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

### Step 1: Identify the components of the complex
The complex consists of platinum (Pt), ethylene (C₂H₄), and three chloride ions (Cl).

### Step 2: Assign oxidation numbers to known components
- The oxidation number of chlorine (Cl) is typically \(-1\).
- Ethylene (C₂H₄) is a neutral molecule, which means its overall oxidation state is \(0\).

### Step 3: Set up the equation for oxidation states
Let the oxidation number of platinum (Pt) be \(X\). The overall charge of the complex ion is \(-1\). Therefore, we can set up the following equation based on the sum of the oxidation states:

\[ X + (0) + 3(-1) = -1 \]

### Step 4: Simplify the equation
This simplifies to:

\[ X - 3 = -1 \]

### Step 5: Solve for \(X\)
Now, we can solve for \(X\):

\[ X = -1 + 3 \]
\[ X = +2 \]

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

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