Question

Which of the following statements is incorrect regarding the structure $Xe{{O}_{2}}{{F}_{4}}$ molecule?
A) $Xe = O$ bonds are present in axial position.
B) All $XeF$ bond lengths are equal
C) Adjacent $F-Xe-F$ angles are ${{90}^{0}}$
D) Shape of the molecule is octahedral

Answer 1

The answer to this question can be deduced only if you draw the structure of$Xe{{O}_{2}}{{F}_{4}}$ molecule based on VSEPR theory and this molecule has $s{{p}^{3}}{{d}^{2}}$ hybridisation. This fact helps you to write the structure of the given molecule.

Complete Solution :
- In the lower classes of chemistry we have studied several theories that predict the shape of the molecules, angle between the atoms in a molecule and also number of bonds between the atoms in a molecule.
- One among such theories is the valence shell electron pair repulsion theory or abbreviated as VSEPR theory.
- Let us now see what this theory says and how the structure or geometry of the molecule can be determined using this theory.
- Valence shell electron pair repulsion theory or VSEPR theory is the one which predicts the shape of the individual molecules based on the number of electron pairs surrounding the central atoms.
- Based on this theory, the structure of the given molecule $Xe{{O}_{2}}{{F}_{4}}$ can be predicted.
In the molecule $Xe{{O}_{2}}{{F}_{4}}$, the central atom xenon has valence of eight electrons in its outermost shell. Among these two oxygen bonds with two pairs of electrons to form a bonding pair and the remaining four electrons are shared by four bonding electrons of fluorine.
Thus, there are a total of six bond pairs and no lone p[air of electrons on the xenon atom. Thus, the hybridisation of $Xe{{O}_{2}}{{F}_{4}}$ is $s{{p}^{3}}{{d}^{2}}$ and is having the octahedral structure. The structure is as shown below,

Now, since the structure is octahedral, there are no axial nor any equatorial positions in this molecule and thus, the $Xe=O$ bonds are not in any of these positions and thus, this statement will be wrong.
Therefore, the correct answer to this question will be option A) $Xe=O$ bonds are present in axial position. So, the correct answer is “Option A”.

Note: Note that in this molecule all $XeF$ are equal and also the angle between the orbitals is ${{90}^{0}}$ because the shape of the molecule is octahedral and also note that this molecule is non - polar in nature.