Structures of Polyatomic Species

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Miya Eberlein 1J
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Joined: Fri Sep 25, 2015 3:00 am

Structures of Polyatomic Species

Postby Miya Eberlein 1J » Sun Oct 18, 2015 11:03 pm

I'm confused about something in the course reader on page 67. When making a structure of a polyatomic species, the example used (NH4)2SO4, and it has 9 valence electrons. how do we know that its minus 1 e or (NH4)+? why does that happen? same thing with the SO4, how do we know its SO4 minus 2 electrons?

Jason Ching
Posts: 16
Joined: Fri Sep 25, 2015 3:00 am

Re: Structures of Polyatomic Species

Postby Jason Ching » Sun Oct 18, 2015 11:22 pm

For SO4 there are four oxygens each having a minus 1 charge and the sulfur itself having a plus 2 charge. Thus SO4 having a total net charge of -2. You can find out the charge for each of the elements by using the formal charge(FC) formula = V -(L+S/2). V being the valence electron, L being the lone pair and S being the shared electrons in the Lewis structure. It is NH4+ because the electron is shared with the SO4-2 to make Sulfate complete an octet (i.e become more stable).


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