Boiling Point

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Nathan Mariano 2G
Posts: 68
Joined: Fri Sep 28, 2018 12:29 am

Boiling Point

Postby Nathan Mariano 2G » Fri Dec 07, 2018 2:16 am

How do you determine which compound has the higher boiling point if they both have similar intermolecular forces? For example, H2S and H2Se.

gillianozawa4I
Posts: 31
Joined: Fri Sep 28, 2018 12:27 am

Re: Boiling Point

Postby gillianozawa4I » Fri Dec 07, 2018 2:21 am

H2Se has the higher boiling point because it has a larger mass and more electrons. Because Se has more electrons, it is more polarizable and therefore has stronger London Dispersion Forces than H2S. This causes it to have a higher boiling point. Hope this helps!

katie_sutton1B
Posts: 61
Joined: Fri Sep 28, 2018 12:17 am

Re: Boiling Point

Postby katie_sutton1B » Fri Dec 07, 2018 8:40 am

After identifying the intermolecular forces, you would want to look at the size, or amount of electrons in the atom. The more electrons there are, the more polarizable it is. The more polarizable element has the strongest Van der Waals forces and therefore Se would be the higher boiling point.

taywebb
Posts: 60
Joined: Fri Sep 28, 2018 12:15 am

Re: Boiling Point

Postby taywebb » Fri Dec 07, 2018 10:17 am

Does H2Se have dipole-dipole forces as well as London dispersion forces?

Eruchi Okpara 2E
Posts: 53
Joined: Fri Sep 28, 2018 12:28 am

Re: Boiling Point

Postby Eruchi Okpara 2E » Sun Dec 09, 2018 1:47 am

Can't you also determine which compound has a higher/ lower boiling point by looking at branching?

Heidi Ibarra Castillo 1D
Posts: 60
Joined: Fri Sep 28, 2018 12:19 am

Re: Boiling Point

Postby Heidi Ibarra Castillo 1D » Sun Dec 09, 2018 7:39 pm

H2Se has the higher boiling point due to having a larger mass and more electrons

Heidi Ibarra Castillo 1D
Posts: 60
Joined: Fri Sep 28, 2018 12:19 am

Re: Boiling Point

Postby Heidi Ibarra Castillo 1D » Sun Dec 09, 2018 7:41 pm

^H2Se does have dipole dipole forces


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