Although B (Boron) is smaller in size as compared to Be (Berellium) but the first ionisation enthalpy of Be (Berellium) is higher than B (Boron).
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Since Be has fully filled 2s^2 orbital & B has 2p^1.It is easy to remove 1 electron from 2p subshell.
Due to this the first ionisation enthalpy of Be (Berellium) is higher than B (Boron).
Due to this the first ionisation enthalpy of Be (Berellium) is higher than B (Boron).
vijay2019:
good answer
thanks to my chemistry teacher
self study
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