Bond Overlaps and Hybridization

What are the Conditions for Bonding?

1. There must be _____________ to bond

2. Each atom must have at least a ____________

3. We need not just a valence electron, but an ______________________, when they unify, their two unpaired orbitals become ______________

two atoms
valence electron
unpaired valence orbital
paired/filled orbital

_____________ result from the combination of atomic orbitals to from molecular orbitals

Covalent bonds

Covalent bonds result from the combination of ______________ to form ___________________

atomic orbitals
molecular orbitals

Bonding —> ____________ —> _____________

lower energy

stabilizing

_____________ is a HEAD-ON overlap, electron density ALONG BOND AXIS

Sigma bond

___________________ is a SIDE-BY-SIDE, electron density ABOVE and BELOW axis

Pi bond

A ____________________ HAS ELECTRON DENSITY directly between the bonded atoms, and is SYMMETRIC with respect to 180 degrees rotation about the bond

Sigma bond

A ________________ HAS NO ELECTRON DENSITY directly between the bonded atoms, and is ANTISYMMETRIC with respect to 180 degrees rotation about the bond

Pi bond

sp3 hybridization

Bonds: ____________
Total substituents: _________
Bond Angle: __________
Geometry:_________________

Four sigma bonds
Four
109.5 degrees
Tetrahedral

sp2 hybridization

Bonds: ____________
Total substituents: _________
Bond Angle: __________
Geometry:_________________

Three sigma bonds, 1 pi bond
Three
120 degrees
Trigonal Planar

sp hybridization

Bonds: ____________
Total substituents: _________
Bond Angle: __________
Geometry:_________________

Two sigma bonds, 2 pi bonds
Two
180 degrees
Linear