r\n<ul id=\"x-ck12-OGRhNTZmZDRlZTRlNTQyOGI0MmNjOGEwZGQxNGJmYzI.-mkj\">\r\n \t<li>Define hydrogen bond.<\/li>\r\n \t<li>Describe molecular structures that will participate in hydrogen bond formation.<\/li>\r\n<\/ul>\r\n<\/div>\r\n<div class=\"textbox examples\">\r\n<h3>What\u2019s the difference between these two molecules?<\/h3>\r\n<p id=\"x-ck12-ZWI4ZjM3NDRiZTcyOWY2MjZmNjk3MWI0MjcyODEwMzY.-ba8\"><span class=\"x-ck12-img-inline\"> <img class=\"aligncenter\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/53\/2014\/08\/19211537\/20140811155258638848.png\" alt=\"Structure of nitrogen gas\" width=\"260\" \/><\/span><\/p>\r\n<p id=\"x-ck12-MTM0MTQ3NjA2ZTI4MTNkMGYzOWVjYmM0ZGI2MzAyMjk.-lw5\"><span class=\"x-ck12-img-inline\"> <img class=\"aligncenter\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/53\/2014\/08\/19211539\/20140811155258714601.png\" alt=\"Structure of ammonia\" width=\"260\" \/><\/span><\/p>\r\n<p id=\"x-ck12-NGU1Y2U3YzUzNTkzNWZmNGViYjljMTk1MzQ0ZTI2N2E.-cm9\">A rough rule of thumb is that higher molecular-weight materials have higher boiling points than their lower molecular weight counterparts.\u00a0 More energy is needed to move the larger molecule from the liquid state to the vapor state.\u00a0 However, ammonia has a boiling point of -33.34\u00b0C and a molecular weight of 17 while nitrogen (molecular weight 28) has a boiling point of -195.8\u00b0C.\u00a0 The lighter ammonia molecule must have other factors that influence its physical properties.<\/p>\r\n\r\n<\/div>\r\n<\/div>\r\n<h2>Hydrogen Bonding<\/h2>\r\n<p id=\"x-ck12-MDc2MWNkMjhhYmJhZDUyMGQ1ZmI3NjA3Njk4YzU3MDM.-lry\">The attractive force between water molecules is a dipole interaction.\u00a0 The hydrogen atoms are bound to the highly electronegative oxygen atom (which also possesses two lone pair sets of electrons, making for a very polar bond.\u00a0 The partially positive hydrogen atom of one molecule is then attracted to the oxygen atom of a nearby water molecule (see <strong> Figure <\/strong> <a href=\"#x-ck12-OTgwNDUtMTM2MTg4MzA2OC04Mi03Mi0z\"> below <\/a> ).<\/p>\r\n\r\n<div id=\"x-ck12-YzE0NzNiMjNlZmFkMDlhNmFmODBkOWUyNTIyYjJiZWE.-tw7\" class=\"x-ck12-img-postcard x-ck12-nofloat\">\r\n\r\n[caption id=\"\" align=\"aligncenter\" width=\"500\"]<img id=\"x-ck12-OTgwNDUtMTM2MTg4MzA2OC04Mi03Mi0z\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/53\/2014\/08\/19211540\/20140811155258796274.png\" alt=\"A hydrogen bond between two water molecules\" width=\"500\" height=\"305\" longdesc=\"A%20hydrogen%20bond%20in%20water%20occurs%20between%20the%20hydrogen%20atom%20of%20one%20water%20molecule%20and%20the%20lone%20pair%20of%20electrons%20on%20an%20oxygen%20atom%20of%20a%20neighboring%20water%20molecule.\" \/> Figure 1. A hydrogen bond in water occurs between the hydrogen atom of one water molecule and the lone pair of electrons on an oxygen atom of a neighboring water molecule.[\/caption]\r\n\r\n&nbsp;\r\n\r\n<\/div>\r\n<p id=\"x-ck12-MTk4OGU5MmU5YjlhNjUwMzcxMGMxZjliZGUyMDg5NGQ.-dav\">A <strong> hydrogen bond <\/strong> is an intermolecular attractive force in which a hydrogen atom that is covalently bonded to a small, highly electronegative atom is attracted to a lone pair of electrons on an atom in a neighboring molecule. Hydrogen bonds are very strong compared to other dipole interactions.