The compound AgF₂ is unstable compound. However, if formed, the compound acts as a very strong oxidising agent. Why?
In the compound , silver is present in the +2 oxidation state. However, from the activity series, we know that silver (Ag) is a very less active metal and shows the lowest reducing activity among Zn, Cu, and Ag (Zn > Cu > Ag). This means silver does not easily lose electrons to form higher oxidation states.
Because of its low tendency to stay in a higher oxidation state, the Ag²⁺ ion in is highly unstable. To attain stability, it readily accepts an electron to get reduced to the more common +1 state. This strong tendency to gain electrons from other substances is why , if formed, acts as a very strong oxidising agent.
Explanation
The provided context highlights that silver is a very less active metal with low reducing activity (Zn > Cu > Ag), meaning it does not readily lose electrons to form higher oxidation states. Consequently, if silver is forced into a +2 oxidation state in AgF2, it becomes highly unstable and readily accepts an electron to revert to a lower, more stable state. This strong tendency to gain electrons makes it a powerful oxidising agent.