Chapter 1
Matter and Energy
What is Chemistry
Chemistry is the study of matter and its
changes
What is Matter?
Matter is anything that occupies space
and has weight.
Examples of Matter
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•
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•
•
•
Pens and pencils
Paper
Students
Desks
Cars
Airplanes
Is Air Matter?
Air would be matter if it takes up space
and has weight.
Is Air Matter?
Air would be matter if it takes up space
and has weight.
Does it?
Is Air Matter?
Air would be matter if it takes up space
and has weight.
Does it?
The space that air takes up is called the
atmosphere.
Does air have weight?
Is Air Matter?
Air would be matter if it takes up space
and has weight.
Does it?
The space that air takes up is called the
atmosphere.
Does air have weight?
Yes air does have weight, if not, then it
would flow into outer space.
Is Air Matter?
Air would be matter if it takes up space and
has weight.
Does it?
The space that air takes up is called the
atmosphere.
Does air have weight?
Yes air does have weight, if not, then it
would flow into outer space. One liter of air
weighs 1.29 grams.
What are Changes?
In the study of chemistry we talk about two
different kinds of changes, physical and
chemical
What are Changes?
In the study of chemistry we talk about two
different kinds of changes, physical and
chemical
Physical change is a change to matter so that
the identity is not altered; i.e. taste, smell….
What are Changes?
In the study of chemistry we talk about two
different kinds of changes, physical and
chemical
Physical change is a change to matter so that
the identity is not altered; i.e. taste, smell….
Chemical change is a change to matter so that
its identity is changed; i.e. different smell, color,
taste.
Examples of Physical Change
• Tearing paper; starts out paper and ends as
paper
• Folding paper ; starts out paper and ends as
paper
• Melting of ice ; starts out water and ends as
water
• Evaporation of water ; starts out water and
ends as water
Examples of Chemical Change
• Wood burning; starts out as wood ends up
as smoke and ashes, different smell and
taste, right?
• Steel rusting; starts out as steel ends up
as rust, different smell and taste
• Healing of a wound; starts out a blood
ends up as scar tissue, different color,
taste and smell
Matter Continued
Is everything matter?
Matter Continued
Is everything matter? No, not everything we
can think of has weight and takes up space.
Matter Continued
Is everything matter? No, not everything we
can think of has weight and takes up space.
For example personality!
Matter Continued
Is everything matter? No, not everything we
can think of has weight and takes up space.
For example personality! One might argue
that personality takes up the space of ones
brain or person, but…
Matter Continued
Is everything matter? No, not everything we
can think of has weight and takes up space.
For example personality! One might argue
that personality takes up the space of ones
brain or person, but…not all personable
people are overweight. Thus personality
does not have weight, and is therefore not
matter.
Matter Continued
How about thought? Again we might argue
that thought takes up the space of ones
brain and your mother told you about heavy
thoughts, but….
Matter Continued
How about thought? Again we might argue
that thought takes up the space of ones
brain and your mother told you about heavy
thoughts, but….If you get on the bathroom
scale and start having heavy thoughts, your
weight does not go up!
Matter Continued
How about thought? Again we might argue
that thought takes up the space of ones
brain and your mother told you about heavy
thoughts, but….If you get on the bathroom
scale and start having heavy thoughts, your
weight does not go up! That means
thought is not matter, so if someone studies
thought, they are not doing chemistry.
Examples of Chemistry
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•
•
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The study of why wood burns
The study of why cement does not burn
The study of why nails rust
The study of milk spoiling
These all fit the definition of chemistry since
they deal with change and matter
History of Chemistry
Who were the first chemists?
History of Chemistry
Who were the first chemists?
History of Chemistry
Who were the first chemists?
Cavemen
History of Chemistry
What kind of matter and changes did the
cavemen study?
History of Chemistry
What kind of matter and changes did the
cavemen study? Fire and food!
Archeologists have found evidence of fire in
caves and animal bones too. Cooking meat
makes meat chewable. Chewing raw meet
wears out ones jaw.
History of Chemistry
The next group that left archeological
evidence of chemistry were the Egyptians.
Their chemistry involved mummies, textile
dyes, ink, paper and paints most of which
can be found inside the pyramids.
