Match the oxidation number of the underlined element in Column I with the value in Column II.
Column I
Column II
A) $\mathrm{N̲_{2}H_{4}}$
P) +1
B) $\mathrm{H_{3}P̲O_{2}}$
Q) +2
C) $\mathrm{K_{4}[Fe(C̲N)_{6}}$ ]
R) -2
D) $\mathrm{S̲O_{2}}$
S) +4

Question

Match the oxidation number of the underlined element in Column I with the value in Column II.

Column I	Column II
A) $\mathrm{N̲_{2}H_{4}}$	P) +1
B) $\mathrm{H_{3}P̲O_{2}}$	Q) +2
C) $\mathrm{K_{4}[Fe(C̲N)_{6}}$ ]	R) -2
D) $\mathrm{S̲O_{2}}$	S) +4

TestHub · Accepted Answer

(A) In N 2 ​ H 4 ​ : 2x + 4 = 0 gives N = -2 (R). (B) In H 3 ​ P O 2 ​ : 3 + x - 4 = 0 gives P = +1 (P). (C) In the C N − ligand, N = -3, so C - 3 = -1 gives C = +2 (Q). (D) In S O 2 ​ : x - 4 = 0 gives S = +4 (S).

Chemistry - Redox Reactions Question with Solution | TestHub

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