Protein Synthesis Puzzle

 

Protein Synthesis
Across 2. a series of three mRNA nucleotides that codes for an amino acid 3. coded for by DNA and made of amino acids 7. process of assembling amino acids into polypeptides in the ribosomes 9. RNA that copies DNA in the nucleus 10. use to translate mRNA transcripts into proteins 11. UGA, UAA, and UAG codons 12. RNA that carries amino acids to be linked together to make proteins 15. site of transcription Down 1. both DNA and RNA are these types of compounds 2. where ribosomes are found 4. series of three bases on tRNA that code for an amino acid 5. base on RNA that replaces thymine 6. holes in the nuclear membrane where mRNA leaves to move to the ribosome 8. methionine codon (AUG) 13. RNA that makes up ribosomes along with proteins 14. site of protein synthesis

 

Protein Degradation

 

Information for the Public
Nobel Prize in Chemistry
6 October 2004

 Discovery of Ubiquitin-Mediated Protein Degradation

A human cell contains some hundred thousand different proteins. These have numerous important functions: as accelerators of chemical reactions in the form of enzymes, as signal substances in the form of hormones, as important actors in the immune defense and by being responsible for the cell’s form and structure. This year’s Nobel Laureates in chemistry, Aaron Ciechanover, Avram Hershko and Irwin Rose, have contributed ground-breaking chemical knowledge of how the cell can regulate the presence of a certain protein by marking unwanted proteins with a label consisting of the polypeptide ubiquitin. Proteins so labeled are then broken down – degraded – rapidly in cellular “waste disposers” called proteasomes.

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Through their discovery of this protein-regulating system Aaron Ciechanover, Avram Hershko and Irwin Rose have made it possible to understand at molecular level how the cell controls a number of very important biochemical processes such as the cell cycle, DNA repair, gene transcription and quality control of newly-produced proteins. New knowledge of this form of controlled protein death has also contributed to explaining how the immune defense functions. Defects in the system can lead to various diseases including some types of cancer.

Proteins labeled for destruction

Degradation needs no energy – or does it?

While great attention and much research have been spent on understanding how the cell controls the synthesis of a certain protein – at least five Nobel Prizes have been awarded in this area – the reverse, the degradation of proteins, has long been considered less important. A number of simple protein-degrading enzymes were already known. One example is trypsin, which in the small intestine breaks down proteins in our food to amino acids. Likewise, a type of cell organelle, the lysosome, in which proteins absorbed from outside are broken down, had long been studied. Common to these processes is that they do not require energy in order to function.

Experiments as long ago as the 1950s showed, however, that the breakdown of the cell’s own proteins does require energy. This long puzzled researchers, and it is precisely this paradox that underlies this year’s Nobel Prize in Chemistry: that the breakdown of proteins within the cell requires energy while other protein degradation takes place without added energy. A first step towards an explanation of this energy-dependent protein degradation was taken by Goldberg and his co-workers who in 1977 produced a cell-free extract from immature red blood cells, reticulocytes, which catalyze the breakdown of abnormal proteins in an ATP-dependent manner (ATP = adenosine triphosphate – the cell’s energy currency).

Using such an extract Aaron Ciechanover, Avram Hershko and Irwin Rose, in a series of epoch-making biochemical studies in the late 1970s and early 1980s, succeeded in showing that protein degradation in cells takes place in a series of step-wise reactions that result in the proteins to be destroyed being labeled with the polypeptide ubiquitin. This process enables the cell to break down unwanted proteins with high specificity, and it is this regulation that requires energy. As distinct from reversible protein modifications such as phosphorylation (Nobel Prize in Physiology or Medicine 1992), regulation through polyubiquitination is often irreversible since the target protein is destroyed. Much of the work was done during a series of sabbatical leaves that Avram Hershko and Aaron Ciechanover of the Technion (Israel Institute of Technology) spent with Irwin Rose at the Fox Chase Cancer Center in Philadelphia, USA.

The label is ubiquitin

The molecule that would later prove to be the label that marks out a protein for degradation was isolated as early as 1975. This 76-amino-acid-long polypeptide was isolated from calf sweetbread and was assumed to participate in the maturation of white blood cells. Since the molecule was subsequently found in numerous different tissues and organisms – but not in bacteria – it was given the name ubiquitin (from Latin ubique, “everywhere”) (fig. 1).