History of Chemistry
The first group of people to leave written
records of their chemistry were the Greeks.
From Greek writings, we can see that the
Greeks made observations, and created
reasons for these observations, called
hypothesis. They did not attempt to prove
their hypothesis by experimentation, thus
their chemistry efforts were philosophical in
nature as opposed to science in nature.
History of Chemistry
The first group of chemists to test hypothesis
with experiments were the alchemists.
Alchemists were a group of Europeans that
were trying to change matter in to different
kinds of matter. For example, they were trying
to change lead into gold. The major results of
their experiments were to prove most of the
Greek ideas of chemistry to be false and to
show a clear distinction between science and
philosophy.
History of Chemistry
A major short coming of the Alchemists
chemistry was irreproducible results, caused
by lack of measurement understanding. For
example, on day 1 mixing two kinds of
matter produced black matter, while doing
the same thing the next day produced red
matter. The Alchemists were the first group
of chemists to make observations, create
hypothesis, and to test their hypothesis
with experiments.
Modern Chemistry
Antoine Lavoisier was the founder of
modern chemistry by making careful
measurements.
Modern Chemistry
Lavoisier’s careful measurements now
made experiments reproducible. Chemists
in other countries could now do the same
experiment and get the same results. This
now allowed chemists to prove a
hypothesis to be correct by
experimentation, thus leading to the
discovery of theories and laws.
Modern Chemistry
Lavoisier’s Theories and Laws
• Law of Conservation of Mass
• Atomic Theory
Scientific Method
Is a sequence of thoughts and
experiments containing the
following:
• A hypothesis is a tentative and
testable explanation for an
observation or a series of
observations.
• A scientific theory is a general
explanation of widely observed
phenomena that have been
extensively tested.
Classification of Matter
Matter
Homogeneous
Substances
Elements
Heterogeneous
Solutions
Compounds
Classification of Matter
Homogeneous and Heterogeneous
Homogeneous matter looks the same
everywhere with a microscope, but since
we lack microscopes we will use our eyes
and not our imagination. Heterogeneous
matter does not look the same
everywhere.
Classification of Matter
Homogeneous or Heterogeneous?
Wood
Carpet
Margarine
Gold
Classification of Matter
Homogeneous or Heterogeneous?
Wood
Heterogeneous
Carpet
Margarine
Gold
Classification of Matter
Homogeneous or Heterogeneous?
Wood
Carpet
Heterogeneous Heterogeneous
Margarine
Gold
Classification of Matter
Homogeneous or Heterogeneous?
Wood
Carpet
Heterogeneous Heterogeneous
Margarine
Homogeneous
Gold
Classification of Matter
Homogeneous or Heterogeneous?
Wood
Carpet
Heterogeneous Heterogeneous
Margarine
Gold
Homogeneous Homogeneous
Classification of Matter
Solution is a homogeneous random
combination of two or more different types of
matter.
For example a random amount of salt and
water combined together produces a
homogeneous mixture, called salt water.
Random combination means some salt and
some water.
Classification of Matter
Any combination the produces a
homogeneous result that is not randomly
created is called a substance.
For example, combining two hydrogen atoms
and one oxygen atom produces a compound
of water, which is a substance. Or the
combination of two oxygen atoms, gives a
molecule of oxygen.
Classification of Matter
Homogeneous matter created by the same
atom is called and element. Exact
combinations of different elements is called
a compound.
Classification of Matter
Label the following examples of matter as
heterogeneous, solution, compound or element.
• Sand
• Sea water
• Tap water
• Steel
• Antimony
• Air
• Distilled water
• Cement
• Wine
Classification of Matter
Label the following examples of matter as
heterogeneous, solution, compound or element.
• Sand-Heterogeneous
• Sea water
• Tap water
• Steel
• Antimony
• Air
• Distilled water
• Cement
• Wine
Classification of Matter
Label the following examples of matter as
heterogeneous, solution, compound or element.
• Sand-Heterogeneous
• Sea water-Heterogeneous
• Tap water
• Steel
• Antimony
• Air
• Distilled water
• Cement
• Wine
Classification of Matter
Label the following examples of matter as
heterogeneous, solution, compound or element.
