$\mathrm{B}$ has a smaller first ionization enthalpy than $\mathrm{B}\mathrm{e}$. Consider the following statement:
(I) it is easier to remove $2\mathrm{p}$ electron than$2\mathrm{s}$  electron
(II) $2\mathrm{p}$ electron of $\mathrm{B}$ is more shielded from the nucleus by the inner core of electrons than the $2\mathrm{s}$ electrons of $\mathrm{B}\mathrm{e}$
(III) $2\mathrm{s}$ electron has more penetration power than $2\mathrm{p}$ electron
(IV) atomic radius of $\mathrm{B}$ is more than $\mathrm{B}\mathrm{e}$
(atomic number $\mathrm{B}:5, \mathrm{B}\mathrm{e}=4$ )
The correct statements are.