Draw the Lewis structure for N2H2, a neutral molecule.

N2H2.

N has 5 + 5 = 10 electrons
H has 1 + 1 = 2 electrons.
Total of 12 electrons.
I would distribute the 12 as follows:
H:N::N:H which accounts for 8. Place a pair of unshared electron on the first N and a pair of unshared electrons on the second N. That will add 4 more electrons to make the 12. Note that there are two electrons for each H and 8 electrons for each N which satisfies the rule of 8 (and 2 for H). Note also that H:N:::N:H only accounts for 10 of the electrons and if an extra pair of electrons is added to one of the N atoms, the rule of 8 is not followed.

To draw the Lewis structure for N2H2, a neutral molecule, we need to determine the total number of valence electrons.

Step 1: Count the total number of valence electrons for each atom.

N (Nitrogen) has 5 valence electrons, and there are two nitrogen atoms, so that's a total of 2 x 5 = 10 electrons.
H (Hydrogen) has 1 valence electron, and there are two hydrogen atoms, so that's a total of 2 x 1 = 2 electrons.

Step 2: Calculate the total number of valence electrons.

Adding the valence electrons together, we have 10 electrons from the nitrogen atoms and 2 electrons from the hydrogen atoms, giving us a total of 12 valence electrons.

Step 3: Determine the central atom.

In Lewis structures, the atom with the lowest electronegativity is usually the central atom. In this case, nitrogen (N) has a lower electronegativity than hydrogen (H), so we will place the nitrogen atoms in the center.

Step 4: Connect the atoms using single bonds.

Since each hydrogen atom needs one electron to complete its valence shell, and each nitrogen atom needs three electrons to achieve an octet, we will connect the nitrogen atoms and hydrogen atoms using single bonds.

H H
\ /
N=N

Step 5: Distribute the remaining electrons.

We have already used 4 electrons in the N-N and N-H bonds (2 electrons per bond), leaving us with 12 - 4 = 8 electrons.

To fulfill the octet rule for nitrogen, we will distribute the remaining electrons as lone pairs around the nitrogen atoms.

H H
| |
H - N - N - H

Step 6: Check for octets.

Both nitrogen atoms now have a complete octet (with 8 electrons) by sharing electrons in the nitrogen-nitrogen bond and having lone pairs of electrons.

Step 7: Check the formal charges.

The formal charge is a theoretical charge assigned to each atom in a molecule. It helps determine the distribution of electrons and determine the most stable Lewis structure.

A formula for formal charge calculation: Formal charge = (number of valence electrons) - (number of lone pair electrons) - (number of shared electrons/2).

For N2H2:
- For each hydrogen atom: Formal charge = 1 - 0 - (2/2) = 0
- For each nitrogen atom: Formal charge = 5 - 2 - (8/2) = 0

Therefore, all the atoms in N2H2 have a formal charge of zero, fulfilling the octet rule and providing a stable Lewis structure.

To summarize, the Lewis structure for N2H2, a neutral molecule, is:

H H
| |
H - N - N - H