unit 8 hs260 anatomy, physiology & chemistry amy habeck, rd, ms, ldn 1
TRANSCRIPT
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Unit 8HS260 Anatomy, Physiology &
ChemistryAmy Habeck, RD, MS, LDN
1
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Questions?
2
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Objectives
3
Answer your questions Review
Chapter 2, Zumdahl: Basic Chemistry- Measurement and Calculations
Chapter 3, Zumdahl: Basic Chemistry- Matter
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Chapter 2
Measurements and Calculations
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Measurement
Copyright © Cengage Learning. All rights reserved Quantitative observation.
Has 2 parts – number and unit. Number tells
comparison. Unit tells scale.
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Copyright © Cengage Learning. All rights reserved• Technique used to express very large or
very small numbers.• Expresses a number as a product of a
number between 1 and 10 and the appropriate power of 10.
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Using Scientific Notation
Copyright © Cengage Learning. All rights reserved• Any number can be represented as the
product of a number between 1 and 10 and a power of 10 (either positive or negative).
• The power of 10 depends on the number of places the decimal point is moved and in which direction.
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Using Scientific Notation
Copyright © Cengage Learning. All rights reserved• The number of places the decimal point is
moved determines the power of 10. The direction of the move determines whether the power of 10 is positive or negative.
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Using Scientific Notation
Copyright © Cengage Learning. All rights reserved• If the decimal point is moved to the left,
the power of 10 is positive.345 = 3.45 × 102
• If the decimal point is moved to the right, the power of 10 is negative.
0.0671 = 6.71 × 10–2
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Concept Check
Copyright © Cengage Learning. All rights reserved
Which of the following correctly expresses 7,882 in scientific notation?
a) 7.882 × 104
b) 788.2 × 103
c) 7.882 × 103
d) 7.882 × 10–3
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Concept Check
Copyright © Cengage Learning. All rights reserved
Which of the following correctly expresses 7,882 in scientific notation?
a) 7.882 × 104
b) 788.2 × 103
c) 7.882 × 103
d) 7.882 × 10–3
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Concept Check
Copyright © Cengage Learning. All rights reserved
Which of the following correctly expresses 0.0000496 in scientific notation?
a) 4.96 × 10–5
b) 4.96 × 10–6
c) 4.96 × 10–7
d) 496 × 107
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Concept Check
Copyright © Cengage Learning. All rights reserved
Which of the following correctly expresses 0.0000496 in scientific notation?
a) 4.96 × 10–5
b) 4.96 × 10–6
c) 4.96 × 10–7
d) 496 × 107
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The Fundamental SI Units
Physical Quantity Name of Unit Abbreviation
Mass kilogram kg
Length meter m
Time second s
Temperature kelvin K
Electric current ampere A
Amount of substance mole mol
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Prefixes Used in the SI SystemCopyright © Cengage Learning. All rights reserved Prefixes are used to change the size of the unit.
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LengthCopyright © Cengage Learning. All rights reserved Fundamental SI unit of length is the meter.
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Volume
Copyright © Cengage Learning. All rights reserved Measure of the
amount of 3-D space occupied by a substance.
SI unit = cubic meter (m3)
Commonly measure solid volume in cm3.
1 mL = 1 cm3
1 L = 1 dm3
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MassCopyright © Cengage Learning. All rights reserved Measure of the
amount of matter present in an object.
SI unit = kilogram (kg)
1 kg = 2.2046 lbs 1 lb = 453.59 g
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Concept Check
Copyright © Cengage Learning. All rights reserved
Choose the statement(s) that contain improper use(s) of commonly used units (doesn’t make sense)?
A gallon of milk is equal to about 4 L of milk.
A 200-lb man has a mass of about 90 kg. A basketball player has a height of 7 m tall. A nickel is 6.5 cm thick.
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Concept Check
Copyright © Cengage Learning. All rights reserved
Choose the statement(s) that contain improper use(s) of commonly used units (doesn’t make sense)?
