Question

The molecule having T-shape is:

• A. $S{F}_4$
• B. $Cl{F}_3$
• C. $BeC{l}_2$
• D. $I_3^{-}$

Answer 1

The correct option is B

$Cl{F}_3$

As per VSEPR theory, we have the formula

$\Rightarrow$ ep = $\frac{(V+L+A-C)}{2}$

Now, first we will look at the central atom of all the options provided.

We know that we have to take the central atom which is least in number.

Therefore,

Central atom -

(a) S (b) Cl (c) Be (d) I

Now, we will calculate the electron pair for each option.

(a) $S{F}_4\to$ ep = $\frac{(6+4)}{2}$ = $\frac{10}{2}$ = 5

(b) $Cl{F}_3\to$ ep = $\frac{(7+3)}{2}$ = $\frac{10}{2}$ =5

(c) $BeC{l}_2\to$ ep = $\frac{(2+2)}{2}$ = 2

In case of (d), to get central atom of $I_3^{-}$, we have to divide $I_3^{-}$.

Therefore,

(d) $I_3^{-}\to$ ep = $\frac{(7+2+1)}{2}$ = 5