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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
Asked by Bhanu Last Modified
Answer (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.
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