1. CHAPTER 1
CE CHEMISTRY

2. SCIENTIFIC METHODS
The steps in a scientific method are repeated until a hypothesis is supported or discarded.

3. MATTER Matter is anything that has mass and takes up space Weight Mass
The law of conservation of mass states that mass is neither created nor destroyed in a chemical reaction, it is conserved.
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The mass of the reactants equals the mass of the products.
massreactants = massproducts

4. States of Matter
The physical forms of matter, either solid, liquid, or gas, are called the states of matter.
Solids are a form of matter that have their own definite shape and volume.
Liquids are a form of matter that have a definite volume but take the shape of the container.

5. Properties of Matter
Gas have no definite shape or volume. They expand to fill their container.
Vapor refers to the gaseous state of a substance that is a solid or liquid at room temperature.

6. PROPERTIES OF MATTER
THE PROPERTIES OF MATTER CANNOT BE BROKEN DOWN WITHOUT A CHEMICAL CHANGE
It is a characteristic that can be observed or measured without changing the sample’s composition.
Extensive properties, such as mass, length, and volume, are dependent on the amount of substance present.
Intensive properties, such as density, are dependent on the what the substance is not how much there is.

7. PHYSICAL PROPERTIES
is a characteristic that can be observed or measured without changing the sample’s composition.

8. PHYSICAL CHANGE
A change that alters a substance without changing its composition
Mercury
ice
transition of matter from one state to another.
Boiling, freezing, melting, and condensing all describe phase changes in chemistry

9. CHEMICAL PROPERTIES
The ability of a substance to combine with or change into one or more other substances
Iron forming rust
Copper turning green in the air
2Na(s) + Cl2(g)  2NaCl(s)
Sodium is a very reactive metal that reacts with water
Chlorine gas is a very reactive nonmetal that will form hydrochloric acid if breathed in

10. CHEMICAL CHANGE
A change that involves one or more substances turning into new substances
Decomposing, rusting, exploding, burning, or oxidizing are all terms that describe chemical changes
When sodium metal reacts with chlorine gas you produce sodium chloride salt
The physical and chemical properties change
Sodium chloride is needed for a human to survive.
Burning a piece of paper
Magnesium burn

11. SUBSTANCES PURE SUBSTANCE ELEMENT COMPOUND
pure substance that cannot be separated into simpler substances by physical or chemical means.
92 elements occur naturally on Earth
COMPOUND
made up of two or more elements combined chemically
Most of the matter in the universe exists as compounds
Unlike elements, compounds can be broken into smaller components by chemical means

12. MIXTURES
MIXTURE
a combination of two or more pure substances in which each pure substance retains its individual chemical properties
HOMOGENEOUS – a mixture where the composition is constant throughout
Also known as a solution
Salt water or air
HETEROGENEOUS – a mixture where the individual substances remain distinct
Sand or wood

13. Separating Mixtures
Filtration is a technique that uses a porous barrier to separate a solid from a liquid in a heterogeneous mixture.
Distillation is a separation technique for homogeneous mixtures that is based on the differences in boiling points of substances.
Crystallization is a separation technique for homogenous mixtures that results in the formation of pure solid particles from a solution containing the dissolved substance.
Sublimation is the process of a solid changing directly to a gas, which can be used to separate mixtures of solids when one sublimates and the other does not
Chromatography is a technique that separates the components of a mixture on the basis of tendency of each to travel across the surface of another material

14. ATOMS AND MOLECULES MOLECULES
Diatomic molecule has two same atoms (know these), Hydrogen gas(H2), Nitrogen gas(N2), Oxygen gas(O2), Fluorine gas(F2), Chlorine gas(Cl2), Bromine liquid(Br2), Iodine solid(I2)
Polyatomic molecules
ATOMS
All elements are single atoms Carbon (C), Aluminum (Al), except for the diatomic molecules

15. MATTER
heterogeneous
mixtures
homogeneous
mixtures(solutions)
physical
methods
physical
methods
pure substances
elements
compounds
chemical
methods
atoms
nucleus
protons neutrons
electrons

