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Chapter 4

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}

Step-by-Step

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.)