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Beryllium the configuration is [He] 2s2 i.e fully filled but still quite reactive

Also in neon [He]2p4 , neither half filled nor fully filled, still quite stable compound (As it forms compound with oxygen)

I have read that half filled orbitals are extra stable due many possible rearrangement of electron I.e symmetrical , this statement was used explain stability of half filled d orbital as explained here Why are full and half filled orbitals the most stable?

my question Why cant we apply the concept of stability of fully filled d orbital to p and s orbital?

P.s

My question is different as I try to ask explanation for not using half filled orbital stability reasoning in case of p and s orbital 1) Why is fluorine the most electronegative atom? 2)Why are atoms with eight electrons in the outer shell extremely stable?

Second part is not dealt with in the answers 3)Why do elements in columns 6 and 11 assume 'abnormal' electron configurations?

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  • $\begingroup$ A large part of your confusion seems to be that you have your electron configurations incorrect. Fluorine is 1s2 2s2 2p5, not 2p3, so it does not have half-filled p orbitals. Neon is 1s2 2s2 2p6, not 2p4, so its p orbitals are completely filled. $\endgroup$ – Andrew Apr 4 at 11:04
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Well, we do consider that half filled p orbitals are more stable, as an example of which Nitrogen has more Ionisation enthalpy than Oxygen despite the trend being of left to right increase.

It should also hold for s orbitals, but then a half filled s orbital does not offer many possibilities of 'rearrangements' (as you quote in your question, I would say it doesn't offer much exchange energy) , hence the effect might not be very apparent, but it does not mean that it isn't there.

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