CHEMISTRY. Chapter 10 Theories of Bonding and Structure. The Molecular Nature of Matter. Jespersen Brady Hyslop SIXTH EDITION
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1 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.
2 Molecular Structures Molecules containing three or more atoms may have different shapes Shapes are made from five basic geometrical structures Three theories explain molecular structures: Valence Shell Electron Pair Repulsion (VSEPR) Valence Bond (VB) Molecular Orbital (MO) 2
3 VSEPR Model Valence Shell Electron Pair Repulsion Simple model using the electron domain concept Two types of electron domains Bonding domains Electron pairs involved in bonds between two atoms Nonbonding domains Electron pairs associated with single atom All electrons in single, double, or triple bond considered to be in the same electron domain 3
4 Five Basic Electron Domains Electron Domains Shape Electron Pair Geometry 2 linear 3 trigonal planar 4 tetrahedral 4
5 Five Basic Electron Domains (con t.) Electron Domains Shape Electron Pair Geometry 5 trigonal bipyramidal has equatorial and axial positions. 5
6 Five Basic Electron Domains (con t.) Electron Domains Shape Electron Pair Geometry 6 octahedral All positions are equivalent 6
7 Structures Based on Three Electron Domains Number of Bonding Domains 3 Number of Nonbonding Domains 0 Structure Molecular Shape Planar Triangular (e.g. BCl 3 ) All bond angles Nonlinear Bent or V-shaped (e.g. SO 2 ) Bond <120 7
8 Four Electron Domains Number of Bonding Domains 4 Number of Nonbonding Domains 0 Structure Molecular Shape Tetrahedron (e.g. CH 4 ) All bond angles Trigonal pyramid (e.g. NH 3 ) Bond angle less than Nonlinear, bent (e.g. H 2 O) Bond angle less than
9 Trigonal Bipyramid Two atoms in axial position 90 to atoms in equatorial plane Three atoms in equatorial position 120 bond angle to atoms in axial position 9
10 Five Electron Domains Number of Bonding Domains 5 Number of Nonbonding Domains 0 Structure Molecular Shape Trigonal bipyramid (e.g. PF 5 ) Ax-eq bond angles 90 Eq-eq Distorted Tetrahedron, or Seesaw (e.g. SF 4 ) Ax-eq bond angles < 90 10
11 Best Place for Lone Pairs Lone pair takes up more space Goes in equatorial plane Pushes bonding pairs Result: distorted tetrahedron 11
12 Number of Bonding Domains 3 Five Electron Domains Number of Nonbonding Domains 2 Structure Molecular Shape T-shape (e.g. ClF 3 ) Bond angles Linear (e.g. I 3 ) Bond angles
13 Six Electron Domains Number of Bonding Domains 6 Number of Nonbonding Domains 0 Structure Molecular Shape Octahedron (e.g. SF 6 ) 5 1 Square Pyramid (e.g. BrF 5 ) 13
14 Structures Based on Six Electron Domains Number of Bonding Domains 4 Number of Nonbonding Domains 2 Structure Molecular Shape Square planar (e.g. XeF 4 ) 14
15 Relative Sizes of Electron Bonding domains More oval in shape Electron density focused between two positive nuclei. Nonbonding domains More bell or balloon shaped Take up more space Domains Electron density only has positive nucleus at one end 15
16 Steps Used to Determine Three Dimensional Structures: 1. Draw Best Lewis Structure of Molecule If several resonance structures exist, pick only one 2. Count electron pair domains Lone pairs and bond pairs around central atom Multiple bonds count as one set (or one effective pair domain) 16
17 Steps Used to Determine Three Dimensional Structures (Cont.) 3. Arrange electron pair domains to minimize repulsions Lone pairs Require more space than bonding pairs May slightly distort bond angles from those predicted. In trigonal bipyramid lone pairs are equatorial In octahedron lone pairs are axial 4. Name molecular structure based on position of atoms only bonding electrons 17
18 Electron Geometry and Molecular Geometry Electron Domains Electron Geometry Molecular Geometries 2 Linear Bond angles Trigonal planar Bond angles Tetrahedral Bond angles Trigonal Bipyramidal Bond angles 90 and Linear - Trigonal planar - Nonlinear (bent) - Tetrahedral - Trigonal pyramidal - Nonlinear (bent) - Trigonal Bipyramidal - Distorted Tetrahedral (Seesaw) - T-shape - Linear 6 Octahedral - Octahedral Bond angles 90 - Square Pyramidal - Square Planar 18
19 Learning Check Identify for each of the following: 1. Number of bonding versus nonbonding domains 2. Molecular geometry/molecular structure H N H H I H H O I I 19
20 Your Turn! For the species, ICl 5, how many bonding domains exist? A. 2 B. 3 C. 4 D. 5 20
21 Your Turn! For the species, ICl 5, how many non-bonding domains exist? A. 4 B. 3 C. 2 D. 1 21
