Ch. 1…(old book ch 1+2)Chemistry; its branches, technology, extensive vs. intensive properties, states
of matter, basic structure of periodic table; metals, nonmetals, metalloids and properties of each, families/groups, rows/periods,
elements vs compounds vs mixtures.

1. Know the definitions of matter.

2. Know the difference between mass
and weight.

3. Know the following words: homogeneous, heterogeneous, solution, mixture, compound, substance, element, atom,
and molecule.

4. Know the difference between physical & chemical properties. (Intensive vs extensive)

5. Know
the difference between physical & chemical changes.

Examples:

a. Give three physical properties

b.
Give three chemical properties

c. Classify as chemical or physical properties:

color, reactivity, flammability,
stability, malleability, solubility, melting point, rusts, evaporates readily

Ch 2…(old book ch 2+3)Scientific Method, quantitative vs qualitative, hypothesis, theory, law, SI
System, density, significant digits, scientific notation, dimensional analysis

More hints:

1. Know the basic units of
the SI system.

2. Know the prefixes of the SI system (micro-mega).

3. Know how to convert between units & prefixed
units. i.e. km to m

4. Know how to convert between different prefixed units. i.e. dm to km

5. Know how to convert between
combinations & complex forms, i.e. mL to cm3, cm3 to dm3, km/h to m/sec

6. Know how to put a number into scientific
notation.

7. Know how to change scientific notation to standard notation.

8. KNOW HOW TO CONVERT USING DIMENTIONAL ANALYSIS.

Conversions:
45mg=__________g 2.05 kg=________mg 101hm=________mm

312 L=__________ml 1.35
km/hr=_________m/s 21cm3=________m3

75.1ml=________cm3
51cm2=________km2 9dg=________g

1.2 X 102 cm=_______mm

MORE CONVERSIONS: make the following conversions and watch your significant digits.

1. 59m to mm 5.
431 cg to g 8. 29min to sec

2. 68kg to dg 6. 104mm to cm 9. 916 cm3 to dm3

3. 5cm3 to ml 7.
44m3 to dm3 10. 47mm / hr to dm / sec

4. 835 m / sec to cm / min

Ch 2…(old book ch 2+3)

Problems:

1. Find the density of an object that has a mass of 45g and a volume of 25.0 cm3.

2. Find
the mass of an object that has a density of 4.5g/cm3 and a volume of 11cm3.

3. Calculate the volume of an object in cm3
that has a mass of 22kg and a density of 8.2kg/dm3.

4. The density of aluminum is 2.70 g/cm3. Calculate the mass of aluminum
that occupies 75.0 cm3.

5. Convert to regular or scientific notation.

a) 12300= ___________ f)
1 x 103= ____________

b) 40120= ___________ g) 1.110 x 104= ________

c) 1120000=
_________ h) 2.12 x 10-5= ________

d) 0.0000123= ________ I) 3.20 x 10-7= ________

e)
0.0120= ___________ j) 4.412 x 1011= ________

More:

Express in scientific notation:

1. 50600 2.
3000000 3. 0.0005 4. 0.023 5. 56

Change from scientific notation to decimal (standard) notation

1.
5 x 105 2. 2.35 x 103 3. 9.056 x 10-3 4. 3.6 x 102 5. 1.01 x 10-6

4. How many sig figs?

7300 ____ 0.00125 _____ 71253 _____ 5.012 _____ 0.5100 _____

5. Answer to the correct sig figs:

a)
85+2.3= ______ e) 42.1/24= ______

b) 213.213-12.3 = _____ f) 101x2134 ______

c)
57+11.1= ______ g) 2123/3143= _____

d) 1.2x103 + 4.2x102=_______ h) 2.23x105 x
5.2x103=______

CH 3….(old book ch 8)

Law of multiple proportions, law of conversion of mass, periodic law, Millikan,
Mendeleev, Bohr, atomic structure, isotopes, mole island, gram mass (formula mass/atomic mass unit (amu)).

