Question

Write formal charges of the atoms in the nitrite ion.

Answer 1

Formal charge is by definition a formalism; it has no physical reality, but may nevertheless be useful for calculation.

We can write the Lewis representation of the nitrate anion as, (O=)N+(−O−)2. The nitrogen centre is quaternized, and bears a positive charge. Why? Because it has a share in 4 bonding electrons: 2 from the the doubly bound oxygen, and 1 each from the 2 N−O bonds. So with the 2 inner core electrons, the nitrogen centre is associated with 6 electrons ONLY rather than the 7 it requires for electrical neutrality. The nitrogen centre thus bears a positive charge.

Compare this with ammonia, a neutral molecule. We write :NH3. The nitrogen centre owns (or has a share in) 5 electrons (2 from the lone pair are entirely associated with the nitrogen; and 3 electrons from the N−H bonds). Ammonia is rightly depicted as a neutral atom with no formal charges.

So back to nitrate: nitrogen has dibs on only 6 electrons, and therefore bears a formal positive charge. The doubly bound oxygen has a share in or owns 8 electrons, and so is depicted as neutral. The singly bound oxygen atoms have 9 electrons associated with them, and so each bears a negative charge. The overall charge on the nitrate ion is of course −1, which this representation is designed to suggest. Can you treat the sulfate anion, SO2−4 in the same way? Where does the formal charge lie?

Answer 2

Answer:

Explanation:

-1

The central N atom: This atom has 5 valence electrons, 2 nonbonding electrons, and 6 bonding electrons.

NOTE: The sum of the formal charges is -1, which is equal to the charge on the nitrite ion.