Final answer:
The ideal bond angles around nitrogen in N2F2 are predicted to be less than 120° due to the trigonal planar electron geometry altered by the presence of a lone pair on each nitrogen, resulting in a bent molecular shape.
Step-by-step explanation:
The ideal bond angles around nitrogen in N2F2 can be predicted using the VSEPR theory. Each nitrogen in N2F2 is surrounded by one other nitrogen atom and two fluorine atoms, making a total of three regions of electron density – the N-N bond and the two N-F bonds. Since VSEPR theory states that electron pairs repel each other and try to get as far apart as possible, each nitrogen atom is expected to have trigonal planar electron geometry. However, nitrogen also contains a lone pair of electrons that does not participate in bonding but does influence the overall shape of the molecule. Therefore, the presence of this lone pair will cause the actual molecular shape around each nitrogen atom to be bent, with a bond angle of less than 120°. This is similar to the molecular shape described for other molecules with two atoms bonded to a central atom and one lone pair on the central atom, resulting in a bent shape due to the electron pair repulsion.