1. Know the
following words: cathode ray tube, isotope, atomic number, mass number, electron, proton, neutron, spectroscopy, and electromagnetic
energy.

2. Know the parts of Dalton’s atomic theory.

3. Know the relative masses of the proton, neutron, and electron.

4.
Be familiar with Thomson, Bohr, and Rutherford.

5. Be familiar with the modern atomic theory.

Problems:

1. What is
the mass of 52 mol of chlorine?

2. How many moles does 212 grams of nickel contain?

3. What is the volume of 2.52 mol
of neon at STP?

4. How many grains of sand are found in 5 x 105 mol of sand?

5. What is the mass (in grams and kilograms)
of 4 x 1020 atoms of potassium?

6. Convert the following:

a) 2.50 x 1024 molecules of water to grams

b)
5.00 grams of salt (NaCl) to molecules

c) 130 grams of RbI to moles

d) 2.00 x 1023 molecules of NO2 to moles

e)
3.5 moles of CO2 to dm3 (gas volume) (ans. = 78.4 dm3)

f) 5.00 moles of HCl to grams

g) 1.50 grams of Al(NO3)3
to molecules

CH 4…(old book ch 13)

Frequency, wavelength, light, electromagnetic spectrum, Heisenberg uncertainty
principle, quantum number, electron spin, diagonal rule, spdf, energy levels, orbital, Pauli’s exclusionary principle,
Hund’s rule, ground state, excited state, electron configuration, valence electrons.

Write the electron configuration (long way) and the noble gas notation (short way) for:

1. chlorine

2.
potassium

3. iron

4. magnesium

5. Californium (short way only)

6. Silver

CH 5…(old book ch 14)

Mendeleev, noble gases, alkaline metals, alkaline earth metals, halogens, atomic
number, mass number, isotopes, spdf-blocks, metals, nonmetals, metalloids, electron affinity, ionization energy, electronegativity,
atomic radius, valence electrons, periodicity, families/groups, periods/ rows.

CH 6…(old book ch 15)

Covalent bonds, ionic bonds, electronegativity, nonpolar bonds, polar bonds,
Lewis structure, octet rule, double bond, single bond, triple bond, VSEPR theory; tetrahedral, linear, trigonal planer, bent,
lattice energy, metallic bond, ions, anions, cations.

Draw Lewis structure for the following:

1. hydrogen

2. potassium

3. calcium

4. CCl4

5. HCl

6.
C2H2

7. C2H6

CH 7…(old book ch 7)

Chemical formulas, subscripts, coefficients, naming and writing compounds: traditional
system and stock system and acids, cation, anion, oxidation numbers, gram/ formula mass, percent composition, empirical formula,
molecular formula, mole island.

1. Know the following terms: symbol, formula, subscript, empirical formula, molecular formula,
polyatomic ion.

2. Know how to give the formula of a named compound.

3. Know how to give the name of a compound from
a formula.

4. Know how to use the tables of oxidation numbers and polyatomic ions.

5. Know the elements that exist as
diatomic molecules. (List them)

Give the formula:

a) potassium nitrate d) manganese (II) oxide

b)
iron (III) chloride e) ammonium bromide

c) sodium carbonate f) tin
(IV) phosphate

Name the following using the Stock System

1. CaCO3 4. AgBr

2. CuCl2 5. Sn5

3.
SnS2 6. CdSO4

Give the formulae for the following ions:

a) ammonium b) carbonate c) nitrate d)
hydroxide

e) sulfate f) phosphate

Name the following using the:

Stock System Traditional System

1.
PCl4 N2O5

2. PbBr2 CCl4

3. PbO SiO2

4.
Cr2(SO4)3 NF3

Write chemical formula for: Name the following acids

1. carbon disulfide 1.
HNO3

2. dinitrogen trioxide 2. H2S

3. calcium fluoride 3.
HCl

4. iron (III) oxide 4. HC2H3O2

Write the chemical formulas for the following acids:

