BIOLOGY. Water and Life CAMPBELL. Reece Urry Cain Wasserman Minorsky Jackson. Lecture Presentation by Nicole Tunbridge and Kathleen Fitzpatrick

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1 CAMPBELL BIOLOGY TENTH EDITION Reece Urry Cain Wasserman Minorsky Jackson 3 Water and Life Lecture Presentation by Nicole Tunbridge and Kathleen Fitzpatrick 2014 Pearson Education, Inc.

2 Overview: The Molecule That Supports All of Life Water is the biological medium on Earth. All organisms are made of mostly water (75-90%) and live in an environment surrounded by water. Water is the only common substance in the natural environment that exists in all three physical states of matter: solid, liquid, and gas. Three-quarters of Earth s surface is submerged in water. The abundance of water is the main reason the Earth is habitable. Water s unique emergent properties help make Earth suitable for life Life on Earth began in water and evolved there for 3 billion years before spreading onto land.

3 Figure 3.1

4 The polarity of water molecules results in hydrogen bonding In the water molecule, the electrons of the polar covalent bonds spend more time near the oxygen than the hydrogen The water molecule is a polar molecule: The opposite ends have opposite charges Polarity allows water molecules to form hydrogen bonds with each other Figure 3.2

5 Hydrogen Bonds and Water Each water molecule can form hydrogen bonds with as many as four neighbors. When water is in its liquid form, its hydrogen bonds are very fragile, about one-twentieth as strong as covalent bonds. Hydrogen bonds form, break, and re-form with great frequency. Each hydrogen bond lasts only a few trillionths of a second, but the molecules continuously form new hydrogen bonds with a succession of partners. At any given instant, a substantial percentage of all water molecules are hydrogen-bonded to their neighbors Pearson Education, Inc.

6 Four emergent properties of water contribute to Earth s suitability for life Four of water s properties that facilitate an environment for life are: Cohesive behavior Ability to moderate temperature Expansion upon freezing Versatility as a solvent

7 Cohesion Collectively, hydrogen bonds hold water molecules together, a phenomenon called cohesion Cohesion helps the transport of water against gravity in plants Adhesion is an attraction between different substances, for example, between water and plant cell walls

8 Fig. 3-3 Adhesion of H 2 O with cell walls resists gravity s downward pull Due to hydrogen bonding between H 2 O molecules holds a column of H 2 O within the cells. Evaporation through Leaves pulls water upward Via water conducting cells. Copyright 2011 Pearson Education, Inc

9 Surface Tension Surface tension is a measure of the force necessary to stretch or break the surface of a liquid, is related to cohesion. Water has a greater surface tension than most other liquids because hydrogen bonds among surface water molecules resist stretching or breaking the surface. Water behaves as if covered by an invisible film. Some animals can stand, walk, or run on water without breaking the surface. Fig. 3-4.

10 Moderation of Temperature Water absorbs heat from warmer air and releases stored heat to cooler air to moderate temperature. Water can absorb or release a large amount of heat with only a slight change in its own temperature.

11 Heat and Temperature Atoms and molecules are always in motion. Kinetic energy is the energy of motion Heat is a measure of the total amount of kinetic energy due to molecular motion. Thermal energy in transfer from one body of matter to another is defined as heat. Temperature measures the intensity of heat due to the average kinetic energy of molecules. When two objects of different temperatures come together, heat passes from the warmer object to the cooler object until the two are the same temperature.

12 Temperature In biology, temperature is measured on the Celsius scale ( C). At sea level, water freezes at 0 C and boils at 100 C. Human body temperature is typically 37 C.

13 Heat Energy Although there are several ways to measure heat energy, one convenient unit is the calorie (cal). One calorie is the amount of heat energy necessary to raise the temperature of 1 g of water by 1 C. A calorie is released when 1 g of water cools by 1 C. In many biological processes, the kilocalorie (kcal) is a more commonly used unit. One kilocalorie is the amount of heat energy necessary to raise the temperature of 1000 g of water by 1 C. Another common energy unit, the joule (J), is equivalent to cal or 1 cal = J...

14 Water s High Specific Heat The specific heat of a substance is the amount of heat that must be absorbed or lost for 1 g of that substance to change its temperature by 1ºC The specific heat of water is 1 cal/g/ºc Water resists changing its temperature because of its high specific heat. Water s high specific heat can be traced to hydrogen bonding Heat is absorbed when hydrogen bonds break Heat is released when hydrogen bonds form The high specific heat of water minimizes temperature fluctuations to within limits that permit life.

15 Why do we care? Figure 3.5 Water absorbs or releases a relatively large quantity of heat for each degree of temperature change. A large body of water can absorb a large amount of heat from the sun during the daytime in the summer and yet warm only a few degrees. At night and during the winter, the warm water heats the cooler air. Therefore, the oceans and coastal land areas have more stable temperatures than inland areas.

