Name the two conditions which must be satisfied for hydrogen bonding to take place in a molecule.
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The 2 conditions given for hydrogen bonding are:
1) A hydrogen atom must be covalently bonded to O, N or F atom. I can understand this part, as O, N and F are highly electronegative and will leave the H with a positive dipole (more or less a H+ ion).
2) The other condition is that the atom with a lone pair which the H is hydrogen-bonded to must be O, N or F. I don't get this part, though. Why can't it be any atom with a lone pair? Is it because O, N and F are highly electronegative and so the lone pair will not be donated directly to the H but will be held on tightly by the O, N or F and form a bond based on electrostatic forces of attraction instead of covalent bond?
1) A hydrogen atom must be covalently bonded to O, N or F atom. I can understand this part, as O, N and F are highly electronegative and will leave the H with a positive dipole (more or less a H+ ion).
2) The other condition is that the atom with a lone pair which the H is hydrogen-bonded to must be O, N or F. I don't get this part, though. Why can't it be any atom with a lone pair? Is it because O, N and F are highly electronegative and so the lone pair will not be donated directly to the H but will be held on tightly by the O, N or F and form a bond based on electrostatic forces of attraction instead of covalent bond?
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""Hydrogen bonding" is a sort of partial "electrostatic force" of "attraction". For "hydrogen bonding" to take place in a "molecule", two conditions that are to be satisfied are
(i) Highly electronegative atom with small size (F, O, and N) must be present in the molecule and hydrogen atom should be covalently bonded to it. They are hydrogen bond donors.
(ii) Another adjacent atom which is highly electronegative should have a "lone pair of electrons". They are hydrogen bond acceptors."
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