The correct options are A XeOF2 C XeF2 D XeO2F2
We had earlier seen that XeF2
has a linear shape. The 3 lone pairs of electrons of central Xe atom lie on the plane perpendicular to the axial Xe – F bonds. The molecule has a trigonal bipyramidal geometry
In this molecule, if one oxygen atom takes the place of a lone pair, we get the geometry of XeOF2
. Do note that Xenon has a double bond with the oxygen atom. Let us look at the ground state and excited state:
Let us look at the geometry:
Now try to deduce the shape and geometry of XeO2F2
A logical leap is to assume that the structure would be similar to replacing two of the three lone pairs with two oxygen atoms in the XeF2
structure. It is a good guess!
As for the geometry, XeF2
all have the same trigonal bipyramidal geometry. XeF2
has a linear shape. XeOF2
is T - Shaped. XeO2F2
is see-saw shaped.
Earlier we had seen that the geometry of XeF4
has a square bipyramidal geometry and square planar shape:
In the above geometry, if we replace a lone pair with an Oxygen atom such that there is a double bond between Xe and O, then we get the geometry of XeOF4
. The four F atoms line in a plane perpendicular to the Xe – O axial sigma bond. This geometry is still the same as XeF4
but the shape will be square pyramidal!
So correct options are a c and d