• Sand-Heterogeneous
• Sea water-Heterogeneous
• Tap water-Solution
• Steel
• Antimony
• Air
• Distilled water
• Cement
• Wine
Classification of Matter
Label the following examples of matter as
heterogeneous, solution, compound or element.
• Sand-Heterogeneous
• Sea water-Heterogeneous
• Tap water-Solution
• Steel-Solution
• Antimony
• Air
• Distilled water
• Cement
• Wine
Classification of Matter
Label the following examples of matter as
heterogeneous, solution, compound or element.
• Sand-Heterogeneous
• Sea water-Heterogeneous
• Tap water-Solution
• Steel-Solution
• Antimony-Element
• Air
• Distilled water
• Cement
• Wine
Classification of Matter
Label the following examples of matter as
heterogeneous, solution, compound or element.
• Sand-Heterogeneous
• Sea water-Heterogeneous
• Tap water-Solution
• Steel-Solution
• Antimony-Element
• Air-Solution
• Distilled water
• Cement
• Wine
Classification of Matter
Label the following examples of matter as
heterogeneous, solution, compound or element.
• Sand-Heterogeneous
• Sea water-Heterogeneous
• Tap water-Solution
• Steel-Solution
• Antimony-Element
• Air-Solution
• Distilled water-Compound
• Cement
• Wine
Classification of Matter
Label the following examples of matter as
heterogeneous, solution, compound or element.
• Sand-Heterogeneous
• Sea water-Heterogeneous
• Tap water-Solution
• Steel-Solution
• Antimony-Element
• Air-Solution
• Distilled water-Compound
• Cement-Heterogeneous
• Wine
Classification of Matter
Label the following examples of matter as
heterogeneous, solution, compound or element.
• Sand-Heterogeneous
• Sea water-Heterogeneous
• Tap water-Solution
• Steel-Solution
• Antimony-Element
• Air-Solution
• Distilled water-Compound
• Cement-Heterogeneous
• Wine-Solution
Classification of Matter
•
Types of Matter
1. Pure Substances have the same
physical and chemical properties
throughout.
2. Mixtures are composed of two or more
substances (elements or compounds) in
variable proportions.
Elements and Compounds
• Most elements are not found in the world in
the pure form. They are found in compounds.
• Hydrogen is found in water, H2O, and other
hydrogen containing compounds.
• The law of constant composition states that
every sample of a compound always contains
the same elements in the same proportions.
Pure Substances
•
Two Groups
1. An element is the simplest kind of
material with unique physical and
chemical properties.
2. A compound is a substance that
consists of two or more elements linked
together in definite proportions.
An Atomic View
• An atom is the smallest particle of an element
that retains the chemical characteristics of
that element.
• A molecule is a collection of atoms chemically
bonded together having constant proportions.
Chemical Formulas
• Chemical bonds link
atoms together to
make molecules.
• Chemical formulas
use symbols to
represent atoms with
subscripts to identify
the number of each
atom present.
Chemical Reactions
• Chemical reactions show
the transformation of one
or more substance into
different substances.
• Chemical equations use
chemical formulas to
express the identities and
quantities of substances
involved in a reaction
Separating Mixtures
• No chemical reactions are needed to
isolate the constituents in a mixture.
 Filtration
 Distillation
Filtration
Distillation
Properties of Matter
• Intensive property - a characteristic that is
independent of the amount of substance
present.
Examples: color, hardness, etc.
• Extensive property - a characteristic that
varies with the quantity of the substance
present.
Examples: length, width, mass, etc.
State of Matter
• Solids have definite shapes and
volumes.
• Liquids occupy definite volumes, but do
not have definite shapes.
• Gases have neither a definite shape nor
volume.
• Plasma, not found on earth, but stars,
similar to a gas, but a mixture of
subatomic particles
Examples
Making Measurements
• Accurate measurements are essential
for our ability to characterize the
physical and chemical properties of
matter.
• Standardization of the units of
measurements is essential.
