Iron is commonly found as Fe, Fe2+, and Fe3+. (a) Write electron configurations for each of the three. (d) The third ionization energy of Ru is less than the third ionization energy of Fe. Explain.

Name: Chemistry
Author: McMurry
ISBN: 9781292336145

검증된 단계별 안내

To write the electron configuration for Fe (neutral iron), first determine the number of electrons. Iron has an atomic number of 26, so it has 26 electrons. The electron configuration is written by filling the orbitals in the order of increasing energy: 1s², 2s², 2p⁶, 3s², 3p⁶, 4s², 3d⁶.

For Fe²⁺, remove two electrons from the neutral Fe configuration. Electrons are removed from the highest energy level first, which is the 4s orbital. Thus, the electron configuration for Fe²⁺ is: 1s², 2s², 2p⁶, 3s², 3p⁶, 3d⁶.

For Fe³⁺, remove one more electron from the Fe²⁺ configuration. The next electron is removed from the 3d orbital, resulting in the configuration: 1s², 2s², 2p⁶, 3s², 3p⁶, 3d⁵.

To explain why the third ionization energy of Ru is less than that of Fe, consider the electron configurations and the stability of half-filled and fully filled subshells. Ru has a more stable electron configuration after losing three electrons compared to Fe, which makes it easier to remove the third electron from Ru.

Additionally, consider the effective nuclear charge and electron shielding. Ru has more protons than Fe, but the additional inner electrons provide more shielding, reducing the effective nuclear charge felt by the outer electrons, making it easier to remove the third electron.

주요 개념

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Electron Configuration

Electron configuration describes the distribution of electrons in an atom's orbitals. For iron (Fe), the electron configuration is 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d⁶. For the ions Fe²⁺ and Fe³⁺, electrons are removed from the outermost orbitals, resulting in configurations of 1s² 2s² 2p⁶ 3s² 3p⁶ 3d⁶ and 1s² 2s² 2p⁶ 3s² 3p⁶ 3d⁵, respectively.

Ionization Energy

Ionization energy is the energy required to remove an electron from an atom or ion in its gaseous state. It generally increases with the atomic number due to increased nuclear charge, but can vary based on electron configuration and stability. The third ionization energy refers to the energy needed to remove the third electron, which can be influenced by the electron's proximity to the nucleus and the overall electron shielding effect.

Comparison of Ionization Energies

When comparing the third ionization energies of different elements, factors such as atomic size, electron configuration, and effective nuclear charge play crucial roles. In the case of Ru and Fe, Ru has a higher atomic number and a more complex electron configuration, which can lead to a lower third ionization energy due to increased electron shielding and repulsion among electrons, making it easier to remove an electron compared to Fe.

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