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Chapter 9: Problem 87

What makes a glass different from a crystalline solid such as \(\mathrm{SiO}_{2}\) ? Under what conditions could \(\mathrm{SiO}_{2}\) become glass-like?

Short Answer

Expert verified
Glass is amorphous and lacks long-range order; \(\mathrm{SiO}_2\) becomes glass-like with rapid cooling.

Step by step solution

01

Understand the Structure of Glass

Glass is an amorphous solid, meaning it lacks the long-range order that is characteristic of crystals. Its atoms are arranged randomly rather than in a repeating pattern.
02

Understand the Structure of Crystalline Solids

Crystalline solids, like silicon dioxide (\(\mathrm{SiO}_2\)), have a regular, repeating atomic structure. In \(\mathrm{SiO}_2\), this structure forms a continuous network, giving the solid definite edges and faces.
03

Glass-Like Conditions for \(\mathrm{SiO}_2\)

\(\mathrm{SiO}_2\) can become glass-like when it is cooled rapidly from a molten state. This rapid cooling prevents the atoms from forming the regular crystal lattice, resulting in a disordered, amorphous structure similar to glass.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Crystalline Solids
Crystalline solids are materials with a highly ordered atomic arrangement. Each atom in a crystalline solid is systematically organized in a repeating pattern, forming a crystal lattice. This order gives crystals their distinct shape with well-defined flat surfaces, known as crystal facets.

Key features of crystalline solids include:
  • Order: Atoms are arranged in a highly ordered structure, creating a regular pattern that repeats throughout the material.
  • Anisotropy: Physical properties like thermal conductivity or refractive index vary with direction due to the ordered structure.
This organized structure is what differentiates crystalline solids from amorphous ones like glass, providing them structural rigidity and distinct melting points.
Atomic Structure
Atomic structure refers to the arrangement of atoms within a substance. In crystalline solids, this arrangement involves a repeated, organized pattern. Each atom occupies a specific position within the lattice structure, contributing to the material's overall properties.

To illustrate this:
  • Lattice Points: Atoms are positioned at lattice points in a three-dimensional space.
  • Unit Cell: The smallest repeating unit that contains the full geometric and chemical repeat of the crystal.
  • Bonding: Atoms typically bond in ways that optimize energy stability, often forming a network that contributes to the material's stability and hardness.
Understanding atomic structure is crucial in materials science, as it affects not only the material's mechanical properties but also its electrical and optical characteristics.
Silicon Dioxide (SiO2)
Silicon dioxide, or \(\mathrm{SiO}_2\), is one of the most common compounds found in nature, primarily occurring in quartz and sand. It is a crystalline solid at room temperature, with each silicon atom covalently bonded to four oxygen atoms in a tetrahedral structure.

Key characteristics and uses of \(\mathrm{SiO}_2\) include:
  • Structure: Its continuous tetrahedral network gives it remarkable strength and stability, contributing to its use in glassware and cement.
  • Versatility: \(\mathrm{SiO}_2\) can also exist in an amorphous state, such as in glass, where the regular crystal structure is absent due to rapid cooling from a molten state.
  • Applications: It is used in various industries, including electronics, where it's valued as an insulator.
By altering cooling rates, the structure of \(\mathrm{SiO}_2\) can shift, showcasing the fascinating intertwining of crystalline and amorphous characteristics.

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Most popular questions from this chapter

Define sublimation.

The ions of \(\mathrm{NaF}\) and \(\mathrm{MgO}\) all have the same number of electrons, and the internuclear distances are about the same ( \(235 \mathrm{pm}\) and \(212 \mathrm{pm}\) ). Why, then, are the melting points of \(\mathrm{NaF}\) and \(\mathrm{MgO}\) so different \(\left(992{ }^{\circ} \mathrm{C}\right.\) and \(2825^{\circ} \mathrm{C},\) respectively \() ?\)

Potassium chloride and rubidium chloride both have the sodium chloride structure (Figure 9.24 ). X-ray diffraction experiments indicate that their cubic unit cell dimensions are \(629 \mathrm{pm}\) and \(658 \mathrm{pm}\), respectively. (i) One \(m o l \mathrm{KCl}\) and \(1 \mathrm{~mol} \mathrm{RbCl}\) are ground together to a very fine powder in a mortar and pestle, and the X-ray diffraction pattern of the pulverized solid is measured. Two patterns are observed, each corresponding to a cubic unit cell-one with an edge length of \(629 \mathrm{pm}\) and one with an edge length of \(658 \mathrm{pm}\). Call this Sample 1 . (ii) One \(\mathrm{mol} \mathrm{KCl}\) and \(1 \mathrm{~mol} \mathrm{RbCl}\) are heated until the entire mixture is molten and then cooled to room temperature. A single X-ray diffraction pattern indicates a cubic unit cell with an edge length of roughly \(640 \mathrm{pm}\). Call this Sample 2 . (a) Suppose that Samples 1 and 2 were analyzed for their chloride content. What fraction of each sample is chloride? Could the samples be distinguished by means of chemical analysis? (b) Interpret the two X-ray diffraction results in terms of the structures of the crystal lattices of Samples 1 and 2 . (c) What chemical formula should you write for Sample \(1 ?\) For Sample \(2 ?\) (d) Suppose that you dissolved \(1.00 \mathrm{~g}\) Sample 1 in \(100 \mathrm{~mL}\) water in a beaker and did the same with \(1.00 \mathrm{~g}\) Sample 2\. Which sample would conduct electricity better, or would both be the same? What ions would be present in each solution at what concentrations?

A liquid has a \(\Delta_{\text {vap }} H\) of \(44.0 \mathrm{~kJ} / \mathrm{mol}\) and a vapor pressure of \(370 \mathrm{mmHg}\) at \(90^{\circ} \mathrm{C}\). Calculate the vapor pressure of the liquid at \(130^{\circ} \mathrm{C}\).

Which substance has the greatest electrical conductivity? The smallest electrical conductivity? Explain your choice briefly. (a) Si (b) Ge (c) \(\mathrm{Ag}\) (d) \(\mathrm{P}_{4}\)
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