Some Prefixes for SI Units
Memorize the ones in blue
Prefixes
Value
Name
Symbol
Exponential
Mega
M
106
Kilo
k
103
Hecto
h
102
Deka
da
10
Deci
d
10-1
Centi
c
10-2
Milli
m
10-3
Micro

10-6
Nano
n
10-9
Pico
p
10-12
SI Base Units
Quantity
Unit Name
Unit
Abbreviation
Mass
Length
Temperature
Kilogram
Meter
Kelvin
kg
m
K
Time
Energy
Second
Joule
s
J
Electrical Current
Amount of
Substance
Ampere
A
Mole
mol
Luminosity
Candela
cd
English Metric Conversions
These are definitions, thus lacking significant figures
• 1 in = 2.54 cm
Length
• 1 lb = 453.6 g
Mass
• 1qt = 946.4 mL
Volume
Scientific Measurements
• A measurement always has some
degree of uncertainty due to the fact
that measuring devices have scales. A
digit that must be estimated is called
uncertain due to the fact that it is
between the scale lines, or appears to
be on a scale line.
Counting Significant Figures
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•
•
•
All numbers counted in a measurement are
significant.
Zero’s sandwiched by two numbers are
counted.
If a zero is used to locate a decimal, then it
is not a number, but a spacer and is not
counted.
Additional information sometimes is
available the make zeros both numbers and
decimal spacers.
Practice
How many significant figures are in the
following numbers?
0.04550 g
100 lb
101.05 mL
350.0 g
Practice
How many significant figures are in the
following numbers?
0.04550 g
100 lb
101.05 mL
350.0 g
Practice
How many significant figures are in the
following numbers?
0.04550 g
100 lb
101.05 mL
350.0 g
4 significant figures
Practice
How many significant figures are in the
following numbers?
0.04550 g
4 significant figures
100 lb
1 significant figure
101.05 mL
350.0 g
Practice
How many significant figures are in the
following numbers?
0.04550 g
4 significant figures
100 lb
1 significant figure
101.05 mL
5 significant figures
350.0 g
Practice
How many significant figures are in the
following numbers?
0.04550 g
4 significant figures
100 lb
1 significant figure
101.05 mL
5 significant figures
350.0 g
4 significant figures
Practice
How many significant figures are in the
following numbers?
0.04550 g
4 significant figures
100 lb
1 significant figure
101.05 mL
5 significant figures
350.0 g
4 significant figures
Counting Significant Figures
• Exact numbers have an infinite
number of significant figures.
• Exact numbers are either counted
or defined.
• 1 inch = 2.54 cm, exactly
Rounding Rules
• Addition and Subtraction: Round
answer so that it contains the same
number of decimal places as the
measurement with the lease
number of decimal places.
• 6.8 + 11.934 = 18.734
 18.7 (1 decimal
place)
Rounding Rules
• Multiplication and Division: Round
answer so that it contains the same
number of significant figures as the
measurement with the least number of
significant figures.
• 6.38  2.0 = 12.76  13 (2 sig figs)
Precision and Accuracy
Precision is how close measurements are to each other
Accuracy is how close a measurement is to the true value.
Unit Conversion Accidents
There have been many serious incidents that have resulted from
errors in converting between systems of units.
Air Canada Flight 143
(Google it for more details)
Unit Conversion Accidents
$125 million Mars Climate Orbiter.
Lost in Space.
Dp you think there is the potential to make errors in the
conversion of units for health care providers?
Conversion Problem Steps
1. Write down the number and unit.
2. Draw lines; a vertical line after the number an
unit and horizontal line below the number and
unit.
3. Insert a fractional fact to cancel out the
original unit.
4. Compare the new unit to the asked for unit
a. If the same, you are done.
b. If not the same, repeat step 3.
Sample Conversion Problems
1. How many grams are in 47.2 mg?
2. Change 702 cL to µL.
Step 1. Write down the number and unit.
47.2 mg
Sample Conversion Problems
1. How many grams are in 47.2 mg?
2. Change 702 cL to µL.
Step 1. Write down the number and unit.
47.2 mg
Step 2. Draw lines
47.2 mg
Sample Conversion Problems
1. How many grams are in 47.2 mg?
2. Change 702 cL to µL.
Step 1. Write down the number and unit.
