Chapter 9 Molecular Geometries. and Bonding Theories
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1 Chapter 9 Molecular Geometries and Bonding Theories
2 Coverage of Chapter 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
3 MOLECULAR SHAPES The shape of a molecule plays an important role in its reactivity. By knowing the number of bonding and nonbonding electron pairs we can predict the shape of the molecule.
4 Two (2) Theories for MOLECULAR GEOMETRY 1. Valence Shell Electron Pair Repulsion (VSEPR) THEORY & 2. The Valence Bond (VB) THEORY
5 Lewis Structures & Formal Charge Formal charge is a charge assigned to each atom in a Lewis structure that helps to distinguish among competing structures.
6 What is the correct formula for Hypo Chlorous Acid HClO (aq) H Cl O or H O Cl
7 Hypo chlorite ion ClO - O Cl Number of Valence e - Number of Nonbonding e - ½ Number of Bonding e - Formal Charge
8 Where does the H go on HClO? O Cl H or H O Cl Valence e - Nonbonding e - ½ Bonding e - O Cl O Cl
9 Electron pairs are refered to as electron domains Single, double or triple bonds all count as one electron domain. The atom A in this molecule, has four electron domains.
10 The First MOLECULAR GEOMETRY theory (VSEPR) Valence Shell Electron Pair Repulsion theory
11 VSEPR Theory 1. To predict molecular shape, assume the valence electrons repel each other 2. The electrons adopt an arrangement in space to minimize e - e - repulsion 3. The molecule adopts whichever 3D geometry minimized this repulsion.
12 What Determines the Shape of a Molecule? Four electron domains on N 3 bonding and 1 nonbonding
13 What Determines the Shape of a Molecule? Electrons, whether they be bonding or nonbonding, repel each other. So electrons are placed as far as possible from each other
14 Two (2) Different Types of Molecules 1. Molecules with NO nonbonding electrons on the central atom 2. Molecules with nonbonding electrons on the central atom
15 Electron Domains & NonBonding Electrons Example 1 CO 2 O = C = O How many electron domains on C How many NonBonding electrons on C 2 0
16 Electron Domains & NonBonding Electrons Example 2 H 2 O.. H O H How many electron domains on O How many NonBonding electrons on O 4 4
17 Molecular Geometries for molecules with no nonbonding electrons on central atom There are five fundamental geometries : 1. Linear 2. Trigonal Planar 3. Tetrahedral 4. Trigonal bepyramidal 5. Octahedral
18
19 Only consider Three in detail 1. Linear 2. Trigonal Planar 3. Tetrahedral
20 In order to determine geometry First Draw Lewis Dot Formula
21 MOLECULES IN WHICH THE CENTRAL ATOM HAS NO LONE PAIRS ZINC CHLORIDE Zn Cl 2 Zn (30) [Ar] 3d 10 4s 2 Cl Zn - Cl B A B AB 2 = LINEAR
22 AB 2 Molecules Such as CO 2 are Linear (Molecules With NO UnPaired Electrons On the Central Atom).... : O = C = O : B A B
23 Molecular Shape and Molecular Polarity
24 AB 3 Molecules Such as BF 3 are Planar (Molecules With NO UnPaired Electrons On the Central Atom) Formula B F 3 Number of Valence e = 24 total Lewis Structure F B F F
25 AB 3 (Molecules With NO UnPaired Electrons On the Central Atom) Such as BF 3 are Planar
26 AB 4 Molecules Such as CH 4 are Tetrahedral (Molecules With NO UnPaired Electrons On the Central Atom) Formula C H 4 Number of Valence e = 8 total H Lewis Structure H C H H
