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Upon the completion of this unit, the students will be aware of the earth’s atmosphere, how our planet preserves itself, and some of the current problems that they will have to start confronting in order to provide a safe environment for themselves and their families. Hopefully, they will become advocates of current environmental issues and force their parents and other adults to realize that we all must do our part in helping to save our planet.
The curriculum unit, “Environmental Studies: An Approach to Educate and Save Our Planet”, will include the following components:
I. Introduction to Environmental Studies
II. The Greenhouse Effect and Its Gases
- (A) The Four Major Layers of the Earth’s Atmosphere
- ____(1) Troposphere
- ____(2) Stratosphere
- ____(3) Mesosphere
- ____(4) Thermosphere
- ________(a) Ionosphere
- ________(b) Exosphere
- (B) The Heating of the Earth’s Atmosphere
- (C) Examples of Natural Cycles Which Occur on Our Planet
- ____(1) The Carbon Cycle
- ____(2) The Nitrogen Cycle
- ____3) The Water Cycle
III. The Acid Rain Controversy
I plan to include as many scientific investigations as possible in my lesson plans so that the students can witness that the environmental problems presented within this unit actually exist, and that they should be concerned about them. Therefore, the focal point of my lesson plans will be geared towards “hands-on” experiences in order to reinforce the objects and concepts which are presented within this curriculum.
Planet Earth is enclosed or surrounded by a mixture of invisible gases called atmosphere. Nitrogen (N) and oxygen (O) alone make up approximately 97 percent of the gaseous mixture of air. Other gases such as argon, carbon dioxide, neon, helium, krypton, hydrogen and xeon make up the remaining one percent. Since these gases make up such a small component of air, they are know as trace gases.
Scientist measure trace gases in units called parts per million or ppm rather than by percentage. For example, neon makes up about .0018 percent of air. But scientists find it much easier to express that number as 18 parts per million, or 18 ppm. This means that in a sample of one million molecules of air, eighteen of the molecules are neon. The chart below will express the percentage that each gas makes up in the composition of air.
|GAS||PERCENTAGE IN DRY AIR|
In addition to the large amounts of water vapor, the troposphere also houses gas and dust particles. As the sunlight passes through the atmosphere, especially the troposphere, it is broken down into spectrum and gives the sky its color. Therefore, white light is broken down into its basic colors- violet, blue, yellow and red. Different particles within the atmosphere scatter different colors. The blue and violet colors of the spectrum are usually scattered more than the yellow and red colors. The sky appears to be blue because the blue and violet rays are reflected into our line of vision. If large particles of dust, smoke, or fog are present, the red and yellow colors scatter just as much as the blue and violet color causing the sky to appear white.
Immediately following a rainstorm usually a natural spectrum of light known as a rainbow may appear in the sky. Rainbows are caused by the separation of sunlight into a range of colors. In this case, rain drops are the means of separation. Bending and reflection of light rays in the falling raindrops separate each separate each ray of white light into a spectrum of colors.
Another characteristic of the troposphere is that its temperature drops as it goes higher. The troposphere’s temperature drops about 6.5 degrees Celsius for every kilometer in which one travels from the earth’s surface. However, after about 12 kilometers above the earth’s surface the temperature seems to stop dropping. The zone at which the temperature starts to remain constant is called the tropopause. It divides the troposphere from the next layer of the atmosphere.
The stratosphere also contains the ozone layer which protects all living things on earth by shielding them from harmful forms of radiation that comes from the sun. Ozone is a pale blue gas that is composed of three oxygen atoms combined together. High concentrations of ozone can be poisonous to all living things. Near the earth’s surface ozone can act as a pollutant in the air.
Ozone in the upper layer of the stratosphere is also responsible for the temperature increase in this area because it has the ability to absorb radiant energy. Radiant energy is the energy that moves in waves, such as visible, invisible light and ultraviolet radiation. If the ozone gas did not absorb most of the radiant energy, our skin would burn and we would loose our eyesight or vision. The small amounts of ultraviolet radiation that reach the earth’s surface causes sunburn and suntans. Too much ultraviolet energy may cause skin cancer.
The temperatures in the lower part of the stratosphere remain constant, while the temperatures in the upper part increase as one moves away from the earth’s surface. The place where the temperature is the highest is called the stratopause. The stratopause separates the stratosphere from the next layer of the atmosphere.
