The structure of `K[PtCl_(3)(C_(2)H_(5))]` and hybridisation of Pt respectively are:

Options

A. square planar, `sp^(2)d^(2)`
B. square planar, `dsp^(2)`
C. tetrahedral, `sp^(3)`
D. octahedral, `d^(2)sp^(3)`

Answer

To determine the structure of the complex \( K[PtCl_3(C_2H_5)] \) and the hybridization of platinum (Pt), we can follow these steps:

### Step 1: Identify the oxidation state of platinum in the complex.
The complex can be broken down into its components:
- \( K^+ \) (potassium ion)
- \( PtCl_3(C_2H_5)^- \) (the coordination complex)

Let the oxidation state of platinum be \( x \). The oxidation states of the ligands are as follows:
- Each chloride ion (\( Cl^- \)) has an oxidation state of -1. Since there are 3 chloride ions, their total contribution is -3.
- The ethyl group (\( C_2H_5 \)) is a neutral ligand and does not contribute to the oxidation state.

The overall charge of the complex is -1. Therefore, we can set up the equation:
\[ x + (-3) + 0 = -1 \]
Solving for \( x \):
\[ x - 3 = -1 \implies x = +2 \]

### Step 2: Determine the electron configuration of \( Pt^{+2} \).
Platinum has the atomic number 78. The electron configuration of neutral platinum is:
\[ [Xe] 4f^{14} 5d^9 6s^1 \]
For \( Pt^{+2} \), we remove two electrons (one from the 6s and one from the 5d):
\[ [Xe] 4f^{14} 5d^8 \]

### Step 3: Analyze the hybridization of platinum in the complex.
Platinum in this complex is coordinated to three chloride ions and one ethyl group. This gives a total of four ligands around the platinum center.

The hybridization can be determined based on the number of ligands:
- For 4 ligands, the hybridization is \( dsp^2 \), which corresponds to a square planar geometry.

### Step 4: Determine the geometry of the complex.
Given that the hybridization is \( dsp^2 \), the geometry of the complex \( K[PtCl_3(C_2H_5)] \) is square planar.

### Final Answer:
The structure of \( K[PtCl_3(C_2H_5)] \) is square planar, and the hybridization of platinum (Pt) is \( dsp^2 \).

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