A gallon of milk is equal to about 4 L of milk.
A 200-lb man has a mass of about 90 kg. A basketball player has a height of 7 m tall. A nickel is 6.5 cm thick.
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Copyright © Cengage Learning. All rights reserved A digit that must be estimated is called
uncertain. A measurement always has some degree of
uncertainty. Record the certain digits and the first
uncertain digit (the estimated number).
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Measurement of Length Using a Ruler
Copyright © Cengage Learning. All rights reserved The length of the pin occurs at about 2.85 cm.
Certain digits: 2.85 Uncertain digit: 2.85
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Rules for Counting Significant FiguresCopyright © Cengage Learning. All rights reserved
1. Nonzero integers always count as significant figures. 3456 has 4 sig figs (significant figures).
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Rules for Counting Significant FiguresCopyright © Cengage Learning. All rights reserved
There are three classes of zeros.a. Leading zeros are zeros that precede all the
nonzero digits. These do not count as significant figures. 0.048 has 2 sig figs.
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Rules for Counting Significant FiguresCopyright © Cengage Learning. All rights reserved
b. Captive zeros are zeros between nonzero digits. These always count as significant figures. 16.07 has 4 sig figs.
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Rules for Counting Significant FiguresCopyright © Cengage Learning. All rights reserved
c. Trailing zeros are zeros at the right end of the number. They are significant only if the number contains a decimal point. 9.300 has 4 sig figs. 150 has 2 sig figs.
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Rules for Counting Significant FiguresCopyright © Cengage Learning. All rights reserved
3. Exact numbers have an infinite number of significant figures. 1 inch = 2.54 cm, exactly. 9 pencils (obtained by counting).
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Questions?
28
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Exponential NotationCopyright © Cengage Learning. All rights reserved Example
300. written as 3.00 × 102
Contains three significant figures. Two Advantages
Number of significant figures can be easily indicated.
Fewer zeros are needed to write a very large or very small number.
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Rules for Rounding Off
Copyright © Cengage Learning. All rights reserved1. If the digit to be removed is less than 5, the
preceding digit stays the same. 5.64 rounds to 5.6 (if final result to 2 sig figs)
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Rules for Rounding Off
Copyright © Cengage Learning. All rights reserved1. If the digit to be removed is equal to or
greater than 5, the preceding digit is increased by 1. 5.68 rounds to 5.7 (if final result to 2 sig figs) 3.861 rounds to 3.9 (if final result to 2 sig figs)
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Rules for Rounding Off
Copyright © Cengage Learning. All rights reserved2. In a series of calculations, carry the extra digits
through to the final result and then round off. This means that you should carry all of the digits that show on your calculator until you arrive at the final number (the answer) and then round off, using the procedures in Rule 1.
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Significant Figures in Mathematical Operations
Copyright © Cengage Learning. All rights reserved1. For multiplication or division, the number of
significant figures in the result is the same as that in the measurement with the smallest number of significant figures.
1.342 × 5.5 = 7.381 7.4
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Significant Figures in Mathematical Operations
Copyright © Cengage Learning. All rights reserved2. For addition or subtraction, the limiting term
is the one with the smallest number of decimal places.
Corrected
23.445
7.83
31.2831.275
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Concept Check Copyright © Cengage Learning. All rights reserved
You have water in each graduated cylinder shown. You then add both samples to a beaker (assume that all of the liquid is transferred).
How would you write the number describing the total volume?
What limits the precision of the total volume?
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Concept Check Copyright © Cengage Learning. All rights reserved
You have water in each graduated cylinder shown. You then add both samples to a beaker (assume that all of the liquid is transferred).
How would you write the number describing the total volume?
3.1 mLWhat limits the precision of the total volume?
1st graduated cylinder
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Copyright © Cengage Learning. All rights reserved
Use when converting a given result from one system of units to another.
1) To convert from one unit to another, use the equivalence statement that relates the two units.
2) Choose the appropriate conversion factor by looking at the direction of the required change (make sure the unwanted units cancel).
