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Chapter 7: Problem 45

Write the electron configurations for the following ions, and determine which have noble-gas configurations: \((\mathbf{a})\mathrm{Co}^{2+}\) \((\mathbf{b})\mathrm{Sn}^{2+},(\mathbf{c}) \mathrm{Zr}^{4+},(\mathbf{d}) \mathrm{Ag}^{+},(\mathbf{e}) \mathrm{S}^{2-}.\)

Short Answer

Expert verified
The electron configurations for the given ions are: a) \(Co^{2+}\): [\(\text{Ar}\)] 3d^7 b) \(Sn^{2+}\): [\(\text{Kr}\)] 4d^10 5s^2 c) \(Zr^{4+}\): [\(\text{Kr}\)] d) \(Ag^{+}\): [\(\text{Kr}\)] 4d^10 e) \(S^{2-}\): [\(\text{Ne}\)] 3s^2 3p^6 The ions with noble-gas configurations are \(Sn^{2+}\), \(Zr^{4+}\), and \(S^{2-}\).

Step by step solution

01

a) Electron Configuration of Co2+ (Cobalt)

Cobalt (Co) has an atomic number of 27. Its electron configuration is [\(\text{Ar}\)] 3d^7 4s^2. To turn Co into Co2+ ion, we need to remove 2 electrons. We will remove the 2 electrons from the higher energy level first, which is the 4s orbital. So, the electron configuration for Co2+ is [\(\text{Ar}\)] 3d^7.
02

b) Electron Configuration of Sn2+ (Tin)

Tin (Sn) has an atomic number of 50. Its electron configuration is [\(\text{Kr}\)] 4d^10 5s^2 5p^2. To turn Sn into Sn2+ ion, we need to remove 2 electrons. We will remove the 2 electrons from the higher energy level first, which is the 5p orbital. So, the electron configuration for Sn2+ is [\(\text{Kr}\)] 4d^10 5s^2.
03

c) Electron Configuration of Zr4+ (Zirconium)

Zirconium (Zr) has an atomic number of 40. Its electron configuration is [\(\text{Kr}\)] 4d^2 5s^2. To turn Zr into Zr4+ ion, we need to remove 4 electrons. We will remove the 2 electrons from the higher energy level first, which are in the 5s orbital. Next, remove 2 electrons from the 4d orbital. So, the electron configuration for Zr4+ is [\(\text{Kr}\)].
04

d) Electron Configuration of Ag+ (Silver)

Silver (Ag) has an atomic number of 47. Its electron configuration is [\(\text{Kr}\)] 4d^10 5s^1. To turn Ag into an Ag+ ion, we need to remove one electron. We will remove the electron from the higher energy level first, which is the 5s orbital. So, the electron configuration for Ag+ is [\(\text{Kr}\)] 4d^10.
05

e) Electron Configuration of S2- (Sulfide)

Sulfur (S) has an atomic number of 16. Its electron configuration is [\(\text{Ne}\)] 3s^2 3p^4. To turn S into an S2- ion, we need to add 2 electrons. We will add the 2 electrons to the 3p orbital. So, the electron configuration for S2- is [\(\text{Ne}\)] 3s^2 3p^6.
06

Noble-Gas Configurations

The ions with noble-gas configurations are: - Sn2+ with an electron configuration of [\(\text{Kr}\)] 4d^10 5s^2, which resembles the noble gas Kr. - Zr4+ with an electron configuration of [\(\text{Kr}\)], which matches the noble gas Kr. - S2- with an electron configuration of [\(\text{Ne}\)] 3s^2 3p^6, which resembles the noble gas Ar.

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Most popular questions from this chapter

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

Give three examples of ions that have an electron configuration of \(n d^{8}(n=3,4,5, \ldots).\)

Chlorine reacts with oxygen to form \(\mathrm{Cl}_{2} \mathrm{O}_{7}\) . (a) What is the name of this product (see Table 2.6) ? (b) Write a balanced equation for the formation of \(\mathrm{Cl}_{2} \mathrm{O}_{7}(l)\) from the elements. (c) Would you expect \(\mathrm{Cl}_{2} \mathrm{O}_{7}\) to be more reactive toward \(\mathrm{H}^{+}(a q)\) or \(\mathrm{OH}^{-}(a q) ?(\mathbf{d})\) If the oxygen in \(\mathrm{Cl}_{2} \mathrm{O}_{7}\) is considered to have the \(-2\) oxidation state, what is the oxidation state of the Cl? What is the electron configuration of Cl in this oxidation state?

Write an equation for the second electron affinity of chlorine. Would you predict a positive or a negative energy value for this process? Is it possible to directly measure the second electron affinity of chlorine?

Provide a brief explanation for each of the following: \((\mathbf{c}) \mathrm{O}^{2-}\) is larger than O.\((\mathbf{b}) S^{2-}\) is larger than \(\mathrm{O}^{2-} .(\mathbf{c}) \mathrm{S}^{2-}\) is larger than \(\mathrm{K}^{+} .(\mathbf{d}) \mathrm{K}^{+}\) is larger than \(\mathrm{Ca}^{2+}.\)
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