The document discusses several key properties of water that are important for living organisms. It explains that water's polarity allows it to form hydrogen bonds between molecules, giving water high cohesion and adhesion. This allows water to have properties like surface tension and capillary action that are essential for life. The document also notes water's high specific heat, heat of vaporization, and ability to act as a solvent and universal transport mechanism in organisms and biological systems.

1. DO NOW
• In nature there are several elements in high
abundance, carbon (C), oxygen (O),
hydrogen (H), and nitrogen (N). Which of
these 2 elements most affects the percentage
of elements found in the human body?

2. DO NOW
• How is the cohesion and adhesion of water
related? Write an example to explain your
answer.

3. AGENDA
• PROPERTIES OF WATER NOTES

4. The ExtraordinaryThe Extraordinary
Properties of WaterProperties of Water

5. Water in Living ThingsWater in Living Things
• Many organisms release excess heat through
water evaporation.
• In organisms, this ability to control
temperature enables cells to maintain a
constant internal temperature when the external
temperature changes.
• In this way, water helps cells maintain
homeostasis

6. WaterWater
• A water molecule (H2O), is made
up of threethree atoms --- one
oxygen and two hydrogen.
H
H
O

7. Water is PolarWater is Polar
• In each water molecule, the oxygenoxygen
atom attracts moreatom attracts more than its "fair
share" of electronselectrons
• The oxygenoxygen end “acts” negativenegative
• The hydrogenhydrogen end “acts” positivepositive
• Causes the water to be POLARPOLAR
• However, Water is neutralneutral (equal
number of e- and p+) --- Zero NetZero Net
ChargeCharge

9. Hydrogen Bonds ExistHydrogen Bonds Exist
Between Water MoleculesBetween Water Molecules
• Formed between a highlyFormed between a highly
Electronegative atom ofElectronegative atom of
a polar molecule and aa polar molecule and a
HydrogenHydrogen
• OneOne hydrogen bond ishydrogen bond is
weakweak , but, but manymany
hydrogen bonds arehydrogen bonds are
strongstrong

10. Interaction Between WaterInteraction Between Water
MoleculesMolecules
Negative Oxygen end of one water molecule isNegative Oxygen end of one water molecule is
attracted to the Positive Hydrogen end of anotherattracted to the Positive Hydrogen end of another
water molecule to form a HYDROGEN BONDwater molecule to form a HYDROGEN BOND

11. What areWhat are
thethe
PropertiesProperties
of Water?of Water?

12. Properties of WaterProperties of Water
• At sea levelAt sea level,, pure water boils atpure water boils at
100 °C and freezes at 0 °C.100 °C and freezes at 0 °C.
• TheThe boiling temperature of waterboiling temperature of water
decreases at higher elevationsdecreases at higher elevations
(lower atmospheric pressure).(lower atmospheric pressure).
• For this reason, anFor this reason, an eggegg will takewill take
longer to boillonger to boil at higher altitudesat higher altitudes

13. Properties of Water Cont..Properties of Water Cont..
• CohesionCohesion

14. Properties of WaterProperties of Water
• CohesionCohesion
• AdhesionAdhesion

15. Properties of WaterProperties of Water
• CohesionCohesion
• AdhesionAdhesion
• High Specific HeatHigh Specific Heat

16. Properties of WaterProperties of Water
• CohesionCohesion
• AdhesionAdhesion
• High Specific HeatHigh Specific Heat
• High Heat of VaporizationHigh Heat of Vaporization

17. Properties of WaterProperties of Water
• CohesionCohesion
• AdhesionAdhesion
• High Specific HeatHigh Specific Heat
• High Heat of VaporizationHigh Heat of Vaporization
• Less Dense as a SolidLess Dense as a Solid
• SolventSolvent

18. CohesionCohesion
• Attraction between particles of theAttraction between particles of the
same substance (same substance ( why water iswhy water is
attracted to itself)attracted to itself)
• Results inResults in Surface tensionSurface tension (a measure(a measure
of the strength of waterof the strength of water’s surface’s surface))
• Produces aProduces a surface filmsurface film on water thaton water that
allows insects to walk on the surfaceallows insects to walk on the surface
of waterof water

19. Cohesion Analogy
Molecules at the surface of water are
linked together by hydrogen bonds like a
crowd of people linked by holding hands.
This attraction between water molecules
causes a condition known as surface
tension.

