CHAPTER 8. Molecular Structure & Covalent Bonding Theories
|
|
|
- Cory Watson
- 6 years ago
- Views:
Transcription
1 CAPTER 8 Molecular Structure & Covalent Bonding Theories 1
2 Chapter Goals 1. A Preview of the Chapter 2. Valence Shell Electron Pair Repulsion (VSEPR) Theory 3. Polar Molecules:The Influence of Molecular Geometry 4. Valence Bond (VB) Theory 2
3 Chapter Goals Molecular Shapes and Bonding 5. Linear Electronic Geometry: AB 2 Species 6. Trigonal Planar Electronic Geometry: AB 3 Species 7. Tetrahedral Electronic Geometry: AB 4 Species 8. Tetrahedral Electronic Geometry: AB 3 USpecies 9. Tetrahedral Electronic Geometry: AB 2 U 2 Species 10. Tetrahedral Electronic Geometry ABU 3 Species 11. Trigonal Bipyramidal Geometry 12. Octahedral Geometry 13. Compounds Containing Double Bonds 14. Compounds Containing Triple Bonds 15. A Summary of Electronic and Molecular Geometries 3
4 Stereochemistry Stereochemistry is the study of the three dimensional shapes of molecules. Some questions to examine in this chapter are: 1. Why are we interested in shapes? 2. What role does molecular shape play in life? 3. ow do we determine molecular shapes? 4. ow do we predict molecular shapes? 4
5 Molecular Shapes The shape of a molecule plays an important role in its reactivity. By noting the number of bonding and nonbonding electron pairs we can easily predict the shape of the molecule. 5
6 Two Simple Theories of Covalent Bonding Valence Shell Electron Pair Repulsion Theory Commonly designated as VSEPR Principal originator R. J. Gillespie in the 1950 s Valence Bond Theory Involves the use of hybridized atomic orbitals Principal originator L. Pauling in the 1930 s & 40 s 6
7 VSEPR Theory In order to attain maximum stability, each atom in a molecule or ion arranges the electron pairs in its valence shell in such a way to minimize the repulsion of their regions of high electron density: (a) Lone (unshared or nonbonding) pairs of electrons (b) Single bond (c) Double bond (d) Triple bond 7
8 VSEPR Theory These four types of regions of high electron density (where the electron are) want to be as far apart as possible. The electrons repel each other. There are five basic molecular shapes based on the number of regions of high electron density around the central atom. 8
9 VSEPR Theory These are the regions of high electron density around the central atom for two through six electron densities around a central atom. 9
10 Electron-Density Geometries All one must do is count the number of electron density in the Lewis structure. The geometry will be that which corresponds to that number of electron density. : : Tetrahedral 10
11 VSEPR Theory 1. Electronic geometry is determined by the locations of regions of high electron density around the central atom(s). 2. Molecular geometry determined by the arrangement of atoms around the central atom(s). Electron pairs are not used in the molecular geometry determination just the positions of the atoms in the molecule are used. 11
12 Molecular Geometries electron-density Geometry - tetrahedral The electron-density geometry is often not the shape of the molecule, however. The molecular geometry is that defined by the positions of only the atoms in the molecules, not the nonbonding pairs. 12
13 VSEPR Theory An example of a molecule that has the same electronic and molecular geometries is methane - C 4. Electronic and molecular geometries are tetrahedral. C 13
14 VSEPR Theory An example of a molecule that has different electronic and molecular geometries is water - 2 O. Electronic geometry is tetrahedral. Molecular geometry is bent or angular. C 14
15 VSEPR Theory Lone pairs of electrons (unshared pairs) require more volume than shared pairs. Consequently, there is an ordering of repulsions of electrons around central atom. Criteria for the ordering of the repulsions: 15
16 VSEPR Theory 1 Lone pair to lone pair is the strongest repulsion. 2 Lone pair to bonding pair is intermediate repulsion. 3 Bonding pair to bonding pair is weakest repulsion. Mnemonic for repulsion strengths lp/lp > lp/bp > bp/bp Lone pair to lone pair repulsion is why bond angles in water are less than o. 16
17 VSEPR Theory lp/bp 17
18 Multiple Bonds and Bond Angles bp/bp repulsion Double and triple bonds place greater electron density on one side of the central atom than do single bonds. Therefore, they also affect bond angles. 18
19 Nonbonding Pairs and Bond Angle Nonbonding pairs are physically larger than bonding pairs. Therefore, their repulsions are greater; this tends to decrease bond angles in a molecule. 19
20 Nonbonding Pairs and Bond Angle 20
21 Polarity In Chapter 7 we discussed bond dipoles. But just because a molecule possesses polar bonds does not mean the molecule as a whole will be polar. 21
22 Polar Molecules: The Influence of Molecular Geometry Molecular geometry affects molecular polarity. Due to the effect of the bond dipoles and how they either cancel or reinforce each other. A B A linear molecule nonpolar A B A angular molecule polar 22
23 Polarity By adding the individual bond dipoles, one can determine the overall dipole moment for the molecule. 23
24 Polarity 24
25 Polar Molecules: The Influence of Molecular Geometry Polar Molecules must meet two requirements: 1. One polar bond or one lone pair of electrons on central atom. 2. Neither bonds nor lone pairs can be symmetrically arranged that their polarities cancel. 25
26 Polarity 26
27 Valence Bond (VB) Theory Covalent bonds are formed by the overlap of atomic orbitals. Atomic orbitals on the central atom can mix and exchange their character with other atoms in a molecule. Process is called hybridization. ybrids are common: 1. Pink flowers 2. Mules ybrid Orbitals have the same shapes as predicted by VSEPR. 27