Fig 1. Ubiquitin – a common polypeptide that represents the “kiss of death”.

The discovery of ubiquitin-mediated protein degradation

After taking his doctorate, Avram Hershko had studied energy-dependent protein degradation in liver cells, but decided in 1977 to transfer to the reticulocyte extract described above. This extract contained large quantities of hemoglobin, which upset the experiments. In their attempts to remove the hemoglobin using chromatography, Aaron Ciechanover and Avram Hershko discovered that the extract could be divided into two fractions, each inactive on its own. But it turned out that as soon as the two fractions were recombined, the ATP-dependent protein degradation restarted. In 1978 the researchers reported that the active component of one fraction was a heat-stable polypeptide with a molecular weight of only 9000 which they termed APF-1 (active principle in fraction 1). This protein later proved to be ubiquitin.

The decisive breakthrough in the research was reported in two works that Ciechanover, Hershko and Rose published in 1980. Until that time the function of APF-1 was entirely unknown. In the first work it was shown that APF-1 was bound covalently, i.e. with a very stable chemical bond, to various proteins in the extract.

In the second work it was further shown that many APF-1 molecules could be bound to the same target protein; the latter phenomenon was termed polyubiquitination. We now know that this polyubiquitination of substrate proteins is the triggering signal that leads to degradation of the protein in the proteasome. It is this reaction that constitutes the actual labeling, the “kiss of death” if you will.

At a stroke, these entirely unanticipated discoveries changed the conditions for future work: it now became possible to concentrate on identifying the enzyme system that binds ubiquitin to its target proteins. Since ubiquitin occurs so generally in various tissues and organisms, it was quickly realized that ubiquitin-mediated protein degradation must be of general significance for the cell. In addition, the researchers guessed that the energy requirement in the form of ATP enabled the cell to control the specificity of the process.

The field was now open and between 1981 and 1983 Ciechanover, Hershko, Rose and their post docs and students developed “the multistep ubiquitin-tagging hypothesis” based on three newly-discovered enzyme activities they termed E1, E2 and E3 (fig. 2). We now know that a typical mammalian cell contains one or a few different E1 enzymes, some tens of E2 enzymes and several hundred different E3 enzymes. It is the specificity of the E3 enzyme that determines which proteins in the cell are to be marked for destruction in the proteasomes.

Fig 2. Ubiquitin-mediated protein degradation

 

  1. The E1 enzyme activates the ubiquitin molecule. This reaction requires energy in the form of ATP.
  2. The ubiquitin molecule is transferred to a different enzyme, E2.
  3. The E3 enzyme can recognize the protein target which is to be destroyed. The E2-ubiquitin complex binds so near to the protein target that the actual ubiquitin label can be transferred from E2 to the target.
  4. The E3 enzyme now releases the ubiquitin-labeled protein.
  5. This last step is repeated until the protein has a short chain of ubiquitin molecules attached to itself.
  6. This ubiquitin chain is recognized in the opening of the proteasome. The ubiquitin label is disconnected and the protein is admitted and chopped into small pieces.

 

All the studies up to this point had been done in cell-free systems. To be able to study the physiological function of ubiquitin-mediated protein degradation as well, Avram Hershko and his co-workers developed an immunochemical method. By using antibodies to ubiquitin, ubiquitin-protein-conjugate could be isolated from cells where the cell proteins had been pulse-labeled with a radioactive amino acid not present in ubiquitin. The results showed that cells really break down faulty proteins using the ubiquitin system, and we now know that up to 30% of the newly-synthesized proteins in a cell are broken down via the proteasomes since they do not pass the cell’s rigorous quality control.

The proteasome – the cell’s waste disposer

What is a proteasome? A human cell contains about 30,000 proteasomes: these barrel-formed structures can break down practically all proteins to 7-9-amino-acid-long peptides. The active surface of the proteasome is within the barrel where it is shielded from the rest of the cell. The only way in to the active surface is via the “lock”, which recognizes polyubiquitinated proteins, denatures them with ATP energy and admits them to the barrel for disassembly once the ubiquitin label has been removed. The peptides formed are released from the other end of the proteasome. Thus the proteasome itself cannot choose proteins; it is chiefly the E3 enzyme that does this by ubiquitin-labeling the right protein for breakdown (fig. 3).

