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Topic: dipole moment  (Read 5162 times)

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dexangeles

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dipole moment
« on: November 11, 2004, 12:20:46 PM »
Can someone explain why chloromethane is categorized under "non-polar" eventhough it has a permanent dipole moment (1.9-2.0) that is even greater the water (1.8)
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Demotivator

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Re:dipole moment
« Reply #1 on: November 11, 2004, 01:00:22 PM »
Chloromethane is a polar molecule.
However, there are those who use fast and loose characterizations to distinguish compounds that are miscible in water from those that are not.
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dexangeles

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Re:dipole moment
« Reply #2 on: November 11, 2004, 01:30:56 PM »
yes it's polar but they still catgeorize it under non-polar when it comes to bonding

it uses a induced-dipole induced-dipole force to bond to each other, why when it already is polar?
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Demotivator

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Re:dipole moment
« Reply #3 on: November 11, 2004, 03:29:40 PM »
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dexangeles

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Re:dipole moment
« Reply #4 on: November 13, 2004, 12:23:26 AM »
if you look up bonding of CH3Cl induced dipole - induced dipole is what's used to describe the bonding

even my Gen Chem and Organic books say it, but don't reason out why  :(
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