{"id":466,"date":"2018-03-20T14:32:33","date_gmt":"2018-03-20T14:32:33","guid":{"rendered":"https:\/\/courses.lumenlearning.com\/suny-orgbiochemistry\/?post_type=chapter&#038;p=466"},"modified":"2018-09-06T15:04:53","modified_gmt":"2018-09-06T15:04:53","slug":"4-1-covalent-bonds","status":"publish","type":"chapter","link":"https:\/\/courses.lumenlearning.com\/suny-monroecc-orgbiochemistry\/chapter\/4-1-covalent-bonds\/","title":{"raw":"4.1 Covalent Bonds","rendered":"4.1 Covalent Bonds"},"content":{"raw":"<div id=\"book-content\">\r\n<div id=\"gob-ch04_s01\" class=\"section\" xml:lang=\"en\">\r\n<div id=\"gob-ch04_s01_n01\" class=\"learning_objectives editable block\">\r\n<div class=\"textbox learning-objectives\">\r\n<h3 class=\"title\">Learning Objective<\/h3>\r\n<ul>\r\n \t<li class=\"title\">Describe how a covalent bond forms.<\/li>\r\n<\/ul>\r\n<\/div>\r\n<span style=\"font-size: 1rem;text-align: initial\">You have already seen examples of substances that contain covalent bonds. One substance mentioned in <\/span><a class=\"xref\" style=\"font-size: 1rem;text-align: initial\" href=\"gob-ch03#gob-ch03\">Chapter 3 \"Ionic Bonding and Simple Ionic Compounds\"<\/a><span style=\"font-size: 1rem;text-align: initial\"> was water (H<\/span><sub class=\"subscript\" style=\"text-align: initial\">2<\/sub><span style=\"font-size: 1rem;text-align: initial\">O). You can tell from its formula that it is not an ionic compound; it is not composed of a metal and a nonmetal. Consequently, its properties are different from those of ionic compounds.<\/span>\r\n\r\n<\/div>\r\n<div id=\"gob-ch04_s01_s01\" class=\"section\">\r\n<h2 class=\"title editable block\">Electron Sharing<\/h2>\r\n<p id=\"gob-ch04_s01_s01_p01\" class=\"para editable block\"><a class=\"xref\" href=\"..\/suny-orgbiochemistry\/chapter\/introduction-3\">Chapter 3 \"Ionic Bonding and Simple Ionic Compounds\"<\/a> described how electrons can be transferred from one atom to another so that both atoms have an energy-stable outer electron shell. Because most filled electron shells have eight electrons in them, chemists called this tendency the octet rule. But there is another way an atom can achieve a full valence shell: atoms can <em class=\"emphasis\">share<\/em> electrons.<\/p>\r\n<p id=\"gob-ch04_s01_s01_p02\" class=\"para editable block\">This concept can be illustrated by using two hydrogen atoms, each of which has a single electron in its valence shell. (For small atoms such as hydrogen atoms, the valence shell will be the first shell, which holds only two electrons.) We can represent the two individual hydrogen atoms as follows:<\/p>\r\n\r\n<div class=\"informalfigure large medium-height block\"><img class=\"aligncenter\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/3101\/2018\/03\/20143026\/53859a050fd8ae291d44ea991720c00f.jpg\" alt=\"image\" \/><\/div>\r\n<p id=\"gob-ch04_s01_s01_p03\" class=\"para editable block\">In contrast, when two hydrogen atoms get close enough together to share their electrons, they can be represented as follows:<\/p>\r\n\r\n<div class=\"informalfigure large medium-height block\"><img class=\"aligncenter\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/3101\/2018\/03\/20143028\/8af74d0a50a40384b12e41497db77e77.jpg\" alt=\"image\" \/><\/div>\r\n<p id=\"gob-ch04_s01_s01_p04\" class=\"para editable block\">By sharing their valence electrons, both hydrogen atoms now have two electrons in their respective valence shells. Because each valence shell is now filled, this arrangement is more stable than when the two atoms are separate. The sharing of electrons between atoms is called a <span class=\"margin_term\"><strong><span class=\"glossterm\">covalent bond<\/span><\/strong><\/span>, and the two electrons that join atoms in a covalent bond are called a <span class=\"margin_term\"><strong><span class=\"glossterm\">bonding pair of electrons<\/span><\/strong><span class=\"glossterm\">.<\/span><\/span>\u00a0A discrete group of atoms connected by covalent bonds is called a <strong><span class=\"margin_term\"><span class=\"glossterm\">molecule<\/span><\/span><\/strong>\u2014the smallest part of a compound that retains the chemical identity of that compound.<\/p>\r\n<p id=\"gob-ch04_s01_s01_p05\" class=\"para editable block\">Chemists frequently use Lewis diagrams to represent covalent bonding in molecular substances. For example, the Lewis diagrams of two separate hydrogen atoms are as follows:<\/p>\r\n\r\n<div class=\"informalfigure large block\"><img class=\"aligncenter\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/3101\/2018\/03\/20143030\/ec5f47749bfa8fdb4ff15ad9b5ebf4db.jpg\" alt=\"image\" \/><\/div>\r\n<p id=\"gob-ch04_s01_s01_p06\" class=\"para editable block\">The Lewis diagram of two hydrogen atoms sharing electrons looks like this:<\/p>\r\n\r\n<div class=\"informalfigure large block\"><img class=\"aligncenter\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/3101\/2018\/03\/20143032\/401c52580cf1eb2f5454ad945c3682d9.jpg\" alt=\"image\" \/><\/div>\r\n<p id=\"gob-ch04_s01_s01_p07\" class=\"para editable block\">This depiction of molecules is simplified further by using a dash to represent a covalent bond. The hydrogen molecule is then represented as follows:<\/p>\r\n\r\n<div class=\"informalfigure large block\"><img class=\"aligncenter\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/3101\/2018\/03\/20143034\/36a110d6a2b14077de9c9c92abba221b.jpg\" alt=\"image\" \/><\/div>\r\n<p id=\"gob-ch04_s01_s01_p08\" class=\"para editable block\">Remember that the dash, also referred to as a <strong><span class=\"margin_term\"><span class=\"glossterm\">single bond<\/span><\/span><\/strong>, represents a <em class=\"emphasis\">pair<\/em> of electrons.