Question:
B has a smaller first ionization enthalpy than Be. Consider the following statements :
(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 $\mathrm{Be}$.
(III) 2 s electron has more penetration power than 2 p electron.
(IV) atomic radius of $\mathrm{B}$ is more than $\mathrm{Be}$
(Atomic number $\mathrm{B}=5, \mathrm{Be}=4$ )
The correct statements are :
Correct Option: 1
Solution:
