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## Q. 4.6

Assign an oxidation number (oxid. no.) to each element in the following species:

(a) $N_{2}$           (b) $N^{3-}$         (c) $NO_{3}^{-}$         (d) BaO         (e) $K_{2}O_{2}$

## Verified Solution

 oxid. no. N = 0 (a) $N_{2}$  is in its elementary state. (Rule 1) oxid. no. N = -3 (b) $N^{3-}$  is a monoatomic ion. (Rule 2) oxid. no. O = -2 3(-2) + x = -1; oxid. no. N = +5 (c) There are no Group 1 or Group 2 metals. (Rule 6) $NO_{3}^{-}$ is a polyatomic ion. (Rule 5) oxid. no. Ba = +2 +2 + x = 0; oxid. no. O = -2 (d) Ba is a Group 2 metal. (Rule 3) The sum of the oxidation numbers is 0. (Rule 5) oxid. no. K = +1 2(1) + 2x = 0; oxid. no. O = -1 (e) K is a Group 1 metal. (Rule 3) The sum of the oxidation numbers is 0. (Rule 5)

END POINT

Always look for the “leading elements” (Group 1 and Group 2 metals and F) in a compound when you start. These elements will lead you to the oxidation numbers of the other elements in the compound. If these leading elements are not present, then look for H and O (+1 and -2, respectively, when not combined with Group 1 or 2 metals.)