<\/p>\r\n<p id=\"gob-ch04_s01_s01_p09\" class=\"para editable block\">The bond in a hydrogen molecule, measured as the distance between the two nuclei, is about 7.4 \u00d7 10<sup class=\"superscript\">\u221211<\/sup> m, or 74 picometers (pm; 1 pm = 1 \u00d7 10<sup class=\"superscript\">\u221212<\/sup> m). This particular <strong><span class=\"margin_term\"><span class=\"glossterm\">bond length<\/span><\/span><\/strong>\u00a0represents a balance between several forces: the attractions between oppositely charged electrons and nuclei, the repulsion between two negatively charged electrons, and the repulsion between two positively charged nuclei. If the nuclei were closer together, they would repel each other more strongly; if the nuclei were farther apart, there would be less attraction between the positive and negative particles.<\/p>\r\n<p id=\"gob-ch04_s01_s01_p10\" class=\"para editable block\">Fluorine is another element whose atoms bond together in pairs to form <em class=\"emphasis\">diatomic<\/em> (two-atom) molecules. Two separate fluorine atoms have the following electron dot diagrams:<\/p>\r\n\r\n<div class=\"informalfigure large block\"><img class=\"aligncenter\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/3101\/2018\/03\/20143036\/f676dbe0c37ec2ca9f34ff93967dc5cb.jpg\" alt=\"image\" \/><\/div>\r\n<p id=\"gob-ch04_s01_s01_p11\" class=\"para editable block\">Each fluorine atom contributes one valence electron, making a single bond and giving each atom a complete valence shell, which fulfills the octet rule:<\/p>\r\n\r\n<div class=\"informalfigure large block\"><img class=\"aligncenter\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/3101\/2018\/03\/20143038\/2c959bbfad372b34620eda65aec99986.jpg\" alt=\"image\" \/><\/div>\r\n<p id=\"gob-ch04_s01_s01_p12\" class=\"para editable block\">The circles show that each fluorine atom has eight electrons around it. As with hydrogen, we can represent the fluorine molecule with a dash in place of the bonding electrons:<\/p>\r\n\r\n<div class=\"informalfigure large block\"><img class=\"aligncenter\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/3101\/2018\/03\/20143040\/15d1db7579f69915a8a3a024fe2de826.jpg\" alt=\"image\" \/><\/div>\r\n<p id=\"gob-ch04_s01_s01_p13\" class=\"para editable block\">Each fluorine atom has six electrons, or three pairs of electrons, that are not participating in the covalent bond. Rather than being shared, they are considered to belong to a single atom. These are called <strong><span class=\"margin_term\"><span class=\"glossterm\">nonbonding pairs (or lone pairs)<\/span><\/span><\/strong>\u00a0of electrons.<\/p>\r\n\r\n<\/div>\r\n<div id=\"gob-ch04_s01_s02\" class=\"section\">\r\n<h2 class=\"title editable block\">Covalent Bonds between Different Atoms<\/h2>\r\n<p id=\"gob-ch04_s01_s02_p01\" class=\"para editable block\">Now that we have looked at electron sharing between atoms of the same element, let us look at covalent bond formation between atoms of different elements. Consider a molecule composed of one hydrogen atom and one fluorine atom:<\/p>\r\n\r\n<div class=\"informalfigure large block\"><img class=\"aligncenter\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/3101\/2018\/03\/20143042\/ad18f007334f4dbe0631add49d10a3b3.jpg\" alt=\"image\" \/><\/div>\r\n<p id=\"gob-ch04_s01_s02_p02\" class=\"para editable block\">Each atom needs one additional electron to complete its valence shell. By each contributing one electron, they make the following molecule:<\/p>\r\n\r\n<div class=\"informalfigure large block\"><img class=\"aligncenter\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/3101\/2018\/03\/20143044\/6a2525cedd105614a96c0c655e1b851a.jpg\" alt=\"image\" \/><\/div>\r\n<p id=\"gob-ch04_s01_s02_p03\" class=\"para editable block\">In this molecule, the hydrogen atom does not have nonbonding electrons, while the fluorine atom has six nonbonding electrons (three lone electron pairs). The circles show how the valence electron shells are filled for both atoms.<\/p>\r\n\r\n<div id=\"gob-ch04_s01_s02_n01\" class=\"exercises editable block\">\r\n<h3 class=\"title\">Example 1<\/h3>\r\n<p id=\"gob-ch04_s01_s02_p04\" class=\"para\">Draw the Lewis diagram for each compound.<\/p>\r\n\r\n<ol id=\"gob-ch04_s01_s02_l01\" class=\"orderedlist\">\r\n \t<li>a molecule composed of two chlorine atoms<\/li>\r\n \t<li>a molecule composed of a hydrogen atom and a bromine atom<\/li>\r\n<\/ol>\r\n<p class=\"simpara\">Solution<\/p>\r\n[reveal-answer q=\"228092\"]Show Answer[\/reveal-answer]\r\n[hidden-answer a=\"228092\"]\r\n<ol>\r\n \t<li>Chlorine has the same valence shell electron configuration as fluorine, so the Lewis diagram for a molecule composed of two chlorine atoms is similar to the one for fluorine:<img class=\"aligncenter\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/3101\/2018\/03\/20143046\/eed7b08d19c1da1224af51bcbc452bec.jpg\" alt=\"image\" \/><\/li>\r\n \t<li>Bromine has the same valence shell electron configuration as fluorine, so the Lewis diagram for a molecule composed of a hydrogen atom and a bromine atom is similar to that for hydrogen and fluorine:<img class=\"aligncenter\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/3101\/2018\/03\/20143048\/7da9829527d58f51bf5d2a09804637a8.jpg\" alt=\"image\" \/>[\/hidden-answer]<\/li>\r\n<\/ol>\r\n<\/div>\r\n<div id=\"gob-ch04_s01_qs01\" class=\"qandaset block\">\r\n<div class=\"textbox exercises\">\r\n<h3>Skill-Building Exercise<\/h3>\r\nDraw the Lewis diagram for each compound.