What is the total number of valence electrons represented in the Lewis structures of each of the following molecules or molecular ions? Draw their Lewis diagrams before responding: a) HOCl molecule, b) ICl4 ion, c) N2O molecule

To determine the total number of valence electrons represented in the Lewis structures of HOCl, ICl₄^–, and N₂O, we first need to consider the valence electrons contributed by each atom in these molecules.

a) HOCl Molecule

In HOCl, we have:

• Hydrogen (H) contributes 1 valence electron.
• Oxygen (O) contributes 6 valence electrons.
• Chlorine (Cl) contributes 7 valence electrons.

Adding these together, we find:

Total for HOCl: 1 + 6 + 7 = 14 valence electrons.

b) ICl₄^– Ion

For the ICl₄^– ion, we account for the following:

• Iodine (I) contributes 7 valence electrons.
• Each Chlorine (Cl) contributes 7 valence electrons, and there are 4 Cl atoms.
• The extra negative charge adds 1 more electron.

Calculating the total, we have:

Total for ICl₄^–: 7 + (7 x 4) + 1 = 7 + 28 + 1 = 36 valence electrons.

c) N₂O Molecule

In the N₂O molecule, we consider:

• Nitrogen (N) has 5 valence electrons, and since there are 2 nitrogen atoms: 5 x 2 = 10.
• Oxygen (O) contributes 6 valence electrons.

So, the total is:

Total for N₂O: 10 + 6 = 16 valence electrons.

In summary, the total number of valence electrons for each molecule is:

• HOCl: 14 valence electrons
• ICl₄^–: 36 valence electrons
• N₂O: 16 valence electrons