Identify the molecule listed below that cannot form Hydrogen bonds with an identical molecule.
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In order to H-bond, a molecule MUST HAVE a lone-pair of electrons on a central atom and be able to attract a neighboring hydrogen that itself is held with a very polar bond. You should draw some lewis structures
In order to form a H-bond you must have a hydrogen attached to a highly electronegative element (N, O and F)
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Look up the options, which one do you think doesn't have a hydrogen attached to any of the electron hogs (highly EN elements; N, O, F)
I agree with @Abhisar
so, I guess it should be BH3 right guys?
H bonds are formed between a hydrogen atom and an electronegative atom.
F>O>N>Cl <---This is the decreasing order of the electronegativity of the main electronegative atoms.
Since Boron is more in to electropostitve side rather than electronegativity side we can for BH3. :)
For hyrogen bonding to occur you need to have either F,O, or N covalently bonded to a hydrogen to act as the hydrogen bond donor, AND a lone pair of electrons to act as a hydrogen bond acceptor.
We can see from these elements here, that in order to hydrogen bond there also must be a lone pair of electrons available to act as an acceptor as you see, so both requirements must be met for this to happen.
Boron is electron deficient, so it has no lone pairs that can participate in H bonding with another BH3 molecule, and also it's not that highly of an electronegative element to do so anyway.
nice one @Photon336
Thanks @arindameducationusc the pictures are a little messy but hey i think I got the point across lol