Which of the following indicates that the bonding in hydrogen chloride is covalent ?
(i) an aqueous solution of hydrogen chloride form hydrogen with metals
(ii) hydrogen chloride is a gas
(iii) hydrogen chloride is not acidic in the absence of water
(iv) dry hydrogen chloride is a non-conductor of electricity

Options

A. (ii), (iii) and (iv) only
B. (i), (ii) and (iii) only
C. (i) and (iv) only
D. (i), (ii), (iii) and (iv)

Answer

To determine which of the statements indicates that the bonding in hydrogen chloride (HCl) is covalent, we will analyze each option step by step.

### Step 1: Analyze Statement (i)
**Statement:** An aqueous solution of hydrogen chloride forms hydrogen with metals.

**Analysis:** This statement indicates that HCl can react with metals to produce hydrogen gas. However, this reaction does not necessarily indicate covalent bonding. It can occur with ionic compounds as well. Therefore, this statement does not support the idea that the bonding in HCl is covalent.

**Conclusion:** This statement does not indicate covalent bonding.

### Step 2: Analyze Statement (ii)
**Statement:** Hydrogen chloride is a gas.

**Analysis:** Hydrogen chloride exists as a gas at room temperature. Gaseous compounds are often covalent in nature, as they typically consist of molecules rather than ions. The fact that HCl is a gas supports the idea of covalent bonding.

**Conclusion:** This statement indicates covalent bonding.

### Step 3: Analyze Statement (iii)
**Statement:** Hydrogen chloride is not acidic in the absence of water.

**Analysis:** Hydrogen chloride (HCl) is a strong acid when dissolved in water, forming H⁺ and Cl⁻ ions. However, in its dry gaseous state, it does not exhibit acidic properties because it lacks the ability to dissociate into ions. This behavior is characteristic of covalent compounds, which do not ionize in the absence of a solvent.

**Conclusion:** This statement indicates covalent bonding.

### Step 4: Analyze Statement (iv)
**Statement:** Dry hydrogen chloride is a non-conductor of electricity.

**Analysis:** For a substance to conduct electricity, it must have free-moving charged particles (ions or electrons). Dry hydrogen chloride does not dissociate into ions and therefore does not conduct electricity. This property is typical of covalent compounds, which do not have free ions in their pure form.

**Conclusion:** This statement indicates covalent bonding.

### Final Conclusion
Based on the analysis:
- Statement (i) does not indicate covalent bonding.
- Statements (ii), (iii), and (iv) indicate covalent bonding.

Thus, the correct answer is that statements (ii), (iii), and (iv) indicate that the bonding in hydrogen chloride is covalent.

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