In `OF_2`, the number of bond pairs and lone pairs of electrons are respectively,

Options

A. `2,6`
B. `2,8`
C. `2,10`
D. `2,9`

Explanation

To determine the number of bond pairs and lone pairs of electrons in the molecule OF₂ (oxygen difluoride), we can follow these steps:

### Step-by-Step Solution:

1. **Count the Valence Electrons**:
- Oxygen (O) has 6 valence electrons.
- Each Fluorine (F) atom has 7 valence electrons, and there are 2 Fluorine atoms.
- Total valence electrons = 6 (from O) + 2 × 7 (from 2 F) = 6 + 14 = 20 valence electrons.

2. **Draw the Skeleton Structure**:
- Oxygen will be the central atom, and it will form single covalent bonds with the two Fluorine atoms.
- This gives us the skeleton structure: F-O-F.

3. **Form Covalent Bonds**:
- Each bond between Oxygen and Fluorine uses 2 electrons. Since there are 2 bonds, we use 2 × 2 = 4 electrons.
- Remaining valence electrons = 20 - 4 = 16 electrons.

4. **Complete the Octet**:
- Fluorine needs 6 more electrons to complete its octet (each F needs 8 total).
- Oxygen also needs 4 more electrons to complete its octet (it needs 8 total).
- Distributing the remaining 16 electrons:
- Each Fluorine gets 6 electrons (3 lone pairs each), using 12 electrons.
- Oxygen gets 4 electrons (2 lone pairs), using 4 electrons.
- Total used = 4 (bonds) + 12 (for F) + 4 (for O) = 20 electrons, which matches our total.

5. **Count Bond Pairs and Lone Pairs**:
- **Bond Pairs**: There are 2 bond pairs (one for each O-F bond).
- **Lone Pairs**:
- Oxygen has 2 lone pairs.
- Each Fluorine has 3 lone pairs.
- Total lone pairs = 2 (O) + 3 (F1) + 3 (F2) = 8 lone pairs.

### Final Answer:
The number of bond pairs and lone pairs of electrons in OF₂ is:
- **Bond pairs**: 2
- **Lone pairs**: 8