Chapter 4: Covalent Bonding And Simple Molecular
Chapter 4: Covalent Bonding and Simple Molecular Compounds1/7/15, 2:57 ompoundsOpening(EssayCholesterol (C27H46O), a compound that is sometimes in the news, is a white, waxy solid producedin the liver of every animal, including humans. It is important for building cell membranes and inproducing certain hormones (chemicals that regulate cellular activity in the body). As such, it isnecessary for life, but why is cholesterol the object of attention?Besides producing cholesterol, we also ingest some whenever we eat meat or other animal-basedfood products. People who eat such products in large quantities, or whose metabolisms are unableto handle excess amounts, may experience an unhealthy buildup of cholesterol in their blood.Deposits of cholesterol, called plaque, may form on blood vessel walls, eventually blocking thearteries and preventing the delivery of oxygen to body tissues. Heart attacks, strokes, and othercirculatory problems can result.Most medical professionals recommend diets that minimize the amount of ingested cholesterol as away of preventing heart attacks and strokes. Tests are available to measure cholesterol in the blood,and there are several drugs capable of lowering cholesterol levels.Figure 4.1A Molecular Model of oncepts-of-chemistry/Final- -simple-mo.htmlPage 1 of 56
Chapter 4: Covalent Bonding and Simple Molecular Compounds1/7/15, 2:57 PMChapter 3 "Ionic Bonding and Simple Ionic Compounds" discussed ionic bonding, which results fromthe transfer of electrons among atoms or groups of atoms. In this chapter, we will consider another typeof bonding—covalent bonding. We will examine how atoms share electrons to form these bonds, and wewill begin to explore how the resulting compounds, such as cholesterol, are different from E1.# Describe#how#a#covalent#bond#forms.You have already seen examples of substances that contain covalent bonds. One substance mentionedin Chapter 3 "Ionic Bonding and Simple Ionic Compounds" was water (H2O). You can tell from itsformula 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.Electron(SharingChapter 3 "Ionic Bonding and Simple Ionic Compounds" described how electrons can be transferredfrom one atom to another so that both atoms have an energy-stable outer electron shell. Because -of-chemistry/Final- -simple-mo.htmlPage 2 of 56
Chapter 4: Covalent Bonding and Simple Molecular Compounds1/7/15, 2:57 PMfilled electron shells have eight electrons in them, chemists called this tendency the octet rule. But thereis another way an atom can achieve a full valence shell: atoms can share electrons.This concept can be illustrated by using two hydrogen atoms, each of which has a single electron in itsvalence shell. (For small atoms such as hydrogen atoms, the valence shell will be the first shell, whichholds only two electrons.) We can represent the two individual hydrogen atoms as follows:In contrast, when two hydrogen atoms get close enough together to share their electrons, they can berepresented as epts-of-chemistry/Final- -simple-mo.htmlPage 3 of 56
Chapter 4: Covalent Bonding and Simple Molecular Compounds1/7/15, 2:57 PMBy sharing their valence electrons, both hydrogen atoms now have two electrons in their respectivevalence shells. Because each valence shell is now filled, this arrangement is more stable than when thetwo atoms are separate. The sharing of electrons between atoms is called a covalent bond, and thetwo electrons that join atoms in a covalent bond are called a bonding pair of electrons. A discretegroup of atoms connected by covalent bonds is called a molecule—the smallest part of a compoundthat retains the chemical identity of that compound.Chemists frequently use Lewis diagrams to represent covalent bonding in molecular substances. Forexample, the Lewis diagrams of two separate hydrogen atoms are as follows:The Lewis diagram of two hydrogen atoms sharing electrons looks like this:This depiction of molecules is simplified further by using a dash to represent a covalent bond. Thehydrogen molecule is