Absorbent Spheres Help Students Soak Up Scientific Principles

March 14, 2012

by:  John Fedors

GROWING SPHERES

Hydrophilic spheres from Educational Innovations offer a variety of interesting applications and opportunities for scientific inquiry. They come in a variety of sizes: small, regular, jumbo, & gigantic. For the following examples, I prefer the regular or #710 size. However, whichever size you choose, they will expand to about 300 times their original dehydrated size. As they absorb the water, they become almost invisible, due to having the same refractive index as water. When placed in de-mineralized or distilled water and kept away from sunlight, they will dehydrate to their original size and can be re-used. Dehydration time will depend on air humidity.

Once enlarged, these clear spheres can be used to demonstrate:

* The lens of an eye (such as those of a shark, calf or sheep) that has the ability to magnify the print on a page. A thin slice may be used to mimic a cornea transplant.

* The suspension of small items such as a coin.

* Roots of a germinating seed.

Enlarged growing spheres can also help to observe the relationship of Surface Area (A=4pr2) to Volume (V=4/3pr3) mass in grams. They can be used to graph relationships.

Using dark vegetable dyes you can also relate to why living cells need to divide. The ratio of surface area to cell volume does not permit timely diffusion of required metabolites in or out of the cell. This can be demonstrated by placing a dyed sphere in clear water for 10 minutes and measuring the clear area of the sphere in relation to the rest of darkened or dyed sphere.

My favorite though is the demonstration of cell organelles/microstructures in eukaryotic cells. In addition to the hydrophilic spheres, this demonstration requires serpent skin tubing. Serpent skin tubing is a crinkled cellulose dialysis tubing that stretches out, remains open and relatively sturdy. It eliminates the usual wetting difficulty in opening traditional dialysis tubing.

To demonstrate cell organelles/microstructures in eukaryotic cells you will need:

* Serpent Skin

* Small nut & bolt (to serve as weight)

* Twist Ties (used in grocery produce departments or with some trash bags)

* #710 Growing Spheres

* Tall glass

* Food Dye

* Distilled or de-mineralized water

Here’s what you do…

Take or cut a 6 to 8 inch length of Serpent Skin and flatten it. Fold it lengthwise 3 to 4 times, creating a long, narrow section. Fold the end up, then slide the folded end through the bolt. The bolt serves as a weight to keep the finished apparatus submerged in the dyed water. Use a twist tie between the bolt and then end of the tubing. I am a fan of the champagne twist – twist six times as you would see the wire is twisted on a champagne bottle top.

Place 25-35 Growing spheres through open end of the serpent skin and add 7-9 drops of dark vegetable dye to a tall glass. Add water to the glass up to an inch from the top or so. Place the weighted serpent skin with the growing spheres into the dyed water.

Results:

The dyed water will diffuse through serpent skin (cell membrane} and will cause the growing spheres to swell (this can take about 24 hours). The spheres will vary in size; larger spheres will collect towards the bottom of the glass while smaller spheres will collect towards the top. Adding more spheres initially will force them up and out. The varying sizes will help to visualize different organelles.

The dark stained organelles can be placed in clear colorless water for 5-10 minutes to demonstrate a colorless, clear outer surface area of diffusion. The spheres center will stay dark even after several water changes.

This also demonstrates the relationship of surface area to organelles volume and the need for the organelles to remain small for efficiency of passive diffusion.


Who Knew They Could Be So Dense?

January 3, 2012

by:  Tami O’Connor

Density is not typically an easy concept for most middle school students and even more difficult for younger students, but it doesn’t need to be.  We all know that D=m/V, but the easiest way I found to explain it to my students was to have them visualize a common dilemma in my home immediately preceding a vacation.  For years, as a poor starving teacher, I only had one suitcase, and it was actually a hand-me-down from my mother.  It was a medium sized Samsonite, hard cased piece of luggage.  When approaching the topic of density in my classroom, down from the attic it came.

My explanation began with an imaginary weeklong summer vacation to a low-key resort.  The class and I would brainstorm the items I needed to pack for my trip.  Generally, the list included items such as a few bathing suits, shorts, t-shirts, a pair of flip flops, some PJs, underwear and a few toiletries.  It was obvious by looking at the size of my suitcase that in addition to my meager belongings, I could have probably also fit one of my students in my bag…  ok, perhaps one of the smaller kids.

I explained that when I closed the suitcase, it was hard to see, simply by looking at it, how heavy it was.  The lesson didn’t stop there.  We now planned my one-week ski vacation to Vermont during the February break.  Once again, my students and I made up my pack list.  The list included a couple of heavy sweaters, long johns, gloves, a hat, boots… as you can imagine, the list went on and on.  The question was, where to put it all.  Of course, since I had only one suitcase, the answer was easy.

I would explain that the night before my winter trips, I could usually be found sitting on top of my very over-stuffed suitcase trying to close the latches!  I was always a little concerned that if the latch broke, my suitcase would explode and my belongings would be everywhere!  That always elicited a round of giggles as my kids visualized that catastrophe!  The interesting point was that once my suitcase was closed and latched, there was no way to determine how heavy it was just by looking at it.  Here it is… density in a suitcase!

The volume or size of my hard-sided suitcase never changed; however, the mass, or all the stuff inside each suitcase I packed was dramatically different.  This is when we started explaining more of the science of density.  The more tightly packed the molecules in an object are, the denser it is.

My next prop included two identical cardboard boxes.  The first had about eight bricks inside and the second was empty.  Without telling my class what to expect, I would ask for a volunteer to lift the box with the bricks.  After a bit of a struggle, the box would slowly rise above the table.  The other students could clearly see that the box was obviously very heavy.  I would then ask the same student to lift the second box.  Without fail, this box was hoisted so high that it almost flew out of the student’s hands!  Once again, we had two objects with basically the same volume but with drastically different masses.

My next question was: suppose my boxes were waterproof?  If I dropped them into the ocean, what would happen?  School aged kids all understand the concept of floating and sinking, so the obvious answer was that the box with the bricks would sink while the empty box would float.  I would explain that the bricks are denser than water, and that is why they sink. The air that filled the lighter box was less dense than the water, however, and therefore it would float.

In the next demonstration, I found two stainless steel spheres from Educational Innovations.  One was small and solid and the other one was much larger and hollow.  I would pass these around the classroom and asked the students to tell me which one had more mass (or was heavier).  Another unanimous answer:  the small, solid sphere was heavier.

