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    In a HF, why is it that the hydrogen bonds form a zigzag structure not what I have drawn? So in other words, why does the F's 2 other lone pairs not form a hydrogen bond with another 2 HF?
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    Each H effectively forms two bonding pairs, which will repel each other to maximum distance, i.e. 180 o.
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    (Original post by BDunlop)
    In a HF, why is it that the hydrogen bonds form a zigzag structure not what I have drawn? So in other words, why does the F's 2 other lone pairs not form a hydrogen bond with another 2 HF?
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    There are four pairs of electrons around the fluorine atoms arranged in a tetrahedral orientation ("bond" angle 109º 28')
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    (Original post by charco)
    There are four pairs of electrons around the fluorine atoms arranged in a tetrahedral orientation ("bond" angle 109º 28')
    Yes, but why could there not be 2 more hydrogen bonds on the fluorine's other 2 LPs
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    (Original post by BDunlop)
    Yes, but why could there not be 2 more hydrogen bonds on the fluorine's other 2 LPs
    You are running out of hydrogen atoms ...

    in the bulk structure there is an average of 1 H atom to 1 fluorine atom
 
 
 
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