\(B\) 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 \(2 s\) electrons of \(Be.\) \((III)\; 2 s\) electron has more penetration power than \(2 \mathrm{p}\) electron. \((IV)\) atomic radius of \(\mathrm{B}\) is more than \(\mathrm{Be}\) (Atomic number \(\mathrm{B}=5, \mathrm{Be}=4\) ) The correct statements are

1. A \((I), (II)\) and \((III)\)
2. B \((II), (III)\) and \((IV)\)
3. C \((I), (III)\) and \((IV)\)
4. D \((I), (II)\) and \((IV)\)