Question

Assign oxidation numbers to the underlined elements in each of the following species:

(a) NaH₂PO₄ (b) NaHSO₄ (c) H₄P₂O₇ (d) K₂MnO₄

(e) CaO₂ (f) NaBH₄ (g) H₂S₂O₇ (h) KAl(SO₄)₂.12 H₂O

Answer 1

(a)

Let the oxidation number of P be x.

We know that,

Oxidation number of Na = +1

Oxidation number of H = +1

Oxidation number of O = –2

Then, we have

Hence, the oxidation number of P is +5.

(b)

Then, we have

Hence, the oxidation number of S is + 6.

(c)

Then, we have

Hence, the oxidation number of P is + 5.

(d)

Then, we have

Hence, the oxidation number of Mn is + 6.

(e)

Then, we have

Hence, the oxidation number of O is – 1.

(f)

Then, we have

Hence, the oxidation number of B is + 3.

(g)

Then, we have

Hence, the oxidation number of S is + 6.

(h)

Then, we have

Or,

We can ignore the water molecule as it is a neutral molecule. Then, the sum of the oxidation numbers of all atoms of the water molecule may be taken as zero. Therefore, after ignoring the water molecule, we have

Hence, the oxidation number of S is + 6.