Draw the Lewis dot structure and predict the molecular structure of OF2.

The Correct Answer and Explanation is:

Lewis Dot Structure and Molecular Structure of OF₂

Correct Lewis Dot Structure of OF₂ (Oxygen Difluoride):

    ..
 :F:   :F:
  |     |
  O
 ..

Oxygen (O) is the central atom.
Each Fluorine (F) atom forms a single covalent bond with the oxygen.
Oxygen has two lone pairs of electrons.
Each Fluorine has three lone pairs of electrons.

Explanation

Oxygen difluoride (OF₂) is a molecule composed of one oxygen atom and two fluorine atoms. To determine its Lewis structure and molecular geometry, we follow these steps:

1. Count Valence Electrons:

Oxygen (group 16) has 6 valence electrons.
Each Fluorine (group 17) has 7 valence electrons.
Total = 6 (O) + 7×2 (F) = 20 valence electrons.

2. Draw the Skeleton Structure:

Place Oxygen in the center (less electronegative than Fluorine).
Connect each Fluorine to Oxygen with a single bond.

3. Distribute Remaining Electrons:

Two O–F bonds use 4 electrons (2 pairs).
Place 6 electrons (3 lone pairs) on each Fluorine to complete their octets: 6×2 = 12 electrons.
4 electrons remain. These are placed as two lone pairs on the central Oxygen.
Now all 20 electrons are used.

4. Check Octet Rule:

Each atom has 8 electrons around it: Oxygen has 2 bonds + 2 lone pairs, and each Fluorine has 1 bond + 3 lone pairs.

5. Predict Molecular Geometry (VSEPR Theory):

The central Oxygen has 2 bonding pairs and 2 lone pairs.
Electron geometry: Tetrahedral (4 regions of electron density).
Molecular geometry: Bent or Angular, because only the atom positions are considered (not lone pairs).

6. Bond Angle:

The ideal tetrahedral angle is 109.5°, but lone pair repulsion reduces this slightly. The actual bond angle is about 103°.

7. Polarity:

OF₂ is polar due to the bent shape and the high electronegativity of Fluorine atoms.

Thus, OF₂ has a bent molecular structure, a polar character, and a correct Lewis dot structure showing all valence electrons.