Question 1: Define a covalent bond.

Answer: A covalent bond is a strong chemical bond formed when two atoms share a pair of electrons.

Question 2: Describe the structure of a diamond at the atomic level.

Answer: Diamond has a three-dimensional tetrahedral structure where each carbon atom is covalently bonded to four other carbon atoms, forming a very strong and rigid lattice.

Question 3: Explain why graphite is a good conductor of electricity while diamond is not.

Answer: Graphite has delocalized electrons that can move freely, allowing electricity to pass through, whereas diamond has no free electrons because all electrons are involved in strong covalent bonds.

Question 1: Calculate the number of covalent bonds in a single diamond crystal consisting of 8 carbon atoms, given each carbon forms four bonds.

Answer: 32 bonds (since each of the 8 carbon atoms forms 4 covalent bonds, total bonds = 8 x 4 / 2 = 16 bonds, counting shared bonds).

Question 2: If the bond energy of a C-C covalent bond is approximately 348 kJ/mol, estimate the total bond energy for the 32 bonds in the diamond crystal calculated above.

Answer: Approximately 11,136 kJ (since 32 bonds x 348 kJ/mol = 11,136 kJ).

Question 1: Describe a simple experiment to demonstrate the difference in electrical conductivity between Graphite and Diamond.

Answer: One possible experiment involves connecting a small piece of graphite and a piece of diamond to a circuit with a battery and a light bulb. Students observe that the bulb lights up with graphite but not with diamond, demonstrating that graphite conducts electricity due to delocalized electrons, whereas diamond does not because it lacks free electrons.

Question 2: Identify three safety precautions to consider when handling chemicals or conducting experiments related to covalent structures.

Answer: Wear safety goggles to protect eyes, handle chemicals with gloves to prevent skin contact, and work in a well-ventilated area to avoid inhaling fumes.

Question 1: A jewelry company wants to use diamond for gemstone jewelry and graphite for industrial lubricants. Explain how the properties of each material influence their applications.

Answer: Diamond's hardness and strength make it ideal for jewelry and cutting tools, while graphite's lubricating properties and ability to conduct electricity make it suitable for industrial lubricants and electrodes.

Question 2: Describe a technological innovation that uses the structure of Graphite to improve electronic devices.

Answer: Graphene, a single layer of graphite, is used in advanced electronic devices due to its excellent electrical conductivity, flexibility, and strength. It allows for the development of faster, lighter, and more efficient electronic components.