Next, I would find another volunteer and blindfold my victim… I mean, my student.  I would then take two identical baskets, paper plates, or small plastic bowls and put each sphere in so they didn’t roll around.  I would ask my student to hold out his or her hands and would then place one plate in each hand and ask which was heavier…  Since both spheres are basically the same mass, the answer did not come as quickly as it did before the mass was spread out along a greater distance.  This was a perfect segue into the next unit on pressure.  But that would have to wait a week or two…

Of course, the observers in class were chomping at the bit to try the blindfold test.  Talk about active learning and a discrepant event!  Now that the class believed that both spheres were the same mass, I pulled out the large glass bowl filled with water, and I would ask my students to predict, based on the fact that we know that both sphere have the same mass, what would happen when I placed each sphere into the water.

This was amazing because, had I asked prior to blindfolding them, every student would have accurately predicted that the small sphere would sink, and the large one would float.  Now, a heated discussion usually ensued.  At this point, the mathematical formula was revealed (D=m/V).  When the mass increases and the volume remains the same, like the example of my luggage or the boxes with the bricks, the density increases.  At the same time, when the mass remains the same but the volume increases (like the small sphere vs. the large one) the density decreases.  Depending on the grade level I was working with. I would substitute simple numbers in the equation to show how changing the mass and volume affected the density.

Now, back to the discussion of floating and sinking spheres… After the explanation of how volume and mass affect density, most, if not all of my students agreed that the small sphere, being very dense, would sink, while the larger, lighter sphere would float.  Another successful seventh grade lesson!


101 Things Everyone Should Know About Science

November 26, 2011

by:  Dia Michels

Science affects everything—yet so many of us wish we understood it better. Using an accessible question-and- answer format, 101 Things Everyone Should Know About Science expands every reader’s knowledge. Key concepts in biology, chemistry, physics, earth, and general science are explored and demystified by an award-winning science writer and a seasoned educational trainer. Endorsed by science organizations and educators, this book is perfect for kids, grown-ups, and anyone interested in gaining a better understanding of how science impacts everyday life.  101 Things Everyone Should Know About Science, written by Dia Michels and Nathan Levy is offered by Educational Innovations for $9.95.

Sample Questions!

1.  Name some characteristics of all mammals
2.  Name three of the bodily fluids
3.  What are the three states of water?
4.  What mineral is found in a saline solution?
5.  What do we use calories to measure?
6.  What happens over time when iron is exposed to oxygen?
7.  At the same pressure, which is more dense—hot air or cold air?
8.  How does a semiconductor work?
9.  Each year, Earth revolves once around what?

  • the sun
  • the moon
  • its axis
  • the Milky Way

10.  What are the four major directions? In which direction does the needle of a compass point?
11.  The continental divide separates:

  • which animals are nocturnal and which are diurnal.
  • the Northern Hemisphere from the Southern Hemisphere.
  • the direction water travels to the sea.
  • where it rains from where it snows.

12.  Why is it colder an hour after sunrise than it is at sunrise itself?
13.  What is a hypothesis?
14.  What is the goal of a double-blind, placebo controlled study?
15.  How can you use a lemon to light a light bulb?
 

Answers:

1. All mammals have backbones, are warm-blooded, have hair or fur, and drink their mother’s milk when they are born.

All mammals are vertebrates, which means they have backbones, unlike worms or insects. They are also able to maintain a constant body temperature, which is called being warm-blooded. Mammals have hair or fur at some point in their lives, and the females produce milk for their young through mammary glands. Mammals have large brains with modified skulls, complex teeth, and three ear bones. Their skulls have adapted over time to support their elaborate chewing muscles, and to better contain their large brains. Scientists believe that mammalian ear bones (the malleus, incus, and stapes) evolved from bones that were no longer needed, such as a bone to support gills. There are three orders of mammals: monotremes (egg-layers), marsupials (pouched mammals), and placentals (which account for the majority of mammals, including humans).

2. Blood, sweat, saliva (or spit), tears, breastmilk, semen, urine, mucus, lymph, plasma, serum, and digestive juices.

The human body is composed mostly of water, which our body uses to produce different fluids. These fluids help the body to work properly. Glands are organs in the body that create and release chemical substances through ducts. Glands produce sweat, saliva, tears, and breastmilk. Blood comprises two fluids and it also carries hormones, nutrients, infection-fighting cells, and oxygen. Plasma is the liquid component in the blood, while serum is the protein-rich fluid that remains after blood clots. Lymph is a milky fluid that contains lymphocytes, a type of white blood cell. It plays a critical role in the body’s immune system by filtering out and destroying toxins and germs. In mature males, the reproductive system produces semen, which contains the sperm needed to reproduce. Our kidneys process urine to carry wastes out of the body. Mucus is a thick secretion made by special tissues, including the inside of the nose and throat.

3. Liquid, solid, and gas.

Water exists in three states. We use the liquid state most often in our daily activities, for drinking, washing things, and cooking. Liquids do not hold a shape, but they maintain the same volume. In humans, liquid water makes up about 70 percent of our bodies. Ice, snow, and frost are frozen water. Water’s freezing temperature—the highest temperature at which water will become solid—is 32°F (0°C). Water vapor is water in its gaseous state. Until it reappears as a liquid or solid, it is invisible. Water evaporates into the air from bodies of water and from plant and animal respiration. Water vapor is an important regulator of the earth’s heat. Without it, and other so-called greenhouse gases, our planet would be very hot by day and very cold at night. A gas doesn’t hold its shape or maintain its volume. For example, if you pour one liter of water from a watering can into a bucket, it’s still one liter. If you take one liter of water vapor and release it into a two-liter bottle, it will spread out to fill the entire bottle. At sea level, water vaporizes at 212°F (100°C).

4. Salt.

Minerals (like salt) are natural compounds formed through geological processes. Saline is the term used to describe something, including a solution, that contains salt. The chemical name for salt is sodium chloride. Oceans are huge saline solutions, containing about 3.5 percent salt. Salt is also found in some rivers, lakes, and seas (e.g., the Dead Sea and Great Salt Lake). There are natural salt beds that are thought to have come from the salt water of evaporated ancient seas.

