[bmu123]

So I've been asked to show that Pb²⁺ and Sn²⁺ can reduce Ag⁺ to Ag and have done this by working out the E^oCell for each reaction and ΔG, which is negative for both and therefore both are capable of reducing Ag⁺.
The question then asks whether I would expect Ge²⁺ to be able to reduce Ag⁺ (without reference to electrode potentials)
I'm a bit stuck on this, I think the answer is yes it would, as Ge²⁺ is less stable than Ge⁴⁺ and therefore is readily oxidised into Ge⁴⁺. Do you think this would be the correct answer? Or would I have to compare it to Pb²⁺ and Sn²⁺?

[unsu]

Ge(II) is a strong reducing agent. Check the reduction potentials to see if the reduction of Ag(I) to Ag(0) is possible.

and have done this by working out the E^oCell for each reaction and ΔG, which is negative for both and therefore both are capable of reducing Ag⁺.

I am not sure your calculations are correct.

[Borek]

Isn't it about trends in the periodic table?

[bmu123]

Ah ok sorry, Sn²⁺ can reduce Ag+ but Pb²⁺ can't. Is this because the stability of the inert pair increases going down the group, and therefore the stability of the +2 oxidation state increases going down the group as the stability of the +4 oxidation state decreases. So Pb²⁺ is more stable than Pb⁴⁺. However Sn²⁺ is less stable than Sn⁴⁺ and so is able to reduce Ag⁺. Therefore Ge²⁺ will be less stable than Sn²⁺ and will also reduce Ag⁺