Question:
Identify the element having highest value of first ionization enthalpy.
Identify the element having highest value of first ionization enthalpy.
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Trend: Noble gases ↑ IE, and IE decreases down the group → Ar > Xe.
Updated On: May 4, 2026
- Se
- Br
- Xe
- Ar
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The Correct Option is D
Solution and Explanation
Concept:
First ionization enthalpy increases:
• Across a period (left to right)
• Decreases down a group Noble gases have the highest ionization enthalpy due to stable electronic configuration.
Step 1: Analyze options.
• Se (Group 16) → lower than noble gases $\times$
• Br (Group 17) → high but less than noble gases $\times$
• Xe (Group 18) → high but lower than Ar (down the group) $\times$
• Ar (Group 18, above Xe) → highest \checkmark
Step 2: Conclusion. \[ \text{Argon has the highest first ionization enthalpy among given options} \]
First ionization enthalpy increases:
• Across a period (left to right)
• Decreases down a group Noble gases have the highest ionization enthalpy due to stable electronic configuration.
Step 1: Analyze options.
• Se (Group 16) → lower than noble gases $\times$
• Br (Group 17) → high but less than noble gases $\times$
• Xe (Group 18) → high but lower than Ar (down the group) $\times$
• Ar (Group 18, above Xe) → highest \checkmark
Step 2: Conclusion. \[ \text{Argon has the highest first ionization enthalpy among given options} \]
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