---
title: "A student tests the electrical conductivity of a pure sample of \\(\\text{KCl}\\) in two different states: as a crystalline solid at \\(25\\ ^\\circ\\text{C}\\) and as a liquid at \\(800\\ ^\\circ\\text{C}\\) (above its melting point of \\(770\\ ^\\circ\\text{C}\\)). Which of the following statements correctly compares the electrical conductivity of the two samples and provides the best particulate-level justification?"
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url: "https://nerd-notes.com/ubq/119621/"
date_modified: "2026-08-21T08:11:49+00:00"
---

# A student tests the electrical conductivity of a pure sample of \(\text{KCl}\) in two different states: as a crystalline solid at \(25\ ^\circ\text{C}\) and as a liquid at \(800\ ^\circ\text{C}\) (above its melting point of \(770\ ^\circ\text{C}\)). Which of the following statements correctly compares the electrical conductivity of the two samples and provides the best particulate-level justification?

A student tests the electrical conductivity of a pure sample of \(\text{KCl}\) in two different states: as a crystalline solid at \(25\ ^\circ\text{C}\) and as a liquid at \(800\ ^\circ\text{C}\) (above its melting point of \(770\ ^\circ\text{C}\)). Which of the following statements correctly compares the electrical conductivity of the two samples and provides the best particulate-level justification?

- **A.** Solid \(\text{KCl}\) has a higher electrical conductivity than molten \(\text{KCl}\) because the closely packed ions in the rigid crystal lattice allow electrostatic charge to transfer rapidly across adjacent sites.
- **B.** Solid \(\text{KCl}\) has a higher electrical conductivity than molten \(\text{KCl}\) because the fixed lattice structure prevents thermal vibrations from scattering mobile valence electrons.
- **C.** Molten \(\text{KCl}\) has a higher electrical conductivity than solid \(\text{KCl}\) because the \(\text{K}^+\) and \(\text{Cl}^-\) ions are mobile in the liquid phase, whereas they are locked into fixed positions in the solid lattice.
- **D.** Molten \(\text{KCl}\) has a higher electrical conductivity than solid \(\text{KCl}\) because melting overcomes ionic attractions to release delocalized valence electrons that freely move throughout the liquid.

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119621/*