The shape of `CIF_(3)` according to VSEPR model is

Options

A. planar triangle
B. T-shape
C. tetrahedral
D. square planar

Answer

To determine the shape of CIF₃ (carbon trifluoride) according to the VSEPR (Valence Shell Electron Pair Repulsion) model, we can follow these steps:

### Step 1: Identify the Central Atom
The central atom in CIF₃ is carbon (C).

### Step 2: Determine the Valence Electrons
Carbon has 4 valence electrons.

### Step 3: Count the Number of Bonds
In CIF₃, carbon forms 3 single bonds with three fluorine (F) atoms.

### Step 4: Consider Lone Pairs
Since carbon has 4 valence electrons and it uses 3 of them to form bonds with fluorine, there is 1 valence electron left. This lone electron will form a lone pair.

### Step 5: Calculate Hybridization
The hybridization can be calculated using the formula:
\[ \text{Hybridization} = \text{Number of valence electrons} + \text{Number of monovalent atoms} - \text{Charge} \]
In this case:
- Number of valence electrons = 4 (from carbon)
- Number of monovalent atoms = 3 (from the three fluorine atoms)
- Charge = 0 (no cations or anions)

So, the calculation is:
\[ \text{Hybridization} = 4 + 3 - 0 = 7 \]
Since we are considering the number of hybrid orbitals, we divide by 2:
\[ \text{Hybridization} = \frac{7}{2} = 3.5 \]
However, we consider the effective hybridization based on the number of bonds and lone pairs, which leads us to sp³ hybridization.

### Step 6: Determine the Molecular Geometry
With 3 bonded pairs (C-F) and 1 lone pair, the molecular geometry will be determined by the arrangement of these pairs. According to VSEPR theory, the arrangement of 3 bonded pairs and 1 lone pair corresponds to a trigonal pyramidal shape.

### Conclusion
The shape of CIF₃ according to the VSEPR model is trigonal pyramidal.

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