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Royal Society of Chemistry, The
Introduction to Glass Science and Technology / Edition 2

Introduction to Glass Science and Technology / Edition 2

by James E Shelby


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Product Details

ISBN-13: 9780854046393
Publisher: Royal Society of Chemistry, The
Publication date: 03/28/2005
Series: RSC Paperbacks Series
Edition description: Second Edition
Pages: 308
Sales rank: 1,165,106
Product dimensions: 6.14(w) x 9.21(h) x 0.76(d)

Read an Excerpt

Introduction to Glass Science and Technology

By James E. Shelby

The Royal Society of Chemistry

Copyright © 2005 The Royal Society of Chemistry
All rights reserved.
ISBN: 978-0-85404-639-3



The presence of glasses in our everyday environment is so common that we rarely notice their existence. Our current casual attitude toward the family of materials known as glasses has not always existed. Early Egyptians considered glasses as precious materials, as evidenced by the glass beads found in the tombs and golden death masks of ancient Pharaohs. The cave-dwellers of even earlier times relied on chipped pieces of obsidian, a natural volcanic glass, for tools and weapons, i.e., scrapers, knives, axes, and heads for spears and arrows.

Humans have been producing glasses by melting of raw materials for thousands of years. Egyptian glasses date from at least 7000 B.C. How did the first production of artificial glasses occur? One scenario suggests that the combination of sea salt (NaCl) and perhaps bones (CaO) present in the embers of a fire built on the sands (SiO2) at the edge of a saltwater sea (the Mediterranean?), sufficiently reduced the melting point of the sand to a temperature where crude, low quality glass could form. At some later time, some other nomad found these lumps of glass in the sand and recognized their unusual nature. Eventually, some genius of ancient times realized that the glass found in the remains of such fires might be produced deliberately, and discovered the combination of materials which lead to the formation of the first commercial glasses.

The first crude man-made glasses were used to produce beads, or to shape into tools requiring sharp edges. Eventually, methods for production of controlled shapes were developed. Bottles were produced by winding glass ribbons around a mold of compacted sand. After cooling the glass, the sand was scraped from inside the bottle, leaving a hollow container with rough, translucent walls and usually lopsided shape. Eventually, the concept of molding and pressing jars and bottles replaced the earlier methods and the quality of the glassware improved. It began to be possible to produce glasses which were reasonably transparent, although usually still filled with bubbles and other flaws.

The invention of glass blowing around the first century B.C. generated a greatly expanded range of applications for glasses. The quality of glass jars and bottles improved dramatically, glass drinking vessels became popular, and the first clear sheet glasses became available; which eventually allowed the construction of buildings with enclosed windows. Colored glasses came into common use, with techniques for production of many colors regarded as family secrets, to be passed on from generation to generation of artisans. The method for producing red glasses by inclusion of gold in the melt, for example, was discovered and then lost, only to be rediscovered hundreds of years later. The combination of the discovery of many new colorants with the invention of glass blowing eventually lead to the magnificent stained glass windows of so many of the great cathedrals of Europe and the Near East.

The advent of the age of technology created many new opportunities for the application of glasses. The evolution of chemistry from the secretive practices of alchemists searching for the philosopher's stone, to a profession involving millions of workers worldwide was strongly influenced by the invention of chemically-resistant borosilicate glasses. Modern electronics became a reality with the invention of glass vacuum tubes, which evolved into the monitors for our computers and the televisions we watch every day. Recently, the development of glass optical fibers has revolutionized the telecommunications industry, with fibers replacing copper wires and radically expanding our ability to transmit flaw-free data throughout the world.

Unlike many other materials, glasses are also esthetically pleasing to an extent which far transcends their mundane applications as drinking vessels and ashtrays, windows and beer bottles, and many other everyday uses. Why are we so delighted with a lead crystal chandelier or a fine crystal goblet? Why do we find glass sculptures in so many art museums? Why are the stained glass windows of the great cathedrals so entrancing? What aspects of objects made of glass make them so desirable for their beauty, as well as their more pragmatic uses?

The answers to these questions may lie in the ability of glasses to transmit light. Very few materials exist in nature which are transparent to visible light. Metals are opaque, as are virtually all natural organic materials. Many liquids are transparent, but they are transient in nature, without the enduring qualities we desire in our possessions. A list of the few transparent natural solids includes diamonds, emeralds, rubies, and many other precious and semi- precious stones. It is difficult to think of a naturally transparent solid which is not highly valued for its transparency and brilliance. Our heritage as humans would seem to provide a bias toward placing a high value on such objects. We are still fascinated by "bright, shiny objects."


What is a "glass"? The glasses used by mankind throughout most of our history have been based on silica. Is silica a required component of a glass? Since we can form an almost limitless number of inorganic glasses which do not contain silica, the answer is obviously, "No, silica is not a required component of a glass." Glasses are traditionally formed by cooling from a melt. Is melting a requirement for glass formation? No, we can form glasses by vapor deposition, by sol-gel processing of solutions, and by neutron irradiation of crystalline materials. Most traditional glasses are inorganic and non-metallic. We currently use a vast number of organic glasses. Metallic glasses are becoming more common with every passing year. Obviously the chemical nature of the material cannot be used to define a glass.

