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2E.25

Posted: Sun Nov 17, 2019 6:34 pm
by JamieVu_2C
How are CH2Cl2 and SF4 polar when their dipole moments cancel in their Lewis structures?

Re: 2E.25

Posted: Sun Nov 17, 2019 6:48 pm
by VLi_2B
Although CH2Cl2 is symmetrical, the differing polarities of the C–H and C–Cl bonds means the effect of the polar bonds is not cancelled, so the molecule is polar

SF4 has 4 bonds with one lone pair which makes it polar.

Re: 2E.25

Posted: Sun Nov 17, 2019 7:21 pm
by Kristina Rizo 2K
VLi_1L wrote:Although CH2Cl2 is symmetrical, the differing polarities of the C–H and C–Cl bonds means the effect of the polar bonds is not cancelled, so the molecule is polar

SF4 has 4 bonds with one lone pair which makes it polar.


Is it because the C-H bond is stronger than the C-Cl bond?

Re: 2E.25

Posted: Sun Nov 17, 2019 8:15 pm
by 005162520
How do we know that the C-H bond is stronger than C-Cl?