Valence Bond & hybridization

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Presentation transcript:

Valence Bond & hybridization Google-youtube referrences: 1. Tro pages 408 and 411 2. Valence bond: molecular shape and Orbital hybridization. 3. Section 7 5 sigma and pi bonds. 4. Sp3 Atomic orbital Hybridization – Chemistry Sigma and Pi bond symmetry

Valence Bond & hybridization The orbital pattern valence electrons for 6C are: __ __ __ __ 2s 2px 2py 2pz The 4 bonds in CH4 are identical. The explanation is that valence electrons hybridize into an sp3 hybrid: __ __ __ __ sp3

Valence Bond;hybridization;polarity B+LP = # bonds (single, double or triple) + # lone pair electrons Comp. B+LP Normal valence orbitals Hybridized orbitals BeF2 2 __ __ __ __ 2s 2p __ __ __ __ sp BF3 3 __ __ __ __ 2s 2p __ __ __ __ sp2 CH4 4 2s 2p sp3 H2O PF5 5 __ __ __ __ __ __ __ 3s 3p __ __ 3d __ __ __ __ __ __ __ sp3d __ __ BrF5 6 4s 4p __ __ 4d sp3d2 __ __

Valence Bond;hybridization;polarity B+LP = # Bonds (single, double, and triple) + # Lone pairs. 2 3 4 5 6

Valence Bond;hybridization;polarity 2s 2px 2py 2p SP3 hybridization The bond angle for H2O is 105o. H2S bond angle is closer to normal p orbitals (90o).

Valence Bond & hybridization Draw the line bond formula for CO2: Hybridized sp orbitals ( 2 bonds ) are around C; hybridized sp2 (1 bond and 2 lone pairs) orbitals are around each oxygen.

Valence Bond;hybridization;polarity The hybridized orbital pattern valence electrons for each 6C in C2H4 (sp2 ) is: __ __ __ __ The sp2 hybrid forms σ bonds, and the p orbital forms a π bond. sp2 p The yellow and green bonds in figures a and c are also σ bonds. The purple bonds in figures b and c are π bonds.

Valence Bond;hybridization;polarity Draw the line bond formula shown right. Write the electron geometry, molecular geometry, and orbital hybridization for the following atoms in the line bond formula: C in CCO 2. C in NCC 3. C in HCH Write the following bond angles: 4. NCC 5. CCO 6. CCC 7. HCH 9. CCH 8. Locate the sigma (σ) and pi (π) bond(s).

Valence Bond;hybridization;polarity Dipoles are represented as vectors. As vectors: A + B + C = R If The tip of C is at the origin, R =0, and the molecule Is non-polar. If R ≠ 0, the molecule is polar.

Valence Bond;hybridization;polarity Identify the electronic and molecular geometries. Draw the molecular formulas. Identify the hybridized orbitals and locate the sigma and pi bonds (if any). Predict the polarity (polar or nonpolar)for the following molecules (not ions): The first non-hydrogen atom is central. 1. CO2 2. CH2O 3. CH4O 4. C2H2 5. NO2- 6. HCN 7. XeF4 8. C2H4O 9. CO32- 10. NO3- 11. BrF5 12. IF4+ 13. C6H6 ( See next slide.) 14. I3-

Valence Bond;hybridization;polarity Benzene (C6H6) has resonance structures (Figure 1) and is often written as shown in Figure 2. Note the σ and π bonds in Figures 3 and 4. Figure 1 π bonds σ bond(s) Figure 2 Figure 3 Figure 4