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
“I’m Curious…”:
Generate a list of at least three things that
you’re most curious about in chemistry.
The Study of
Chemistry
Properties of
Matter
Units of
Measurement
Uncertainty
in
Measurement
Dimensional
Analysis
Essential Question (E.Q.): Can I explain from my perspective
what chemistry is about and why it is useful to learn
chemistry?

Study of composition and behavior of matter.

Matter – Physical material of the universe. Has
mass, occupies space, and created by elements.

Atom – Building block of matter.

Element – Basic particles created by atoms.
117 are currently known!

Every change in our observable world has
its basis in the world of atoms.

We’ll speak in terms of two realms:
Macroscopic (Macro = large)
Submicroscopic ( Atoms, compounds, and
molecules.



Understand how the world works
Extremely practical!
Public concern
Environmental protection
Food, clothing, and shelter
Food production
Understand how chemicals effect us

Chemistry – THE CENTRAL SCIENCE

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

Top Eight Chemicals Produced by the Chemical
Industry
Ran
k
Chemical
Formul
a
2006
Production
Principal Uses
1
Sulfuric Acid
H2SO4
79B pounds
Fertilizers
2
Ethylene
C2H4
55B pounds
Plastics, antifreeze
3
Lime
CaO
45B pounds
Paper, cement
4
Propylene
C3H6
35B pounds
Plastics
5
Phosphoric acid
H3PO4
24B pounds
Fertilizers, Coca-Cola
6
Ammonia
NH3
23B pounds
Fertilizers
7
Chlorine
Cl2
23B pounds
Bleaches, plastics
8
Sodium
hydroxide
NaOH
18B pounds
Aluminum
production, soap
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Baking Soda
Borax
Clorox™
Hydrogen Peroxide
Pepto-Bismol™
Vinegar
Windex™
Zerex™ (Antifreeze)
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Sodium bicarbonate
Sodium borate
Sodium hypochlorite
Hydrogen peroxide
Bismuth subsilicate
Acetic acid
Acetic acid
Ethylene glycol

Plants
 Respiration
 Plant Defense
 Seasonal Change

Animals
 Respiration
 Defense/Immunity
 Growth and reproduction


Discuss what chemicals you’d like to learn
more about.
*Explain from your perspective what
chemistry is about and why its useful to
learn chemistry.

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
What is chemistry about?
What is matter composed of?
Where is chemistry useful?
Study your notes!

In a brief paragraph, opine how cooking and
chemistry are alike.
The Study of
Chemistry
Properties of
Matter
Units of
Measurement
Uncertainty
in
Measurement
Dimensional
Analysis
E.Q.: Can I identify and explain the different properties of
matter?

Each substance has a unique set of properties.

These properties can be physical or chemical.

Physical Property – Physically observable
properties (color, odor, density, melting point,
boiling point, and hardness).

Chemical Property – Describes a substance by
its identity (reactivity and flammability).
Copper is redbrown, opaque,
solid: physical
properties.

Observe the image...
Ethanol is flammable:
a chemical property.

With physical and chemical properties
come physical and chemical changes!

Physical Property – Changes physical
appearance but not its chemical identity.
 Ex. Changes of state: boiling, freezing,
sublimation, etc.

Chemical Property – Changes a chemical
identity.
 Ex. Chemical reactions

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Physical change - No
change in composition.
No new substances are
formed.
 Ex. Evaporation; melting;
cutting wood; dissolving
sugar in water.
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Chemical change or
chemical reaction - A
change in composition.
New substances are
formed.
 Ex. Burning gasoline;
dissolving metal in acid;
spoilage of food.
The vapor burns,
combining with
oxygen: a
chemical change.
The liquid fuel
evaporates: a
physical change.
19
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Because each component of mixtures has its
own properties, we can separate a mixture
into its components. Three methods:

Chromatography

Distillation
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Filtration

Identify each as a physical or chemical
change:
 Photosynthesis
 Water vapor in the air on a cold day forms frost.

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
What are the properties of matter?
What type of changes can matter undergo?
What are the three types of separation
techniques?
Study Your Notes!

In a brief paragraph, explain everything you
know about units of measurement.
The Study of
Chemistry
Properties of
Matter
Units of
Measurement
Uncertainty
in
Measurement
Dimensional
Analysis
E.Q.: How do I explain the importance of accurate units of
measurement in chemical and physical processes?

Many properties of matter are quantitative.
 Quantitative – Relating to NUMBERS!

When a number represents a measurement, its
units must be specified.

The units used for scientific measurement are
those of the metric system.