then represented as follows:Remember that the dash, also referred to as a single bond, represents a pair of electrons.The bond in a hydrogen molecule, measured as the distance between the two nuclei, is about 7.4 10 11m, or 74 picometers (pm; 1 pm 1 10 12 m). This particular bond length represents a balancebetween several forces: the attractions between oppositely charged electrons and nuclei, the repulsionbetween two negatively charged electrons, and the repulsion between two positively charged nuclei. Ifthe nuclei were closer together, they would repel each other more strongly; if the nuclei were fartherapart, there would be less attraction between the positive and negative particles.Fluorine is another element whose atoms bond together in pairs to form diatomic (two-atom)molecules. Two separate fluorine atoms have the following electron dot cepts-of-chemistry/Final- -simple-mo.htmlPage 4 of 56
Chapter 4: Covalent Bonding and Simple Molecular Compounds1/7/15, 2:57 PMEach fluorine atom contributes one valence electron, making a single bond and giving each atom acomplete valence shell, which fulfills the octet rule:The circles show that each fluorine atom has eight electrons around it. As with hydrogen, we canrepresent the fluorine molecule with a dash in place of the bonding electrons:Each fluorine atom has six electrons, or three pairs of electrons, that are not participating in thecovalent bond. Rather than being shared, they are considered to belong to a single atom. These arecalled nonbonding pairs (or lone pairs) of ow that we have looked at electron sharing between atoms of the same element, let us look at covalentbond formation between atoms of different elements. Consider a molecule composed of one hydrogenatom and one fluorine atom:Each atom needs one additional electron to complete its valence shell. By each contributing oneelectron, they make the following cepts-of-chemistry/Final- -simple-mo.htmlPage 5 of 56
Chapter 4: Covalent Bonding and Simple Molecular Compounds1/7/15, 2:57 PMIn this molecule, the hydrogen atom does not have nonbonding electrons, while the fluorine atom hassix nonbonding electrons (three lone electron pairs). The circles show how the valence electron shellsare filled for both pound.1.# a#molecule#composed#of#two#chlorine#atoms2.# ne#atomSolu configura #shell#electron#configura ompound.1.# ��uorine#atom2.# ncepts-of-chemistry/Final- -simple-mo.htmlPage 6 of 56
Chapter 4: Covalent Bonding and Simple Molecular Compounds1/7/15, 2:57 PMLarger molecules are constructed in a similar fashion, with some atoms participating in more than onecovalent bond. For example, water, with two hydrogen atoms and one oxygen atom, and methane(CH4), with one carbon atom and four hydrogen atoms, can be represented as follows:Atoms typically form a characteristic number of covalent bonds in compounds. Figure 4.2 "How ManyCovalent Bonds Are Formed?" shows the number of covalent bonds various atoms typically form.Figure 4.2 How Many Covalent Bonds Are Formed?In molecules, there is a pattern to the number of covalent bonds that different atoms can form. Each blockwith a number indicates the number of covalent bonds formed by that atom in neutral compounds.CONCEPT(REVIEW(EXERCISES1.# # to#sa top/chemistry/concepts-of-chemistry/Final- -simple-mo.htmlPage 7 of 56
Chapter 4: Covalent Bonding and Simple Molecular Compounds1/7/15, 2:57 PM1.# ctrons.2.# The#atoms#in#group#6A#make#two#covalent#bonds.K E Y ( TA K E #sharing#electrons.EXERCISES1.# Define#covalent)bond.2.# What#is#electron#sharing?3.# e#Br2#molecule.4.# e#I2#molecule.5.# e#HCl#molecule.6.# e#HI#molecule.7.# ormula#unit?8.# en#they#form#covalent#bonds?9.# ctrons#are#in#the#molecule?10.# ctrons#are#in#the#molecule?11.# ctrons#are#in#the#molecule?12.# sktop/chemistry/concepts-of-chemistry/Final- -simple-mo.htmlPage 8 of 56
Chapter 4: Covalent Bonding and Simple Molecular Compounds1/7/15, 2:57 PM13.# ally#form?#Why?14.# lly#form?#Why?15.# gen.16.# onds#would#a# een# n#and#hydrogen.17.# Asta ne#is#a#synthe c#element,#made#one#atom#at#a# .# s#an#atom#of#this#element#would#form.ANSWERS1.# ctrons.3.#4.#7.# A#molecule#is#a#discrete#combina on#of#atoms;#a#formula#unit#is#the#lowest#ra o#of#ions#in#a#crystal.9.# stry/Final- -simple-mo.htmlPage 9 of 56