The mesosphere aids in protecting the earth from being struck by large rocklike materials in space called meteoroids. When meteoroids enter the atmosphere, they burn up in the mesosphere. The burning is caused by the friction between the meteoroid and the atmosphere. When this process occurs it can be seen the sky at night as a streak of light flashing across the sky. It is often referred to as a meteor in the sky. The majority of meteoroids usually burn completely, but sometimes a few pieces actually hit the earth’s surface. These pieces are called meteorites. When artificial satellites fall from orbit, they also burn up when they reach the earth’s atmosphere. However, a few pieces of the United States’ Skylab and Russia’s Cosmos reached the earth’s surface.
(A) The Ionosphere
The lower part of the thermosphere is referred to as the ionosphere. It extends from 80 kilometers to 550 kilometers above the earth’s surface. The actual size of the ionosphere depends upon the number of ultraviolet rays and x-rays given off by the sun on a given day.
The ionosphere contains oxygen, nitrogen oxide, and other gas particles which absorb the ultraviolet rays and x-rays from the sun. These particles then become electrically charged and are called ions. Ions are atoms that have either gained or lost electrons, the negatively charged parts of an atom.
The ions located within the ionosphere are important to radio communication. Radio waves bounce off the ions in the ionosphere and return to the earth’s surface thus allowing radio messages to be sent over great distances.
(B) The Exosphere
The upper region of the thermosphere is called the ionosphere. The exosphere is thousands of kilometers from the surface of the earth. Air within this region of the atmosphere is so thin that particles can travel great distances without hitting each other. Artificial satellites orbit the earth within this region. Satellites are important to people because they allow us to view events that occur all over the world through television, communicate through telephones and other types of technology, and take pictures of other planets, etc.
Only infrared waves with wavelengths between seven to thirteen micrometers can easily pass through the atmosphere and out into space. Infrared waves possessing this characteristic are referred to as “windows” because they pass through the earth’s atmosphere as if there is nothing in its path. As the atmospheric gases absorbs the infrared energy’s waves, it becomes warmer and gives off infrared energy into the atmosphere. Dust within the environment, along with clouds, scatter some light back to space. Even though small amounts of carbon dioxide and water vapor absorb the infrared waves, the majority of the energy is absorbed by vegetation, rocks and water. Carbon dioxide and water vapor in the air absorb the infrared waves. This results in the trapping of heat energy in the low part of the earth’s atmosphere. The trapping of heat in the lowest layer of the atmosphere is referred to as the “greenhouse effect”.
Now that the students are introduced to the interaction of the four major layers of the atmosphere that surround planet earth, they realize that they do utilize the atmosphere in some manner and the atmosphere itself does interact with. However, I would like to focus mainly on the tropospheric layer because it houses the air we breathe and planet earth which provides us with our means of survival.
Our civilization has made insurmountable gains technologically. However, through our eagerness to invent more, produce more, and gain new height; we fail to reflect -until recently- on how we are affecting our means of survival.
Finally we are realizing the necessity of the need to recycle. Children also should be introduced to the fact that planet earth naturally recycles the elements that we need in order to survive. This can be seen through several of the natural cycles that I will present to you within this section of the paper. I will briefly describe just a few of these cycles including the carbon, nitrogen, and water cycles. We must keep in mind that a cycle has no true beginning or end but it continues to repeat itself over and over again.
Both producers and consumers discard their carbon-bearing wastes and at some point in their life die, leaving their remains on earth in the form of carbon compounds. The saprovores complete the process of releasing the carbon (in the form of carbon dioxide) from such wastes and dead bodies. Most of these final consumers, the saprovores, are microorganisms though some, such as the toadstool, are visible to the naked eye.
The process carried on by the saprovores is extremely slow. Over millions of years large masses or carbon compounds may accumulate in the earth as peat, coal, and petroleum. Some organisms also sidetrack carbon into shells that are deposited as rock. However, the main pathway in the carbon cycle is from the earth’s atmosphere or waters into living things and the process starts all over again.
All consumers get nitrogen-containing compounds in the things they eat and all foods can be traced back to the producer. Producers get their nitrogen-bearing compounds for the soil or water in which they grow. Nitrogen gas is present in the soil, dissolved in water. Living in the soil or in the roots of certain plants are nitrogen-fixing bacteria. They convert nitrogen to a form they or other organisms can use. Nitrogen fixers convert nitrogen gas to ammonia, which can be used to synthesized proteins and other nitrogen-containing compounds.