3) Multiply the quantity to be converted by the conversion factor to give the quantity with the desired units.
4) Check that you have the correct number of sig figs.
5) Does my answer make sense?
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Example #1
To convert from one unit to another, use the equivalence statement that relates the two units.
1 ft = 12 inThe two unit factors are:
1 ft 12 in and
12 in 1 ft
Copyright © Cengage Learning. All rights reserved
A golfer putted a golf ball 6.8 ft across a green. How many inches does this represent?
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Example #1
Copyright © Cengage Learning. All rights reserved
Choose the appropriate conversion factor by looking at the direction of the required change (make sure the unwanted units cancel).
A golfer putted a golf ball 6.8 ft across a green. How many inches does this represent?
6.8 ft12 in
1 ft
in
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Example #1
Copyright © Cengage Learning. All rights reserved
Multiply the quantity to be converted by the conversion factor to give the quantity with the desired units.
Correct sig figs? Does my answer make sense?
A golfer putted a golf ball 6.8 ft across a green. How many inches does this represent?
6.8 ft12 in
1 ft
82 in
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Example #2
Copyright © Cengage Learning. All rights reserved
An iron sample has a mass of 4.50 lb. What is the mass of this sample in grams?
(1 kg = 2.2046 lbs; 1 kg = 1000 g)
4.50 lbs1 kg
2.2046 lbs
1000 g
1 kg 3= 2.04 10 g
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Concept Check
Copyright © Cengage Learning. All rights reserved
What data would you need to estimate the money you would spend on gasoline to drive your car from New York to Los Angeles? Provide estimates of values and a sample calculation.
1 gal $3.252500 mi = $325
25 mi 1 gal
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Concept Check
Copyright © Cengage Learning. All rights reservedWhat data would you need to estimate the
money you would spend on gasoline to drive your car from New York to Los Angeles? Provide estimates of values and a sample calculation.Sample Answer:Distance between New York and Los Angeles: 2500 milesAverage gas mileage: 25 miles per gallonAverage cost of gasoline: $3.25 per gallon
1 gal $3.252500 mi = $325
25 mi 1 gal
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Three Systems for Measuring Temperature
Copyright © Cengage Learning. All rights reserved Fahrenheit
Celsius Kelvin
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The Three Major Temperature Scales
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Converting Between Scales Copyright © Cengage Learning. All rights reserved
K C C K
FC F C
+ 273 273
32 1.80 + 32
1.80
T T T T
TT T T
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Exercise
Copyright © Cengage Learning. All rights reserved
The normal body temperature for a dog is approximately 102oF. What is this equivalent to on the Kelvin temperature scale?
a) 373 Kb) 312 Kc) 289 Kd) 202 K
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Exercise
Copyright © Cengage Learning. All rights reserved
The normal body temperature for a dog is approximately 102oF. What is this equivalent to on the Kelvin temperature scale?
a) 373 Kb) 312 Kc) 289 Kd) 202 K
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Exercise
Copyright © Cengage Learning. All rights reserved
At what temperature does C = F?
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Solution
Copyright © Cengage Learning. All rights reserved
Since °C equals °F, they both should be the same value (designated as variable x).
Use one of the conversion equations such as:
Substitute in the value of x for both T°C and T°F. Solve for x.
FC
32
1.80
TT
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Solution
Copyright © Cengage Learning. All rights reserved
So –40°C = –40°F
FC
32
1.80
TT
32
1.80
xx
40 x
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Copyright © Cengage Learning. All rights reserved Mass of substance per unit volume of the
substance. Common units are g/cm3 or g/mL.
massDensity =
volume
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Measuring the Volume of a Solid Object by Water Displacement
Copyright © Cengage Learning. All rights reserved
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Example #1Copyright © Cengage Learning. All rights reserved
massDensity =
volume
3
17.8 gDensity =
2.35 cm
Density = 37.57 g/cm
A certain mineral has a mass of 17.8 g and a volume of 2.35 cm3. What is the density of this mineral?
