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Chapter 11: Problem 53

A solid is very hard and has a high melting point. Neither the solid nor its melt conducts electricity. Classify the solid.

Short Answer

Expert verified
The solid is a Covalent-Network Solid.

Step by step solution

01

Identifying Key Information

First, note down all the key properties given in the exercise: the solid is very hard, has a high melting point, and does not conduct electricity either in solid or melted form.
02

Compare Characteristics with Types of Solid

Four types of solids are generally identified: metallic, ionic, covalent-network, and molecular. Metallic and Ionic solids conduct electricity therefore they can't be an option. Between the remaining two, covalent-network solids are hard, have high melting points, and do not conduct electricity, these all match with the given properties.
03

Classifying the solid

The solid has characteristics of a Covalent-Network Solid. So, the given solid can be classified as a Covalent-Network Solid.

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Most popular questions from this chapter

As a liquid is heated at constant pressure, its temperature rises. This trend continues until the boiling point of the liquid is reached. No further rise in temperature of the liquid can be induced by heating. Explain.

A \(1.20-\mathrm{g}\) sample of water is injected into an evacuated \(5.00-\mathrm{L}\) flask at \(65^{\circ} \mathrm{C} .\) What percentage of the water will be vapor when the system reaches equilibrium? Assume ideal behavior of water vapor and that the volume of liquid water is negligible. The vapor pressure of water at \(65^{\circ} \mathrm{C}\) is \(187.5 \mathrm{mmHg}\)

Calculate the \(\Delta H^{\circ}\) for the following processes at \(25^{\circ} \mathrm{C}\) (a) \(\mathrm{Br}_{2}(l) \longrightarrow \mathrm{Br}_{2}(g)\) and (b) \(\mathrm{Br}_{2}(g) \longrightarrow\) \(2 \mathrm{Br}(g) .\) Comment on the relative magnitudes of these \(\Delta H^{\circ}\) values in terms of the forces involved in each case. \\{Hint: See Table \(9.4,\) and given that \(\left.\Delta H_{\mathrm{f}}^{\circ}\left[\mathrm{Br}_{2}(g)\right]=30.7 \mathrm{~kJ} / \mathrm{mol} .\right\\}\)

The fluorides of the second-period elements and their melting points are: \(\mathrm{LiF}, 845^{\circ} \mathrm{C} ; \mathrm{BeF}_{2}\), \(800^{\circ} \mathrm{C} ; \mathrm{BF}_{3},-126.7^{\circ} \mathrm{C} ; \mathrm{CF}_{4},-184^{\circ} \mathrm{C} ; \mathrm{NF}_{3}\) \(-206.6^{\circ} \mathrm{C} ; \quad \mathrm{OF}_{2},-223.8^{\circ} \mathrm{C} ; \quad \mathrm{F}_{2},-219.6^{\circ} \mathrm{C}\) Classify the type(s) of intermolecular forces present in each compound.

Explain how water's phase diagram differs from those of most substances. What property of water causes the difference?
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