Homework 3F1

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Jasmine 2C
Posts: 119
Joined: Wed Sep 18, 2019 12:18 am

Homework 3F1

Postby Jasmine 2C » Wed Nov 20, 2019 10:21 pm

For this question "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", is it asking what IMFs can arise if two of the same molecule (i.e. 2 of NH2OH) were to interact?
Can someone also explain why each molecule have their respective intermolecular interactions?

Marty Hockey
Posts: 47
Joined: Wed Sep 18, 2019 12:19 am

Re: Homework 3F1

Postby Marty Hockey » Wed Nov 20, 2019 11:43 pm

It is asking what kind of interactions these molecules could potentially have. NH2OH, for example, can have hydrogen bonds, dipole-dipole interactions, and London forces because it has an OH bond and is polar. CBr4 can only have London forces because it is nonpolar, and SO2 can have London and dipole-dipole because it is polar.

Eileen Si 1G
Posts: 81
Joined: Fri Aug 30, 2019 12:17 am

Re: Homework 3F1

Postby Eileen Si 1G » Fri Nov 22, 2019 9:16 am

H2SeO4 is also polar, so it will have dipole-dipole interactions as well as London dispersion forces.

Anika Chakrabarti 3K
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Joined: Sat Aug 24, 2019 12:17 am

Re: Homework 3F1

Postby Anika Chakrabarti 3K » Fri Nov 22, 2019 9:23 am

I had trouble with part c at first, but H2SeO4 will also have hydrogen bonding. This is because its lewis structure has the four oxygens bonded to the central Se atom, and the two H atoms are bonded to two of the hydrogens. Any time an H atom is bonded to an O, F or N atom, there will be hydrogen bonding.

ValerieChavarin 4F
Posts: 56
Joined: Wed Sep 18, 2019 12:18 am

Re: Homework 3F1

Postby ValerieChavarin 4F » Sat Nov 23, 2019 3:50 pm

The question is asking what are the IMF of each molecule. For H2SeO4, due to its polarity, it has dipole-dipole and induced-induced. On top of that, it can also form hydrogen bonds.


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