Question:
In which of the following, elements are not in correct order with respect to the property mentioned in brackets?
In which of the following, elements are not in correct order with respect to the property mentioned in brackets?
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When evaluating "not in correct order" questions, always check for common anomalies like full-filled/half-filled orbitals in Ionization Enthalpy and specific group vs. period positioning for Electronegativity.
Updated On: Jun 8, 2026
- \( S < P < N < O \) (Electronegativity)
- \( Br < Ge < Ga < Ca \) (Atomic radius)
- \( Al < Mg < S < P \) (First ionization enthalpy)
- \( Mg < Ca < K < Cs \) (Metallic nature)
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The Correct Option is D
Solution and Explanation
Concept:
To determine if elements are in the correct order for a specific periodic property, we must consider the general trends in the periodic table:
• Electronegativity: Increases across a period (left to right) and decreases down a group.
• Atomic Radius: Decreases across a period and increases down a group.
• First Ionization Enthalpy: Generally increases across a period and decreases down a group.
• Metallic Nature: Decreases across a period and increases down a group.
Step 1: Evaluating Option (1) for Electronegativity.
Nitrogen (N) and Oxygen (O) are in the 2nd period, while Phosphorus (P) and Sulfur (S) are in the 3rd period. The actual electronegativity values show the trend \( O > N > S > P \). Therefore, the provided order \( S < P < N < O \) is incorrect as \( P < S \).
Step 2: Evaluating Option (2) for Atomic Radius.
For the 4th-period elements, atomic radius decreases from left to right. The trend is \( Ca > Ga > Ge > Br \), making the given order \( Br < Ge < Ga < Ca \) correct.
Step 3: Evaluating Option (3) for First Ionization Enthalpy.
Due to stable electronic configurations (\( 3s^2 \) for Mg and \( 3p^3 \) for P), the order \( Al < Mg < S < P \) is correct.
Step 4: Evaluating Option (4) for Metallic Nature.
Metallic character increases down a group. Group 1 elements are more metallic than Group 2, so the order \( Mg < Ca < K < Cs \) is correct.
• Electronegativity: Increases across a period (left to right) and decreases down a group.
• Atomic Radius: Decreases across a period and increases down a group.
• First Ionization Enthalpy: Generally increases across a period and decreases down a group.
• Metallic Nature: Decreases across a period and increases down a group.
Step 1: Evaluating Option (1) for Electronegativity.
Nitrogen (N) and Oxygen (O) are in the 2nd period, while Phosphorus (P) and Sulfur (S) are in the 3rd period. The actual electronegativity values show the trend \( O > N > S > P \). Therefore, the provided order \( S < P < N < O \) is incorrect as \( P < S \).
Step 2: Evaluating Option (2) for Atomic Radius.
For the 4th-period elements, atomic radius decreases from left to right. The trend is \( Ca > Ga > Ge > Br \), making the given order \( Br < Ge < Ga < Ca \) correct.
Step 3: Evaluating Option (3) for First Ionization Enthalpy.
Due to stable electronic configurations (\( 3s^2 \) for Mg and \( 3p^3 \) for P), the order \( Al < Mg < S < P \) is correct.
Step 4: Evaluating Option (4) for Metallic Nature.
Metallic character increases down a group. Group 1 elements are more metallic than Group 2, so the order \( Mg < Ca < K < Cs \) is correct.
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