A: Hg is a liquid transition metal
R: It has strong metallic bonding

Options

A. If both Assertion & Reason are true and the reason is the correct explanation of the assertion, then mark (1)
B. If both Assertion & Reason are true but the reason is not the correct explanation of the assertion, then mark (2)
C. If Assertion is true statement but Reason is false, then mark (3)
D. If both Assertion and Reason are false statements, then mark (4)

Answer

To analyze the assertion (A) and reasoning (R) regarding mercury (Hg), we will break down the information step by step.

### Step 1: Understanding the Assertion (A)
The assertion states that "Hg is a liquid transition metal."

- **Analysis**: Mercury (Hg) is indeed a liquid at room temperature, which is a unique characteristic among metals. However, to classify it as a transition metal, we need to consider its electron configuration and oxidation states.

### Step 2: Transition Metal Definition
Transition metals are defined as d-block elements that have an incomplete d-subshell in their elemental state or in one of their oxidation states.

- **Electron Configuration of Hg**: The electron configuration of mercury is [Xe] 4f14 5d10 6s2. In both its elemental form and common oxidation states (like Hg^2+), the d-orbitals are fully filled (5d10).

### Step 3: Conclusion on Assertion (A)
Since the d-orbital in mercury is fully filled in both its ground state and common oxidation state, it does not meet the criteria for being classified as a transition metal.

- **Final Conclusion for A**: Therefore, the assertion that "Hg is a liquid transition metal" is **false**.

### Step 4: Understanding the Reasoning (R)
The reasoning states, "It has strong metallic bonding."

- **Analysis of Metallic Bonding**: Transition metals typically exhibit strong metallic bonding due to the presence of unpaired d-electrons that can participate in bonding. However, in the case of mercury, the d-orbitals are fully filled.

### Step 5: Conclusion on Reasoning (R)
Since the d-orbitals in mercury are fully filled, it does not have the same capacity for metallic bonding as other transition metals like iron, cobalt, or nickel, which have unpaired d-electrons.

- **Final Conclusion for R**: Thus, the reasoning that "It has strong metallic bonding" is also **false**.

### Step 6: Final Answer
Both the assertion (A) and the reasoning (R) are **false**.

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