Localized Electron Model
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1 Localized Electron Model
2 Models for Chemical Bonding Localized electron model (Valence bond model) Molecular orbital model
3 Localized Electron Model Useful for explaining the structure of molecules especially nonmetals bonded to nonmetals
4 Localized electron model Electron pair can be shared when halffilled orbital of one atom overlaps with half-filled orbital of another. δ Bond: orbitals overlap along the internuclear axis π Bond: side by side overlap of orbitals parallel to the internuclear axis
5 Potential energy 0 Distance of separation
6 As the atoms approach each other, each electron is attracted by the nucleus of the other atom; at the same time, the electrons repel each other, as do the nuclei
7 δ Bond in H 2 s H H s H H δ
8 H2
9 δ Bond in HF H F 1s 2p H F
10 F2
11 Structure of Methane (CH 4 ) structure of methane seems inconsistent with electron configuration of carbon
12 carbon only two unpaired electrons 2p Carbon Should form δ bonds with 2s only two Hydrogen atoms?
13 Hybridization of Atomic Orbitals
14 Hybrid orbitals atomic orbitals obtained when two or nonequivalent orbitals of the same atom combine in preparation for covalent bond formation
15 sp 3 Hybridization
16 sp 3 Hybridization Promote an electron from the 2s to the 2p orbital 2p 2p 2s 2s
17 sp 3 Hybridization Mix together (hybridize) the 2s orbital and the three 2p orbitals 2p 2 sp 3 2s
18 sp 3 Hybridization Mix together (hybridize) the 2s orbital and the three 2p orbitals 2 sp 3
19
20 Shapes of orbitals s p sp 3
21 δ Bond in CH 4 H C s sp 3 δ C H H C
22
23 Justification for Orbital Hybridization The model is consistant with structure of methane Allows for the formation of more bonds (4 rather than 2) Bonds involving sp 3 orbitals are stronger than s-s overlap or p-p overlap
24 Remember Four electron pairs = tetrahedral arangement of those electron pairs = sp 3 hybridization
25 Four electron pairs tetrahedral arrangement of electron pairs N : : C : S
26 NH 3 : N 2 sp 3
27 sp Hybridization
28 Beryllium chloride ( BeCl 2 ) Promote an electron from the 2s to the 2p orbital 2p 2p 2s 2s
29 Beryllium chloride ( BeCl 2 ) Mix together (hybridize) the 2s orbital and one 2p orbitals 2p 2s
30 Beryllium chloride ( BeCl 2 ) Mix together (hybridize) the 2s orbital and one 2p orbitals 2p 2sp
31 The Be Cl δ Bond in BeCl p Cl Be sp Be Cl Cl Be
32 The Be Cl δ Bond in BeCl p Cl Be sp Cl Be Cl
33 sp 2 Hybridization
34 Boron trifloride Promote an electron from the 2s to the 2p orbital 2p 2p 2s 2s
35 Boron trifloride Mix together (hybridize) the 2s orbital and two 2p orbitals 2p 2s
36 Boron trifloride Mix together (hybridize) the 2s orbital and two 2p orbitals 2p 2 sp 2
37 F B Boron trifloride
38 F F B Boron trifloride F
39 Hybridizing Atomic Orbitals hybrid orbitals are used only for atoms in a molecule, not for isolated atoms hybrid orbitals are different in shape from the atomic orbitals from which we derive them number of hybrid orbitals equals number of atomic orbitals from which they were generated hybridization permits more bonds and stronger bonds covalent bond results from overlap of half-filled orbitals
40 Procedure For Hybridizing Atomic Orbitals draw the Lewis structure of the molecule predict the overall arrangement of the electron pairs using the VSEPR model deduce the hybridization of the central atom
41 SF 6 PF 5
42 Hybridization of s, p, and d Orbitals Beginning with the third period of the periodic table 1 3s orbital + 3 3p orbital + 1 3d orbital gives sp 3 d Permits five electron pairs ( trigonal bipyramidal ) 1 3s orbital + 3 3p orbital + 2 3d orbital gives sp 3 d 2 Permits six electron pairs ( octahedral )
43 π -Bonds
44 Review :Valence bond model Electron pair can be shared when the half-filled orbital of one atom overlaps with half-filled orbital of another. δ Bond: orbitals overlap along the internuclear axis π Bond: side by side overlap of orbitals
45 Structure of Ethylene C 2 H 4 CH 2 CH 2 planar Bond angle 120 Requires hybridization different from sp 3
46 Orbital Hybridization Promote an electron from the 2s to the 2p orbital 2p 2p 2s 2s
47 Orbital Hybridization Mix together (hybridize) the 2s orbital and the two 2p orbitals 2p 2s
48 Orbital Hybridization Mix together (hybridize) the 2s orbital and the two 2p orbitals 2p 2 sp 2
49 Lewis model : Ethylene H π Bond H C C H δ Bond H The carbon-carbon double bond of ethylene is a combination of an δ Bond and πbond
50 π Bonding in Ethylene 2 sp 2
51 π Bonding in Ethylene 2p sp 2
52 π Bonding in Ethylene
53 π Bonding in Ethylene
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