The incorrect statement among the following is: (a) The...

The incorrect statement among the following is: (a) The first ionisation potential of $\mathrm{Al}$ is less than the first ionisation potential of $\mathrm{Mg}$ $\square$ (b) The second ionisation potential of $\mathrm{Mg}$ is greater than the second ionisation potential of $\mathrm{Na}$ $\square$ (c) The first ionisation potential of $\mathrm{Na}$ is less than the first ionisation potential of $\mathrm{Mg}$ $\square$ (d) The third ionisation potential of $\mathrm{Mg}$ is greater than third ionisation potential of $\mathrm{Al}$ 0

The incorrect statement among the following is:
(a) The first ionisation potential of $\mathrm{Al}$ is less than the first ionisation potential of $\mathrm{Mg}$ $\square$
(b) The second ionisation potential of $\mathrm{Mg}$ is greater than the second ionisation potential of $\mathrm{Na}$ $\square$
(c) The first ionisation potential of $\mathrm{Na}$ is less than the first ionisation potential of $\mathrm{Mg}$ $\square$
(d) The third ionisation potential of $\mathrm{Mg}$ is greater than third ionisation potential of $\mathrm{Al}$ 0

Key Concepts

Ionization Energy

Ionization energy is the energy required to remove an electron from an atom or ion in the gaseous state. It is a fundamental property of atoms that influences their chemical reactivity and bonding behavior. The concept extends to first, second, third ionization energies, etc., with each successive ionization generally requiring more energy due to the increased effective nuclear charge experienced by the remaining electrons.

Periodic Trends

Periodic trends refer to the systematic variations in properties such as ionization energy across periods and down groups in the periodic table. Typically, ionization energy increases across a period due to increasing nuclear charge with little additional shielding, and decreases down a group because of the greater distance of the outer electrons from the nucleus and increased electron shielding.

Successive Ionizations

Successive ionizations involve removing more than one electron from an atom. The energy required for each subsequent ionization typically increases significantly since the removal of an electron results in a higher effective nuclear charge on the remaining electrons, making them more tightly bound to the nucleus.

Electron Configuration

Electron configuration describes the distribution of electrons in an atom's orbitals, which directly affects its ionization energy. The stability associated with certain configurations, such as half-filled or fully filled subshells, can lead to deviations from expected periodic trends and affect the energy required to remove electrons.

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