Predict the structure of \(XeOF_4\)

Square pyramidal

The correct answer is option 2. Square pyramidal.

We can draw the Lewis structure of the compound, so that we will get the idea about the shape of the molecule.

We know that Fluorine generally binds with one atom and oxygen generally binds with two atoms. This structure involves six atoms. So, Xenon must be the central atom.

In the Lewis structure, Xenon has 8 valence electrons as it is a noble gas, oxygen has 6 electrons and fluorine has 7 valence electrons. Let’s make bonds between them and see the structure.

We can see that xenon uses 4 of its electrons to make bonds with 4 fluorine atoms. 2 of the valence electrons of xenon make double bonds with oxygen and the remaining two are as a lone pair.

As lone pairs have strong repulsive effects on bonds, Xe-F bonds have a tendency to be as far as possible from the lone pair.

Xenon-Oxygen double bonds also have a repulsive effect as oxygen and fluorine atoms have 2 and 3 lone pairs respectively.

So, Xe-F bonds lie in a plane to make repulsive forces least as possible and on two sides of the plane, oxygen atoms and lone pairs reside.