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Ch.7 - Periodic Properties of the Elements
Brown - Chemistry: The Central Science 14th Edition
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoBrown 14th EditionCh.7 - Periodic Properties of the ElementsProblema 29a
Capitolo 7, Problema 29a

Which neutral atom is isoelectronic with each of the following ions? Ga3+, Zr4+, Mn7+, I−, Pb2+.

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Identify the atomic number of each element in the ions: Gallium (Ga), Zirconium (Zr), Manganese (Mn), Iodine (I), and Lead (Pb).
Determine the number of electrons in each ion by considering the charge. For cations (positive charge), subtract the charge from the atomic number; for anions (negative charge), add the charge to the atomic number.
Find the neutral atom that has the same number of electrons as each ion. This can be done by matching the electron count obtained in the previous step to the atomic number of a neutral atom.
Verify that the neutral atom and the ion have the same electron configuration by writing out the electron configuration for both and comparing them.
Confirm that each match is correct by ensuring that the total number of electrons in the neutral atom equals the total number of electrons in the ion, accounting for the ion's charge.

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Isoelectronic Species

Isoelectronic species are atoms, ions, or molecules that have the same number of electrons, resulting in identical electron configurations. This concept is crucial for determining which neutral atom corresponds to a given ion, as it allows for the comparison of electron counts despite differences in charge.
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Amphoteric Species

Electron Configuration

Electron configuration describes the distribution of electrons among the various orbitals of an atom. Understanding how to write and interpret electron configurations is essential for identifying isoelectronic species, as it reveals how many electrons a neutral atom or ion possesses and how they are arranged.
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Electron Configuration Example

Charge and Electron Count

The charge of an ion indicates the number of electrons lost or gained compared to its neutral atom. For example, a +3 charge means the ion has three fewer electrons than its neutral counterpart. This relationship is fundamental when determining which neutral atom is isoelectronic with a given ion, as it directly affects the total electron count.
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Formal Charge
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Use data from Appendix C, Figure 7.10, and Figure 7.12 to calculate the lattice energy of RbCl.

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Some ions do not have a corresponding neutral atom that has the same electron configuration. For each of the following ions, identify the neutral atom that has the same number of electrons and determine if this atom has the same electron configuration. (a) CI−, (b) Sc3+, (c) Fe2+, (d) Zn2+, (e) Sn4+.

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Consider the isoelectronic ions F- and Na+. (b) Using Equation 7.1 and assuming that core electrons contribute 1.00 and valence electrons contribute 0.00 to the screening constant, S, calculate Zeff for the 2p electrons in both ions.

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Consider the isoelectronic ions F- and Na+. (c) Repeat this calculation using Slater’s rules to estimate the screening constant, S.