Question 1: Define ionic bonding in terms of electron transfer and electrostatic attraction.

Answer: Ionic bonding is the electrostatic attraction between positively charged ions (cations) and negatively charged ions (anions) resulting from the transfer of electrons from one atom to another.

Question 2: Describe the typical physical properties of ionic compounds.

Answer: Ionic compounds are usually solid at room temperature, have high melting and boiling points, are brittle, and conduct electricity when molten or dissolved in water.

Question 3: Explain why ionic compounds conduct electricity when dissolved in water but not in solid form.

Answer: In solid form, ions are fixed in a lattice and cannot move, so they do not conduct electricity. When dissolved in water, ions are free to move, allowing electrical current to pass.

Question 4: Calculate the number of ions produced when 5 grams of sodium chloride (NaCl) dissolves in water. (Atomic masses: Na=23, Cl=35.5; Molar mass of NaCl=58.5 g/mol)

Answer: Approximately 5.09 x 10^23 ions (Na+ and Cl- ions combined).

Question 5: Identify two safety precautions to observe when handling ionic compounds in the laboratory.

Answer: Wear safety goggles and gloves to prevent contact with harmful substances; work in a well-ventilated area to avoid inhaling any dust or fumes.

Question 6: Describe a simple experiment to test the conductivity of an ionic compound in water.

Answer: Set up a circuit with two electrodes connected to a power source and a conductivity meter. Dissolve the ionic compound in water and place the electrodes into the solution. Observe the meter; a high reading indicates good conductivity due to free ions in solution.

Question 7: Analyze how the properties of ionic compounds make them suitable for use in salt bridges in electrochemical cells.

Answer: Ionic compounds like potassium chloride are used in salt bridges because they are soluble in water, produce free ions that conduct electricity, and are chemically stable. Their high solubility and electrical conductivity enable efficient transfer of ions, maintaining electrical neutrality in electrochemical cells.

Question 8: In what ways do the properties of ionic compounds influence their use in everyday products such as table salt and bath salts?

Answer: Their high solubility in water, high melting points, and ability to conduct electricity when dissolved make ionic compounds like table salt useful for seasoning, preserving food, and in bath salts for mineral supplementation and relaxation.

Question 9: Explain why ionic compounds tend to form crystalline structures and how this affects their properties.

Answer: Ionic compounds form crystalline structures because of the regular arrangement of ions in a lattice, which maximizes electrostatic attraction. This structure contributes to their high melting points, brittleness, and ability to dissolve in water.

Question 10: Discuss the impact of ionic bond properties on the development of new materials in technology.

Answer: The properties of ionic bonds, such as high melting points, electrical conductivity in solutions, and crystalline structures, are exploited in developing ceramics, electrolytes for batteries, and other electronic materials. These properties enable the design of durable, conductive, and stable components essential in modern technology.