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Chapter 24: Problem 2

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.

Short Answer

Expert verified
Alkaline earth metals belonging to the Group IIA like Magnesium have two electrons in their outermost shell. Thus, they prefer to lose these two electrons to achieve a stable noble gas configuration, forming \(M^{2+}\) ions. Losing one additional electron would cost a lot of energy, making the formation of \(M^{3+}\) ions unfavorable.

Step by step solution

01

Understanding the Alkaline Earth Metals

Alkaline earth metals like Magnesium belong to Group IIA of the Periodic Table. They have two electrons in their outermost shell, which can be known from their position in the periodic table.
02

Interpretation of Ion formation

When these metals react with other elements, they tend to lose two electrons to achieve a stable electronic configuration, which corresponds to the nearest noble gas. As a result, they form \(M^{2+}\) ions.
03

Why not \(M^{3+}\) ions

Forming \(M^{3+}\) ions would mean that these metals have to lose an extra electron from a lower energy level, which is stable. This process requires a significant amount of energy and therefore is unfavorable. Hence, Group IIA elements, like Magnesium, preferably form \(M^{2+}\) ions, which is the reason why they form \(M^{2+}\) ions rather than \(M^{3+}\) ions.

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Most popular questions from this chapter

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.

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?

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.

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.

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