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Chapter 8: Problem 46

Write electron configurations for the most stable ion formed by each of the elements Te, Cl, Sr, and Li (when in stable ionic compounds).

Short Answer

Expert verified
The electron configurations for the most stable ions of the given elements when in stable ionic compounds are: - Te²⁻ (Tellurium): \(\mathrm{[Kr] \: 4d^{10} \: 5s^2 \: 5p^6}\) - Cl⁻ (Chlorine): \(\mathrm{[Ne] \: 3s^2 \: 3p^6}\) - Sr²⁺ (Strontium): \(\mathrm{[Kr]}\) - Li⁺ (Lithium): \(\mathrm{1s^2}\)

Step by step solution

01

Te (Tellurium)

The atomic number of Te is 52. Its electron configuration for the neutral atom is: \[\mathrm{[Kr] \: 4d^{10} \: 5s^2 \: 5p^4}\]
02

Cl (Chlorine)

The atomic number of Cl is 17. Its electron configuration for the neutral atom is: \[\mathrm{[Ne] \: 3s^2 \: 3p^5}\]
03

Sr (Strontium)

The atomic number of Sr is 38. Its electron configuration for the neutral atom is: \[\mathrm{[Kr] \: 5s^2}\]
04

Li (Lithium)

The atomic number of Li is 3. Its electron configuration for the neutral atom is: \[\mathrm{1s^2 \: 2s^1}\] Step 2: Determine the charges of the most stable ions
05

Te (Tellurium)

To achieve a stable electron configuration, Te needs to gain 2 electrons to fill its 5p subshell. Therefore, the charge of the most stable Te ion is -2.
06

Cl (Chlorine)

To achieve a stable electron configuration, Cl needs to gain 1 electron to fill its 3p subshell. Therefore, the charge of the most stable Cl ion is -1.
07

Sr (Strontium)

To achieve a stable electron configuration, Sr needs to lose its 2 electrons in the 5s subshell to expose the filled 4d subshell. Therefore, the charge of the most stable Sr ion is +2.
08

Li (Lithium)

To achieve a stable electron configuration, Li needs to lose its 1 electron in the 2s subshell to expose the filled 1s subshell. Therefore, the charge of the most stable Li ion is +1. Step 3: Write the electron configurations for the stable ions
09

Te²⁻ (Tellurium)

The electron configuration for the Te²⁻ ion is: \[\mathrm{[Kr] \: 4d^{10} \: 5s^2 \: 5p^6}\]
10

Cl⁻ (Chlorine)

The electron configuration for the Cl⁻ ion is: \[\mathrm{[Ne] \: 3s^2 \: 3p^6}\]
11

Sr²⁺ (Strontium)

The electron configuration for the Sr²⁺ ion is: \[\mathrm{[Kr]}\]
12

Li⁺ (Lithium)

The electron configuration for the Li⁺ ion is: \[\mathrm{1s^2}\]

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Most popular questions from this chapter

Which member of the following pairs would you expect to be more energetically stable? Justify each choice. a. \(\mathrm{NaBr}\) or \(\mathrm{NaBr}_{2}\) b. \(\mathrm{ClO}_{4}\) or \(\mathrm{ClO}_{4}^{-}\) c. \(\mathrm{SO}_{4}\) or \(\mathrm{XeO}_{4}\) d. \(\mathrm{OF}_{4}\) or \(\mathrm{SeF}_{4}\)

Arrange the atoms and/or ions in the following groups in order of decreasing size. a. \(\mathrm{O}, \mathrm{O}^{-}, \mathrm{O}^{2-}\) b. \(\mathrm{Fe}^{2+}, \mathrm{Ni}^{2+}, \mathrm{Zn}^{2+}\) c. \(\mathrm{Ca}^{2+}, \mathrm{K}^{+}, \mathrm{Cl}^{-}\)

Although both \(\mathrm{Br}_{3}^{-}\) and \(\mathrm{I}_{3}^{-}\) ions are known, the \(\mathrm{F}_{3}-\) ion has not been observed. Explain.

Write electron configurations for a. the cations \(\mathrm{Mg}^{2+}, \mathrm{K}^{+},\) and \(\mathrm{Al}^{3+}\) . b. the anions \(\mathrm{N}^{3-}, \mathrm{O}^{2-}, \mathrm{F}^{-},\) and \(\mathrm{Te}^{2-}\)

The lattice energies of \(\mathrm{FeCl}_{3}, \mathrm{FeCl}_{2},\) and \(\mathrm{Fe}_{2} \mathrm{O}_{3}\) are (in no particular order) \(-2631,-5359,\) and \(-14,774 \mathrm{kJ} / \mathrm{mol}\) . Match the appropriate formula to each lattice energy. Explain.
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