ionization enthalpy of Be is greater than Boron.
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The first ionization of Beryllium is greater than that of Boron because Beryllium has a stable complete electronic configuration (1s22s2) so it, require more energy to remove the first electron from it, where as Boron has electronic configuration (1s22s23s1) which need lesser energy than that of Beryllium.
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Explanation:
The first ionization of Beryllium is greater than that of Boron because Beryllium has a stable complete electronic configuration (1s22s2) so it, require more energy to remove the first electron from it, where as Boron has electronic configuration (1s22s23s1) which need lesser energy than that of Beryllium.
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