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Chapter 8: Problem 64

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

Short Answer

Expert verified
Alkali metals show a higher electron affinity than alkaline earth metals because after losing their single outer electron, they become more positively charged and tend to attract electrons. Conversely, alkaline earth metals, with two electrons in their outer shell, have a lower tendency to attract additional electrons.

Step by step solution

01

Alkali Metals Affinity

Firstly, it is necessary to understand the electron affinity of alkali metals. Alkali metals have one electron in their outer shell. This single electron is relatively easy to remove, essentially meaning alkali metals tend to readily give away this electron to achieve a stable electronic configuration. However, after losing this electron, they become more charged positively and want to gain an electron, hence they display a good electron affinity.
02

Alkaline Earth Metals Affinity

Next, consider the electron affinity of alkaline earth metals. These metals have two electrons in their outermost shell. Because they have two rather than one electron, they are relatively more difficult to remove - the force of attraction between the nucleus and the second electron is stronger. Therefore, alkaline earth metals are less willing than alkali metals to attract an extra electron.
03

Comparison

In conclusion, alkali metals have higher electron affinity than alkaline earth metals because they readily lose their outer electron and become positively charged, which attracts electrons. On the other hand, alkaline earth metals, having two outer electrons, don't show this much eagerness towards gaining electrons.

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Most popular questions from this chapter

Match each of the elements on the right with its description on the left: (a) A pale yellow gas that reacts with water. (b) A soft metal that reacts with water to produce hydrogen. (c) A metalloid that is hard and has a high melting point. (d) A colorless, odorless gas. (e) A metal that is more reactive than iron, but does not corrode in air. Nitrogen \(\left(\mathrm{N}_{2}\right)\) Boron (B) Aluminum (Al) Fluorine \(\left(\mathrm{F}_{2}\right)\) Sodium (Na)

Explain, in terms of their electron configurations, why \(\mathrm{Fe}^{2+}\) is more easily oxidized to \(\mathrm{Fe}^{3+}\) than \(\mathrm{Mn}^{2+}\) is to \(\mathrm{Mn}^{3+}\)

Define atomic radius. Does the size of an atom have a precise meaning?

As discussed in the chapter, the atomic mass of argon is greater than that of potassium. This observation created a problem in the early development of the periodic table because it meant that argon should be placed after potassium. (a) How was this difficulty resolved? (b) From the following data, calculate the average atomic masses of argon and potassium: Ar-36 (35.9675 amu; 0.337 percent), \(\begin{array}{lll}\text { Ar- } 38 & (37.9627 & \text { amu } ; & 0.063 \text { percent), } & \text { Ar-40 }\end{array}\) \((39.9624 \mathrm{amu} ; 99.60\) percent \() ; \mathrm{K}-39(38.9637 \mathrm{amu} ;\) 93.258 percent \(,\) K- 40 ( 39.9640 amu; 0.0117 percent), K-41 \((40.9618\) amu; 6.730 percent).

The air in a manned spacecraft or submarine needs to be purified of exhaled carbon dioxide. Write equations for the reactions between carbon dioxide and (a) lithium oxide \(\left(\mathrm{Li}_{2} \mathrm{O}\right),\) (b) sodium peroxide \(\left(\mathrm{Na}_{2} \mathrm{O}_{2}\right),\) and \((\mathrm{c})\) potassium superoxide \(\left(\mathrm{KO}_{2}\right)\)
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