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### Lewis Structure for N2O

Posted: Sun Nov 04, 2018 10:10 pm
I'm confused on trying to write out a Lewis Structure for N2O. How would it be written/Which atom goes in the center of the Lewis Structure in this case and why?

### Re: Lewis Structure for N2O

Posted: Sun Nov 04, 2018 10:18 pm
N goes in the center because you want to have the lowest ionization energy element in the center. The structure has a triple bond to the other N atom, and a single on the O atom.

### Re: Lewis Structure for N2O

Posted: Mon Nov 05, 2018 4:50 pm
^but doesn't Oxygen have a lower Ionization Energy than Nitrogen because Nitrogen is more stable due to having a half-filled p-orbital?

### Re: Lewis Structure for N2O

Posted: Mon Nov 05, 2018 5:19 pm
Nitrogen should be in the center of the Lewis structure since it is the least electronegative atom of the two.

### Re: Lewis Structure for N2O

Posted: Mon Nov 05, 2018 11:22 pm
why is nitrogen more electronegative than oxygen? Does it relate to the number of electrons filling the d-orbital?

### Re: Lewis Structure for N2O

Posted: Tue Nov 06, 2018 12:01 am
Oxygen is more electronegative than nitrogen, thus nitrogen is the LEAST electronegative of the two and should be in the center.

### Re: Lewis Structure for N2O

Posted: Tue Nov 06, 2018 5:34 pm
I think people are confused because N has a higher ionization energy than O, but O is still more electronegative than N.

### Re: Lewis Structure for N2O

Posted: Tue Nov 06, 2018 7:19 pm
Oxygen is more electronegative than nitrogen because oxygen has a greater nuclear charge (more protons). Electronegativity in a sense measures how tightly an atoms holds its electrons, where atoms with high electronegativity are more likely to gain/share electrons rather than lose them. Nitrogen is placed in the center of the Lewis structure because it is the least electronegative, and since oxygen is more electronegative, its formal charge will have to be negative and therefore it is not placed in the center (even though it has lower ionization energy).

Nitrogen has a higher ionization energy because it has a half-filled 2p shell that makes it more stable unlike oxygen which has 2 unpaired electrons in its 2p shell which results in more electron repulsions (and therefore lowers the ionization energy). Ionization energy represents the amount of energy required to remove a valence electron.