What is the shape of the `ClF_(3)` molecule?

Options

A. Trigonal planar
B. Trigonal pyramidal
C. T-shaped
D. Tetrahedral

Explanation

To determine the shape of the ClF₃ molecule, 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. Each fluorine (F) atom contributes 1 valence electron, and since there are 3 fluorine atoms, they contribute a total of 3 electrons. Therefore, the total number of valence electrons in ClF₃ is:
\[ 7 \, (\text{from Cl}) + 3 \times 1 \, (\text{from F}) = 10 \, \text{valence electrons} \]

### Step 2: Draw the Lewis Structure
In the Lewis structure of ClF₃, chlorine is the central atom. It forms three single bonds with the three fluorine atoms. After forming these bonds, we have:
- 3 bonds (3 pairs of electrons) used, which accounts for 6 electrons.
- This leaves us with 4 electrons (2 lone pairs) remaining on the chlorine atom.

### Step 3: Calculate the Steric Number
The steric number is calculated as the sum of the number of sigma bonds and the number of lone pairs around the central atom. In ClF₃:
- There are 3 sigma bonds (one for each Cl-F bond).
- There are 2 lone pairs on the chlorine atom.

Thus, the steric number is:
\[ \text{Steric Number} = 3 \, (\text{sigma bonds}) + 2 \, (\text{lone pairs}) = 5 \]

### Step 4: Determine the Hybridization
The hybridization corresponding to a steric number of 5 is sp³d.

### Step 5: Identify the Geometry
With sp³d hybridization, the geometry of the molecule is trigonal bipyramidal.

### Step 6: Determine the Molecular Shape
However, since there are 2 lone pairs, they will occupy the equatorial positions in the trigonal bipyramidal geometry to minimize repulsion. This results in a T-shaped molecular geometry for ClF₃.

### Final Answer
The shape of the ClF₃ molecule is T-shaped.

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