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

Electronegativity is the tendency of an atom to attract a bonding pair of electrons. The electronegativity increases as you move across a period (from left to right) and decreases as you move down a group (from top to bottom). Let's analyze the given elements: - \( \text{N} \) (Nitrogen) has an electronegativity value of 3.04. - \( \text{O} \) (Oxygen) has an electronegativity value of 3.44. - \( \text{F} \) (Fluorine) has the highest electronegativity value of 3.98. - \( \text{Ne} \) (Neon) is a noble gas and does not readily form bonds, so it does not have a defined electronegativity in typical cases. The correct order of electronegativity from highest to lowest is \( F>O>N>Ne \). Hence, the correct answer is option (4) \( c>b>d>a \).