The correct order of dipole moment of HF, HCl, HBr, HI and `H_(2)` is :

Options

A. `H_(2)ltHFltHClltHBrltHI`
B. `H_(2)ltHFltHBrltHClltHI`
C. `H_(2)ltHIltHBrltHClltHF`
D. `H_(2)ltHIltHBrltHFltHCl`

Explanation

To determine the correct order of dipole moments for the molecules HF, HCl, HBr, HI, and H₂, we will follow these steps:

### Step 1: Understand Dipole Moment
The dipole moment (μ) is a measure of the polarity of a chemical bond. It is defined as the product of the charge (Q) and the distance (D) between the charges. The formula is given by:
\[ \mu = Q \times D \]

### Step 2: Identify Electronegativity
The dipole moment depends on the difference in electronegativity between the two atoms involved in the bond. The greater the difference in electronegativity, the larger the dipole moment. The electronegativity values for the relevant elements are:
- Fluorine (F): 4.0
- Chlorine (Cl): 3.0
- Bromine (Br): 2.8
- Iodine (I): 2.5
- Hydrogen (H): 2.1

### Step 3: Analyze Each Molecule
1. **HF**: The electronegativity difference is highest between H and F, leading to the largest dipole moment.
2. **HCl**: The electronegativity difference between H and Cl is less than that of HF, resulting in a smaller dipole moment than HF.
3. **HBr**: The electronegativity difference between H and Br is less than that of HCl, leading to a smaller dipole moment than HCl.
4. **HI**: The electronegativity difference between H and I is the smallest among these bonds, resulting in the smallest dipole moment.
5. **H₂**: Since both atoms are the same, the dipole moment is zero.

### Step 4: Order the Dipole Moments
Based on the analysis:
- HF has the highest dipole moment.
- HCl comes next.
- HBr follows.
- HI has the lowest dipole moment among the halides.
- H₂ has a dipole moment of zero.

Thus, the order of dipole moments from highest to lowest is:
\[ \mu(HF) > \mu(HCl) > \mu(HBr) > \mu(HI) > \mu(H_2) = 0 \]

### Final Answer
The correct order of dipole moments is:
\[ HF > HCl > HBr > HI > H_2 \]