# why fluorine and oxygen have different behaviour towards electron gain enthalapy and electronegativity? [closed]

I have seen following definitions in my textbook:

Electron gain enthalapy may be defined as enthalpy change taking place when an isolated gaseous atom of the element accepts an electron to form a monovalent gaseous anion.

Electronegativity may be defined as the tendency of an atom in molecule to attract towards itself the shared pair of an electron.

I know that fluorine and Oxygen have low $${\Delta H_{eg}}$$ than Chlorine and Sulpher respectively due to the fact when an electron is added to these atoms, the electron goes to the relatively compact second energy level which results in significant repulsion from other electrons present in the shell.

But I have seen that Fluorine and Oxygen have very high electronegativity.

(i)I can't understand how can an atom attract shared pair of electron very well when it is unwilling to add elctron in its valence shell?

## closed as unclear what you're asking by Mithoron, A.K., Todd Minehardt, Waylander, Ben NorrisOct 6 '18 at 20:36

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• Very unreactive? Flourine still has the second highest electron affinity in the periodic system. Flourine and oxygen are by far smaller than chlorine and sulfur, so the repulsion is higher. Etc. A very similar question is why HI is the strongest of the HHal acids, and HF the weakest. Stability of the ion has no direct relation to electronegativity in a covalent bond. It's a different electronic configuration, you cannot compare the two just like that. – Karl Oct 6 '18 at 9:14
• @Karl : thanks for the answer, but the (i) question is still unclear to me. – pranjal verma Oct 6 '18 at 9:52
• The one electron is added to an atom orbital. The other phenomenon is the pull on a pair of electrons that are already in a molecular orbital. It's incomparabale. And both oxygen and fluorine have a negative electron affinity, it's just slightly weaker than of sulphur and chlorine. ?! – Karl Oct 6 '18 at 12:35