What is the shape of the ClF_3 molecule? | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(C) To determine the shape of the $ClF_3$ molecule,we calculate the number of electron pairs around the central atom $Cl$ using the formula: $X = \fra

Vedclass · Accepted Answer

$T$-shaped

Vedclass · Answer

(C) To determine the shape of the $ClF_3$ molecule,we calculate the number of electron pairs around the central atom $Cl$ using the formula: $X = \frac{1}{2} [V + M - C + A]$,where $V$ is the number of valence electrons of the central atom $(Cl = 7)$,$M$ is the number of monovalent atoms $(F = 3)$,$C$ is the cationic charge $(0)$,and $A$ is the anionic charge $(0)$.$X = \frac{1}{2} [7 + 3] = 5$.This indicates $sp^3d$ hybridization.Out of $5$ electron pairs,$3$ are bond pairs (forming $3$ $\sigma$-bonds with $F$ atoms) and $2$ are lone pairs.According to $VSEPR$ theory,the $2$ lone pairs occupy the equatorial positions to minimize repulsion,resulting in a $T$-shaped molecular geometry.

$I. SnCl_2$	$II. BeF_2$
$III. SO_2$	$IV. NO_2^+$
$V. C_2H_2$

What is the shape of the $ClF_3$ molecule?

Similar Questions

Which of the following has the largest bond angle?

Identify the isostructural pairs from the following species: $NF_3, NO_3^-, BF_3, H_3O^+, HN_3$

Which of the following have linear structure?

$I. SnCl_2$ $II. BeF_2$

$III. SO_2$ $IV. NO_2^+$

$V. C_2H_2$

The molecular shapes of $SF_4$, $CF_4$ and $XeF_4$ are

In gaseous triethylamine,the $C-N-C$ bond angle is $.....$ degrees.

Vedclass Test Series

Exam Paper Generator

Online Exam Module