Draw the lewis Structure of the molecule N2

Question

How many valence electrons (total) are you working with?

Which atom is the central atom? What criteria must you use to decide this ?

Do the atoms in this molecule all obey the Octet rule ?

Are there any lone pair on the central atom in your final structure? How many?

What types of bonds (Single, Double, Triple) Exist between the central and outer atoms in your final structure?

Answer 1

Nitrogen has 5 valence electrons since it is in Group 5. you have 2 nitrogens, so 5 x 2 = 10. You are working with 10 valence electrons. And they do follow the octet rule. So to determine how many bonds they will form. Multiply 8 by 2, so you need 16 electrons to satisfy the octet rule. since you only have 10. Then 16-10 = 6. They need to share 6 electrons. Therefore 6/2 (since 1 bond contains to electrons), 3 bonds will be formed. Thus, you'll have:

        :N-triplebond-N:

sorry, i cant make a triple bond here...N2 is a gas

Answer 2

Best Lewis structure (minimizing formal charges)

:N ||| N:

" ||| " indicates triple bond.

" : " indicates lone pair.

Each N has 5 valence electrons, so you have 10 total VEs to work with.

The central atom must be N (obviously, since it's N2 and there are no other atoms present).  Do you think the Lewis structure I provided satisfy the octet rule?  Does each atom have 8 VEs bonded to it?  Count that yourself.

[Answer: see above]

Answer 3

Okay, so Valence of nitrogen is 5,

Following the octet rule, you can have:

N-N

N=N

N=-N   (triple bond)

or N==N (four bonds) ----> doesn't exist,

Now use lewis to solve,

First one, you have one bond, and 6 electrons (following octet rule), this gives you (5-(1+6)) = -2 on each N, wrong.

Second, One double bond, 4 electrons (following octet), so you have (5-(2+4) = -1 on each N, wrong again.

Third, One TB, 2 e on each N... (5-(3+2)) = 0, so you get a neutral N molecule = stable, this could be right.

So, based on lewis, a triple bond with 2 electrons on each N is correct. you get a stable molecule.

Total valence e = 4, central atom is for a triatomic molecules or more, N2 is diatomic and there is symmetry.

They do obey the octet

You can cofirm this at: http://grandinetti.org/Teaching/Chem121/...

Answer 4

N has 7 electron and the electronic configuration is 2.5.

Each N atom has 5 valence electrons

Since N2 is a diatomic molecules, we should not follow the Valence Shell Electron Pair Repulsion Theory (VSEPR Theory). As a result, there is no central atom presence.

According to Octet Rules, an atom tend to receive, donate or share their electron in order to achieve stable noble gas type of electroic configuration.

N atom form triple bond between another N atom by sharing 3 electron in their valence shell to achieve the stable octet electronic configuration in order to achieve stability. The bond formed is very strong and a lot of energy need to be used in order to break the bond.

Since there is no central atom presence, there is also no lone pair electron on the central atom.