Three atoms have the following electron configurations: (a)...

Three atoms have the following electron configurations: (a) $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{1}$ (b) $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{5}$ (c) $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{1}$ Which of the three has the largest $E_{\mathrm{il}}$ ? Which has the smallest $E_{\mathrm{i} 4} ?$

Three atoms have the following electron configurations:
(a) $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{1}$
(b) $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{5}$
(c) $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{1}$
Which of the three has the largest $E_{\mathrm{il}}$ ? Which has the smallest $E_{\mathrm{i} 4} ?$

Key Concepts

Electron Configuration

Electron configuration describes the arrangement of electrons in an atom's orbitals, following the principles of quantum mechanics, such as the Aufbau principle, the Pauli exclusion principle, and Hund's rule. It provides a basis for understanding an element’s chemical properties and how electrons are distributed among different energy levels and subshells.

Ionization Energy

Ionization energy is the energy required to remove an electron from a gaseous atom or ion. It is a fundamental property that reflects how strongly an electron is held by the nucleus. The concept is crucial for understanding chemical reactivity and periodic trends, as variations in ionization energy can indicate differences in atomic structure and electron–nucleus interactions.

Successive Ionization Energies

Successive ionization energies refer to the energies required to remove electrons one after another from an atom. Typically, each successive removal requires significantly more energy, especially when an electron begins to be removed from a newly formed cation with a stable electron configuration or from a lower energy level, due to increased effective nuclear charge on the remaining electrons.

Effective Nuclear Charge

Effective nuclear charge is the net positive charge experienced by an electron in an atom after accounting for the shielding or screening effect of inner electrons. It plays a critical role in determining the strength of the attraction between the nucleus and electrons, which in turn influences ionization energies and other properties related to electron removal.

Shielding Effect

The shielding effect is a phenomenon where inner electrons partially block the nuclear charge from being felt by outer electrons. This reduction in the effective nuclear charge on valence electrons influences ionization energies, as electrons that are more effectively shielded are generally easier to remove than those experiencing a stronger net pull from the nucleus.

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