Question

In which of the compounds does 'manganese' exhibit the highest oxidation number?

• A. \( \text{MnO}_2 \)
• B. \( \text{Mn}_3\text{O}_4 \)
• C. \( \text{K}_2\text{MnO}_4 \)
• D. \( \text{MnSO}_4 \)

Hint:

The oxidation state of an element in a compound can be determined by considering the charges of the other elements or groups present in the compound.

Answer 1

The Correct Option is C

To find the oxidation number of Mn in \( \text{K}_2\text{MnO}_4 \), use the equation: \[ 2(+1) + x + 4(-2) = 0, \] where \( x \) denotes the oxidation state of Mn.
Simplifying: \[ 2 + x - 8 = 0 \implies x = +6. \] For the other compounds, the oxidation numbers of Mn are: - In \( \text{MnO}_2 \), Mn = \( +4 \), - In \( \text{Mn}_3\text{O}_4 \), Mn = \( +\frac{8}{3} \) (average), - In \( \text{MnSO}_4 \), Mn = \( +2 \). Hence, the highest oxidation number occurs in \( \text{K}_2\text{MnO}_4 \). Final Answer: \[ \boxed{\text{K}_2\text{MnO}_4} \]