Salt manufacturers obtain salt either from these beds or by evaporating seawater. People have used salt as a seasoning and to preserve food supplies since ancient times. It was even used as money, in the form of salt cakes, by the Hebrews and other societies during Biblical times. There are references in the Christian Bible to salt and its value (e.g., “any man worth his salt.”) In Roman times, salt was an important item of trade and was used as money as well. Roman soldiers received part of their pay in salt, and newborn babies were rubbed with salt to promote good health. To compare a person to the “salt of the earth” is to say that they are valuable and have worth. Before refrigeration, rubbing salt into meat was the only way to preserve it. Salt is an excellent cleaning agent, drives away ants, is an effective antiseptic, and is used in skin treatments. Solutions of salts in water are called electrolytes. Both electrolytes and molten salts conduct electricity. Electrolytes also help the kidneys retain proper fluid levels and help balance the amounts of acids and bases in our bodies. They also help the cells in our bodies maintain a proper “voltage” so that the nerve cells can communicate with each other via electrical signals. Electrolyte drinks containing sodium and potassium salts are used to replenish the body’s water and electrolyte levels after water loss. Excessive water loss, resulting in dehydration, can be caused by exercise, diarrhea, vomiting, starvation, or surgery.

5. Energy.

We use calories to measure heat or energy. Scientists define the small calorie, or gram calorie (c), as the amount of heat it takes to raise the temperature of one gram of water 1°C. The large calorie, or kilocalorie (C), is equal to 1,000 small calories and is used to measure the amount of energy produced by the food we eat. Some items we consume have no calories, like water, coffee, or artificially-sweetened drinks, and provide us with no energy—although coffee and some diet sodas contain caffeine, which can create the illusion of energy. Other foods, such as cake and doughnuts, have lots of calories, but they provide little energy since they are very low in nutrients. These are known as empty calories. Any extra calories we consume beyond what is needed for our daily activities are stored by the body as fat.

6. It rusts.

Rust is the common name for a very common compound, iron oxide. For iron (chemical symbol Fe) to become iron oxide, three things are required: iron, water, and oxygen. Iron oxide, (Fe2O3) is so common because iron readily combines with oxygen (so readily, in fact, that pure iron is only rarely found in nature). Iron or steel rusting is an example of corrosion, an electrochemical process. Water speeds the process because it allows for the formation of hydroxide (OH-) ions. The rust that forms is much weaker than iron; when iron becomes severely rusted, it will crumble away. To prevent rusting (or the oxidation of iron), rustproof paint can be applied—a common occurrence on the Golden Gate Bridge in San Francisco. In other applications, nickel and chromium are added to iron to bind together the atoms and prevent them from rusting.

7. Cold air.

Cold air is more dense than warm air. Air is made up of nitrogen, oxygen, and other molecules that are moving around at incredible speeds, colliding with each other and all other objects. The higher the temperature is, the faster the molecules move. As the air is heated, the molecules speed up and push harder against their surroundings and each other. If the volume of the area is not fixed, this increases the space between the molecules, making the air less dense. For example, when the air in a hot-air balloon is heated, it expands (molecules speed up and spread apart). Now less dense than the surrounding air, the balloon rises. When the heater is turned off, the air in the balloon cools, the molecules slow down and move closer together, and the balloon descends.

8. By conducting electric impulses in a controlled fashion.

Semiconductors have had a monumental impact on our society. You find semiconductors inside most microprocessor chips—the heart of any normal computer. Anything that’s computerized or uses radio waves depends on semiconductors. Semiconductors, often created with silicon, allow the transmission and control of electric impulses in microscopic circuits. The smallness of these circuits has led to portable technology that could not have been built with the previous technology of vacuum tubes. For example, the computing power of a modern laptop computer would have required a large building full of power-hungry equipment and a large maintenance staff were it not for semiconductor technology. A diode is the simplest possible semiconductor device, and is therefore an excellent beginning point if you want to understand how semiconductors work. A diode allows current to flow in one direction but not the other. You may have seen turnstiles at a stadium that let people go through in only one direction. A diode is a one-way turnstile for electrons. Most diodes are made from silicon. You can change the behavior of silicon and turn it into a conductor by mixing a small amount of an impurity into the silicon crystal. A minute amount of an impurity turns a silicon crystal into a viable, but not great, conductor—hence the name “semiconductor.”

9. Earth’s orbit around the sun is called Earth revolution.

This celestial motion takes 365.26 days to complete one cycle. Earth’s orbit around the sun is not circular but elliptical. An elliptical orbit causes the distance from Earth to the sun to vary annually. Because Earth’s axis is tilted in relation to its orbit, the Northern Hemisphere receives longer and more direct exposure to the sun for half the year. For the other half, the Southern Hemisphere receives the warmer weather. The moon revolves around Earth much in the same way that Earth revolves around the sun, but it takes only 28 days for the moon’s revolution. Earth’s axis is the invisible line extending through its center from pole to pole. Earth spins, or rotates, on its axis one rotation every 24 hours, causing day and night. The Milky Way is the galaxy to which our solar system belongs.

10. The four major directions are north, south, east, and west; a compass needle points north.

A compass, often used when hiking or sailing, is a navigational tool used to tell direction. Magnets in the compass align themselves along a magnetic north-south orientation, which causes the needle to align with the magnetic North Pole, so it points north. The compass card inside the glass has the four headings shown as N, E, S, and W (going clockwise) and subheadings of northeast, southeast, southwest, and northwest. Numbers appear every 30 degrees. Long vertical marks occur every 10 degrees, with intervening short marks at 5-degree points. The compass card containing the magnets is mounted on a small pivot point in the center of the card assembly. This allows the compass card to rotate and float freely. The enclosure of the compass is filled with white kerosene to provide a medium to dampen out vibrations and unwanted oscillations. A lubber line is etched onto the glass face of the instrument to enable exact reading of the compass. When a compass points north, it is pointing towards magnetic north, or in the direction of the earth’s magnetic field. True north, also known as geographical north, is the actual northernmost point on the earth, or the center of the North Pole. The two measurements differ because the Earth’s magnetic “north pole” is actually in Canada. In order for an explorer to determine his actual location, he has to know the difference between true north and magnetic north, which changes depending on the longitude.

11. The direction water travels to the sea.

The North American continental divide is a mountain ridge that runs irregularly north and south through the Rocky Mountains and separates eastward-flowing from westward flowing waterways. The waters that flow eastward empty into the Gulf of Mexico by way of the Mississippi and other rivers. The waters that flow westward empty into the Pacific Ocean. Every continent with the exception of Antarctica has a continental divide. Some continents may have more than one.

North America also has an eastern continental divide, which runs along the Appalachian Mountains. Rivers to the west of this divide drain into the Mississippi and other rivers that flow into the Gulf of Mexico. Waterways to the east of the divide flow into the Atlantic Ocean.

Nocturnal and diurnal refers to the active time for an organism. An animal that is active during the day and rests at night is diurnal. An animal that primarily rests during the day and is active at night is nocturnal. The equator, an imaginary line drawn around the earth halfway between the north and south poles, separates the northern and southern hemispheres. Rain is liquid precipitation while snow is solid crystals. There are several factors that affect whether precipitation falls as snow or rain, such as temperature and elevation.

