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Biochemical Properties of Water - Advanced Loading... Found a content error?
We will now look at a few of the properties of water.
It should be clear now, that water is an amazing compound, and that without its unique properties, life on Earth would definitely not be possible.
Explain why water takes a long time to heat up, but the pot that you are heating it in gets hot quickly.
We are asked why water takes a long time to heat up compared to the pot you are heating it in. The property that applies here is the high specific heat of water. The other properties of water do not apply here since we are comparing the pot to the water and the pot is not changing phase.
Water has a high specific heat, while the metal that the pot is made of does not. The metal pot needs less energy to heat it up and so it gets hotter faster. Water needs a lot of energy to change its temperature and so it takes longer to get hot. An experiment for informal assessment is included in this chapter. This experiment is very similar to the one on intermolecular forces. In this experiment learners focus on the properties of water. This is a good experiment to do to guide learners in understanding the properties of water. When working with Bunsen burners learners should ensure that loose clothing is tucked away and long hair is tied back. As always with chemistry experiments you should open all the windows to ensure a well ventilated room. At the end of the experiment check that all Bunsen burners are turned off. If learners leave the beaker of water on the Bunsen burner for to long and the water starts to boil or steam is observed, then make sure the learners do not touch the beaker as they will be burn themselves. Carry out some research into: water bags on cars, clay pots and carafes for water and safe or “cool” rooms to keep food cool. Find out which people groups use these things and how the properties of water help in each case. Textbook Exercise 4.3
What property of ice cubes allows them to float in the water?
Ice cubes are less dense than liquid water. Water has a less dense solid phase than solid water.
Briefly describe how this property affects the survival of aquatic life during winter.
If the ice did not float on top of the water then all bodies of water would freeze from the bottom up. This would mean that aquatic life would not be able to survive through the cold winters as there would be no habitat for them.
Which properties of water allow it to remain in its liquid phase over a large temperature range? Explain why this is important for life on earth.
High boiling point and low melting point. Water has strong hydrogen bonds between molecules. These bonds require a lot of energy before they will break. This leads to water having a higher boiling point than if there were only weaker dipole-dipole forces. Water also has a high specific heat. If water did not have such a large range in which it is a liquid, bodies of water would freeze over faster, destroying the life in them. Also if the boiling point of water was lower, then all the water could evaporate on a hot day, which would cause all life to die.
Which property of water allows the oceans to act as heat reservoirs? What effect does this have on the Earths climate?
Water is able to absorb infrared radiation (heat) from the sun. This heat energy is stored in the oceans. Without this effect, the heat from the sun would cause the daytime temperatures on the Earth to become unbearably hot.
Learning Outcomes
Do you ever wonder why scientists spend time looking for water on other planets? It is because water is essential to life; even minute traces of it on another planet can indicate that life could or did exist on that planet. Water is one of the more abundant molecules in living cells and the one most critical to life as we know it. Approximately 60–70 percent of your body is made up of water. Without it, life simply would not exist. Water Is PolarThe hydrogen and oxygen atoms within water molecules form polar covalent bonds. The shared electrons spend more time associated with the oxygen atom than they do with hydrogen atoms. There is no overall charge to a water molecule, but there is a slight positive charge on each hydrogen atom and a slight negative charge on the oxygen atom. Because of these charges, the slightly positive hydrogen atoms repel each other and form the unique shape seen in Figure 2. Each water molecule attracts other water molecules because of the positive and negative charges in the different parts of the molecule. Water also attracts other polar molecules (such as sugars), forming hydrogen bonds. When a substance readily forms hydrogen bonds with water, it can dissolve in water and is referred to as hydrophilic (“water-loving”). Hydrogen bonds are not readily formed with nonpolar substances like oils and fats (Figure 1). These nonpolar compounds are hydrophobic (“water-fearing”) and will not dissolve in water. Water Stabilizes TemperatureThe hydrogen bonds in water allow it to absorb and release heat energy more slowly than many other substances. Temperature is a measure of the motion (kinetic energy) of molecules. As the motion increases, energy is higher and thus temperature is higher. Water absorbs a great deal of energy before its temperature rises. Increased energy disrupts the hydrogen bonds between water molecules. Because these bonds can be created and disrupted rapidly, water absorbs an increase in energy and temperature changes only minimally. This means that water moderates temperature changes within organisms and in their environments. As energy input continues, the balance between hydrogen-bond formation and destruction swings toward the destruction side. More bonds are broken than are formed. This process results in the release of individual water molecules at the surface of the liquid (such as a body of water, the leaves of a plant, or the skin of an organism) in a process called evaporation. Evaporation of sweat, which is 90 percent water, allows for cooling of an organism, because breaking hydrogen bonds requires an input of energy and takes heat away from the body. Conversely, as molecular motion decreases and temperatures drop, less energy is present to break the hydrogen bonds between water molecules. These bonds remain intact and begin to form a rigid, lattice-like structure (e.g., ice) (Figure 3a). When frozen, ice is less dense than liquid water (the molecules are farther apart). This means that ice floats on the surface of a body of water (Figure 3b). In lakes, ponds, and oceans, ice will form on the surface of the water, creating an insulating barrier to protect the animal and plant life beneath from freezing in the water. If this did not happen, plants and animals living in water would freeze in a block of ice and could not move freely, making life in cold temperatures difficult or impossible. Water Is an Excellent SolventBecause water is polar, with slight positive and negative charges, ionic compounds and polar molecules can readily dissolve in it. Water is, therefore, what is referred to as a solvent—a substance capable of dissolving another substance. The charged particles will form hydrogen bonds with a surrounding layer of water molecules. This is referred to as a sphere of hydration and serves to keep the particles separated or dispersed in the water. In the case of table salt (NaCl) mixed in water (Figure 4), the sodium and chloride ions separate, or dissociate, in the water, and spheres of hydration are formed around the ions. A positively charged sodium ion is surrounded by the partially negative charges of oxygen atoms in water molecules. A negatively charged chloride ion is surrounded by the partially positive charges of hydrogen atoms in water molecules. These spheres of hydration are also referred to as hydration shells. The polarity of the water molecule makes it an effective solvent and is important in its many roles in living systems. Water Is CohesiveHave you ever filled up a glass of water to the very top and then slowly added a few more drops? Before it overflows, the water actually forms a dome-like shape above the rim of the glass. This water can stay above the glass because of the property of cohesion. In cohesion, water molecules are attracted to each other (because of hydrogen bonding), keeping the molecules together at the liquid-air (gas) interface, although there is no more room in the glass. Cohesion gives rise to surface tension, the capacity of a substance to withstand rupture when placed under tension or stress. When you drop a small scrap of paper onto a droplet of water, the paper floats on top of the water droplet, although the object is denser (heavier) than the water. This occurs because of the surface tension that is created by the water molecules. Cohesion and surface tension keep the water molecules intact and the item floating on the top. It is even possible to “float” a steel needle on top of a glass of water if you place it gently, without breaking the surface tension (Figure 5). These cohesive forces are also related to the water’s property of adhesion, or the attraction between water molecules and other molecules. This is observed when water “climbs” up a straw placed in a glass of water. You will notice that the water appears to be higher on the sides of the straw than in the middle. This is because the water molecules are attracted to the straw and therefore adhere to it. Cohesive and adhesive forces are important for sustaining life. For example, because of these forces, water can flow up from the roots to the tops of plants to feed the plant.
Which of the following statements is not true?
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