Fig 3. The cell’s waste disposer, the proteasome. The black spots indicate active, protein-degrading surfaces.

 

More recent research

While the biochemical mechanisms underlying ubiquitin-labeled protein degradation were laid bare around 1983 its physiological significance had not yet been fully understood. That it is of importance in destroying defective intracellular proteins was known but, to proceed, a mutated cell was needed in the ubiquitin system. By studying in detail how the mutated cell differs from a normal cell under various growth conditions, it was hoped to gain a better idea of what reactions in the cell depend on the ubiquitin system.

A mutated mouse cell had been isolated in 1980 by a research group in Tokyo. Their mouse-cell mutant contained a protein that, because of the mutation, was sensitive to temperature. At lower temperatures the protein functioned as it should, but not at higher. Cells cultured at the higher temperature stopped growing. In addition, they showed defective DNA synthesis and other erroneous functions at the higher temperature. Researchers in Boston quickly showed that the heat-sensitive protein in the mutant mouse cell was the ubiquitin-activating enzyme E1. Obviously, ubiquitin activation was necessary for the cell to function and reproduce itself at all. Controlled protein breakdown was not only important for degrading incorrect proteins in the cell but it probably also took part in control of the cell cycle, DNA replication and chromosome structure.

Since the late 1980s a number of physiologically important substrates for ubiquitin-mediated protein breakdown have been identified. Only a few of the most important will be mentioned here.

Prevention of self-pollination in plants

Most plants are bisexual, hermaphroditic. Self-pollination leads to a gradual decline in genetic diversity which in the long run can cause the whole species to die out. To prevent this, plants use ubiquitin-mediated degradation to reject “own” pollen. The exact mechanism has not yet been clarified but the E3 enzyme has been encountered and when proteasome inhibitors have been introduced, the rejection has been impaired.

Regulation of the cell cycle

When a cell is to make a copy of itself, many chemical reactions are involved. In a human being, six thousand million base pairs must be duplicated in DNA. These are gathered in 23 chromosome pairs that must be copied. Ordinary cell division, mitosis, and the formation of sex cells, meiosis, have many points of contact with the subjects of this year’s Nobel Prize. The E3 enzyme responsible, a protein complex termed the “anaphase-promoting complex” (APC) checks that the cell goes out of mitosis. This enzyme complex has also proved to play an important role in the separation of the chromosomes during mitosis and meiosis. A different protein complex acts like a rope around the chromosome pair, holding it together. At a given signal, the APC labels an inhibitor of a certain protein-degrading enzyme, whereupon the inhibitor is carried to the proteasome and destroyed. The enzyme is released, is activated and cuts the rope around the chromosome pair. Once the rope is gone, the chromosome pair can be separated. Incorrect chromosome division during meiosis is the commonest cause of spontaneous miscarriage during pregnancy, and an extra chromosome 21 in humans leads to Down’s syndrome. Most malignant tumors have cells with changed numbers of chromosomes as a result of incorrect chromosome division during mitosis.

 

 DNA repair, cancer and programmed cell death

Protein p53 has been dubbed “the guardian of the genome” and it is a tumor-suppressor gene. This means that as long as a cell can produce p53 the development of cancer is hampered. Sure enough, the protein is mutated in at least 50% of all human cancer. The amount of protein p53 in a normal cell is low in consequence of continual production and breakdown. The breakdown is regulated through ubiquitination and the E3 enzyme responsible forms a complex with protein p53. Following DNA injury, protein p53 is phosphorylated and can no longer bind to its E3 enzyme. The breakdown stops and the quantity of p53 in the cell rises rapidly. Protein p53 acts as a transcription factor, i.e. a protein that controls the expression of a certain gene. Protein p53 binds to and controls genes that regulate DNA repair and programmed cell death. Raised levels of protein p53 lead first to interruption of the cell cycle to allow time for repair of DNA damage. If the damage is too extensive the cell triggers programmed cell death and “commits suicide”.

Infection with human papilloma virus correlates strongly to the occurrence of cervical cancer. The virus avoids the protein p53 control function through one of its proteins activating and changing the recognition pattern of a certain cellular E3 enzyme, E6-AP, which is tricked into ubiquitinating the protein p53, which is totally destroyed. In consequence of this the infected cell can no longer repair DNA damage in a normal manner or trigger programmed cell death. The DNA mutations increase in number and this can ultimately lead to the development of cancer.

