Can anybody explain why Xenon can still form covalent bonds?!

[Chromeo33]

If Xe has a full octet (considering its in group 18 of the periodic table), why does it still have an ability to form covalent bonds (as in the molecule of XeF₄)?

[Mao]

If Xe has a full octet (considering its in group 18 of the periodic table), why does it still have an ability to form covalent bonds (as in the molecule of XeF₄)?

The simple rules stop working for large atoms like Xe. I would imagine the 5p orbital will be very similar in energy compared to the 4f orbitals, so

[VivaTequila]

It has D orbitals which can start filling

I think D orbitals are lower in energy than 2p orbitals?

[thushan]

Put simply, the outer shell of electrons for Xenon can accommodate more than 8 electrons, that's why after it has its octet it can form more covalent bonds to have 10, 12, 14 electrons on the outer shell.

[VivaTequila]

Put simply, the outer shell of electrons for Xenon can accommodate more than 8 electrons, that's why after it has its octet it can form more covalent bonds to have 10, 12, 14 electrons on the outer shell.

would it be able to accomodate up to 18 considering that it has 5 d orbitals which can hold 2 electrons each?

or does it not have "access" to those 5 orbitals because of it's atomic number?

[Chromeo33]

Far out.... Are these just random exceptions that I'm supposed to just memorise or is there a way to systematically work this out?

[VivaTequila]

These aren't exceptions... it's all of Lewis Structures and VSEPR. Check out the most recent guys lectures. We need to know how to do them, not memorize them.