Chapter 1
1.6 to 1.9
Chemical
Foundations
Chapter 1
Table of Contents
1.6
1.7
1.8
1.9
Dimensional Analysis
Temperature
Density
Classification of Matter
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Section 1.6
Dimensional Analysis
•
Use when converting a given result from one
system of units to another.



To convert from one unit to another, use the
equivalence statement that relates the two units.
Derive the appropriate unit factor by looking at the
direction of the required change (to cancel the
unwanted units).
Multiply the quantity to be converted by the unit
factor to give the quantity with the desired units.
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Section 1.6
Dimensional Analysis
Example #1
A golfer putted a golf ball 6.8 ft across a green. How
many inches does this represent?
To convert from one unit to another, use the
equivalence statement that relates the two units.
1 ft = 12 in
The two unit factors are:
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Section 1.6
Dimensional Analysis
Example #1
A golfer putted a golf ball 6.8 ft across a green. How
many inches does this represent?
•
Derive the appropriate unit factor by looking at the
direction of the required change (to cancel the
unwanted units).
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Section 1.6
Dimensional Analysis
Example #1
A golfer putted a golf ball 6.8 ft across a green. How
many inches does this represent?
•
Multiply the quantity to be converted by the unit factor
to give the quantity with the desired units.
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Section 1.6
Dimensional Analysis
Example #2
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)
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• What data would you need to estimate
the money you would spend on
gasoline to drive your car from New
York to Chicago? Provide estimates of
values and a sample calculation.
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Section 1.6
Dimensional Analysis
Concept Check
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.
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Examples
l
Because you never learned dimensional
analysis, you have been working at a
fast food restaurant for the past 35
years wrapping hamburgers. Each hour
you wrap 184 hamburgers. You work 8
hours per day. You work 5 days a week.
you get paid every 2 weeks with a
salary of $840.34. How many
hamburgers will you have to wrap to
make your first one million dollars?
l
A senior was applying to college and
wondered how many applications she
needed to send. Her counselor explained
that with the excellent grade she
received in chemistry she would probably
be accepted to one school out of every
three to which she applied. She
immediately realized that for each
application she would have to write 3
essays, and each essay would require 2
hours work. Of course writing essays is
no simple matter. For each hour of
serious essay writing, she would need to
Units to a Power
l
How many m3 is 1500 cm3?
1500 cm3
1500
1m
1m
1m
100 cm 100 cm 100 cm
cm3
1m
100 cm
3
Units to a Power
l
l
How many cm2 is 15 m2?
36 cm3 is how many mm3?
Section 1.7
Temperature
Three Systems for Measuring Temperature
•
•
•
Fahrenheit
Celsius
Kelvin
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Section 1.7
Temperature
The Three Major Temperature Scales
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Section 1.7
Temperature
Converting Between Scales
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• At what temperature does C = F?
• Prove your answer.
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1–28
0ºC is not 0ºF
ºF
9
5
ºC
(0,32)= (C1,F1)
ºF
ºC
(0,32) = (C1,F1)
(100,212) = (C2,F2)
ºF
ºC
Section 1.7
Temperature
Exercise
At what temperature does C = F?
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Section 1.7
Temperature
Solution
•
•
•
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 TC and TF. Solve
for x.
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Section 1.7
Temperature
Solution
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Section 1.8
Density
•
•
Mass of substance per unit volume of the
substance.
Common units are g/cm3 or g/mL.
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Section 1.8
Density
Example #1
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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Section 1.8
Density
Example #2
What is the mass of a 49.6-mL sample of a liquid, which
has a density of 0.85 g/mL?
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Section 1.9
Classification of Matter
Matter
•
•
Anything occupying space and having mass.
Matter exists in three states.



Solid
Liquid
Gas
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Section 1.9
Classification of Matter
The Three States of Water
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Section 1.9
Classification of Matter
Solid
•
•
Rigid
Has fixed volume and shape.
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Section 1.9
Classification of Matter
Structure of a Solid
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Section 1.9
Classification of Matter
Liquid
•
•
Has definite volume but no specific shape.
Assumes shape of container.
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Section 1.9
Classification of Matter
Structure of a Liquid
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Section 1.9
Classification of Matter
Gas
•
•
Has no fixed volume or shape.
Takes on the shape and volume of its
container.
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Section 1.9
Classification of Matter
Structure of a Gas
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Section 1.9
Classification of Matter
Mixtures
•
Have variable composition.
Homogeneous Mixture

Having visibly indistinguishable parts; solution.
Heterogeneous Mixture

Having visibly distinguishable parts.
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Section 1.9
Classification of Matter
Homogeneous Mixtures
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Section 1.9
Classification of Matter
Homogeneous vs. Heterogeneous Mixtures
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Section 1.9
Classification of Matter
Compound vs. Mixture
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Section 1.9
Classification of Matter
Concept Check
Which of the following is a homogeneous
mixture?





