Question

The nuclear charge actually experienced by an electron is termed as the effective nuclear charge. The effective nuclear charge Z* actually depends on the type of shell and orbital in which electron is actually present. The relative extent to which the various orbitals penetrate the electron clouds of other orbitals is $s>p>d>f$ (for the same value of $n$)

The phenomenon in which penultimate shell electrons act as screen or shield in between nucleus and valence shell electrons and thereby reducing nuclear charge is known as shielding effect. The penultimate shell electrons repel the valence shell electron to keep them loosely held with the nucleus. It is thus evident that more is the shielding effect, lesser is the effective nuclear charge and lesser is the ionization energy.

Which of the following is not concerned with effective nuclear charge?

• A. Higher ionization potential of carbon than boron
• B. Higher ionization potential of magnesium than aluminium
• C. Higher values of successive ionization energy
• D. Higher electronegativity of higher oxidation state

Answer 1

Answer: (B)

Higher ionization potential of magnesium than aluminium

Mg has high potential energy than Al, due to stable full filled s-orbital configuration.