1. phosphoric acid

2. hydrobromic acid

3. sulfuric
acid

4. hydroiodic acid

Calculate the gram/formula mass of: Calculate the percent composition of:

1. Ca(OH) 2
Ca_________

2. NaCl Na_________ Cl__________

3.
MgCl2 Mg_________

4. CO C__________
O__________

Problems:

1. How many oxygen atoms are present in 0.500 mol of CO2?

2. How many moles are present
in 10.37 g of LiF?

3. What is the empirical formula for a compound that is 43.6% phosphorous and 56.4% oxygen?

4. What
is the empirical formula for a compound that is 7.9% lithium and 92.1% bromine?

5. A compound contain 27.3 g of C and 72.7
g of O. What is the empirical formula for this compound?

6. A compounds empirical formula is C2H5. If the formula mass
is 58 amu, what is the molecular formula?

7. A compounds empirical formula is N2O5. If the formula mass is 108 amu, what
is the molecular formula?

8. Find the gram formula mass of the following compounds:

a. (NH4)4SiF6 b.
PbO2 c. Cs3PO3 d. Ga2(CO3)3

9. Find the percent composition of Ca3(PO4)2

10. Calculate the empirical and molecular
formula of a compound whose molecular mass is determined to be 27.5 and is 75% boron and 25.0% hydrogen.

11. What is the
difference between an empirical formula and a molecular formula?

12. Find the percent composition of Fe2(SeO4)3.

Ch 8…(old book ch 9)

KNOW THE FOLLOWING

1. Definitions: equation, subscript, coefficient, reactant,
product, l, g, aq, s.

2. Recognize the major types of reactions – synthesis, decomposition, single displacement,
double displacement, combustion

3. Be able to complete unfinished reactions of known type.

Be able to write equations
from word equations.

Be able to differentiate between endothermic reactions and exothermic reactions.

BALANCE THE FOLLOWING EQUATIONS, and identify the type of reaction.

1. C3H7OH + O2 CO2 + H2O

2.
Ca(OH)2 + H3PO4 H2O + Ca3(PO4)2

3. KClO3 + H2SO3 KCl + H2SO4

4. Mg + Fe3O4 MgO + Fe

5.
KNO3 KNO2 + O2

6. CO + O2 CO2

7. SrO + H2O Sr(OH)2

Write the equation and balance it after predicting the products.

8. Silver oxide decomposes

9. Magnesium reacts with oxygen

10. Hydrochloric acid plus silver nitrate (double displacement)

11. Zinc reacts with sulfuric acid (single displacement)

12. C2H6 goes through combustion

Ch 9…(old book ch 10)

Mole ratio, mol-mol problems, mass-mass problems (4 step problems), limiting
reactant, reactant in excess, percent yield

Problems:

1. For the decomposition reaction of potassium chlorate, how many
moles of potassium chlorate are required to produce 2.50 g of oxygen.

2. For the synthesis reaction of sodium chloride,
how many grams of hydrogen are produced if 1.20 g of sodium and 80 g of water are available?

3. How many moles of potassium
chloride are produced when 119 g of potassium bromide is reacted with chlorine?

4. When reacted with hydrogen, how many
moles of nitrogen are required to produce 18 mol of ammonia

5. For the reaction:

CaO
+ H2O Ca(OH)2

If 7.0 grams of CaO and 3.0 grams of water are available, what is the limiting reaction?

What amount
of Ca(OH)2 can be formed? What is the reactant in excess and by how much?

6. Calculate the percent yield if 200.0 g of
chlorine react with excess sodium to produce 240.0 g of sodium chloride.

7. How many dm3 of hydrogen gas can be produced
from 7.50 grams of aluminum reacting with excess Hydrochloric acid (HCl) in a single displacement reaction?

8. How many
grams of Iron can be produced from 250 grams of Iron Oxide according to the following reaction Fe2 O3 + 3CO 2Fe + 3CO2?