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Polarity

Posted: Sun Nov 03, 2019 1:23 pm
by Shanzey
When labeling the dipole moment on a Lewis structure, how are we able to tell if the structure is polar or nonpolar? How are we able to tell if there is no net dipole?

Re: Polarity

Posted: Sun Nov 03, 2019 2:06 pm
by John Arambulo 1I
You would know based on the electronegativity of the elements by using the periodic trends and also by formal charges because a negative formal charge would mean the electron density his higher around that atom.

Re: Polarity

Posted: Sun Nov 03, 2019 3:55 pm
by Maya Gollamudi 1G
You can compare the electronegativity of the elements using the periodic table- there will be a greater electron density around the element with a higher electronegativity.

Re: Polarity

Posted: Sun Nov 03, 2019 5:58 pm
by Justin Quan 4I
If you see that all the dipole forces cancels out, then the molecule is nonpolar. However, if there is a net dipole moment that's not zero, then you can tell that the molecule is polar.

Re: Polarity

Posted: Sun Nov 03, 2019 6:05 pm
by alex_4l
Also, if the Lewis Structure contains all the same elements then the molecule is nonpolar, but if there is just one difference it can be polar.
For example, if there are 4 Cl attached to a centered Cl, that would have polar bonds but be a nonpolar molecule. But if there are 4 Cl attached to a centered C, that would have polar bonds and be a polar molecule.
It all really depends on the number of polar bonds--if there is an equal number of polar bonds, it's not polar, but if there is an inequality of polar bonds, it's polar.