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STATEMENT-1 : Hg exists in liquid state ...

STATEMENT-1 : Hg exists in liquid state at room. Temperature
and
STATEMENT-2: Hg has `(n-1)d^(10)ns^(2)` E.C.

A

Statement-1 is True , Statement-2 is True , Statement-2 is a correct explanation for Statement-1

B

Statement-1 is True , Statement-2 is True , Statement-2 is NOT a correct explanation for Statement-1

C

Statement-1 is True , Statement-2 is False

D

Statement-1 is False , Statement-2 is True

Text Solution

AI Generated Solution

The correct Answer is:
To analyze the statements provided in the question, we will evaluate each statement separately and determine their validity. ### Step 1: Evaluate Statement 1 **Statement 1:** Hg exists in liquid state at room temperature. - Mercury (Hg) is known to be the only metal that is liquid at room temperature (approximately 25°C). This property is well-documented in chemistry. - The reason for mercury's liquid state at room temperature is due to its unique electronic configuration and the weak metallic bonding associated with it. **Conclusion for Statement 1:** True ### Step 2: Evaluate Statement 2 **Statement 2:** Hg has `(n-1)d^(10)ns^(2)` electronic configuration. - Mercury belongs to Group 12 of the periodic table, which includes elements like Zinc (Zn), Cadmium (Cd), and Mercury (Hg). - The electronic configuration of mercury is: - For Zn: [Ar] 3d^10 4s^2 - For Cd: [Kr] 4d^10 5s^2 - For Hg: [Xe] 4f^14 5d^10 6s^2 - The notation `(n-1)d^(10)ns^(2)` refers to the electronic configuration where `n` is the principal quantum number of the outermost shell. For mercury, n=6, thus: - (n-1) = 5, so we have 5d^10 and 6s^2. - Therefore, the electronic configuration of mercury indeed fits the form `(n-1)d^(10)ns^(2)`. **Conclusion for Statement 2:** True ### Step 3: Determine the relationship between the statements - Both statements are true. - However, Statement 2 does not provide a correct explanation for Statement 1. The liquid state of mercury is primarily due to its weak metallic bonding, which arises from its fully filled d-orbitals (D^10 configuration), rather than just the electronic configuration itself. ### Final Conclusion - **Statement 1 is true.** - **Statement 2 is true.** - **Statement 2 is not a correct explanation for Statement 1.** Thus, the answer is that both statements are true, but Statement 2 does not explain Statement 1. ---
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