Chapter 4: Covalent Bonding and Simple Molecular Compounds1/7/15, 2:57 PM11.# bonding#electrons:#8;#nonbonding#electrons:#2413.# #they#have#only#one#valence#electron#to#pair.15.# two;#H2Te17.# ING(OBJECTIVES1.# t#compound#from#its#name.2.# rom#its#chemical#formula.What elements make covalent bonds? Covalent bonds form when two or more nonmetals combine. Forexample, both hydrogen and oxygen are nonmetals, and when they combine to make water, they do soby forming covalent bonds. Nonmetal atoms in polyatomic ions are joined by covalent bonds, but theion as a whole participates in ionic bonding. For example, ammonium chloride has ionic bonds betweena polyatomic ion, NH4 , and Cl ions, but within the ammonium ion, the nitrogen and hydrogen atomsare connected by covalent ts-of-chemistry/Final -simple-mo.htmlPage 10 of 56
Chapter 4: Covalent Bonding and Simple Molecular Compounds1/7/15, 2:57 s,#covalent#bonds,#or#both?1.# Na2O2.# Na3PO43.# N2O4Solu on1.# hich#form#ionic#bonds.2.# #and#covalent#bonds.3.# ,#or#both?1.# Ba(OH)22.# F23.# PCl3The chemical formulas for covalent compounds are referred to as molecular formulas because thesecompounds exist as separate, discrete molecules. Typically, a molecular formula begins with thenonmetal that is closest to the lower left corner of the periodic table, except that hydrogen is almostnever written first (H2O is the prominent exception). Then the other nonmetal symbols are listed.Numerical subscripts are used if there is more than one of a particular atom. For example, we -of-chemistry/Final -simple-mo.htmlPage 11 of 56
Chapter 4: Covalent Bonding and Simple Molecular Compounds1/7/15, 2:57 PMalready seen CH4, the molecular formula for methane.Naming binary (two-element) covalent compounds is similar to naming simple ionic compounds. Thefirst element in the formula is simply listed using the name of the element. The second element isnamed by taking the stem of the element name and adding the suffix -ide. A system of numericalprefixes is used to specify the number of atoms in a molecule. Table 4.1 "Numerical Prefixes for NamingBinary Covalent Compounds" lists these numerical prefixes. Normally, no prefix is added to the firstelement’s name if there is only one atom of the first element in a molecule. If the second element isoxygen, the trailing vowel is usually omitted from the end of a polysyllabic prefix but not a monosyllabicone (that is, we would say “monoxide” rather than “monooxide” and “trioxide” rather than “troxide”).Table 4.1 Numerical Prefixes for Naming Binary Covalent CompoundsNumber(of(Atoms(in(Compound ame.Let us practice by naming the compound whose molecular formula is CCl4. The name begins with thename of the first element—carbon. The second element, chlorine, becomes chloride, and we attach thecorrect numerical prefix (“tetra-”) to indicate that the molecule contains four chlorine atoms. Puttingthese pieces together gives the name carbon tetrachloride for this cepts-of-chemistry/Final -simple-mo.htmlPage 12 of 56
Chapter 4: Covalent Bonding and Simple Molecular Compounds1/7/15, 2:57 mpound.1.# chlorine#trifluoride2.# phosphorus#pentachloride3.# sulfur#dioxide4.# dinitrogen#pentoxideSolu one#atom#ofthat#element#in#a#molecule.1.# ClF32.# PCl53.# SO24.# 1.# nitrogen#dioxide2.# dioxygen#difluoride3.# sulfur#hexafluoride4.# hemistry/concepts-of-chemistry/Final -simple-mo.htmlPage 13 of 56
Chapter 4: Covalent Bonding and Simple Molecular Compounds1/7/15, 2:57 PMBecause it is so unreactive, sulfur hexafluoride is used as a spark suppressant in electrical devicessuch as ound.1.# BrF52.# S2F23.# COSolu on1.# bromine#pentafluoride2.# disulfur#difluoride3.# me#for#each#compound.1.# CF42.# SeCl23.# SO3For some simple covalent compounds, we use common names rather than systematic names. We havealready encountered these compounds, but we list them here explicitly:H2O: s-of-chemistry/Final -simple-mo.htmlPage 14 of 56
