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Chapter 12: Problem 13

A white substance melts with some decomposition at \(730^{\circ} \mathrm{C}\). As a solid, it does not conduct electricity, but it dissolves in water to form a conducting solution. Which type of solid (molecular, metallic, covalent- network, or ionic) might the substance be?

Short Answer

Expert verified
Based on the given properties (melts at \(730^{\circ} \mathrm{C}\), does not conduct electricity as a solid, and forms a conducting solution when dissolved in water), the white substance is most likely an ionic solid.

Step by step solution

01

Analyze Molecular Solids

Molecular solids are held together by weak intermolecular forces (e.g., Van der Waals forces) and typically have low melting points. They do not conduct electricity as solids or in solution. Given that the substance in question melts at a high temperature (730掳C) and forms a conducting solution when dissolved in water, we can rule out the possibility of it being a molecular solid.
02

Analyze Metallic Solids

Metallic solids have a "sea of electrons" which allows them to conduct electricity well in both solid and liquid states. They can have a wide range of melting points depending on the metal. However, the white substance does not conduct electricity as a solid and only forms a conducting solution when dissolved in water. Therefore, it is not a metallic solid.
03

Analyze Covalent-Network Solids

Covalent-network solids are held together by strong covalent bonds giving them high melting points and thermally stable structures. They do not conduct electricity in any state and do not dissolve in water. Since our white substance dissolves in water and forms a conducting solution, we can rule out it being a covalent-network solid.
04

Analyze Ionic Solids

Ionic solids are formed by the electrostatic force between positive and negative ions. They typically have high melting points and do not conduct electricity in a solid state. However, when dissolved in water, the ions separate and are free to move, allowing the resulting solution to conduct electricity. Since the white substance dissolves in water, forms a conducting solution, and has a high melting point, this indicates that it is likely an ionic solid.
05

Conclusion

Based on the analysis of the given properties, the white substance is most likely an ionic solid.

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A white substance melts with some decomposition at \(730^{\circ} \mathrm{C}\). As a solid, it does not conduct electricity, but it dissolves in water to form a conducting solution. Which type of solid (molecular, metallic, covalent- network, or ionic) might the substance be?

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