\r\n<ol id=\"gob-ch04_s01_qs01_qd01\" class=\"qandadiv\">\r\n \t<li id=\"gob-ch04_s01_qs01_qd01_qa01\" class=\"qandaentry\">\r\n<div class=\"question\">\r\n<p id=\"gob-ch04_s01_qs01_p02\" class=\"para\">a molecule composed of one chlorine atom and one fluorine atom<\/p>\r\n\r\n<\/div><\/li>\r\n \t<li id=\"gob-ch04_s01_qs01_qd01_qa02\" class=\"qandaentry\">\r\n<div class=\"question\">\r\n<p class=\"para\">a molecule composed of one hydrogen atom and one iodine atom<span style=\"font-size: 1rem;text-align: initial;background-color: #ffffff\">\u00a0<\/span><\/p>\r\n\r\n<\/div><\/li>\r\n<\/ol>\r\n<\/div>\r\n<p class=\"title\">Larger molecules are constructed in a similar fashion, with some atoms participating in more than one covalent bond. For example, water, with two hydrogen atoms and one oxygen atom, and methane (CH<sub class=\"subscript\" style=\"font-weight: normal;text-align: initial;color: #373d3f\">4<\/sub><span style=\"font-size: 1rem;font-weight: normal;text-align: initial;color: #373d3f\">), with one carbon atom and four hydrogen atoms, can be represented as follows:<\/span><\/p>\r\n\r\n<\/div>\r\n<div class=\"informalfigure large block\"><img class=\"aligncenter\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/3101\/2018\/03\/20143050\/6943594c038dd3a2da09bb899ed7bd7e.jpg\" alt=\"image\" \/><\/div>\r\n<p id=\"gob-ch04_s01_s02_p09\" class=\"para editable block\">Atoms typically form a characteristic number of covalent bonds in compounds. Often the number of bonds is the same as the number of electrons short of an octet.<\/p>\r\n\r\n<div id=\"gob-ch04_s01_s02_f01\" class=\"figure large editable block\"><\/div>\r\n<div id=\"gob-ch04_s01_qs02\" class=\"qandaset block\">\r\n<div class=\"textbox exercises\">\r\n<h3 class=\"title\">Concept Review Exercises<\/h3>\r\n<div class=\"question\">\r\n<ol>\r\n \t<li id=\"gob-ch04_s01_qs02_p01\" class=\"para\">How is a covalent bond formed between two atoms?<\/li>\r\n \t<li class=\"para\">How does covalent bonding allow atoms in group 16 to satisfy the octet rule?<\/li>\r\n<\/ol>\r\n<\/div>\r\n<div class=\"question\">\r\n<h3>Answers<\/h3>\r\n[reveal-answer q=\"355164\"]Show Answer[\/reveal-answer]\r\n[hidden-answer a=\"355164\"]\r\n<ol>\r\n \t<li>Covalent bonds are formed by two atoms sharing electrons.<\/li>\r\n \t<li>The atoms in group 16 make two covalent bonds.[\/hidden-answer]<\/li>\r\n<\/ol>\r\n&nbsp;\r\n\r\n<\/div>\r\n<\/div>\r\n<\/div>\r\n<div id=\"gob-ch04_s01_s02_n04\" class=\"key_takeaways editable block\">\r\n<div class=\"textbox key-takeaways\">\r\n<div id=\"gob-ch04_s01_s02_n04\" class=\"key_takeaways editable block\">\r\n<h3 class=\"title\">Key Takeaway<\/h3>\r\n<ul id=\"gob-ch04_s01_s02_l05\" class=\"itemizedlist\">\r\n \t<li>A covalent bond is formed between two atoms by sharing electrons.<\/li>\r\n<\/ul>\r\n<\/div>\r\n<\/div>\r\n<div class=\"textbox exercises\">\r\n<div id=\"gob-ch04_s01_s02_n04\" class=\"key_takeaways editable block\">\r\n<h3 class=\"title\">Exercises<\/h3>\r\n<\/div>\r\n<div id=\"gob-ch04_s01_qs03\" class=\"qandaset block\">\r\n<ol id=\"gob-ch04_s01_qs03_qd01\" class=\"qandadiv\">\r\n \t<li id=\"gob-ch04_s01_qs03_qd01_qa01\" class=\"qandaentry\">\r\n<div class=\"question\">\r\n<p id=\"gob-ch04_s01_qs03_p01\" class=\"para\">Define <em class=\"emphasis\">covalent bond<\/em>.<\/p>\r\n\r\n<\/div><\/li>\r\n \t<li id=\"gob-ch04_s01_qs03_qd01_qa02\" class=\"qandaentry\">\r\n<div class=\"question\">\r\n<p id=\"gob-ch04_s01_qs03_p03\" class=\"para\">What is electron sharing?<\/p>\r\n\r\n<\/div><\/li>\r\n \t<li id=\"gob-ch04_s01_qs03_qd01_qa03\" class=\"qandaentry\">\r\n<div class=\"question\">\r\n<p id=\"gob-ch04_s01_qs03_p05\" class=\"para\">Draw the Lewis diagram for the covalent bond in the Br<sub class=\"subscript\">2<\/sub> molecule.<\/p>\r\n\r\n<\/div><\/li>\r\n \t<li id=\"gob-ch04_s01_qs03_qd01_qa04\" class=\"qandaentry\">\r\n<div class=\"question\">\r\n<p id=\"gob-ch04_s01_qs03_p06\" class=\"para\">Draw the Lewis diagram for the covalent bond in the I<sub class=\"subscript\">2<\/sub> molecule.<\/p>\r\n\r\n<\/div><\/li>\r\n \t<li id=\"gob-ch04_s01_qs03_qd01_qa05\" class=\"qandaentry\">\r\n<div class=\"question\">\r\n<p id=\"gob-ch04_s01_qs03_p07\" class=\"para\">Draw the Lewis diagram for the covalent bond in the HCl molecule.<\/p>\r\n\r\n<\/div><\/li>\r\n \t<li id=\"gob-ch04_s01_qs03_qd01_qa06\" class=\"qandaentry\">\r\n<div class=\"question\">\r\n<p id=\"gob-ch04_s01_qs03_p08\" class=\"para\">Draw the Lewis diagram for the covalent bond in the HI molecule.<\/p>\r\n\r\n<\/div><\/li>\r\n \t<li id=\"gob-ch04_s01_qs03_qd01_qa07\" class=\"qandaentry\">\r\n<div class=\"question\">\r\n<p id=\"gob-ch04_s01_qs03_p09\" class=\"para\">What is the difference between a molecule and a formula unit?<\/p>\r\n\r\n<\/div><\/li>\r\n \t<li id=\"gob-ch04_s01_qs03_qd01_qa08\" class=\"qandaentry\">\r\n<div class=\"question\">\r\n<p id=\"gob-ch04_s01_qs03_p11\" class=\"para\">Why do hydrogen atoms not follow the octet rule when they form covalent bonds?