• Physical properties: mass, volume, color,
hardness, melting point, boiling point
• Chemical properties: reactivity, flammability,
ability to rust (react with oxygen)
• Physical Changes : evaporating, melting,
condensing, breaking, cutting
• Chemical Changes : corroding, exploding,
rotting, reacting, burning
Chemistry – the study of the composition of
matter and the changes it undergoes
How many sig fig do the following have?
Round each to the number in parentheses.
a. 0.0002030 (2) --> .00020
b. 99,000 (1)  100,000
c. 10.00 (2)  10.
d. 50,000. (1)  50,000
e. 0.00001 (1)  0.00001
Express the following, using the correct number
of sig figs:
a. 2.220 x 5.00 = 11.1
b. 5.00 + 162.10 = 167.10
c. 3.20 / 6.232 = .513
d. 232 – 16.23 = 216
• Express the quantity .000075 nm in meters
(109 nm = 1m)
• Answer  7.5 x 10 -14
• Convert 987,000,000 micrograms to
kilograms (106 mg = 1 g) (103 g = 1 kg)
Answer  .987
• What is the density of an object with a mass
of 3.00g and a volume of 62.2cm3?
• Answer  .0482g/cm3
• What is the volume of 45.5g of silver if the
density is 10.5 g/ml?
• Answer 478ml
Express the following in scientific notation:
a. 0.000230
b. 430,000,000
c. .0000000000001
Compounds and Mixtures
• Compounds are made up of 1 phase; mixtures
more than one
• Compounds can be separated by chemical
means; mixtures by physical means
• Mixtures are sometimes uniform in
composition (homogeneous), but sometimes
not (heterogeneous)
Atoms
- are electrically neutral, meaning the number
of protons equal the number of electrons
Atomic Number
• Equal to the number of protons in an element
Electron Configuration
Potassium –1s22s22p63s23p64s1
Silver- 1s22s22p63s23p64s23d104p65s24d9
• Metals, nonmetals, and metalloids location on
the periodic table
• Representative elements, transition metals,
inner transition metals, noble gases location
on periodic table
Charges
Group 1A  +1
Group 2A +2
Group 3A +3
Group 4A none
Group 5A -3
Group 6A -2
Group 7A -1
Group 8A  none
Valence Electrons
• Equal to the group number for representative
elements
• For example, Magnesium has 2 valence
electrons
• Iodine has 7 valence electrons
Ionic Bonds
• Electrostatic force of attraction between 2
oppositely charged ions
What are ionic compounds made up
of?
• A metal and a nonmetal, for example,
magnesium and fluorine
What is the formula for potassium
phosphide?
• K3P
Unshared pairs of electrons
• Pairs of electrons that do not participate in
bonding
When are parentheses used in ionic
compound names?
• When there is a transition metal that can have
more than one charge
What does an –ate or –ite ending
indicate about an ionic compound?
• It contains a polyatomic ion
What is the formula for sodium
sulfate?
• Na2SO4
What is the correct name for FeCl2?
• Iron (II) chloride
How can you tell by the formula if the
substance is an acid?
• The cation is H
Empirical Formula
• The smallest whole number ratio of atoms in a
compound
Avogadro’s Number
• The number of representative particles of a
substance present in 1 mole of that substance
STP
• 0 degrees Celsius and 1 atmosphere of
pressure
Mole
• The SI unit used to measure amount of a
substance
Calculate the number of moles in 635g
of NaNO2.
• 9.20 moles
The reaction Al + O2  Al2O3
• Combination
What is a skeleton equation?
• An unbalanced chemical equation (does not
show relative amounts of reactants or
products)
What type of reaction is CH4 + O2 
CO2 + H2O
• combustion
In a chemical reaction, the mass of
reactants must equal the mass of
products, according to the law of
conservation of mass
Limiting and Excess reacants
• The amount of product obtained is
determined by the limiting reactant
• A balanced equation is needed to determine
which reactant is the limiting reactant
• Some of the excess reactant is left over after
the reaction is complete
• The reactant that produces the least product
is the limiting reactant
2CO + O2  2CO2
a. What is the ratio of moles of O2 used to moles
of CO2 produced?
- 1:2
b. How many moles of CO are needed to react
completely with 2.23 moles of O2?
- 4.46