The shape of `Cl F_(2)^(-)` , is

Options

A. Linear
B. Trigonal bipyramidal
C. Square pyramidal
D. T -shape

Answer

To determine the shape of the ClF₂⁻ ion, we can follow these steps:

### Step 1: Determine the Valence Electrons
- Chlorine (Cl) has 7 valence electrons.
- Each Fluorine (F) atom has 7 valence electrons, and there are 2 F atoms, contributing a total of 14 electrons.
- Since the ion has a negative charge (−1), we add 1 more electron.

**Calculation:**
- Total valence electrons = 7 (from Cl) + 14 (from 2 F) + 1 (from the negative charge) = 22 valence electrons.

### Step 2: Determine the Central Atom and Electron Pairs
- Chlorine is the central atom.
- The total number of electron pairs can be calculated by dividing the total valence electrons by 2 (since each pair consists of 2 electrons).

**Calculation:**
- Total electron pairs = 22 valence electrons / 2 = 11 electron pairs.

### Step 3: Identify Bonding and Lone Pairs
- ClF₂⁻ has 2 bonding pairs (from the two Cl-F bonds).
- The remaining electron pairs will be lone pairs.

**Calculation:**
- Total pairs = 11
- Bonding pairs = 2 (from 2 Cl-F bonds)
- Lone pairs = 11 - 2 = 9 lone pairs.

### Step 4: Determine Hybridization
- The hybridization can be determined based on the number of electron pairs around the central atom.
- With 11 electron pairs, the hybridization will be sp³d² (since it involves 5 orbitals).

### Step 5: Determine the Shape
- The arrangement of the electron pairs will dictate the molecular geometry.
- With 2 bonding pairs and 9 lone pairs, the shape will be influenced primarily by the positions of the bonding pairs.

**Conclusion:**
- The shape of ClF₂⁻ is T-shaped due to the presence of 2 bonding pairs and 3 lone pairs occupying the equatorial positions.

### Final Answer:
The shape of ClF₂⁻ is T-shaped.

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