This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
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Here's the solution to question (a)(iv): a) (iv) Explain why silicon dioxide exists as a solid of high melting point whereas carbon dioxide is a gas even though silicon and carbon belong to the same group. Step 1: Describe the structure of carbon dioxide. Carbon dioxide (CO_2) is a simple molecular substance. It consists of discrete CO_2 molecules held together by weak intermolecular forces (van der Waals forces). Step 2: Describe the structure of silicon dioxide. Silicon dioxide (SiO_2) has a giant covalent network structure. Each silicon atom is covalently bonded to four oxygen atoms, and each oxygen atom is covalently bonded to two silicon atoms, forming a continuous three-dimensional network. Step 3: Relate the structures to their physical properties. To melt CO_2, only a small amount of energy is required to overcome the weak intermolecular forces, which is why it is a gas at room temperature. In contrast, to melt SiO_2, a large amount of energy is needed to break the strong covalent bonds throughout its giant network structure, resulting in a high melting point and solid state at room temperature. The difference in structure is due to carbon's ability to form stable double bonds with oxygen, leading to discrete CO_2 molecules, while silicon prefers to form single bonds with oxygen, leading to an extended network. What's next? Send 'em! 📸