Explain the following facts giving appropriate reason in each case.
(i) $N F_{3}$ is an exothermic compound whereas $N C I_{3}$ is not.
(ii) All the bond in $S F_{4}$ are not equivalent.

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Solution

i) Cl atom has large size when compared to F atom (because as we move down in VII group the atom size increases) so the bond strength of $N C l_{3}$ is less leading to form endothermic where as the bond strength of $N F_{3}$ is more, so it is exothermic.

ii)The five electron pairs around sulphur in $S F_{4}$ attain trigonal bi-pyramidal geometry in which one position is occupied by lone pair. This lone pair finds a position that minimizes the number of repulsion it has with bonding electron pairs. It occupies an equatorial position with two repulsion. The bonded electrons occupy the axial and equatorial positions. The axial S-F bonds are bent slightly away from the lone pair. Hence, all the bonds in $S F_{4}$ are not equivalent.

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