octect rule

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Maldonado3K
Posts: 39
Joined: Fri Sep 29, 2017 7:07 am

octect rule

Postby Maldonado3K » Sun May 13, 2018 3:16 am

How do we know when we can break the octet rule? If we are allowed to break it, should we always find a way not to or can we just break it if its faster in helping us draw the lewis structure? Would we penalized?

Tina Wen 1G
Posts: 31
Joined: Fri Apr 06, 2018 11:05 am

Re: octect rule

Postby Tina Wen 1G » Sun May 13, 2018 4:12 am

We can break the octect rule when the bonding atom has empty d or f orbitals that are available for additional bonding. We should always find the optimized bonding with individual formal charge closest to zero. First try following the octect rule but if involving d or f orbitals would lead to more stable structure then break the octect rule.

004985802
Posts: 27
Joined: Fri Feb 02, 2018 3:00 am

Re: octect rule

Postby 004985802 » Sun May 13, 2018 12:24 pm

atoms only break the octet rule when moving additional electrons to the d or f orbitals make the atom more stable, which can be determined by calculating formal charges to determine how many electrons are required

Amanda 1A
Posts: 31
Joined: Fri Apr 06, 2018 11:01 am

Re: octect rule

Postby Amanda 1A » Sun May 13, 2018 12:44 pm

we can break the octet rule when when there are available d or f orbitals (3rd row and below of the periodic table) and to get the most stable bonding (or get the formal charges of the atoms in the molecule closest to zero). I think on the tests, we are required to draw the most stable molecule, and if we can or need to break the octet rule in order to do that, we should.

Amir Akhavan 1E
Posts: 34
Joined: Fri Apr 06, 2018 11:01 am

Re: octect rule

Postby Amir Akhavan 1E » Sun May 13, 2018 1:37 pm

You can only break the octet rule if the atom has extra electrons available from the d or f subshells. If not the rule cannot be broken and a maximum of 8 electrons must be used for that element. Only break the rule when it allows for a proper lewis structure to be formed.


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