28 Valence Bond (VB) Theory Regions of Electronic ybridization igh Electron Geometry Density 2 Linear sp 3 Trigonal planar sp 2 4 Tetrahedral sp 3 5 Trigonal bipyramidal sp 3 d 6 Octahedral sp 3 d 2 28
29 Molecular Shapes and Bonding In the next sections we will use the following terminology: A = central atom B = bonding pairs around central atom U = lone pairs around central atom For example: AB 3 U designates that there are 3 bonding pairs and 1 lone pair around the central atom. 29
30 Linear Electronic Geometry:AB 2 Species (No Lone Pairs of Electrons on A) Some examples of molecules with this geometry are: BeCl 2, BeBr 2,BeI 2, gcl 2, CdCl 2 All of these examples are linear, nonpolar molecules. Important exceptions occur when the two substituents are not the same! BeClBr or BeIBr will be linear and polar! 30
31 Linear Electronic Geometry: AB 2 Species (No Lone Pairs of Electrons on A) Electronic Geometry C 31
32 Linear Electronic Geometry: AB 2 Species (No Lone Pairs of Electrons on A) Polarity 32
33 Linear Electronic Geometry: AB 2 Species (No Lone Pairs of Electrons on A) Valence Bond Theory (ybridization) 33
34 Linear Electronic Geometry: AB 2 Species (No Lone Pairs of Electrons on A) 34
35 Linear Electronic Geometry: AB 2 Species (No Lone Pairs of Electrons on A) 35
36 Trigonal Planar Electronic Geometry: AB 3 Species (No Lone Pairs of Electrons on A) Some examples of molecules with this geometry are: BF 3, BCl 3 All of these examples are trigonal planar, nonpolar molecules. Important exceptions occur when the three substituents are not the same! BF 2 Cl or BCI 2 Br will be trigonal planar and polar! 36
37 Trigonal Planar Electronic Geometry: AB 3 Species (No Lone Pairs of Electrons on A) Dot Formula Electronic Geometry 37 C
38 Trigonal Planar Electronic Geometry: AB 3 Species (No Lone Pairs of Electrons on A) Polarity 38
39 Trigonal Planar Electronic Geometry: AB 3 Species (No Lone Pairs of Electrons on A) Valence Bond Theory (ybridization) 3s 3p Cl [Ne] 39
40 Trigonal Planar Electronic Geometry: AB 3 Species (No Lone Pairs of Electrons on A) 40
41 Trigonal Planar Electronic Geometry: AB 3 Species (No Lone Pairs of Electrons on A) 41
42 Tetrahedral Electronic Geometry: AB 4 Species (No Lone Pairs of Electrons on A) Some examples of molecules with this geometry are: C 4, CF 4, CCl 4, Si 4, SiF 4 All of these examples are tetrahedral, nonpolar molecules. Important exceptions occur when the four substituents are not the same! CF 3 Cl or C 2 CI 2 will be tetrahedral and polar! 42
43 Tetrahedral Electronic Geometry: AB 4 Species (No Lone Pairs of Electrons on A) 43
44 Tetrahedral Electronic Geometry: AB 4 Species (No Lone Pairs of Electrons on A) 44
45 Tetrahedral Electronic Geometry: AB 4 Species (No Lone Pairs of Electrons on A) 45
46 46
47 47
48 48
49 Tetrahedral Electronic Geometry: AB 3 U Species (One Lone Pair of Electrons on A) Some examples of molecules with this geometry are: N 3, NF 3, P 3, PCl 3, As 3 These molecules are our first examples of central atoms with lone pairs of electrons. Thus, the electronic and molecular geometries are different. All three substituents are the same but molecule is polar. N 3 and NF 3 are trigonal pyramidal, polar molecules. 49
50 Tetrahedral Electronic Geometry: AB 3 U Species (One Lone Pair of Electrons on A) Valence Bond Theory 50
51 51
52 Tetrahedral Electronic Geometry: AB 3 U Species (One Lone Pair of Electrons on A) 52
53 Electronic Geometry 53
54 54
55 Molecular Geometry 55
56 Tetrahedral Electronic Geometry: AB 3 U Species (One Lone Pair of Electrons on A) Polarity 56
57 Tetrahedral Electronic Geometry: AB 2 U 2 Species (Two Lone Pairs of Electrons on A) Some examples of molecules with this geometry are: 2 O, OF 2, OCl 2, 2 S These molecules are our first examples of central atoms with two lone pairs of electrons. Thus, the electronic and molecular geometries are different. Both substituents are the same but molecule is polar. Molecules are angular, bent, or V-shaped and polar. 57
58 Tetrahedral Electronic Geometry: AB 2 U 2 Species (Two Lone Pairs of Electrons on A) Valence Bond Theory (ybridization) 2s O [e] 2p four sp 3 hybrids C 58
59 Tetrahedral Electronic Geometry: ABU 3 Species (Three Lone Pairs of Electrons on A) Some examples of molecules with this geometry are: F, Cl, Br, I, FCl, IBr These molecules are examples of central atoms with three lone pairs of electrons. Again, the electronic and molecular geometries are different. Molecules are linear and polar when the two atoms are different. Cl 2, Br 2, I 2 are nonpolar. 59
60 Tetrahedral Electronic Geometry: ABU 3 Species (Three Lone Pairs of Electrons on A) Dot Formula F Molecular Geometry : F : 3 lone pairs Electronic Geometry : F : tetrahedral : Polarity F is a polar molecule. : linear C 60
61 Tetrahedral Electronic Geometry: ABU 3 Species (Three Lone Pairs of Electrons on A) Valence Bond Theory (ybridization) 2s 2p four sp 3 hybrids F [e] : F : : tetrahedral 61
62 Trigonal Bipyramidal Electronic Geometry: AB 5, AB 4 U, AB 3 U 2, and AB 2 U 3 Some examples of molecules with this geometry are: PF 5, AsF 5, PCl 5, etc. These molecules are examples of central atoms with five bonding pairs of electrons. The electronic and molecular geometries are the same. Molecules are trigonal bipyramidal and nonpolar when all five substituents are the same. If the five substituents are not the same polar molecules 62 can result, AsF 4 Cl is an example.
