5 days to review and create a study book
Final Exam on May 12th & 13th
*the info in this review does not cover everything on the final
– but it’s a good starting place
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Take 5 pieces of BIG paper and fold in half to
make a booklet. Staple along the fold to hold
them together.
Write some sort or a title on the front page
(you may need room to add notes here as
well). Don’t forget your name and period#.
Each day you will be given a topic and some
review questions to work on. The slides will
be up for 5-10 minutes before moving on to
the next one. Use you time wisely so you do
not miss out on any review.
You may write whatever you want in the
review booklet.
FUNDAMENTALS OF CHEMISTRY: MATTER AND CHANGE
 Define chemistry.
 Which of the following observations is evidence used to imply that a
chemical reaction has occurred?
a. gas evolution b. a precipitate forms
c. the color changes
d. temperature changes e. the odor changes
f. sound is produced
g. change in taste
 Describe a physical property vs. a chemical property.
 What is the difference between a physical change and a chemical
change?
 Identify each type of change (physical or chemical).
a. boiling water
b. rusting iron
c. burning candles
d. breaking glass
e. melting wax
 Be able to classify matter: mixtures (homogeneous, heterogeneous) vs.
pure substances (compounds or elements)
 Identify each as an element, compound or mixture.
a. lead
b. water
c. kool-aid
d. table salt
e. soda
f. oxygen
 What are the characteristic of a metal, metalloid and non-metal? Identify
each type of element: a. Zn
b. As
c. S
d. Ne
e. Na
MEASUREMENTS AND CALCULATIONS
 Discuss the steps in the scientific method.
 What are the rules/guidelines of determining significant figures?
 How many significant figures in:
a. 1234
b. 123.0
c. 123400
d. 0.001234
e. 0.01230
 Report the above problems (a-e) in correct scientific notation.
 What are the common SI Units? Know the prefixes from milli to
kilo and be able to convert between units in the metric system.
 What is the difference between mass and weight?
 Multiply: 5.98 mm x 3.2 mm = ?
 Add 3.258 cm + 12.0 cm = ?
 Give an example of a qualitative observation
 Give an example of a quantitative observation.
 What is the difference between accuracy and precision?
 How many grams of mercury would you have if you had 32 cm3
of mercury? The density of mercury is 13.6 g/cm3.
 Ronnie has a piece of aluminum which has a mass of 10.8 grams
and a volume of 4 cubic centimeters. Calculate the density of
aluminum.
ATOMIC THEORY AND NUCLEAR CHEMISTRY
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Describe Dalton’s Atomic Theory.
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What did we learn from Rutherford’s Gold Foil Experiment and how did it work?
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What did J. J. Thomson discover with his Cathode Ray experiment?
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Define the atomic number, mass number, average atomic mass and isotopes.
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Explain the difference between atoms, ions, cations, anions.
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Know the charge, location and size of the three subatomic particles.
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An element has 30 protons, 35 neutrons, and 30 electrons. What element is this?
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An ion of an element has 29 protons, 35 neutrons, and 27 electrons. What ion is this? Write its
symbol with the correct charge.
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State the Law of Conservation of Mass (Matter).
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Most of the volume of the atom is taken up by the electron cloud. True or False?
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How many particles are there in 1 mole of anything? What is the name for this number of
particles?
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What is the molar mass of sodium? What is the molar mass of Na2SO4?
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Indicate the number of molecules, and the total number of each type of atom for each of the
following: 4H2O 2Al2(SO4)3
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Be able to convert: Grams to Moles or Moles to Grams and Grams to Atoms or Atoms to Grams
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How many moles are in 222 g of copper?
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How many atoms are in 4.00 g of sulfur?
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What is Avogadro’s number? What is the significance of it?
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Be able to balance simple nuclear equations.
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What is radioactive decay? Half-life? (no equations)
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Describe the process of nuclear fission and nuclear fusion?
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What are the penetrating strength differences between alpha particles, beta particles and
gamma rays?
ELECTRON CONFIGURATIONS
 What is the frequency of an electromagnetic wave traveling at the speed
of light with a wavelength of 6.80 x 10-7 m?
 All types of electromagnetic radiation have the same _________.
 Identify the parts of an electromagnetic wave on a diagram (i.e.
wavelength, amplitude, etc.).
 What is a quantum of electromagnetic energy called?
