Methane has 4 C-H sigma bonds. Four bonds of equal length. Bond vector separated by 109.5°. This angle also happens to be the angle that places the substituents around the carbon as far apart as possible. Since each electron pair of the 4 sigma bonds will be concentrated between the C-H atoms, the bond angle minimizes the repulsion between the electron pair of one bond and its 3 neighbouring bonds

Structure of Ethane C 2 H 6 Lewis or Dot Structure Line Bond Structure

Hybridization: The structure of Ethene or Ethylene - sp 2 Hybrid Orbitals Ethylene C 2 H 4 Since Carbon is tetravalent ethylene must contain a carbon to carbon double bond.

sp 2 Hybridization

sp Hybridization:-

Predicting Shapes of Molecules Valence-Shell Electron Pair RepulsionVSEPR Model - electrons in a molecule arrange themselves to minimize electrostatic repulsion. CCl 4 like methane (CH 4 ) is tetrahedral because this is how the four groups of electron pairs that make the bonds between carbon and chlorine can be the farthest apart.

To Apply this idea use the following steps:- 1.Count electron groups on an atom. These are of the following type Lone Pair - one group Any pair or set of pairs of electrons - one group. 2.Assume each group moves as far apart as possible. Valence-Shell Electron Pair Repulsion VSEPR

Acetylene C 2 H 2 The geometry of the molecule is linear and the bond angle = 180°.

CH 5 N

CH 5 N

C 2 H 6 O There are two plausible Lewis or Line Bond structures. Both are acceptable structures.

C 2 H 6 O There are two plausible Lewis or Line Bond structures. Both are acceptable structures.

Benzene C 6 H 6

Benzene C 6 H 6

Acetonitrile C 2 H 3 N Lewis structure? Hybridization? Shape?