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Boiling Point

Posted: Fri Dec 07, 2018 2:16 am
by Nathan Mariano 2G
How do you determine which compound has the higher boiling point if they both have similar intermolecular forces? For example, H2S and H2Se.

Re: Boiling Point

Posted: Fri Dec 07, 2018 2:21 am
by gillianozawa4I
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!

Re: Boiling Point

Posted: Fri Dec 07, 2018 8:40 am
by katie_sutton1B
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.

Re: Boiling Point

Posted: Fri Dec 07, 2018 10:17 am
by taywebb
Does H2Se have dipole-dipole forces as well as London dispersion forces?

Re: Boiling Point

Posted: Sun Dec 09, 2018 1:47 am
by Eruchi Okpara 2E
Can't you also determine which compound has a higher/ lower boiling point by looking at branching?

Re: Boiling Point

Posted: Sun Dec 09, 2018 7:39 pm
by Heidi Ibarra Castillo 1D
H2Se has the higher boiling point due to having a larger mass and more electrons

Re: Boiling Point

Posted: Sun Dec 09, 2018 7:41 pm
by Heidi Ibarra Castillo 1D
^H2Se does have dipole dipole forces