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Ch.6 - Ionic Compounds: Periodic Trends and Bonding Theory
McMurry - Chemistry 8th Edition
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Tutti i libri di testoMcMurry 8th EditionCh.6 - Ionic Compounds: Periodic Trends and Bonding TheoryProblema 104b
Capitolo 6, Problema 104b

Iron is commonly found as Fe, Fe2+, and Fe3+. (b) What are the n and l quantum numbers of the electron removed on going from Fe2+ to Fe3+?

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Determine the electron configuration of Fe^{2+}.
Identify the electron configuration of Fe^{3+}.
Compare the electron configurations of Fe^{2+} and Fe^{3+} to find the electron that is removed.
Identify the quantum numbers n and l for the removed electron.
Conclude with the n and l values for the electron removed from Fe^{2+} to form Fe^{3+}.

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Quantum Numbers

Quantum numbers are numerical values that describe the unique quantum state of an electron in an atom. The four quantum numbers include the principal quantum number (n), which indicates the energy level, and the azimuthal quantum number (l), which describes the shape of the orbital. Understanding these numbers is essential for determining the electron configuration and the specific electron being removed during ionization.
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Principal Quantum Number

Electron Configuration

Electron configuration refers to the distribution of electrons in an atom's orbitals. For iron (Fe), the electron configuration is [Ar] 4s² 3d⁶. When iron loses electrons to form ions, the electrons are removed from the outermost energy levels first, which is crucial for identifying which electron is lost when transitioning from Fe²⁺ to Fe³⁺.
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Electron Configuration Example

Ionization

Ionization is the process of removing one or more electrons from an atom or ion, resulting in a positively charged ion. In the case of Fe²⁺ to Fe³⁺, one electron is removed from the 3d subshell. Understanding the ionization process helps in determining the specific quantum numbers of the electron that is lost during the transition between these two oxidation states.
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Auto-Ionization and Kw
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Iron is commonly found as Fe, Fe2++, and Fe3+. (c) The third ionization energy of Fe is Ei3 = +2952 kJ/mol. What is the longest wavelength of light that could ionize Fe2+(g) to Fe3+(g)?

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Consider the electronic structure of the element bismuth. (a) The first ionization energy of bismuth is Ei1 = +703 kJ/ mol. What is the longest possible wavelength of light that could ionize an atom of bismuth?

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