Draw the Lewis Structure for Hypochlorous Acid as HClO.

Draw the Lewis Structure for Hypochlorous Acid as HClO. Include formal charges

The Correct Answer and Explanation is:

Lewis Structure for Hypochlorous Acid (HClO):

Structure:

   H — O — Cl
        ..
       ..

Step-by-Step Lewis Structure:

1. Count valence electrons:
   • H = 1
   • O = 6
   • Cl = 7
     Total = 1 + 6 + 7 = 14 valence electrons
2. Skeleton structure:
   Place H bonded to O, and O bonded to Cl. Hydrogen must form only one bond.
   → H–O–Cl
3. Add electrons to complete octets:
   • H has 2 electrons (1 bond) – satisfies its duet rule.
   • O shares 2 electrons with H and 2 with Cl (4 total). Add 4 more as lone pairs to make 8.
   • Cl shares 2 electrons with O. Add 6 more as lone pairs to make 8.
   Structure:
   • H–O–Cl
   • O has 2 lone pairs
   • Cl has 3 lone pairs
4. Formal Charges:
   • H: Valence = 1, Bonds = 1, Lone Pairs = 0 → FC = 1 – 1 – 0 = 0
   • O: Valence = 6, Bonds = 2, Lone Pairs = 4 → FC = 6 – 4 – 2 = 0
   • Cl: Valence = 7, Bonds = 1, Lone Pairs = 6 → FC = 7 – 6 – 1 = 0

All atoms have formal charges of zero, so this is the most stable structure.

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Explanation

Hypochlorous acid (HClO) is a simple molecule consisting of hydrogen (H), chlorine (Cl), and oxygen (O). When drawing its Lewis structure, we begin by calculating the total number of valence electrons. Hydrogen contributes 1 electron, oxygen contributes 6, and chlorine contributes 7, giving us a total of 14 valence electrons.

Next, we construct the basic skeletal structure. Hydrogen, due to its limited bonding capacity, must be on the end and can form only one bond. This means it bonds to the oxygen atom, which can form two bonds. The remaining atom, chlorine, is then attached to the oxygen. This gives us the backbone: H–O–Cl.

We then distribute the remaining valence electrons to satisfy the octet rule for oxygen and chlorine. Oxygen already has two bonds (one to H and one to Cl), so it needs 4 more electrons (two lone pairs) to complete its octet. Chlorine, with one bond to oxygen, needs 6 more electrons (three lone pairs) to reach 8.

Finally, we assess formal charges to ensure the structure is the most stable one possible. Formal charge calculations show that each atom has a formal charge of zero, indicating that the electron distribution is optimal. This confirms that the drawn structure is the correct and most stable Lewis structure for HClO.

This Lewis structure helps explain the molecular geometry and polarity of HClO. The oxygen atom is the central atom, and the presence of lone pairs introduces bent geometry around it. The molecule is polar, with a partial negative charge near oxygen and a partial positive charge near hydrogen, contributing to the molecule’s reactivity and its effectiveness as a disinfectant in aqueous solutions.