Draw and Explain the Lewis Structure for CN2H2

To draw the Lewis structure for CN₂H₂, we need to first determine the total number of valence electrons in the molecule.

Carbon (C) has 4 valence electrons, Nitrogen (N) has 5 valence electrons, and Hydrogen (H) has 1 valence electron. Therefore, for CN₂H₂:

• Carbon: 1 × 4 = 4
• Nitrogen: 2 × 5 = 10
• Hydrogen: 2 × 1 = 2

This gives us a total of:

Total valence electrons = 4 + 10 + 2 = 16

Next, we start by placing the carbon atom in the center, as it is less electronegative than nitrogen. We can arrange the two nitrogen atoms and the two hydrogen atoms around the carbon:

H
|
H-C-N
|
N

Now, we will start filling the bonds. Each bond requires 2 electrons:

1. Place a single bond between C and each N.
2. Place a single bond between C and each H.

Now we have:

H
|
H-C=N
|
N

This gives us 8 electrons used (2 from C-H bonds and 4 from C-N bonds), leaving us with 8 electrons remaining.

Next, we distribute the remaining electrons to satisfy the octet rule. We can place a lone pair on each nitrogen atom:

H
|
H-C:N:
|
N:

Now we’ve used 12 electrons (including the bonds):

– 4 for two C-H bonds
– 4 for two C-N bonds
– 4 for the lone pairs on nitrogen.

This structure leaves us with 4 electrons remaining, which we can use to form a triple bond between the carbon and one of the nitrogen atoms. This results in:

H
|
H-C≡N
|
N:

Now, the carbon atom has 8 electrons (4 from the triple bond and 2 from the C-H bonds), and both nitrogen atoms also satisfy the octet rule.

In summary, the Lewis structure for CN₂H₂ shows a carbon at the center double bonded to one nitrogen and single bonded to the other nitrogen with connected hydrogens.