20. Cohesion …Cohesion …
Helps insects walk across
water

21. Lizard Walking on Water!
• https://www.youtube.com/watch?v=Qhsxo7vY8a

22. AdhesionAdhesion
• Attraction between two differentAttraction between two different
substances.substances.
• Water will makeWater will make hydrogen bonds with otherhydrogen bonds with other
surfacessurfaces such as glass, soil, plant tissues,such as glass, soil, plant tissues,
and cotton.and cotton.
• Capillary actionCapillary action-- when water moleculeswhen water molecules “tow”“tow”
or carry each other along without the help ofor carry each other along without the help of
gravity.gravity.
• Example:Example: TranspirationTranspiration is ais a process whichprocess which
plants and trees remove water from the soil,plants and trees remove water from the soil,
and paper towels soak up water.and paper towels soak up water.

23. Adhesion Causes CapillaryAdhesion Causes Capillary
ActionAction
Which gives water the
ability to “climb”
structures

24. Adhesion Also CausesAdhesion Also Causes
Water to …Water to …
Form spheres &
hold onto plant
leaves
Attach to a
silken spider
web

25. Adhesion Causes CapillaryAdhesion Causes Capillary
Action in PlantsAction in Plants
• http://study.com/academy/lesson/capillary-action-

26. DO NOW
• What makes water a polar
molecule? Think about the
structure of a water molecule.

27. High Specific HeatHigh Specific Heat
• Amount of heat needed to raise orAmount of heat needed to raise or
lower 1g of a substance 1° Clower 1g of a substance 1° C..
• WaterWater resistsresists temperature changetemperature change,,
both for heating and cooling.both for heating and cooling.
• Water can absorb or release largeWater can absorb or release large
amounts of heat energy with littleamounts of heat energy with little
change in actual temperature.change in actual temperature.

28. High Heat of VaporizationHigh Heat of Vaporization
• Amount of energy it takes toAmount of energy it takes to
convert 1g of a substance from aconvert 1g of a substance from a
liquid to a gasliquid to a gas
• In order for water to evaporate,In order for water to evaporate,
hydrogen bonds must be brokenhydrogen bonds must be broken..
• As water evaporates, it removes aAs water evaporates, it removes a
lot of heat with itlot of heat with it..

29. High Heat of VaporizationHigh Heat of Vaporization
• Water's heat of vaporization is 540540
cal/g.cal/g.
• In order for water toIn order for water to evaporateevaporate,,
each gram musteach gram must GAIN 540GAIN 540 caloriescalories
(temperature doesn(temperature doesn’t change ---’t change ---
100100oo
C).C).
• As water evaporatesAs water evaporates, it removes a, it removes a
lot oflot of heatheat with itwith it (cooling effect)(cooling effect)..

30. • Water vaporWater vapor forms a kind of
global ‘‘blanket” which helps to
keep the Earth warm.
• Heat radiated from the sunHeat radiated from the sun
warms the surface of the earth
is absorbed and heldabsorbed and held
by the vaporby the vapor.

31. Water is Less Dense as aWater is Less Dense as a
SolidSolid
• Ice is less denseIce is less dense as a solid than as a
liquid (ice floats)
• Liquid water has hydrogen bondshydrogen bonds that
are constantly being broken andconstantly being broken and
reformed.reformed.
• Frozen waterFrozen water forms a crystal-likecrystal-like
latticelattice whereby molecules are set at
fixed distances.

32. Water is Less Dense as aWater is Less Dense as a
SolidSolid
•Which is ice and which is water?Which is ice and which is water?

33. Water is Less Dense as aWater is Less Dense as a
SolidSolid
IceIce WaterWater

34. HomeostasisHomeostasis
• Ability to maintain aAbility to maintain a steady statesteady state
despite changing conditionsdespite changing conditions
• Water is important to this processWater is important to this process
because:because:
a. Makes a good insulatora. Makes a good insulator
b. Resists temperature changeb. Resists temperature change
c. Universal solventc. Universal solvent
d. Coolantd. Coolant
e. Ice protects against temperaturee. Ice protects against temperature
extremes (insulates frozenextremes (insulates frozen
lakes)lakes)

35. Solutions & SuspensionsSolutions & Suspensions
• Water is usually part of aWater is usually part of a
mixture.mixture.
• There are two types ofThere are two types of
mixtures:mixtures:
– SolutionsSolutions
– SuspensionsSuspensions

36. SolutionSolution
• Ionic compoundsIonic compounds are evenlyare evenly
distributed ordistributed or dispersed asdispersed as ionsions inin
waterwater
• SOLUTESOLUTE
– Substance that is being dissolvedSubstance that is being dissolved
• SOLVENTSOLVENT
– Substance into which the soluteSubstance into which the solute
dissolvesdissolves

37. SolutionSolution

38. SuspensionsSuspensions
• Substances that
dondon’t dissolve but’t dissolve but
separateseparate into tiny
pieces.
• Water keeps theWater keeps the
pieces suspendedpieces suspended
so they don’t
settle out.