Immune and inflammatory reactions

A certain transcription factor regulates many of the genes in the cell that are important for immune defense and inflammatory reactions. This protein, the transcription factor, occurs bound to an inhibitor protein in the cytoplasm of the cell, and the bound form of the transcription factor lacks activity. When cells are exposed to bacteria or various signal substances, the inhibitor protein is phosphorylated, and this results in its being ubiquitinated and broken down in the proteasome. The released transcription factor is transported to the cell nucleus where it binds to, and activates the expression of, specific genes.

The ubiquitin-proteasome system also produces the peptides that are presented by the immune defense on the surface of a virus-infected cell by breaking down virus proteins to suitable sizes. T lymphocytes recognize these peptides and attack the cell as an important part of our defense against virus infections.

Cystic fibrosis (CF)

The hereditary disease cystic fibrosis, CF, is caused by a non-functioning plasma membrane chloride channel called CFTR, the “cystic fibrosis transmembrane conductance regulator”. Most CF patients have one and the same genetic damage, loss of the amino acid phenylalanine in the CFTR protein. The mutation causes faulty folding of the protein and this in turn leads to the protein being retained in the cell’s control system for protein quality. This system ensures that the incorrectly folded protein is destroyed through ubiquitin-mediated protein breakdown instead of being transported out to the cell wall. A cell with no functioning chloride channel can no longer transport chloride ions through its wall. This affects secretion in, among other organs, the lungs and leads to the accretion of thick phlegm in the lungs which impairs their function, greatly increasing the risk of infection.

The ubiquitin system has become an interesting area of research for medicines against various diseases. Such preparations can be aimed at components of the ubiquitin-mediated breakdown system to prevent the degradation of specific proteins. They can also be designed to cause the system to destroy unwanted proteins. A medicine already being tested clinically is the proteasome inhibitor Velcade (PS341) which is used against multiple myeloma, a cancer disease that affects the body’s antigen-producing cells.

This year’s Laureates have explained the molecular background to a protein regulation system of great importance for all higher cells. New cell functions controlled by ubiquitin-mediated protein degradation are being discovered all the time and this research is being conducted in numerous laboratories all over the world.

The Laureates
Aaron Ciechanover

Technion (Israel Institute of
Technology)
Rappaport Institute
1 Efron Street
P.O. Box 9697
Haifa 31096
Israel

 

Israeli citizen. Born 1947 (57 years) in Haifa, Israel. Doctor’s degree in medicine in 1975 at Hebrew University of Jerusalem, and in biology in 1982 at the Technion (Israel Institute of Technology), Haifa. Distinguished Professor at the Center for Cancer and Vascular Biology, the Rappaport Faculty of Medicine and Research Institute at the Technion, Haifa, Israel.

Aaron Ciechanover

 

Avram Hershko

Technion (Israel Institute of Technology)
Rappaport Institute
1 Efron Street
P.O. Box 9697
Haifa 31096
Israel

 

Israeli citizen. Born 1937 (67 years) in Karcag, Hungary. Doctor’s degree in medicine in 1969 at the Hadassah and the Hebrew University Medical School, Jerusalem. Distinguished Professor at the Rappaport Family Institute for Research in Medical Sciences at the Technion, Haifa, Israel.

Avram Hershko
Irwin Rose

Dept. of Physiology and Biophysics
College of Medicine
University of California, Irvine
Irvine, CA 92697
USA

 

American citizen. Born 1926 (78 years) in New York, USA. Doctor’s degree in in 1952 at the University of Chicago, USA. Specialist at the Department of Physiology and Biophysics, College of Medicine, University of California, Irvine, USA.

Irwin Rose

Illustrations: Typoform

Source: http://nobelprize.org/nobel_prizes/chemistry/laureates/2004/press.html

 

Properties of Water Labs

Properties of Water

INTRODUCTION:

Water covers about three fourths of the surface of the earth? It is ubiquitous. It is also one of the simplest yet most important molecules in living systems. It makes up from 50 to 95 percent of the weight of living organisms. The cytoplasm of a cell is a water-based solution that contains a variety of ions, salts, and molecules which make life ‘happen.’ Water is literally involved in every facet of life.

