Chemical Bonding 4.8. Valence Bond Theory Hybrid Orbital Theory Multiple Bonds High School Chem Solutions. All rights reserved.
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1 Chemical Bonding 4.8 Valence Bond Theory Hybrid Orbital Theory Multiple Bonds
2 Valence Bond Theory Combines Lewis theory of filling octets by sharing pairs of electrons with the electron configuration of atomic orbitals. Valence Bond Theory states that bonding occurs when atomic orbital overlap.
3 Building BF 3 with Valence Bond Theory B: F: 1s 2s 2p 1s 2s 2p
4 Building BF 3 with Valence Bond Theory B: 1s 2s 2p Boron enters an excited state where an electron from the 2s orbital is promoted to the 2p y orbital.
5 Valence Bond Theory has problems with the shape F 2p y 2p x Valence Bond Theory Views bonding as an overlapping of atomic orbitals. B F 2s F Gets the bond angle wrong
6 Problems with Valence Bond Theory and BF 3 Problem (the bond angle is wrong) Valence Bond Theory says 90 o and a random angle for the fluorine bonded to the s-orbital. VSEPR theory says 120 o Solution (Hybrid Orbitals) When the electron is promoted, the 2s, 2p x, and 2p y orbitals of boron morph into three separate sp 2 hybrid orbitals that are identical in shape and size.
7 sp 2 Hybrid Orbitals F sp 2 sp 2 sp 2 F F The 2s and two 2p orbitals morph into three identical sp 2 hybrid orbitals
8 sp 2 Hybrid Orbitals sp 2 s + + p = p sp 2 sp 2
9 sp 3 Hybrid Orbitals (e.g. CH 4 ) H: C: 1s 1s 2s 2p
10 sp 3 Hybrid Orbitals (e.g. CH 4 ) H: 1s C: 1s 2s 2p Hybridization of Carbon C: 1s sp 3
11 sp 3 Hybrid Orbitals (e.g. CH 4 ) H sp 3 Bond Angle = o H sp 3 sp 3 sp 3 H H
12 Valence Bond Theory and Lone Pairs (e.g. H 2 O) Building H 2 O with Valence Bond Theory O: H: H: 1s 2s 2p 1s 1s Oxygen could accept one electron from one Hydrogen in its p y orbital and another from the other Hydrogen in its p z orbital.
13 Valence Bond Theory and Lone Pairs (e.g. H 2 O) Valence Bond Theory views bonding as an overlapping of atomic orbitals. p y H p y p z p x p z p x H Valence Bond Theory get the angle wrong again!
14 Problems with Valence Bond Theory in the H 2 O Example The bond angle is wrong. Valence Bond Theory predicts 90 o VSEPR Theory predicts o The orbital shape must be wrong. Shared electrons are not spending enough time with the Hydrogen.
15 Hybrid Orbital Theory and Lone Pairs (e.g. H 2 O) O: H: H: 1s 1s 1s sp 3 Electrons are not promoted here, but every orbital in the n = 2 energy level becomes hybridized.
16 sp 3 Hybrid Orbitals (H 2 O) sp 3 sp 3 sp 3 H Four sp 3 hybrid orbitals are formed sp 3 H Bond Angle = o
17 Hybrid Orbital Theory and 5 Charge Clouds! (e.g. PCl 5 ).. :Cl.. :Cl:.... :Cl:.. P Cl:.. :Cl:..
18 sp 3 d Hybrid Orbitals Atomic Orbitals P: 3s 3p 3d Promotion P: 3s 3p 3d Hybridization P: sp 3 d
19 Hybrid Orbital Theory and 6 Charge Clouds! (e.g. SF 6 ) :Ḟ... :F:.... :F: S :F:.... F:.. :F:..
20 sp 3 d 2 Hybrid Orbitals Atomic Orbitals S: 3s 3p 3d Promotion S: 3s 3p 3d Hybridization S: sp 3 d 2
21 Summary Charge Clouds Hybridization 2 sp 3 sp 2 4 sp 3 5 sp 3 d 6 sp 3 d 2
22 Double Bonds (e.g. C 2 H 4 ) H H C C H H Each carbon has 3 charge clouds. sp 2 hybrid orbitals
23 Double Bonds (e.g. C 2 H 4 ) Atomic Orbitals C: 2s 2p Promotion C: 2s 2p Hybridization C: sp 2 2p
24 Double Bond (C 2 H 4 ) H p sp 2 H H sp 2 sp 2 sp 2 σ Bond sp 2 p sp 2 H π Bond
25 Triple Bonds (e.g. C 2 H 2 ) H C C H Each carbon has two charge clouds. sp hybrid orbitals
26 Triple Bonds (e.g. C 2 H 2 ) Atomic Orbitals C: 2s 2p Promotion C: 2s 2p Hybridization C: sp 2p
27 Triple Bond (C 2 H 2 ) p σ Bond p sp p sp sp p sp Two π Bonds
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