Question

Given below are two statements:
Statement I: The metallic radius of Na is 1.86 Å and the ionic radius of Na$^+$ is lesser than 1.86 Å.
Statement II: Ions are always smaller in size than the corresponding elements.
In the light of the above statements, choose the correct answer from the options given below:

• A. Statement I is correct but Statement II is false
• B. Both Statement I and Statement II are true
• C. Both Statement I and Statement II are false
• D. Statement I is incorrect but Statement II is true

Answer 1

The Correct Option is A

Step 1: Analysis of Statement I
- The metallic radius of Na (neutral sodium atom) is 1.86 ̊A.
- The ionic radius of Na⁺ is smaller than the neutral atom due to one fewer electron, leading to reduced electron-electron repulsion and increased effective nuclear charge on remaining electrons. - Thus, Statement I is correct.
Step 2: Analysis of Statement II - Cations (Na⁺) are consistently smaller than their neutral atoms, whereas anions (e.g., Cl^-) are larger than their neutral atoms due to augmented electron-electron repulsion in the outer shell.
- Consequently, ions are not universally smaller than their parent elements.
- Thus, Statement II is false.
Step 3: Conclusion - Statement I is accurate, while Statement II is inaccurate.
Final Answer: (1)