1) Chemistry is the study of matter and its properties. Matter can exist as solids, liquids, or gases and can undergo physical or chemical changes. 2) The metric system is the international standard for measurement and uses base units related by powers of 10. Measurements include mass, volume, length, and temperature. 3) Energy exists in various forms and can be transformed from one to another but not created or destroyed. Chemical energy is stored in chemical bonds and released during chemical reactions.

1. Chapter One
Matter Energy and Measurement

2. The Central Science?

3. • Matter can change from one form to another:
• matter is anything that has mass and takes up
space
• Chemistry is the study of matter
1) Physical changes
2) Chemical changes

4. • occur when objects undergo a change that
does not change their chemical nature
Examples of physical change include:
• Change of state
• Creation or separation of a mixtures
• Physical deformation

5. 1) Physical Properties of Matter
Those characteristics that can be
observed without changing the
substance into another substance:
 Color
 Taste
 Density (g/ml)
 Melting point
 Odor
 Hardness
 Solubility
 Boiling point

6. • occur when substance(s) are changed into
another substance(s), involving chemical
reactions
• A chemical reaction produces new substances
by changing the way in which atoms are
arranged
Examples include:
• rusting or oxidation
• digestion of food
• bleaching hair
• burning propane
CH3CH2CH3 + 5O2 3CO2 + 4H2O

7. 2) Chemical Properties of Matter
Those characteristics that
can be observed when the
substance undergoes a
change in composition
 reactivity
 combustibility

8. Changes in Matter
1) Physical Changes: does not alter the
composition of the substance
2) Chemical Changes or Chemical
Reactions: alters the composition

9. Physical or Chemical changes?
1) Melting a marshmallow
2) Burning a marshmallow
3) Cutting paper
4) Rusted nail
5) Digestion of food
6) Evaporation
7) Striking a match
8) Bleaching hair

10. • Fact is a statement based on direct experience
• Hypothesis is a statement that is proposed, without
actual proof, to explain the facts and their
relationships
• Theory is the formulation of an apparent relationship
of certain observed phenomena
• is the process by which scientists, collectively
and over time, endeavor to construct an
accurate representation of the world
Fact Hypothesis Theory Law

11. The Scientific Method

12. •Used to represent very large or very small numbers
as powers of 10
Examples:
0.00002 is written as 2 x 10-5
2,000,000 is written as 2 x 106
Exponential Notation

13. • is the number of digits of a measured number
that have uncertainty only in the last digit
Rules:
1. Nonzero digits are always significant
2. Zeros at the beginning of a number are never significant
3. Zeros between nonzero digits are always significant
4. Zeros at the end of a number that contains a decimal point
are always significant
* Additional rules apply for addition and multiplication/ dividing (Appendix II)
Significant Figures

14. Measurements and the Metric System

16. • consist of 2 parts: number and unit
• The metric system uses one base unit for each
kind of measurement
Measurements

17. • The metric system uses units that are related
by powers of 10

18. • Mass vs. Weight
• Mass is the quantity of matter in an object and is
independent of weight
• Weight is the force mass experiences under the pull
of gravity
• Volume
1 mL = 1 cc
• Volume is the space occupied by that substance

19. temperature
degree
Celsius
degree
Fahrenheit
symbol °C °F
boiling point of water 100 212
average human body
temperature
37 98.6
average room
temperature
20 to 25 68 to 77
melting point of ice 0 32
˚F = 9/5 ˚C + 32
˚C = 5/9 (˚F – 32)

20. • The size of Kelvin degree
is the same as Celsius
•The only difference is the
zero point
• Absolute zero = 0˚K
0˚K = -273˚C

21. • converting one unit into another:
grams (g) to centigrams (mg)
pounds (lbs) to grams (g)
liters (l) to milliliters (ml)
kilometers (km) to miles
• Examples
If the speed limit is 70 km/h, what is the speed limit in miles per
hour?
70 km
1.0 hr
x
1.0 mile
1.609 km
= 44 mph
Convert 525 mm to cm
525 mm x 1m x
m1
100cm
1000 mm
= 52.5 cm
Factor Label Method for Unit Conversions

22. • matter can exist in 3 states: gas, liquid, and
solid
• Gases have no definite shape or volume 
highly compressible
• Liquids have no definite shape but they do
have a definite volume  slightly compressible
• Solids have a definite shape and a definite
volume  incompressible
• most substances can exist in all 3 states:
temperature dependent

23. The Three Physical State of Matter

24. • defines as mass per unit volume
• is a physical property that is constant at a
given temperature
• density usually increases with decreasing
temperature  water is an exception
• for liquids and solids: g/ml
• for gas: g/L
d =
m
d = density
m = mass
V = volumeV

25. • is a physical property
that is numerically the
same as density but
has no units
• specific gravity is a
comparison of density of a
substance with the density
of H2O
The density of H2O at 1˚C
is 1.00 g/ml
Urinometer

26. • is defined as the ability to do
work or to bring about change
• kinetic energy is the energy of motion:
mechanical energy, light, heat, electrical energy
• potential energy is stored energy

27. •In chemistry, the most important form of
potential energy is chemical energy
•chemical energy is stored in chemical
substances, as for example in foods such as
carbohydrates and fats it is given off when
substances take part in chemical reactions

28. First Law of Thermodynamics:
Law of conservation of energy
 Energy can be neither created nor
destroyed, it can only be transformed from
one form to another.
 No energy transformation is 100% efficient
 % efficiency = usable energy X 100
total energy
 Humans are only 20-25%
efficient
 Wasted energy is usually
lost as heat

29. • heat is a form of energy but temperature is not
• heat is commonly measured in calories (cal)
• calorie is the heat necessary to raise the
temperature of 1 g of water by 1˚ C
• Nutritionists use Calories (C)
1 C = 1000 cal = 1 kcal

30. • the heat necessary to raise the temperature of
1 g of any substance by 1˚ C
Specific Heat