8-2.4 Hybrid Orbital Theory

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Presentation transcript:

8-2.4 Hybrid Orbital Theory Ⅰ. The Central Themes of Hybridization Theory Hybridization is the process of mixing the atomic orbitals in an atom (usually the central atom) to generate a set of new atomic orbitals.

(2) The new atomic orbitals are called hybrid orbitals. Hybrid orbital is atomic orbitals obtained when two or more nonequivalent orbitals of the same atom combine, are then used to form covalent bonds. (3) The number of hybrid orbitals generated is equal to the number of atomic orbitals. (4) The spatial orientation of these new orbitals lead to more stable bonds and are consistent with the observed molecular shapes.

The following points are useful for an understanding of hybridization The concept of hybridization does not apply to isolated atoms. It is used only to explain a bonding scheme in a molecule. (2) Hybrid orbital is not a pure atomic orbital. Hybrid orbitals have very different shapes from pure atomic orbitals.

(3) All the hybrid orbitals are equivalent in every respect, except in their relative orientations in space. (4) Covalent bonds in polyatomic molecules are formed by the overlap of a hybrid orbital and a pure atomic orbital, or of two hybrid orbitals.

Ⅱ. Types of Hybrid Orbitals 1. sp Hybridization One s orbital and one p orbital form two sp hybrid orbital Hybridization of all s orbital and a p orbital (of the same atom) produce two sp hybrid orbitals. The two sp hybrid orbitals have a linear arrangement.

two sp hybrid orbitals

BeCl2 molecules 4Be: 2s2 2p0 ↑↓ ↑↓ sp hybrid orbital

The sp hybrid orbitals in gaseous BeCl2 Be (excitated) The sp hybrid orbitals in gaseous BeCl2

2. sp2 Hybridization One s orbital and two p orbital form three sp2 hybrid orbital

BF3 BF3 molecules 5B: 2s2 2p1 sp2-p sp2 hybrid orbital ↑ ↑↓ ↑↓ ↑↓ ↑↓ ↑

Figure: The sp2 hybrid orbitals in BF3

3. sp3 Hybridization One s orbital and three p orbital form four sp3 hybrid orbital

sp3-s σ 6C: 2s2 2p2 CH4 (methane) ↑↓ ↑↓ ↑↓ ↑↓ sp3 hybrid orbital

Figure: The sp3 hybrid orbitals in CH4

CH4

sp: BeCl2 sp2: BF3 , C2H4 sp3: CH4 , CCl4 Equivalent hybridization Hybridization Nonequivalent hybridization sp3: NH3 , H2O

NH3 molecule Nonequivalent hybridization sp3 Hybrid orbital Central atom N 7N: 1s2 2s2 2p3 sp3 Hybrid orbital (one lone pair electrons)

Predict correct bond angle

H2O molecule sp3 Hybrid orbital (two lone pair electrons) Central atom O 8O: 1s2 2s2 2p4 sp3 Hybrid orbital (two lone pair electrons)

bonding-pair vs. bonding pair repulsion lone-pair vs. bonding < lone-pair vs. lone pair repulsion

H2O NH3

sp2 Hybridization of Ethylene 6C: 2s2 2p2 CH2=CH2 (ethylene) 2py orbital sp2 hybrid orbital

sp Hybridization of Acetylene 6C: 2s2 2p2 CH ≡ CH (acetylene) ↑↓ ↑↓ ↑↓ ↑↓ ↑ ↑ sp hybrid orbital

Geometry of the molecule sp :180° linear sp2 :120° trigonal planar sp3 :109.5°tetrahedral NH3 :107.3° trigonal pyramidal H2O :104.5° Bent /Angular