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Example #2
Copyright © Cengage Learning. All rights reserved
massDensity =
volume
What is the mass of a 49.6 mL sample of a liquid, which has a density of 0.85 g/mL?
0.85 g/mL = 49.6 mL
x
mass = = 42 gx
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Exercise
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If an object has a mass of 243.8 g and occupies a volume of 0.125 L, what is the density of this object in g/cm3?
a) 0.513b) 1.95c) 30.5d) 1950
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Exercise
Copyright © Cengage Learning. All rights reserved
If an object has a mass of 243.8 g and occupies a volume of 0.125 L, what is the density of this object in g/cm3?
a) 0.513b) 1.95c) 30.5d) 1950
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Concept Check
Copyright © Cengage Learning. All rights reserved
Copper has a density of 8.96 g/cm3. If 75.0 g of copper is added to 50.0 mL of water in a graduated cylinder, to what volume reading will the water level in the cylinder rise?
a) 8.4 mLb) 41.6 mLc) 58.4 mLd) 83.7 mL
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Questions?
59
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Chapter 3
Matter
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The Organization of MatterCopyright © Cengage Learning. All rights reserved
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Matter
Copyright © Cengage Learning. All rights reserved Anything occupying space and having mass.
Matter exists in three states. Solid Liquid Gas
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The Three States of Water
Copyright © Cengage Learning. All rights reserved
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Solid
Copyright © Cengage Learning. All rights reserved Rigid
Has a fixed volume and shape. Examples:
Ice cube, diamond, iron bar
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Liquid
Copyright © Cengage Learning. All rights reserved Has a definite volume but no specific shape.
Assumes shape of container. Examples:
Gasoline, water, alcohol, blood
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Gas
Copyright © Cengage Learning. All rights reserved Has no fixed volume or shape.
Takes the shape and volume of its container. Examples:
Air, helium, oxygen
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Physical PropertiesCopyright © Cengage Learning. All rights reserved The characteristics of matter that can be
changed without changing its composition. Characteristics that are directly observable. Examples:
Odor, color, volume, state (s, l, or g), density, melting point, and boiling point
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Chemical PropertiesCopyright © Cengage Learning. All rights reserved A substance’s ability to form new
substances. The characteristics that determine how the
composition of matter changes as a result of contact with other matter or the influence of energy.
Characteristics that describe the behavior of matter.
Examples: Flammability, rusting of steel, and the
digestion of food
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Concept Check
Copyright © Cengage Learning. All rights reserved
Classify each of the following as a physical or chemical property.
Ethyl alcohol boiling at 78°C Hardness of a diamond Sugar fermenting to form ethyl alcohol
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Concept Check
Copyright © Cengage Learning. All rights reserved
Classify each of the following as a physical or chemical property.
Ethyl alcohol boiling at 78°C Hardness of a diamond Sugar fermenting to form ethyl alcohol
physicalphysicalchemical
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Physical Change
Copyright © Cengage Learning. All rights reserved Change in the form of a substance, not in its
chemical composition. Example:
Boiling or freezing water
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Three States of Water
Copyright © Cengage Learning. All rights reserved In all three phases, water molecules are still intact.
Motions of molecules and the distances between them change.
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Chemical Change
Copyright © Cengage Learning. All rights reserved A given substance becomes a new substance
or substances with different properties and different composition.
Example: Bunsen burner (methane reacts with
oxygen to form carbon dioxide and water)
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Concept Check
Copyright © Cengage Learning. All rights reserved
How many of the following are examples of a chemical change?
Pulverizing (crushing) rock salt Burning of wood Dissolving of sugar in water Melting a popsicle on a warm summer
day
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Concept Check
Copyright © Cengage Learning. All rights reserved
How many of the following are examples of a chemical change?
Pulverizing (crushing) rock salt Burning of wood Dissolving of sugar in water Melting a popsicle on a warm summer
day
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Concept Check
Copyright © Cengage Learning. All rights reserved
Classify each of the following as a physical or chemical change.
