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Colored Glass Chemistry
How Does It Work?
By Anne Marie Helmenstine, Ph.D.
Early glass derived its
color from impurities that were present when the glass was formed.
For example, 'black
bottle glass' was a dark brown or green glass, first produced in 17th Century
England.
This glass was dark due
to the effects of the iron impurities in the sand used to make the glass and
the sulfur from the smoke of the burning coal
used to melt the glass.
Man-made Glass Coloration
In addition to natural
impurities, glass is colored by purposely introducing minerals or purified
metal salts (pigments).
Examples of popular
colored glasses include ruby glass (invented in 1679, using gold chloride) and
uranium glass (invented in the 1830s, glass that glows in the dark, made using
uranium oxide).
Sometimes it is necessary
to remove unwanted color caused by impurities to make clear glass or to prepare
it for coloring.
Decolorizers are used to
precipitate out iron and sulfur compounds. Manganese dioxide and cerium
oxide are common decolorizers.
Special Effects
Many special effects can
be applied to glass to affect its color and overall appearance.
Iridescent glass,
sometimes called iris glass, is made by adding metallic compounds to the glass or by
spraying the surface with stannous chloride or lead chloride and reheating it in
a reducing atmosphere.
Ancient glasses appear
iridescent from the reflection of light off of many layers of weathering.
Dichroic glass is an
iridescent effect in which the glass appears to be different colors, depending
on the angle from which it is viewed.
This effect is caused by
applying very thin layers of colloidal metals (e.g., gold or silver) to the
glass. The thin layers are usually coated with clear glass to protect them from
wear or oxidation.
Glass
Pigments
Compounds
|
Colors
|
iron
oxides
|
greens,
browns
|
manganese
oxides
|
deep
amber, amethyst, decolorizer
|
cobalt
oxide
|
deep
blue
|
gold
chloride
|
ruby
red
|
selenium
compounds
|
reds
|
carbon
oxides
|
amber/brown
|
a
mix of manganese, cobalt, iron
|
black
|
antimony
oxides
|
white
|
uranium
oxides
|
yellow-green
(glows!)
|
sulfur
compounds
|
amber/brown
|
copper
compounds
|
light
blue, red
|
tin
compounds
|
white
|
lead
with antimony
|
yellow
|
Anne
Marie Helmenstine, Ph.D.
Chemistry
Expert
Education
Ph.D.,
Biomedical Sciences, University of Tennessee at Knoxville
B.A.,
Physics and Mathematics, Hastings College
Introduction
Ph.D.
in biomedical sciences from the University of Tennessee at Knoxville - Oak
Ridge National Laboratory.
Science
educator with experience teaching chemistry, biology, astronomy, and
physics at the high school, college, and graduate levels.
ThoughtCo
and About Education chemistry expert since 2001.
Widely-published
graphic artist, responsible for printable periodic tables and other
illustrations used in science.
Experience
Anne
Helmenstine, Ph.D. has covered chemistry for ThoughtCo and About Education
since 2001, and other sciences since 2013. She taught chemistry, biology,
astronomy, and physics at the high school, college, and graduate levels.
She has worked as a research scientist and also abstracting and indexing
diverse scientific literature for the Department of Energy.
In
addition to her work as a science writer, Dr. Helmenstine currently serves as a
scientific consultant, specializing in problems requiring an interdisciplinary
approach. Previously, she worked as a research scientist and college
professor.
Education
Dr.
Helmenstine holds a Ph.D. in biomedical sciences from the University of
Tennessee at Knoxville and a B.A. in physics and mathematics with a minor
in chemistry from Hastings College. In her doctoral work, Dr. Helmenstine
developed ultra-sensitive chemical detection and medical diagnostic tests.
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