63 Trigonal Bipyramidal Electronic Geometry: AB 5, AB 4 U, AB 3 U 2, and AB 2 U 3 Valence Bond Theory 63
64 Trigonal Bipyramidal Electronic Geometry: AB 5, AB 4 U, AB 3 U 2, and AB 2 U 3 64
65 65
66 Molecular Geometry Trigonal Bipyramidal 66
67 Trigonal Bipyramidal Electronic Geometry: AB 5, AB 4 U, AB 3 U 2, and AB 2 U 3 If lone pairs are incorporated into the trigonal bipyramidal structure, there are three possible new shapes. 1. One lone pair - Seesaw shape 2. Two lone pairs - T-shape 3. Three lone pairs linear The lone pairs occupy equatorial positions because they are 120 o from two bonding pairs and 90 o from the other two bonding pairs. Results in decreased repulsions compared to lone pair in axial position. 67
68 Trigonal Bipyramidal Electronic Geometry: AB 5, AB 4 U, AB 3 U 2, and AB 2 U 3 AB 4 U molecules have: 1. trigonal bipyramid electronic geometry 2. seesaw shaped molecular geometry 3. and are polar One example of an AB 4 U molecule is SF 4 ybridization of S atom is sp 3 d. 68
69 Trigonal Bipyramidal Electronic Geometry: AB 5, AB 4 U, AB 3 U 2, and AB 2 U 3 Lewis Dot Molecular Geometry C seesaw Electronic Geometry 69
70 70
71 Trigonal Bipyramidal Electronic Geometry: AB 5, AB 4 U, AB 3 U 2, and AB 2 U 3 AB 3 U 2 molecules have: 1. trigonal bipyramid electronic geometry 2. T-shaped molecular geometry 3. and are polar One example of an AB 3 U 2 molecule is IF 3 ybridization of I atom is sp 3 d. 71
72 Trigonal Bipyramidal Electronic Geometry: AB 5, AB 4 U, AB 3 U 2, and AB 2 U 3 Molecular Geometry C 72
73 Trigonal Bipyramidal Electronic Geometry: AB 5, AB 4 U, AB 3 U 2, and AB 2 U 3 AB 2 U 3 molecules have: 1.trigonal bipyramid electronic geometry 2.linear molecular geometry 3.and are nonpolar One example of an AB 3 U 2 molecule is XeF 2 ybridization of Xe atom is sp 3 d. 73
74 Trigonal Bipyramidal Electronic Geometry: AB 5, AB 4 U, AB 3 U 2, and AB 2 U 3 Molecular Geometry C 74
75 Trigonal Bipyramidal Electronic Geometry: AB 5, AB 4 U, AB 3 U 2, and AB 2 U 3 75
76 Octahedral Electronic Geometry: AB 6, AB 5 U, and AB 4 U 2 Some examples of molecules with this geometry are: SF 6, SeF 6, SCl 6, etc. These molecules are examples of central atoms with six bonding pairs of electrons. Molecules are octahedral and nonpolar when all six substituents are the same. If the six substituents are not the same polar molecules can result, SF 5 Cl is an example. 76
77 Octahedral Electronic Geometry: AB 6, AB 5 U, and AB 4 U 2 Nonpolar 77
78 Octahedral Electronic Geometry: AB 6, AB 5 U, and AB 4 U 2 78
79 Octahedral Electronic Geometry: AB 6, AB 5 U, and AB 4 U 2 79
80 Octahedral Electronic Geometry: AB 6, AB 5 U, and AB 4 U 2 If lone pairs are incorporated into the octahedral structure, there are two possible new shapes. 1. One lone pair - square pyramidal 2. Two lone pairs - square planar The lone pairs occupy axial positions because they are 90 o from four bonding pairs. Results in decreased repulsions compared to lone pairs in equatorial positions. 80
81 Octahedral Electronic Geometry: AB 6, AB 5 U, and AB 4 U 2 AB 5 U molecules have: 1.octahedral electronic geometry 2.Square pyramidal molecular geometry 3.and are polar. One example of an AB 4 U molecule is IF 5 ybridization of I atom is sp 3 d 2. 81
82 Octahedral Electronic Geometry: AB 6, AB 5 U, and AB 4 U 2 Molecular Geometry C 82
83 Octahedral Electronic Geometry: AB 6, AB 5 U, and AB 4 U 2 AB 4 U 2 molecules have: 1.octahedral electronic geometry 2.square planar molecular geometry 3.and are nonpolar. One example of an AB 4 U 2 molecule is XeF 4 ybridization of Xe atom is sp 3 d 2. 83
84 Octahedral Electronic Geometry: AB 6, AB 5 U, and AB 4 U 2 Molecular Geometry Polarity C nonpolar 84
85 Octahedral Electronic Geometry: AB 6, AB 5 U, and AB 4 U 2 85
86 Sigma (σ) Bonds Sigma bonds are characterized by ead-to-head overlap. Cylindrical symmetry of electron density about the internuclear axis. 86
87 Pi (π) Bonds Pi bonds are characterized by Side-to-side overlap. Electron density above and below the internuclear axis. 87
88 Single Bonds Single bonds are always σ bonds, because σ overlap is greater, resulting in a stronger bond and more energy lowering. 88
89 Multiple Bonds In a multiple bond one of the bonds is a σ bond and the rest are π bonds. 89
90 Compounds Containing Double Bonds Ethene or ethylene, C 2 4, is the simplest organic compound containing a double bond. Lewis dot formula N = 2(8) + 4(2) = 24 A = 2(4) + 4(1) = 12 S = 12 Compound must have a double bond to obey octet rule. C C or C C 90
91 Compounds Containing Double Bonds VSEPR Theory suggests that the C atoms are at center of trigonal planes. Valence Bond Theory (ybridization) C atom has four electrons.three electrons from each C atom are in sp 2 hybrids. One electron in each C atom remains in an unhybridized p orbital C C 91
92 Compounds Containing Double Bonds An sp 2 hybridized C atom has this shape. Remember there will be one electron in each of the three lobes. Top view of an sp 2 hybrid The single 2p orbital is perpendicular to the trigonal planar sp 2 lobes. The fourth electron is in the p orbital. Side view of sp 2 hybrid with p orbital included. 92
93 Compounds Containing Double Bonds Two sp 2 hybridized C atoms plus p orbitals in proper orientation to form C=C double bond. The head-on overlap of the sp 2 hybrids is designated as a σ bond. 93
94 Compounds Containing Double Bonds The other portion of the double bond, resulting from the side-on overlap of the p orbitals, is designated as a π bond. 94
95 Compounds Containing Double Bonds Thus a C=C bond looks like this and is made of two parts, one σ and one π bond. C C 95
96 Multiple Bonds In a molecule like formaldehyde (shown at left) an sp 2 orbital on carbon overlaps in σ fashion with the corresponding orbital on the oxygen. The unhybridized p orbitals overlap in π fashion. 96
97 Compounds Containing Triple Bonds Ethyne or acetylene, C 2 2, is the simplest triple bond containing organic compound. Lewis Dot Formula N = 2(8) + 2(2) = 20 A = 2(4) + 2(1) =10 S = 10 Compound must have a triple bond to obey octet rule. C C or C C 97
98 Compounds Containing Triple Bonds VSEPR Theory suggests regions of high electron density are 180 o apart. C C Valence Bond Theory (ybridization) Carbon has 4 electrons. Two of the electrons are in sp hybrids. Two electrons remain in unhybridized p orbitals. 98
