Amongst `H_2O, H_2S, H_2 Se` and `H_2 Te`, the one with the highest boiling point is :

Options

A. `H_(2)O` because of hydrogen bonding
B. `H_(2)Te` because of higher molecular weight
C. `H_(2)S` because of hydrogen boning
D. `H_(2)Se` because of lower molecular weight

Explanation

To determine which of the compounds \( H_2O, H_2S, H_2Se, \) and \( H_2Te \) has the highest boiling point, we can follow these steps:

### Step 1: Identify the Compounds
The compounds in question are:
- \( H_2O \) (water)
- \( H_2S \) (hydrogen sulfide)
- \( H_2Se \) (hydrogen selenide)
- \( H_2Te \) (hydrogen telluride)

### Step 2: Understand the Group Trends
All these compounds are hydrides of group 16 elements:
- Oxygen (O) for \( H_2O \)
- Sulfur (S) for \( H_2S \)
- Selenium (Se) for \( H_2Se \)
- Tellurium (Te) for \( H_2Te \)

As we move down the group from oxygen to tellurium, the molecular weight of the hydrides increases.

### Step 3: Consider Molecular Weight
The boiling point of a substance is generally influenced by its molecular weight. The trend in molecular weights for these compounds is:
- \( H_2O \) has a molecular weight of approximately 18 g/mol.
- \( H_2S \) has a molecular weight of approximately 34 g/mol.
- \( H_2Se \) has a molecular weight of approximately 78 g/mol.
- \( H_2Te \) has a molecular weight of approximately 130 g/mol.

From this trend, we can see that \( H_2Te \) has the highest molecular weight.

### Step 4: Consider Hydrogen Bonding
However, boiling points are also significantly affected by the presence of hydrogen bonding. \( H_2O \) exhibits strong hydrogen bonding due to the highly electronegative oxygen atom. This results in a much higher boiling point compared to the other hydrides, which do not exhibit hydrogen bonding to the same extent.

### Step 5: Compare Boiling Points
- \( H_2O \) has a boiling point of 100 °C.
- \( H_2S \) has a boiling point of -60 °C.
- \( H_2Se \) has a boiling point of -41 °C.
- \( H_2Te \) has a boiling point of -2 °C.

### Conclusion
Despite \( H_2Te \) having the highest molecular weight, the presence of hydrogen bonding in \( H_2O \) leads to it having the highest boiling point among the four compounds.

Thus, the compound with the highest boiling point is **\( H_2O \)**.

---