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Chapter 15: Problem 26

Give the electronic configuration for (a) \(\mathrm{Fe}^{3+}\) (b) \(\mathrm{V}^{2+}\) (c) \(\mathrm{Zn}^{2+}\) (d) \(\mathrm{Cu}^{+}\) (e) \(\mathrm{Mn}^{4+}\)

Short Answer

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Question: Determine the electronic configuration for the following ions: Fe\(^{3+}\), V\(^{2+}\), Zn\(^{2+}\), Cu\(^{+}\), and Mn\(^{4+}\). Answer: The electronic configurations are as follows: 1. Fe\(^{3+}\): 1s\(^2\) 2s\(^2\) 2p\(^6\) 3s\(^2\) 3p\(^6\) 3d\(^5\) 2. V\(^{2+}\): 1s\(^2\) 2s\(^2\) 2p\(^6\) 3s\(^2\) 3p\(^6\) 3d\(^3\) 3. Zn\(^{2+}\): 1s\(^2\) 2s\(^2\) 2p\(^6\) 3s\(^2\) 3p\(^6\) 3d\(^{10}\) 4. Cu\(^{+}\): 1s\(^2\) 2s\(^2\) 2p\(^6\) 3s\(^2\) 3p\(^6\) 3d\(^{10}\) 5. Mn\(^{4+}\): 1s\(^2\) 2s\(^2\) 2p\(^6\) 3s\(^2\) 3p\(^6\) 3d\(^3\)

Step by step solution

01

1. Fe\(^{3+}\) Electronic Configuration

The atomic number of iron (Fe) is 26. Thus, its electronic configuration is 1s\(^2\) 2s\(^2\) 2p\(^6\) 3s\(^2\) 3p\(^6\) 4s\(^2\) 3d\(^6\). Since Fe\(^{3+}\) lost 3 electrons, we need to remove 3 electrons from its configuration. We'll take 2 electrons from the 4s orbital and 1 from the 3d orbital, leaving us with the electronic configuration 1s\(^2\) 2s\(^2\) 2p\(^6\) 3s\(^2\) 3p\(^6\) 3d\(^5\).
02

2. V\(^{2+}\) Electronic Configuration

The atomic number of vanadium (V) is 23. Thus, its electronic configuration is 1s\(^2\) 2s\(^2\) 2p\(^6\) 3s\(^2\) 3p\(^6\) 4s\(^2\) 3d\(^3\). Since V\(^{2+}\) lost 2 electrons, we need to remove 2 electrons from its configuration. We'll take 2 electrons from the 4s orbital, leaving us with the electronic configuration 1s\(^2\) 2s\(^2\) 2p\(^6\) 3s\(^2\) 3p\(^6\) 3d\(^3\).
03

3. Zn\(^{2+}\) Electronic Configuration

The atomic number of zinc (Zn) is 30. Thus, its electronic configuration is 1s\(^2\) 2s\(^2\) 2p\(^6\) 3s\(^2\) 3p\(^6\) 4s\(^2\) 3d\(^{10}\). Since Zn\(^{2+}\) lost 2 electrons, we need to remove 2 electrons from its configuration. We'll take 2 electrons from the 4s orbital, leaving us with the electronic configuration 1s\(^2\) 2s\(^2\) 2p\(^6\) 3s\(^2\) 3p\(^6\) 3d\(^{10}\).
04

4. Cu\(^{+}\) Electronic Configuration

The atomic number of copper (Cu) is 29. Thus, its electronic configuration is 1s\(^2\) 2s\(^2\) 2p\(^6\) 3s\(^2\) 3p\(^6\) 4s\(^1\) 3d\(^{10}\). Since Cu\(^{+}\) lost 1 electron, we need to remove 1 electron from its configuration. We'll take 1 electron from the 4s orbital, leaving us with the electronic configuration 1s\(^2\) 2s\(^2\) 2p\(^6\) 3s\(^2\) 3p\(^6\) 3d\(^{10}\).
05

5. Mn\(^{4+}\) Electronic Configuration

The atomic number of manganese (Mn) is 25. Thus, its electronic configuration is 1s\(^2\) 2s\(^2\) 2p\(^6\) 3s\(^2\) 3p\(^6\) 4s\(^2\) 3d\(^5\). Since Mn\(^{4+}\) lost 4 electrons, we need to remove 4 electrons from its configuration. We'll take 2 electrons from the 4s orbital and 2 from the 3d orbital, leaving us with the electronic configuration 1s\(^2\) 2s\(^2\) 2p\(^6\) 3s\(^2\) 3p\(^6\) 3d\(^3\).

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Most popular questions from this chapter

A child eats \(10.0 \mathrm{~g}\) of paint containing \(5.0 \% \mathrm{~Pb}\). How many grams of the sodium salt of EDTA, \(\mathrm{Na}_{4}(\mathrm{EDTA})\), should he receive to bring the lead into solution as \(\mathrm{Pb}\). EDTA?

Analysis of a coordination compound gives the following results: \(22.0 \% \mathrm{Co}, 31.4 \% \mathrm{~N}, 6.78 \% \mathrm{H}\), and \(39.8 \% \mathrm{Cl} .\) One mole of the compound dissociates in water to form four moles of ions. (a) What is the simplest formula of the compound? (b) Write an equation for its dissociation in water.

WEB Indicate whether each of the following is true or false. If the statement is false, correct it. (a) The coordination number of iron(III) in \(\mathrm{Fe}\left(\mathrm{NH}_{3}\right)_{4}(\mathrm{en})^{3+}\) is 5 . (b) \(\mathrm{Ni}(\mathrm{CN})_{6}^{4-}\) is expected to absorb at a longer wavelength than \(\mathrm{Ni}\left(\mathrm{NH}_{3}\right)_{6}{ }^{2+}\)

There are four iron atoms in each hemoglobin molecule. The mass percent of iron in a hemoglobin molecule is \(0.35 \%\). Estimate the molar mass of hemoglobin.

Consider the complex ion \(\left[\mathrm{Co}(\mathrm{en})_{2}(\mathrm{SCN}) \mathrm{Cl}\right]^{+} .\) (a) Identify the ligands and their charges. (b) What is the oxidation number of cobalt? (c) What is the formula for the sulfide salt of this ion?
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