Calculate the oxidation number of the underlined atom in the following species.
`K_(4)ul(Fe)(CN)_(6)`

Explanation

To calculate the oxidation number of iron (Fe) in the compound \( K_4[Fe(CN)_6] \), we can follow these steps:

### Step 1: Identify the oxidation states of known elements
- Potassium (K) has an oxidation number of +1.
- The cyanide ion (CN) has an oxidation number of -1.

### Step 2: Set up the equation
Since \( K_4[Fe(CN)_6] \) is a neutral compound, the sum of the oxidation numbers must equal zero. Let the oxidation number of iron (Fe) be \( x \).
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