What, then, is required in the definition of a glass? All glasses found to date share two common characteristics. First, no glass has a long range, periodic atomic arrangement. And even more importantly, every glass exhibits time-dependent glass transformation behavior. This behavior occurs over a temperature range known as the glass transformation region. A glass can thus be defined as "an amorphous solid completely lacking in long range, periodic atomic structure, and exhibiting a region of glass transformation behavior." Any material, inorganic, organic, or metallic, formed by any technique, which exhibits glass transformation behavior is a glass.


We have established that any material which exhibits glass transformation behavior is a glass. What, then, is glass transformation behavior? We traditionally discuss glass transformation behavior on the basis of either enthalpy or volume versus temperature diagrams, such as that shown in Figure 1.1; (this diagram will be discussed in considerably more detail in Chapter 6). Since enthalpy and volume behave in a similar fashion, the choice of the ordinate is somewhat arbitrary. In either case, we can envision a small volume of a liquid at a temperature well above the melting temperature of that substance. As we cool the liquid, the atomic structure of the melt will gradually change and will be characteristic of the exact temperature at which the melt is held. Cooling to any temperature below the melting temperature of the crystal would normally result in the conversion of the material to the crystalline state, with the formation of a long range, periodic atomic arrangement. If this occurs, the enthalpy will decrease abruptly to the value appropriate for the crystal. Continued cooling of the crystal will result in a further decrease in enthalpy due to the heat capacity of the crystal.

If the liquid can be cooled below the melting temperature of the crystal without crystallization, a supercooled liquid is obtained. The structure of the liquid continues to rearrange as the temperature decreases, but there is no abrupt decrease in enthalpy due to discontinuous structural rearrangement. As the liquid is cooled further, the viscosity increases. This increase in viscosity eventually becomes so great that the atoms can no longer completely rearrange to the equilibrium liquid structure, during the time allowed by the experiment. The structure begins to lag behind that which would be present if sufficient time were allowed to reach equilibrium. The enthalpy begins to deviate from the equilibrium line, following a curve of gradually decreasing slope, until it eventually becomes determined by the heat capacity of the frozen liquid, i.e., the viscosity becomes so great that the structure of the liquid becomes fixed and is no longer temperature-dependent. The temperature region lying between the limits where the enthalpy is that of the equilibrium liquid and that of the frozen solid, is known as the glass transformation region. The frozen liquid is now a glass.

Since the temperature where the enthalpy departs from the equilibrium curve is controlled by the viscosity of the liquid, i.e., by kinetic factors, use of a slower cooling rate will allow the enthalpy to follow the equilibrium curve to a lower temperature. The glass transformation region will shift to lower temperatures and the formation of a completely frozen liquid, or glass, will not occur until a lower temperature. The glass obtained will have a lower enthalpy than that obtained using a faster cooling rate. The atomic arrangement will be that characteristic of the equilibrium liquid at a lower temperature than that of the more rapidly cooled glass.

Although the glass transformation actually occurs over a temperature range, it is convenient to define a term which allows us to express the difference in thermal history between these two glasses. If we extrapolate the glass and supercooled liquid lines, they intersect at a temperature defined as the fictive temperature. The structure of the glass is considered to be that of the equilibrium liquid at the fictive temperature. Although the fictive temperature concept is not a completely satisfactory method for characterizing the thermal history of glasses, it does provide a useful parameter for discussion of the effect of changes in cooling rate on glass structure and properties. The changes that occur in the fictive temperature, and the properties of glasses with subsequent reheating into the glass transformation region will be discussed in detail in Chapter 6.

Finally, we need to define a term, which, while commonly used, has only a vague scientific meaning. As indicated above, the glass transformation occurs over a range of temperatures and cannot be characterized by any single temperature. It is, however, convenient to be able to use just such a single temperature as an indication of the onset of the glass transformation region during heating of a glass. This temperature, which is termed either the glass transformation temperature, or the glass transition temperature, (Tg), is rather vaguely defined by changes in either thermal analysis curves or thermal expansion curves. The values obtained from these two methods, while similar, are not identical. The value obtained for Tg is also a function of the heating rate used to produce these curves. Since Tg is a function of both the experimental method used for the measurement and the heating rate used in that measurement, it cannot be considered to be a true property of the glass. We can, however, think of Tg as a useful indicator of the approximate temperature where the supercooled liquid converts to a solid on cooling, or, conversely, of which the solid begins to behave as a viscoelastic solid on heating. The utility of the concept of a glass transformation temperature will become much clearer in the following chapters.


1. Draw a volume/enthalpy diagram showing the behavior of a melt which cools to form (a) glass and (b) crystals. Label each section of this diagram. Show the curves for rapidly- and slowly-cooled melts.


