Ionic bonding: Practice Questions

A neutral magnesium atom (\(Mg\)) has an electronic configuration of 2.8.2. How does a magnesium atom achieve a stable electron configuration, and what ion does it form?

Which statement best explains why ionic compounds, such as potassium chloride (\(KCl\)), have high melting points?

Iron(III) sulfate is an ionic compound. Given that the iron(III) ion is \(Fe^{3+}\) and the sulfate ion is \(SO_4^{2-}\), what is the correct formula for iron(III) sulfate?

Why can solid ionic compounds not conduct electricity?

Ionic compounds generally have high melting points. This property is best explained by the need to overcome:

Explain why solid lithium chloride, an ionic compound, is unable to conduct electricity.

State the chemical formula for the ionic compound formed between zinc ions (\(Zn^{2+}\)) and nitrate ions (\(NO_3^-\)), and explain how the ratio of these ions ensures the compound is electrically neutral.

Ionic compounds are often described as brittle. Explain this characteristic property by considering the effect of a physical force displacing layers of ions within the rigid giant lattice.

Ionic compounds are formed when cations and anions attract each other. Use your knowledge of ion charges to determine the chemical formula for the following compounds:

a) Iron(III) Nitrate (The ions are iron(III) ( \(Fe^{3+}\) ) and nitrate ( \(NO_3^- ))

b) Copper(II) Carbonate (The ions are copper(II) (\)C\(u^{2+}\)\) ) and carbonate ( \(CO_3^{2-}\) )

Potassium Iodide ( \(KI\) ) is an ionic compound.

a) Describe the general arrangement of the ions in solid Potassium Iodide.

b) Explain why Potassium Iodide has a high melting point, relating this property to its structure and the nature of the ionic bonding.

c) Explain the difference in electrical conductivity of Potassium Iodide when it is in the solid state compared to when it is dissolved in water (aqueous solution).