Chapter 4: Covalent Bonding and Simple Molecular Compounds1/7/15, 2:57 PMNH3: ammoniaCH4: methaneMethane is the simplest organic compound. Organic compounds are compounds with carbon atomsand are named by a separate nomenclature system that we will introduce in Section 4.6 "Introductionto Organic Chemistry".CONCEPT(REVIEW(EXERCISES1.# How#do#you#recognize#a#covalent#compound?2.# What#are#the#rules#for#wri ound?3.# mpound?ANSWERS1.# more#nonmetal#elements.2.# ent#name.3.# of#the#second#element.K E Y ( TA K E AWAY top/chemistry/concepts-of-chemistry/Final -simple-mo.htmlPage 15 of 56
Chapter 4: Covalent Bonding and Simple Molecular Compounds1/7/15, 2:57 PM1.# Iden fy#whether#each#compound#has#covalent#bonds.a.# NaIb.# Na2CO3c.# N2Od.# SiO22.# Iden fy#whether#each#compound#has#covalent#bonds.a.# C2H6b.# C6H5Clc.# KC2H3O2d.# Ca(OH)23.# Iden #bonds,#or#both.a.# Na3PO4b.# K2Oc.# COCl2d.# CoCl24.# Iden #bonds,#or#both.a.# FeCl3b.# Fe(NO3)3c.# (NH2)2COd.# SO35.# iH4?#Explain.6.# S?#Explain.7.# Write#the#name#for#each#covalent#compound.a.# SiF4b.# of-chemistry/Final -simple-mo.htmlPage 16 of 56
Chapter 4: Covalent Bonding and Simple Molecular Compounds1/7/15, 2:57 PMc.# CS2d.# P2O58.# Write#the#name#for#each#covalent#compound.a.# COb.# S2O3c.# BF3d.# GeS29.# Write#the#formula#for#each#covalent#compound.a.# iodine#trichlorideb.# disulfur#dibromidec.# arsenic#trioxided.# xenon#hexafluoride10.# Write#the#formula#for#each#covalent#compound.a.# boron#trichlorideb.# carbon#dioxidec.# tetraphosphorus#decoxided.# germanium#dichloride11.# er#than#systema c#names.12.# ture#for#binary#covalent#compounds?ANSWERS1.# a.# nob.# yesc.# yesd.# of-chemistry/Final -simple-mo.htmlPage 17 of 56
Chapter 4: Covalent Bonding and Simple Molecular Compounds1/7/15, 2:57 PM3.# a.# bothb.# ionicc.# covalentd.# ionic5.# isted#first#in#a#covalent#compound.7.# a.# silicon#tetrafluorideb.# nitrogen#dioxidec.# carbon#disulfided.# diphosphorus#pentoxide9.# a.# ICl3b.# S2Br2c.# AsO3d.# XeF611.# )4.3(MulZple(Covalent(BondsLEARNING(OBJECTIVE1.# Recognize#molecules#that#are#likely#to#have#mul ple#covalent#bonds.In many molecules, the octet rule would not be satisfied if each pair of bonded atoms shares twoelectrons. Consider carbon dioxide (CO2). If each oxygen atom shares one electron with the carbonatom, we get the ncepts-of-chemistry/Final -simple-mo.htmlPage 18 of 56
Chapter 4: Covalent Bonding and Simple Molecular Compounds1/7/15, 2:57 PMThis does not give the carbon atom a complete octet; you will find only six electrons in its valence shell.In addition, each oxygen atom has only seven electrons in its valence shell. Finally, no atom makes thenumber of bonds it typically forms (Figure 4.2 "How Many Covalent Bonds Are Formed?"). Thisarrangement of shared electrons is far from satisfactory.Sometimes more than one pair of electrons must be shared between two atoms for both atoms to havean octet. In carbon dioxide, a second electron from each oxygen atom is also shared with the centralcarbon atom, and the carbon atom shares one more electron with each oxygen atom:In this arrangement, the carbon atom shares four electrons (two pairs) with the oxygen atom on the leftand four electrons with the oxygen atom on the right. There are now eight electrons around each atom.Two pairs of electrons shared between two atoms make a double bond between the atoms, which isrepresented by a double dash:Some molecules contain triple bonds, covalent bonds in which three pairs of electrons are shared bytwo atoms. A simple compound that has a triple bond is acetylene (C2H2), whose Lewis diagram is ncepts-of-chemistry/Final -simple-mo.htmlPage 19 of 56
Chapter 4: Covalent Bonding and Simple Molecular Compounds1/7/15, 2:57 e.1.# N22.# CH2O#(The#carbon#atom#is#the#central#atom.)Solu follows:NoteOne application of CH2O, also called formaldehyde, is the preservation of biological specimens.Aqueous solutions of CH2O are called formalin and have a sharp, characteristic (pungent) s-of-chemistry/Final -simple-mo.htmlPage 20 of 56
