Chemical Forums
Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: PicturesOfLilly on May 09, 2021, 04:05:12 PM
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Hydrogen bonding is basically the same thing as dipole-dipole forces? It's just that the atoms H, O & F make these dipole-dipole forces stronger. So can hydrogen bonding be considered a specific type of dipole-dipole interaction?
In my book it says it's when "H is bonded to a small electronegative atoms like flourine, nitrogen or oxygen". Isn't that strange that it uses the word 'like'? Are there any other small electronegative elements that could be included in this definition? Like Sb? What's going on with SbH3, in that it has a higher boiling point than NH3?
Please post straight forward answers.
Thank you
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So can hydrogen bonding be considered a specific type of dipole-dipole interaction?
"Dipole-dipole interaction" suggests interaction between permanent or induced dipole, while molecule (donor or acceptor) can be completely non-polar. It just need polarized -H bond for donor and lone pairs on O or N atom for acceptor.
"H is bonded to a small electronegative atoms like flourine, nitrogen or oxygen". Isn't that strange that it uses the word 'like'? Are there any other small electronegative elements that could be included in this definition?
S, Cl and Br can also act as acceptors.
What's going on with SbH3, in that it has a higher boiling point than NH3?
It's like give wings to an elephant - it is still too heavy.
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What's going on with SbH3, in that it has a higher boiling point than NH3?
It's like give wings to an elephant - it is still too heavy.
So you're saying that even though there is no hydrogen bonding in SbH3, it still has a higher boiling point than NH3 due to the fact that Sb is such a heavy element.
What about PH3 so? Isn't Phosphorus heavier than Nitrogen?
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What about PH3 so? Isn't Phosphorus heavier than Nitrogen?
Nothing. Weaker hydrogen bonding lowers boiling point.