99 Compounds Containing Triple Bonds An sp hybridized C atom has this shape. Remember there will be one electron in each of the two lobes. The two 2p orbital are perpendicular to the sp lobes. The third and fourth electrons are in the p orbitals. The head-on overlap of the sp 2 hybrids is designated as a σ bond. 99
100 Compounds Containing Triple Bonds A σ bond results from the head-on overlap of two sp hybrid orbitals. 100
101 Compounds Containing Triple Bonds The unhybridized p orbitals form two π bonds. Note that a triple bond consists of one σ and two π bonds. The final result is a bond that looks like this. C 101
102 Larger Molecules In larger molecules, it makes more sense to talk about the geometry about a particular atom rather than the geometry of the molecule as a whole. 102
103 Larger Molecules This approach makes sense, especially because larger molecules tend to react at a particular site in the molecule. 103
104 ere is the structure for most students friend: CAFFEINE 1- Assign hybridization on C, N, and O. Beware I did not put the lone pairs of electrons into the chemical drawing. 2- ow many sigma bonds are present? 3- ow many pi bonds are present? 4- ow many lone pairs of electrons are present? (You have to look for them) C O N C C C N C O C N N C C 104
105 ere is the structure Theobromine, one of the components of TEA 1- Assign hybridization on C, N, and O. Beware I did not put the lone pairs of electrons into the chemical drawing. 2- ow many sigma bonds are present? 3- ow many pi bonds are present? 4- ow many lone pairs of electrons are present? (You have to look for them) O N C C C N C O C N N C C 105
106 End of Chapter 8 This is a difficult chapter. Essential to your understanding of chemistry! 106
107 omework Assignment One-line Web Learning (OWL): Chapter 8 Exercises and Tutors Optional 107
Hybridization and Molecular Orbital (MO) Theory
ybridization and Molecular Orbital (MO) Theory Chapter 10 istorical Models G.N.Lewis and I. Langmuir (~1920) laid out foundations Ionic species were formed by electron transfer Covalent molecules arise
Molecular Geometry. Valence Shell Electron Pair. What Determines the Shape of a Molecule? Repulsion Theory (VSEPR) Localized Electron Model
Molecular Geometry Learn Shapes you will Because the physical and chemical properties of compounds are tied to their structures, the importance of molecular geometry can not be overstated. Localized Electron
Chapter , Exam 2
Chapter 4 4.5-4.7, 4.9-4.10 Exam 2 Covalent Bonding Covalent bonds are formed when two nonmetals combine The atoms share electrons. If the atoms share 2 electrons a single covalent bond is formed. If the
Chemical Bonding II. Molecular Geometry Valence Bond Theory Phys./Chem. Properties Quantum Mechanics Sigma & Pi bonds Hybridization MO theory
Chemical Bonding II Molecular Geometry Valence Bond Theory Phys./Chem. Properties Quantum Mechanics Sigma & Pi bonds ybridization MO theory 1 Molecular Geometry 3-D arrangement of atoms 2 VSEPR Valence-shell
Molecular Geometry. Dr. Williamson s Molecular Geometry Notes. VSEPR: Definition of Terms. Dr. V.M. Williamson Texas A & M University Student Version
Molecular Geometry Dr. V.M. Williamson Texas A & M University Student Version Valence Shell Electron Pair Repulsion- VSEPR 1. Valence e- to some extent 2. Electron pairs move as far away as possible to
Molecular Geometry. Dr. Williamson s Molecular Geometry Notes. VSEPR: Definition of Terms. VSEPR: Electronic Geometries VSEPR
Molecular Geometry Dr. V.M. Williamson Texas A & M University Student Version Valence Shell Electron Pair Repulsion- VSEPR 1. Valence e- to some extent 2. Electron pairs move as far away as possible to
Chapter 9. Molecular Geometries and Bonding Theories. Lecture Presentation. John D. Bookstaver St. Charles Community College Cottleville, MO
Lecture Presentation Chapter 9 Theories John D. Bookstaver St. Charles Community College Cottleville, MO Shapes The shape of a molecule plays an important role in its reactivity. By noting the number of
General and Inorganic Chemistry I.
General and Inorganic Chemistry I. Lecture 1 István Szalai Eötvös University István Szalai (Eötvös University) Lecture 1 1 / 29 Outline István Szalai (Eötvös University) Lecture 1 2 / 29 Lewis Formulas
Chapter 9. and Bonding Theories
Chemistry, The Central Science, 11th edition Theodore L. Brown, H. Eugene LeMay, Jr., and Bruce E. Bursten Chapter 9 Theories John D. Bookstaver St. Charles Community College Cottleville, MO Shapes The
Chapter 9. Molecular Geometries and Bonding Theories. Lecture Presentation. John D. Bookstaver St. Charles Community College Cottleville, MO
Lecture Presentation Chapter 9 Theories John D. Bookstaver St. Charles Community College Cottleville, MO Shapes The shape of a molecule plays an important role in its reactivity. By noting the number of
Chapter 9. and Bonding Theories. Molecular Shapes. What Determines the Shape of a Molecule? 3/8/2013
Chemistry, The Central Science, 10th edition Theodore L. Brown, H. Eugene LeMay, Jr., and Bruce E. Bursten Chapter 9 Theories John D. Bookstaver St. Charles Community College St. Peters, MO 2006, Prentice-Hall,
Shapes of Molecules and Hybridization
Shapes of Molecules and Hybridization A. Molecular Geometry Lewis structures provide us with the number and types of bonds around a central atom, as well as any NB electron pairs. They do not tell us the
Lewis Dot Structures for Methane, CH 4 The central C atom is bonded by single bonds (-) to 4 individual H atoms
Chapter 10 (Hill/Petrucci/McCreary/Perry Bonding Theory and Molecular Structure This chapter deals with two additional approaches chemists use to describe chemical bonding: valence-shell electron pair
CHEMISTRY. Chapter 10 Theories of Bonding and Structure. The Molecular Nature of Matter. Jespersen Brady Hyslop SIXTH EDITION
CHEMISTRY The Molecular Nature of Matter SIXTH EDITION Jespersen Brady Hyslop Chapter 10 Theories of Bonding and Structure Copyright 2012 by John Wiley & Sons, Inc. Molecular Structures Molecules containing
Experiment 15. The Valence Shell Electron Pair Repulsion (VSEPR) Theory of Directed Valency: An exercise
Experiment 15 The Valence Shell Electron Pair Repulsion (VSEPR) Theory of Directed Valency: An exercise Attempts to understand and predict the shapes of molecules using either the valencebond theory or
Chapter 9: Molecular Geometries and Bonding Theories Learning Outcomes: Predict the three-dimensional shapes of molecules using the VSEPR model.
