Ozone Depletion Article
(from www.beyonddiscovery.org)
This article can be used with the ozone graphing exercise as additional information.
THE OZONE DEPLETION PHENOMENON
For four months of every year, Antarctica's McMurdo Research Station lies shrouded in darkness. Then the first rays of
light peek out over the horizon. Each day, the sun lingers in the sky just a little longer and the harsh polar winter slowly
gives way to spring.
Spring also brings another type of light to the Antarctic, a light that harms instead of nurtures. In this season of new
beginnings, the hole in the ozone layer reforms, allowing lethal ultraviolet radiation to stream through Earth's
atmosphere.
The hole lasts for only two months, but its timing could not be worse. Just as sunlight awakens activity in dormant plants
and animals, it also delivers a dose of harmful ultraviolet radiation. Spring also brings another type of light to the
Antarctic, a light that harms instead of nurtures. In this season of new beginnings, the hole in the ozone layer reforms,
allowing lethal ultraviolet radiation to stream through Earth's atmosphere.
After eight weeks, the hole leaves Antarctica, only to pass over more populated areas, including New Zealand and
Australia. This biologically damaging, high-energy radiation can cause skin cancer, injure eyes, harm the immune system,
and upset the fragile balance of an entire ecosystem.
Although, two decades ago, most scientists would have scoffed at the notion that industrial chemicals could destroy
ozone high up in the atmosphere, researchers now know that chlorine creates the hole by devouring ozone molecules.
Years of study on the ground, in aircraft, and from satellites has conclusively identified the source of the chlorine:
human-made chemicals called chlorofluorocarbons (CFCs) that have been used in spray cans, foam packaging, and
refrigeration materials.
EXPLORING EARTH'S ATMOSPHERE
Like many lines of scientific inquiry, research leading to the prediction and discovery of global ozone depletion and the
damaging effects of CFCs followed a path full of twists and turns. Investigators did not set out to determine whether
human activity affects our environment nor did they know much about chemical pollutants. Instead, they began with basic
questions about the nature of Earth's atmosphere--its composition, density, and temperature distribution.
The composition of our planet's atmosphere fascinated humans long before chemistry became a formal science. "The
storm thundered and lightened, and the air was filled with
sulfur," Homer wrote in the Odyssey, referring to the sharp odor, created during thunderstorms, of what later became
known as ozone.
By the late 1800s, atmospheric scientists had isolated carbon monoxide and inferred the existence of a second
combustible gas in the air, which they tentatively identified as methane, the simplest hydrocarbon. But in attempting to
further analyze the composition of the atmosphere, researchers at the turn of the century faced a major stumbling
block: virtually all gases, except for molecular nitrogen and oxygen, exist in such minute concentrations that available
equipment could not detect them.
Help, however, was on the way. During the 1880s, scientists had begun perfecting a new, highly precise method of
identifying a compound by recording a special kind of chemical fingerprint--the particular pattern of wavelengths of light
it emits or absorbs. Scientists call this pattern a spectrum.
In the 1920s, G.M.B. Dobson developed a spectrometer that could measure small concentrations of ozone. Soon,
scientists had the tools to detect other atmospheric gases that occur in concentrations one-tenth to one-hundredth as
great as that. By the 1950s, researchers had identified 14 atmospheric chemical constituents.
Such research spurred advances on two fronts: a substantial increase in the precision and accuracy of measurements of
atmospheric gases and a striking decrease in the minimum concentration of a compound that must be present to be
detected. As a result, the number of atmospheric compounds identified by scientists has increased from 14 in the early
1950s to more than 3,000 today. Detectors today routinely measure compounds at concentrations below one part per
trillion, and some can record gases that occur in concentrations one-thousandth as great at that.
Even in some of the most remote locations on Earth, scientists have detected hundreds of compounds. Curiously, some of
the substances that occur in the smallest concentrations rank as some of the biggest players in altering the atmosphere.
A case in point: the group of chemicals known as CFCs.
THE OUTCOME: POTENTIAL CATASTROPHE AVERTED
Painstaking research on ozone and the atmosphere over the past 40 years has led to a global ban on CFC production.
Since 1987, more than 150 countries have signed an international agreement, the Montreal Protocol, which called for a
phased reduction in the release of CFCs such that the yearly amount added to the atmosphere in 1999 would be half that
of 1986. Modifications of that treaty called for a complete ban on CFCs which began in January 1996. Even with this ban
in effect, chlorine from CFCs will continue to accumulate in the atmosphere for another decade. It may take until the
middle of the next century for ozone levels in the Antarctic to return to 1970s levels.
More globally, ozone depletion is expected to remain a fact of life for several decades to come, but thanks to the
research that led to early recognition of the problem and steps that have been taken to address it, the potential
consequences are much less severe than they otherwise would have been.
Scientists estimate, for example, that if active research in stratospheric chemistry had not been in place at the time
the ozone hole was discovered in 1985 and confirmed in 1986, global ozone depletion, measuring 4 percent today, would
be close to 10 percent by the year 2000. Even larger ozone depletion would have been observed over the United States
and Eastern Europe, substantially exceeding the current measurements there of about 10 percent loss in winter and
spring and 5 percent in summer and autumn. These larger losses have been avoided because basic research in the
atmospheric sciences had already advanced to a level where it was able to explain the chemical reactions occurring in the
ozone layer. That knowledge allowed other informed political and regulatory decisions to be made.
As lawmakers and the public face new challenges in the struggle to protect the environment, they will increasingly rely on
basic research to open new vistas and suggest new solutions about these pressing concerns.
CREDITS
This article was adapted by Ron Cowen from an article written by Dr. F. Sherwood Rowland for Beyond DiscoveryTM :The
Path from Research to Human Benefit, a project of the National Academy of Sciences. The Academy, located in
Washington, D.C., is a society of distinguished scholars engaged in scientific and engineering research, and dedicated to
the use of science and technology for the public welfare. For over a century, it has provided independent, objective
scientific advice to the nation
Analysis Questions
1. What is the purpose of the ozone layer?
2. How did this article demonstrate that science is a process, and that science depends on advances in technology?
3. What are the main ideas of this article?