Finding Oxidation Numbers for Transition Metals

Determining the oxidation states of transition metals when they are bonded to other elements involves looking at the oxidation states of the other elements they are bonded to in the compound.

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For example, here's a step-by-step process using the example for finding the oxidation state for the transition metal, Mn, in Potassium permanganate (KMnO₄):

Identify known oxidation states:
Potassium (K) always has an oxidation state of +1.
Oxygen (O) typically has an oxidation state of -2 in compounds.

2. Assign the oxidation state for oxygen:
Since there are four oxygen atoms in KMnO₄, the total negative charge from oxygen is -8 (4 atoms × -2 oxidation state).

3. Determine the oxidation state of manganese (Mn):
Let x be the oxidation state of manganese (Mn).
The equation is: +1 + x - 8 = -1
Solve for x: x = +7

4. Verify the oxidation states:
Confirm that the sum of the oxidation states equals the overall charge of the compound. In this case, +1 + (+7) - 8 = -1.

Therefore, in potassium permanganate (KMnO₄), the oxidation state of manganese (Mn) is +7. This method applies to other compounds containing transition metals, considering the known oxidation states of other elements in the compound.

So, in potassium permanganate (KMnO₄), the oxidation state of manganese (Mn) is +7. This method can be applied to other compounds containing transition metals, taking into account the known oxidation states of other elements in the compound.