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Electron-Electron repulsion

Why is it that fluorine has more electron pairs in the same outer subshell (2p) than oxygen and yet the first IE of fluorine is still higher? Surely there is more electron-electron repulsion in the 2p subshell of fluorine.

Is it that nuclear charge or electronegativity is in favour of the electron electron repulsion in the fluorine atom which means the e-e repulsion can be ignored? If so, why?

help pls D:
Original post by CookieHero
Why is it that fluorine has more electron pairs in the same outer subshell (2p) than oxygen and yet the first IE of fluorine is still higher? Surely there is more electron-electron repulsion in the 2p subshell of fluorine.

Is it that nuclear charge or electronegativity is in favour of the electron electron repulsion in the fluorine atom which means the e-e repulsion can be ignored? If so, why?

help pls D:


The nuclear charge is greater. This has more influence than the e-e repulsion.
Reply 2
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CookieHero
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Original post by charco
The nuclear charge is greater. This has more influence than the e-e repulsion.


How does nuclear charge give a greater influence than the e-e repulsion? Just out of curiosity.
Original post by CookieHero
How does nuclear charge give a greater influence than the e-e repulsion? Just out of curiosity.


Electrostatic force is a function of the average distance between the charged particles..

The force of attraction for 9 protons on the electron in the 2pz orbital has more influence than that of one electron in the same orbital.
Reply 4
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CookieHero
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Original post by charco
Electrostatic force is a function of the average distance between the charged particles..

The force of attraction for 9 protons on the electron in the 2pz orbital has more influence than that of one electron in the same orbital.


Thanks for your help :biggrin:

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