<\/p>\r\n\r\n<\/div><\/li>\r\n \t<li id=\"gob-ch04_s01_qs03_qd01_qa09\" class=\"qandaentry\">\r\n<div class=\"question\">\r\n<p id=\"gob-ch04_s01_qs03_p13\" class=\"para\">Draw the Lewis diagram for the covalent bonding in H<sub class=\"subscript\">2<\/sub>S. How many bonding electrons and nonbonding electrons are in the molecule?<\/p>\r\n\r\n<\/div><\/li>\r\n \t<li id=\"gob-ch04_s01_qs03_qd01_qa10\" class=\"qandaentry\">\r\n<div class=\"question\">\r\n<p id=\"gob-ch04_s01_qs03_p15\" class=\"para\">Draw the Lewis diagram for the covalent bonding in NI<sub class=\"subscript\">3<\/sub>. How many bonding electrons and nonbonding electrons are in the molecule?<\/p>\r\n\r\n<\/div><\/li>\r\n \t<li id=\"gob-ch04_s01_qs03_qd01_qa11\" class=\"qandaentry\">\r\n<div class=\"question\">\r\n<p id=\"gob-ch04_s01_qs03_p17\" class=\"para\">Draw the Lewis diagram for the covalent bonding in CF<sub class=\"subscript\">4<\/sub>. How many bonding electrons and nonbonding electrons are in the molecule?<\/p>\r\n\r\n<\/div><\/li>\r\n \t<li id=\"gob-ch04_s01_qs03_qd01_qa12\" class=\"qandaentry\">\r\n<div class=\"question\">\r\n<p id=\"gob-ch04_s01_qs03_p19\" class=\"para\">Draw the Lewis diagram for the covalent bonding in PCl<sub class=\"subscript\">3<\/sub>. How many bonding electrons and nonbonding electrons are in the molecule?<\/p>\r\n\r\n<\/div><\/li>\r\n \t<li id=\"gob-ch04_s01_qs03_qd01_qa13\" class=\"qandaentry\">\r\n<div class=\"question\">\r\n<p id=\"gob-ch04_s01_qs03_p21\" class=\"para\">How many covalent bonds does a hydrogen atom typically form? Why?<\/p>\r\n\r\n<\/div><\/li>\r\n \t<li id=\"gob-ch04_s01_qs03_qd01_qa14\" class=\"qandaentry\">\r\n<div class=\"question\">\r\n<p id=\"gob-ch04_s01_qs03_p23\" class=\"para\">How many covalent bonds does an oxygen atom typically form? Why?<\/p>\r\n\r\n<\/div><\/li>\r\n<\/ol>\r\n<\/div>\r\n<\/div>\r\n<div class=\"textbox exercises\">\r\n<div id=\"book-content\">\r\n<div id=\"gob-ch04_s01\" class=\"section\" xml:lang=\"en\">\r\n<div id=\"gob-ch04_s01_s02\" class=\"section\">\r\n<div id=\"gob-ch04_s01_s02_n04\" class=\"key_takeaways editable block\">\r\n<h3 class=\"title\">Answers<\/h3>\r\n[reveal-answer q=\"280760\"]Show Answer[\/reveal-answer]\r\n[hidden-answer a=\"280760\"]\r\n\r\n1. A covalent bond is formed when two atoms share electrons.\r\n\r\n3.\u00a0 \u00a0<img class=\"aligncenter\" style=\"font-size: 0.9em\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/3101\/2018\/03\/20143054\/11e792b5e5ae5392d8e8ef9cfa01a65f.jpg\" alt=\"image\" \/>\r\n\r\n5.\u00a0 \u00a0<img class=\"aligncenter\" style=\"font-size: 0.9em\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/3101\/2018\/03\/20143055\/c9813bfc8791306efe5c8f057cfee159.jpg\" alt=\"image\" \/>\r\n\r\n7. A molecule is a discrete combination of atoms; a formula unit is the lowest ratio of ions in a crystal.\r\n\r\n9.\u00a0 \u00a0\u00a0<img class=\"aligncenter\" style=\"font-size: 0.9em\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/3101\/2018\/03\/20143057\/5fe557d9da4fdda4eeacadcc7b1ea637.jpg\" alt=\"image\" \/>\r\n\r\nbonding electrons: 4; nonbonding electrons: 4\r\n\r\n11.\u00a0 \u00a0 \u00a0\u00a0<img class=\"aligncenter\" style=\"font-size: 0.9em\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/3101\/2018\/03\/20143058\/4eca5d32adae81361b7ce0bdc4ddc51d.jpg\" alt=\"image\" \/>\r\n\r\nbonding electrons: 8; nonbonding electrons: 24\r\n\r\n13. Hydrogen atoms form only one covalent bond because they have only one valence electron to pair.\r\n\r\n[\/hidden-answer]<span style=\"font-size: 0.9em\">\u00a0<\/span>\r\n\r\n<\/div>\r\n<\/div>\r\n<\/div>\r\n<\/div>\r\n<\/div>\r\n&nbsp;\r\n\r\n<\/div>\r\n<\/div>\r\n<\/div>\r\n<\/div>","rendered":"<div id=\"book-content\">\n<div id=\"gob-ch04_s01\" class=\"section\" xml:lang=\"en\">\n<div id=\"gob-ch04_s01_n01\" class=\"learning_objectives editable block\">\n<div class=\"textbox learning-objectives\">\n<h3 class=\"title\">Learning Objective<\/h3>\n<ul>\n<li class=\"title\">Describe how a covalent bond forms.<\/li>\n<\/ul>\n<\/div>\n<p><span style=\"font-size: 1rem;text-align: initial\">You have already seen examples of substances that contain covalent bonds. One substance mentioned in <\/span><a class=\"xref\" style=\"font-size: 1rem;text-align: initial\" href=\"gob-ch03#gob-ch03\">Chapter 3 &#8220;Ionic Bonding and Simple Ionic Compounds&#8221;<\/a><span style=\"font-size: 1rem;text-align: initial\"> was water (H<\/span><sub class=\"subscript\" style=\"text-align: initial\">2<\/sub><span style=\"font-size: 1rem;text-align: initial\">O). You can tell from its formula that it is not an ionic compound; it is not composed of a metal and a nonmetal. Consequently, its properties are different from those of ionic compounds.<\/span><\/p>\n<\/div>\n<div id=\"gob-ch04_s01_s01\" class=\"section\">\n<h2 class=\"title editable block\">Electron Sharing<\/h2>\n<p id=\"gob-ch04_s01_s01_p01\" class=\"para editable block\"><a class=\"xref\" href=\"..\/suny-orgbiochemistry\/chapter\/introduction-3\">Chapter 3 &#8220;Ionic Bonding and Simple Ionic Compounds&#8221;<\/a> described how electrons can be transferred from one atom to another so that both atoms have an energy-stable outer electron shell. Because most filled electron shells have eight electrons in them, chemists called this tendency the octet rule. But there is another way an atom can achieve a full valence shell: atoms can <em class=\"emphasis\">share<\/em> electrons.