27 AB 4 Such as CH 4 are Tetrahedral (Molecules With NO UnPaired Electrons On the Central Atom)
28 AB 4 Molecules Such as CCl 4 are Tetrahedral Carbon TetraChloride
29 AB 5 Such as PCl 5 are Triangular bipyramidal Name? Number of Bonds? Lewis dot structure? Cl Cl P Cl Cl Cl
30 AB 6 Such as SF 6 are Octahedral Name? Number of Bonds? Lewis dot structure?
31 Molecules With NO UNPaired e-
32 Molecules with NO unpaired e - on Central Atom 1. 2 Bonds AB 2 or AX e.g. CO Bonds... AB 3 or AX e.g. BF Bonds AB 4 or AX e.g. CH Bonds... AB 5 or AX e.g. PCl Bonds... AB 6 or AX e.g. SF 6 6
33 Polarity
34 Part 2. of VSEPR Theory CENTRAL ATOM HAS LONE PAIRS
35 Molecules With UnPaired Electrons On the Central Atom Class Example Geometry AB 2 E SO 2 & O 3 AB 2 E 2 H 2 O AB 3 E NH 3 Bent Bent Trigonal pyramidal
36 1. AB 2 E OZONE O O O O O O 2. AB 2 E 2 WATER
37 AB 2 E 2 (Molecules With UnPaired Electrons On the Central Atom) Such as H 2 O are Bent
38 3. AB 3 E AMMONIA
39 AB 3 E (Molecules With UnPaired Electrons On the Central Atom) Such as NH 3 are NOT Planar
40 Predict Molecular Shapes 1. SiCl 4 2. CH 2 Cl 2 3. GeCl 2 4. OF 2 5. NH 3 6. PH 3
41 Give the electron domain and molecular geometries for (a) N 2 O (b) SO 3 (c) PCl 3 (d) NH 2 Cl electron domain molecular geometry
42 Examples of AB 2 molecules Linear AB 2 How many bonds CO 2 Bent AB 2 E How many bonds SO 2 and NO 2 - Bent AB 2 E 2 How many bonds H 2 O
43 Examples of AB 3 molecules Planar AB 3 How many bonds BF 3 Pyramidal AB 3 E How many bonds NH 3 T shape AB 3 E 2 How many bonds ClF 3
44
45 Two (2) Theories for MOLECULAR GEOMETRY 1. Valence Shell Electron Pair Repulsion (VSEPR) THEORY Now consider 2. The Valence Bond (VB) THEORY
46 Method uses molecular orbitals not Atomic Orbitals WHAT IS A MOLECULAR ORGITAL? Orbitals used in bonding of Molecules
47 CH 4 as an EXAMPLE Ground State Electron Configuration C (6 e - ) 1s 2 2s 2 2p 2 = ( ) ( ) ( ) ( ) ( ) Only place for two bonds to form Therefore would predict CH 2 formation and not CH 4 But CH 2 does not exist while CH 4 does
48 C (6 e - ) 1s 2 2s 2 2p 2 = ( ) ( ) ( ) ( ) ( ) Only place for two bonds to form Excited State Electron Configuration C (6 e - ) 1s 2 2s 1 2p 3 = ( ) ( ) ( ) ( ) ( ) Now a place for four bonds One electron from H goes into an s orbital and Three from H go into the p orbitals
49 The BONDS in CH 4 are ALL the SAME! One electron in an s orbital and Three in p orbitals would create different bonds. Since All the Bonds are Equal, this cannot be correct INTRODUCE THE CONCEPT OF HYBRIDIZATION
50 Hybridization In order to made All Bonding sites equal, we must create NEW Orbitals. s, p, d, f are ATOMIC ORBITALS MOLECULAR ORBITALS are formed from Atomic orbitals
51 VALENCE SHELL ORBITALS HYBRIDIZE THE ORIENTATION OF ALL HYBRID VALENCE SHELL ORBITALS DETERMINES THE GEOMETRY OF THE MOLECULE
52 are formed from ATOMIC ORBITALS Atomic Orbitals one S + one P one S + two P one S + three P Molecular Orbitals Two (2) SP Three (3) SP 2 Four (4) SP 3
53 They are called SP SP 2 SP 3 SP 3 d and SP 3 d 2
54 sp 3 HYBRIDIZATION TETRAHEDRAL Bond Angles 109½ o Methane CH 4 Four σ Bonds on C
55 sp 2 HYBRIDIZATION
56 sp HYBRIDIZATION one S orbital + one P orbital
57 Carbon is NOT The Only Element That Undergoes sp 3 HYBRIDIZATION
58 In CH 3 COOH, there are three (3) hybridized atoms. Geometry is assign about each hybridized atom separately.
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