Figure 2. Polarity of Water Molecule

 

The simplicity of the water molecule belies the complexity of its properties. Based on its small size and light weight, one can predict how it should behave, yet it remains liquid at a much higher temperatures than expected. It also boils and freezes at much too high, or low, of a temperature for a molecule of its size. Many of these unexpected properties of water are due to the fact that water molecules are attracted to each other like small magnets (cohesion). This attraction results in turn from the structure of the water molecule and the characteristics of the atoms it contains.

Each molecule of water is made up of two atoms of hydrogen connected to one atom of oxygen, as shown below. This summarized in the familiar formula, H2O.

Figure 3.  Formation of a Water Molecule

Hydrogen in water will take on a partial positive charge and why oxygen will take on a partial negative charge. This causes a water molecule to be polar, having opposite + and – charges on each end of the molecule. These partial charges cause water molecules to ‘stick’ to each other like magnets. The ‘stickiness’ in this particular case is due to ‘hydrogen bonding‘. In this case, hydrogen bonding involves the attraction between the positively charged hydrogen atom of one water molecule and the negatively charged oxygen atom of another water molecule. As no electrons are actually shared however, hydrogen bonds are much weaker than covalent bonds – they easily break and easily form again.

Figure 4. Hydrogen Bonding in Water

 

Water is everywhere. It’s in the air we breathe. It’s in our sink faucets, and it’s in every cell of our body. Water is an unusual substance with special properties. The properties of water help to answer several questions such as:

  1.  “How does water rise from the roots of a redwood tree to the very top?”
  2.  “How do insects walk on water?”
  3.  “Why does ice float rather than sink?”
  4.  “Why do people become seriously ill, or die, if they go without water for a week or so?”
  5. “How would life in a lake be affected if ice sank and lakes froze from the bottom up? “

In this first lab, we will investigate the properties of water in an attempt to understand how water behaves in relation to both our bodies and the environment. Through a set of experiments, the unique properties of water and its consequent importance to living things will become apparent.

MATERIALS:

chromatography paper strips
detergent
vis-a-vis black ink pens
wax paper
pennies
glue
cooking oil
red food coloring
water
10 ml grad cylinders
50 ml grad. cylinders
beaker
glass slides
stirring rods
medicine droppers
scissors

 

 

 

 

 

Objectives

 

Once you have completed this exercise you should be able to:
1. Describe the polarity of a water molecule and explain how that polarity affects the properties of water.
2. Explain why water climbs the inside of a thin glass capillary but not a thin plastic capillary.
3. Explain why water climbs a paper strip.

Properties of Water

 

Properties of Water

Introduction

Water covers about three quarters of the earth’s surface and makes up about three quarters of our body weight.  In fact, without water, life would not be possible.  This simple fact is why scientists are constantly looking for water on other planets – the presence of water could indicate the presence of life.

We have discussed some of the properties of water in previous lessons.  This lesson will consider water’s properties in more depth.  As you read about the characteristics of water, take some time to think about how these characteristics relate to the fields of water and wastewater treatment.

Water Molecule

As you should remember, water is represented by the formula H2O.  The picture below can also be used to represent water.

Water molecule

Lesson 5 explained how hydrogen bonds form between water molecules.  The ability of water molecules to form hydrogen bonds, as shown below, causes many of water’s unique characteristics.  For example, you should recall that hydrogen bonding makes water an excellent solvent.

Hydrogen bond

 

 

Temperature

Introduction

Water is unique in that it is found as a gas, a liquid, and a solid at natural earth temperatures.  In contrast, most other substances are naturally found in only one or two states.  This property of water is integral to our daily lives, and is especially important in the hydrologic cycle.

On this page, we will consider how water is influenced by temperature.  The surrounding air temperature can change the temperature of water, change water’s state, and change water’s density.

Specific Heat Capacity

Specific heat capacity is the amount of heat required to raise the temperature of one gram of a substance by one degree Celsius.  Every substance has its own specific heat capacity, with the specific heat capacity of water being 1 cal/(g°C).

The specific heat capacity of water is much higher than that of other common substances.  For the sake of comparison, the specific heat capacity of oil is about 0.5 cal/(g°C) and the specific heat capacity of aluminum is about 0.2 cal/(g°C).  This means that it takes a lot more heat to raise the temperature of water compared to the amount of heat it would take to raise the temperature of oil or aluminum.

