Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 9: Problem 13

In which of the following states would \(\mathrm{NaCl}\) be electrically conducting? (a) solid, (b) molten (that is, melted), (c) dissolved in water. Explain your answers.

Short Answer

Expert verified
In its solid state, NaCl is electrically non-conducting. However, when it's molten or dissolved in water, it becomes an electrical conductor due to the freedom of movement of its ions.

Step by step solution

01

Analyze NaCl in Solid State

In its solid state, NaCl is composed of a crystal lattice where every sodium ion is surrounded by six chloride ions and vice versa. Because the ions are locked in place within this structure, they are not free to move. Consequently, solid NaCl does not conduct electricity.
02

Analyze NaCl in Molten State

In its molten state, the ionic lattice of NaCl breaks down, and the ions become free to move. The presence of mobile ions makes molten NaCl an electrically conducting substance.
03

Analyze NaCl Dissolved in Water

When NaCl is dissolved in water, the crystal lattice is disrupted, and Na and Cl ions are dispersed into the water, where they are free to move. Their movement, similar to the molten state case, allows the solution to conduct electricity.

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

An ionic bond is formed between a cation \(\mathrm{A}^{+}\) and an anion \(\mathrm{B}^{-}\). How would the energy of the ionic bond [see Equation (9.2)\(]\) be affected by the following changes? (a) doubling the radius of \(\mathrm{A}^{+},\) (b) tripling the charge on \(A^{+},(\mathrm{c})\) doubling the charges on \(\mathrm{A}^{+}\) and \(\mathrm{B}^{-},\) (d) decreasing the radii of \(\mathrm{A}^{+}\) and \(\mathrm{B}^{-}\) to half their original values.

Write Lewis structures for the reaction $$ \mathrm{AlCl}_{3}+\mathrm{Cl}^{-} \longrightarrow \mathrm{AlCl}_{4}^{-} $$ What kind of bond is between \(\mathrm{Al}\) and \(\mathrm{Cl}\) in the product?

What is the difference between a Lewis dot symbol and a Lewis structure?

Using this information: $$ \begin{array}{rr} \mathrm{C}(s) \longrightarrow \mathrm{C}(g) & \Delta H_{\mathrm{rxn}}^{\circ}=716 \mathrm{~kJ} / \mathrm{mol} \\ 2 \mathrm{H}_{2}(g) \longrightarrow 4 \mathrm{H}(g) & \Delta H_{\mathrm{rxn}}^{\circ}=872.8 \mathrm{~kJ} / \mathrm{mol} \end{array} $$ and the fact that the average \(\mathrm{C}-\mathrm{H}\) bond enthalpy is \(414 \mathrm{~kJ} / \mathrm{mol}\), estimate the standard enthalpy of formation of methane \(\left(\mathrm{CH}_{4}\right)\).

Which of these molecules has the shortest nitrogento-nitrogen bond? Explain. $$ \begin{array}{llll} \mathrm{N}_{2} \mathrm{H}_{4} & \mathrm{~N}_{2} \mathrm{O} & \mathrm{N}_{2} & \mathrm{~N}_{2} \mathrm{O}_{4} \end{array} $$
See all solutions

Recommended explanations on Chemistry Textbooks

Making Measurements

Read Explanation

Organic Chemistry

Read Explanation

Chemical Reactions

Read Explanation

Inorganic Chemistry

Read Explanation

Nuclear Chemistry

Read Explanation

The Earths Atmosphere

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free