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Chapter 24: Problem 1

The ions formed in molecules from Group IA atoms (the alkali metals, such as \(\mathrm{Li}\) ) are almost exclusively \(\mathrm{M}^{+}\) ions rather than \(\mathrm{M}^{2+}\) ions. Explain this result.

Short Answer

Expert verified
Alkali metals such as Lithium typically form M+ ions because they have one electron in their outermost shell that they can lose with relatively low ionization energy to achieve a stable electronic configuration. Forming M2+ ions would require them to lose a second electron, which is closer to the nucleus and would require significantly more energy due to the increase in ionization energy. Because of this significant energy requirement, alkali metals primarily form M+ ions, not M2+ ions.

Step by step solution

01

Understanding atomic structure

Elements belonging to Group IA have one electron in their outermost shell. This is because Group IA is the first group in the periodic table and it includes alkali metals like Lithium (Li). The valence electron, or the electron in the outermost shell, is the one that is involved in chemical reactions or forms ions.
02

Understanding ion formation

Ions are formed when atoms lose or gain electrons to obtain a stable electronic configuration. Losing electrons results in positive ions (cations) and gaining electrons forms negative ions (anions). In this case, alkali metals form cations by losing the electron in their valence shell.
03

Understanding Ionization Energy

Ionization energy is the energy needed to remove an electron from an atom. The first ionization energy is the energy required to remove one electron, while the second ionization energy is the energy needed to remove a second electron. Removing more electrons requires more energy because the electrons are closer to the nucleus and thus, more attracted to the positive charge of it.
04

Applying the knowledge

Group IA elements like Lithium, having one electron in their outermost shell, can naturally lose one electron with a relatively low amount of ionization energy, as a result, forming M+ ions. To form M2+ ions, they would need to lose a second electron, which is closer to the nucleus and thus requires significantly more energy. Therefore, it's less likely to find these elements as M2+ ions as the high second ionization energy makes this process less likely to occur.

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Most popular questions from this chapter

The ions formed in molecules from Group IIA atoms (the alkaline earth metals, such as Mg) are almost exclusively \(\mathrm{M}^{2+}\) ions rather than \(\mathrm{M}^{3+}\) ions. Explain this result.

The ions formed in molecules from Group VIIA atoms (the halogens, such as Cl) are almost exclusively \(\mathrm{X}^{-}\) ions rather than \(\mathrm{X}^{2-}\) ions. Explain this result.
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