Calculate oxidation state of Ag in [Ag(S2O3)2]3− molecule

To calculate the oxidation state of Ag in [Ag(S2O3)2]3− molecule, we need to know the oxidation states of the other atoms in the molecule.

The oxidation state of S in S2O3 (thiosulfate ion) is +2. Since there are two S atoms, the total oxidation state for S in S2O3 is +4.

The oxidation state of O in S2O3 is -2. Since there are three O atoms, the total oxidation state for O in S2O3 is -6.

The total oxidation state of the thiosulfate ion (S2O3) is -2 (since it carries a 2- charge), and there are two thiosulfate ions in the molecule, so the total oxidation state for the two thiosulfate ions is -4.

The molecule [Ag(S2O3)2]3− carries a 3- charge, so the sum of the oxidation states of all the atoms in the molecule must equal -3.

Let's denote the oxidation state of Ag as x. So, we have the equation:

x + (-4) = -3

Solving for x gives:

x = -3 + 4 = +1

So, the oxidation state of Ag in [Ag(S2O3)2]3− is +1.