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Chapter 8: Problem 61

From the electron-affinity values for the alkali metals, do you think it is possible for these metals to form an anion like \(\mathrm{M}^{-},\) where \(\mathrm{M}\) represents an alkali metal?

Short Answer

Expert verified
While theoretically, alkali metals can form an anion due to their negative electron affinity (meaning energy is released when an electron is added), the resulting anion is likely not stable since alkali metals typically prefer to lose an electron to achieve stability. Therefore, in practical terms, it is uncommon for alkali metals to form anions.

Step by step solution

01

Understand Electron Affinity

Electron affinity refers to the energy change that occurs when an electron is added to a neutral atom. It measures the attraction (or repulsion) between the electron and the atom's nucleus. Alkali metals, being in the first group of the periodic table, have one electron in their outermost shells. Adding an electron would mean filling this shell, leading to increased stability.
02

Apply the Concept to Alkali Metals

Remember that the alkali metals (Group 1 elements excluding Hydrogen) are Lithium (Li), Sodium (Na), Potassium (K), Rubidium (Rb), Cesium (Cs), and Francium (Fr). These metals have a single electron in their outermost orbital, and they are also known for their low ionization energies. Given that electron affinity values are generally negative for alkali metals, they would release energy when an additional electron is added, potentially forming an anion.
03

Consider the Stability of the Anion

While it is possible for an alkali metal to gain an electron and form an anion due to its negative electron affinity, the anion may not be stable. This is because alkali metals prefer to lose an electron to achieve a stable electron configuration. Thus, even though the formation of an anion is energetically favored, these anions may not be stable and can lose the electron easily.

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Most popular questions from this chapter

Write ground-state electron configurations for these ions, which play important roles in biochemical processes in our bodies: (a) \(\mathrm{Na}^{+},\) (b) \(\mathrm{Mg}^{2+},\) (c) \(\mathrm{Cl}^{-}\) (d) \(\mathrm{K}^{+},\) (e) \(\mathrm{Ca}^{2+},\) (f) \(\mathrm{Fe}^{2+},(\mathrm{g}) \mathrm{Cu}^{2+},\) (h) \(\mathrm{Zn}^{2+}\)

Name the ions with +3 charges that have these electron configurations: (a) \([\mathrm{Ar}] 3 d^{3},(\mathrm{~b})[\mathrm{Ar}],\) (c) \([\mathrm{Kr}] 4 d^{6}\) (d) \([\mathrm{Xe}] 4 f^{14} 5 d^{6}\)

Group these electron configurations in pairs that would represent similar chemical properties of their atoms: (a) \(1 s^{2} 2 s^{2} 2 p^{5}\) (b) \(1 s^{2} 2 s^{1}\) (c) \(1 s^{2} 2 s^{2} 2 p^{6}\) (d) \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{5}\) (e) \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{1}\) (f) \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{2} 3 d^{10} 4 p^{6}\)

Which elements are more likely to form acidic oxides? basic oxides? amphoteric oxides?

Based on your knowledge of the chemistry of the alkali metals, predict some of the chemical properties of francium, the last member of the group.
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