Question

With reference to Pauling's Electronegativity scale, which one of the following options shows the correct order of electronegativity values of elements?

• A. Na $>$ Cs $>$ K
• B. Mg $>$ Al $>$ Si
• C. B $>$ C $>$ Al
• D. N $>$ S $>$ P

Hint:

In general, electronegativity increases across a period from left to right and decreases as we move down a group in the periodic table. Always refer to the periodic trends when comparing electronegativity values.

Answer 1

The Correct Option is D

Pauling's electronegativity scale measures the ability of an atom to attract electrons towards itself in a chemical bond. The electronegativity values of elements increase across a period and decrease down a group. Let's examine the elements in each option: - 
Option A: Na $>$ Cs $>$ K
- This order is incorrect because electronegativity decreases as we move down a group. Therefore, Cs should have the lowest electronegativity, followed by K, and Na having the highest among them. - 
Option B: Mg $>$ Al $>$ Si
- This is incorrect as well. Electronegativity increases as we move from left to right across a period, so Si should have a higher electronegativity than Al and Mg. - 
Option C: B $>$ C $>$ Al
- This is partially correct but not the best match. Carbon has a higher electronegativity than both B and Al, but we need to check other options for a more precise match. - 
Option D: N $>$ S $>$ P
- This is correct. Nitrogen (N) has the highest electronegativity among these three, followed by Sulfur (S) and Phosphorus (P), as electronegativity decreases as we move down a group. Thus, the correct order of electronegativity values is \(\text{N $>$ S $>$ P}\).