The high specific heat of water helps the earth’s temperature remain moderate since water traps heat during the day and releases it slowly at night.  As a result, the temperature on earth’s surface does not vary very widely, ranging from extremes of 134°F to -129°F.  For comparison, the moon has no liquid water and its temperatures can range from 240°F to -290°F.  (The lack of atmosphere on the moon, along with other factors, also contributes to the wide range of temperature.)

Boiling Point

Water also has a very high boiling point, meaning that liquid water turns into water vapor at a higher temperature (212°F) than would be expected due to the size and weight of the molecule.  The high boiling point of water is due to the hydrogen bonds which tend to hold water molecules together, preventing them from breaking apart and entering the gaseous state.

Since it takes such a large amount of energy to change the state of water, sweating is a very effective method of cooling the body.  In order to evaporate, the sweat requires the input of a great deal of heat energy, some of which comes from our bodies.  So, as our sweat evaporates, we begin to feel cooler.

Density and Expansion

As you should remember from ENV 110, density is the ratio of mass to volume.  Dense objects feel heavier and tend to sink while less dense objects feel lighter and tend to float.

The density of most objects changes slightly as the temperature changes.  In general, warmer temperatures tend to make substances less dense because the greater random kinetic energy makes the molecules spread out.  The amount that objects expand when heated is known as the coefficient of expansion.

The density of water, once again, is a special case.  Water is most dense at 39°F, and as it cools or warms from this temperature, the water expands slightly.  This means that ice is slightly less dense than cold water, which is why ice floats on the surface of bodies of water.  The floating ice slows the freezing process by insulating the water underneath, which contributes to the moderate temperatures on earth.  In addition, the layer of ice prevents many lakes from freezing solid, allowing fish and other organisms to survive under the ice.

Turnover of a lake

The changing density of water at different temperatures is also responsible for turnover.  Turnover occurs when the water on the surface of a lake cools in the fall.  Eventually, this cold water will become more dense than the warmer water beneath, so the cold water will sink to the bottom and the warm water will rise to the surface.  When lakes are used as the water source for water treatment plants, turnover can cause abrupt changes in the quality of the raw water.

 

 

Other Properties

Surface Tension

In a body of water, hydrogen bonds between water molecules are constantly pulling the molecules in many different directions.  However, at the water’s surface, the molecules are only being pulled from side to side and down, with no hydrogen bonds pulling them upwards.  This results in a skin of water at the surface in which the molecules are held together very tightly.

Surface tension is a measurement of the amount of force required to break this skin on the surface of water.  Other liquids have a surface tension as well, but the surface tension in water is quite strong due to the hydrogen bonds.  The pictures below show some examples of the results of water’s strong surface tension.

Examples of surface tension.

Surface tension is what holds drops of water together in a round shape.  Surface tension allows both water striders and paperclips to float on water even though they are more dense than the water.  In addition, surface tension allows you to fill a cup slightly over the brim with water.

Capillary Action

Surface tension is also responsible for another phenomena known as capillary action.  Capillary action occurs when water climbs upward through a small space, defying gravity due to the forces of adhesion and surface tension.  The image below shows one example of capillary action – a narrow straw was placed in a cup of water and the water crept upwards through the straw.

Capillary action

What causes the movement of water during capillary action?  The first factor is adhesion, the attraction between water and another object.  In this case, adhesion attracted the water within the straw to the surface of the straw.  Molecules of water which came in contact with the straw tended to move upward along the inside of the straw, as shown below:

Adhesion pulls water up the sides of the straw

Water’s surface tension is so strong that, as water is pulled upward along the straw’s walls, the water in between tends to be pulled upward also.  The downward pull of gravity prevents the central water from rising quite as high as the water which is adhered to the straw, so the result is a meniscus, as shown in the first picture in this section.

Capillary action is important in moving water upwards through small spaces.  Plants depend on capillary action to move water upward from the roots to the leaves.  In the soil, capillary action also tends to move water upward between the soil particles.

Review

Water has many unique properties, many of which are based on its molecules’ ability to form hydrogen bonds.  Water is found at earth’s temperatures as a solid, liquid, and gas.  It has a high specific heat capacity and boiling point.  Water is most dense at 39°F.  Water also has a strong surface tension.

