Calculate the total number of bond pairs and lone pairs of electrons present in `OF_(2)` molecule.

Options

A. 10
B. 4
C. 6
D. 8

Explanation

To calculate the total number of bond pairs and lone pairs of electrons in the `OF_(2)` molecule, we can follow these steps:

### Step 1: Determine the Valence Electrons
- Oxygen (O) has an atomic number of 8, which means it has 6 valence electrons (since its electron configuration is 1s² 2s² 2p⁴).
- Each Fluorine (F) atom has an atomic number of 9, which means it has 7 valence electrons. Since there are 2 fluorine atoms, the total number of valence electrons from fluorine is \(2 \times 7 = 14\).

### Step 2: Calculate Total Valence Electrons
- Total valence electrons in `OF_(2)` = Valence electrons from O + Valence electrons from F
- Total = 6 (from O) + 14 (from 2 F) = 20 valence electrons.

### Step 3: Draw the Lewis Structure
- In the Lewis structure of `OF_(2)`, the oxygen atom is in the center, and it forms two single bonds with two fluorine atoms.
- Each bond consists of 2 electrons, so 2 bonds will use \(2 \times 2 = 4\) electrons.

### Step 4: Calculate Remaining Electrons
- Remaining electrons after forming bonds = Total valence electrons - Electrons used in bonds
- Remaining = 20 - 4 = 16 electrons.

### Step 5: Assign Lone Pairs to Fluorine Atoms
- Each fluorine atom needs 3 lone pairs to complete its octet (since it already has 1 bond with oxygen).
- For 2 fluorine atoms, this uses \(2 \times 3 = 6\) electrons (3 pairs = 6 electrons per F).
- Remaining electrons after assigning to fluorine = 16 - 6 = 10 electrons.

### Step 6: Assign Lone Pairs to Oxygen Atom
- The oxygen atom will have 5 remaining electrons after bonding with fluorine.
- This means it will have 2 lone pairs (4 electrons) and 1 single unpaired electron.

### Step 7: Count Bond Pairs and Lone Pairs
- Bond pairs: There are 2 bond pairs (one bond with each fluorine).
- Lone pairs:
- Oxygen has 2 lone pairs.
- Each fluorine has 3 lone pairs.
- Total lone pairs = 2 (from O) + 3 (from F) + 3 (from F) = 8 lone pairs.

### Step 8: Total Pairs
- Total pairs = Bond pairs + Lone pairs = 2 (bond pairs) + 8 (lone pairs) = 10.

Thus, the total number of bond pairs and lone pairs in `OF_(2)` is **10**.