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: Calculate the Total Valence Electrons
- Chlorine (Cl) has 7 valence electrons.
- Each Fluorine (F) atom has 7 valence electrons, and there are two Fluorine atoms.
- The anionic charge (-1) contributes an additional electron.

**Calculation:**
\[ \text{Total valence electrons} = 7 (\text{from Cl}) + 2 \times 7 (\text{from F}) + 1 (\text{from charge}) = 7 + 14 + 1 = 22 \]

### Step 2: Determine Bond Pairs and Lone Pairs
- To find the number of bond pairs, we divide the total number of valence electrons by 8 (to account for the octet rule).

**Calculation:**
\[ \text{Bond pairs} = \frac{22}{2} = 11 \quad \text{(This is incorrect; we should divide by 2 to find bond pairs)} \]
Instead, we can directly calculate the bond pairs:
- Each bond pair consists of 2 electrons. Since we have 22 electrons, we can find the number of bond pairs:
\[ \text{Bond pairs} = \frac{22 - \text{Lone pair electrons}}{2} \]

### Step 3: Calculate Lone Pairs
- After forming bond pairs, the remaining electrons will be lone pairs.
- Since we have 2 bond pairs (from ClF2), we can calculate the lone pairs:
\[ \text{Total electrons used in bond pairs} = 2 \times 2 = 4 \]
\[ \text{Remaining electrons} = 22 - 4 = 18 \quad \text{(These will be lone pairs)} \]
Since each lone pair consists of 2 electrons:
\[ \text{Lone pairs} = \frac{18}{2} = 9 \quad \text{(This is incorrect; we should have 3 lone pairs)} \]

### Step 4: Determine the Shape
- The steric number (the number of bond pairs + lone pairs) for ClF2⁻ is:
\[ \text{Steric number} = 2 (\text{bond pairs}) + 3 (\text{lone pairs}) = 5 \]
- According to VSEPR theory, a steric number of 5 corresponds to a trigonal bipyramidal geometry.
- The arrangement of the lone pairs will affect the molecular shape. With 3 lone pairs occupying equatorial positions, the shape of the molecule will be linear.

### Final Answer
The shape of ClF2⁻ is **linear**, while the geometry is **trigonal bipyramidal**.

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