The shape around the central form in `ClF_(4)^(+)` is

Options

A. square planar
B. square pyramidal
C. octahedral
D. see - saw

Answer

To determine the shape around the central atom in \( \text{ClF}_4^+ \), we can follow these steps:

### Step 1: Determine the Valence Electrons
Chlorine (Cl) is in group 17 of the periodic table, which means it has 7 valence electrons.

### Step 2: Count the Monovalent Atoms
Fluorine (F) is a monovalent atom, meaning each fluorine contributes 1 electron. In \( \text{ClF}_4^+ \), there are 4 fluorine atoms, contributing a total of \( 4 \times 1 = 4 \) electrons.

### Step 3: Account for the Cation Charge
The \( +1 \) charge indicates that there is one less electron than the total count of valence electrons. Therefore, we will subtract 1 from the total.

### Step 4: Apply the Formula
Using the formula for hybridization:
\[ \text{Hybridization} = \frac{1}{2} \left( V + M - C + A \right) \]
Where:
- \( V \) = Valence electrons from the central atom (Cl) = 7
- \( M \) = Number of monovalent atoms (F) = 4
- \( C \) = Cation charge = 1
- \( A \) = Anion charge = 0

Substituting the values:
\[ \text{Hybridization} = \frac{1}{2} \left( 7 + 4 - 1 + 0 \right) = \frac{1}{2} \left( 10 \right) = 5 \]

### Step 5: Determine the Hybridization Type
A hybridization number of 5 corresponds to \( sp^3d \) hybridization.

### Step 6: Predict the Molecular Geometry
For \( sp^3d \) hybridization, the molecular geometry can be either trigonal bipyramidal or square pyramidal. Since there are 4 fluorine atoms and one lone pair on chlorine, the shape will be square pyramidal.

### Conclusion
The shape around the central atom in \( \text{ClF}_4^+ \) is **square pyramidal**.

---