Questions: What is the oxidation number of Mn in MnO4-?

Transcript text: What is the oxidation number of Mn in $\mathrm{MnO}_{4}^{-}$?

Solution

Step 1: Understand the Problem

We need to determine the oxidation number of manganese (Mn) in the permanganate ion, $\mathrm{MnO}_{4}^{-}$.

Step 2: Assign Known Oxidation Numbers

In the permanganate ion, $\mathrm{MnO}_{4}^{-}$, oxygen (O) typically has an oxidation number of $-2$.

Step 3: Set Up the Equation

The sum of the oxidation numbers in a polyatomic ion is equal to the charge of the ion. For $\mathrm{MnO}_{4}^{-}$, the total charge is $-1$.

Let the oxidation number of Mn be $x$. Then, the equation for the sum of the oxidation numbers is:

\[ x + 4(-2) = -1 \]

Step 4: Solve the Equation

Simplify and solve for $x$:

\[ x - 8 = -1 \]

\[ x = -1 + 8 \]

\[ x = 7 \]

The oxidation number of Mn in $\mathrm{MnO}_{4}^{-}$ is $\boxed{+7}$.

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