\u00a0 The strength of a typical hydrogen bond is about 5% of that of a covalent bond.<\/p>\r\n<p id=\"x-ck12-OWNjMDY0ZThkNjIyMWNjYzE4NTdhYzYxNDQzYTFjODc.-bsr\">Hydrogen bonding occurs only in molecules where hydrogen is covalently bonded to one of three elements: fluorine, oxygen, or nitrogen.\u00a0 These three elements are so electronegative that they withdraw the majority of the electron density in the covalent bond with hydrogen, leaving the H atom very electron-deficient.\u00a0 The H atom nearly acts as a bare proton, leaving it very attracted to lone pair electrons on a nearby atom.<\/p>\r\n<p id=\"x-ck12-NTA1Y2U3M2U4ZDJkYmNjZTQ2NDNmMGQ1YTFiZjY2YmI.-vz4\">The hydrogen bonding that occurs in water leads to some unusual, but very important properties.\u00a0 Most molecular compounds that have a mass similar to water are gases at room temperature.\u00a0 Because of the strong hydrogen bonds, water molecules are able to stay condensed in the liquid state.\u00a0 The figure<strong>\u00a0<\/strong>below shows how the bent shape and two hydrogen atoms per molecule allows each water molecule to be able to hydrogen bond to two other molecules.<\/p>\r\n\r\n<div id=\"x-ck12-YzUxZmVjYWFhMjczZWUwYTkxOTQ1OGJhMzg5NTk0NDY.-hys\" class=\"x-ck12-img-postcard x-ck12-nofloat\">\r\n\r\n[caption id=\"\" align=\"aligncenter\" width=\"500\"]<img id=\"x-ck12-OTgwNDUtMTM2MTg4MzIxMC03Ny0yMC00\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/53\/2014\/08\/19211541\/20140811155258974586.jpeg\" alt=\"Multiple hydrogen bond between water molecules\" width=\"500\" height=\"488\" longdesc=\"Multiple%20hydrogen%20bonds%20occur%20simultaneously%20in%20water%20because%20of%20its%20bent%20shape%20and%20the%20presence%20of%20two%20hydrogen%20atoms%20per%20molecule.\" \/> Figure 2. Multiple hydrogen bonds occur simultaneously in water because of its bent shape and the presence of two hydrogen atoms per molecule.[\/caption]\r\n\r\n<\/div>\r\n<p id=\"x-ck12-OTA4MDU2NGRjNTBiOTE3OWMzM2M5YmQxYTBiNjBlODg.-g4m\">In the liquid state, the hydrogen bonds of water can break and reform as the molecules flow from one place to another.\u00a0 When water is cooled, the molecules begin to slow down.\u00a0 Eventually, when water is frozen to ice, the hydrogen bonds become permanent and form a very specific network.<\/p>\r\n\r\n<div id=\"x-ck12-ZmUyNTBkMGVjMmQ1NmFlNTM4N2VmM2M5NThjMDM3M2Y.-ntm\" class=\"x-ck12-img-thumbnail x-ck12-nofloat\">\r\n\r\n[caption id=\"\" align=\"aligncenter\" width=\"192\"]<img id=\"x-ck12-OTgwNDUtMTM2MTg4MzI0OC03NS0xMDAtNQ..\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/53\/2014\/08\/19211542\/20140811155259105866.png\" alt=\"The hydrogen bonding network in ice\" width=\"192\" height=\"160\" longdesc=\"When%20water%20freezes%20to%20ice%2C%20the%20hydrogen%20bonding%20network%20becomes%20permanent.%20Each%20oxygen%20atom%20has%20an%20approximately%20tetrahedral%20geometry%20%E2%80%93%20two%20covalent%20bonds%20and%20two%20hydrogen%20bonds.