Sugar fermenting to form ethyl alcohol Iron metal melting Iron combining with oxygen to form rust
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Concept Check
Copyright © Cengage Learning. All rights reserved
Classify each of the following as a physical or chemical change.
Sugar fermenting to form ethyl alcohol Iron metal melting Iron combining with oxygen to form rust
chemicalphysicalchemical
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ElementCopyright © Cengage Learning. All rights reserved A substance that cannot be broken down
into other substances by chemical methods. Examples:
Iron (Fe), aluminum (Al), oxygen (O2), and hydrogen (H2)
All of the matter in the world around us contains elements.
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Compound
Copyright © Cengage Learning. All rights reserved A substance composed of a given
combination of elements that can be broken down into those elements by chemical methods.
Examples: Water (H2O), carbon dioxide (CO2), table
sugar (C12H22O11) A compound always contains atoms of
different elements. A compound always has the same
composition (same combination of atoms).
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Concept Check
Copyright © Cengage Learning. All rights reserved
How many of the following are compounds?
H2O, N2O4, NaOH, MnO2, HF
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Concept Check
Copyright © Cengage Learning. All rights reserved
How many of the following are compounds?
H2O, N2O4, NaOH, MnO2, HF
Five – All of the substances are compounds.
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Pure SubstancesCopyright © Cengage Learning. All rights reserved Always have the same composition.
Either elements or compounds. Examples:
Pure water (H2O), carbon dioxide (CO2), hydrogen (H2), gold (Au)
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Mixtures
Copyright © Cengage Learning. All rights reserved Have variable composition.
Examples Wood, wine, coffee
Can be separated into pure substances: elements and/or compounds.
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Homogeneous MixtureCopyright © Cengage Learning. All rights reserved Same throughout.
Having visibly indistinguishable parts. A solution. Does not vary in composition from one
region to another.
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Homogeneous Mixture – Examples
Copyright © Cengage Learning. All rights reserved Air around you
Brass Table salt stirred into water
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Heterogeneous Mixture
Copyright © Cengage Learning. All rights reserved Having visibly distinguishable parts.
Contains regions that have different properties from those of other regions.
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Heterogeneous Mixture – Examples
Copyright © Cengage Learning. All rights reserved Oil and vinegar dressing
Sand stirred into water
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Concept Check
Copyright © Cengage Learning. All rights reserved
Which of the following is a homogeneous mixture?
Pure water Gasoline Jar of jelly beans Soil Copper metal
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Concept Check
Copyright © Cengage Learning. All rights reserved
Which of the following is a homogeneous mixture?
Pure water Gasoline Jar of jelly beans Soil Copper metal
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Copyright © Cengage Learning. All rights reserved Mixtures can be separated based on different
physical properties of the components.
EvaporationVolatility
ChromatographyAdherence to a surface
FiltrationState of matter
(solid/liquid/gas)
DistillationBoiling point
TechniqueDifferent Physical Property
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Copyright © Cengage Learning. All rights reserved No chemical change occurs when salt water
is distilled.
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Filtration
Copyright © Cengage Learning. All rights reserved Separates a liquid
from a solid.
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The Organization of Matter
Copyright © Cengage Learning. All rights reserved
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Questions?
94
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Unit 8 Activities to Help Study for Unit 10 Exam
95
Activities
Multiple Choice: All of the questions in this
activity are representative of exam questions Practice the activity as many times a you need to in
order to get them all correct. 16/20 of the self-check quiz are similar questions
to the exam questions for the unit Take the self-check quiz as many times as you need to
in order to help prepare for the exam.
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Unit 9 Project
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Resources Plagiarism information
http://extmedia.kaplan.edu/global/PlagiarismGuide_s.pdf
APA formatting http://citationmachine.net/index2.php?start=&reqstylei
d=0&stylebox=2 Type in the ISBN number of a book and it will generate
the citations for you
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Farewell
97
Thank you for your kind attention and participation!
Email any time [email protected] Call if your matter is urgent
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