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Chapter 7: Problem 68

Silver and rubidium both form \(+1\) ions, but silver is far less reactive. Suggest an explanation, taking into account the ground-state electron configurations of these elements and their atomic radii.

Short Answer

Expert verified
Silver (Ag) is far less reactive than rubidium (Rb) because, although they both form +1 ions and have one valence electron in the 5s orbital, the atomic radius of rubidium is larger than that of silver. This means the valence electron in rubidium is easier to remove compared to silver, and hence, rubidium is more chemically reactive than silver.

Step by step solution

01

Determine the electron configurations of silver and rubidium atoms

In order to determine the electron configurations of silver and rubidium, we can refer to the periodic table where their atomic numbers are given. Silver (Ag) has an atomic number of 47, while rubidium (Rb) has an atomic number of 37. Using the atomic numbers, we can write the electron configurations for both elements as follows: Silver (Ag): \( 1s^2 2s^2 2p^6 3s^2 3p^6 3d^{10} 4s^2 4p^6 4d^{10} 5s^1 \) Rubidium (Rb): \( 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10} 4p^6 5s^1 \) It is important to analyze the outermost electrons, also known as valence electrons. Silver has one valence electron in the 5s orbital, while rubidium has one valence electron in the 5s orbital as well.
02

Analyze the atomic radii of silver and rubidium atoms

The other factor that can be taken into account is the atomic radii. In the periodic table, atoms increase in size as you move down a group (vertical column) and decrease in size as you move across a period (horizontal row). Rubidium is located in the alkali metals group and found in period 5. Silver is located in the transition metals group and found in period 5 as well. Since rubidium is on the far left of the period and silver is several elements to the right, we can conclude that rubidium has a larger atomic radius compared to silver.
03

Discuss the reactivity of silver and rubidium

The reactivity of an element is mainly determined by the ease with which it loses or gains electrons. Since both silver and rubidium have one valence electron in the 5s orbital, forming +1 ions, the atomic radius becomes an important factor to consider. Rubidium, with a larger atomic radius, means that its 5s valence electron is located farther from its nucleus and is less tightly bound, making it easier to be removed. On the other hand, silver's valence electron is closer to the nucleus due to its smaller atomic radius, resulting in a stronger attraction making it harder to be removed.
04

Conclusion

Silver (Ag) is far less reactive than rubidium (Rb) because, although they both form +1 ions and have one valence electron in the 5s orbital, the atomic radius of rubidium is larger than that of silver. This means the valence electron in rubidium is easier to remove compared to silver, and hence, rubidium is more chemically reactive than silver.

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Most popular questions from this chapter

(a) Why is calcium generally more reactive than magnesium? (b) Why is calcium generally less reactive than potassium?

Based on their positions in the periodic table, predict which atom of the following pairs will have the smaller first ionization energy\(:(\mathbf{a}) \mathrm{Cl}, \mathrm{Ar} ;(\mathbf{b}) \mathrm{Be}, \mathrm{Ca} ;(\mathbf{c}) \mathrm{K}, \mathrm{Co} ;(\mathbf{d}) \mathrm{S}, \mathrm{Ge} ;(\mathbf{e}) \mathrm{Sn}, \mathrm{Te}.\)

(a) Why does xenon react with fluorine, whereas neon does not? (b) Using appropriate reference sources, look up the bond lengths of \(\mathrm{Xe}-\mathrm{F}\) bonds in several molecules. How do these numbers compare to the bond lengths calculated from the atomic radii of the elements?

Which element has the highest second ionization energy: Li, K, or Be?

Compare the elements bromine and chlorine with respect to the following properties: (a) electron configuration, (b) most common ionic charge, (c) first ionization energy, (d) reactivity toward water, (e) electron affinity, (f) atomic radius. Account for the differences between the two elements.
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