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Chapter 22: Problem 7

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?

Short Answer

Expert verified
a) The charge on the cation formed from \(\mathrm{Mg}\) is +2. b) The charge on the anion formed from \(\mathrm{O}\) is -2. c) The formula for the ionic compound containing magnesium ions and oxide ions is \(\mathrm{MgO}\).

Step by step solution

01

Determine the charge on the Magnesium ion

The element Magnesium (Mg) is in the second group of the periodic table, which means it has 2 valence electrons. To achieve a stable configuration, it tends to lose its 2 valence electrons. When it loses 2 electrons, it develops a charge of +2. Therefore, the charge on the cation formed from Magnesium (\(\mathrm{Mg}\)) is +2.
02

Determine charge on the Oxygen ion

The element Oxygen (O) is in the sixth group of the periodic table, which means it has 6 valence electrons. It needs two more electrons to reach a stable electron configuration. When it gains 2 electrons, it will have a charge of -2. Therefore, the charge on the anion formed from Oxygen (\(\mathrm{O}\)), the oxide ion, is -2.
03

Determine the formula of the ionic compound

An ionic compound is neutral overall, meaning the number of positive charges must equal the number of negative charges. This implies that 1 Mg+2 ion can combine with 1 O-2 ion to form a neutral compound. Thus, the formula for the ionic compound formed from magnesium ions and oxide ions will be MgO.

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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) Determine the core charge and valence shell for \(\mathrm{F}^{-}\), and \(\mathrm{F}^{2-}\). Drawing diagrams may be helpful. b) Based on your answer to part a, explain why an attempt to add an electron to \(\mathrm{F}^{-}\) does not result in the formation of \(\mathrm{F}^{2-}-\) that is, the "added" electron does not stay "attached" to the original \(\mathrm{F}^{-}\) ion. c) The ions formed in molecules from Group 17 atoms (the halogens, such as \(\mathrm{F}\) ) are almost exclusively \(\mathrm{X}^{-}\) ions rather than \(\mathrm{X}^{2-}\) ions. Explain this result based on your answers to parts a and b.

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

When an ionic bond is formed, what type of atom (in terms of relative electronegativity) is likely to: a) lose one or more electrons? b) gain one or more electrons? Explain your reasoning.
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