Properties of Water

 

Properties of Water

 

Introduction:

Water’s chemical description is H2O. As the diagram to the left shows, that is one atom of oxygen bound to two atoms of hydrogen. The hydrogen atoms are “attached” to one side of the oxygen atom, resulting in a water molecule having a positive charge on the side where the hydrogen atoms are and a negative charge on the other side, where the oxygen atom is. This uneven distribution of charge is called polarity. Since opposite electrical charges attract, water molecules tend to attract each other, making water kind of “sticky.” As the right-side diagram shows, the side with the hydrogen atoms (positive charge) attracts the oxygen side (negative charge) of a different water molecule. (If the water molecule here looks familiar, remember that everyone’s favorite mouse is mostly water, too). This property of water is known as cohesion.

All these water molecules attracting each other mean they tend to clump together. This is why water drops are, in fact, drops! If it wasn’t for some of Earth’s forces, such as gravity, a drop of water would be ball shaped — a perfect sphere. Even if it doesn’t form a perfect sphere on Earth, we should be happy water is sticky. Water is called the “universal solvent” because it dissolves more substances than any other liquid. This means that wherever water goes, either through the ground or through our bodies, it takes along valuable chemicals, minerals, and nutrients.

Water, the liquid commonly used for cleaning, has a property called surface tension. In the body of the water, each molecule is surrounded and attracted by other water molecules. However, at the surface, those molecules are surrounded by other water molecules only on the water side. A tension is created as the water molecules at the surface are pulled into the body of the water. This tension causes water to bead up on surfaces (glass, fabric), which slows wetting of the surface and inhibits the cleaning process. You can see surface tension at work by placing a drop of water onto a counter top. The drop will hold its shape and will not spread.

In the cleaning process, surface tension must be reduced so water can spread and wet surfaces. Chemicals that are able to do this effectively are called surface active agents, or surfactants. They are said to make water “wetter.” Surfactants perform other important functions in cleaning, such as loosening, emulsifying (dispersing in water) and holding soil in suspension until it can be rinsed away. Surfactants can also provide alkalinity, which is useful in removing acidic soils.

Pre-Lab Questions (Click here)

Materials:

Box of small paper clips, small plastic container, eyedropper, cup, stirring rod, water, liquid soap, plastic tray

Procedure (Part A) Cohesiveness of Water:

  1. Estimate how many paper clips will fit into a completely full cup of water. Record this number in data table 1.
  2. Place your small container on a tray to contain any water that may spill.
  3. Fill a plastic cup with tap water.
  4. Pour tap water from your cup into your small container.
  5. Continue to add water by eyedropper until the top surface appears rounded.
  6. Slowly add paper clips one at a time to the cup keeping count of all paper clips that you add.
  7. Stop adding paper clips to the container whenever water spills from the top.
  8. Record your paper clip count. Compare the actual number of paper clips to the estimated number.

Procedure (Part B) Soap’s effect on Surface Tension:

  1. Again estimate how many paper clips will fit into a completely full cup of soapy water. Record this number in data table 2.
  2. Place your small container on a tray to contain any water that may spill.
  3. Fill a plastic cup with tap water.
  4. Add several drops of liquid soap & use a stirring rod to mix.
  5. Pour soapy water from your cup into your small container.
  6. Continue to add soapy water by eyedropper until the top surface appears rounded.
  7. Slowly add paper clips one at a time to the cup keeping count of all paper clips that you add.
  8. Stop adding paper clips to the container whenever water spills from the top.
  9. Record your paper clip count. Compare the actual number of paper clips to the estimated number.

Data:

Table 1

 

Cohesiveness of Tapwater
Estimated Number of Paper Clips Actual Number of paper Clips Difference
 

 

 

Table 2

 

Cohesiveness of Soapy water
Estimated Number of Paper Clips Actual Number of paper Clips Difference
 

 

 

Questions: 

1. How did your estimated number compare to your actual number?

2. What happened to the surface of the water as more clips were added?

 

3. What property of water was shown in Part A?

4. How is this property of water used in nature?

5. Explain why water shows surface tension.

 

6. Explain why water is a polar molecule and include a diagram of several water molecules in a drop of water.

 

 

7. In order to clean a surface, what must happen to surface tension?

 

8. What is the job of a surfactant?

 

9. Name a surfactant used in Part B?

10. Using your data from Part B, explain what proof you gathered in Part B to support your answer to question 9.