`Cl_(2)+underset((Excess))(F_(2)) overset(573K)to(A)`
Shape of compound (A) is

Options

A. (A) Linear
B. (B) Tetrahedral
C. (C) Bent T Shape
D. (D) Trigonal bipyramidal

Answer

To determine the shape of compound (A) formed from the reaction of Cl₂ and excess F₂ at 573 K, we will follow these steps:

### Step 1: Identify the Product
The reaction given is:
\[ \text{Cl}_2 + \text{Excess} \, \text{F}_2 \overset{573K}{\rightarrow} \text{A} \]

When chlorine (Cl₂) reacts with fluorine (F₂), the product formed is chlorine trifluoride (ClF₃).

### Step 2: Write the Balanced Equation
The balanced chemical equation for the reaction is:
\[ \text{Cl}_2 + 3\text{F}_2 \rightarrow 2\text{ClF}_3 \]

### Step 3: Determine the Hybridization of ClF₃
To find the shape of ClF₃, we need to determine the hybridization of the chlorine atom in this compound. We can use the formula for hybridization:
\[ H = \frac{1}{2} (M + V - C) \]
Where:
- \( M \) = number of monovalent atoms attached to the central atom (3 fluorine atoms)
- \( V \) = number of valence electrons of the central atom (chlorine has 7 valence electrons)
- \( C \) = overall charge on the molecule (0 for neutral molecules)

Substituting the values:
- \( M = 3 \)
- \( V = 7 \)
- \( C = 0 \)

Calculating:
\[ H = \frac{1}{2} (3 + 7 - 0) = \frac{1}{2} (10) = 5 \]

### Step 4: Identify the Hybridization Type
The hybridization of 5 indicates that chlorine undergoes \( sp^3d \) hybridization. This means the geometry around the chlorine atom is trigonal bipyramidal.

### Step 5: Determine the Shape of ClF₃
In ClF₃, there are 3 fluorine atoms and 2 lone pairs of electrons on the chlorine atom. The presence of lone pairs affects the shape.

- The trigonal bipyramidal geometry has 5 positions: 3 equatorial and 2 axial.
- The 3 fluorine atoms will occupy the equatorial positions, while the 2 lone pairs will occupy the axial positions.

### Step 6: Final Shape Determination
When considering the shape (which ignores lone pairs), ClF₃ appears to have a T-shaped configuration due to the arrangement of the three fluorine atoms and the two lone pairs. The repulsion between lone pairs and bond pairs causes the shape to be bent T-shaped.

### Conclusion
The shape of compound (A), ClF₃, is **bent T-shaped**.