Question

Correct order of electronegativity in below elements:

• A. \( \text{1s}^2 \text{2s}^2 \text{2p}^3 \) (N)
• B. \( \text{1s}^2 \text{2s}^2 \text{2p}^4 \) (O)
• C. \( \text{1s}^2 \text{2s}^2 \text{2p}^5 \) (F)
• D. \( \text{1s}^2 \text{2s}^2 \text{2p}^6 \) (Ne)

Hint:

Remember that electronegativity increases across periods and decreases down groups in the periodic table. The noble gases (like Ne) do not typically have electronegativity values.

Answer 1

The Correct Option is D

The tendency of an atom to attract electrons in a bond is termed electronegativity. This property increases across a period (left to right) and decreases down a group (top to bottom). Analyzing the provided elements:- Nitrogen (\( \text{N} \)) exhibits an electronegativity of 3.04.- Oxygen (\( \text{O} \)) has an electronegativity of 3.44.- Fluorine (\( \text{F} \)) possesses the highest electronegativity at 3.98.- Neon (\( \text{Ne} \)), as a noble gas, typically does not form bonds and thus lacks a defined electronegativity.The electronegativity ranking from highest to lowest is \( F>O>N>Ne \). Therefore, the correct option is (4), corresponding to \( c>b>d>a \).