Question

In which of the following compounds Mn has the highest oxidation state?

• A. MnO₄
• B. MnO₂
• C. MnO₄^2-
• D. Mn₂O₃

Answer 1

The Correct Option is A

To determine in which compound manganese (Mn) has the highest oxidation state, we need to calculate the oxidation state of Mn in each compound given in the options.

1. For MnO₄ (Permanganate):

   Let the oxidation state of Mn be x. Oxygen has a known oxidation state of -2.

   Since there are 4 oxygen atoms, the oxidation state contribution from oxygen is 4 \times (-2) = -8.

   According to the charge neutrality principle, the sum of oxidation states is equal to the total charge of the compound (which is zero because it's a neutral compound).

   Equation: x + 4(-2) = 0 \Rightarrow x - 8 = 0 \Rightarrow x = +8.

   Thus, the oxidation state of Mn in MnO₄ is +8.

2. For MnO₂ (Manganese(IV) oxide):

   Again, let the oxidation state of Mn be x.

   Equation: x + 2(-2) = 0 \Rightarrow x - 4 = 0 \Rightarrow x = +4.

   The oxidation state of Mn in MnO₂ is +4.

3. For MnO₄^2- (Manganate ion):

   Equation: x + 4(-2) = -2 \Rightarrow x - 8 = -2 \Rightarrow x = +6.

   The oxidation state of Mn in MnO₄^2- is +6.

4. For Mn₂O₃ (Manganese(III) oxide):

   This compound contains two Mn atoms and three oxygen atoms.

   Equation: 2x + 3(-2) = 0 \Rightarrow 2x - 6 = 0 \Rightarrow 2x = 6 \Rightarrow x = +3.

   The oxidation state of Mn in Mn₂O₃ is +3.

From the above calculations, we conclude that the highest oxidation state is found in MnO₄, where Mn has an oxidation state of +8. Therefore, the correct answer is MnO₄.