What is the Lewis dot structure for HOFO

What is the Lewis dot structure for HOFO?

The correct answer and explanation is :

Sure! Let’s go through it carefully:

---

Lewis Structure for HOFO:

The molecule HOFO (hypofluorous acid) can be drawn as:

H–O–F=O

Here’s the breakdown:

• Hydrogen (H) is bonded to an oxygen (O).
• That oxygen is bonded to a fluorine (F).
• The fluorine is double bonded to another oxygen (O).

Step-by-Step Explanation:

1. Count total valence electrons:

• H: 1 electron
• O: 6 electrons × 2 = 12 electrons
• F: 7 electrons
• Total = 1 + 12 + 7 = 20 valence electrons.

1. Sketch the skeleton structure:

• H always forms one bond, so it must be connected to O.
• F usually forms one bond (very electronegative, prefers single bond).
• Remaining O can form double bonds. A logical starting skeleton: H–O–F–O.

1. Connect atoms with single bonds first:
   Each single bond uses 2 electrons:

• H–O bond → 2 electrons
• O–F bond → 2 electrons
• F–O bond → 2 electrons
  → 3 bonds × 2 = 6 electrons used.

1. Distribute the remaining electrons:
   20 – 6 = 14 electrons left.

• Start filling outer atoms’ octets (especially F and O).

1. Adjust to satisfy octet rule:
   Fluorine prefers a single bond, so the bond between F and O must be a single bond.
   The second oxygen (the one after F) would prefer to complete its octet via a double bond with F. Corrected structure:

   H–O–F=O

6. Final check:

• H: 2 electrons (1 bond) → full for hydrogen.
• First O: 2 bonds (H and F) + 2 lone pairs → 8 electrons.
• F: 1 bond (single) + 3 lone pairs → 8 electrons.
• Second O: 1 double bond + 2 lone pairs → 8 electrons.

Why this structure is correct:

• Formal charges are minimized:
• Hydrogen: 0
• Oxygen: 0
• Fluorine: 0
• F, being highly electronegative, avoids extra bonds.
• O can form double bonds, satisfying octet.

Thus, the Lewis structure for HOFO is:

H–O–F=O

where every atom satisfies its octet (or duet for hydrogen), and the molecule is neutral with formal charges close to zero.

---