1. Day 6 1-17 Group Quest: Previewing Assignment:
Read / review section 15.1 and complete #s
1-7 on page 493
Day
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2. Q of the Day Day 1 12-5 Day 3 1-30 Calculate and record your % grade.
Quest 5 = ____
Did you meet your goal? Why or why not.
3. SPECIFIC study (preparation) plan for next test?
Next time I will study by …
4. Record your new goal:
- If you met your goal you must improve by at least one point. If not your goal stays the same.
Day
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3. Assignment
page 493 #s 1-7
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4. Chapter 15 Water and Aqueous Systems 15.1 Water and Its Properties
15.2 Homogeneous Aqueous
Systems
15.3 Heterogeneous Aqueous
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5. PERIOD 1 = Friday 2-7 day 1 PERIOD 3 = Monday 2-10 day 2 Quarterly #2
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6. What properties of water make it essential to life on Earth?
CHEMISTRY & YOU
What properties of water make it essential to life on Earth?
Water covers about three quarters of Earth’s surface. All known life forms are made mostly of water.
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7. Water in the Liquid State
Molecule has net polarity
Polar bonds δ– δ+
Liquid water
Hydrogen bond
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8. Water in the Liquid State
Many unique and important properties of water—including its high surface tension, low vapor pressure, and high boiling point—result from hydrogen bonding.
Liquid water
Hydrogen bond
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9. Water in the Liquid State
Vapor Pressure
Hydrogen bonding between water molecules also explains water’s unusually low vapor pressure.
An extensive network of hydrogen bonds holds the molecules in liquid water to one another.
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10. Water in the Solid State
As water begins to cool, it behaves initially like a typical liquid.
It contracts slightly, and its density gradually increases.
When the temperature of the water falls below 4˚C, the density of water actually starts to decrease.
Density of Liquid Water and Ice
Temperature (˚C)
Density (g/cm3)
100 (liquid water)
0.9584 50
0.9881 25
0.9971 10
0.9997 4
1.0000
0 (liquid water)
0.9998
0 (ice)
0.9168
normal
unique to water
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11. Water in the Solid State
Below 4˚C, water no longer behaves like a typical liquid.
Ice, which forms at 0˚C, has about a 10% lower density than water at 0˚C.
Ice is one of only a few solids that floats in its own liquid.
Density of Liquid Water and Ice
Temperature (˚C)
Density (g/cm3)
100 (liquid water)
0.9584 50
0.9881 25
0.9971 10
0.9997 4
1.0000
0 (liquid water)
0.9998
0 (ice)
0.9168
unique to water
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12. Water in the Solid State
Why is ice less dense than liquid water?
The structure of ice is a regular open framework of water molecules in a hexagonal arrangement.
The hexagonal symmetry of a snowflake reflects the structure of the ice crystal.
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13. Water in the Solid State
The unique properties of ice are a result of hydrogen bonding.
Extensive hydrogen bonding in ice holds the water molecules farther apart in a more ordered arrangement than in liquid water.
Hydrogen bond
Ice
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14. Water in the Solid State
The fact that ice floats has important consequences for all organisms.
The liquid water at the bottom of an otherwise frozen body of water is warmer than 0˚C, so fish and other aquatic life are better able to survive.
If ice were denser than liquid water, bodies of water would tend to freeze solid during the winter months, destroying many types of organisms.
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15. CHEMISTRY & YOU
What properties of water that result from hydrogen bonding make it essential to life on Earth?
The low vapor pressure of water keeps the liquid water in all of Earth’s lakes and oceans from evaporating rapidly.
If water did not have such a high boiling point, it would be a vapor at the usual temperatures found on Earth.
The fact that ice floats allows fish and other aquatic life to survive the winter months.
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16. Bonding and Interactions
BIG IDEA
Bonding and Interactions
Water molecules are held together through hydrogen bonds.
The hydrogen bonding interactions between water molecules account for the unique properties of water, including its high surface tension, low vapor pressure, and high boiling point.
Hydrogen bonding also accounts for the fact that ice is less dense than liquid water.
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17. I. What is a solution? water solvent
A. An aqueous solution is formed when
________ is the _________.
water
solvent
An aqueous solution is water that contains dissolved substances.
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18. Solutions
Solvents and Solutes
In a solution, the dissolving medium is the solvent.
The dissolved particles in a solution are the solute.
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19. I. What is a solution? alcohol solvent solute solvent
B. A tincture is formed when _________ is
the _________.
C. Concentration is the amount of
________ dissolved in a given amount of
_________
alcohol
solvent
solute
solvent
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20. I. What is a solution? concentration M = 1. Molarity, M or M
a. Most widely-used unit of
__________________
b. Formula
c. Ex:
concentration
# mols of solute
M =
# L of solution
5g glucose in 100mL sol’n
C6H12O6  6(12) + 12(1) + 6(16) =
1 mol x
5 g =
mol
÷ .1L = M
180 g
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21. (Volume of Conc.)(M Conc.) = (Volume of Dilute)(M of Dilute sol’n)
I. What is a solution?
2. Other units of concentration include
___________________, _______________,
_________, and ____________
D. Dilution is adding more ________ to a
solution to reduce the ________________.
1. Used to prepare solutions from
_______________ solutions.
2. Formula
mass percentage
mole fraction
molality
normality
solvent
concentration
stock or conc.
VcMc = VdMd
(Volume of Conc.)(M Conc.) = (Volume of Dilute)(M of Dilute sol’n) 21
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22. Vc(10 M K2Cr2O7) = (250 mL)(5 M K2Cr2O7)
I. What is a solution?
3. Ex.
How much 10M K2Cr2O7 should you use to prepare 250 mL of 5M K2Cr2O7?
VcMc = VdMd
Vc(10 M K2Cr2O7) = (250 mL)(5 M K2Cr2O7)
Vc=
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23. Assignment
page 493 #s 1-7
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24. Period 1 = Double = Prelab
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