Read the following statements regarding the ionization enthalpies of second period elements: Statement I: The first ionization enthalpy of boron is slightly less than that of beryllium because a 2p electron of boron is more shielded from the nucleus by the inner core of electrons than the 2s electron of beryllium. Statement II: The first ionization enthalpy of oxygen is less than that of nitrogen because the two elec

Step-by-step solution

Let us evaluate each statement: Statement I is correct. The 2s electron in Be is more penetrating towards the nucleus than the 2p electron in B. Consequently, the 2p electron of B is more shielded by the inner core, making it easier to remove than the 2s electron of Be. Statement II is correct. Nitrogen has a stable half-filled configuration ( 2p³ ), whereas oxygen ( 2p⁴ ) has two electrons paired in one 2p orbital, leading to increased electron-electron repulsion. This makes it easier to remove the fourth 2p elect