12. Because the planet continues losing heat after sunrise.

We think the minimum temperature should occur at sunrise because the earth has been cooling down all night. The temperature drops throughout the night because of two processes. The earth no longer receives energy from the sun, and the earth radiates energy to space. Overnight, the balance is strongly negative, and the earth loses heat. At sunrise, solar energy again arrives, but the heat loss due to radiation to space dominates until about an hour after sunrise. At that time, incoming solar radiation increases enough to overcome the radiational heat loss.

13. A proposed explanation for why something happens.

In common usage today, a hypothesis (which is Greek for assumption) is a provisional idea whose merit must be evaluated. Science happens in many ways. In some instances, a scientist observes a phenomenon—such as, food left at room temperature spoils more rapidly than food kept cool—and then develops a hypothesis for why. Other times, scientists set out to answer a question—such as, will mice be healthier if they eat vegetables or chocolate. Whether the hypothesis comes from an intellectual pursuit or an observation, the job of scientists is to perform tests in order to validate or negate their ideas. Through rigorous testing, scientists can help us learn what is speculation and what is real.

14. To eliminate the chance of bias.

In a single-blind experiment, the individual subjects do not know whether they are so-called test subjects or members of an experimental control group, but the researchers do. In such an experiment, there is a risk that the subjects are influenced by interaction with the researchers. This is known as the experimenter effect. Double-blind describes an especially stringent way of conducting a scientific experiment. In a double-blind experiment, neither the individuals nor the scientists know who belongs to the control group. Only after all the data is recorded (and in some cases, analyzed) are scientists permitted to learn which individuals are which. Performing an experiment in double-blind fashion is a way to lessen the influence of prejudice and unintentional cues on the results. Strictly speaking, in this type of experiment, every scientist who interacts with or treats a subject should be “blinded.” This doesn’t mean that they are really sight-impaired, it means they don’t know who is receiving a particular test or intervention.

15. Turn the lemon into a battery.

A lemon can be used like a battery by placing a copper penny and a steel paper clip (or a zinc-coated nail) into slits cut into the lemon skin, then connecting the penny and clip with a small piece of wire. The two different metals react with the acid in the lemon juice and cause electrons to travel from the negative terminal (the steel or zinc) to the positive terminal (the penny). An electric potential is created when the different metals are immersed in the lemon, and you can measure this with a voltmeter. One lemon alone will probably not produce enough power to light a bulb, but if you link four or more lemons together in a circuit by connecting the negative terminal of one lemon to the positive terminal of the next, and so on, you may get enough electricity to light an LED bulb, or some other small device.

Dia Michels is the founder and president of Platypus Media, an independent press in Washington, DC, whose goal is to create and distribute materials that promote family life by educating grown-ups about infant development and by  teaching children about the world around them. She is an award-winning science writer who has written or edited over a dozen books for adults and children. She has spoken at national and international conferences for such groups as American Association for the Advancement of Science, national Association of Biology Teachers, La Leche League International, Smithsonian Institution, and the Museum of Science.

Nathan Levy is the author of Stories with Holes, Whose Clues? and Nathan Levy’s 100 intriguing Questions. A gifted educator, Nathan worked directly with children, teachers, and parents in his 35 years as a teacher and principal. He has developed unique teaching strategies that encouraged the love of learning. He has also mentored more than 30 current principals and superintendents, as well as helped to train thousands of teachers and parents in better ways to help children learn.


Ghost Eyeballs

October 14, 2011

by: Norman Barstow

Educational Innovations’ Growing Spheres can be used to add a note of ‘horror’ to your classroom or home Halloween experience.  Once fully expanded, Growing Spheres have an index of refraction almost identical to that of water. This means that when the Growing Spheres are placed in water, they are nearly invisible.

Materials:

  • A large (2 qt or larger) translucent plastic storage container and lid.
  • Growing Spheres : GB-720 or GB-730 (these are the size used for the photos)
  • Water
  • Label for the container lid: GHOST EYEBALLS

Procedure:

1. Fill the storage container about ¾ full with water.

2. Add a pinch or two of Growing Spheres.

3. Wait about a day to let the spheres expand in size.

‘THE HORROR’

Place the container of ‘ghost eyeballs’ either on your school desk or at home on a table or chair on the front porch.  Place a ghost mask and/or ghost costume near the container of eyeballs.  Invite your students or trick or treaters to reach into the bowl and touch the ghost eyeballs.

CAUTION:

The eyeballs won’t be visible at first, but after several hand insertions, the water will get a little dirty and the eyeballs will be visible.

HUMOROUS FOLLOW-UP.

When I finished taking the pictures for this Blog entry, I put the Growing Spheres into the soil of a large plant we have in the house.  When we’re away for the summer, we leave the plant with a friend.  One day, after a rainy spell, our neighbor noticed the spheres sticking up out of the soil. “What,” she thought, “Snake eggs?”

So she rushed a sample over to a local nursery where she learned that these snake eggs were actually a form of water gel crystals.

What Are Water Gel Crystals?

When placed in water, over time these hard crystals expand to about 300 times their size, producing gel-like spheres. Students love to feel the slippery, spherical gel! The Large size start with a diameter of about 3.0 mm and end with a diameter of about 20.0 mm.  For a lesson activity, ask students to determine the change in volume, using V = 4/3 pr3.  These polymer spheres are great for starting seeds and growing plants so that the roots can be seen! They can be colored using food coloring. The polymer is similar to our super-absorbent, polyacrylamide polymer (#GB-5B and #GB-3) and can be dried and reused. These spheres are available in four sizes: Regular (~1.4 cm expanded), Large (~2.3 cm expanded),  Jumbo (~3.3 cm expanded) and Gigantic-Sized Spheres (start with a diameter of ~15 mm and grow to a diameter of ~57 mm!)



Make Your Own Time

October 10, 2011

by: Martin Sagendorf

A Definition:

Clocks measure time – it can be a continuous measure of events passing or the measure of the interval between two events.

Of Hours:

After years of evolution, our modern clocks now divide the day into 24 equal length hours.  And, as we know, there are two systems in use today: Americans use the “double-twelve” system while the rest of the world uses the 24 hour system.

As An Aside:

The word “hour’ comes from the Latin and Greek words meaning season, or time of day.  A “minute” from the medieval Latin pars minuta prima (first minute or small part), originally described the one-sixtieth of a unit in the Babylonian system of sexagesimal fractions.  And “second” from partes minutae secundae, was a further subdivision on the base of sixty – i.e. “a second minute”.  (ref. Pg. 42 The Discoverers by Daniel J. Boorstin)

The “Double-Twelve” Clock Face:

Has 12 at the top – probably because at noon the sun is at its highest point in the sky.

