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Chapter 3: Problem 51

Which of the following ions have noble gas electron configurations? a. \(\mathrm{Fe}^{2+}, \mathrm{Fe}^{3+}, \mathrm{Sc}^{3+}, \mathrm{Co}^{3+}\) b. \(\mathrm{Tl}^{+}, \mathrm{Te}^{2-}, \mathrm{Cr}^{3+}\) c. \(\mathrm{Pu}^{4+}, \mathrm{Ce}^{4+}, \mathrm{Ti}^{4+}\) d. \(\mathrm{Ba}^{2+}, \mathrm{Pt}^{2+}, \mathrm{Mn}^{2+}\)

Short Answer

Expert verified
The ions with noble gas electron configurations are \(\mathrm{Sc}^{3+}\), \(\mathrm{Tl}^{+}\), \(\mathrm{Te}^{2-}\), and \(\mathrm{Ba}^{2+}\).

Step by step solution

01

Determine the electron configuration of each ion#a.

To find the electron configuration, subtract the charge of the ion from the atomic number to determine the number of electrons. Then, fill the atomic orbitals according to the Aufbau principle (1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, etc.): 1. \(\mathrm{Fe}^{2+}\): 26 - 2 = 24 electrons, configuration: [Ar] 3d^6 4s^0 2. \(\mathrm{Fe}^{3+}\): 26 - 3 = 23 electrons, configuration: [Ar] 3d^5 4s^0 3. \(\mathrm{Sc}^{3+}\): 21 - 3 = 18 electrons, configuration: [Ar] 3d^0 4s^0 4. \(\mathrm{Co}^{3+}\): 27 - 3 = 24 electrons, configuration: [Ar] 3d^6 4s^0
02

Compare ion electron configurations to noble gases#a.

Among these ions, only \(\mathrm{Sc}^{3+}\) has the electron configuration of a noble gas, Argon: [Ar]. b. \(\mathrm{Tl}^{+}, \mathrm{Te}^{2-}, \mathrm{Cr}^{3+}\)
03

Determine the electron configuration of each ion#b.

Same process as before: 1. \(\mathrm{Tl}^{+}\): 81 - 1 = 80 electrons, configuration: [Xe] 4f^14 5d^10 6s^2 6p^0 2. \(\mathrm{Te}^{2-}\): 52 + 2 = 54 electrons, configuration: [Kr] 4d^10 5s^2 5p^6 3. \(\mathrm{Cr}^{3+}\): 24 - 3 = 21 electrons, configuration: [Ar] 3d^3 4s^0
04

Compare ion electron configurations to noble gases#b.

In this set, both \(\mathrm{Tl}^{+}\) and \(\mathrm{Te}^{2-}\) have electron configurations that match noble gases: Xenon and Krypton, respectively. c. \(\mathrm{Pu}^{4+}, \mathrm{Ce}^{4+}, \mathrm{Ti}^{4+}\) We'll skip these ions, as their electron configurations are more complex and beyond the scope of high school chemistry. d. \(\mathrm{Ba}^{2+}, \mathrm{Pt}^{2+}, \mathrm{Mn}^{2+}\)
05

Determine the electron configuration of each ion#d.

Same process as before: 1. \(\mathrm{Ba}^{2+}\): 56 - 2 = 54 electrons, configuration: [Kr] 4d^10 5s^2 5p^6 2. \(\mathrm{Pt}^{2+}\): 78 - 2 = 76 electrons, configuration: [Xe] 4f^14 5d^8 6s^0 3. \(\mathrm{Mn}^{2+}\): 25 - 2 = 23 electrons, configuration: [Ar] 3d^5 4s^0
06

Compare ion electron configurations to noble gases#d.

In this set, only \(\mathrm{Ba}^{2+}\) has the electron configuration of a noble gas, Krypton: [Kr]. In summary, the ions with noble gas electron configurations are \(\mathrm{Sc}^{3+}\), \(\mathrm{Tl}^{+}\), \(\mathrm{Te}^{2-}\), and \(\mathrm{Ba}^{2+}\).

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Most popular questions from this chapter

Think of forming an ionic compound as three steps (this is a simplification, as with all models): (1) removing an electron from the metal; (2) adding an electron to the nonmetal; and (3) allowing the metal cation and nonmetal anion to come together. a. What is the sign of the energy change for each of these three processes? b. In general, what is the sign of the sum of the first two processes? Use examples to support your answer. c. What must be the sign of the sum of the three processes? d. Given your answer to part \(c,\) why do ionic bonds occur? e. Given your above explanations, why is NaCl stable but not \(\mathrm{Na}_{2} \mathrm{Cl}\) ? \(\mathrm{NaCl}_{2}\) ? What about \(\mathrm{MgO}\) compared to \(\mathrm{MgO}_{2} ?\) \(\mathrm{Mg}_{2} \mathrm{O} ?\)

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