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Topic: LDF's  (Read 1617 times)

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Offline kershaw22

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LDF's
« on: March 11, 2014, 02:37:50 AM »
Why does H2Te have stronger LDF's compared to H20?
Doesn't water have hydrogen bonding as well? Which would make it stronger than H2Te...
Thanks!
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Offline Babcock_Hall

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Re: LDF's
« Reply #1 on: March 11, 2014, 09:11:01 AM »
London dispersion forces are not the same thing as hydrogen bonds.  What molecular property correlates with the strength of London forces?
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Offline kershaw22

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Re: LDF's
« Reply #2 on: March 12, 2014, 01:29:06 AM »
So it is between non-polar molecules/atoms? And increases as atomic and molecular size increases?
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Offline Babcock_Hall

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Re: LDF's
« Reply #3 on: March 12, 2014, 10:04:26 AM »
London forces occur between all molecules, polar and nonpolar.  They correlate with surface area of a molecule (I am not sure how perfect the correlation is).
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