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6 (a) Explain, in terms of their structure, how metals conduct electricity - Edexcel - GCSE Chemistry - Question 6 - 2017 - Paper 1
Question 6
6 (a) Explain, in terms of their structure, how metals conduct electricity. (b) Oxygen is a simple molecular, covalent substance. The electronic configuration of an... show full transcript
Worked Solution & Example Answer:6 (a) Explain, in terms of their structure, how metals conduct electricity - Edexcel - GCSE Chemistry - Question 6 - 2017 - Paper 1
Step 1
Explain, in terms of their structure, how metals conduct electricity.
Answer
Metals conduct electricity due to the presence of delocalized electrons. These electrons are not fixed to any particular atom and can move freely throughout the metallic lattice. This movement of electrons allows electrical current to flow through the metal.
Step 2
Draw the dot and cross diagram of an oxygen molecule, O2. Show outer electrons only.
Answer
The dot and cross diagram for an oxygen molecule, O2, would show two oxygen atoms bonded together, where each atom has six outer electrons. In the diagram, the electrons from one oxygen atom can be represented by dots (•) and the electrons from the other by crosses (x). Each oxygen shares two electrons in a double bond, resulting in a complete outer shell for both atoms.
Step 3
Explain why potassium chloride has such a high melting point.
Answer
Potassium chloride has a high melting point due to the strong electrostatic forces of attraction between the positively charged potassium ions and the negatively charged chloride ions. These strong ionic bonds require a large amount of heat energy to break, resulting in a high melting point.
Step 4
Explain, using ideas about their structures, why diamond and graphite are suitable for these uses.
Answer
Diamond has a strong tetrahedral structure where each carbon atom is covalently bonded to four other carbon atoms, making it extremely hard and suitable for cutting tools. In contrast, graphite has a layered structure where each carbon atom is bonded to three others in flat sheets. These sheets can slide over one another, making graphite an excellent lubricant. Additionally, the delocalized electrons in graphite allow it to conduct electricity, making it suitable for use in electrodes.