How does the polarizability of an apolar compound influence properties such as its boiling temperature?
In non-polar liquids, the intermolecular forces are known as London dispersion forces (or dipole induced dipole interaction). This is the weakest interaction that exists between molecules.
The strength of this interaction depends on polarisability of non-polar molecule. As an example, let's take the following examples:
$$
\begin{array}{lr|lr|lr|lr}
\hline
\text{Compound} &amp; \mathrm{bp}/\pu{°C} &amp; \text{Compound} &amp; \mathrm{bp}/\pu{°C} &amp; \text{Compound} &amp; \mathrm{bp}/\pu{°C} &amp; \text{Compound} &amp; \mathrm{bp}/\pu{°C} \\
\hline
\ce{CO2}  &amp; -78.5 &amp; \ce{CCl4} &amp; 76.7  &amp; \ce{CBr4}  &amp; 189.5 &amp; \ce{CI4}   &amp; 329.2 \\
\ce{CS2}  &amp; 46.3  &amp; \ce{CBr4} &amp; 189.5 &amp; \ce{SiCl4} &amp; 57.7  &amp; \ce{SiBr4} &amp; 153.0\\
\ce{CSe2} &amp; 125.5 &amp; \ce{CI4}  &amp; 329.2 &amp;            &amp;       &amp;                 \\
\hline
\end{array}
$$
In these molecules, polarisability depends on polarisability of anions $(\alpha),$ which depends as
$$\alpha \propto q \times r,$$
where $q$ is the charge and $r$ is the ionic radius.
As charge on each anion is same, hence we can conclude that, greater the radius, greater is the polarisability, and thus greater is London dispersion forces.
Therefore, greater boiling point.