Question 1: Define an ionic bond and explain how it forms between atoms.

Answer: An ionic bond is the electrostatic attraction between oppositely charged ions, formed when a metal atom loses electrons to a non-metal atom.

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

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

Question 1: Calculate the number of moles in 50 grams of sodium chloride (NaCl). (Molar mass of NaCl = 58.44 g/mol)

Answer: 0.855 moles

Question 2: If 1 mole of calcium carbonate (CaCO3) decomposes, how many grams of calcium oxide (CaO) are produced if the reaction is: CaCO3 → CaO + CO2? (Molar mass of CaO = 56.08 g/mol)

Answer: 56.08 grams

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

Answer: To test solubility, add a fixed amount of the ionic compound to water at room temperature and stir. Measure the maximum amount that dissolves without residue to determine solubility. Control variables include temperature, amount of water, and amount of compound. Safety precautions involve wearing gloves and goggles to handle chemicals safely.

Question 1: A commercial water softener uses sodium chloride to remove calcium and magnesium ions from hard water. Explain how ionic bonding plays a role in this process and why sodium chloride is effective.

Answer: Sodium chloride dissociates into sodium and chloride ions, which exchange places with calcium and magnesium ions through ionic bonds. Sodium ions replace calcium and magnesium ions in the water, softening it because ionic bonds in the salts are broken, removing hardness.

Question 1: Explain why ionic compounds such as sodium chloride are used in the manufacture of everyday consumer products like bath salts and de-icing materials. Discuss their properties that make them suitable and any safety considerations.

Answer: Ionic compounds like sodium chloride have high solubility in water, allowing them to dissolve easily and release ions that can influence physical and chemical processes. In bath salts, their solubility helps in relaxing muscles, and in de-icing, their ability to lower freezing points is useful. Their high melting points and brittleness make them stable during storage. Safety considerations include handling with care to avoid skin irritation or environmental impact from overuse.