But…

We can make a clock with 12 o’clock anywhere we wish and the clock will still work just fine.

Here we have a clock with 12:00 where 5:00 usually is.  Now, if the hour hand points to 12 and the minute hand points to 2, the time would be 10 minutes past 12.

Or:

We can rearrange the face:

Or:

We can replace the numbers:

Or:

We can divide the day into ten hours (times 2).

Suitable Clocks & How:

-       Good candidates are battery operated clocks with face diameters of 8 inches or less.

-       There are a variety of these clocks – all I’ve seen can be disassembled if one is careful.  When a front cover face must be removed, it is usually secured by three small tabs at the inner part of the face – use a worn common screwdriver to gently pry inwards, over a tab location, between the side of the cover face and the clock body – this will release the tab and allow the cover face to be gently ‘worked’ outwards.  Other clock designs are held together by multiple screws from the rear – be careful, some of these have real glass for the cover face.

-       The hands can be pried-off by using one’s fingernails on opposite sides of the hub of each hand.

-       A new dial face should be of ‘card stock’ (8-1/2” x 11” is readily available) – standard weight paper is too light.

-       A dial face must be a little smaller (1/16” on the diameter) than the opening into which it is placed – this will prevent buckling from expansion due to high humidity.

-       The dial face can be hand-drawn or computer-generated (using any of the popular computer drawing programs).

-       A punch or a craft knife can be used to cut out the center hole.

-       Sometimes the original dial face can be removed – sometimes not – it is not really necessary.  In either case, multiple small pieces of double-sided tape are used to fasten the new dial face.

-       When reinstalling the hands, they must be synchronized – the easiest way to do this is to set (press on) all the hands pointing to the (original) 12:00 position.

And More:

Over the years I, and my students, have made dozens of different clock faces – there seems to be never-ending variations.  You, and your students, will think of many different ones – just think of anything that represents numbers.  And, what’s neat is that each individual clock can have the maker’s name and/or school name included on its face.

Marty Sagendorf is a retired physicist and teacher; he is a firm believer in the value of hands-on experiences when learning physics.  He authored the book Physics Demonstration Apparatus.  This amazing book is available from Educational Innovations – it includes ideas and construction details for the creation and use of a wide spectrum of awe-inspiring physics demonstrations and laboratory equipment.  Included are 49 detailed sections describing hands-on apparatus illustrating mechanical, electrical, acoustical, thermal, optical, gravitational, and magnetic topics.  This book also includes sections on tips and hints, materials sources, and reproducible labels.


The Law of Dulong and Petit

September 3, 2011

by: Dr. Jean Oostens

Atoms were proposed in antiquity without any experimental evidence by Democritus, a Philosopher.  This must have been a problem for Newton and Leibnitz who posited that there was always a mean of considering smaller and smaller intervals of space to calculate the “instantaneous velocity”.

The introduction of the precision balance in chemistry by Lavoisier paved the way for Dalton to formulate his laws on the “definite and multiple proportions” governing chemical reactions.  This supported the atomic theory, without giving it general acceptance.

Specific heat was defined as the quantity of heat needed to increase one gram of a substance by one degree.  There was no definite pattern when specific heats of various substances were compared.  Until two French scientists, Dulong and Petit in 1819 calculated specific heat by atomic mass.  There appeared a number of cases where the results were quite similar: about 6 calorie per mole.  This was equivalent to stating that any atom is as good as any other to store heat!  This was a small step towards acceptance of the existence of atoms.   An explanation for this, and the reason for the exceptions, had to wait the early 20th century explanation by Albert Einstein.  By that time, atoms had gained wide acceptance from the work of Rutherford, and soon by Bohr.
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The Lesson:

You are given several chunks of metal, each containing 0.6 1024 atoms (i.e. one mole) of one element.   How will each of those samples, when dropped in a standard quantity of hot water (typically 200 mL and 70 C) affect the temperature?

Step 1  Use a good balance (at least 0.1 gm resolution) to determine which element you are dealing with.  If possible confirm your identification with an additional cue.

Step 2 . Select one of the computers available, and look at the readings of the two temperature probes (lower left corner of the screen).  They will tell which pair of element your are assigned to investigate.

Step 3.  Prepare your two standardized water containers.  Fill the two Styrofoam cups with equal amount of tap water. Check that the two temperature sensors read the same within 0.1 C.   Then bring the two cups to the microwave oven and heat for 2 minutes.  Exchange the positions of the cups in the microwave oven and repeat another 2 minutes of heating (this will uniformize the temperatures).

Carefully bring back the two cups (the water may be very hot) to your station and insert the temperature probes into their respective cup.  You need to note which cup is to receive the required element (Gold => Yellow and Silver => Grey for example).   When the probes reach an equilibrium, after 5 to10 seconds, verify that the two temperatures match within a degree or less.  If necessary, use a 60 mL syringe to transfer water from one cup to the other and then the other way.  The idea is to have the same quantity of water at the same temperature within reason.

Step 4.  Start the measurement.  Hit the “START” button with the mouse and wait 10 to 15 seconds during which an horizontal line should appear, with both traces nearly on top of each other (if this is not so, go ahead anyway: you can always get another chance).

Drop your two samples the same time, one in each cup and watch until the completion of the three minutes.

Compare your results with the other teams’ and draw conclusions of the exercise.

This experiment on Dulong and Petit Law was performed by the students of Professor Shuffett’s Chemistry class at Lindsey Wilson College (Columbia, KY). It uses the mole set from Educational Innovations and takes advantage of existing data acquisition capabilities at that college.

About the Author:  After 20 years of research in Particle and Nuclear Physics, Dr. Oostens included in his activities, teaching at several college and universities all over the US. After moving to Kentucky 17 years ago, he co-founded a local Alliance, STASCKY (Science Teachers Alliance – South Central Kentucky).  He hasserved as STASCKY’s secretary since its inception.

For more than forty years he has kept a small research activity in collaboration with Los Alamos National Laboratory in New Mexico.  His involvement there started when Dr. Louis Rosen started a non-programmatic (i.e. not defense) group to attract more talents from all over the world. In 1970, he invited Dr. Oostens to participate in that project as the first non-American to work there. Dr. Louis’ idea was predicated on a high intensity 800 MeV accelerator called LAMPF (for Los Alamos Meson Proton Facility). Later on, the proton beam was used to create a flexible neutron source, LANSCE, that attracted a variety of researchers from all fields.


