Question

What is the formula for titanium (IV) chloride?

Answer 1

Hint: According to Aufbau Principle, Pauli exclusion principle and Hund’s rule, the electronic configuration of cations is assigned by removing electrons first in the outermost p orbital, followed by the s orbital and then the d orbital.

Complete answer:
Titanium is a d block element which has the electronic configuration of
$[Ar]3{d^2}4{s^2}$
While is a p block element with very high electronegativity which on while attacking the titanium distorts the configuration resulting the electronic configuration to change such that one of the electron from the s orbital jumps to one of the d orbitals and the configuration becomes:
$[Ar]3{d^3}4{s^1}$
Now all these electrons in the outermost d orbital of the titanium are unpaired.
While the high electronegative chlorine of the p block part of the periodic table, has the electronic configuration:
$[Ne]3{s^2}3{p^5}$
In the outermost p orbital of the chlorine atom there are five electrons present, out of which 4 electrons are paired while one electron is unpaired.
Now on reaction of chlorine with titanium, due to the high electronegativity of the chlorine distorts the outside s and p orbitals resulting in it having 4 unpaired electrons. Now 4 chlorine atoms attack these 4 unpaired electrons resulting in the formation of $TiC{l_4}$.

Note:
High electronegative atoms have the tendency to distort the outside orbitals so that the greatest number of such electronegative atoms can react and form a stable structure.