16. METRIC PREFIXES Giga G 109 There are 109 units (puppies) in
Mega M gigapuppy
Kilo k
Hecto h
Deca da
Unit (anything can be a unit)
Common chemistry units gram, liter, meter, second, watt
Deci d There are 101decigrams in 1 gram
Centi c
Milli m
Micro u
Nano n

17. SI UNITS moles Length is measured in meters Mass is measured in
kilograms
Time is measured in
seconds
Temperature is measured in
Kelvin
Amount of substance is
measured in
moles

18. CONVERSIONS THINGS TO REMEMBER
In the metric system, the smaller prefix unit will always have a larger number than the prefix unit it is equal to.
1000 m = 1km (overhead)
METER IS A SMALLER PREFIX UNIT
Kelvin is absolute zero or oC. You can not have a temperature lower than this so KELVIN CAN NEVER BE A NEGATIVE NUMBER
oC = K
K = oC

19. Units and Measurements
SECTION2.1
Units and Measurements
Zero kelvin is the point where there is virtually no particle motion or kinetic energy, also known as absolute zero.
Two other temperature scales are Celsius and Fahrenheit.
F = 1.8 C + 32

20. TEMPERATURE Celsius (oC) Freezing of water 0 oC
Boiling of water oC
Convert the following temperatures
323 K to oC
-20 oC to K
129 K to oF

21. Representing Data Graphing
On line graphs, independent variables are plotted on the x-axis and dependent variables are plotted on the y-axis.

22. Significant Figures Often, precision is limited by the tools available
Significant figures include all known digits plus one estimated digit

23. SIGNIFICANT FIGURES
State of degree of confidence in the measurement cited
Pacific and Atlantic rule
If there is a decimal point present, start from the left, go to the first nonzero number. Start counting the numbers
0.0025
1.109
57000.
If there is no decimal point, start from the right, go to the first nonzero number. Start counting the number
57000
100600
Three students weigh an object on different balances. How many significant figures are there in each value?
A g
B g
C kg

24. ROUNDING NUMBERS OFF
In a series of calculations carry all digits unit the final solution, THEN ROUND
If a digit needs to be rounded
If it is less than 5, the preceding digit remains the same
4.499
5.234
If the digits are equals or is greater than 5, the preceding digit is increased by one.
4.8501
506
5.236
A person’s height is measured to be inches. What is the height in centimeters? (Hint 1 inch = 2.54 cm)

25. UNCERTAINTIES IN MULTIPLICATION, DIVISION, ADDITION, AND SUBTRACTION
Multiplication and division
Least number of significant figures
Addition and subtraction
Least accurate number
Three students each weigh a object
Student g
Student g
Student g
How many sig. figs. Should be reported for the total weight?

26. EXACT NUMBERS What is an exact number?
1 cal = J gives two conversion factors
1cal J
4.184 J cal
A piece of iron with a volume of 2.50 gal weighs lbs. Calculate the density of iron in scruple/drachm. Some conversion factors are:
1.00 L = gal mL = drachm
1.000 kg = lb g = 1 kg
1.000 scruple = g 1000 mL = 1 L

27. SCIENTIFIC NOTATION All chemistry uses scientific notation
Uses the base 10
1000 = 10 x 10x 10 =103
0.001=1/1000=1/10 x 1/10 x 1/10=10-3
23000 = 2.3 x 104
1010. = x 103
= 1.20 x 10-3

28. PERCENTAGES Calculating percentages
Percent =number of specific items x 100
Total items in the group
A count of white blood cells was found in a patient, if the normal white blood count is What percent of white blood cells does this patient have?

29. DENSITY
Density is a derived unit, g/cm3, the amount of mass per unit volume.
The density equation is density = mass/volume
A merchant sold you a chain that was suppose to be pure gold. You took it home, when you weighed it was 23.5 g. You then filled up a graduated cylinder to mL, when you put the chain in the water it went up to mL. Is this pure gold? (Hint gold’s density is 19.2 g/mL)