Decomposers in the soil breaks down the complex organic compounds in dead plant and animal bodies. They use the energy in those compounds and convert them to simpler substances. The main nitrogen containing substance is ammonia. Ammonia is a gas, and some of it escapes into the atmosphere. However, it also dissolves immediately in water. In watered soil, ammonia reacts chemically with hydrogen ions to form ammonia ions which is absorbed by the roots of plants. It is then built into living material again by plants. The nitrogen gas gradually escapes back into the atmosphere, and the cycle of nitrogen is complete.
During a rain storm, some of the rainwater evaporates as it falls to the ground. But most of the rainwater runs along the surface of the ground and travels to rivers, streams and ponds. The water running along theses surfaces are known as runoff water. Large amounts of precipitation also enter the soil to become ground water. The warm air that rises through the atmosphere contains tiny droplets of water. This water cools as it climbs higher into the atmosphere causing the water vapor to condense into droplets of water which form clouds. The droplets collect to form drops that eventually fall from the clouds as rain. If the water vapor condenses at a temperature below the freezing point of water then snow is formed.
Ground water is also a part of the water cycle. The ground holds and receives water from precipitation. However, some of the water moves downward into subsoil and fills the spaces around the rock particles. In the upper level of the soil, where it is saturated with water, the water will run off the surface instead of penetrating into the soil. The depth of the water table depends on the amount of precipitation, the nature of the rock layer under the soil, the proximity of large bodies of water, and the conditions of the soil receiving water.
Land organisms may pick up water at various points in this cycle. Most commonly, land animals get their water by drinking, and the plants by absorbing it from the soil. In all organisms some water becomes chemically incorporated into living substances, later to reappear when the substances are broken down. Furthermore, all organism contain water in which most of the living processes take place. Thus water is always involved both in the structure and in the activities of living things.
On land, both plants and animals lose water to the atmosphere: in plants, largely from the leaves; in animals through breathing or evaporation from the skin. Still more water is released when animals discharge wastes. Eventually all water taken in by organisms return to the atmosphere.
These are just a few of the cycles that exist within nature. I will now focus on two of the many environmental crises that exist on our planet- the greenhouse effect and acid rain. I will attempt to explain what these concepts are and state the problems that they are creating on our planet. I will also list some of the ways in which we can help in preventing these processes from destroying our planet.
Next to carbon dioxide, methane gas is the second most important greenhouse gas. Even though there is far less methane in the air than carbon dioxide, a methane molecule absorbs twenty times more infrared rediation than one molecule of carbon dioxide. Methane is produced by several natural sources such as cattle, termites, and microorganisms that live in waterlogged soils. The burning of grasslands and rainforests also contributes to the methane in the air because it causes the soil microorganisms to increase their methane-producing activities.
Nitrous oxide is another greenhouse gas that is becoming more abundant in our atmosphere. It is a colorless gas known to most people as laughing gas. Nitrous oxide is released into the atmosphere through automobile exhaust, the burning of fossil fuels, and through farmers spreading nitrogen fertilizer on open fields. As these fertilizers break down into the soil, nitrous oxide is released into the air.
Scientists have analyzed air trapped in ice cores and found that the atmospheric concentration of nitrous oxide was about 0.20 ppm around the year 1900. However eighty years later they found that the atmospheric concentration of nitrous oxide had increased to 3.0 ppm. This may not seem alarming, but nitrous oxide has the potential to stay in the troposphere anywhere from 120 to 175 years before moving into the stratosphere. Therefore, the gas nitrous oxide has the potential to become extremely abundant in our atmosphere since we place an additional five million tons of this gas into our environment each year.
CFCs are used as a coolant in air conditioners and refrigerators. They are also used to clean computer chips, electronic circuit boards, and even to sterilize medical equipment. Chlorofluorocarbons are used as propellants in spray cans. They play a major role in the production of all plastic foam products.
Chlorofluorocarbons rise very slowly into the atmosphere. They have the ability to stay in the troposphere unchanged for seventy to one hundred fifty years. Once CFCs enter the stratosphere, they collide with the ultraviolet radiation released by the sun. The ultraviolet radiation reacts with the CFCs by breaking apart the molecules of CFCs to form chlorine. The chlorine atoms combines with ozone which aids in its depletion. One chlorine atom can destroy 100,000 molecules of ozone.