Chapter 4: Covalent Bonding and Simple Molecular Compounds1/7/15, 2:57 r#each#molecule.1.# O22.# C2H4CONCEPT(REVIEW(EXERCISE1.# What#is#one#clue#that#a#molecule#has#a#mul ple#bond?ANSWER1.# atoms#(except#hydrogen)#an#octet,#mul ple#covalent#bondsmay#be#present.K E Y ( TA K E AWAYSome#molecules#must#have#mul ple#covalent#bonds#between#atoms#to#sa sfy#the#octet#rule.EXERCISES1.# Each#molecule#contains#mul �rst#element#is#the#centralatom.a.# CS2b.# C2F4c.# COCl22.# of-chemistry/Final -simple-mo.htmlPage 21 of 56
Chapter 4: Covalent Bonding and Simple Molecular Compounds1/7/15, 2:57 PMthe#central#atom,#unless#otherwise#noted.a.# N2b.# HCN#(The#carbon#atom#is#the#central#atom.)c.# POCl#(The#phosphorus#atom#is#the#central#atom.)3.# s.4.# ewis#diagram#for#MgO?ANSWERS1.# a.#b.#c.#3.# Hydrogen#can#accept#only#one#more#electron;#mul try/Final -simple-mo.htmlPage 22 of 56
Chapter 4: Covalent Bonding and Simple Molecular Compounds1/7/15, 2:57 PMLEARNING(OBJECTIVE1.# #bond#polarity.Covalent bonds have certain characteristics that depend on the identities of the atoms participating inthe bond. Two characteristics are bond length and bond polarity.Bond(LengthIn Section 4.1 "Covalent Bonds", we stated that the covalent bond in the hydrogen molecule (H2) has acertain length (about 7.4 10 11 m). Other covalent bonds also have known bond lengths, which aredependent on both the identities of the atoms in the bond and whether the bonds are single, double, ortriple bonds. Table 4.2 "Approximate Bond Lengths of Some Single Bonds" lists the approximate bondlengths for some single covalent bonds. The exact bond length may vary depending on the identity ofthe molecule but will be close to the value given in the table.Table 4.2 Approximate Bond Lengths of Some Single BondsBond Length(( (10 4C–N147C–O143N–N145O–O145Table 4.3 "Comparison of Bond Lengths for Single and Multiple Bonds" compares the lengths of ts-of-chemistry/Final -simple-mo.htmlPage 23 of 56
Chapter 4: Covalent Bonding and Simple Molecular Compounds1/7/15, 2:57 PMcovalent bonds with those of double and triple bonds between the same atoms. Without exception, asthe number of covalent bonds between two atoms increases, the bond length decreases. With moreelectrons between the two nuclei, the nuclei can get closer together before the internuclear repulsion isstrong enough to balance the attraction.Table 4.3 Comparison of Bond Lengths for Single and Multiple BondsBond Length(( (10 12(m)C–C154C C134C C120C–N147C N128C N116C–O143C O120C O113N–N145N N123N N110O–O145O O121ElectronegaZvity(and(Bond(PolarityAlthough we defined covalent bonding as electron sharing, the electrons in a covalent bond are notalways shared equally by the two bonded atoms. Unless the bond connects two atoms of the sameelement, there will always be one atom that attracts the electrons in the bond more strongly than theother atom does, as shown in Figure 4.3 "Polar versus Nonpolar Covalent Bonds". When such animbalance occurs, there is a resulting buildup of some negative charge (called a partial negative chargeand designated δ ) on one side of the bond and some positive charge (designated δ ) on the other -of-chemistry/Final -simple-mo.htmlPage 24 of 56
Chapter 4: Covalent Bonding and Simple Molecular Compounds1/7/15, 2:57 PMof the bond. A covalent bond that has an unequal sharing of electrons, as in part (b) of Figure 4.3 "Polarversus Nonpolar Covalent Bonds", is called a polar covalent bond. A covalent bond that has an equalsharing of electrons (part (a) of Figure 4.3 "Polar versus Nonpolar Covalent Bonds") is called anonpolar covalent bond.Figure 4.3 Polar versus Nonpolar Covalent Bonds(a) The electrons in the covalent bond are equally shared by both hydrogen atoms. This is a nonpolar covalentbond. (b) The fluorine atom attracts the electrons in the bond more than the hydrogen atom does, leading toan imbalance in the electron distribution. This is a polar covalent bond.Any covalent bond between atoms of different elements is a polar bond, but the degree of polarity varieswidely. Some bonds between different elements are only minimally polar, while others are stronglypolar. Ionic bonds can be considered the ultimate in polarity, with electrons being transferred ratherthan shared. To judge the relative polarity of a covalent bond, chemists use electronegativity, whichis a relative measure of how strongly an atom attracts electrons when it forms a covalent bond. s-of-chemistry/Final -simple-mo.htmlPage 25 of 56