47.2 mg
Step 2. Draw lines
47.2 mg
Step 3. Insert fractional fact crossing out original unit
Sample Conversion Problems
1. How many grams are in 47.2 mg?
2. Change 702 cL to µL.
Step 1. Write down the number and unit.
47.2 mg
Step 2. Draw lines
47.2 mg
Step 3. Insert fractional fact crossing out original unit
47.2 mg 10-3 g
mg
Sample Conversion Problems
1. How many grams are in 47.2 mg?
2. Change 702 cL to µL.
Step 1. Write down the number and unit.
47.2 mg
Step 2. Draw lines
47.2 mg
Step 3. Insert fractional fact crossing out original unit
47.2 mg 10-3 g
mg
Step 4. Compare new unit to the asked for unit.
Sample Conversion Problems
1. How many grams are in 47.2 mg?
2. Change 702 cL to µL.
Step 1. Write down the number and unit.
47.2 mg
Step 2. Draw lines
47.2 mg
Step 3. Insert fractional fact crossing out original unit
47.2 mg 10-3 g
mg
Step 4. Compare new unit to the asked for unit.
A. If the same you are done
b. If not the same repeat step 3.
Sample Conversion Problems
1. How many grams are in 47.2 mg?
2. Change 702 cL to µL.
Step 1. Write down the number and unit.
47.2 mg
Step 2. Draw lines
47.2 mg
Step 3. Insert fractional fact crossing out original unit
47.2 mg 10-3 g
= 0.0472 g
mg
Step 4. Compare new unit to the asked for unit.
A. If the same you are done
b. If not the same repeat step 3.
Sample Conversion Problems
1. How many grams are in 47.2 mg?
2. Change 702 cL to µL.
Step 1. Write down the number and unit.
702 cL
Step 2. Draw lines
702 cL
Step 3. Insert fractional fact crossing out original unit
10-2 L
cL
Step 4. Compare new unit to the asked for unit.
A. If the same you are done
b. If not the same repeat step 3.
702 cL
Sample Conversion Problems
1. How many grams are in 47.2 mg?
2. Change 702 cL to µL. Not a match repeat step #3
Step 1. Write down the number and unit.
702 cL
Step 2. Draw lines
702 cL
Step 3. Insert fractional fact crossing out original unit
10-2 L
cL
Step 4. Compare new unit to the asked for unit.
A. If the same you are done
b. If not the same repeat step 3.
702 cL
Sample Conversion Problems
1. How many grams are in 47.2 mg?
2. Change 702 cL to µL. It’s a match, done
Step 1. Write down the number and unit.
702 cL
Step 2. Draw lines
702 cL
Step 3. Insert fractional fact crossing out original unit
10-2 L μL
cL
10-6 L
Step 4. Compare new unit to the asked for unit.
A. If the same you are done
b. If not the same repeat step 3.
702 cL
Sample Conversion Problems
1. How many grams are in 47.2 mg?
2. Change 702 cL to µL. It’s a match, done
Step 1. Write down the number and unit.
702 cL
Step 2. Draw lines
702 cL
Step 3. Insert fractional fact crossing out original unit
702 cL
10-2 L μL
cL
10-6 L
= 7.02 x 106 μL
Step 4. Compare new unit to the asked for unit.
A. If the same you are done
b. If not the same repeat step 3.
DENSITY
• What is heavier 5 pounds of lead or 5
pounds of feathers?
• What takes up more space, 5 pounds of
lead or 5 pounds of feathers?
DENSITY
• What is heavier 5 pounds of lead or 5
pounds of feathers? Both the same.
This is an old riddle to confuse density
with weight
• What takes up more space, 5 pounds of
lead or 5 pounds of feathers?
DENSITY
• What is heavier 5 pounds of lead or 5
pounds of feathers? Both the same.
This is an old riddle to confuse density
with weight
• What takes up more space, 5 pounds of
lead or 5 pounds of feathers? Feathers,
since they are less dense.
Archimedes Principle
We can determine the volume of irregularly shaped objects by
displacement.
How can we determine the volume of a gas?
Gases fill whatever container they are placed in. So it’s the
volume of the container !
DENSITY UNITS
g/ml, g/cm3, (for solids and liquids), or g/L for
gases
The End
MATTER AND ENERGY