For a given period, why is the boiling point of the halogen greater than that of the noble gas?

The boiling point of bromine, a halogen, is $\pu{58.8^\circ C}$, while the boiling point of krypton, the noble gas in the same period as bromine, is $\pu{-153.4 ^\circ C}$. 


I thought that the larger the atomic radius of an element, the more loosely the electrons would be held by the nucleus. So it would be easier for the atom to develop an instantaneous dipole, strengthening the London forces between the atoms of the element, and increasing the boiling point of the substance. 


Krypton has a larger atomic radius than bromine. Using my reasoning from above, I thought that the boiling point of krypton would be higher than that of bromine. However, bromine actually has a higher boiling point than krypton. 


Why is this? And where is my reasoning incorrect?




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**Complete data for reference:** notice that the boiling point of a halogen is always higher than that of the corresponding noble gas, and the difference increases down the group.


$$
\begin{array}{|c|c|c|}\hline
\text{Period}&\text{Halogen boiling point} (\pu{^\circ C})&\text{Noble gas boiling point} (\pu{^\circ C})\\\hline
2&−188.11&−246.046 \\\hline
3&−34.04&−185.848 \\\hline
4&58.8&−153.415 \\\hline
5&184.3&−108.099 \\\hline
\end{array}
$$


