Question

The oxidation number of Tin in $Sn(OH)_6^-$ is

• A. +3
• B. +1
• C. +4
• D. +2

Answer 1

Answer: (C)

+4

Answer 2

Let the oxidation state of Sn = x.
Each hydroxide (OH⁻) contributes –1. For the complex ion, assuming the common hexahydroxostannate ion is $[Sn(OH)_6]^{2-}$, the total charge balance is:

$x + 6(–1) = –2$

$x – 6 = –2$

$x = +4$

Thus, the oxidation number of tin is +4.