Polarity with non-polar bonds

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Polarity with non-polar bonds

Postby romina_4C » Fri Nov 22, 2019 10:20 am

Can a molecule be polar if it only has non-polar bonds? How do lone pairs factor into the polarity of a molecule?

Sartaj Bal 1J
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Re: Polarity with non-polar bonds

Postby Sartaj Bal 1J » Fri Nov 22, 2019 10:52 am

If a molecule only has non polar bonds, then the it will be non polar. Usually when a molecule has a lone pair, it is polar. However, in molecules like XeF4 (2 lone pairs), the dipole moments and lone pairs cancel out, rendering the molecule non polar. Hope this helps!

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Re: Polarity with non-polar bonds

Postby 405335722 » Fri Nov 22, 2019 11:31 am

as long as dipoles (differences in electronegativity) cancel out symmetrically around the central atom, the molecule will be nonpolar

Kaitlyn Ang 1J
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Re: Polarity with non-polar bonds

Postby Kaitlyn Ang 1J » Fri Nov 22, 2019 12:12 pm

Adding to this, make sure to recognize that just because a Lewis structure might look like it's symmetrical, you have to take into account the VSEPR shape to see if the molecule truly is symmetrical (i.e. tetrahedrals such as CH2Cl2 in a Lewis structure looks symmetrical, but in VSEPR, it's not)

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