lone pairs

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Savannah Mance 4G
Posts: 107
Joined: Fri Aug 30, 2019 12:17 am

lone pairs

Postby Savannah Mance 4G » Mon Nov 18, 2019 8:59 pm

How do you know when the central atom will have lone pairs instead of more bonds?

Alexis Webb 2B
Posts: 124
Joined: Thu Jul 11, 2019 12:15 am

Re: lone pairs

Postby Alexis Webb 2B » Mon Nov 18, 2019 9:07 pm

check the formal charges and also if its a hydrogen, it wouldn't have more than a single bond or if its a halogen (Group 7 elements), they usually like single bonds too, so any extra electrons would go on the central atom.

Ashley Tran 2I
Posts: 108
Joined: Thu Jul 11, 2019 12:17 am

Re: lone pairs

Postby Ashley Tran 2I » Mon Nov 18, 2019 9:11 pm

Also, check the octet rule to see if the central atom can hold more than 8 e- (whether those be lone pairs and/or bonds).

Pablo 1K
Posts: 118
Joined: Sat Feb 02, 2019 12:15 am

Re: lone pairs

Postby Pablo 1K » Mon Nov 18, 2019 9:27 pm

Do your normal lewis diagram and ensure all electrons are accounted for. If all bound atoms are full it means there is most likely a central atom with an expanded octet.

LeAirraBullingor2k
Posts: 77
Joined: Wed Mar 13, 2019 12:15 am

Re: lone pairs

Postby LeAirraBullingor2k » Sun Nov 24, 2019 11:48 pm

Make sure to check the valence electrons and remember that the atom that is more electronegative will hold more electrons.

AnayaArnold_3L
Posts: 56
Joined: Wed Sep 18, 2019 12:19 am

Re: lone pairs

Postby AnayaArnold_3L » Tue Dec 03, 2019 10:51 am

Do lone pairs automatically make a molecule nonpolar?

Kaitlynn Tran 3F
Posts: 54
Joined: Wed Sep 18, 2019 12:20 am

Re: lone pairs

Postby Kaitlynn Tran 3F » Thu Dec 05, 2019 11:34 pm

You would have to consider the total number of electrons, formal charges, the octet rule, and exceptions to the octet rule to know when to add a lone pair.

Kaitlynn Tran 3F
Posts: 54
Joined: Wed Sep 18, 2019 12:20 am

Re: lone pairs

Postby Kaitlynn Tran 3F » Thu Dec 05, 2019 11:36 pm

AnayaArnold_3L wrote:Do lone pairs automatically make a molecule nonpolar?


Yes, lone pairs disrupt symmetry, which makes molecules polar.


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