Water and the Fitness of the Environment Chapter 3.

Slides:



Advertisements
Similar presentations
Water and the Environment
Advertisements

Copyright © 2005 Pearson Education, Inc. publishing as Benjamin Cummings PowerPoint Lectures for Biology, Seventh Edition Neil Campbell and Jane Reece.
Water.
M. Saadatian Water 1. Water Water contributes to the fitness of the environment to support life. Life on earth probably.
CHAPTER 3 WATER AND THE FITNESS OF THE ENVIRONMENT 1.The polarity of water molecules results in hydrogen bonding 2.Organisms depend on the cohesion of.
Water has unusual properties: the key is that the electrons of each covalent bond are not shared equally between oxygen and hydrogen atoms. Oxygen pulls.
Chapter 3 Water and the Fitness of the Environment.
Water.  Water is the biological medium on Earth  All living organisms require water more than any other substance  Most cells are surrounded by water,
Should we control a chemical that: Causes excessive sweating and vomiting. Causes excessive sweating and vomiting. Is a major component in acid rain. Is.
The Single most abundant compound in most living things
Water – Chapter 3.
Water and Fitness in the Environment
Chapter 3 Water and the Fitness of the Environment
50-95% of any functioning living system. 98% of water on earth is in liquid form.
CHAPTER 2 Water and Life
Copyright © 2005 Pearson Education, Inc. publishing as Benjamin Cummings Water and the Fitness of the Environment Chapter 3.
Chapter 3: WATER AND THE FITNESS OF THE ENVIRONMENT.
Water and the Fitness of the Environment Chapter 3 Biology – Campbell Reece.
WATER’S LIFE-SUPPORTING PROPERTIES. Water’s polarity leads to hydrogen bonding and other unusual properties The charged regions on water molecules are.
Figure 3.2 Hydrogen bonds between water molecules Evolution Living cells are 70-95% H2O H2O covers 3/4 of the planet Solid Liquid Gas Polarity and H-bonds.
NOTES: 2.2 – Properties of Water. Water Overview… Water is perhaps the most important compound in living organisms Because so many substances can dissolve.
Water: The Molecule of Life
Chapter 3 Water and the Fitness of the Environment.
10/8/14 Objective: What are the properties of water? Do Now: Take out your HW Chapter 4: The Chemical Basis of Life.
 Chapter 3 Water & The Fitness of the Environment.
Happy Wednesday 9/2/15 Hand in Mealworm lab Chemistry Quiz
Properties of Water Polar molecule Cohesion and adhesion High specific heat Density – greatest at 4 o C Universal solvent of life.
Water.
Water. Water  2 Hydrogen atoms + 1 Oxygen atom covalently bonded (polar)  Makes up 70-95% of living things, covers 75% of Earth  DRAW and LABEL this.
Copyright © 2005 Pearson Education, Inc. publishing as Benjamin Cummings PowerPoint Lectures for Biology, Seventh Edition Neil Campbell and Jane Reece.
Copyright © 2005 Pearson Education, Inc. publishing as Benjamin Cummings Water and the Fitness of the Environment Figure 3.1.
Properties of Water.
Copyright © 2008 Pearson Education, Inc., publishing as Pearson Benjamin Cummings PowerPoint ® Lecture Presentations for Biology Eighth Edition Neil Campbell.
Chapter 3 Water and the Fitness of the Environment.
CH. 3 Water and the Fitness of the Environment. The Effects of Water’s Polarity The polarity of water molecules results in hydrogen bonding Organisms.
Water. Properties of Water Polar molecule Cohesion and adhesion High specific heat Density – greatest at 4 o C Universal solvent of life.
Water Mrs. Hedges Properties of Water Polar molecule Cohesion and adhesion High specific heat Density – greatest at 4 o C Universal solvent of.
Unique Properties of Water
Water and the Fitness of the Environment. Polarity of Water Water is a polar molecule Water is a polar molecule Hydrogen of one H 2 O is attracted to.
1 Water and the Fitness of the Environment chapter 3.
Chapter 3 Notes Water and the Fitness of the Environment.
Properties of Water.
Water and the Fitness of the Environment
The Biological Medium on Earth.  To get the most out of these notes, you MUST read along with pages in the textbook  Not everything in these pages.
 Water The molecule that supports all life.. The impact of water  Water is the biological medium on Earth  All organisms require more water than any.
Properties of Water. Polar molecule Cohesion and adhesion High specific heat Density – greatest at 4 o C Universal solvent of life.
Chapter 3 Water and the Fitness of the Environment Mr. Karns AP biology notes.
CAMPBELL BIOLOGY Reece Urry Cain Wasserman Minorsky Jackson © 2014 Pearson Education, Inc. TENTH EDITION CAMPBELL BIOLOGY Reece Urry Cain Wasserman Minorsky.
Water is a Polar Molecule! What is the molecular formula of water? Draw water and label it. Place a negative sign by oxygen and a positive sign by the.
1. 2 Polarity of Water In a water molecule two hydrogen atoms form single polar covalent bonds with an oxygen atom. Gives water more structure than other.
Water ä Water is necessary for life ä Life evolved in water.
Water and the Fitness of the Environment (for life) Chapter 3.
Chapter 3: Water and the Fitness of the Environment
NOTES: 2.2 – Properties of Water
Chapter 3 – Water and Fitness of the Environment
Properties of Water.
Water and the Fitness of the Environment
Properties of Water Polar molecule Cohesion and adhesion
Chapter 3: Water AP Biology
Chapter 3 Water.
Water and the Fitness of the Environment
WATER AND THE FITNESS OF THE ENVIRONMENT
Chapter 2 Section 5 Bozeman Tutorial -- Water: A Polar Molecule (8:36)
Water and the Fitness of the Environment
Water and the Fitness of the Environment
Chapter 2: The Molecules of Cells
Water and the Fitness of the Environment
Overview: The Molecule That Supports All of Life
Fig. 3-1 Figure 3.1 Why does the abundance of water allow life to exist on the planet Earth?
Presentation transcript:

