Question

In the structure of CIF3, the number of lone pair of
electrons on central atom 'Cl' is
(1) One
(2) Two
(3) Three
(4) Four​

Answer 1

Answer:chlorine have 2 lone pairs in clf3.

Explanation:because it have 7 electrons in its valence shell.from which three electrons of chlorine make sigma bond with 3 atom of fluorine. So left 4 electrons make 2 lone pair in a pair of 2.

Answer 2

Answer: (2) Two

Explanation:

Formula used for hybridization:

$\text{Number of electrons}=\frac{1}{2}[V+N-C+A]$

where,

V = number of valence electrons present in central atom

N = number of monovalent atoms bonded to central atom

C = charge of cation

A = charge of anion

Now we have to determine the hybridization of the $ClF_3$ molecule.

$\text{Number of electrons}=\frac{1}{2}\times [7+3]=5$

Bond pair electrons = 3

Lone pair electrons = 5 - 3 = 2

The number of electrons are 5 that means the hybridization will be $sp^3d$ and the electronic geometry of the molecule will be trigonal bipyramidal.

But as there are three atoms around the central chlorine atom, the fourth and fifth position will be occupied by lone pair of electrons. The repulsion between lone and bond pair of electrons is more and hence the molecular geometry will be T- shaped.

Hence, the number of lone pairs of electrons present on the central atom are 2.