Single Choice

Beryllium has higher ionization enthalpy than boron. This can be explained as :

Aberyllium has higher size than boron hence its ionisation enthalpy is higher
Bpenetration of $$2p- $$electrons to the nucleus is more than the $$2s-$$electrons
Cit is easier to remove an electron from $$2p-$$orbital as compared to $$2s-$$orbital due to more penetration of $$s-$$electrons
Correct Answer
Dionisation energy increases in a period

Solution

Beryllium has higher ionization enthalpy than boron. This can be explained by the electronic configuration of the two:
Be:1s22s2
B:1s22s22p1
In Be, the completely filled 2s orbital has high penetration and provides extra stability whereas in B, the lower penetration of 2p makes it is easier to remove the electron and thus have lower ionization enthalpy.

SIMILAR QUESTIONS

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