Which one among the following does not have the hydrogen bond?

Options

A. Phenol
B. Liquid `NH_(3)`
C. Water
D. HCl

Explanation

To determine which compound among the given options does not exhibit hydrogen bonding, we need to understand the conditions necessary for hydrogen bonding to occur. Here’s a step-by-step solution:

### Step 1: Understand the Conditions for Hydrogen Bonding
Hydrogen bonding occurs under the following conditions:
1. There must be a hydrogen atom covalently bonded to a highly electronegative atom (like fluorine, oxygen, or nitrogen).
2. The electronegative atom should be small in size to allow effective overlap and interaction with hydrogen.

### Step 2: Analyze Each Option
Now, let’s analyze each compound to see if they meet the criteria for hydrogen bonding.

1. **Phenol (C6H5OH)**:
- Contains the hydroxyl group (–OH).
- Oxygen is highly electronegative and small in size.
- Therefore, hydrogen bonding is possible in phenol.

2. **Liquid Ammonia (NH3)**:
- Contains nitrogen bonded to hydrogen.
- Nitrogen is also highly electronegative and small in size.
- Thus, hydrogen bonding can occur in liquid ammonia.

3. **Water (H2O)**:
- Contains two hydrogen atoms bonded to oxygen.
- Oxygen is highly electronegative and small.
- Therefore, water can form hydrogen bonds.

4. **Hydrochloric Acid (HCl)**:
- Contains hydrogen bonded to chlorine.
- Although chlorine is electronegative, it is relatively large in size compared to oxygen and nitrogen.
- The large size of chlorine prevents effective hydrogen bonding.

### Step 3: Conclusion
Based on the analysis, the compound that does not exhibit hydrogen bonding is **Hydrochloric Acid (HCl)**.

### Final Answer:
**HCl does not have hydrogen bonding.**

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