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Mya Majewski 1L
Posts: 89
Joined: Fri Sep 25, 2015 3:00 am


Postby Mya Majewski 1L » Thu Oct 22, 2015 8:12 pm

When making a Lewis Structure, how do you know whether to put a single, double, or triple bond? I know you look at the valence electrons but I get confused when deciding how many dots are around the element

Shrita Pendekanti 4B
Posts: 22
Joined: Fri Sep 25, 2015 3:00 am

Re: Bonds

Postby Shrita Pendekanti 4B » Thu Oct 22, 2015 8:39 pm

One of the most important things to look at when drawing Louis Structures is the formal charge of each atom. Doing this should help you figure out which bond will provide for the most stable structure. (Stability is essentially based on filling necessary octets in the most energy efficient manner.)

Vanessa A 3F
Posts: 29
Joined: Fri Sep 25, 2015 3:00 am

Re: Bonds

Postby Vanessa A 3F » Thu Oct 22, 2015 9:02 pm

When making a Lewis Structure, you don't initially know how many bonds there will end up being. So start by counting up all of the valence electrons each atom in the molecule has. This is how many electrons there need to be in the Lewis structure.
Then use a single bond to connect them to each other, and then give each atom an appropriate number of lone pairs. Now count up all of the electrons in your Lewis Structure. If this number is greater than the valence electron number you started with, you know you will have to add bonds, until the number of electrons in your structure matches the number of valence electrons you initially calculated. Keep in mind, each bond line signifies two electrons.
This video example may be helpful:

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