Formation of Xenon Flouride

Regarding to the formation of compounds and bonds, I have discovered a interesting,additional fact and would like to share it here,which I also did it for my ACE too.The compound name xenon flouride certainly looks difficult but cool. Let us understand it then.As we know, xenon is an unreactive, stable noble gas,with the electronic configuration of 2.8.8, while flourine is a halogen with the configuration of 2.7. It is widely regarded that noble gases will not combine with other elements to form compounds. Why can this compound still form a covalent compound with the electronic configuration of XeF2(xenon flouride can still exist in many other forms). First of all, it would be due to the structure of the xenon atom. As xenon is located at the foot of its group, it has a large number of shells and are thus heavier than the lighter ones.Hence, the outermost electrons experience a shielding effect from the inner electrons that makes them more easily ionised, since they are less strongly attracted to the positively-charged nucleus. This results in an ionization energy low enough to form stable compounds with the most electronegative elements, fluorine and oxygen, and even with less electronegative elements such as nitrogen and carbon under certain circumstances. Ionisation energy is the force or energy needed for an atom to give up and remove its electrons. Electronegativity would then mean an atom's ability or tendency to attract electrons to itself to form a anion. Each element's has its own electronegativity represented by a value. It is classified that elements that have the electronegativity difference of 0.2-0.5 would form non-polar covalent bonds(where there is equal sharing of electrons), 0.5-1.6(polar covalent bonds,unequal sharing) and above which will belong to ionic bonds. Xenon's electronegativity is 2.60, while flourine's is 3.98. The difference would thus mean a non-polar covalent bond formed. For those who don't quite understand what I am discussing about, you can refer to the electronegativity table online. Nonetheless, after all this, you will find this extremely interesting.