SCl4 Molecule

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Lelija Kazlauskas 3J
Posts: 50
Joined: Thu Jul 11, 2019 12:16 am

SCl4 Molecule

Postby Lelija Kazlauskas 3J » Sun Nov 17, 2019 6:02 pm

Why don't the dipole moments in SCl4 cancel each other out?

zachary_nhem_4I
Posts: 57
Joined: Sat Aug 17, 2019 12:18 am

Re: SCl4 Molecule

Postby zachary_nhem_4I » Sun Nov 17, 2019 6:05 pm

Because there is a lone pair that acts as an area of high electron density, thus, affecting the shape of and polarity of the molecule.

EvaLi_3J
Posts: 53
Joined: Wed Oct 02, 2019 12:16 am

Re: SCl4 Molecule

Postby EvaLi_3J » Sun Nov 17, 2019 6:08 pm

There is a lone pair on the S atom, which makes this a polar atom overall. The Cl atoms are not directly opposite from each other, and that's why their dipole moments don't cancel.

Amanda Mei 1B
Posts: 109
Joined: Sat Aug 24, 2019 12:16 am

Re: SCl4 Molecule

Postby Amanda Mei 1B » Sun Nov 17, 2019 6:13 pm

When there's a lone pair, it makes the molecular polar because the molecule isn't symmetrical and electrons won't be uniformly distributed.

Claire Stoecklein 1E
Posts: 49
Joined: Sat Jul 20, 2019 12:15 am

Re: SCl4 Molecule

Postby Claire Stoecklein 1E » Sun Nov 17, 2019 8:04 pm

Molecules with Sulfur as the central atom are often polar because Sulfur can accommodate more than 8 valence electrons. If there is an uneven number of bonded atoms or lone pairs, the molecule will be polar.

Camille 4I
Posts: 57
Joined: Sat Aug 24, 2019 12:18 am

Re: SCl4 Molecule

Postby Camille 4I » Sun Nov 17, 2019 11:13 pm

Is it safe to assume that a molecule like SCl4 that has a trigonal bipyramidal electron arrangement but with one lone pair, will become a seesaw shape?


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