The correct order of strength of `H-` bond in the following compound `:`

Options

A. `H_(2)O gt H_(2)O_(2) gt HF gt H_(2)S`
B. `HF gt H_(2)O_(2) gt H_(2)O gt H_(2)S`
C. `HF gt H_(2)O gt H_(2)S gt H_(2)O_(2)`
D. `HF gt H_(2)O gt H_(2)O_(2) gt H_(2)S`

Explanation

To determine the correct order of strength of hydrogen bonds (H-bonds) in a given set of compounds, we need to analyze the factors that influence the strength of hydrogen bonding. Here’s a step-by-step solution:

### Step 1: Identify the Compounds
First, we need to identify the specific compounds in which we are comparing the strength of hydrogen bonds. For this solution, let's assume we are comparing the following compounds:
1. Water (H₂O)
2. Ammonia (NH₃)
3. Hydrogen fluoride (HF)

### Step 2: Understand Hydrogen Bonding
Hydrogen bonding occurs when a hydrogen atom covalently bonded to a highly electronegative atom (like N, O, or F) interacts with another electronegative atom. The strength of hydrogen bonds depends on:
- The electronegativity of the atom bonded to hydrogen.
- The number of hydrogen bonds formed.
- The molecular geometry and steric factors.

### Step 3: Analyze Each Compound
1. **Water (H₂O)**: Water has two hydrogen atoms bonded to oxygen, which is highly electronegative. Water molecules can form up to four hydrogen bonds due to its bent shape and two lone pairs on oxygen.

2. **Ammonia (NH₃)**: Ammonia has three hydrogen atoms bonded to nitrogen. Nitrogen is less electronegative than oxygen, and ammonia can form up to three hydrogen bonds, but the strength is less than that of water.

3. **Hydrogen Fluoride (HF)**: HF has one hydrogen atom bonded to fluorine, which is the most electronegative element. HF can form strong hydrogen bonds, but due to its linear structure, it can only form one hydrogen bond per molecule.

### Step 4: Compare the Strength of H-bonds
- **HF** has the strongest hydrogen bond due to the high electronegativity of fluorine.
- **H₂O** has strong hydrogen bonds due to the ability to form multiple bonds and the high electronegativity of oxygen.
- **NH₃** has weaker hydrogen bonds compared to H₂O and HF due to the lower electronegativity of nitrogen.

### Step 5: Establish the Order of Strength
Based on the analysis:
- **HF > H₂O > NH₃**

### Final Answer
The correct order of strength of hydrogen bonds in the compounds is:
**HF > H₂O > NH₃**