CFCs also have the ability to absorb ultraviolet radiation released from the sun. One molecule of CFC-11 has the same heat-trapping ability as ten thousand molecules of carbon dioxide. Since CFCs remain in our environment for such a long period of time, they can be extremely detrimental in the greenhouse effect.
Researchers have become concerned about the increases in chlorofluorocarbons, and the other greenhouse gases previously mentioned because they do not absorb infrared radiation with wavelengths between seven and thirteen micrometers. Thus, additional heat energy is trapped in the troposphere that would normally pass through. Therefore, the trapped heat energy lingers in the atmosphere causing the window to become dirty and trap even more heat into the earth’s atmosphere.
Energy conservation is the best method to reduce the buildup of carbon dioxide in the atmosphere. The average coal-fired plant adds over one million tons of carbon dioxide to the air annually. A car will ass at least its own weight in carbon dioxide to the atmosphere each year. This alone demonstrates that we need to change our attitudes and the way we live in order to aid in saving planet earth.
Some suggestive methods of saving energy could include the following, and I’m sure that you can make additions to the list: (a) use energy-efficient home appliances (b) weatherize and insulate your homes (c) reduce the amount of hot water usage (d) use alternative energy sources such as solar power (e) monitor television, radio and stereo usage (f) carpool and use mass transportation as much as possible (g) use recyclable products, etc. (h) plant trees (i) use nonchlorofluorocarbonated products.
Before discussing acid rain, we must first become acquainted with the pH scale. The pH scale is used to measure the degree of acidity or alkalinity of a solution. The scale ranges from 0 to 14, with the value of 7 representing that a solution is neutral. Values below 7 indicate greater acidity and numbers above 7 indicate greater alkalinity. The pH scale is logarithmic, meaning that each whole number indicates a ten-fold difference. Until recently it was believed that unpolluted rain naturally has a pH of about 5.6. However, studies in uncontaminated remote areas have shown that precipitation usually has a pH closer to 5. Unfortunately, in most areas within several hundred kilometers of large centers of human activity, precipitation has much lower pH values. Rain, or precipitation with these values is termed acid rain.
The best known effect of acid rain is the lowering of pH in thousands of lakes in Scandinavia, Canada, and the northeastern United States. As the pH drops, the organisms that live in or near lakes and streams are affected. Accompanying the lower pH have been a substantial increase in dissolved aluminum, which is leached from the soil by the acidic waters. This increase of dissolved aluminum is toxic to fish and wildlife. As a consequence, some lakes are devoid of fish while others are approaching this condition.
The effects of acid rain on lakes varies from one lake to another. These variations is related to the nature of the soil and rock materials surrounding the lake. Minerals such as calcite in some rocks and soils can neutralize acid solutions which would keep the lakes from becoming acidic. However, over a certain period of time, the pH of lakes that have not yet been acidified may drop as the buffering material in the surrounding rocks and soil become depleted. Lakes that lack the buffering materials such as calcite and limestone are more likely to be or become acidic.
Lakes at high altitudes are particularly sensitive to acid rain. Only about 5 or 10% of the water in a lake comes from precipitation that has directly fallen on lakes; the vast majority of water is from rain that has fallen on the surrounding watershed and run off into the lakes. Meaning that most of the water in a lake has had an opportunity to be neutralized by soil. However, lakes at a higher altitudes are often located in rocky outcropping, and comprise a large fraction of their whole watershed. In some cases the rainwater runs uninterrupted over a few bare rocks, directly into the lake. The problem is multiplied during the winter and spring when a carpet of snow or ice prevents rain and melted water from contacting the ground at all before running into a lake. In this case the lake receives a surge of acidic waters which can kill fish and other aquatic life outright.
There has been recent evidence to show that acid rain may be responsible for the widespread decline in the growth of evergreen forests in the eastern United States and Western Europe during the past decades. Acid rain has caused such severe damage to the forest in Germany that they have taken major action to reduce sulfur dioxide emissions.
Laboratory and field studies have shown that acid deposition can have the following effects on forest: (1) damage leaves, roots and microorganisms that form beneficial symbiotic association with roots; (2) decrease a plant’s resistance to other forms of stress, including climate, insects, and pathogens; (3) leach nutrients such as calcium and magnesium from soils; (4) dissolve metals in the soil such as aluminum at levels potentially toxic to plants; and (5) impair reproduction and the survival of seedlings.