Chapter 9: Molecular Geometries and Bonding Theories Learning Outcomes: Predict the three-dimensional shapes of molecules using the VSEPR model. Determine whether a molecule is polar or nonpolar based
Subtopic 4.2 MOLECULAR SHAPE AND POLARITY
Subtopic 4.2 MOLECULAR SHAPE AND POLARITY 1 LEARNING OUTCOMES (covalent bonding) 1. Draw the Lewis structure of covalent molecules (octet rule such as NH 3, CCl 4, H 2 O, CO 2, N 2 O 4, and exception to
Covalent Compounds: Bonding Theories and Molecular Structure
CHM 123 Chapter 8 Covalent Compounds: Bonding Theories and Molecular Structure 8.1 Molecular shapes and VSEPR theory VSEPR theory proposes that the geometric arrangement of terminal atoms, or groups of
Name Unit Three MC Practice March 15, 2017
Unit Three: Bonding & Molecular Geometry Name Unit Three MC Practice March 15, 2017 1. What is the hybridization of the oxygen atom in water? a) sp b) sp 2 c) sp 3 d) It is not hybridized 2. When a double
Chapter 9 Molecular Geometry and Bonding Theories
Chapter 9 Molecular Geometry and Bonding Theories molecular shapes the VSEPR model molecular shape and molecular polarity covalent bonding and orbital overlap hybrid orbitals multiple bonds 9.1 Molecular
Molecular Geometry and Chemical Bonding Theory
Molecular Geometry and Chemical Bonding Theory The Valence -Shell Electron -Pair Repulsion (VSEPR) Model predicts the shapes of the molecules and ions by assuming that the valence shell electron pairs
Introduction to VSEPR Theory 1
1 Class 8: Introduction to VSEPR Theory Sec 10.2 VSEPR Theory: The Five Basic Shapes Two Electron Groups: Linear Geometry Three Electron Groups: Trigonal Planar Geometry Four Electron Groups: Tetrahedral
Valence Shell Electron Pair repulsion
Molecular Geometry Valence Shell Electron Pair repulsion The valence shell electron pair repulsion model (VSEPR model) assumes that electron pairs repel one another. (VSEPR) model gives helps determine
Chapter 10. Geometry
Chapter 10 Molec cular Geometry 1 CHAPTER OUTLINE Molecular Geometry Molecular Polarity VSEPR Model Summary of Molecular Shapes Hybridization Molecular Orbital Theory Bond Angles 2 MOLECULAR GEOMETRY Molecular
Chapter Molecules are 3D. Shapes and Bonds. Chapter 9 1. Chemical Bonding and Molecular Structure
Chapter 9 Chemical Bonding and Molecular Structure 1 Shape 9.1 Molecules are 3D Angle Linear 180 Planar triangular (trigonal planar) 120 Tetrahedral 109.5 2 Shapes and Bonds Imagine a molecule where the
Molecular shape is determined by the number of bonds that form around individual atoms.
Chapter 9 CH 180 Major Concepts: Molecular shape is determined by the number of bonds that form around individual atoms. Sublevels (s, p, d, & f) of separate atoms may overlap and result in hybrid orbitals
Molecular shape is only discussed when there are three or more atoms connected (diatomic shape is obvious).
Chapter 10 Molecular Geometry (Ch9 Jespersen, Ch10 Chang) The arrangement of the atoms of a molecule in space is the molecular geometry. This is what gives the molecules their shape. Molecular shape is
Chemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals
Chemical Bonding II: and ybridization of Atomic rbitals Chapter 10 Valence shell electron pair repulsion (VSEPR) model: Predict the geometry of the molecule from the electrostatic repulsions between the
Structures, Shapes and Polarity. of Molecules. Level 2 recap: - Polar and non polar bonds - Lewis diagrams - Lone pairs - Shapes - Polarity
Structures, Shapes and Polarity Level 2 recap: - Polar and non polar bonds - Lewis diagrams - Lone pairs - Shapes - Polarity of Molecules Do now: Brainstorm what you know/remember about these L2 concepts
Chapter 9. Chemical Bonding II: Molecular Geometry and Bonding Theories
Chapter 9 Chemical Bonding II: Molecular Geometry and Bonding Theories Topics Molecular Geometry Molecular Geometry and Polarity Valence Bond Theory Hybridization of Atomic Orbitals Hybridization in Molecules
Molecular Geometry and intermolecular forces. Unit 4 Chapter 9 and 11.2
1 Molecular Geometry and intermolecular forces Unit 4 Chapter 9 and 11.2 2 Unit 4.1 Chapter 9.1-9.3 3 Review of bonding Ionic compound (metal/nonmetal) creates a lattice Formula doesn t tell the exact
Ex. 1) F F bond in F = 0 < % covalent, no transfer of electrons
#60 Notes Unit 8: Bonding Ch. Bonding I. Bond Character Bonds are usually combinations of ionic and covalent character. The electronegativity difference is used to determine a bond s character. Electronegativity
Chapter 8. Molecular Shapes. Valence Shell Electron Pair Repulsion Theory (VSEPR) What Determines the Shape of a Molecule?