\" \/> Figure 3. When water freezes to ice, the hydrogen bonding network becomes permanent. Each oxygen atom has an approximately tetrahedral geometry \u2013 two covalent bonds and two hydrogen bonds.[\/caption]\r\n\r\n&nbsp;\r\n\r\n<\/div>\r\n<p id=\"x-ck12-ZDk0ZGY5M2M4MTUzMzkzYzhjM2Y0MmUzZDRlMzA3ZDg.-lp4\">The bent shape of the molecules leads to gaps in the hydrogen bonding network of ice.\u00a0 Ice has the very unusual property that its solid state is less dense than its liquid state.\u00a0 Ice floats in liquid water.\u00a0 Virtually all other substances are denser in the solid state than in the liquid state.\u00a0 Hydrogen bonds play a very important biological role in the physical structures of proteins and nucleic acids.<\/p>\r\n\r\n<div class=\"textbox key-takeaways\">\r\n<h3>Summary<\/h3>\r\n<ul id=\"x-ck12-ZDEzZmU1M2VlZTJiM2U3MzdkODg4NjM5N2Q3OWZmZGM.-si9\">\r\n \t<li>Hydrogen bonds form when a H attached to a N, O, or F atom interacts with another N, O, or F atom.<\/li>\r\n<\/ul>\r\n<\/div>\r\n<div class=\"textbox exercises\">\r\n<h3>Practice<\/h3>\r\n<p id=\"x-ck12-Y2JlMjQ5M2YzMTNmNmRjMzNmZTI0MTMzYzcwM2IzZmY.-lei\">Use the link below to answer the following questions:<\/p>\r\n<p id=\"x-ck12-NGMzZDcxMTZlOGUyZmFhN2JlZDM1MzY3ODkyOWM2ZDg.-gav\"><a href=\"https:\/\/web.archive.org\/web\/20120522042855\/http:\/\/www.elmhurst.edu\/~chm\/vchembook\/161Ahydrogenbond.html\" target=\"_blank\" rel=\"noopener\">hydrogen bonds<\/a><\/p>\r\n\r\n<ol id=\"x-ck12-YmViZTZhM2JjNzAxOTcyYjM5ZmM2YjA1NWY4ZjFjY2U.-ral\">\r\n \t<li>What are the features of N and O that cause then to form H bonds with H?<\/li>\r\n \t<li>Will all H atoms form H-bonds?<\/li>\r\n \t<li>What is the length of an H-bond compared to the length of a covalent bond?<\/li>\r\n<\/ol>\r\n<\/div>\r\n<div class=\"textbox exercises\">\r\n<h3>Review<\/h3>\r\n<ol id=\"x-ck12-Y2EzMzg3NTVhMWZkMDZhNjU4YThiZDZhNjZmY2RmYzc.-coi\">\r\n \t<li>How strong is a hydrogen bond?<\/li>\r\n \t<li>What happens when H is covalently bonded to N, O, or F?<\/li>\r\n \t<li>How does the shape of the water molecule affect its properties?<\/li>\r\n<\/ol>\r\n<\/div>\r\n<h2 class=\"x-ck12-data-problem-set\">Glossary<\/h2>\r\n<div class=\"x-ck12-data-vocabulary\">\r\n<ul id=\"x-ck12-ZDIzZTUwNTEyNjZlNjZjZDhjZDJlMmM3MTczOTI5YmQ.-1fw\">\r\n \t<li><strong> hydrogen bond: <\/strong> An intermolecular attractive force in which a hydrogen atom that is covalently bonded to a small, highly electronegative atom is attracted to a lone pair of electrons on an atom in a neighboring molecule.<\/li>\r\n<\/ul>\r\n<\/div>\r\n[reveal-answer q=\"836080\"]Show References[\/reveal-answer]\r\n[hidden-answer a=\"836080\"]\r\n<h2>References<\/h2>\r\n<ol>\r\n \t<li>CK-12 Foundation - Joy Sheng, using 3D molecular structure by Ben Mills (Wikimedia: Benjah-bmm27). Molecular structure: <a href=\"http:\/\/commons.wikimedia.org\/wiki\/File:Nitrogen-3D-vdW.png\" target=\"_blank\" rel=\"noopener\">http:\/\/commons.wikimedia.org\/wiki\/File:Nitrogen-3D-vdW.png<\/a>.