The `N_(2)H_(4)` molecule contains :

Options

A. 4 lone pairs of electrons
B. 3 lone pairs of electrons
C. 2 lone pairs of electrons
D. No lone pair of electrons

Explanation

To determine the components of the N₂H₄ (hydrazine) molecule, we can follow these steps:

### Step 1: Identify the number of atoms in N₂H₄
The molecular formula N₂H₄ indicates that there are 2 nitrogen (N) atoms and 4 hydrogen (H) atoms.

### Step 2: Determine the valence electrons for each atom
- Nitrogen (N) has 5 valence electrons.
- Hydrogen (H) has 1 valence electron.

### Step 3: Calculate the total number of valence electrons
For N₂H₄:
- Total from nitrogen: 2 N × 5 = 10 valence electrons
- Total from hydrogen: 4 H × 1 = 4 valence electrons
- Total valence electrons = 10 + 4 = 14 valence electrons.

### Step 4: Draw the Lewis structure
1. Start by connecting the two nitrogen atoms with a single bond (1 bond = 2 electrons).
2. Each nitrogen atom will also bond with two hydrogen atoms. This means:
- Each nitrogen shares one electron with each hydrogen (2 H × 1 electron = 2 electrons).
3. After forming these bonds, we have used:
- 2 electrons for the N-N bond,
- 4 electrons for the N-H bonds (2 electrons for each nitrogen).
4. Total used so far = 2 (N-N) + 4 (N-H) = 6 electrons.
5. We have 14 - 6 = 8 electrons remaining, which can be placed as lone pairs on the nitrogen atoms.
6. Each nitrogen atom will have one lone pair of electrons.

### Step 5: Count the lone pairs
In the Lewis structure of N₂H₄:
- Each nitrogen atom has 1 lone pair.
- Therefore, the total number of lone pairs in N₂H₄ = 1 (from the first N) + 1 (from the second N) = 2 lone pairs.

### Conclusion
The N₂H₄ molecule contains **two lone pairs of electrons**.

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