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

Options

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

Explanation

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

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

### Step 2: Identify the Oxidation States of Other Components
- The ethylene ligand \((C_2H_4)\) is a neutral ligand, so its oxidation state is \( 0 \).
- Each chlorine (Cl) atom has an oxidation state of \(-1\). Since there are three chlorine atoms, their total contribution to the oxidation state 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 the Equation
Now, 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 the complex \([Pt(C_2H_4)Cl_3]^{-}\) is \( +2 \).

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

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