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Chapter 8: Problem 82

Arrange the following species in isoelectronic pairs: \(\mathrm{O}^{+}, \mathrm{Ar}, \mathrm{S}^{2-}, \mathrm{Ne}, \mathrm{Zn}, \mathrm{Cs}^{+}, \mathrm{N}^{3-}, \mathrm{As}^{3+}, \mathrm{N}, \mathrm{Xe}\)

Short Answer

Expert verified
The isoelectronic pairs are \([\mathrm{O^{+}}, \mathrm{N}]\), \([\mathrm{Ar}, \mathrm{S^{2-}}]\), \([\mathrm{Ne}, \mathrm{N^{3-}}]\), \([\mathrm{Zn}, \mathrm{As^{3+}}]\), \([\mathrm{Cs^{+}}, \mathrm{Xe}]\)

Step by step solution

01

Identify the Number of Electrons

Count the number of electrons for each species. For neutral atoms, it equals to the atomic number. For ions, add or subtract the charge from the atomic number. Here are the results: \(\mathrm{O^{+}}\) has 7 electrons, \(\mathrm{Ar}\) has 18 electrons, \(\mathrm{S^{2-}}\) has 18 electrons, \(\mathrm{Ne}\) has 10 electrons, \(\mathrm{Zn}\) has 30 electrons, \(\mathrm{Cs^{+}}\) has 54 electrons, \(\mathrm{N^{3-}}\) has 10 electrons, \(\mathrm{As^{3+}}\) has 30 electrons, \(\mathrm{N}\) has 7 electrons, \(\mathrm{Xe}\) has 54 electrons.
02

Match Isoelectronic Pairs

Now, find the pairs that have the same electron count. The pairs obtained are: \([\mathrm{O^{+}}, \mathrm{N}]\), \([\mathrm{Ar}, \mathrm{S^{2-}}]\), \([\mathrm{Ne}, \mathrm{N^{3-}}]\), \([\mathrm{Zn}, \mathrm{As^{3+}}]\), \([\mathrm{Cs^{+}}, \mathrm{Xe}]\)

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Most popular questions from this chapter

Predict the atomic number and ground-state electron configuration of the next member of the alkali metals after francium.

Two atoms have the electron configurations \(1 s^{2} 2 s^{2} 2 p^{6}\) and \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{1} .\) The first ionization energy of one is \(2080 \mathrm{~kJ} / \mathrm{mol}\), and that of the other is \(496 \mathrm{~kJ} / \mathrm{mol} .\) Match each ionization energy with one of the given electron configurations. Justify your choice.

State whether each of the following elements is a gas, a liquid, or a solid under atmospheric conditions. Also state whether it exists in the elemental form as atoms, as molecules, or as a three-dimensional network: \(\mathrm{Mg}, \mathrm{Cl}, \mathrm{Si}, \mathrm{Kr}, \mathrm{O}, \mathrm{I}, \mathrm{Hg}, \mathrm{Br}\)

Sketch the outline of the periodic table and show group and period trends in the first ionization energy of the elements. What types of elements have the highest ionization energies and what types the lowest ionization energies?

Write an account on the importance of the periodic table. Pay particular attention to the significance of the position of an element in the table and how the position relates to the chemical and physical properties of the element.
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