Expanded Octet

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ElizabethP1L
Posts: 59
Joined: Wed Nov 15, 2017 3:01 am

Expanded Octet

Postby ElizabethP1L » Sun May 13, 2018 4:23 pm

Hey, everyone! So I know elements from 3p and below on the periodic table are able to form an expanded octet (that is, they can have more than 8 overall electrons). However, do they ALWAYS form expanded octets (e.g. will Cl aways have more than 8 electrons in a Lewis structure)? Thanks in advance :)

Jared Pagal 1J
Posts: 24
Joined: Fri Apr 06, 2018 11:04 am

Re: Expanded Octet

Postby Jared Pagal 1J » Sun May 13, 2018 4:41 pm

I don't think that they will always have more than 8 electrons because it depends on the total count of the valence electrons in the molecule. For example, when sodium and chlorine form NaCl, Cl does not have more than 8 electrons in its valence shell. The expanded octet rule does not mean that they will always have an expanded octet, rather, it states that the elements in 3p and below are capable of accepting more electrons because they can hold electrons in their unfilled d orbitals.

Salena Chowdri 1I
Posts: 66
Joined: Fri Apr 06, 2018 11:02 am

Re: Expanded Octet

Postby Salena Chowdri 1I » Sun May 13, 2018 5:18 pm

These elements are capable of forming expanded octets (some more often than others), but you will not always find the elements in that state. For instance, compare Sulfur oxide (SO2) to sulfur hexafluoride (SF6).


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