The following actions will result in lowering the emission of deadly chemicals such as sulfur dioxide and nitrous oxide into the air, and in turn reduce acid rain: (a) use energy-efficient appliances (b) purchase products made from recycled materials because they take less energy to make. (c) purchase fuel-efficient cars (d) use compact fluorescent energy efficient light bulbs (e) minimize the use of automobiles by walking, carpooling, bicycling (f) use mass transportation as much as possible.
- MATERIALS NEEDED: Two cardboard shoe boxes with lids, scissors, clear plastic wrap transparent tape, two thermometers, compass
- PROCEDURES: (1) Use scissors to cut out a rectangular hole in one side of each of the two shoe boxes. Cover the hole in each box with a piece of clear plastic wrap. Use transparent tape to attach the plastic wrap. (2) Place a thermometer inside each box and put the lids on. (3) Take the boxes outdoors on a sunny day. They represent buildings that receive solar energy. Use a compass to find north and south. Place one box so that its “window” faces south. Place the other box so that its “window” faces north. (4) Open the boxes and check the temperature in each box. Record these numbers as the starting temperature in your chart. Now close the boxes. Predict how the temperatures in the two boxes will change during the next forty minutes. (5) Every ten minutes, for the next forty minutes, record in your chart the temperatures inside each box.
- RESULTS (1) In which box was the final temperature greater? (2) Make a graph showing how the temperature in each box changed.
- THE GREENHOUSE EFFECT
- MATERIALS NEEDED: three glass saucers, water, thermometer
- PROCEDURES: (1) Take two glass saucers and place them in the sun. (2) Pour the same amount of water straight from the faucet. (3) Measure the temperature of the water, and record the temperature. (4) Cover one of the saucers with another saucer. (5) Measure the temperature every ten minutes in each saucer and record the temperatures. (6) Depict you data on a line graph.
- RESULTS: (1) Which saucer had the highest temperature? (2) How does this experiment demonstrate the greenhouse effect?
- WHAT DOES NATURE RECYCLE
- MATERIALS NEEDED: plastic shoe box, small rock, enough soil to fill the shoebox, scissors, newspaper, a stick about 25 cm long, assorted liter- including plastic bag, polystrene foam, leaves, food scraps, aluminum foil, small piece of glass
- PROCEDURES: (1) Place enough soil in the box until it is about one-third full. (2) Cut, crush, tear, of break the litter into small pieces. (3) Scatter the litter over the soil. (4) Cover the litter with soil until the pot is almost full. (5) Sprinkle the soil with water until it is thoroughly dampened but not completely soaked. (6) Place the plastic shoebox in a warm dark place. (7) Check the soil in the box regularly and add water as needed to keep it moist. (8) After about four weeks, empty the contents of the plastic shoebox onto open sheets of newspaper. (9) Use a platic ruler to spread the contents of the litter box over the newspaper. (10) Carefully observe and record the contents of the soil.
- RESULTS: (1) Which materials decomposed and which did not? (2) What does nature recycle? (3) Compare your plastic box to a landfill (the students should be allowed to go to the library to find any necessary information).
- THE CARBON-OXYGEN CYCLE
- MATERIALS NEEDED: living fresh-water snails, several sprigs of elodea (or other suitable aquatic plant), three test tubes, stoppers to fit the test tubes, test tube rack, glass-marking pencil, pond or aquarium water to put in test tubes
- PROCEDURES: (1) Mark three test tubes one, two and three with a glassmarking pencil. (2) Fill each test tube three-quarters full of pond water or aquarium water. (3) Place a snail in tube one and place the stopper in the test tube. (4) Place a snail and two or more sprigs of elodea in test tube marked number two and close with a stopper. (5) Place an equal amount of elodea in the third test tube and close with a stopper. (6) Examime the tubes daily for five consecutive days and record observations.
- RESULTS: As you examine the tubes, record your observations on the based on the following criteria: (A) Is the snail alive? If so, is it active, e.g., moving on the side of the tube, feeding on the elodea leaves, etc . . . (B) Does the elodea appear to be growing, or is there evidence that it is unhealthy or dying? (C) What is the condition of the water? Is it clear or cloudy (turbid), indicating decomposition of plant or animal substances? Record the observations you make each day on a chart or table.
(B) Determining the pH of Pond Water and Rain Water Samples
- MATERIALS NEEDED: red cabbage leaves, a heat source, water, 250 ml beaker
- PROCEDURES: (1) Boil several red cabbage leaves in water until the mixture turns dark red. (2) Let the mixture cool for about 1 hour or let set for the remainder of the day.
