In addition to NF3, two other fluoro derivatives of nitrogen are known: N2F4 and N2F2.a. What shapes should these two molecules have around each nitrogen atom?b. What is the hybridization for the nitrogen atoms in each molecule?

N2F2 is trigonal planar with sp2 hybridization

N2F4 is tetrahedral with sp3 hybridization

Explanation:

In N2F4 the hybridisation of the nitrogen atom is sp3, because Nitrogen has four regions of electron density pointing in four directions in space: twice N-F; one N-N and one free electron pair. Hence, the implication of this is that the F-N-F angle is approximately 109°. This is the tetrahedral bond angle.

In N2F2, each nitrogen has 4 electron pairs. Now, because two of these electron pairs are in a double bond,then each nitrogen atom could be treated as having a set of 3 electron pairs. Thus there are two possible configurations: trigonal pyramidal and trigonal planar. Trigonal planar arrangement is preferred because the repulsions between the other nitrogen and the adjacent fluorine are too high in the trigonal pyramidal structure.