if you had a complex ion [Mn(NH3)2(H2O)3(OH)]^+2 would the oxidation state of the metal atom be 5 and what would be the charge on the complex if all ligands were chloride ions
Not 5? Wouldn't Mn be +3. If Mn is +3 and OH is -1, that leaves a charge of +2 on the ion? right? If the 1 OH, 3 H2O, and 2 NH3 became Cl (that's 6 the way I count), then [MnCl6] must have a charge of
+3+(-6) = -3 so we would write [MnCl6]^-3. Check my thinking.
for the oxidation state of the Mn doesn't the NH3 have a charge. So OH is -1 and NH3 has a -1 charge plus 2 so its -2 or does it not have a charge
No. NH3 is neutral. The NH3 is a compound and all compounds are zero charge. NH3 is a gas but we usually use it dissolved in water.
To determine the oxidation state of the metal atom in a complex ion, you need to consider two things: the charges of the ligands and the overall charge of the complex.
In the given complex ion [Mn(NH3)2(H2O)3(OH)]^+2, we are dealing with a manganese (Mn) atom.
To find the oxidation state of the manganese atom, we need to assign oxidation states to the ligands first. In this case, NH3 (ammonia) and H2O (water) are neutral ligands, so their oxidation state is 0. The OH^- (hydroxide) ligand usually has a -1 oxidation state.
Next, we calculate the overall charge of the complex if all ligands were chloride ions. Since chloride (Cl^-) has a -1 charge, and there are five ligands (two NH3, three H2O, and one OH), the total charge contributed by the ligands is -1 x 5 = -5.
The complex ion, [Mn(NH3)2(H2O)3(OH)]^+2, has a charge of +2. Therefore, the manganese atom must have an oxidation state that balances the overall charge of the complex.
To calculate the oxidation state of manganese, we can use the following equation:
Oxidation state of Mn + (Oxidation state of NH3 x number of NH3) + (Oxidation state of H2O x number of H2O) + (Oxidation state of OH^- x number of OH^-) = Overall charge of the complex.
Let's assume that the oxidation state of manganese is x:
x + (0 x 2) + (0 x 3) + (-1 x 1) = 2.
x - 1 = 2.
x = 2 + 1.
x = 3.
Therefore, the oxidation state of the manganese atom in the complex [Mn(NH3)2(H2O)3(OH)]^+2 is +3, not +5 as you suggested.
Additionally, since all ligands have been replaced with chloride ions, the charge on the complex would be -5, in order to balance the +2 overall charge: [MnCl5]^-2.