<\/p>\n<p id=\"gob-ch04_s01_s01_p02\" class=\"para editable block\">This concept can be illustrated by using two hydrogen atoms, each of which has a single electron in its valence shell. (For small atoms such as hydrogen atoms, the valence shell will be the first shell, which holds only two electrons.) We can represent the two individual hydrogen atoms as follows:<\/p>\n<div class=\"informalfigure large medium-height block\"><img decoding=\"async\" class=\"aligncenter\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/3101\/2018\/03\/20143026\/53859a050fd8ae291d44ea991720c00f.jpg\" alt=\"image\" \/><\/div>\n<p id=\"gob-ch04_s01_s01_p03\" class=\"para editable block\">In contrast, when two hydrogen atoms get close enough together to share their electrons, they can be represented as follows:<\/p>\n<div class=\"informalfigure large medium-height block\"><img decoding=\"async\" class=\"aligncenter\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/3101\/2018\/03\/20143028\/8af74d0a50a40384b12e41497db77e77.jpg\" alt=\"image\" \/><\/div>\n<p id=\"gob-ch04_s01_s01_p04\" class=\"para editable block\">By sharing their valence electrons, both hydrogen atoms now have two electrons in their respective valence shells. Because each valence shell is now filled, this arrangement is more stable than when the two atoms are separate. The sharing of electrons between atoms is called a <span class=\"margin_term\"><strong><span class=\"glossterm\">covalent bond<\/span><\/strong><\/span>, and the two electrons that join atoms in a covalent bond are called a <span class=\"margin_term\"><strong><span class=\"glossterm\">bonding pair of electrons<\/span><\/strong><span class=\"glossterm\">.<\/span><\/span>\u00a0A discrete group of atoms connected by covalent bonds is called a <strong><span class=\"margin_term\"><span class=\"glossterm\">molecule<\/span><\/span><\/strong>\u2014the smallest part of a compound that retains the chemical identity of that compound.<\/p>\n<p id=\"gob-ch04_s01_s01_p05\" class=\"para editable block\">Chemists frequently use Lewis diagrams to represent covalent bonding in molecular substances. For example, the Lewis diagrams of two separate hydrogen atoms are as follows:<\/p>\n<div class=\"informalfigure large block\"><img decoding=\"async\" class=\"aligncenter\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/3101\/2018\/03\/20143030\/ec5f47749bfa8fdb4ff15ad9b5ebf4db.jpg\" alt=\"image\" \/><\/div>\n<p id=\"gob-ch04_s01_s01_p06\" class=\"para editable block\">The Lewis diagram of two hydrogen atoms sharing electrons looks like this:<\/p>\n<div class=\"informalfigure large block\"><img decoding=\"async\" class=\"aligncenter\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/3101\/2018\/03\/20143032\/401c52580cf1eb2f5454ad945c3682d9.jpg\" alt=\"image\" \/><\/div>\n<p id=\"gob-ch04_s01_s01_p07\" class=\"para editable block\">This depiction of molecules is simplified further by using a dash to represent a covalent bond. The hydrogen molecule is then represented as follows:<\/p>\n<div class=\"informalfigure large block\"><img decoding=\"async\" class=\"aligncenter\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/3101\/2018\/03\/20143034\/36a110d6a2b14077de9c9c92abba221b.jpg\" alt=\"image\" \/><\/div>\n<p id=\"gob-ch04_s01_s01_p08\" class=\"para editable block\">Remember that the dash, also referred to as a <strong><span class=\"margin_term\"><span class=\"glossterm\">single bond<\/span><\/span><\/strong>, represents a <em class=\"emphasis\">pair<\/em> of electrons.<\/p>\n<p id=\"gob-ch04_s01_s01_p09\" class=\"para editable block\">The bond in a hydrogen molecule, measured as the distance between the two nuclei, is about 7.4 \u00d7 10<sup class=\"superscript\">\u221211<\/sup> m, or 74 picometers (pm; 1 pm = 1 \u00d7 10<sup class=\"superscript\">\u221212<\/sup> m). This particular <strong><span class=\"margin_term\"><span class=\"glossterm\">bond length<\/span><\/span><\/strong>\u00a0represents a balance between several forces: the attractions between oppositely charged electrons and nuclei, the repulsion between two negatively charged electrons, and the repulsion between two positively charged nuclei. If the nuclei were closer together, they would repel each other more strongly; if the nuclei were farther apart, there would be less attraction between the positive and negative particles.<\/p>\n<p id=\"gob-ch04_s01_s01_p10\" class=\"para editable block\">Fluorine is another element whose atoms bond together in pairs to form <em class=\"emphasis\">diatomic<\/em> (two-atom) molecules. Two separate fluorine atoms have the following electron dot diagrams:<\/p>\n<div class=\"informalfigure large block\"><img decoding=\"async\" class=\"aligncenter\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/3101\/2018\/03\/20143036\/f676dbe0c37ec2ca9f34ff93967dc5cb.jpg\" alt=\"image\" \/><\/div>\n<p id=\"gob-ch04_s01_s01_p11\" class=\"para editable block\">Each fluorine atom contributes one valence electron, making a single bond and giving each atom a complete valence shell, which fulfills the octet rule:<\/p>\n<div class=\"informalfigure large block\"><img decoding=\"async\" class=\"aligncenter\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/3101\/2018\/03\/20143038\/2c959bbfad372b34620eda65aec99986.jpg\" alt=\"image\" \/><\/div>\n<p