<\/li>\r\n \t<li>(Left) User:Booyabazooka\/Wikimedia Commons; (Right) Ben Mills (Wikimedia: Benjah-bmm27). (Left) <a href=\"http:\/\/commons.wikimedia.org\/wiki\/File:Ammonia_lone_electron_pair.svg\" target=\"_blank\" rel=\"noopener\">http:\/\/commons.wikimedia.org\/wiki\/File:Ammonia_lone_electron_pair.svg<\/a>; (Right) <a href=\"http:\/\/commons.wikimedia.org\/wiki\/File:Ammonia-3D-balls-A.png\" target=\"_blank\" rel=\"noopener\">http:\/\/commons.wikimedia.org\/wiki\/File:Ammonia-3D-balls-A.png<\/a>.<\/li>\r\n \t<li>Ben Mills (Wikimedia: Benjah-bmm27).<a href=\"http:\/\/commons.wikimedia.org\/wiki\/File:Hydrogen-bonding-in-water-2D.png\">http:\/\/commons.wikimedia.org\/wiki\/File:Hydrogen-bonding-in-water-2D.png <\/a>.<\/li>\r\n \t<li>Laura Guerin. CK-12 Foundation.<\/li>\r\n \t<li>User:Materialscientist\/Wikimedia Commons.<a href=\"http:\/\/commons.wikimedia.org\/wiki\/File:Hex_ice.GIF\">http:\/\/commons.wikimedia.org\/wiki\/File:Hex_ice.GIF <\/a>.<\/li>\r\n<\/ol>\r\n[\/hidden-answer]","rendered":"<div class=\"x-ck12-data-objectives\">\n<div class=\"textbox learning-objectives\">\n<h3>Learning Objectives<\/h3>\n<ul id=\"x-ck12-OGRhNTZmZDRlZTRlNTQyOGI0MmNjOGEwZGQxNGJmYzI.-mkj\">\n<li>Define hydrogen bond.<\/li>\n<li>Describe molecular structures that will participate in hydrogen bond formation.<\/li>\n<\/ul>\n<\/div>\n<div class=\"textbox examples\">\n<h3>What\u2019s the difference between these two molecules?<\/h3>\n<p id=\"x-ck12-ZWI4ZjM3NDRiZTcyOWY2MjZmNjk3MWI0MjcyODEwMzY.-ba8\"><span class=\"x-ck12-img-inline\"> <img decoding=\"async\" class=\"aligncenter\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/53\/2014\/08\/19211537\/20140811155258638848.png\" alt=\"Structure of nitrogen gas\" width=\"260\" \/><\/span><\/p>\n<p id=\"x-ck12-MTM0MTQ3NjA2ZTI4MTNkMGYzOWVjYmM0ZGI2MzAyMjk.-lw5\"><span class=\"x-ck12-img-inline\"> <img decoding=\"async\" class=\"aligncenter\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/53\/2014\/08\/19211539\/20140811155258714601.png\" alt=\"Structure of ammonia\" width=\"260\" \/><\/span><\/p>\n<p id=\"x-ck12-NGU1Y2U3YzUzNTkzNWZmNGViYjljMTk1MzQ0ZTI2N2E.-cm9\">A rough rule of thumb is that higher molecular-weight materials have higher boiling points than their lower molecular weight counterparts.\u00a0 More energy is needed to move the larger molecule from the liquid state to the vapor state.\u00a0 However, ammonia has a boiling point of -33.34\u00b0C and a molecular weight of 17 while nitrogen (molecular weight 28) has a boiling point of -195.8\u00b0C.\u00a0 The lighter ammonia molecule must have other factors that influence its physical properties.<\/p>\n<\/div>\n<\/div>\n<h2>Hydrogen Bonding<\/h2>\n<p id=\"x-ck12-MDc2MWNkMjhhYmJhZDUyMGQ1ZmI3NjA3Njk4YzU3MDM.-lry\">The attractive force between water molecules is a dipole interaction.\u00a0 The hydrogen atoms are bound to the highly electronegative oxygen atom (which also possesses two lone pair sets of electrons, making for a very polar bond.\u00a0 The partially positive hydrogen atom of one molecule is then attracted to the oxygen atom of a nearby water molecule (see <strong> Figure <\/strong> <a href=\"#x-ck12-OTgwNDUtMTM2MTg4MzA2OC04Mi03Mi0z\"> below <\/a> ).<\/p>\n<div id=\"x-ck12-YzE0NzNiMjNlZmFkMDlhNmFmODBkOWUyNTIyYjJiZWE.