Question 1: Explain what is meant by the term 'ionic bond' and how it influences the properties of ionic compounds.

Answer: An ionic bond is a type of chemical bond formed when electrons are transferred from one atom to another, resulting in positively and negatively charged ions. This electrostatic attraction gives ionic compounds their characteristic properties such as high melting points and solubility in water.

Question 2: List three common physical properties of ionic compounds.

Answer: High melting and boiling points, solubility in water, and brittleness.

Question 1: Define solubility and explain why ionic compounds are generally soluble in water but insoluble in non-polar solvents.

Answer: Solubility is the ability of a substance to dissolve in a solvent. Ionic compounds are soluble in water because water molecules are polar and can stabilize the charged ions, but they are insoluble in non-polar solvents because these lack the polarity needed to separate and stabilize the ions.

Question 2: Describe how the structure of an ionic compound relates to its brittleness.

Answer: Ionic compounds have a regular, repeating crystal lattice structure. When a force causes layers to shift, like charges align, causing repulsion and resulting in the crystal breaking, which makes ionic compounds brittle.

Question 1: Calculate the molar mass of sodium chloride (NaCl). Given atomic masses: Na = 23 g/mol, Cl = 35.5 g/mol.

Answer: 58.5 g/mol

Question 2: If 5 grams of potassium iodide (KI) dissolves in 100 mL of water, what is its molarity? Atomic masses: K = 39 g/mol, I = 127 g/mol.

Answer: 0.33 mol/L

Question 1: Describe a simple experiment to test the solubility of an ionic compound in water. Include the variables involved and safety precautions.

Answer: Dissolve a fixed amount of the ionic compound in varying volumes of water at room temperature. Variables include the amount of compound, volume of water, and temperature. Safety precautions include wearing gloves and goggles, working in a well-ventilated area, and handling chemicals carefully.

Question 1: A set of ionic compounds shows the following melting points: Compound A - 800°C, Compound B - 600°C, Compound C - 400°C. Explain what factors could account for these differences.

Answer: Differences in melting points can be due to varying strengths of ionic bonds, lattice energies, and ionic sizes. Stronger bonds and higher lattice energies generally lead to higher melting points.

Question 2: Given that sodium chloride dissolves readily in water and has a high melting point, analyze how its ionic structure contributes to these properties.

Answer: Sodium chloride’s ionic structure involves a strong electrostatic attraction between Na+ and Cl- ions within a crystal lattice, resulting in high melting points. Its polarity and ability of water molecules to stabilize the ions through ion-dipole interactions enable it to dissolve readily in water.

Question 1: Explain how ionic compounds are used in the manufacture of table salt and why their properties are suited for this purpose.

Answer: Table salt is sodium chloride, an ionic compound that is soluble in water, stable at room temperature, and safe for consumption. Its high melting point allows it to be processed at high temperatures without decomposition.

Question 2: Discuss how ionic compounds contribute to the development of salt-based batteries for energy storage.

Answer: Salt-based batteries utilize ionic compounds like sodium or lithium salts that can conduct ions between electrodes. Their high ionic conductivity, stability, and ability to transfer charge efficiently make them suitable for energy storage applications in sustainable technologies.