id=\"gob-ch04_s01_s01_p12\" class=\"para editable block\">The circles show that each fluorine atom has eight electrons around it. As with hydrogen, we can represent the fluorine molecule with a dash in place of the bonding electrons:<\/p>\n<div class=\"informalfigure large block\"><img decoding=\"async\" class=\"aligncenter\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/3101\/2018\/03\/20143040\/15d1db7579f69915a8a3a024fe2de826.jpg\" alt=\"image\" \/><\/div>\n<p id=\"gob-ch04_s01_s01_p13\" class=\"para editable block\">Each fluorine atom has six electrons, or three pairs of electrons, that are not participating in the covalent bond. Rather than being shared, they are considered to belong to a single atom. These are called <strong><span class=\"margin_term\"><span class=\"glossterm\">nonbonding pairs (or lone pairs)<\/span><\/span><\/strong>\u00a0of electrons.<\/p>\n<\/div>\n<div id=\"gob-ch04_s01_s02\" class=\"section\">\n<h2 class=\"title editable block\">Covalent Bonds between Different Atoms<\/h2>\n<p id=\"gob-ch04_s01_s02_p01\" class=\"para editable block\">Now that we have looked at electron sharing between atoms of the same element, let us look at covalent bond formation between atoms of different elements. Consider a molecule composed of one hydrogen atom and one fluorine atom:<\/p>\n<div class=\"informalfigure large block\"><img decoding=\"async\" class=\"aligncenter\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/3101\/2018\/03\/20143042\/ad18f007334f4dbe0631add49d10a3b3.jpg\" alt=\"image\" \/><\/div>\n<p id=\"gob-ch04_s01_s02_p02\" class=\"para editable block\">Each atom needs one additional electron to complete its valence shell. By each contributing one electron, they make the following molecule:<\/p>\n<div class=\"informalfigure large block\"><img decoding=\"async\" class=\"aligncenter\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/3101\/2018\/03\/20143044\/6a2525cedd105614a96c0c655e1b851a.jpg\" alt=\"image\" \/><\/div>\n<p id=\"gob-ch04_s01_s02_p03\" class=\"para editable block\">In this molecule, the hydrogen atom does not have nonbonding electrons, while the fluorine atom has six nonbonding electrons (three lone electron pairs). The circles show how the valence electron shells are filled for both atoms.<\/p>\n<div id=\"gob-ch04_s01_s02_n01\" class=\"exercises editable block\">\n<h3 class=\"title\">Example 1<\/h3>\n<p id=\"gob-ch04_s01_s02_p04\" class=\"para\">Draw the Lewis diagram for each compound.<\/p>\n<ol id=\"gob-ch04_s01_s02_l01\" class=\"orderedlist\">\n<li>a molecule composed of two chlorine atoms<\/li>\n<li>a molecule composed of a hydrogen atom and a bromine atom<\/li>\n<\/ol>\n<p class=\"simpara\">Solution<\/p>\n<div class=\"qa-wrapper\" style=\"display: block\"><span class=\"show-answer collapsed\" style=\"cursor: pointer\" data-target=\"q228092\">Show Answer<\/span><\/p>\n<div id=\"q228092\" class=\"hidden-answer\" style=\"display: none\">\n<ol>\n<li>Chlorine has the same valence shell electron configuration as fluorine, so the Lewis diagram for a molecule composed of two chlorine atoms is similar to the one for fluorine:<img decoding=\"async\" class=\"aligncenter\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/3101\/2018\/03\/20143046\/eed7b08d19c1da1224af51bcbc452bec.jpg\" alt=\"image\" \/><\/li>\n<li>Bromine has the same valence shell electron configuration as fluorine, so the Lewis diagram for a molecule composed of a hydrogen atom and a bromine atom is similar to that for hydrogen and fluorine:<img decoding=\"async\" class=\"aligncenter\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/3101\/2018\/03\/20143048\/7da9829527d58f51bf5d2a09804637a8.jpg\" alt=\"image\" \/><\/div>\n<\/div>\n<\/li>\n<\/ol>\n<\/div>\n<div id=\"gob-ch04_s01_qs01\" class=\"qandaset block\">\n<div class=\"textbox exercises\">\n<h3>Skill-Building Exercise<\/h3>\n<p>Draw the Lewis diagram for each compound.<\/p>\n<ol id=\"gob-ch04_s01_qs01_qd01\" class=\"qandadiv\">\n<li id=\"gob-ch04_s01_qs01_qd01_qa01\" class=\"qandaentry\">\n<div class=\"question\">\n<p id=\"gob-ch04_s01_qs01_p02\" class=\"para\">a molecule composed of one chlorine atom and one fluorine atom<\/p>\n<\/div>\n<\/li>\n<li id=\"gob-ch04_s01_qs01_qd01_qa02\" class=\"qandaentry\">\n<div class=\"question\">\n<p class=\"para\">a molecule composed of one hydrogen atom and one iodine atom<span style=\"font-size: 1rem;text-align: initial;background-color: #ffffff\">\u00a0<\/span><\/p>\n<\/div>\n<\/li>\n<\/ol>\n<\/div>\n<p class=\"title\">Larger molecules are constructed in a similar fashion, with some atoms participating in more than one covalent bond. For example, water, with two hydrogen atoms and one oxygen atom, and methane (CH<sub class=\"subscript\" style=\"font-weight: normal;text-align: initial;color: #373d3f\">4<\/sub><span style=\"font-size: 1rem;font-weight: normal;text-align: initial;color: #373d3f\">), with one carbon atom and four hydrogen atoms, can be represented as follows:<\/span><\/p>\n<\/div>\n<div class=\"informalfigure large block\"><img decoding=\"async\" class=\"aligncenter\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/3101\/2018\/03\/20143050\/6943594c038dd3a2da09bb899ed7bd7e.jpg\" alt=\"image\" \/><\/div>\n<p id=\"gob-ch04_s01_s02_p09\" class=\"para editable block\">Atoms typically form a characteristic number of covalent bonds in compounds. Often the number of bonds is the same as the number of electrons short of an octet.