Chapter 4: Covalent Bonding and Simple Molecular Compounds1/7/15, 2:57 PMare various numerical scales for rating electronegativity. Figure 4.4 "Electronegativities of VariousElements" shows one of the most popular—the Pauling scale. The polarity of a covalent bond can bejudged by determining the difference in the electronegativities of the two atoms making the bond. Thegreater the difference in electronegativities, the greater the imbalance of electron sharing in the bond.Although there are no hard and fast rules, the general rule is if the difference in electronegativities isless than about 0.4, the bond is considered nonpolar; if the difference is greater than 0.4, the bond isconsidered polar. If the difference in electronegativities is large enough (generally greater than about1.8), the resulting compound is considered ionic rat
Chapter 3 "Ionic Bonding and Simple Ionic Compounds" discussed ionic bonding, which results from the transfer of electrons among atoms or groups of atoms. In this chapter, we will consider another type of bonding—covalent bonding. We will examine how atoms share electrons to form these bonds, and we
Covalent Bonding 1. What is covalent bonding? 2. Ionic or covalent? a. CH 4 ionic or covalent b. Fe 2 O 3 ionic or covalent c. I 2 ionic or covalent d. H 2 O ionic or covalent e. BeCl 2 ionic or covalent 3. Lewis dot structures Helpful hints: Least electronegative compound goes in the middle
Chem 103, Section F0F Unit VI - Compounds Part II: Covalent Compounds Lecture 15 The formation of covalent bonds Naming binary covalent and organic compounds The covalent bonding model Lecture 15 - Covalent Bonding Reading in Silberberg Chapter 2, Section 7 (pp. 62-64)-The Formation of Covalent Compounds Chapter 2, Section 8 (pp. 70-72)-Compounds, Formulas and Names
Chapter 8 Covalent Bonding 8.1 Molecular Compounds 8.2 The Nature of Covalent Bonding 8.3 Bonding Theories 8.4 Polar Bonds and Molecules . . type of covalent bonding different from that seen in water, ammonia, methane, and carbon
Pure covalent bonding only occurs when two nonmetal atoms of the same kind bind to each other. When two different nonmetal atoms are bonded or a nonmetal and a metal are bonded, then the bond is a mixture of cova-lent and ionic bonding called polar covalent bonding. Covalent Bonding In METALLIC BONDING the valence electrons are
What is a coordinate covalent bond? A coordinate covalent bond is an atom in which one atom provides both bonding electrons Example - Carbon monoxide. How does bonding in carbon monoxide work? Once a coordinate covalent bond forms, it is like any other covalent bond. It is often drawn as an arrow in a structural formula
A)Metallic bonding B)hydrogen bonding C)covalent bonding D)ionic bonding 26.The particle diagram below represents a solid sample of silver. Which type of bonding is present when valence electrons move within the sample? A)ionic B)metallic C)nonpolar covalent D)polar covalent 27.Which type of bonding is present in a sample of an element that is .
2 Ionic/Covalent Beryllium nitride Li 2S Ionic/Covalent Lithium sulphide B 2O 3 Ionic/Covalent Diboron trioxide CaBr 2 Ionic/Covalent Calcium bromide Si 2Cl 6 Ionic/Covalent Disilicon hexachloride N 4S 5 Ionic/Covalent Tetranitrogen pentasulfide 2.Determine if the compound is ionic or covalent
Chapter 9 - Covalent Bonding I. Covalent Bonding: attractive force produced as a result of shared (pgs 189electrons. -193) A. A _is formed when two or more atoms bond covalently. B. Bonds form when there is a balance of attractive and repulsive forces between two atoms: C. Single Covalent Bond & Lewis Structures
