Calculate the oxidation state of the underlined atoms in the given species.
(a) `ul(N)O_(2)^(+)`

Explanation

To calculate the oxidation state of nitrogen in the species \( \text{NO}_2^+ \), we can follow these steps:

### Step 1: Assign the oxidation state variable
Let the oxidation state of nitrogen (N) be represented as \( X \).

### Step 2: Determine the oxidation state of oxygen
In compounds, oxygen typically has an oxidation state of -2. Since there are two oxygen atoms in \( \text{NO}_2^+ \), the total contribution from oxygen will be:
\[
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