3f.1

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Annie Ye
Posts: 106
Joined: Wed Sep 18, 2019 12:22 am

3f.1

Postby Annie Ye » Tue Nov 12, 2019 4:16 am

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

Kevin Antony 2B
Posts: 65
Joined: Sat Sep 07, 2019 12:16 am

Re: 3f.1

Postby Kevin Antony 2B » Tue Nov 12, 2019 6:56 am

All of the molecules can have London Dispersion forces. A, C, and D will have dipole-dipole interactions, but only A and C will have Hydrogen bonding.

Ashley Tran 2I
Posts: 94
Joined: Thu Jul 11, 2019 12:17 am

Re: 3f.1

Postby Ashley Tran 2I » Tue Nov 12, 2019 8:44 am

A good tip to have in mind is carbon generally only has London dispersion intermolecular forces. This is due to the symmetry it creates from the bonds it forms with other elements (carbon is tetravalent). However, in addition to that, there could be other intermolecular forces among the other elements in a compound containing carbon. For example, if there is an OH group, there would be hydrogen bonding present.

305385703
Posts: 90
Joined: Thu Jul 11, 2019 12:15 am

Re: 3f.1

Postby 305385703 » Tue Nov 12, 2019 9:57 am

NH2OH is a molecule that has a very weak dipole moment (the electrons are distributed unevenly throughout the molecule, but not that unevenly). Thus, there will be dipole-dipole and london dispersion. Also, after drawing the Lewis structure, you will see that hydrogen has an N on one side and an O on the other side, creating a hydrogen bond.

CBr4 is a nonpolar molecule and thus it will have london dispersion forces.

H2SeO4 will have london dispersion forces and dipole-dipole for the same reasons as a). It will also have hydrogen bonding as you can see from the lewis structure.

SO2 will have dipole-dipole interactions and london dispersion forces for the same reasons as a).


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