Question 4.25

[Megan Purl 1E]

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]

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]

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.