PowerPoint to accompany Molecular Shapes Chapter 8 Molecular Geometry and Bonding Theories Figure 8.2 The shape of a molecule plays an important role in its reactivity. By noting the number of bonding
Chapter 9. Molecular Geometry and Bonding Theories
Chapter 9. Molecular Geometry and Bonding Theories 9.1 Molecular Shapes Lewis structures give atomic connectivity: they tell us which atoms are physically connected to which atoms. The shape of a molecule
Hybridization of Orbitals
Hybridization of Orbitals Structure & Properties of Matter 1 Atomic Orbitals and Bonding Previously: Electron configurations Lewis structures Bonding Shapes of molecules Now: How do atoms form covalent
How does the number of bonds and nonbonded pairs of electrons affect the shape of a molecule?
Reading: Chapter 9, sections 9.1-9.6 As you read these sections ask yourself: ow does the number of bonds and nonbonded pairs of electrons affect the shape of a molecule? Why is the repulsion between two
Organic Chemistry. Review Information for Unit 1. VSEPR Hybrid Orbitals Polar Molecules
rganic hemistry Review Information for Unit 1 VSEPR ybrid rbitals Polar Molecules VSEPR The valence shell electron pair repulsion model (VSEPR) can be used to predict the geometry around a particular atom
Chemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals
Chemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals Chapter 10 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. 1 Valence shell electron
Molecular Geometries. Molecular Geometries. Remember that covalent bonds are formed when electrons in atomic orbitals are shared between two nuclei.
Molecular Geometries Lewis dot structures are very useful in determining the types of bonds in a molecule, but they may not provide the best insight into the spatial geometry of a molecule, i.e., how the
Chapter 9: Molecular Geometry and Bonding Theories
Chapter 9: Molecular Geometry and Bonding Theories 9.1 Molecular Geometries -Bond angles: angles made by the lines joining the nuclei of the atoms in a molecule -Bond angles determine overall shape of
At the end of this lesson, students should be able to :
At the end of this lesson, students should be able to : (a) Explain Valence Shell Electron Pair Repulsion theory (VSEPR) (b) Draw the basic molecular shapes: linear, planar, tetrahedral, and octahedral.
Molecular Geometry & Polarity
Molecular Geometry & Polarity Learn Shapes you will Because the physical and chemical properties of compounds are tied to their structures, the importance of molecular geometry can not be overstated. Localized
Chemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals Chapter 1
Chemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals Chapter 1 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. How to get the book of
Chapter 9 Molecular Geometry and Bonding Theories
Lecture Presentation Chapter 9 Geometry James F. Kirby Quinnipiac University Hamden, CT Shapes Lewis Structures show bonding and lone pairs, but do not denote shape. However, we use Lewis Structures to
Chapter 10. VSEPR Model: Geometries
Chapter 10 Molecular Geometry VSEPR Model: Geometries Valence Shell Electron Pair Repulsion Theory Electron pairs repel and get as far apart as possible Example: Water Four electron pairs Farthest apart
Chapter 9. Lewis Theory-VSEPR Valence Bond Theory Molecular Orbital Theory
Chapter 9 Lewis Theory-VSEPR Valence Bond Theory Molecular Orbital Theory Problems with Lewis Theory Lewis theory generally predicts trends in properties, but does not give good numerical predictions.
Lecture outline: Section 9. theory 2. Valence bond theory 3. Molecular orbital theory. S. Ensign, Chem. 1210
Lecture outline: Section 9 Molecular l geometry and bonding theories 1. Valence shell electron pair repulsion theory 2. Valence bond theory 3. Molecular orbital theory 1 Ionic bonding Covalent bonding
Chemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals Chapter 10
Chemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals Chapter 10 Linear Trigonal 180 o planar 120 o Tetrahedral 109.5 o Trigonal Bipyramidal 120 and 90 o Octahedral 90 o linear Linear
CHEM 110 Exam 2 - Practice Test 1 - Solutions
CHEM 110 Exam 2 - Practice Test 1 - Solutions 1D 1 has a triple bond. 2 has a double bond. 3 and 4 have single bonds. The stronger the bond, the shorter the length. 2A A 1:1 ratio means there must be the
VSEPR. Valence Shell Electron Pair Repulsion Theory
VSEPR Valence Shell Electron Pair Repulsion Theory Vocabulary: domain = any electron pair or bond (single, double or triple) is considered one domain. bonding pair = shared pair = any electron pair that
1s atomic orbital 2s atomic orbital 2s atomic orbital (with node) 2px orbital 2py orbital 2pz orbital
Atomic Orbitals 1s atomic orbital 2s atomic orbital 2s atomic orbital (with node) 2px orbital 2py orbital 2pz orbital Valence Bond Theory and ybridized Atomic Orbitals Bonding in 2 1s 1s Atomic Orbital
Instant download Test bank for Chemistry The Central Science 10th Edition by Brown, LeMay, Bursten CLICK HERE
Chemistry, 10e (Brown) Chapter 9, Molecular Geometry and Bonding Theories Instant download Test bank for Chemistry The Central Science 10th Edition by Brown, LeMay, Bursten CLICK HERE http://testbankair.com/download/test-bank-for-chemistry-the-central-science-10th-edition-by-brown-lemay-bursten/
Chapter 10. VSEPR Model: Geometries
Chapter 10 Molecular Geometry VSEPR Model: Geometries Valence Shell Electron Pair Repulsion Theory Electron pairs repel and get as far apart as possible Example: Water Four electron pairs Two bonds Two
CHAPTER TEN MOLECULAR GEOMETRY MOLECULAR GEOMETRY V S E P R CHEMICAL BONDING II: MOLECULAR GEOMETRY AND HYBRIDIZATION OF ATOMIC ORBITALS
CHAPTER TEN CHEMICAL BONDING II: AND HYBRIDIZATION O ATOMIC ORBITALS V S E P R VSEPR Theory In VSEPR theory, multiple bonds behave like a single electron pair Valence shell electron pair repulsion (VSEPR)
Test bank for Chemistry The Central Science 10th Edition by Brown, LeMay, Bursten
Test bank for Chemistry The Central Science 10th Edition by Brown, LeMay, Bursten Chapter 9, Molecular Geometry and Bonding Theories Multiple-Choice and Bimodal 1) For a molecule with the formula A) linear
Localized Electron Model
Localized Electron Model Models for Chemical Bonding Localized electron model (Valence bond model) Molecular orbital model Localized Electron Model Useful for explaining the structure of molecules especially
Chapter 13: Phenomena
Chapter 13: Phenomena Phenomena: Scientists measured the bond angles of some common molecules. In the pictures below each line represents a bond that contains 2 electrons. If multiple lines are drawn together
Chapter 10 Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory
10.1 Artificial Sweeteners: Fooled by Molecular Shape 425 10.2 VSEPR Theory: The Five Basic Shapes 426 10.3 VSEPR Theory: The Effect of Lone Pairs 430 10.4 VSEPR Theory: Predicting Molecular Geometries
Chapter 10 Molecular Geometry and Chemical Bonding Theory. Copyright Cengage Learning. All rights reserved. 10 1
Chapter 10 Molecular Geometry and Chemical Bonding Theory Copyright Cengage Learning. All rights reserved. 10 1 Molecular geometry is the general shape of a molecule, as determined by the relative positions
Lewis structures show the number and type of bonds between atoms in a molecule or polyatomic ion.