-tw7\" 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-OTgwNDUtMTM2MTg4MzA2OC04Mi03Mi0z\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/53\/2014\/08\/19211540\/20140811155258796274.png\" alt=\"A hydrogen bond between two water molecules\" width=\"500\" height=\"305\" longdesc=\"A%20hydrogen%20bond%20in%20water%20occurs%20between%20the%20hydrogen%20atom%20of%20one%20water%20molecule%20and%20the%20lone%20pair%20of%20electrons%20on%20an%20oxygen%20atom%20of%20a%20neighboring%20water%20molecule.\" \/><\/p>\n<p class=\"wp-caption-text\">Figure 1. A hydrogen bond in water occurs between the hydrogen atom of one water molecule and the lone pair of electrons on an oxygen atom of a neighboring water molecule.<\/p>\n<\/div>\n<p>&nbsp;<\/p>\n<\/div>\n<p id=\"x-ck12-MTk4OGU5MmU5YjlhNjUwMzcxMGMxZjliZGUyMDg5NGQ.-dav\">A <strong> hydrogen bond <\/strong> is an intermolecular attractive force in which a hydrogen atom that is covalently bonded to a small, highly electronegative atom is attracted to a lone pair of electrons on an atom in a neighboring molecule. Hydrogen bonds are very strong compared to other dipole interactions.\u00a0 The strength of a typical hydrogen bond is about 5% of that of a covalent bond.<\/p>\n<p id=\"x-ck12-OWNjMDY0ZThkNjIyMWNjYzE4NTdhYzYxNDQzYTFjODc.-bsr\">Hydrogen bonding occurs only in molecules where hydrogen is covalently bonded to one of three elements: fluorine, oxygen, or nitrogen.\u00a0 These three elements are so electronegative that they withdraw the majority of the electron density in the covalent bond with hydrogen, leaving the H atom very electron-deficient.\u00a0 The H atom nearly acts as a bare proton, leaving it very attracted to lone pair electrons on a nearby atom.<\/p>\n<p id=\"x-ck12-NTA1Y2U3M2U4ZDJkYmNjZTQ2NDNmMGQ1YTFiZjY2YmI.-vz4\">The hydrogen bonding that occurs in water leads to some unusual, but very important properties.\u00a0 Most molecular compounds that have a mass similar to water are gases at room temperature.\u00a0 Because of the strong hydrogen bonds, water molecules are able to stay condensed in the liquid state.\u00a0 The figure<strong>\u00a0<\/strong>below shows how the bent shape and two hydrogen atoms per molecule allows each water molecule to be able to hydrogen bond to two other molecules.<\/p>\n<div id=\"x-ck12-YzUxZmVjYWFhMjczZWUwYTkxOTQ1OGJhMzg5NTk0NDY.-hys\" 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-OTgwNDUtMTM2MTg4MzIxMC03Ny0yMC00\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/53\/2014\/08\/19211541\/20140811155258974586.jpeg\" alt=\"Multiple hydrogen bond between water molecules\" width=\"500\" height=\"488\" longdesc=\"Multiple%20hydrogen%20bonds%20occur%20simultaneously%20in%20water%20because%20of%20its%20bent%20shape%20and%20the%20presence%20of%20two%20hydrogen%20atoms%20per%20molecule.\" \/><\/p>\n<p class=\"wp-caption-text\">Figure 2. Multiple hydrogen bonds occur simultaneously in water because of its bent shape and the presence of two hydrogen atoms per molecule.<\/p>\n<\/div>\n<\/div>\n<p id=\"x-ck12-OTA4MDU2NGRjNTBiOTE3OWMzM2M5YmQxYTBiNjBlODg.-g4m\">In the liquid state, the hydrogen bonds of water can break and reform as the molecules flow from one place to another.\u00a0 When water is cooled, the molecules begin to slow down.