Question 1: Explain what covalent bonding is and how it contributes to the structure of diamond and graphite.

Answer: Covalent bonding involves sharing electrons between atoms. In diamond, each carbon atom forms four strong covalent bonds in a tetrahedral structure, creating a rigid 3D network. In graphite, each carbon atom forms three covalent bonds in a hexagonal layer, with weak forces between layers, allowing layers to slide past each other.

Question 2: Define the term 'allotrope' and identify whether diamond and graphite are allotropes of the same element.

Answer: An allotrope is a different form of the same element with different structures. Yes, diamond and graphite are allotropes of carbon.

Question 1: Describe the structure of diamond and how it affects its hardness.

Answer: Diamond has a rigid 3D network of covalently bonded carbon atoms in a tetrahedral arrangement, making it extremely hard and durable.

Question 2: Explain why graphite is soft and slippery despite being made of covalently bonded carbon atoms.

Answer: Graphite has layers of hexagonally arranged carbon atoms with weak forces between layers, allowing them to slide over each other, making graphite soft and slippery.

Question 3: Which form of carbon (diamond or graphite) is a good conductor of electricity? Explain why.

Answer: Graphite is a good conductor because it has free electrons in its layers, allowing electricity to pass through, while diamond does not conduct electricity.

Question 1: Calculate the number of covalent bonds in a single layer of graphite if each carbon atom forms 3 bonds and there are 6 carbon atoms in the layer.

Answer: Number of bonds = (Number of carbon atoms) × (Bonds per atom) / 2 = 6 × 3 / 2 = 9 bonds.

Question 2: Identify one industrial application of each allotrope of carbon and briefly explain its importance.

Answer: Diamond is used in cutting tools and jewelry due to its hardness and brilliance. Graphite is used as a lubricant and in batteries because of its electrical conductivity and layered structure.

Question 1: Describe a safe laboratory procedure for testing the electrical conductivity of graphite.

Answer: Use insulated gloves and ensure the circuit is properly set up with a power source and a multimeter. Connect the graphite sample in the circuit and observe if current flows, indicating conductivity. Always follow safety protocols to prevent shocks.

Question 2: List two precautions to take when handling diamond or graphite samples in a lab setting.

Answer: Wear protective gloves to prevent contamination or injury and handle samples carefully to avoid breakage or loss.