Which of the following molecule has triple bond ?

Options

A. `O_(2)`
B. `N_(2)`
C. `P_(4)`
D. `S_(8)`

Answer

To determine which of the given molecules has a triple bond, we can analyze the molecular structures of the options provided. Here’s a step-by-step solution:

### Step 1: Identify the Molecules
Let's assume the options given are:
1. O2 (Oxygen)
2. N2 (Nitrogen)
3. P4 (Phosphorus)
4. S8 (Sulfur)

### Step 2: Analyze O2 (Oxygen)
- Oxygen has 6 valence electrons.
- When we draw the Lewis structure for O2, we find that:
- Each oxygen shares two pairs of electrons (double bond).
- Thus, O2 has a **double bond**, not a triple bond.

### Step 3: Analyze N2 (Nitrogen)
- Nitrogen has 5 valence electrons.
- In the Lewis structure for N2:
- Each nitrogen shares three pairs of electrons (triple bond).
- Thus, N2 has a **triple bond**.

### Step 4: Analyze P4 (Phosphorus)
- Phosphorus has 5 valence electrons.
- In the Lewis structure for P4:
- Each phosphorus atom forms single bonds with three other phosphorus atoms.
- Thus, P4 has **single bonds**, not a triple bond.

### Step 5: Analyze S8 (Sulfur)
- Sulfur has 6 valence electrons.
- In the Lewis structure for S8:
- Each sulfur atom shares two pairs of electrons with adjacent sulfur atoms.
- Thus, S8 has **single bonds**, not a triple bond.

### Conclusion
After analyzing all the given molecules, we find that:
- **N2 (Nitrogen)** is the only molecule that has a **triple bond**.

### Final Answer
The molecule that has a triple bond is **N2**.

---