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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 (Li), form M+ ions rather than M2+ ions because they contain a single electron in their outermost shell. They achieve stability by losing this electron, forming a M+ ion. Forming a M2+ ion would require losing another electron from a stable inner shell, which is energetically unfavorable, and therefore does not typically occur.

Step by step solution

01

Electronic Configuration

Group IA elements belong to the first group of the periodic table. They have one electron in their outermost shell following the '2n^2' rule (where 'n' represents the principal quantum number, or energy level). Having one electron in their outermost shell makes them highly unstable.
02

Formation of Positive Ions

In order to achieve stability, alkali metals tend to lose one electron from their outermost shell. When they lose an electron, they form a cation (positive ion) - denoted as M+. This is due to the fact that by losing an electron, the alkali metals now have one more proton than electron, thus gaining a positive charge.
03

Lack of M2+ ions formation

In order for a M2+ ion to form, the alkali metal would need to lose two electrons. However, after losing their single electron in the outermost shell, the alkali metals reach a state of stability, similar to that of the noble gases. Losing another electron would require breaking into the stable inner shell, which requires a lot of energy and is generally not favorable. Therefore, M2+ ions typically do not form.

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Most popular questions from this chapter

a) What is the charge on the cation formed from \(\mathrm{Mg}\) ? b) What is the charge on the anion formed from \(\mathrm{O}\) (called the oxide ion)? c) What is the formula for the ionic compound containing magnesium ions and oxide ions?

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

Consider the ionic compounds \(\mathrm{MgO}\) and \(\mathrm{MgS}\) : a) In which compound is the Coulombic force of attraction greater? b) \(\mathrm{MgO}\) has a melting point of \(2852^{\circ} \mathrm{C}\). Which of these would you predict is the melting point of \(\mathrm{MgS}:\) about \(2000{ }^{\circ} \mathrm{C}\), about \(2850{ }^{\circ} \mathrm{C}\), about \(4000{ }^{\circ} \mathrm{C}\) ? Explain your reasoning.

Consider the ionic compounds \(\mathrm{NaF}\) and \(\mathrm{NaCl}\) : a) In which compound is the Coulombic force of attraction greater? b) \(\mathrm{NaCl}\) has a melting point of \(801{ }^{\circ} \mathrm{C}\). Which of these would you predict is the melting point of \(\mathrm{NaF}: 609^{\circ} \mathrm{C}, 800{ }^{\circ} \mathrm{C}, 993{ }^{\circ} \mathrm{C} ?\) Explain your reasoning.

In \(\mathrm{NaCl}\), what are the charges on the ions? Explain your reasoning.
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