Pure water
Gasoline
Jar of jelly beans
Soil
Copper metal
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40
Key Terms: Properties
• A physical property is
displayed by a sample of
matter without undergoing
any change in the
composition of the matter.
Copper is redbrown, opaque,
solid: physical
properties.
– Physical properties include mass,
color, volume, temperature,
density, melting point, etc.
• Chemical property –
displayed by a sample of
matter as it undergoes a
change in composition.
Ethanol is flammable: a
chemical property.
– Flammability, toxicity, reactivity,
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© 2005 are all chemical
properties.
General Chemistry
4 edition, Hill, Petrucci, McCreary, Perry
th
Chapter One
Section 1.9
Classification of Matter
Physical Change
•
Change in the form of a substance, not in its
chemical composition.

•
Example: boiling or freezing water
Can be used to separate a mixture into pure
compounds, but it will not break compounds
into elements.



Distillation
Filtration
Chromatography
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Section 1.9
Classification of Matter
Chemical Change
•
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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43
Key Terms: Properties
• In a physical change, there
is no change in composition.
• No new substances are
formed.
– Examples include: evaporation;
melting; cutting a piece of wood;
dissolving sugar in water.
• In a chemical change or
chemical reaction, the matter
undergoes a change in
composition.
The vapor burns,
• New substances are formed. combining with
oxygen: a
– Examples include: burning
chemical change.
gasoline; dissolving metal in
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General Chemistry 4 edition, Hill, Petrucci, McCreary, Perry
acid; spoilage of food.
th
The liquid fuel
evaporates: a
physical change.
Chapter One
Section 1.9
Classification of Matter
Concept Check
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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Section 1.9
Classification of Matter
The Organization of Matter
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Classifying
Matter
Figure 1.9
Atoms
46
Molecules
make up
ALL MATTER
which exists as
Pure
Substances
Mixtures
which may be
which may be
Elements
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Compounds
Homogeneous
General Chemistry 4th edition, Hill, Petrucci, McCreary, Perry
Heterogeneous
Chapter One
The Organization of Matter
Matter
Mixtures:
a) Homogeneous (Solutions)
b) Heterogeneous
Pure Substances
Elements
Compounds
Atoms
Nucleus
Protons
Quarks
Electrons
Neutrons
Quarks
48
Classifying Matter
• A (pure) substance has a definite or fixed
composition that does not vary from one sample
to another.
• All substances are either elements or compounds.
• An element cannot be broken down into other
simpler substances by chemical reactions.
– About 100 elements known at this time
– Each element has a chemical symbol: O, H, Ag, Fe, Cl, S,
Hg, Au, U, etc.
• A compound is made up of two or more elements
in fixed proportions, and can be broken down into
simpler substances.
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Chapter One
General Chemistry 4th edition, Hill, Petrucci, McCreary, Perry
49
Classifying Matter
• A mixture does not have a fixed composition.
• A homogeneous mixture has the same
composition throughout, though the composition
of different homogeneous mixtures may vary.
– Soda pop, salt water, 14K gold, and many plastics are
homogeneous mixtures.
– 10K gold and 14K gold have different compositions but both
are homogeneous.
• A heterogeneous mixture varies in composition
and/or properties from one part of the mixture to
another.
– Adhesive tape, CD, pen, battery, chair, and people are
examples of heterogeneous mixtures.
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General Chemistry 4th edition, Hill, Petrucci, McCreary, Perry
Chapter One
The Organization of Matter
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1–39
Phase
Differences
Solid – definite volume and shape; particles packed in
fixed positions.
Liquid – definite volume but indefinite shape;
particles close together but not in fixed positions
Gas – neither definite volume nor definite shape;
particles are at great distances from one another
Plasma – high temperature, ionized phase of matter as
found on the sun.
Properties of Matter
Extensive properties depend on the amount of
matter that is present.
Volume
Mass
Energy Content (think Calories!)
Intensive properties do not depend on the
amount of matter present.
Melting point
Boiling point
Density
Separation of a Mixture
The constituents of the mixture retain
their identity and may be separated by
physical means.
Separation of a Mixture
The components of
dyes such as ink may
be separated by
paper
chromatography.
Figure 1.15a
A Line of the
Mixture to be
Separated is
Placed at
One End of
a Sheet
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1–
Figure 1.15b
The Paper
Acts as a
Wick to
Draw up the
Liquid
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1–
Figure
1.15c
Component
with the
Weakest
Attraction
for the
Paper
Travels
Faster
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1–
Separation of a Mixture
by Distillation
Separation of a Compound
The Electrolysis of water
Compounds must be
separated by chemical
means.
With the application of
electricity, water can
be separated into its
elements
Reactant Products
Water
 Hydrogen + Oxygen
2 H2O
2 H2
+
O2
• Sketch a magnified view (showing
atoms/molecules) of each of the
following:
– a heterogeneous mixture of two different
compounds.
– a homogeneous mixture of an
element and a compound.
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1–43