Water and the Fitness of the Environment Chapter 3

Water Life depends on water Human body and cells  % water Abundance of water  Earth can support life Water exists in three possible states: ice, liquid, and vapor

Properties of Water Polar Molecule Cohesion- Adhesion High Surface Tension High Specific Heat Low Density of ice Excellent solvent

Structure of Water Water is a polar molecule  uneven distribution of charge between the hydrogen and oxygen atoms  regions of partial + and – charges Each water molecule can form H- bonds with up to 4 neighbors.

Structure of Water

Cohesion - Adhesion Cohesion  tendency of molecules of the same kind to stick together. Strongest in water. Adhesion  attraction between unlike molecules

Cohesion - Adhesion

Surface Tension Surface Tension  a measure of how difficult it is to stretch or break the surface of a liquid At the surface water molecules are H- bonded to one another and to the water molecules below  resist stretching or breaking the surface Water behaves as if covered by an invisible film.

Water Moderates Temperatures on Earth Water stabilizes air temperatures  absorbing heat from warmer air and releasing heat to cooler air. Water is a heat bank  can absorb or release relatively large amounts of heat with only a slight change in its own temperature

Heat and Temperature Kinetic Energy  the energy of motion Heat is a measure of the total quantity of kinetic energy due to molecular motion in a body of matter. Temperature measures the intensity of heat due to the average kinetic energy of molecules When two object of different temperature meet, heat passes from the warmer to the cooler until the two are the same temperature.

Temperature is measured on the Celsius scale ( o C).  At sea level, water freezes at O o C and boils at 100 o C.  Human body temperature averages 37 o C. Heat energy = calorie (cal)  One calorie is the amount of heat energy necessary to raise the temperature of 1 g of water by 1 o C.  Biological processes  the kilocalorie (kcal) A kilocalorie is the amount of heat energy necessary to raise the temperature of 1000g of water by 1 o C. The joule (J), is equivalent to cal

High Specific Heat Water’s high specific heat is due to hydrogen bonding Water resists changes in temperature because it takes a lot of energy to speed up its molecules.

