Question

Question:

(a) The first noble-gas compound, prepared by Neil Bartlett in 1962, was an orange-yellow ionic solid that consisted of ${\mathbf{\text{XeF}}}^{\mathbf{\text{+}}}$and ${\mathbf{\text{PtF}}}_{\mathbf{11}}^{\mathbf{-}}$. Draw a Lewis diagram for ${\mathbf{\text{XeF}}}^{\mathbf{\text{+}}}$.

(b) Shortly after the preparation of the ionic compound discussed in part (a), it was found that the irradiation of mixtures of xenon and fluorine with sunlight produced white crystalline role="math" localid="1661750003447" ${\mathbf{\text{XeF}}}_{\mathbf{2}}$. Draw a Lewis diagram for this molecule, allowing valence expansion on the central xenon atom.

Short answer

(a)

(b)

Step-by-step solution

Subpart (a) A Lewis diagram for the given molecule.

The Lewis diagram for${\text{XeF}}^{+}$ is;

Here, xenon has 8 valence electrons as it is a noble gas with a complete octet rule.

When it donates one electron and forms one bond with fluorine, the number of lone pairs that exist is three (3).

Also, the given molecule${\text{XeF}}^{+}$ has a xenon with a complete octet.

Subpart (b) The Lewis diagram for the given molecule, allowing valence expansion on the central xenon atom.

The molecule ${\text{XeF}}_2$has xenon with 10 complete valence electrons.

Therefore, the molecule shows the valence expansion on the central xenon atom.