Explanation:

N2O3 is a covalent compound that contains two nitrogen atoms and three oxygen atoms. In order to determine the total number of lone pairs of electrons in N2O3, we need to first determine the Lewis structure of the molecule.

Lewis Structure:

To draw the Lewis structure of N2O3, we need to follow the following steps:

Step 1: Calculate the total number of valence electrons in the molecule.

N = 2 × 5 = 10

O = 3 × 6 = 18

Total = 28

Step 2: Determine the central atom.

In N2O3, both nitrogen atoms are central atoms.

Step 3: Connect the central atoms with single bonds.

N ≡ N

Step 4: Add electrons to the outer atoms to complete their octets.

O-N≡N-O

Step 5: Add any remaining electrons to the central atoms.

O-N≡N-O

Counting Lone Pairs:

In N2O3, each oxygen atom has two lone pairs of electrons. Therefore, the total number of lone pairs of electrons in N2O3 is:

Number of oxygen atoms × Number of lone pairs of electrons per oxygen atom

= 3 × 2

= 6

In addition, each nitrogen atom has one lone pair of electrons. Therefore, the total number of lone pairs of electrons in N2O3 is:

Number of nitrogen atoms × Number of lone pairs of electrons per nitrogen atom

= 2 × 1

= 2

Therefore, the total number of lone pairs of electrons in N2O3 is:

6 + 2 = 8

Hence, the correct answer is 8.