39. DO NOW
You are experiencing pain, burning, or
discomfort in the chest when taking a deep
breath, chest tightness, wheezing, or
shortness of breath. You are most likely
experiencing
a)a loss of energy
b)a lack of oxygen intake
c)a side effect due to ozone pollution
d)a lack of sleep

40. Acids, Bases and pHAcids, Bases and pH
One water moleculeOne water molecule in 550 millionin 550 million
naturallynaturally dissociatesdissociates into a Hydrogeninto a Hydrogen
IonIon (H+)(H+) and a Hydroxide Ionand a Hydroxide Ion (OH-)(OH-)
Hydrogen Ion Hydroxide IonHydrogen Ion Hydroxide Ion
AcidAcid BaseBase
H2O  H+
+ OH-

41. The pH ScaleThe pH Scale
• Indicates the concentration of Hconcentration of H++
ions or how acidic a substance isions or how acidic a substance is
• Ranges from 0 – 140 – 14
• pH of 7 is neutral7 is neutral
• pH 0 up to 7 is acid0 up to 7 is acid … H+
• pH above 7 – 14 is babove 7 – 14 is basic… OH-
• Each pH unit represents a factor of
10X10X change in concentration
• pH 3 is 10 x 10 x 10 (1000)pH 3 is 10 x 10 x 10 (1000)
stronger than a pH of 6stronger than a pH of 6

42. AcidsAcids
• StrongStrong
AcidsAcids
have a pHhave a pH
of 1-3of 1-3
• ProduceProduce
lots oflots of
HH++
ionsions

43. BasesBases
• StrongStrong
BasesBases have
a pH of 1111
to 14to 14
• Contain
lots of OHlots of OH--
ionsions and
fewer H+
ions

44. BuffersBuffers
• Weak acids or bases that react withWeak acids or bases that react with
strong acids or bases to preventstrong acids or bases to prevent
sharp, sudden changes in pHsharp, sudden changes in pH
(neutralization).(neutralization).
• Produced naturally by the bodyProduced naturally by the body toto
maintain homeostasismaintain homeostasis
Weak AcidWeak Acid Weak BaseWeak Base

45. DO NOW
• What is the relationship between a
solute and a solvent?

46. DO NOW
• Explain the difference between a
solution and a suspension.

47. DO NOW
• How are acids and bases different?
How do their pH values differ?

48. Objectives
• Summarize the characteristics of organic
compounds.
• Compare the structures and function of
different types of biomolecules.
• Describe the components of DNA and RNA.
• State the main role of ATP in cells.
• the main role of ATP in cells.

49. DO NOW
Look at all the different foods that are shown. Write
down what you think all of these substances have in
common. How are they different?

50. AGENDA
•DO NOW
•NOTES
•WORKSHEET
•EXIT TICKET

51. Today’s Objective
Describe the unique qualities of
carbon.
Summarize the characteristics of
organic compounds.
Describe the structures and functions
of each of the four groups of
macromolecules.

52. The Chemistry of Carbon
• Carbon can bond with many different
elements such as hydrogen (H), oxygen (O),
phosphorus (P), sulfur (S), and nitrogen (N) to
form the molecules of life.

53. A Few Examples

55. Carbon Compounds
• Carbohydrates
• are organic compounds made of carbon,
hydrogen, and oxygen atoms in the
proportion of 1:2:1
• Carbohydrates are a key source of energy, and
they are found in most foods—especially
fruits, vegetables, and grains.

56. Carbon Compounds cont.
Carbohydrates
• The building blocks of carbohydrates are
single sugars, called monosaccharides, such as
glucose, C6H12O6, and fructose.
• Simple sugars such as glucose are a major
source of energy in cells.

57. Carbon Compounds, cont.
Carbohydrates
• Disaccharides are double sugars formed when
two monosaccharides are joined.
• Sucrose, or common table sugar, is a
disaccharide that consists of both glucose and
fructose.

58. Disaccharides

59. Carbon Compounds, cont.
Carbohydrates
• Polysaccharides such as starch, shown below,
are chains of three or more monosaccharides.

60. Polysaccharides
• Poly=many
• Saccharide=sugar

61. Lipids

64. DO NOW

65. DO NOW