Textbook 2E #27c

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

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Emma Strassner 1J
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Joined: Wed Sep 30, 2020 9:50 pm

Textbook 2E #27c

Postby Emma Strassner 1J » Fri Nov 20, 2020 11:57 pm

Predict whether each of the following molecules is likely to be polar or nonpolar:
(c) CHCl3
(trichloromethane, also known as chloroform, a common organic solvent and once used as an anesthetic).

Why exactly is this molecule polar?

Brett Lieuallen 2A
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Re: Textbook 2E #27c

Postby Brett Lieuallen 2A » Sat Nov 21, 2020 12:12 am

I believe this molecule is polar because the three Cl atoms have a higher electronegativity than H. As a result the electrons spend more time around the Cl atoms. This creates a negative charge on the Cl dense end of the molecule and a positive charge on the H end of the molecule.

Jessie Hsu 1C
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Re: Textbook 2E #27c

Postby Jessie Hsu 1C » Sat Nov 21, 2020 2:15 am

The C-Cl bond is polar resulting in a dipole on all three C-Cl bonds. CHCl3 has a tetrahedral shape, so having 3 polar bonds and 1 nonpolar bond doesn't allow the dipoles to cancel, resulting in an overall polar molecule.

Jiapeng Han 1C
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Re: Textbook 2E #27c

Postby Jiapeng Han 1C » Sat Nov 21, 2020 3:40 am

C-Cl bond is polar while C-H bond is non-polar. As a result, the dipoles can't cancel out.

Sejal Parsi 3K
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Re: Textbook 2E #27c

Postby Sejal Parsi 3K » Sat Nov 21, 2020 4:04 am

Hi! Like they said above, the C-Cl bond is polar while the C-H bond is non-polar, so the dipoles won’t cancel out.

Earl Garrovillo 2L
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Re: Textbook 2E #27c

Postby Earl Garrovillo 2L » Sat Nov 21, 2020 11:12 am

The difference in electronegativity between C and Cl would result in three of the bonds in CHCl3 to be polar. The C-H bond is also slightly polar but it's neither as strong as C-Cl or as numerous. Because of the shape of CHCl3 (tetrahedral if I'm not mistaken), then the electron density of the molecule would be towards the 3 C-Cl bonds which makes the molecule polar.

Emma Strassner 1J
Posts: 92
Joined: Wed Sep 30, 2020 9:50 pm

Re: Textbook 2E #27c

Postby Emma Strassner 1J » Sat Nov 21, 2020 8:28 pm

That makes sense, thank you!


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