Water `(H_(2)O)` is liquid while all others of equivalent and even higher molecular weight molecules are gaseous because of the presence of

Options

A. Covalent bonding between Hydrogen and Oxygen
B. Electrostatic attraction amongst water molecules
C. Hydrogen bond
D. Ionic bonds.

Answer

**Step-by-Step Solution:**

1. **Understanding the Question**: The question asks why water (H₂O) is in a liquid state while other molecules with similar or higher molecular weights are in a gaseous state.

2. **Identifying the Key Concept**: The key concept to focus on is the type of bonding present in water compared to other molecules.

3. **Analyzing Water's Structure**: Water consists of two hydrogen atoms covalently bonded to one oxygen atom. The oxygen atom is highly electronegative, which means it attracts electrons more strongly than hydrogen.

4. **Understanding Hydrogen Bonds**: The electronegativity of oxygen leads to the formation of hydrogen bonds between water molecules. These are weak attractions that occur between the positively charged hydrogen atoms of one water molecule and the negatively charged oxygen atoms of another.

5. **Comparing with Other Molecules**: Most other molecules with similar or higher molecular weights do not exhibit hydrogen bonding. Instead, they may have weaker van der Waals forces or no significant intermolecular forces, which allows them to exist in a gaseous state at room temperature.

6. **Conclusion**: The presence of hydrogen bonds in water creates a strong intermolecular attraction that keeps the molecules close together, resulting in a liquid state. In contrast, other molecules lack this strong intermolecular force, allowing them to remain gaseous.

7. **Final Answer**: Water is liquid while all others of equivalent and even higher molecular weight molecules are gaseous because of the presence of hydrogen bonds.

---