Question

Ammoniated solutions of alkali metals are reducing agents due to the presence of free or solvated electrons and can reduce :

• A. $O_2$ to $O_2^{2-}$
• B. $\left[K_2\right(Ni\left(CN{)}_4\right]$ to $K_4\left[Ni\right(CN{)}_4]$
• C. Both (a) & (b)
• D. None of the above

Answer 1

The correct option is C Both (a) & (b)

Ammoniated solutions of alkali metals are reducing agents due to the presence of free or solvated electrons from metal ions.

$M\to M^{+}+e^{-}$

And this electron is used to reduce these reagents.

$\left[Ni\right(CN{)}_4{]}^{-2}+2e^{-}\to \left[Ni\right(CN{)}_4{]}^{-4}$