\u00a0 Eventually, when water is frozen to ice, the hydrogen bonds become permanent and form a very specific network.<\/p>\n<div id=\"x-ck12-ZmUyNTBkMGVjMmQ1NmFlNTM4N2VmM2M5NThjMDM3M2Y.-ntm\" class=\"x-ck12-img-thumbnail x-ck12-nofloat\">\n<div style=\"width: 202px\" class=\"wp-caption aligncenter\"><img loading=\"lazy\" decoding=\"async\" id=\"x-ck12-OTgwNDUtMTM2MTg4MzI0OC03NS0xMDAtNQ..\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/53\/2014\/08\/19211542\/20140811155259105866.png\" alt=\"The hydrogen bonding network in ice\" width=\"192\" height=\"160\" longdesc=\"When%20water%20freezes%20to%20ice%2C%20the%20hydrogen%20bonding%20network%20becomes%20permanent.%20Each%20oxygen%20atom%20has%20an%20approximately%20tetrahedral%20geometry%20%E2%80%93%20two%20covalent%20bonds%20and%20two%20hydrogen%20bonds.\" \/><\/p>\n<p class=\"wp-caption-text\">Figure 3. When water freezes to ice, the hydrogen bonding network becomes permanent. Each oxygen atom has an approximately tetrahedral geometry \u2013 two covalent bonds and two hydrogen bonds.<\/p>\n<\/div>\n<p>&nbsp;<\/p>\n<\/div>\n<p id=\"x-ck12-ZDk0ZGY5M2M4MTUzMzkzYzhjM2Y0MmUzZDRlMzA3ZDg.-lp4\">The bent shape of the molecules leads to gaps in the hydrogen bonding network of ice.\u00a0 Ice has the very unusual property that its solid state is less dense than its liquid state.\u00a0 Ice floats in liquid water.\u00a0 Virtually all other substances are denser in the solid state than in the liquid state.\u00a0 Hydrogen bonds play a very important biological role in the physical structures of proteins and nucleic acids.<\/p>\n<div class=\"textbox key-takeaways\">\n<h3>Summary<\/h3>\n<ul id=\"x-ck12-ZDEzZmU1M2VlZTJiM2U3MzdkODg4NjM5N2Q3OWZmZGM.-si9\">\n<li>Hydrogen bonds form when a H attached to a N, O, or F atom interacts with another N, O, or F atom.<\/li>\n<\/ul>\n<\/div>\n<div class=\"textbox exercises\">\n<h3>Practice<\/h3>\n<p id=\"x-ck12-Y2JlMjQ5M2YzMTNmNmRjMzNmZTI0MTMzYzcwM2IzZmY.-lei\">Use the link below to answer the following questions:<\/p>\n<p id=\"x-ck12-NGMzZDcxMTZlOGUyZmFhN2JlZDM1MzY3ODkyOWM2ZDg.-gav\"><a href=\"https:\/\/web.archive.org\/web\/20120522042855\/http:\/\/www.elmhurst.edu\/~chm\/vchembook\/161Ahydrogenbond.html\" target=\"_blank\" rel=\"noopener\">hydrogen bonds<\/a><\/p>\n<ol id=\"x-ck12-YmViZTZhM2JjNzAxOTcyYjM5ZmM2YjA1NWY4ZjFjY2U.-ral\">\n<li>What are the features of N and O that cause then to form H bonds with H?<\/li>\n<li>Will all H atoms form H-bonds?<\/li>\n<li>What is the length of an H-bond compared to the length of a covalent bond?<\/li>\n<\/ol>\n<\/div>\n<div class=\"textbox exercises\">\n<h3>Review<\/h3>\n<ol id=\"x-ck12-Y2EzMzg3NTVhMWZkMDZhNjU4YThiZDZhNjZmY2RmYzc.-coi\">\n<li>How strong is a hydrogen bond?<\/li>\n<li>What happens when H is covalently bonded to N, O, or F?<\/li>\n<li>How does the shape of the water molecule affect its properties?<\/li>\n<\/ol>\n<\/div>\n<h2 class=\"x-ck12-data-problem-set\">Glossary<\/h2>\n<div class=\"x-ck12-data-vocabulary\">\n<ul id=\"x-ck12-ZDIzZTUwNTEyNjZlNjZjZDhjZDJlMmM3MTczOTI5YmQ.-1fw\">\n<li><strong> hydrogen bond: <\/strong> An intermolecular attractive force in which a hydrogen atom that is covalently bonded to a small, highly electronegative atom is attracted to a lone pair of electrons on an atom in a neighboring molecule.