Question 4.25

(Polar molecules, Non-polar molecules, etc.)

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Megan Purl 1E
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Joined: Fri Sep 29, 2017 7:07 am

Question 4.25

Postby Megan Purl 1E » Sun Nov 12, 2017 11:42 pm

Can someone help with the following question:
Write the Lewis Structure and predict whether each of the following molecules is polar or nonpolar: a) CH2Cl; b)CCl4; c)CS2; d)SF4.

K Stefanescu 2I
Posts: 68
Joined: Fri Sep 29, 2017 7:04 am

Re: Question 4.25

Postby K Stefanescu 2I » Mon Nov 13, 2017 12:09 pm

1) Draw the Lewis structures of the molecules in the question.

2) Determine which bonds have the greatest difference in electronegativity (for example, C-Cl has a greater difference than C-H).

3) Draw the dipole moments for those bonds of greatest electronegativity difference.

4)Compare the directions of the dipole moments- if they cancel, it is nonpolar; if they do not cancel, it is polar.

Cooper1C
Posts: 50
Joined: Fri Sep 29, 2017 7:07 am

Re: Question 4.25

Postby Cooper1C » Mon Nov 13, 2017 4:39 pm

You also have to think about the shape of the molecule. For example, in part (a) (CH2Cl2), the molecule has a tetrahedral shape, so the dipole moments do not cancel, even though they look they could in the Lewis structure -> The molecule is polar.


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