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For the question you provided, here’s the breakdown:

1(a) Complete the table by providing the correct type of structure for each substance.

• Substance A: Poor electrical conductivity in solid and liquid states, with a low melting point. This indicates a simple molecular structure.
• Substance B: Poor electrical conductivity in solid and liquid states, but with a high melting point. This indicates a giant covalent (or macromolecular) structure.
• Substance C: Good electrical conductivity in solid and liquid states, with a high melting point. This indicates a metallic structure.
• Substance D: Poor electrical conductivity in solid state, but good in liquid state, with a high melting point. This indicates an ionic structure.

The completed table is as follows:

Substance	Electrical conductivity: in solid state	Electrical conductivity: in liquid state	Melting point	Type of structure
A	Poor	Poor	Low	Simple molecular
B	Poor	Poor	High	Giant covalent
C	Good	Good	High	Metallic
D	Poor	Good	High	Ionic

1(b) Explain why:

• 1(b)(i) Substance A is a poor conductor in both solid and liquid states. Substance A has a simple molecular structure. These molecules lack free-moving ions or delocalized electrons to carry electric charge. Therefore, they cannot conduct electricity in either state.

• 1(b)(ii) Substance D conducts electricity in liquid state but not in solid state. Substance D has an ionic structure. In solid state, ions are fixed in place and cannot move. In liquid state (when melted), ions are free to move and can carry electric charge.

• 1(b)(iii) Give an example of a substance that would show similar properties to substance C. Substance C has a metallic structure. Metals have delocalized electrons that can move freely, allowing them to be good conductors of electricity in both solid and liquid states. Example: Copper.