Question

The first ionisation energy of Be is smaller than that of B while the second ionisation energy of Be is higher than that of B.
Answer whether the above statement is true or false.
If true enter 1, else enter 0.

Answer 1

The first ionisation energy of $Be$ is higher than that of $B$ while the second ionisation energy of $Be$ is smaller than that of $B$.

The ionization of Be requires removal of an electron from the 2s subshell. Ionization of B, however, requires removal of an electron from a 2p subshell. The 2p subshell is higher in energy than the 2s subshell (this why we fill the 2s subshell first when constructing an electron configuration) resulting in a lower than expected first ionization energy for boron.

While the removal of second electron from B is difficult as it is to be removed from a completely filled 2s orbital while the removal of second electron from Be is comparatively easier as it is to be removed from a half filled 1s orbital.