The oxidation number of `Pt` in `[Pt (C_(2)H_(4))Cl_(3))"]"^(ө)` is

Options

A. `+1`
B. `+2`
C. `+3`
D. `+4`

Answer

To find the oxidation number of platinum (Pt) in the complex ion \([Pt(C_2H_4)Cl_3]^{\text{-}}\), we can follow these steps:

### Step 1: Assign Variables
Let the oxidation number of platinum (Pt) be \(x\).

### Step 2: Identify the Oxidation States of Other Elements
- The ethylene ligand \((C_2H_4)\) is a neutral ligand, so it contributes 0 to the overall charge.
- Each chlorine (Cl) atom has an oxidation state of \(-1\). Since there are three chlorine atoms, their total contribution is \(3 \times (-1) = -3\).

### Step 3: Set Up the Equation
The overall charge of the complex ion is \(-1\). Therefore, we can set up the equation based on the sum of the oxidation states:
\[ x + 0 + (-3) = -1 \]

### Step 4: Solve for \(x\)
Now, we can simplify the equation:
\[ x - 3 = -1 \]
Adding 3 to both sides gives:
\[ x = -1 + 3 \]
\[ x = +2 \]

### Conclusion
The oxidation number of platinum (Pt) in \([Pt(C_2H_4)Cl_3]^{\text{-}}\) is \(+2\).