How to Make a Rocket (Scientist)

July 1, 2011

by:  Tami O’Connor

A few months ago I had occasion to conduct two hands-on workshops for elementary and middle school teachers at the NSTA National Convention in San Francisco on behalf of Educational Innovations.  One presentation focused on film canister rockets.  This is a tried-and-true way to teach Newtown’s First and Third Laws of Motion and also brings to light concepts such as the four forces of flight; thrust, drag, weight, and lift.  It also reinforces instruction on 3-D shapes and 2-D plane figures such as circles, cones, cylinders, rectangles, and triangles.

I presented the lesson to the teachers in much the same way I would to my students.  The first thing we did was to brainstorm the features all rockets have.  After a bit of discussion it was agreed that they all have a nose cone, a cylindrical body, fins, and an engine.  I then handed out a paper template imprinted with the pattern of a nose cone and fins, a regular 8½ x 11 sheet of white paper, a piece of goldenrod paper, and a white translucent film canister.  Also required are scissors, tape, ¼ piece of an Alka Seltzer tablet, and paper towels.

The only canister that works with this rocket is the type that has the lid that fits snugly inside the canister.  The canisters that have a lid that wraps around the outside rim, however, will not allow enough pressure to build up inside the chamber.

The first step in building a film canister rocket is to construct the body of the rocket.  The easiest way is to curl the white 8 ½ x 11 paper into a cylindrical shape using the film canister (without the top) as a guide.  The paper can be rolled around the film canister and then taped along the edges.  The easiest way to recover the film canister is to blow into one end of the rolled cylinder, forcing the canister out the other end.

When I conduct this activity I am careful not to offer any suggestion as to whether students should roll the paper in the long or short direction, nor do I discuss how much tape should be used.  The results are very interesting.  Students (adults and children) are very creative, especially when they are not bombarded too much instructional advice.

At this point, you should use Scotch tape to affix the film canister to the cylinder.  This is one of the most critical steps.  First, the canister must have the open end extending far enough from the end of the cylinder so that no tape overlaps the opening of the canister.  If any tape extends over the opening, the lid will not form a complete seal, and sufficient pressure to launch the rocket may not build up.  Second, if the canister is not taped securely, it will launch into the cylinder and propel only the canister rather than the entire rocket.

The next step is to cut out a nose cone and fins.  I use the attached template in my workshops.  The nose cone is actually a circle with a ¼ pie slice cut out.  For those old enough to remember, it closely resembles a Pac Man figure.  The nose cone is made by curling the PacMan so the edges of the missing pie piece begin to overlap forming a cone shape.  Though the template I passed out had cut lines for the nose cone and fins, I give very little direction as to the size of the nose cone or the total number of fins each student should use.FilmCanRocketTemplate copy

When the construction of the rocket is finally completed, it’s time for the launch!  I have students lay the piece of goldenrod paper on their desk and clear from the launch area any papers or other things that might get wet.  I invite students one at a time to the front of the room so everyone can see the results of their construction techniques.  During teacher workshops where time is limited, I have everyone launch at the same time.

When we’re ready to launch I hand out approximately ¼ piece of an Alka Seltzer tablet.  It is important when working with students to remind them not to put anything in their mouths (especially Alka Seltzer!).  Since the Alka Seltzer is the last step in the process I have students place the tablet piece on the desk and leave it there until I specifically tell them to pick it up!

While holding the rocket upside down students are instructed to fill an eyedropper or pipette with water and add a squirt or two into the film canister.  The amount of water is not critical in the grand scheme of things.

The next step is far more critical, so it is important that students are paying attention at this point.  Once the Alka Seltzer is added to the water in the film canister, it will begin to fizz and give off Carbon Dioxide gas.  The total release of gas is not immediate and therefore will continue for more than a minute which allows plenty of time for the student to secure the cap onto the film canister.  If students become flustered and attempt to jam the top onto their canister while holding the paper cylinder portion of their rocket rather than holding the canister portion they will likely damage their rocket.  Thirty seconds is much longer than most people think.  Having the students relax is the key!  The important thing to remember is to grip the rocket around the film canister and NOT the paper cylinder.

Once the top of the canister is secure the rocket should be placed in the center of the goldenrod paper and the student should step back and wait.  The results are wonderful!!!  Inside the closed film canister pressure continues to build until the container can no longer contain it.  At this point, the top separates from the canister.  Since the top is unable to move with the table behind it, the rocket is propelled upward with a loud popping noise.   Since Goldenrod paper is an indicator for bases, students will notice the launch pattern that is left behind on their launch pad!  Kids find this almost as cool as the rocket launch!

After the activity is over students will note with interest which rockets flew the highest.  This is when the true lesson begins!  Here is the opportunity to identify the many variables and the effects of each variable on the rockets’ flight characteristics.  Examples will include the width of the nose cone, the length of the cylinder, whether any excess paper from the cylinder was trimmed and discarded, and the amount of tape that was added to the rocket during construction.

Since the film canisters are reusable, and the construction materials are quite inexpensive, students should be given the opportunity to redesign their rockets based on discoveries they made during the launch trials and the class discussion.  This is one activity that generates so much enthusiasm with every age group that I fit it in whenever possible.  I’ve brought this activity to Girl Scout meetings with varied ages, Daisys to Cadettes. And with 16 years of teaching experience from 1st grade to 7th, I managed a successful launch in each and every class!  This activity is so adaptable that there is certainly no shortage of learning!


Silicon from Sand

March 2, 2011

by: Carl Ahlers

Next time you step onto the beach, bend down, grab a handful of sand and admire the fact:   By mass 47% of what you hold in your hand is the element silicon. The rest is simply oxygen.  Remarkable!

Silicon is the second most abundant element in the earth’s crust (27.7%) – only oxygen beats it – and can easily be extracted from white sand (SiO2) in a spectacular reaction in the school science laboratory.

Thermite Reactions

In Thermite reactions metal oxides react with aluminum to produce the molten metal.  These redox reactions require substantial activation energy to get going and are highly exothermic.

They have been used industrially for welding (even under water), the preparation of metals from their oxides (reduction) and the production of incendiary devices.  The process is initiated by heat but then becomes self-sustaining.

In the early 1900’s a product called Thermit® was developed and used worldwide to weld rail tracks.  The photo (taken by J J Szerkeszto) was taken in 2010 proving that it is still in use today.  This is the reaction:

Fe2O3 +    2Al    →    2Fe    +    Al2O3 +   energy

The question is:  Can silicon be persuaded to give up its oxygen in a similar thermite process?

