CHEM 6A Lecture 23: 11-16 lecture

• School: UCSD
• Department: Chemistry and Biochemistry
• Course: CHEM 6A
• Professor: Christine Johnson

Document Summary

Valence electrons are localized between atoms (or are lone pairs) A set of overlapping orbitals has a mazimum o ftwo electrons that must have opposite spins. Half-filled atomic orbitals overlap to form bonds - the greater the overlap the stronger the bond hybridization. Hybridization produces 4 new orbitals , the sp3 hybrid orbitals that have an energy that is the average of the s and p atomic orbitals\ This is how methane gets it tetrahedral shape. Bonding is due to an overlap of an sp3 orbital from carbon and a 1s orbital from hydrogen. Can only form sigma bonds from hybrid orbitals. Count the number of things attached to the central atom (remember lone pairs count as things and multiple bonds count as only one thing) Starting with the s-orbital, count off an orbital for every thing that is attached to the central atom.