According to Octet Rule, each atom gains or loses electrons to complete its outermost shell. As a result, molecules are formed. Each contributing element has 8 electrons in the outermost shell, but there are some limitations to this rule in which central atom of some molecules has more han 8 electrons. Some molecules like NO and `NO_(2)` don't satisfy octet rule as they have odd electrons in them.
On the basis of above paragraph, answer the following :
(i) Writer the Lewis structurre of `N_(2)` molecule.
(ii) How the structure of `SF_(6)` cannot be explained on the basis of octet rule ?

Explanation

(i) Each N atom has five valence electrons. Out of these are shared between `overset(* *)N:::overset(* *)N` them while one pair of electrons is present as lone pair on both the atoms.
(ii) Structure of `SF_(6)` does not follow octet rule. It is in fact, limitation to the octet rule. The central 'S' atom has six electron pairs after sharing. But the molucule is stable on account of its symmetrical (octahedral) shape.