In 1960, an international agreement was
reached to expressed a choice of metric units –
SI Units.
SI Base Units
Physical Quantity
Name of Unit
Abbreviation
Mass
Kilogram
kg
Length
Meter
m
Time
Second
s
Temperature
Kelvin
K
Amount of Substance
Mole
mol
Electric Current
Ampere
A
Luminous Intensity
Candela
cd
Metric Prefixes
Prefix
Abbreviation
Meaning
Example
Tera
T
1012
1 gigameter (Tm) = 1 x 1012 m
Giga
G
109
1 gigameter (Gm) = 1 x 109 m
Mega
M
106
1 megameter (Mm) = 1 x 106 m
Kilo
K
103
1 kilometer (km) = 1 x 103 m
Deci
d
10-1
1 decimeter = 1 x 10-1 m
Centi
c
10-2
1 centimeter = 1 x 10-2 m
Milli
m
10-3
1 millimeter = 1 x 10-3 m
Micro
μ
10-6
1 micrometer = 1 x 10-6 m
Nano
n
10-9
1 nanometer = 1 x 10-9 m
Pico
p
10-12
1 picometer = 1 x 10-12 m
Fempto
f
10-15
1 femptomenter = 1 x 10-15 m

Measure of the hotness or coldness of an
object.

Speed

Force

Pressure

Energy

Density…The only one that we’ll look at!

Burette

Syringe

Pipette

Graduated Cylinder

Volumetric Flask

Property of matter defined as the amount of
mass in a unit of volume of substance.

Usually expressed in grams per milliliter
(g/mL).

More dense items sink; less dense float!
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Biofuels

New element created (Element 118)

Antibiotic Modified to Combat Bacterial
Resistance

The Hole Story (Ozone)

Calculate the density of 18.0g of mercury
occupying a volume of 100.0mL.

Indicate the SI units for mass, length,
volume, and temperature.

Units of Measurement…

Density…
Study Your Notes!

What is meant by the term “Uncertainty”?
The Study of
Chemistry
Properties of
Matter
Units of
Measurement
Uncertainty
in
Measurement
Dimensional
Analysis
E.Q.: Can I realize the relationship between accuracy and
precision?

Two types of numbers are encountered in
scientific work:

Exact numbers (1 dozen = 12, 1.0m =
100cm)
Inexact numbers (Numbers obtained by
measurement)


Which of the following is an exact number?
 Number of students in class OR mass of a penny
PRECISION

How closely many
measurements agree with
one another
ACCURACY

How closely many
measurements agree with
the “correct” value

Uncertainties always exist in
measurements.

These uncertainties are shown by
significant figures.

Significant figures - All digits of a measured
quantity.
2.2g = 2 sig figs
5.46g = ______ sig figs
2.2405g = 5 sig figs
1.67g = ______sig figs

Zeros between nonzero digits are always
significant – 1005kg (four); 1.03kg (three)

Zeros at the beginning of a number are
never significant – 0.02L (one); 0.0026L
(two)

Zeros at the end of a number are significant
if number contains a decimal – 0.0200kg
(three)
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General: Base the number of digits in a result
on the measurements and not on known
values (such as atomic masses, accurately
known densities, other physical constants, etc.)
Multiplication and division:
 Use the same number of sig figs in the result as the
data with the fewest sig figs.

Addition and Subtraction:
 Use the same number of decimal places in the result
as the data with the fewest decimal places.
45
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WE GO LUNCH AT 11:42004332233AM!!!

I WEIGH 187.0004LBS!!!

The width, length, and height of a small box
are 15.5cm, 27.3cm, and 5.4cm. Calculate
the volume of the box using correct sig figs!

10.5m x 100.00m = _________m2

(3.2 + 12.00)g = _________g
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
Uncertainty in Measurements…
Accuracy vs. Precision…
Sig Figs…

Try these at home:

3.45g + 5.00g = _________g

100.5m - 10.00m = _________m2

2.30m x 5.00m = _________m2

100.00m2 / 10.00m = _________m2

In your own words, define analysis.
The Study of
Chemistry
Properties of
Matter
Units of
Measurement
Uncertainty
in
Measurement
Dimensional
Analysis
E.Q.: How is dimensional analysis used to solve scientific
problems?

An aid in problem solving

Units “cancel out” to yield proper answers.

If a woman has a mass of 115lb, calculate
her mass in grams. (HINT: 1.0lb = 453.6g)

We also have conversion factor that convert
from one measure to a different measure.

The average speed of a nitrogen molecule in
air is 515m/s. Convert this speed to miles
per hour (mph). (1600m = 1.0mi)

A car travels 28mi per gallon (mpg) of
gasoline. Convert these unit to km per liter
(km/L). (HINT: 3.8L = 1.0 gallon).

Using your knowledge of metric units,
convert the following:
 0.076L to mL
 0.05m to mm
 5.0 days to seconds.

ACCELERATED: Try these also!
 Speed of light is 3.00 x 108m/s to miles per hour
(mph)
 5.85gal/hr to liters per second (L/s)
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
Dimensional analysis...
Measurement conversions...
Study your notes!