Chemistry - Redox Reactions Question with Solution | TestHub

The compound AgO is actually Ag[AgO₂]. For the compound to be diamagnetic, all electrons must be paired. This requires one Ag to be in the +1 oxidation state and the other Ag to be in the +3 oxidation state, resulting in a net charge of +2 for the two silver ions.

Let the oxidation state of one Ag be $x$ and the other be $y$.

The compound is Ag[AgO₂].

Oxygen typically has an oxidation state of -2.

So, $x+y+2(-2)=0$

$x+y-4=0$

$x+y=4$

For diamagnetism, both Ag ions must have paired electrons.

Ag(I) has an electron configuration of $[Kr]4d^{10}$, which is diamagnetic.

Ag(III) has an electron configuration of $[Kr]4d^8$, which can be diamagnetic in a square planar geometry.

If one Ag is +1 and the other is +3:

$1+3=4$. This satisfies the condition.

Thus, the oxidation states are +1 and +3.