Upload
jesus
View
43
Download
0
Tags:
Embed Size (px)
DESCRIPTION
Chapter 3: Water and Life. Essential Knowledge. 2.a.3 – Organisms must exchange matter with the environment to grow, reproduce, and maintain organization (3.1-3.3). 7 Properties of Water. 1) Cohesive 2) Adhesive 3) High surface tension 4) Stabilizes temperatures - PowerPoint PPT Presentation
Citation preview
Chapter 3: Water and Life
Essential Knowledge
2.a.3 – Organisms must exchange matter with the environment to grow, reproduce, and maintain organization (3.1-3.3).
7 Properties of Water 1) Cohesive 2) Adhesive 3) High surface tension 4) Stabilizes temperatures 5) High heat of vaporization 6) Expands when frozen 7) Versatile solvent
1) Liquid Water Is Cohesive Water sticks to water. Why?
• Because the polarity of water results in hydrogen bonding.
Contributes to transport of nutrients (plants)
2) Liquid Water is Adhesive Water sticks to other molecules. Why?
• Hydrogen bonding. Plants:
• Water adheres to cell walls (helps pull water and nutrients through plant)
Water transport in trees uses Cohesion and Adhesion
3) Water Has A High Surface Tension
The surface of water is difficult to stretch or break.
Why? Hydrogen bonding. Greater surf tension than most
liquids
4) Water Stabilizes Temperature Water can absorb and store a huge
amount of heat from the sun. Result - climate moderation Result - organisms are able to
survive temperature changes.
5) Water Has A High Heat Of Vaporization
Heat of Vaporization: • The quantity of heat a liquid must
absorb for 1g of it to convert to a gaseous state.
Results:• Water cools organisms from excessive
heat buildup.• Why?
Hydrogen bonding
6) Water Expands When It Freezes
The distance between water molecules INCREASES from the liquid to the solid form.
Result:• Aquatic life can live under ice.
Why?• Hydrogen bonding
Solids and Liquids
Water Benzene
Floats Sinks
Solid Liquid Gas
States of Matter
7) Water Is A Versatile Solvent Water will form a solution with many
materials. Considered the best solvent Why?
• Hydrogen bonding
Solvent The dissolving agent. The material in the greater quantity. Ex:
• Water• Alcohols• Buffers
Water is the best solvent • Why? Versatile (can dissolve MOST
solutes)
Solute The substance that is dissolved. The material in the lesser quantity. Ex:
• Salt• Sugar• Kool-aid powder
Hydrophilic Materials
Materials that dissolve in water.• Hydro - water• philic - to like or love
Have ionic or polar regions (polar covalent bonds) on their molecules for H+ bonds.
Hydrophobic Materials that repel water. Hydro - water phobic - to fear Have non-polar covalent bonds.
• Remember: In npc bonds, e- are shared evenly.
Ex:• Lipids• Cell membrane components
Quick Review What is cohesion? What is adhesion? Name the main reason that water
possesses the properties that it does. Give an example of each of the
following:• Solute• Solvent
Solution Concentration Usually based on Molarity. Molarity - the number of moles of
solute per liter of solution. Use mass to calculate # of molecules
Moles The molecular weight of a substance
in grams. One Avogadro’s number of
molecules. • 6.02 X 1023 = 1 mole
One Mole of each
Sulfur
Sugar
Copper Sulfate
Mercury Oxide
Copper
Sodium Chloride
Dissociation of Water Water can sometimes split into two
ions.
In pure water the concentration of each ion is 10-7 M
Dissociation of Water, Continued
Adding certain solutes disrupts the balance between the two ions.
The two ions are very reactive and can drastically affect a cell.
Acids Materials that can release H+ (when
dissolved in water) pH = 0-7 (6.9) Example: HCl HCl H+ + Cl-
Bases Materials that can absorb H+
Often reduce H+ (by producing OH- ) pH = 7.1-14 Example: NaOH, blood (7.4-7.8),
bleach
Neutrals Materials that are neither acids nor
bases. pH = 7 (ish)
• Usually 6.5-7.4 Ex:
• Urine
pH Scale A logarithmic scale for showing H+
concentration pH = - log [H+]
pH Scale
Example:For a neutral solution:[H+] is 10-7
or - log 10-7 or - (-7)or 7
pH, cont. Acids: pH <7 etc. Bases: pH >7 etc. Each pH unit is a 10x change in H+
[H+] + [OH-] = 14 Therefore, if you know the
concentration of one ion, you can easily calculate the other.
Buffers Materials that have both acid and
base properties. Resist pH shifts. Cells and other biological solutions
often contain buffers
Buffers, cont. Advantage:
• Prevents damage to cell/DNA• pH changes can denature proteins
Ex:• Buffers in blood keep pH around a
slightly basic pH Most are acid-base pairs
Summary Recognize the chemical structure of water. Relate the structure of water to its properties. Identify and discuss the unique properties of
water. Calculate specific concentrations of solutions
(moles). Recognize pH and the pH scale. Recognize acids, bases, and buffers.