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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 free to move throughout the metal lattice. When an electric potential is applied, these delocalized electrons flow through the metal, allowing the conduction of electric current.
Step 2
Draw the dot and cross diagram of an oxygen molecule, O2. Show outer electrons only.
Answer
In an oxygen molecule (O2), each oxygen atom has six outer electrons. The dot-and-cross diagram shows the two oxygen atoms sharing two electrons each, forming a double bond, which can be represented as:
:O: - :O:
Here, the dots represent the electrons from one oxygen atom and the crosses represent the electrons from the other.
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 (K+) and negatively charged chloride ions (Cl-). These ionic bonds require a large amount of energy to break, which results 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 rigid, tetrahedral structure where each carbon atom is covalently bonded to four other carbon atoms. This structure provides diamond its hardness, making it suitable for cutting tools. In contrast, graphite has a layered structure where carbon atoms are arranged in planes, allowing layers to slide over each other easily. This makes graphite suitable for use as a lubricant and in electrodes, as it can facilitate the movement of electrons within its layers.