Question

The element with highest electronegativity value after fluorine is

• A. Nitrogen
• B. Oxygen
• C. Chlorine
• D. Bromine

Hint:

Electronegativity generally increases across a period and decreases down a group. Fluorine is the most electronegative element, followed by oxygen.

Answer 1

The Correct Option is B

Step 1: Recall Pauling's electronegativity values.
Electronegativity on Pauling's scale: F = 4.0 (highest of all elements), O = 3.5, N = 3.0, Cl = 3.0, C = 2.5, H = 2.1.
Step 2: Identify the element with highest electronegativity after F.
After F (4.0), the next highest is O (3.5). This is significantly higher than N (3.0) and Cl (3.0) which are tied for third place.
Step 3: Explain the trend: why O has higher electronegativity than N and Cl.
Oxygen is in Period 2, Group 16. It has higher nuclear charge than N and a smaller atomic radius. Despite N being in the same period, O has one more proton, drawing electrons more strongly. Cl is in Period 3 with larger radius, reducing electron attraction.
Step 4: Compare N and Cl.
N and Cl have the same Pauling electronegativity (3.0). N is smaller but in the same period as O; Cl is larger but has the same group trends. Both are less electronegative than O.
Step 5: Order from highest to lowest electronegativity.
F (4.0) > O (3.5) > N = Cl (3.0) > C (2.5). After fluorine, oxygen has the second highest electronegativity.
Step 6: Final answer.
The element with the highest electronegativity after fluorine is Oxygen (O), with a Pauling electronegativity value of 3.5.
\[ \boxed{\text{Oxygen (option 2), electronegativity = 3.5}} \]