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Chris Tai 1B
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Joined: Sat Aug 24, 2019 12:16 am


Postby Chris Tai 1B » Sat Nov 09, 2019 2:24 pm

Identify the types of attractive intermolecular interactions that might arise between molecules of each of the following substances: (a) NH2OH; (b) CBr4; (c) H2SeO4; (d) SO2.

Can someone walk me through parts B and C? Why wouldn't part b have dipole-dipole interactions (isn't Br way more electronegative than C), and why would part c be conducive to hydrogen bonds?

Trinity Vu 1D
Posts: 53
Joined: Fri Aug 30, 2019 12:15 am

Re: 3F.1

Postby Trinity Vu 1D » Sat Nov 09, 2019 2:31 pm

For part b, although C and Br have an electronegativity difference of about .45, because since C is surrounded by Br atoms and doesn't have any lone pairs, the partially negatively charged Br atoms of other CBr4 molecules cannot have dipole interactions with it. Only the Br molecules have lone pairs and would repel each other since they have the same charge. H2SeO4 has hydrogen bonds because if you draw out the molecule, the H atoms are attached to O (which is one of the three atoms needed, O, F, or N) and the O has lone pairs.

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