Question

Explain why beryllium has higher ionization enthalpy than boron

Answer 1

electronic configuration of both elements are-
Be=1S2,2S2
B=1S2,2S2,2P1

since taking out one electron is easy in p orbital rather than taking one electron from fully filled s orbital .

this is the reason behind more ionization enthalpy in Be than B.

hope this will help you.

Answer 2

Answer:

Ionization energy is defined as the energy required to remove an electron from an isolated gaseous atom. It is represented as $E_i$

This energy will be higher for fully filled and half-filled electronic configuration than partially filled electronic configuration. This is so because half filled and fully filled configurations are stable.

Electronic configuration of beryllium= $1s^22s^2$

This element has completely filled orbital, and thus is stable. Thus,  ionization enthalpy will be higher.

Electronic configuration of boron= $1s^22s^22p^1$

This element has partially filled 'p'-orbital. Thus, first ionization potential will be lower.

Hence, this is so because beryllium has completely filled orbitals , which are stable and hence ionization enthalpy will be higher.