Hydrogen electron get to close to Flourine atoms????

What happens when hydrogen’s electron gets close to the valence shell of a fluorine atom?

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  • Anonymous
    1 decade ago
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    When hydrogen and fluorine atoms bond, a permanent net dipole forms resulting from hydrogen being covalently bonded to the fluorine as hydrogen bonds form.

    the hydrogen bond is the strongest type of intermolecular force since the hydrogen nucleus is extremely small and positively charged and fluorine is very electronegative so that the electron on the hydrogen atom is strongly attracted to the fluorine. this leaves a highly localised positive charge on the hydrogen atom and highly negative localised charge on the fluorine.

    this means the electrostatic attraction between these molecules will be greater than for the polar molecules that do not have hydrogen covalently bonded to either fluorine.

    because the fluorine atom is unstable, as is the hydrogen, because they have not filled up their valence shell, they bond together quickly, and because of their opposing charges, very strongly.

    have a look at some online animations, with will become very clear to you.

    (-) (-) (-) (strong hydrogen bonds)

    (-) F --------------------------------------------- H (+)

    (-) (-)

    it looks a little bit like that, the (-) negative charges on the fluorine attract the positive (+) charge on the hydrogen, forming in hydrogen bonds (----). The fluorine has 7 electrons and the (---) is where both H and F share the electron - look at http://www.ausetute.com.au/intermof.html and http://images.google.com.au/imgres?imgurl=http://u...

    good luck.

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