VSEPR & Geometry Lewis structures show the number and type of bonds between atoms in a molecule or polyatomic ion. Lewis structures are not intended to show the 3-dimensional structure (i.e. shape or geometry)
Carbon-based molecules are held together by covalent bonds between atoms
hapter 1: hemical bonding and structure in organic compounds arbon-based molecules are held together by covalent bonds between atoms omposition: Mainly nonmetals; especially,, O, N, S, P and the halogens
Molecular Geometry and Bonding Theories. Chapter 9
Molecular Geometry and Bonding Theories Chapter 9 Molecular Shapes CCl 4 Lewis structures give atomic connectivity; The shape of a molecule is determined by its bond angles VSEPR Model Valence Shell Electron
2011, Robert Ayton. All rights reserved.
Chemical Bonding Outline 1. Lewis Dot Structures 2. Bonds 3. Formal Charges 4. VSEPR (Molecular Geometry and Hybridzation) 5. Common Resonance Structures and Dimerization Review 1. Lewis Dot Structures
Chapter 9 Molecular Geometry. Lewis Theory-VSEPR Valence Bond Theory Molecular Orbital Theory
Chapter 9 Molecular Geometry Lewis Theory-VSEPR Valence Bond Theory Molecular Orbital Theory Sulfanilamide Lewis Structures and the Real 3D-Shape of Molecules Lewis Theory of Molecular Shape and Polarity
Chemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals
Chemical Bonding II: and Hybridization of Atomic Orbitals Chapter 10 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. 1 Valence shell electron pair repulsion (VSEPR)
Chapter 9 Molecular Geometry Valence Bond and Molecular Orbital Theory
Chapter 9 Molecular Geometry Valence Bond and Molecular Orbital Theory Chapter Objectives: Learn the basics of Valence Bond Theory and Molecular Orbital Theory and how they are used to model covalent bonding.
Chapter 7 Chemical Bonding and Molecular Structure
Chapter 7 Chemical Bonding and Molecular Structure Three Types of Chemical Bonding (1) Ionic: formed by electron transfer (2) Covalent: formed by electron sharing (3) Metallic: attraction between metal
Shapes of Molecules. Lewis structures are useful but don t allow prediction of the shape of a molecule.
Shapes of Molecules Lewis structures are useful but don t allow prediction of the shape of a molecule. H O H H O H Can use a simple theory based on electron repulsion to predict structure (for non-transition
Chapter 9. Molecular Geometry and Bonding Theories
9.1 Molecular Shapes Read Sec. 9.1 and 9.2, then complete the Sample and Practice Exercises in these sections. Sample Exercise 9.1 (p. 347) Use the VSEPR model to predict the molecular geometries of a)
COVALENT BONDING CHEMICAL BONDING I: LEWIS MODEL. Chapter 7
Chapter 7 P a g e 1 COVALENT BONDING Covalent Bonds Covalent bonds occur between two or more nonmetals. The two atoms share electrons between them, composing a molecule. Covalently bonded compounds are
10-1. The Shapes of Molecules, chapter 10
10-1 The Shapes of Molecules, chapter 10 The Shapes of Molecules; Goals 10.1 Depicting Molecules and Ions with Lewis Structures 10.2 Valence-Shell Electron-Pair Repulsion (VSEPR) Theory 10.3 Molecular
Periodic Trends. Homework: Lewis Theory. Elements of his theory:
Periodic Trends There are various trends on the periodic table that need to be understood to explain chemical bonding. These include: Atomic/Ionic Radius Ionization Energy Electronegativity Electron Affinity
Chapter 9 Molecular Geometries. and Bonding Theories
Chapter 9 Molecular Geometries and Bonding Theories Coverage of Chapter 9 9.1 All 9.2 All 9.3 All 9.4 All 9.5 Omit Hybridization Involving d Orbitals 9.6 All 9.7 and 9.8 Omit ALL MOLECULAR SHAPES The shape
Adapted from CHM 130 Maricopa County, AZ Molecular Geometry and Lewis Dot Formulas Introduction
Adapted from CHM 130 Maricopa County, AZ Molecular Geometry and Lewis Dot Formulas Introduction A chemical bond is an intramolecular (within the molecule) force holding two or more atoms together. Covalent
B. (i), (iii), and (v) C. (iv) D. (i), (ii), (iii), and (v) E. (i), (iii), (iv), and (v) Answer: B. SO 3, and NO 3 - both have 24 VE and have Lewis
SCCH 161 Homework 3 1. Give the number of lone pairs around the central atom and the molecular geometry of CBr 4. Answer: Carbon has 4 valence electrons and bonds to four bromine atoms (each has 7 VE s).
Lecture B2 VSEPR Theory
Lecture B2 VSEPR Theory Covalent Bond Theories 1. VSEPR (valence shell electron pair repulsion model). A set of empirical rules for predicting a molecular geometry using, as input, a correct Lewis Dot
Valence Bond Theory - Description
Bonding and Molecular Structure - PART 2 - Valence Bond Theory and Hybridization 1. Understand and be able to describe the Valence Bond Theory description of covalent bond formation. 2. Understand and
Bonding. Polar Vs. Nonpolar Covalent Bonds. Ionic or Covalent? Identifying Bond Types. Solutions + -
Chemical Bond Mutual attraction between the nuclei and valence electrons of different atoms that binds them together. Bonding onors Chemistry 412 Chapter 6 Types of Bonds Ionic Bonds Force of attraction
CHEMISTRY 112 LECTURE EXAM II Material
CHEMISTRY 112 LECTURE EXAM II Material Part I Chemical Bonding I Lewis Theory Chapter 9 pages 376-386 A. Drawing electron dot structures HOW TO: 1. Write e- dot structure for the individual atoms. 2. a)
SHAPES OF MOLECULES (VSEPR MODEL)
1 SAPES MLEULES (VSEPR MDEL) Valence Shell Electron-Pair Repulsion model - Electron pairs surrounding atom spread out as to minimize repulsion. - Electron pairs can be bonding pairs (including multiple
Assignment 09 A. 2- The image below depicts a seesaw structure. Which of the following has such a structure?