For Fe2O3 ,  ∆Hf =  -822 kJ/mole; for SiO2 , ∆Hf =  – 859 kJ/mole

In 1902, Kuhn described a method that is a variation of the thermite reaction for the reduction of silicon from silicon oxide.  In this process a primary reaction provides the activation energy to initiate the secondary reduction reaction.

Extracting Silicon from Sand

Safety / Risk Assessment

★    Burning magnesium produces bright light that may cause temporary loss of sight.  Avoid looking directly at the flare.

★    Magnesium is very reactive and contact with other chemicals may result in explosion.

★    This demonstration produces intense heat and molten silicon. A dry-powder fire extinguisher should be readily available at all times. DO NOT use water as an extinguisher as this will produce potentially explosive hydrogen gas.

★    The near-impossibility of smothering and the high temperatures generated make thermite reactions potentially hazardous.  Appropriate precautions must be taken before thermite is ignited.  Keep all flammable material away from the area.

★    The reaction should be performed in a fume cupboard or outdoors behind a safety shield as it produces intense heat, smoke and molten metal. Sparks can fly up to 2 m horizontally.

★    Wear heat-protective welding gloves and use metal tongs to handle the fragments of the clay pot and molten silicon after the reaction has taken place.

★    Wear protective clothing and safety glasses.

Chemical Safety

Aluminum (Al)

Risk phrases: R10 – 15   Extremely flammable; Contact with water liberates highly flammable gases.

Safety phrase: S7/8/44  Keep container tightly closed;  Keep container dry.

Magnesium (Mg)

Risk phrases: R11-15   Extremely flammable; Contact with water liberates highly flammable gases.

Safety phrase: S7/8-43  Keep container tightly closed;  Keep container dry.

Hydrochloric Acid (HCl) is a strong acid. Treat with the greatest respect.

Risk phrases: R34-37   Causes severe burns; Irritating to eyes & respiratory system.

Safety phrase: S2-26  Keep out of reach of children; In case of contact with eyes, rinse immediately with plenty of water and seek medical advice; Wear suitable gloves and eye/face protection.

Sodium hydroxide (NaOH) destroys clothes and causes injury to the skin.  Treat with the greatest respect.

Risk phrases: R35   Causes severe burns

Safety phrase: S2/26/37/39  Keep out of reach of children; In case of contact with eyes, rinse immediately with plenty of water and seek medical advice; Wear suitable gloves and eye/face protection.

What You Will Need

Chemicals

•     Aluminum powder,  325 mesh or finer

•     Powdered sulfur

•     Dry white sand – beach sand or washed white builder’s sand

•     Hydrochloric acid, 4M (add 180 mL conc. HCl to 500 mL water)

Initiator chemicals:

•     Fine magnesium powder & magnesium ribbon (5 cm)  or Potassium permanganate (KMnO4) and glycerine

Other

•     Mortar & pestle

•     Small clay flower pot, ∼ 6.5 cm (2.5”) inside top diameter

•     Small glass beaker & plastic container

•     Electronic balance, 100 g ± 0.1 g

•     Heat resistant pad

•     Transparent safety shield or fume cupboard

•     Heat-protective gloves eg. welding gloves

•     Spatula & metal tongs

•     Fire lighter with long stem

Here’s How

1.   Dry about 50 g of sand in an oven for 2 hours (∼ 350℉) and then grind the sand to a powdered form in a mortar and pestle.

2.  Weigh and mix the following to form a homogenous mix:

8 g of dry aluminum powder

10 g of powdered sulfur

7 g of dry powdered sand

3.  The best mix is obtained by shaking the mixture for a minute in a sealed plastic container.  Do NOT grind them together in a mortar and pestle.

4.  Use the small clay flower pot. If it has a hole in the bottom – cover the hole with paper. Transfer all of the mix to the pot.

5.  Make a small cone-shaped indentation at the top (¾” deep and ¾” wide) and fill this with magnesium powder to facilitate ignition.  (For an alternative method see Note 1 in the book).  Fray a 5 cm (2”) magnesium ribbon’s end with scissors.  This will enlarge its surface area and aid ignition. Push this fuse into the magnesium powder pile.

Safety: Position the pot on a heat resistant pad in a fume cupboard or outdoors away from any combustible material. Use a safety shield. Wear protective eye wear, gloves and a lab coat.

Light the frayed end of the magnesium ribbon using a long stemmed fire lighter.  It may take a few seconds before the ribbon starts burning. Once this happens – step back immediately.  Ignition of the mixture is not instantaneous and might take as long as 60 seconds.  The reaction will produce lots of spattering, bright light and intense heat. The temperature is reported to be well above 2,200℃ (4,000℉).  The residue will have an orange-red glow and be hot for some time.  If required, carefully pick up the red-hot residue using metal tongs.

If the reaction fails to react: Wait 3 minutes. Do not approach the reaction vessel until you are sure ignition is not possible.  Replace the ribbon or add more magnesium powder. Try again.

7.   Purify the silicon residue.

Leave the clay pot to cool for 20 minutes. Break the pot apart and separate the silicon residue from the clay pieces.  Break the residue into smaller pieces using light taps from a hammer.

8.  The silicon (Si) and aluminum oxide (Al2O3) is now separated from the aluminum sulphide (Al2S3) by adding the residue to diluted hydrochloric acid in a glass beaker (acid – take care!).  Copious amounts of hydrogen sulphide will be evolved – foul smelling rotten egg gas – use a fume cupboard or perform outside.

Al2S3 +    6HCl   →   2AlCl3 +    3H2S

Leave the residue in the acid until gas formation subsides. This process may take up to 20 minutes. The finer the residue, the faster this reaction.

9.  Now, carefully discard the acid under running water and wash the residue in the beaker for 30 seconds.  The silicon will be found in the form of pea-size, hard, black, crystalline globules. It is insoluble in most acids.  Boil the globules in a glass beaker using dilute hydrochloric acid for further purification.

Disposal

Allow the solids and clay fragments to cool to room temperature. The clay flower pot invariably cracks and should not be re-used. Dispose of all solids in the waste bin.

The Chemistry

There are basically three reactions here that produce a chain reaction effect.  Magnesium burns in oxygen and produces the activation energy to get the sulfur and aluminum going.

2Mg   +   O2 →   2MgO   +   energy

The aluminum and sulfur again, react in an exothermic reaction that is the source of activation energy for the silica and aluminum.

2Al   +   3S   →   Al2S3 +   energy

3SiO2 +   4Al   →   2Al2O3 +   3Si   +  energy

In the book “Expose, Excite, Ignite!” the author describes two simple tests that can be performed in the school lab to establish if the globules are indeed the semi-conductor, silicon.  You can purchase this book from Educational Innovations at http://www.teachersource.com.


