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Postby Goyama_2A » Sat Nov 02, 2019 11:25 am

What are the general exceptions to the octet rule we should know? And how many electrons can those exceptions hold when bonding?

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Re: Bonding

Postby kpang_4H » Sat Nov 02, 2019 11:53 am

The 3rd row and beyond can have expanded octet, more than 8 electrons. H, He, Li, Be will always have an incomplete octet. The 13th column or the Boron column can have an incomplete octet.

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Re: Bonding

Postby Maia_Jackson_2C » Sun Nov 03, 2019 6:51 pm

I don't think there is a specific number of electrons that each expanded octet can hold that we need to know, just know that it is more than 8

Callum Guo 1H
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Re: Bonding

Postby Callum Guo 1H » Sun Nov 03, 2019 7:12 pm

Anything in period 3 or larger can have a expanded shell because electrons can fill the D orbital

Sofia Barker 2C
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Re: Bonding

Postby Sofia Barker 2C » Sun Nov 03, 2019 10:37 pm

Hydrogen, Helium, and Lithium will follow a duet rule. This is because their electrons are present the 1s orbital, which is most stable when full (2 electrons). Hydrogen thus wants to gain an electron while Lithium wants to lose an electron in order to have the most stable electron configuration, which is that of Helium.

Aadil Rehan 1D
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Re: Bonding

Postby Aadil Rehan 1D » Sun Nov 03, 2019 11:26 pm

Not an exception to the octet rule, but to the typical electron configuration pattern - chromium and copper. They're [Ar]3d54s1 and [Ar]3d104s1 respectively, you just have to know that a half-filled or full d is more stable than a full s subshell.

Arvind 4G
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Re: Bonding

Postby Arvind 4G » Thu Nov 07, 2019 10:44 am

The third row of the periodic table and beyond can have expanded octets as they have the d orbital available and are also larger atoms.

Juana Abana 1G
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Re: Bonding

Postby Juana Abana 1G » Thu Nov 07, 2019 8:51 pm

Anything from the third row the periodic table and the rows that follow can have expanded octets.

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