22 Your Turn! For the species, ICl 5, what is the electron domain geometry? A. trigonal planar B. tetrahedron C. trigonal bipyramid D. octahedron 22
23 Your Turn! For the species, ICl 5, what is the molecular geometry? A. trigonal bipyramid B. trigonal planar C. distorted tetrahedron D. square pyramid 23
24 Polar Molecules Have net dipole moment Negative end Positive end Polar molecules attract each other. Positive end of polar molecule attracted to negative end of next molecule. Strength of this attraction depends on molecule's dipole moment Dipole moment can be determined experimentally 24
25 Polar Molecules Polarity of molecule can be predicted by taking vector sum of bond dipoles Bond dipoles are usually shown as crossed arrows, where arrowhead indicates negative end 25
26 Molecular Shape and Molecular Polarity Many physical properties (melting and boiling points) affected by molecular polarity For molecule to be polar: Must have net dipole Many molecules with polar bonds are nonpolar Certain arrangements of bond dipoles cancel 26
27 Molecular Polarity Symmetrical molecules Nonpolar because bond dipoles cancel All five shapes are symmetrical when all domains attached to them are composed of identical atoms 27
28 Cancellation of Bond Dipoles In Symmetrical Trigonal Bipyramidal and Octahedral Molecules 28
29 Molecular Polarity Molecule is usually polar if All atoms attached to central atom are NOT same or, There are one or more lone pairs on central atom 29
30 Molecular Polarity Water and ammonia both have non-bonding domains Bond dipoles do not cancel Molecules are polar 30
31 Molecular Polarity No net dipole Nonpolar molecule Nonbonding domains (lone pairs) are symmetrically placed around central atom 31
32 Your Turn! Which of the following molecules is polar? A. BClF 2 B. BF 3 C. CH 4 D. CO 2 E. C 2 H 2 32
33 Valence Bond Theory Individual atoms have their own orbitals. Orbitals overlap to form bonds Extent of overlap of atomic orbitals is related to bond strength Overlapped atomic orbitals will share two pair of electrons with paired (opposite) spins Orbital may mix or hybridize to explain certain molecular shapes. 33
34 Valence Bond Theory H 2 H 2 bonds form because 1s atomic valence orbital from each H atom overlaps Orbital overlap define a Sigma ( ) bond Sigma ( ) bond concentrate electron density between nuclei of two atoms Sigma ( ) bond contains 2 paired electrons (opposite spins) 34
35 Valence Bond Theory F 2 F 2 bond - atomic valence orbitals of F overlap 2p overlaps with 2p a bond Sigma ( ) bond contains 2 paired electrons (opposite spins) Same for all halogens, but different np orbitals 35
36 Valence Bond Theory HF HF involves overlaps between 1s orbital on H and 2p orbital of F Form a bond containing 2 paired electrons (opposite spins) 1s 2p 36
37 Valence Bond Theory and H 2 S Unpaired electrons in S and H are free to form paired bond H S bond forms between s and p orbital Predicted 90 bond angle is very close to experimental value of
38 Difficulties With Valence Bond Theory Example: CH 4 C: 1s 2 2s 2 2p 2 and H: 1s 1 In methane, CH 4 All four bonds are the same Bond angles are all Carbon atoms have All paired electrons except the two unpaired 2p p orbitals are 90 apart Atomic orbitals predict CH 2 with 90 angles 38
39 Hybridization Mixing of atomic orbitals to allow formation of bonds that fit experimental bond angles. Hybridization mixing of wave functions. New hybrid orbital set will hold electrons Bonds will tend to get maximum possible overlap 39
40 New Names for These New Orbitals Symbols for hybrid orbitals combine the symbols of the orbitals used to form them s + p s + p + p form two sp hybrid orbitals form three sp 2 hybrid orbitals One type of atomic orbital is used for each hybrid orbital formed Sum of exponents in hybrid orbital notation must add up to number of atomic orbitals used 40
41 Let s See How Hybridization Works Mixing or hybridizing s and p orbital of same atom results in two sp hybrid orbitals Two sp hybrid orbitals point in opposite directions 41
42 Using sp Hybrid Orbitals to Form Bonds Now have two sp hybrid orbitals Oriented in correct direction for bonding 180 bond angles As predicted by VSEPR Verified by experiment Bonding = Overlap of H 1s atomic orbitals with sp hybrid orbitals on Be 42
43 Ex: BeH 2 Experiment and VSEPR show that BeH 2 (g) is linear bond angle Be must have Two hybrid orbitals pointing in opposite directions to give correct bond angle Each Be orbital must contain one electron Each resulting bond with H contains only two electrons Each H supplies one electron 43
