Draw the Lewis structure of `NO_(2)^(-)` (Nitrite ion) .

Explanation

Count the total number of valence electrons of the nitrogen atom the oxygen atoms and the additional one negative charge (equal to one electron)
`N(2s^(2) 2p^(3)),O(2s^(2)2p^(4))`
`5 + (2 xx 6) + 1 = 18` electrons
Step 2 The skeletal struture of `NO_(2)^(Θ)` is written as `O N.O`
Step 3 Draw a single bond (one shared electron pair) between the nitrogen if the remaining two electrons constitute lone pair on it
`[:underset(..)overset(..)O:overset(..)N:underset(..)overset(..)O:]^(Θ)`
Hence we have to resort to multiple bonding between nitrogen and one of the oxygen atoms (in the case a double bond) This leads to the following Lewis dot
`[underset(..)overset(..)O ::overset(..)N: underset(..)overset(..)O:]^(Θ) or [underset(..)overset(..)O=overset(..)N-underset(..)overset(..)O:]^(Θ)or [:underset(..)overset(..)O-overset(..)N=underset(..)overset(..)O]^(Θ)` .