2E. 18

(Polar molecules, Non-polar molecules, etc.)

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Maggie Doan 1I
Posts: 61
Joined: Fri Sep 28, 2018 12:24 am

2E. 18

Postby Maggie Doan 1I » Sat Nov 24, 2018 10:32 pm

d) Draw the lewis structure, VESPR formula, molecular shape, and bond angles: N2O
Why doesn't the lewis structure for N2O have a lone pair?

Matthew Choi 2H
Posts: 59
Joined: Fri Sep 28, 2018 12:18 am

Re: 2E. 18

Postby Matthew Choi 2H » Sat Nov 24, 2018 11:12 pm

In total, there are 16 valence electrons. After drawing the skeletal structure for N2O with single bonds stemming from the central N to the other N and O, you are left with 12 valence electrons. The way I was taught in high school was to add the remaining electrons to the outer atoms to fill their octets first. If you do it this way, then you use up the remaining 12 valence electrons in completing the octet for the outer N and O. If you were to have remaining valence electrons, then you would add those to the central atom in the form of lone pairs, but since you don't have any left, then the central N wouldn't have a lone pair.


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