44 Hybrid Orbitals Two sp hybrids Linear Three sp 2 hybrids All angles 120 Trigonal Planar Four sp 3 hybrids All angles Tetrahedral 44
45 Expanded Octet Hybrid Orbitals 45
46 Hybrid Orbitals Hybrid Atomic Orbitals Used sp s + p Linear Electron Geometry Bond angles 180 sp 2 s + p + p Trigonal planar Bond angles 120 sp 3 s + p + p + p Tetrahedral Bond angles sp 3 d s + p + p + p + d Trigonal Bipyramidal Bond angles 90 and 120 sp 3 d 2 s + p + p + p + d + d Octahedral Bond angles 90 46
47 Double and Triple Bonds Formed from two types of bond that result from orbital overlap Sigma ( ) bond Accounts for first bond Pi ( ) bond Accounts for second and third bonds 47
48 Sigma ( ) Bonds Formed by head-on overlap of orbitals that lie along imaginary line joining their nuclei Concentrate electron density mostly between nuclei of two atoms s + s p + p sp + sp 48
49 Pi ( ) Bonds Sideways overlap of unhybridized p orbitals Electron density divided into two regions Lie on opposite sides of imaginary plane connecting nuclei of two atoms Electron density above and below bond. 49
50 Properties of -Bonds Can t rotate about double bond bond must first be broken before rotation can occur 50
51 Bonding in BCl 3 Overlap of each halffilled 3p orbital on Cl with each half-filled sp 2 hybrid on B Forms three equivalent bonds Trigonal planar shape 120 bond angle sp 2 2p 51
52 Bonding in CH 4 Overlap of each halffilled 1s orbital on H with each half-filled sp 3 hybrid on carbon Forms four equivalent bonds Tetrahedral geometry bond angle sp 3 52
53 Your Turn! What is the hybridization of oxygen in OCl 2? A. sp B. sp 3 C. sp 2 D. sp 3 d 53
54 Hybridization in Molecules That Have Lone Pair Electrons CH 4 sp 3 tetrahedral geometry bond angle NH bond angle H 2 O bond angle Angles suggest that NH 3 and H 2 O both use sp 3 hybrid orbitals in bonding Not all hybrid orbitals used for bonding e Lone pairs can occupy hybrid orbitals Lone pairs must always be counted to determine geometry 54
55 Hybridization in Molecules That Have Lone Pair Electrons NH 3 2s 2p hybridize form bonds lone pair sp 3 bonding electrons 55
56 Hybridization in Molecules that Have Lone Pair Electrons H 2 O 2s 2p hybridize form bonds lone pairs sp 3 bonding electrons 56
57 Your Turn! For the species ClF 2+, determine the following: 1. electron domain geometry 2. molecular geometry A. tetrahedron, trigonal planar B. pentagon, tetrahedron C. tetrahedron, bent D. trigonal planar, bent 57
58 Your Turn! For the species ClF 2+, determine the following: 1. hybridization around the central atom 2. polarity A. sp 2, polar B. sp 3, non-polar C. sp 3, polar D. sp 2, non-polar 58
59 Your Turn! For the species XeF 4 O (Xe is central atom), determine the following: 1. electron domain geometry 2. molecular geometry A.octahedral, square pyramidal B.trigonal bipyramidal, distorted tetrahedral C.square pyramidal, octahedral D.trigonal bipyramidal, planar 59
60 Your Turn! For the species XeF 4 O, determine the following: 1. hybridization around the central atom 2. the molecular polarity A. sp 3 d, polar B. sp 3 d 2, polar C. sp 3 d, nonpolar D. sp 3 d 2, nonpolar 60
61 Bonding in Ethene (C 2 H 4 ) Each carbon is sp 2 hybridized (violet) has one unhybridized p orbital (red) C=C double bond is one bond (sp 2 sp 2 ) one bond (p p) p p overlap forms a C C bond 61
62 Bonding in Formaldehyde C and O each sp 2 hybridized (violet) Has one unhybridized p orbital (red) H H C O C=O double bond is one bond (sp 2 sp 2 ) one bond (p p) 62
63 N N triple bond one bond sp sp two bonds p x p x p y p y Bonding in N 2 Each nitrogen sp hybridized (violet) Has two unhybridized p orbitals, p x and p y (red) 63
64 H Bonding in Ethyne (Acetylene) C C H Each carbon is sp hybridized (violet) Has two unhybridized p orbitals, p x and p y (red) C C triple bond one bond sp sp two bonds p x p x p y p y 64
65 Benzene, In Valence Bond Terms Can write benzene as two resonance structures But actual structure is resonance hybrid Electrons are delocalized Have three pairs of electrons delocalized over six C atoms Extra stability is resonance energy Functionally, resonance and delocalization energy are the same thing 65
66 Benzene Six C atoms, each sp 2 hybridized (3 bonds) Each C also have one unhybridized p orbital (6 total) So three bonds 66
67 Your Turn! How many and bonds are there in CH 2 CHCHCH 2, and what is the hybridization around the carbon atoms? A. 7, 1, sp B. 8, 2, sp 3 C. 9, 2, sp 2 D. 9, 3, sp 2 E. 8, 2, sp 67
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