<\/p>\n<div id=\"gob-ch04_s01_s02_f01\" class=\"figure large editable block\"><\/div>\n<div id=\"gob-ch04_s01_qs02\" class=\"qandaset block\">\n<div class=\"textbox exercises\">\n<h3 class=\"title\">Concept Review Exercises<\/h3>\n<div class=\"question\">\n<ol>\n<li id=\"gob-ch04_s01_qs02_p01\" class=\"para\">How is a covalent bond formed between two atoms?<\/li>\n<li class=\"para\">How does covalent bonding allow atoms in group 16 to satisfy the octet rule?<\/li>\n<\/ol>\n<\/div>\n<div class=\"question\">\n<h3>Answers<\/h3>\n<div class=\"qa-wrapper\" style=\"display: block\"><span class=\"show-answer collapsed\" style=\"cursor: pointer\" data-target=\"q355164\">Show Answer<\/span><\/p>\n<div id=\"q355164\" class=\"hidden-answer\" style=\"display: none\">\n<ol>\n<li>Covalent bonds are formed by two atoms sharing electrons.<\/li>\n<li>The atoms in group 16 make two covalent bonds.<\/div>\n<\/div>\n<\/li>\n<\/ol>\n<p>&nbsp;<\/p>\n<\/div>\n<\/div>\n<\/div>\n<div id=\"gob-ch04_s01_s02_n04\" class=\"key_takeaways editable block\">\n<div class=\"textbox key-takeaways\">\n<div id=\"gob-ch04_s01_s02_n04\" class=\"key_takeaways editable block\">\n<h3 class=\"title\">Key Takeaway<\/h3>\n<ul id=\"gob-ch04_s01_s02_l05\" class=\"itemizedlist\">\n<li>A covalent bond is formed between two atoms by sharing electrons.<\/li>\n<\/ul>\n<\/div>\n<\/div>\n<div class=\"textbox exercises\">\n<div id=\"gob-ch04_s01_s02_n04\" class=\"key_takeaways editable block\">\n<h3 class=\"title\">Exercises<\/h3>\n<\/div>\n<div id=\"gob-ch04_s01_qs03\" class=\"qandaset block\">\n<ol id=\"gob-ch04_s01_qs03_qd01\" class=\"qandadiv\">\n<li id=\"gob-ch04_s01_qs03_qd01_qa01\" class=\"qandaentry\">\n<div class=\"question\">\n<p id=\"gob-ch04_s01_qs03_p01\" class=\"para\">Define <em class=\"emphasis\">covalent bond<\/em>.<\/p>\n<\/div>\n<\/li>\n<li id=\"gob-ch04_s01_qs03_qd01_qa02\" class=\"qandaentry\">\n<div class=\"question\">\n<p id=\"gob-ch04_s01_qs03_p03\" class=\"para\">What is electron sharing?<\/p>\n<\/div>\n<\/li>\n<li id=\"gob-ch04_s01_qs03_qd01_qa03\" class=\"qandaentry\">\n<div class=\"question\">\n<p id=\"gob-ch04_s01_qs03_p05\" class=\"para\">Draw the Lewis diagram for the covalent bond in the Br<sub class=\"subscript\">2<\/sub> molecule.<\/p>\n<\/div>\n<\/li>\n<li id=\"gob-ch04_s01_qs03_qd01_qa04\" class=\"qandaentry\">\n<div class=\"question\">\n<p id=\"gob-ch04_s01_qs03_p06\" class=\"para\">Draw the Lewis diagram for the covalent bond in the I<sub class=\"subscript\">2<\/sub> molecule.<\/p>\n<\/div>\n<\/li>\n<li id=\"gob-ch04_s01_qs03_qd01_qa05\" class=\"qandaentry\">\n<div class=\"question\">\n<p id=\"gob-ch04_s01_qs03_p07\" class=\"para\">Draw the Lewis diagram for the covalent bond in the HCl molecule.<\/p>\n<\/div>\n<\/li>\n<li id=\"gob-ch04_s01_qs03_qd01_qa06\" class=\"qandaentry\">\n<div class=\"question\">\n<p id=\"gob-ch04_s01_qs03_p08\" class=\"para\">Draw the Lewis diagram for the covalent bond in the HI molecule.<\/p>\n<\/div>\n<\/li>\n<li id=\"gob-ch04_s01_qs03_qd01_qa07\" class=\"qandaentry\">\n<div class=\"question\">\n<p id=\"gob-ch04_s01_qs03_p09\" class=\"para\">What is the difference between a molecule and a formula unit?<\/p>\n<\/div>\n<\/li>\n<li id=\"gob-ch04_s01_qs03_qd01_qa08\" class=\"qandaentry\">\n<div class=\"question\">\n<p id=\"gob-ch04_s01_qs03_p11\" class=\"para\">Why do hydrogen atoms not follow the octet rule when they form covalent bonds?<\/p>\n<\/div>\n<\/li>\n<li id=\"gob-ch04_s01_qs03_qd01_qa09\" class=\"qandaentry\">\n<div class=\"question\">\n<p id=\"gob-ch04_s01_qs03_p13\" class=\"para\">Draw the Lewis diagram for the covalent bonding in H<sub class=\"subscript\">2<\/sub>S. How many bonding electrons and nonbonding electrons are in the molecule?<\/p>\n<\/div>\n<\/li>\n<li id=\"gob-ch04_s01_qs03_qd01_qa10\" class=\"qandaentry\">\n<div class=\"question\">\n<p id=\"gob-ch04_s01_qs03_p15\" class=\"para\">Draw the Lewis diagram for the covalent bonding in NI<sub class=\"subscript\">3<\/sub>. How many bonding electrons and nonbonding electrons are in the molecule?<\/p>\n<\/div>\n<\/li>\n<li id=\"gob-ch04_s01_qs03_qd01_qa11\" class=\"qandaentry\">\n<div class=\"question\">\n<p id=\"gob-ch04_s01_qs03_p17\" class=\"para\">Draw the Lewis diagram for the covalent bonding in CF<sub class=\"subscript\">4<\/sub>. How many bonding electrons and nonbonding electrons are in the molecule?<\/p>\n<\/div>\n<\/li>\n<li id=\"gob-ch04_s01_qs03_qd01_qa12\" class=\"qandaentry\">\n<div class=\"question\">\n<p id=\"gob-ch04_s01_qs03_p19\" class=\"para\">Draw the Lewis diagram for the covalent bonding in PCl<sub class=\"subscript\">3<\/sub>. How many bonding electrons and nonbonding electrons are in the molecule?<\/p>\n<\/div>\n<\/li>\n<li id=\"gob-ch04_s01_qs03_qd01_qa13\" class=\"qandaentry\">\n<div class=\"question\">\n<p id=\"gob-ch04_s01_qs03_p21\" class=\"para\">How many covalent bonds does a hydrogen atom typically form? Why?<\/p>\n<\/div>\n<\/li>\n<li id=\"gob-ch04_s01_qs03_qd01_qa14\" class=\"qandaentry\">\n<div class=\"question\">\n<p id=\"gob-ch04_s01_qs03_p23\" class=\"para\">How many covalent bonds does an oxygen atom typically form? Why?