Lecture 1 Example


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VGonzalez
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Joined: Fri Sep 28, 2018 12:18 am

Lecture 1 Example

Postby VGonzalez » Thu Nov 01, 2018 6:50 pm

In Monday's lecture we did an example with a nitrate ion. Dr. Lavelle wrote how many valence electrons there were in Nitrogen and Oxygen and then he wrote -1 charge. Why did he write the -1 charge? Is that the value we have to calculate with the formal charge equation?

Alyssa Wilson 2A
Posts: 65
Joined: Fri Sep 28, 2018 12:18 am

Re: Lecture 1 Example

Postby Alyssa Wilson 2A » Thu Nov 01, 2018 6:59 pm

I believe Dr. Lavelle wrote -1 since we know from the question that NO3^- has a negative charge, because it is an anion. Therefore we have to add one valence electron into the equation of our lewis structure. Hope this helps!

Kailey Nichols 4B
Posts: 30
Joined: Fri Sep 28, 2018 12:28 am

Re: Lecture 1 Example

Postby Kailey Nichols 4B » Fri Nov 02, 2018 12:22 am

Yes, in a nitrate ion (NO3-), N has 5 valence electrons, O has 18 valence electrons (6 x 3 = 18), and because this is an anion with a -1 charge, Dr. Lavelle added another e- for a total of 24 e-. So the -1 charge was not due to the formal charge equation, but rather it was already given by NO3-.


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