No Pop Bubbles!

December 3, 2010

by: Ron Perkins

At first glance No-Pop Bubbles may seem like any other bubbles.  While the bubble solution is a bit more viscous, one blows No-Pop Bubbles like any other bubble.  The small bubble wand suspends a bubble film which, when air is blown through it, releases small bubbles into the air.  These bubbles, however, are no ordinary bubbles.  No-Pop Bubble solution begins as a regular soap and water bubble solution.  Added to this solution is a small amount of a non-toxic water soluble polymer.  When No-Pop Bubbles are fist blown, the bubbles behave like ordinary bubbles.  As the water evaporates from the bubble’s surface, however, an extremely thin plastic ‘bubble skeleton’ remains.  It is this plastic bubble skeleton which has the properties for which No-Pop Bubbles are named.

Blow No-Pop Bubbles up into the air.  Observe the colors (interference patterns) in the bubbles as they float.  In approximately 10 seconds (depending on the relative humidity) the colors in the bubbles will begin to disappear.  When the bubble are colorless, they may be caught on your finger without popping!

Try This!

Blow up an ordinary latex balloon.  Then blow a bunch of No-Pop Bubbles into the air.  While the bubbles are ‘drying’, rub the balloon vigorously on your hair in order to develop a static charge.  Use the charged balloon to attract the No-Pop Bubbles.  Observe how the bubbles behave before and after they are in contact with the charged balloon.  Experiment with other static sources, rods or Van de Graaf generators, etc.  The Fun Fly Stick is perfect for this activity!  After your bubbles have hardened bring your charged Fun Fly Stick close to your bubbles.  Watch what happens as the bubbles get closer to the Fun Fly Stick!

Blow No-Pop Bubbles outside, next to your school building on a windy day.  Observe how the bubbles float and fly in the air currents as the wind blows around the building.  See if you can find mini-tornadoes of air!

No-Pop Bubbles that fluoresce under a black light are also available at Educational Innovations!  After they are blown, these bubbles glow brilliantly, and all you need is a UV flashlight!

The activities you can do with these little bubbles are endless!  You’ll find yourself blowing them and enjoying their soothing properties!  Get your No-Pop Bubbles today at Educational Innovations!


Bubble Basics

November 12, 2010

by: Michelle Bertke and Melanie Bunda

Bubbles are always a fun and interesting activity for kids of all ages.  However, bubbles are not only fun, they are also an excellent teaching tool for some abstract concepts such as air density, dissolved gasses, and air pressure.  Below is a collection of bubbly activities that highlight each of these topics. Educational Innovations offers a full line of wonderful bubble products!

Gravity Defying Bubbles

Different gasses have different densities.  The air around us is mostly nitrogen (N2) and oxygen (O2), which are both lighter than carbon dioxide (CO2).  When a heavy gas, such as CO2 is placed in a tank, it will sink to the bottom without mixing.  This can be achieved by placing a few blocks of dry ice in a large fish tank or clear plastic bin covered loosely with a lid and allowing them to sublime.  This will take several minutes. Always use caution when handling dry ice by using proper gloves and safety goggles. Once full, blow bubbles over the surface of the tank.  When the bubbles reach the interface of the two gasses, they will float.  If you fill the tank with CO2 unnoticed, have the kids speculate as to why they think the bubbles didn’t reach the bottom, and what might be in the tank.  An alternative is to fill a balloon with CO2 by filling it with baking soda (or an alka seltzer tablet) and placing it over the opening of a bottle filled with vinegar (or water).  Lift the balloon so the contents spill into the bottle and react with the liquid, allow the balloon to fill from the reaction, twist and remove.  Use it to blow bubbles.  Compare these bubbles to those blown with regular air (use a fan, not your breath for best results).  Have students compare the two bubbles.  Which one falls faster? Which one floats longer?

Dancing Raisins

All kids will know that soda pop is fizzy, but they may not know where all those little bubbles come from.  This demonstration will highlight the dissolved gasses in soda.  Fill a glass with a clear soda.  As you pour in the soda (pour gently down the side to retain maximum fizziness in the liquid), you will see bubbles forming from the bottom and the sides of the glass.  Ask the students why they think that bubbles only form in these places.  Next, take a few raisins and drop them into the soda (you may need to break the raisins into smaller pieces).  You will notice that bubbles immediately begin to form in the crevices of the raisins.  As more bubbles collect on a raisin, it will begin to rise.  When it reaches the top, the bubbles on the outside will escape into the air and this will cause the raisins to sink, and the cycle to begin again.  Pretty soon you will have a glass of dancing raisins.  This should raise discussion about dissolved gasses and buoyancy.  Students can experiment with different sodas and different materials to see what may cause more or less bubbles to come out of solution.

Mentos and Soda

Another classic example of dissolved gasses is the Mentos and soda demonstration.  This demonstration can be done by anyone with just a two liter bottle of soda and a pack of original Mentos.  Make sure you are in an area which can get messy and sticky.  Simply open the soda and the pack of Mentos.  (Fashion a Mentos delivery apparatus out of a rolled up piece of paper to prevent getting sprayed.)  Quickly drop the Mentos into the soda all at once and immediately step back.  The ensuing fountain will go high into the air and cause widespread excitement.  The same tests can be done as were mentioned in the raisins: what kind of soda makes the highest fountain? Do different types of Mentos cause differences in the height of the fountain?

Square Bubbles

All bubbles are round.  Or are they?  A free flying bubble, no matter what shape wand produced it, will always be round.  Why is this?  When you blow a bubble, the soap solution stretches as the air flows into it, and the air pushes equally on all sides of the bubble.  This creates a perfectly spherical bubble with equal pressure on all sides.  But what happens when the wand is a three dimensional cube?  Make a cube frame out of pipe cleaners.  (Make sure to attach a handle to hold on to.)  Fill a tall beaker with soap solution and dip the cube into it, fully submerging it.  Remove the cube from the container, and you will see a square “bubble” stretched between the sides of the form.   If you blow on one side of the cube structure, the sides will collapse in on each other and come together at a point.  Now take a straw and gently blow into the center of that point.  If you get it just right, you can form a cubic bubble in a bubble!  Give the students several pipe cleaners and allow them to create their own 3D bubble wands.  See what other kinds of bubbles they can form.

Any way you look at it, either from a scientific point of view or as a kid on a sunny day, bubbles are a fascinating activity to be shared by all.  Next time you are strapped for something to do, just whip up a batch of bubble solution and let your imagination run wild.


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