Carbon-nitrogen-oxygen bond angles

Like the carbon atom in methane and the nitrogen atom in methylamine, the oxygen atom in methanol (methyl alcohol) and many other organic molecules can also be described as sp3-hybridized. The C-O-H bond angle in methanol is 108.5°, very close to the 109.5° tetrahedral angle. Two of the four sp3 hybrid... 

In this picture of ethylene, the two orbitals that make up the double bond are not equivalent. The a orbital is ellipsoidal and symmetrical about the C—C axis. The 71 orbital is in the shape of two ellipsoids, one above the plane and one below. The plane itself represents a node for the n orbital. In order for the p orbitals to maintain maximum overlap, they must be parallel. This means that free rotation is not possible about the double bond, since the two p orbitals would have to reduce their overlap to allow one H C H plane to rotate with respect to the other. The six atoms of a double bond are therefore in a plane with angles that should be 120°. Double bonds are shorter than the corresponding single bonds because maximum stability is obtained when the p orbitals overlap as much as possible. Double bonds between carbon and oxygen or nitrogen are similarly represented they consist of one a and one n orbital. 

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