<\/li>\n<\/ul>\n<\/div>\n<div class=\"qa-wrapper\" style=\"display: block\"><span class=\"show-answer collapsed\" style=\"cursor: pointer\" data-target=\"q836080\">Show References<\/span><\/p>\n<div id=\"q836080\" class=\"hidden-answer\" style=\"display: none\">\n<h2>References<\/h2>\n<ol>\n<li>CK-12 Foundation &#8211; Joy Sheng, using 3D molecular structure by Ben Mills (Wikimedia: Benjah-bmm27). Molecular structure: <a href=\"http:\/\/commons.wikimedia.org\/wiki\/File:Nitrogen-3D-vdW.png\" target=\"_blank\" rel=\"noopener\">http:\/\/commons.wikimedia.org\/wiki\/File:Nitrogen-3D-vdW.png<\/a>.<\/li>\n<li>(Left) User:Booyabazooka\/Wikimedia Commons; (Right) Ben Mills (Wikimedia: Benjah-bmm27). (Left) <a href=\"http:\/\/commons.wikimedia.org\/wiki\/File:Ammonia_lone_electron_pair.svg\" target=\"_blank\" rel=\"noopener\">http:\/\/commons.wikimedia.org\/wiki\/File:Ammonia_lone_electron_pair.svg<\/a>; (Right) <a href=\"http:\/\/commons.wikimedia.org\/wiki\/File:Ammonia-3D-balls-A.png\" target=\"_blank\" rel=\"noopener\">http:\/\/commons.wikimedia.org\/wiki\/File:Ammonia-3D-balls-A.png<\/a>.<\/li>\n<li>Ben Mills (Wikimedia: Benjah-bmm27).<a href=\"http:\/\/commons.wikimedia.org\/wiki\/File:Hydrogen-bonding-in-water-2D.png\">http:\/\/commons.wikimedia.org\/wiki\/File:Hydrogen-bonding-in-water-2D.png <\/a>.<\/li>\n<li>Laura Guerin. CK-12 Foundation.<\/li>\n<li>User:Materialscientist\/Wikimedia Commons.<a href=\"http:\/\/commons.wikimedia.org\/wiki\/File:Hex_ice.GIF\">http:\/\/commons.wikimedia.org\/wiki\/File:Hex_ice.GIF <\/a>.<\/li>\n<\/ol>\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-3071\">\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><\/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":16,"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\":\"\"}]","CANDELA_OUTCOMES_GUID":"","pb_show_title":"on","pb_short_title":"","pb_subtitle":"","pb_authors":[],"pb_section_license":""},"chapter-type":[],"contributor":[],"license":[],"class_list":["post-3071","chapter","type-chapter","status-publish","hentry"],"part":2330,"_links":{"self":[{"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/pressbooks\/v2\/chapters\/3071","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":6,"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/pressbooks\/v2\/chapters\/3071\/revisions"}],"predecessor-version":[{"id":3664,"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/pressbooks\/v2\/chapters\/3071\/revisions\/3664"}],"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\/3071\/metadata\/"}],"wp:attachment":[{"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/wp\/v2\/media?parent=3071"}],"wp:term":[{"taxonomy":"chapter-type","embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/pressbooks\/v2\/chapter-type?post=3071"},{"taxonomy":"contributor","embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/wp\/v2\/contributor?post=3071"},{"taxonomy":"license","embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/umes-cheminter\/wp-json\/wp\/v2\/license?post=3071"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}