Assignment 09 A 1- Give the total number of electron domains, the number of bonding and nonbonding domains, and the molecular geometry, respectively, for the central atom of P 3. a) four electron domains,
LESSON 10. Glossary: Molecular Geometry. a quantitative measure of the degree of charge separation in a molecule. Dipole moment
LESSON 10 Glossary: Molecular Geometry Dipole moment Electronegativity Molecular geometry Pi bond Polar covalent bond Sigma bond Valence-shell electronpair repulsion (VSEPR) model a quantitative measure
Ch. 9- Molecular Geometry and Bonding Theories
Ch. 9- Molecular Geometry and Bonding Theories 9.0 Introduction A. Lewis structures do not show one of the most important aspects of molecules- their overall shapes B. The shape and size of molecules-
Chapter 9. Molecular Geometry and Bonding Theories
Chapter 9 Molecular Geometry and Bonding Theories MOLECULAR SHAPES 2 Molecular Shapes Lewis Structures show bonding and lone pairs do not denote shape Use Lewis Structures to determine shapes Molecular
CHAPTER 5: Bonding Theories - Explaining Molecular Geometry. Chapter Outline
CHAPTER 5: Bonding Theories - Explaining Molecular Geometry Chapter Outline 5.1 Molecular Shape 5.2 Valence-Shell Electron-Pair Repulsion Theory (VSEPR) 5.3 Polar Bonds and Polar Molecules» What Makes
Molecular Geometry and Bonding Theories. Molecular Shapes. Molecular Shapes. Chapter 9 Part 2 November 16 th, 2004
Molecular Geometry and Bonding Theories Chapter 9 Part 2 November 16 th, 2004 8 Molecular Shapes When considering the geometry about the central atom, we consider all electrons (lone pairs and bonding
CHEMICAL BONDING. Chemical Bonds. Ionic Bonding. Lewis Symbols
CHEMICAL BONDING Chemical Bonds Lewis Symbols Octet Rule whenever possible, valence electrons in covalent compounds distribute so that each main-group element is surrounded by 8 electrons (except hydrogen
Lecture Presentation. Chapter 10 Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory
Lecture Presentation Chapter 10 Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory Predicting Molecular Geometry 1. Draw the Lewis structure. 2. Determine the number
Fill in the chart below to determine the valence electrons of elements 3-10
Chemistry 11 Atomic Theory IV Name: Date: Block: 1. Lewis Diagrams 2. VSEPR Lewis Diagrams Lewis diagrams show the bonding between atoms of a molecule. Only the outermost electrons of an atom (called electrons)
SMK SULTAN ISMAIL JB, NUR FATHIN SUHANA BT AYOB
SMK SULTAN ISMAIL JB, NUR FATHIN SUHANA BT AYOB POLAR AND NON POLAR BONDS BOND POLARITY 1. Atoms with different electronegative from polar bonds (difference in EN) 2. Depicted as polar arrow : 3. Example
Electron Geometry Hybrid Orbitals
Molecular Shape and Hybridized Orbitals CH2000: Introduction to General Chemistry, Plymouth State University Introduction: In chemistry, the three dimensional shape of a molecule is as important as the
I. Multiple Choice Questions (Type-I)
I. Multiple Choice Questions (Type-I) 1. Isostructural species are those which have the same shape and hybridisation. Among the given species identify the isostructural pairs. (i) [NF 3 and BF 3 ] [BF
CHEMISTRY - ZUMDAHL 2E CH.4 - MOLECULAR STRUCTURE AND ORBITALS.
!! www.clutchprep.com CONCEPT: ELECTRONIC GEOMETRY When drawing a compound you have to take into account two different systems of geometrical shape. The simpler system known as electronic geometry or shape
PART 3 Chemical Bonds, Valence Bond Method, and Molecular Shapes. Reference: Chapter 9 10 in textbook
PART 3 Chemical Bonds, Valence Bond Method, and Molecular Shapes Reference: Chapter 9 10 in textbook 1 Valence Electrons Valence ae Electron Define: the outer shell electrons Important for determination
VSEPR Theory, Valence Bond Theory, Characteristic of Covalent Compounds 1. Which of the following is not correct? 1. A sigma bond is weaker than pi bond. 2. A sigma bond is stronger than pi bond.. A double
Chapter 4. Molecular Structure and Orbitals
Chapter 4 Molecular Structure and Orbitals Chapter 4 Table of Contents (4.1) (4.2) (4.3) (4.4) (4.5) (4.6) (4.7) Molecular structure: The VSEPR model Bond polarity and dipole moments Hybridization and
Chemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals
Chemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals 1 Chemical Bonding II Molecular Geometry (10.1) Dipole Moments (10.2) Valence Bond Theory (10.3) Hybridization of Atomic Orbitals
5 Polyatomic molecules
s manual for Burrows et.al. Chemistry 3 Third edition 5 Polyatomic molecules Answers to worked examples WE 5.1 Formal charges in N 2 (on p. 221 in Chemistry 3 ) Use formal charges to decide whether oxygen
Chapter 10. Structure Determines Properties! Molecular Geometry. Chemical Bonding II
Chapter 10 Chemical Bonding II Structure Determines Properties! Properties of molecular substances depend on the structure of the molecule The structure includes many factors, including: the skeletal arrangement
(A) 1 bonding pair (B) 1 bonding pair and 1 lone pair (C) 2 bonding pairs (D) 2 bonding pairs and 2 lone pairs
AP Chemistry - Problem Drill 13: Lewis Structures and VSPER No. 1 of 10 1. Lewis structure is used to model covalent bonds of a molecule or ion. Covalent bonds are a type of chemical bonding formed by