Chemistry 141 Monday, November 20, 2017 Lecture 32 Hybridization

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Presentation transcript:

Chemistry 141 Monday, November 20, 2017 Lecture 32 Hybridization Chemistry 11 - Lecture 11 9/30/2009 Chemistry 141 Monday, November 20, 2017 Lecture 32 Hybridization

Questions for today: What makes a molecule polar? What is a covalent bond? How can we understand molecular shapes in terms of orbitals?

Polarity of Molecules A NONPOLAR molecule A POLAR molecule

Orbital overlap and bonding

Hybrid orbitals SN=4  tetrahedral (Example: CH4)

sp2 hybrid orbitals SN=3  trigonal planar (Example: BCl3)

Hybrid orbitals for linear geometry SN=2  linear (Example: BeCl2)

dsp3 hybrid orbitals SN=5  trigonal bipyramidal (Example: PCl5)

Hybrid orbitals and bonding for other SNs SN=6  octahedral (Example: SF6)

Hybridization summary

Sigma () and Pi () Bonds Sigma bonds are characterized by head-to-head overlap. cylindrical symmetry of electron density about the internuclear axis. Pi bonds are characterized by side-to-side overlap. electron density above and below the internuclear axis.

Bonding in Ethylene

Bonding in Acetylene

Benzene