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Chapter 8: Problem 43

In each of the following pairs, indicate which one of the two species is smaller: (a) \(\mathrm{Cl}\) or \(\mathrm{Cl}^{-},\) (b) Na or \(\mathrm{Na}^{+}\), (c) \(\mathrm{O}^{2-}\) or \(\mathrm{S}^{2-},\) (d) \(\mathrm{Mg}^{2+}\) or \(\mathrm{Al}^{3+},\) (e) \(\mathrm{Au}^{+}\) or \(\mathrm{Au}^{3+}\).

Short Answer

Expert verified
The smaller species of each pair are: Cl, Na+, S2-, Al3+, Au3+.

Step by step solution

01

Analyze Cl and Cl-

When atoms gain electrons they become larger, as the added electrons are added to the same shell and electron-electron repulsion is increased. Therefore, \(\mathrm{Cl}^{-}\) which has gained an electron is larger than \(\mathrm{Cl}\).
02

Analyze Na and Na+

When atoms lose electrons, they become smaller as electrons are removed from the outermost shell, reducing the electron-electron repulsion. Therefore, \(\mathrm{Na}^{+}\) which has lost an electron is smaller than \(\mathrm{Na}\) .
03

Analyze O2- and S2-

\(\mathrm{O}^{2-}\) and \(\mathrm{S}^{2-}\) are both anions (negative ions) and have the same number of electrons. According to periodic trends, atomic radius increases down the group. So \(\mathrm{S}^{2-}\) is larger than \(\mathrm{O}^{2-}\) because Sulfur is below Oxygen in the Periodic Table.
04

Analyze Mg2+ and Al3+

\(\mathrm{Mg}^{2+}\) and \(\mathrm{Al}^{3+}\) have the same number of electrons. The cation with the greater nuclear charge will be smaller. Therefore, \(\mathrm{Al}^{3+}\) is smaller than \(\mathrm{Mg}^{2+}\) because it has a higher nuclear charge.
05

Analyze Au+ and Au3+

Both \(\mathrm{Au}^{+}\) and \(\mathrm{Au}^{3+}\) are cations from the same atom so the ion with the greater charge will be smaller as it has lost more electrons. Therefore, \(\mathrm{Au}^{3+}\) is smaller than \(\mathrm{Au}^{+}\) .

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Most popular questions from this chapter

State whether each of the elements listed here 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: \(\mathrm{Mg}, \mathrm{Cl}, \mathrm{Si}, \mathrm{Kr}, \mathrm{O}, \mathrm{I}\) \(\mathrm{Hg}, \mathrm{Br}\).

A technique called photo electron spectroscopy is used to measure the ionization energy of atoms. A sample is irradiated with ultraviolet (UV) light, and electrons are ejected from the valence shell. The kinetic energies of the ejected electrons are measured. Because the energy of the UV photon and the kinetic energy of the ejected electron are known, we can write \( h v=I E+\frac{1}{2} m u^{2} \) in which \(\nu\) is the frequency of the UV light, and \(m\) and \(u\) are the mass and velocity of the electron, respectively. In one experiment the kinetic energy of the ejected electron from potassium is found to be \(5.34 \times 10^{-19} \mathrm{~J}\) using a UV source of wavelength \(162 \mathrm{nm}\). Calculate the ionization energy of potassium. How can you be sure that this ionization energy corresponds to the electron in the valence shell (that is, the most loosely held electron)?

On the basis of their positions in the periodic table, select the atom with the larger atomic radius in each of these pairs: (a) \(\mathrm{Na}, \mathrm{Cs} ;\) (b) Be, \(\mathrm{Ba}\); (c) \(\mathrm{N}, \mathrm{Sb}\) (d) \(\mathrm{F}, \mathrm{Br},(\mathrm{e}) \mathrm{Ne}, \mathrm{Xe}\)

Explain why alkali metals have a greater affinity for electrons than alkaline earth metals do.

Write the outer electron contigurations for (a) the alkali metals, (b) the alkaline earth metals, (c) the halogens, (d) the noble gases.
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