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Chapter 7: Problem 29

Which neutral atom is isoelectronic with each of the following ions? \(\mathrm{H}^{-}, \mathrm{Ca}^{2+}, \mathrm{In}^{3+}, \mathrm{Ge}^{2+}\)

Short Answer

Expert verified
The neutral atoms isoelectronic with the given ions are: \(\mathrm{He}\) for \(\mathrm{H}^{-}\), \(\mathrm{Ar}\) for \(\mathrm{Ca}^{2+}\), \(\mathrm{Pd}\) for \(\mathrm{In}^{3+}\), and \(\mathrm{Zn}\) for \(\mathrm{Ge}^{2+}\).

Step by step solution

01

Find the number of electrons for each ion

To determine which neutral atom is isoelectronic with each ion, we must first find the number of electrons for the given ions. To do this, we need the atomic number (number of protons) of each element and the ion's charge. An ion's atomic number minus its charge gives the number of electrons. From the periodic table, we have the atomic numbers for H (Hydrogen)=1, Ca (Calcium)=20, In (Indium)=49, and Ge (Germanium)=32.
02

Determine the neutral atom isoelectronic to \(\mathrm{H}^{-}\)

For \(\mathrm{H}^{-}\), the charge is -1. Therefore, the number of electrons is 1 (atomic number) - (-1) = 2. A neutral atom with 2 electrons is Helium (He). Therefore, \(\mathrm{He}\) is isoelectronic with \(\mathrm{H}^{-}\).
03

Determine the neutral atom isoelectronic to \(\mathrm{Ca}^{2+}\)

For \(\mathrm{Ca}^{2+}\), the charge is +2. Therefore, the number of electrons is 20 (atomic number) - 2 = 18. A neutral atom with 18 electrons is Argon (Ar). Therefore, \(\mathrm{Ar}\) is isoelectronic with \(\mathrm{Ca}^{2+}\).
04

Determine the neutral atom isoelectronic to \(\mathrm{In}^{3+}\)

For \(\mathrm{In}^{3+}\), the charge is +3. Therefore, the number of electrons is 49 (atomic number) - 3 = 46. A neutral atom with 46 electrons is Palladium (Pd). Therefore, \(\mathrm{Pd}\) is isoelectronic with \(\mathrm{In}^{3+}\).
05

Determine the neutral atom isoelectronic to \(\mathrm{Ge}^{2+}\)

For \(\mathrm{Ge}^{2+}\), the charge is +2. Therefore, the number of electrons is 32 (atomic number) - 2 = 30. A neutral atom with 30 electrons is Zinc (Zn). Therefore, \(\mathrm{Zn}\) is isoelectronic with \(\mathrm{Ge}^{2+}\). From this analysis, we found that: 1. \(\mathrm{He}\) is isoelectronic with \(\mathrm{H}^{-}\) 2. \(\mathrm{Ar}\) is isoelectronic with \(\mathrm{Ca}^{2+}\) 3. \(\mathrm{Pd}\) is isoelectronic with \(\mathrm{In}^{3+}\) 4. \(\mathrm{Zn}\) is isoelectronic with \(\mathrm{Ge}^{2+}\)

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Most popular questions from this chapter

(a) Which ion is smaller, \(\mathrm{Co}^{3+}\) or \(\mathrm{Co}^{4+} ?\) (b) In a lithium-ion battery that is discharging to power a device, for every \(\mathrm{Li}^{+}\) that inserts into the lithium cobalt oxide electrode, a \(\mathrm{Co}^{4+}\) ion must be reduced to a \(\mathrm{Co}^{3+}\) ion to balance charge. Using the CRC Handbook of Chemistry and Physics or other standard reference, find the ionic radii of \(\mathrm{Li}^{+}, \mathrm{Co}^{3+},\) and \(\mathrm{Co}^{4+}\). Order these ions from smallest to largest. (c) Will the lithium cobalt oxide cathode expand or contract as lithium ions are inserted? (d) Lithium is not nearly as abundant as sodium. If sodium ion batteries were developed that function in the same manner as lithium ion batteries, do you think "sodium cobalt oxide" would still work as the electrode material? Explain. (e) If you don't think cobalt would work as the redox-active partner ion in the sodium version of the electrode, suggest an alternative metal ion and explain your reasoning.

(a) Why is calcium generally more reactive than beryllium? (b) Why is calcium generally less reactive than rubidium?

(a) If the core electrons were totally effective at screening the valence electrons and the valence electrons provided no screening for each other, what would be the effective nuclear charge acting on the \(3 s\) and \(3 p\) valence electrons in P? (b) Repeat these calculations using Slater's rules. (c) Detailed calculations indicate that the effective nuclear charge is \(5.6+\) for the \(3 s\) electrons and \(4.9+\) for the \(3 p\) electrons. Why are the values for the \(3 s\) and \(3 p\) electrons different? (d) If you remove a single electron from a Patom, which orbital will it come from?

Identify each statement as true or false: (a) Cations are larger than their corresponding neutral atoms. (b) \(\mathrm{Li}^{+}\) is smaller than Li. (c) \(\mathrm{Cl}^{-}\) is bigger than I .

The following observations are made about two hypothetical elements \(\mathrm{A}\) and \(\mathrm{B}:\) The \(\mathrm{A}-\mathrm{A}\) and \(\mathrm{B}-\mathrm{B}\) bond lengths in the elemental forms of \(\mathrm{A}\) and \(\mathrm{B}\) are 236 and \(194 \mathrm{pm}\), respectively. A and \(B\) react to form the binary compound \(A B_{2}\), which has a linear structure (that is \(\left.\angle \mathrm{B}-\mathrm{A}-\mathrm{B}=180^{\circ}\right) .\) Based on these statements, predict the separation between the two B nuclei in a molecule of \(\mathrm{AB}_{2}\).
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