Principles of Glass Formation


The earliest glasses used by man were found in nature. The ease of formation of sharp edges on obsidians, for example, allowed the production of knives, arrow heads, and other cutting tools. These naturally occurring glasses, which result from the cooling of molten rock, or lava, contain a wide variety of components, including alkali, alkaline earths, and transition metal oxides. In every case, however, silica is found to be the major constituent of these materials.

Since naturally occurring glasses proved to be so useful to early man, it is not surprising that the desire to produce glasses at will developed thousands of years ago. Furthermore, since all known glasses were silicates, it is also not surprising to find that the earliest man-made glasses were also silicates. In fact, very few non-silicate glasses were known prior to 1900. As a result, the first theories advanced to explain why some materials form glasses while others do not, were based heavily on the existing knowledge of the behavior of silicate melts and the structure of silicate crystals. These theories tend to assume that some unique feature of certain melts leads to glass formation for those materials, while the lack of these features prevents the formation of glasses from other materials. These theories are often grouped under the heading of Structural Theories of Glass Formation.

In recent years, we have recognized the existence of a vast number of non-silicate glasses. In fact, we now know that polymers and metals can also readily be formed as glasses, as can a large number of non-oxide, inorganic compositions. We now recognize that virtually any material can be formed as a glass. Theories of glass formation no longer address the question of why a specific material will form a glass, but rather "what do I have to do to make this material form a glass?" Since the emphasis has shifted from control of glass formation by selection of materials, to control of glass formation by changes in processing, the importance of kinetics has become obvious. As a result, a new approach to glass formation, known as the Kinetic Theory of Glass Formation, has largely replaced the earlier structural theories.


Perhaps the earliest, and simplest, theory of glass formation was based on the observation by Goldschmidt that glasses of the general formula RnOm form most easily when the ionic radius ratio of the cation, R, to the oxygen ion lies in the range 0.2 to 0.4. Since radius ratios in this range tend to produce cations surrounded by four oxygen ions in the form of tetrahedra, Goldschmidt believed that only melts containing tetrahedrally-coordinated cations form glasses during cooling. This contention was purely empirical, with no attempt to explain why tetrahedral coordination should be so favorable to glass formation.

A few years later, Zachariasen published a paper which extended the ideas of Goldschmidt and attempted to explain why certain coordination numbers might favor glass formation. Although intended only as an explanation for glass formation, this paper has become the basis for the most widely used models for glass structures, and is probably the most frequently cited (and misquoted) paper in the inorganic glass literature. Essentially, Zachariasen noted that the silicate crystals which readily form glasses instead of recrystallizing after melting and cooling, have network, as opposed to close-packed, structures. These networks consist of tetrahedra connected at all four corners, just as in the corresponding crystals, but the networks are not periodic and symmetrical as in crystals. These networks extend in all three dimensions, such that the average behavior in all directions is the same, i.e., the properties of glasses are isotropic. Zachariasen contends that the ability to form such networks thus provides the ultimate condition for glass formation.

After establishing that the formation of a vitreous network is necessary for glass formation, Zachariasen considered the structural arrangements which could produce such a network. First, he contends that no oxygen atom can be linked to more than two network cations. Higher coordination numbers for the oxygen cations prevent the variations in cation–oxygen–cation bond angles necessary to form a non-periodic network. Zachariasen further noted that the only glasses known at the time of his work contain network cations in either triangular (B2O3) or tetrahedral (silicates, GeO2, P2O5) coordination. He then generalized this observation by stating that the number of oxygen atoms surrounding the network cation must be small, specifically either 3 or 4. Zachariasen clearly states that this requirement is empirical and is based solely on the lack of knowledge of any glasses in which the coordination number of the network cation is neither 3 nor 4. The formation of a network in which the cations are located as far apart as possible, further requires that the oxygen polyhedra be connected only at the corners and do not share either edges or faces. Finally, he states that the network can only be 3-dimensional if at least three corners of each oxygen polyhedron are shared.


Excerpted from Introduction to Glass Science and Technology by James E. Shelby. Copyright © 2005 The Royal Society of Chemistry. Excerpted by permission of The Royal Society of Chemistry.
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Table of Contents

Introduction; Principles of Glass Formation; Glass Melting; Immiscibility/Phase Separation; Structure of Glasses; Viscosity of Glassforming Melts; Density and Thermal Expansion; Transport Properties; Mechanical Properties; Optical Properties; Glass Technology; Bibliography; Subject Index.

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Introduction to Glass Science and Technology 4 out of 5 based on 0 ratings. 1 reviews.
Dr_Science More than 1 year ago
Professor Shelby has written an excellent intro to glass science. It covers many practical aspects of glass chemistry, formation and melting. It contains chapters on unique chemistries such as borate glasses, which are covered in no other book that I know of. It also has very good coverage of ionic conduction in several glass systems. Much of the research covered in the book is based on work done at Alfred University. My one complaint is that no references are given, so it is hard to look up the original papers on which the book is based.