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Home Q & A Board Science-Related Homework Help Chemistry (Moderator: Laser_3)
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toni_malvina toni_malvina
wrote...
10 years ago
I keep finding such controversial "facts" all over the Internet on polarity tutorials and VSEPR geometry. Which is right, and why?
(When using arrows to show polarity on a VSEPR diagram, shouldn't the arrowheads of these bonds all be pointing in opposite directions, thus effectively cancelling each other out and making it non-polar? And it is symmetrical, depending on where you place each halogen.)
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wrote...
#1
10 years ago
In dichlorodifluoromethane, the fluorine is more electronegative than the chlorine,
So the side of the molecule with both F atoms will have a higher electron density then the side with the two chlorines.
Meaning you've got a polar molecule. not strongly polar, since all four halogen atoms will pull electrons away from the carbon, but the F pulls stronger than the Cl

Thank you for introducing me to valence pair electron pair repulsion.
Just because bond angles are symmetrical, doesn't mean the electron density will be.
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