Question 1: Define covalent bonding and explain how it contributes to the structure of diamond.

Answer: Covalent bonding is a type of chemical bond where atoms share pairs of electrons. In diamond, each carbon atom forms four strong covalent bonds with four other carbon atoms, creating a rigid three-dimensional lattice.

Question 2: Describe the arrangement of atoms in graphite and how this affects its physical properties.

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

Question 1: Calculate the number of covalent bonds in a diamond crystal containing 8 carbon atoms.

Answer: Each carbon atom forms 4 covalent bonds; total bonds = (8 atoms × 4 bonds) / 2 (since each bond is shared between two atoms) = 16 bonds.

Question 2: The melting point of diamond is approximately 3550°C. Convert this temperature to Kelvin.

Answer: Kelvin temperature = 3550 + 273 = 3823 K.

Question 1: Outline a simple experiment to compare the electrical conductivity of graphite and diamond. Include the variables you would control and safety precautions.

Answer: To compare electrical conductivity, connect each sample in a circuit with a power source and a light bulb. Control variables include sample size, temperature, and contact points. Safety precautions include handling electrical equipment carefully, ensuring no water contact, and wearing safety goggles.

Question 1: A sample of graphite conducts electricity efficiently, while a sample of diamond does not. Explain the reason based on their structures.

Answer: Graphite's layers have free electrons that can move and carry charge, making it conductive. Diamond's atoms are rigidly bonded in a three-dimensional network with no free electrons, so it is an insulator.

Question 2: Discuss one industrial application of each allotrope of carbon and how their structure influences their use.

Answer: Diamond is used in cutting tools and jewellery because of its hardness, which results from its strong covalent bonds in a rigid lattice. Graphite is used as a lubricant and in electrodes due to its layered structure that allows layers to slide and its good electrical conductivity.