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Abigail Menchaca_1H
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Postby Abigail Menchaca_1H » Sun Dec 08, 2019 9:58 pm

How do you calculate the formal charges for each atom in CN-?

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Joined: Sat Aug 17, 2019 12:17 am

Re: Cyanide

Postby Jared_Yuge » Sun Dec 08, 2019 10:09 pm

just draw a lewis dot structure of the molecule, make sure to add the extra charge somewhere, and then count the electrons directly touching the atom and find the difference between the number of electrons its supposed to have in a neutral state. Do that for both, and experiment with the bonds and try to get the numbers as close as possible to 0 but if one has to be negative it should be the more electronegative atom, which in this case is the N.

Amanda Mei 1B
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Re: Cyanide

Postby Amanda Mei 1B » Sun Dec 08, 2019 10:11 pm

After drawing the Lewis structure, you would count the number of valence electrons of one of the atoms, then subtract the number of bonds that atom makes, then subtract the number of lone electrons on that atom. So valence electrons - (# bonds + # lone electrons).

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Re: Cyanide

Postby saigorijavolu2k » Sun Dec 08, 2019 10:23 pm

you draw the lewis structure and then subtract the valence electrons from bonds and lone pairs. CN has a triple bond.

Hussain Chharawalla 1G
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Re: Cyanide

Postby Hussain Chharawalla 1G » Sun Dec 08, 2019 10:35 pm

When drawing the lewis structure, make sure each element has a complete octet then count the lowest charge configuration.

Kevin Liu 1J
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Re: Cyanide

Postby Kevin Liu 1J » Sun Dec 08, 2019 11:02 pm

Based on the number of electrons bonded, the cyanide should have a triple bond between carbon and nitrogen along with a lone pair on each atom.

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