16 Evaporative Cooling Evaporation is transformation of a substance from liquid to gas Vaporization occurs when a molecule moves fast enough to overcome the attraction of other molecules in the liquid. Heat of vaporization is the heat a liquid must absorb for 1 g to be converted to gas. As a liquid evaporates, its remaining surface cools, a process called evaporative cooling Evaporative cooling of water helps stabilize temperatures in organisms and bodies of water

17 Fig. 3-6 Insulation of Bodies of Water by Floating Ice Hydrogen bond Ice Hydrogen bonds are stable Liquid water Hydrogen bonds break and re-form Ice floats in liquid water because hydrogen bonds in ice are more ordered, making ice less dense Water reaches its greatest density at 4 C If ice sank, all bodies of water would eventually freeze solid, making life impossible on Earth. Many scientists are worried that global warming, caused by carbon dioxide and other greenhouse gases, is having a profound effect on icy environments around the globe The rate at which glaciers and Arctic sea ice are disappearing is posing an extreme challenge to animals that depend on ice for their survival

18 Water is a common solvent of Life A liquid that is a completely homogeneous mixture of two or more substances is called a solution. A sugar cube in a glass of water eventually dissolves to form a uniform solution of sugar and water. The dissolving agent is the solvent, and the substance that is dissolved is the solute. In our example, water is the solvent and sugar is the solute. In an aqueous solution, water is the solvent. Water is a versatile solvent due to its polarity, which allows it to form hydrogen bonds easily When an ionic compound is dissolved in water, each ion is surrounded by a sphere of water molecules called a hydration shell

19 NaCl Dissolves in H 2 O Water is an effective solvent because it readily forms hydrogen bonds with charged and polar covalent molecules. For example, when a crystal of salt (NaCl) is placed in water, the Na+ cations interact with the partial negative charges of the oxygen regions of water molecules. The Cl anions interact with the partial positive charges of the hydrogen regions of water molecules. Figure 3.7

20 δ + δ δ δ + Figure 3.8 Water can also dissolve compounds made of nonionic polar molecules. Even large polar molecules such as proteins can dissolve in water if they have ionic and polar regions.

21 Hydophilic Substances A substance that has an affinity for water is hydrophilic (water-loving). Hydrophilic substances are dominated by ionic or polar bonds. Some hydrophilic substances do not dissolve because their molecules are too large.

22 Hydrophobic Substances Substances that have no affinity for water are hydrophobic (water-fearing). Hydrophobic substances are nonionic and have nonpolar covalent bonds. Because no regions consistently have partial or full charges, water molecules cannot form hydrogen bonds with hydrophobic molecules. Oils such as vegetable oil are hydrophobic because the dominant bonds, carbon-carbon and carbon-hydrogen, share electrons equally. Hydrophobic molecules are components of cell membranes. A colloid is a stable suspension of fine particles in a liquid

23 Molecular Mass We know the mass of each atom in a given molecule, so we can calculate its molecular mass, which is the sum of the masses of all the atoms in a molecule. We measure the number of molecules in units called moles. The actual number of molecules in a mole is called Avogadro s number, Let us calculate how can make 1 mole of table sugar Glucose solution?

24 Moles and Mass How can we measure 1 mole of glucose (C 6 H 12 O 6 )? From the Periodic Table we know that carbon atom weighs- 12 daltons, hydrogen 1 dalton, and oxygen 16 daltons. So C=6X12=72, H=1X12=12, O=6X16=96; Total is =180 One molecule of sucrose weighs 180 daltons, the sum of the weights of all the atoms in glucose, or the molecular weight of glucose. So chemists/biologists use a measure of molar mass that we can actually measure in the lab, in GRAM.To get 1 mole of sucrose, we would weigh out 180 g.

25 Molarity Molarity (M) is the number of moles of solute per liter of solution. A one-molar (1 M) solution has 1 mole of a substance dissolved in 1 liter of a solvent. To make a 1 M solution of glucose (C 6 H 12 O 6 ), we would slowly add water to 180 g of glucose until the total volume was 1 liter and all the sugar was dissolved.

26 Possible Evolution of Life on Other Planets with Water. The remarkable properties of water support life on Earth in many ways Astrobiologists seeking life on other planets are concentrating their search on planets with water To date, more than 200 planets have been found outside our solar system; one or two of them contain water In our solar system, Mars has been found to have water Figure 3.9 Evidence for subsurface liquid water on Mars

27 Acidic and basic conditions affect living organisms A hydrogen atom in a hydrogen bond between two water molecules can shift from one to the other:. The hydrogen atom leaves its electron behind and is transferred as a proton, or hydrogen ion (H+) The molecule with the extra proton is now a hydronium ion (H3O+), though it is often represented as H+ The molecule that lost the proton is now a hydroxide ion (OH )

28 A simplified way to view this process is to say that a water molecule dissociates into a hydrogen ion and a hydroxide ion: H 2 O H + + OH At equilibrium, the concentration of water molecules greatly exceeds the concentration of H+ and OH. Although the dissociation of water is reversible and statistically rare, it is very important in the chemistry of life. Because hydrogen and hydroxide ions are very reactive, changes in their concentrations can drastically affect the chemistry of a cell.

