I don't think molecules have electronegativity - look at the definition:
"Electronegativity, symbol χ, is a chemical property that describes the tendency of an atom or a functional group to attract electrons (or electron density) towards itself." - wikipedia
The difference in electronegativity can tell you if a molecule is polar, non-polar or ionic. Also, some groups can "hog" electrons, as I remember from organic chemistry and you can call them electronegative.
I think I can answer the second question, but please take this with a pinch of salt.
The closer the electron is to the nucleus, the stronger the electrostatic force. Fluorine is a very small atom, and the p orbitals are closer to the nucleus than in other atoms; the electrostatic attraction between the nucleus and an e
- is very strong. That's why you never see F
+ except if you bombard it with some kind of radiation, but that's another story. (this story (ionization energy) is actually very important depending on which electronegativity you are talking about)
Now, when fluorine forms an ionic bond with say Na, that new electron finds it's place in a p orbital.
You may think that other electrons (-) push it away, and you would be right. However, the
effective charge (
Zeff)the new electron is experiencing is so strong (compared to other atoms in the PTE) that no other atom can pull it away. Fluorine just won't let go of it.
(unless a
24He core flies nearby
)