Evaporative Cooling As a liquid evaporates, the surface of the liquid that remains behind cools - evaporative cooling.  This occurs because the most energetic molecules are the most likely to evaporate, leaving the lower kinetic energy molecules behind. Evaporative cooling moderates temperature in lakes and ponds and prevents terrestrial organisms from overheating.  Evaporation of water from the leaves of plants or the skin of humans removes excess heat.

Low Density of Ice Water is unusual because it is less dense as a solid than as a liquid. Ice floats on the cool water below. This has important consequences for life.

Low Density of Ice If ice sank  all ponds, lakes, and oceans would freeze solid. The surface layer of ice insulates liquid water below, preventing it from freezing and allowing life to exist under the frozen surface.

Water is the Solvent of Life A liquid that is a completely homogeneous mixture of two or more substances is called a solution The dissolving agent is the solvent and the substance that is dissolved is the solute. In an aqueous solution, water is the solvent.

Water as an Aqueous Solution C 6 H 12 O 6  6(12)+12(1)+6(16)=180g= MW 180g =1 mole of glucose Add 1L H2O Avogadro's number 6.02x10 23 molecules /mole

Water surrounds and separates the positive and negative ions

The Dissociation of Water A hydrogen atom shared by two water molecules shifts from one molecule to the other.  leaves its electron behind and is transferred as a single proton - a hydrogen ion (H + ).  molecule that lost a proton is now a hydroxide ion (OH - ).

Dissociation of Water Water molecule dissociates into a hydrogen ion and a hydroxide ion:  H 2 O H + + OH - (reaction is reversible) At equilibrium the concentration of water molecules greatly exceeds that of H + and OH In pure water only one water molecule in every 554 million is dissociated.  At equilibrium the concentration of H + or OH - is M (25°C)  Adding acids or bases can change this equilibrium and modify the the conc. of H + and OH -

Acids and Bases Acid  compound that donates H+ ions Hydrochloric acid, added to water, hydrogen ions dissociate from chloride ions:  HCl -> H + + Cl - Addition of an acid makes a solution more acidic

Acids and Bases Base  compounds that donate OH- ions or removes H+ ions Some bases reduce H + directly by accepting hydrogen ions. Ammonia (NH 3 ) acts as a base when the nitrogen’s unshared electron pair attracts a hydrogen ion from the solution, creating an ammonium in (NH 4 + ).  NH 3 + H + NH 4 + Other bases reduce H + indirectly by dissociating to OH - that combines with H + to form water.  NaOH -> Na + + OH - OH - + H + -> H 2 O Solutions with more OH - than H + are basic solutions.

pH Scale The scale that describes how acid or basic a solution is. Ranges from 0-14 pH 2 is 10X more acidic than pH 3 pH 7 is neutral

pH Scale In any solution the product of their H + and OH - concentrations is constant at pH = -log[H + ]  [H + ] [OH - ] =  If [H + ] = M,then [OH - ] = M  In a neutral solution, [H + ] = M and [OH - ] = M, pH =7

pH Scale The pH of a neutral solution is 7. Acidic solutions have pH values less than7 and basic solutions have pH values more than 7. Most biological fluids have pH values in the range of 6 to 8. However, pH values in the human stomach can reach 2. Each pH unit represents a tenfold difference in H + and OH - concentrations. A small change in pH actually indicates a substantial change in H + and OH - concentrations

Buffers Substances that can prevent or resist sharp changes in pH Important – because molecules in cells are very sensitive to concentrations of H+ or OH- ions. Even the slightest maybe harmful to living things

Buffers typically consist of a weak acid and its corresponding base Buffer in human blood and other biological solutions is carbonic acid.  The chemical equilibrium between carbonic acid and bicarbonate acts at a pH regulator.  The equilibrium shifts left or right as other metabolic processes add or remove H + from the solution.

Carbonate-bicarbonate buffer

Acid Precipitation Uncontaminated rain has a slightly acidic pH of 5.6. The acid is a product of the formation of carbonic acid from carbon dioxide and water. Acid precipitation occurs when rain, snow, or fog has a pH that is more acidic than 5.6. Effects of acid rain??