- RESULTS: (1) What is the purpose of the indicator?
(C) Testing the pH of Soil Samples:
- MATERIALS NEEDED: jars or beakers, indicator (see above procedure to make indicator), samples of pond water collected from different ponds, samples of rain water collected over a period of time
- PROCEDURES: (1) Assign students to collect pond water samples from different places in their community. Also tell students to collect and date rainwater samples whenever it rains. (2) Place 25ml of each sample in a labled beaker. (3) Test the rainwater and pond water samples with your indicator. (4) Record your results on a chart stating the color of the samples after adding two ml of indicator to your samples. (5) Use a ph chart to record the pH of each sample.
- RESULTS: (1) What is the pH of your rain water samples? (2) How does the pH of your rainwater compare to that of normal rainwater (pH 5.6)? (3) Give some possible reasons why your think your rainwater is or is not very acidic. (4) What is the pH of your pond water samples? (5) How does the pH of your pond water sample compare to that of a healthy pond? (6) Do you think that the pond water sample is too acidic, why?
- MATERIALS NEEDED: funnel, beaker, soil sample, water, heat source
- PROCEDURES: (1) Place filter paper in a funnel and fill the funnel with your soil samples. (2) Hold the end of the funnel over a small beaker and pour 100 ml of boiled distilled water through the soil; dirty water will collect in the beaker. (3) Place about 20 ml of indicator into the water sample and stir. Record the color change of the sample on a chart for each sample taken. (4) Determine and record the pH of the collected water from the siol sample.
- RESULTS: (1) What is the pH of the soil samples? (2) Consider the data on the pH of the rainwater of your area. In what way, if any, is this rainwater affecting the acidity of your soil?
Gould, Roy. Going Sour: Science and Politics of Acid Rain. Birkhauser Press: Boston, 1985. This book offers an in-depth account of the science and politics of acid rain. The author also present several case studies showing the devastating effects of acid rain.
Gray, Kathlyn. Acid Rain. Franklin Watts Publishing: London, 1983. This text examines the direct and indirect effects of acid rain, how it is formed and how it is being studied.
Hare, Tony. The Greenhouse Effect. Gloucester Press: New York, 1990. This book discusses all aspect of the greenhouse effect and how the earth is affected by it.
Hollender, Jeffrey. How to Make the World a Better Place: A Guide to Doing Good. Quill William Murrow: New York, 1990. The author presents over 120 specific actions that we can take to help save our planet. The text also lists several addresses and phone numbers where you can get additional information from environmental groups.
Javna, John. 50 Simple Things Kids Can Do To Save The Earth. Andrews and McMeel Press: Kansas, 1990. This text explains how specific things in a child’s environment to the rest of the world, and helps children to develop habits that are environmentally sound.
Johnson, Rebecca. The Greenhouse Effect: Life on a Warmer Planet. Lerner Publications Company: Minnesota, 1990. This text explains what the greenhouse effect is and what impact it may have on the planet. She also gives an account of what scientist thinks will happen.
Regens, James and Rycroft, Robert. The Acid Rain Controversy. University Press of Pittsburg: Pennsylvania, 1989. The author gives an indepth look at the acid rain controversy from a scientific, political and economic viewpoint.
Schwartz, Linda. Earth Book For Kids: Activities to Help Heal the Environment. The Learning Works, Incorporation: California, 1990. This text is designed to provide children and their parents with an array of factual information about current environmental issues. The book also contain a large amount of activities that families can do together in order to improve the environment.
Silverstein, Alvin, Virginia and Robert. Recycling: Meeting the Challenge of the Trash Crisis. G.P. Putnam’s and Son, New York, 1992. This text discusses the impact that the overabundance of garbage being generated by Americans, and introduce ways of generating less trash.
Simon, Seymour. Science Projects in Pollution. Holiday House: New York,1972. This book contains numerous amounts of scientific investigation dealing with air land and water pollution.
Weiss, Malcolm. Toxic Waste: Clean-Up or CoverUp? Moffa Press: New York, 1978. This text examines the issues surrounding the disposal of toxic waste. It also gives a brief history of how waste has been managed in the past. The author also details measures currently being taken to clean up toxic waste.
Contents of 1993 Volume V | Directory of Volumes | Index | Yale-New Haven Teachers Institute