A) \[A{{l}^{3+}}<M{{g}^{2+}}\,N{{a}^{+}}<{{F}^{-}}\]: Increasing ionic size
B) \[\operatorname{B} < C < N < O\]: Increasing first ionization enthalpy
C) \[\operatorname{I}< Br < F < Cl\]: Increasing electron gain enthalpy (with negative sign)
D) \[\operatorname{Li} < Na < K < Rb\]: Increasing metallic radius
Correct Answer: B
Solution :
\[\operatorname{B} < C < N <O\]. When we move from B to O in a periodic table the first ionisation enthalpy increases due to the attraction of nucleus towards the outermost of electron.
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