<\/p>\n<\/div>\n<\/li>\n<\/ol>\n<\/div>\n<\/div>\n<div class=\"textbox exercises\">\n<div id=\"book-content\">\n<div id=\"gob-ch04_s01\" class=\"section\" xml:lang=\"en\">\n<div id=\"gob-ch04_s01_s02\" class=\"section\">\n<div id=\"gob-ch04_s01_s02_n04\" class=\"key_takeaways editable block\">\n<h3 class=\"title\">Answers<\/h3>\n<div class=\"qa-wrapper\" style=\"display: block\"><span class=\"show-answer collapsed\" style=\"cursor: pointer\" data-target=\"q280760\">Show Answer<\/span><\/p>\n<div id=\"q280760\" class=\"hidden-answer\" style=\"display: none\">\n<p>1. A covalent bond is formed when two atoms share electrons.<\/p>\n<p>3.\u00a0 \u00a0<img decoding=\"async\" class=\"aligncenter\" style=\"font-size: 0.9em\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/3101\/2018\/03\/20143054\/11e792b5e5ae5392d8e8ef9cfa01a65f.jpg\" alt=\"image\" \/><\/p>\n<p>5.\u00a0 \u00a0<img decoding=\"async\" class=\"aligncenter\" style=\"font-size: 0.9em\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/3101\/2018\/03\/20143055\/c9813bfc8791306efe5c8f057cfee159.jpg\" alt=\"image\" \/><\/p>\n<p>7. A molecule is a discrete combination of atoms; a formula unit is the lowest ratio of ions in a crystal.<\/p>\n<p>9.\u00a0 \u00a0\u00a0<img decoding=\"async\" class=\"aligncenter\" style=\"font-size: 0.9em\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/3101\/2018\/03\/20143057\/5fe557d9da4fdda4eeacadcc7b1ea637.jpg\" alt=\"image\" \/><\/p>\n<p>bonding electrons: 4; nonbonding electrons: 4<\/p>\n<p>11.\u00a0 \u00a0 \u00a0\u00a0<img decoding=\"async\" class=\"aligncenter\" style=\"font-size: 0.9em\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/3101\/2018\/03\/20143058\/4eca5d32adae81361b7ce0bdc4ddc51d.jpg\" alt=\"image\" \/><\/p>\n<p>bonding electrons: 8; nonbonding electrons: 24<\/p>\n<p>13. Hydrogen atoms form only one covalent bond because they have only one valence electron to pair.<\/p>\n<\/div>\n<\/div>\n<p><span style=\"font-size: 0.9em\">\u00a0<\/span><\/p>\n<\/div>\n<\/div>\n<\/div>\n<\/div>\n<\/div>\n<p>&nbsp;<\/p>\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-466\">\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>The Basics of General, Organic, and Biological Chemistry v. 1.0. <strong>Provided by<\/strong>: Saylor Academy. <strong>Located at<\/strong>: <a target=\"_blank\" href=\"https:\/\/saylordotorg.github.io\/text_the-basics-of-general-organic-and-biological-chemistry\/\">https:\/\/saylordotorg.github.io\/text_the-basics-of-general-organic-and-biological-chemistry\/<\/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>. <strong>License Terms<\/strong>: This text was adapted by Saylor Academy under a Creative Commons Attribution-NonCommercial-ShareAlike 3.0 License without attribution as requested by the work&#039;s original creator or licensor.<\/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":44985,"menu_order":2,"template":"","meta":{"_candela_citation":"[{\"type\":\"cc\",\"description\":\"The Basics of General, Organic, and Biological Chemistry v. 1.0\",\"author\":\"\",\"organization\":\"Saylor Academy\",\"url\":\"https:\/\/saylordotorg.github.io\/text_the-basics-of-general-organic-and-biological-chemistry\/\",\"project\":\"\",\"license\":\"cc-by-nc\",\"license_terms\":\"This text was adapted by Saylor Academy under a Creative Commons Attribution-NonCommercial-ShareAlike 3.0 License without attribution as requested by the work\\'s original creator or licensor.\"}]","CANDELA_OUTCOMES_GUID":"","pb_show_title":"on","pb_short_title":"","pb_subtitle":"","pb_authors":[],"pb_section_license":""},"chapter-type":[],"contributor":[],"license":[],"class_list":["post-466","chapter","type-chapter","status-publish","hentry"],"part":257,"_links":{"self":[{"href":"https:\/\/courses.lumenlearning.com\/suny-monroecc-orgbiochemistry\/wp-json\/pressbooks\/v2\/chapters\/466","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/courses.lumenlearning.com\/suny-monroecc-orgbiochemistry\/wp-json\/pressbooks\/v2\/chapters"}],"about":[{"href":"https:\/\/courses.lumenlearning.com\/suny-monroecc-orgbiochemistry\/wp-json\/wp\/v2\/types\/chapter"}],"author":[{"embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/suny-monroecc-orgbiochemistry\/wp-json\/wp\/v2\/users\/44985"}],"version-history":[{"count":9,"href":"https:\/\/courses.lumenlearning.com\/suny-monroecc-orgbiochemistry\/wp-json\/pressbooks\/v2\/chapters\/466\/revisions"}],"predecessor-version":[{"id":3402,"href":"https:\/\/courses.lumenlearning.com\/suny-monroecc-orgbiochemistry\/wp-json\/pressbooks\/v2\/chapters\/466\/revisions\/3402"}],"part":[{"href":"https:\/\/courses.lumenlearning.com\/suny-monroecc-orgbiochemistry\/wp-json\/pressbooks\/v2\/parts\/257"}],"metadata":[{"href":"https:\/\/courses.lumenlearning.com\/suny-monroecc-orgbiochemistry\/wp-json\/pressbooks\/v2\/chapters\/466\/metadata\/"}],"wp:attachment":[{"href":"https:\/\/courses.lumenlearning.com\/suny-monroecc-orgbiochemistry\/wp-json\/wp\/v2\/media?parent=466"}],"wp:term":[{"taxonomy":"chapter-type","embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/suny-monroecc-orgbiochemistry\/wp-json\/pressbooks\/v2\/chapter-type?post=466"},{"taxonomy":"contributor","embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/suny-monroecc-orgbiochemistry\/wp-json\/wp\/v2\/contributor?post=466"},{"taxonomy":"license","embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/suny-monroecc-orgbiochemistry\/wp-json\/wp\/v2\/license?post=466"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}