29 Effects of Changes in ph Concentrations of H + and OH are equal in pure water Adding certain solutes, called acids and bases, modifies the concentrations of H + and OH Biologists use the ph scale to describe whether a solution is acidic or basic

30 What are acids and bases? An acid is any substance that increases the H + concentration of a solution When hydrochloric acid is added to water, hydrogen ions dissociate from chloride ions: HCl H + + Cl The extra H + generated means the solution will have more H + than OH -

31 Bases A base is any substance that reduces the H + concentration of a solution Some bases reduce the H+ concentration directly by accepting hydrogen ions. Ammonia (NH3) acts as a base when the nitrogen s unshared electron pair attracts a hydrogen ion from the solution, creating an ammonium ion (NH4+): NH 3 + H + NH 4+. Other bases reduce the H+ concentration indirectly by dissociating to OH, which then combines with H+ to form water. NaOH Na + + OH OH + H + H 2 O

32 Weak and Strong Strong acids and bases, like HCl and NaOH, dissociate completely when mixed with water. Weak acids are like carbonic acid or acetic acid i.e. vinegar and weak bases ammonia or baking soda, are reversible reactions so they reversibly release and accept hydrogen ions.

33 The ph Scale In any aqueous solution at 25 C, the product of the H+ and OH- concentrations is constant at M. Brackets ([H+] and [OH ]) indicate the molar concentration of the enclosed substance. [H+] [OH ] = In a neutral solution, [H+] = 10 7 M and [OH ] = 10 7 M. Solutions with more OH than H+ are basic solutions; solutions with more H+ than OH- are acidic; solutions in which the concentrations of OH- and H+ are equal are neutral. H+ and OH concentrations are typically expressed with the ph scale.

34 The ph Scale The ph (scale = 1 to 14) of a solution is defined by the negative logarithm of H + concentration, written as ph = log [H + ] For a neutral aqueous solution [H + ] is 10 7 = ( 7) = 7 The ph decreases as the H+ concentration increases. Most biological fluids have ph values in the range of 6 to 8 for example our blood ph is 7.4.

35 Acids and Bases An acid is any substance that increases the H + concentration of a solution A base is any substance that reduces the H + concentration of a solution Acidic solutions have ph values less than 7 Basic solutions have ph values greater than 7 Most biological fluids have ph values in the range of 6 to 8

36 The ph Scale Each ph unit represents a tenfold difference in H+ and OH concentrations. A small change in ph indicates a substantial change in H+ and OH concentrations. A solution of ph 2 is not twice as acidic as a solution of ph 4 but 1,00 times more acidic!

37 Figure 3.10 ph Scale 0 1 Battery acid H + H+ H + H + OH OH H + H + H + H + Acidic solution OH OH H + H + OH OH OH H + H + H+ Neutral solution OH OH OH H + OH OH OH H + OH Basic solution Increasingly Acidic [H + ] > [OH ] Neutral [H + ] = [OH ] Increasingly Basic [H + ] < [OH ] Gastric juice, lemon juice Vinegar, wine, cola Tomato juice Beer Black coffee Rainwater Urine Saliva Pure water Human blood, tears Seawater Inside of small intestine Milk of magnesia Household ammonia Household bleach Oven cleaner

38 Buffers The internal ph of most living cells must remain close to ph 7 Buffers are substances that minimize changes in concentrations of H + and OH in a solution Most buffers consist of an acid-base pair that reversibly combines with H +

39 Buffers Buffers resist changes in the ph of a solution when H+ or OH is added to the solution. Buffers accept hydrogen ions from the solution when they are in excess and donate hydrogen ions when they have been depleted. Buffers typically consist of a weak acid and its corresponding base. One important buffer in human blood and other biological solutions is carbonic acid (H 2 CO 3 ), formed when CO 2 reacts with water in blood plasma. Carbonic acid dissociates to yield a bicarbonate ion (HCO 3 -) and a hydrogen ion (H+). The chemical equilibrium between carbonic acid and bicarbonate acts as a ph regulator. The equilibrium shifts left or right as other metabolic processes add or remove H+ from the solution. H 2 CO 3 HCO H + H= donor (acid) H+ acceptor (base)

40 Acidification: A Threat to Water Quality Human activities such as burning fossil fuels threaten water quality CO 2 is the main product of fossil fuel combustion About 25% of human-generated CO 2 is absorbed by the oceans CO 2 dissolved in sea water forms carbonic acid; this process is called ocean acidification

41 Figure 3.11 CO 2 CO 2 + H 2 O H 2 CO 3 H 2 CO 3 H + + HCO 3 H + + CO 3 2 HCO 3 CO Ca 2+ CaCO 3

42 As seawater acidifies, H + ions combine with carbonate ions to produce bicarbonate Carbonate is required for calcification (production of calcium carbonate) by many marine organisms, including reef-building corals We have made progress in learning about the delicate chemical balances in oceans, lakes, and rivers

43 Figure 3.12 IMPACT: The Threat of Ocean Acidification to Coral Reef Ecosystems (a) (b) (c)

44 The burning of fossil fuels is also a major source of sulfur oxides and nitrogen oxides These compounds react with water in the air to form strong acids that fall in rain or snow Acid precipitation is rain, fog, or snow with a ph lower than 5.2 Acid precipitation damages life in lakes and streams and changes soil chemistry on land