 Write the full electron configuration for: C, As, and S2 How many outer electrons does each of the following have? Na As Br
O2- K+
 How many electrons must each of the following lose or gain to achieve
an octet? (State whether it loses or gains and how many) Cl Ca Xe P
 Which element has similar chemical properties like Si? Why? At Al N C
 When electrons absorb energy, what is the result?
 What color of light has the most energy?
 What is the probability map for an electron called?
 What occurs when an electron moves from a higher energy level to a
lower energy level in an atom?
 The
indicates the main energy level occupied
by the electrons (n).
 How many electrons can occupy an s orbital, p orbital, d and f orbitals?
 Which atom would have an octet of electrons (full s and p orbitals): Fe,
Ar, O or He
PERIODIC TABLE
 Who is Dmitri Mendeleev?
 What charge do all elements in the following columns form when
they are ions? 1, 2, 13, 15, 17, 18
 What is the chemical family name for column: 1, 2, 17 and 18?
 What are the following groups most characteristic properties?
1, 2, 17, 18
 Write the complete electron structure for a neutral sodium atom.
According to its electron structure, what period of the periodic
table should sodium be in? How many valence electrons does it
have? What ion will sodium tend to form?
 What is meant by a noble gas electron configuration? Why are
they more stable?
 Define: electronegativity, ionization energy, electron affinity
 Describe the trends (across a period, down a group) in the
periodic table for: Atomic radius, Ionization energy,
Electronegativity
 State the periodic law.
CHEMICAL BONDING
 What is a chemical bond?
 What are valence electrons and why are they important?
 State the octet rule.
 What is the difference between ionic, covalent and metallic
bonding?
 What type of bond (ionic or covalent) will form in the following
compounds? How do you know? CO2 NaCl F2
 Using an electronegativity chart identify each type of bonding
(ionic, polar covalent, nonpolar covalent): Cs – Cl H – O Br – I
Cl – Cl
 List the seven diatomic molecules.
 What is a polar molecule?
 What is VSEPR theory?
 Use VSEPR theory to predict the molecular geometry of the
following (common geometries: linear, trigonal planar,
tetrahedral):
CO2
CH4
BF3
NOMENCLATURE AND USING CHEMICAL FORMULAS
 Use the following ions and write the correct formula for the
compound made from them:
a. Na+ and Brb. Mg2+ and Ic. Ca2+ and NO3d. Fe3+ and SO42 Name the above compounds (a-d) and the following:
e. KOH
f. CuF
g. CuSO4
 Which compounds below are ionic? Which are molecular
(covalently bonded)?a. N2 b. CaF2 c. NO2 d. CuSO4 e. CCl4
 Given SO42- and the compound Zr2(SO4)3 , what is the charge on
Zirconium?
 What is the chemical formula for potassium chloride? What is the
formula for iron(III) sulfide?
 What is the formula for lithium carbonate?
 What is the molar mass of an element? What is the molar mass of
CuSO4?
 What is the percent composition of carbon in carbon dioxide?
 Name each of the following acids: a. HCl b H2SO4
c.
HNO3
d. HI
Chemical Reactions
Writing Chemical Reactions
 Writing Chemical
Formulas
 Balancing
 States
Classifying Reactions
 Synthesis
 Decomposition
 Single Replacement
 Double Replacement
 Combustion
Stoichiometry
Defining Stoichiometry
 Describe the types of
relationships indicated
by a balanced chemical
equation
 State the mole ratios
from a balanced chemical
equation
 Explain role of limiting
reagent
Stoichiometric Calculations
(no show work, however
need to solve)
 Moles to moles
States of Matter
Identify Characteristics of the States of Matter
Forces of Attraction
 Identify the types of intermolecular forces, how they work,
which is strongest
◦ Hydrogen bonding
◦ Dispersion forces
◦ Dipole-Dipole
Identify the role of intermolecular force in states of matter
Phase Changes
 Explain phase/state changes
 Explain how the addition and removal of energy can cause a
phase change
 Interpret a phase diagram
Interpret a Temperature-Time Graph (Heating or Cooling Curve
of Water)
 Recognize phase and temperature
 Identify endo- and exothermic processes and constant
temperature
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Gases
The Gas Laws
 State the relationships among pressure,
temperature and volume of a constant amount of
gas
 Apply the gas laws to problems involving the
pressure, temperature, and volume of a constant
amount of gas
◦ Combined Gas Law (will be given equation on front of final
exam)
◦ Boyle’s Law
◦ Charles’s Law
◦ Gay-Lussac’s Law
◦ Ideal Gas Law (will be given equation on front of final exam)
◦ Remember all gas laws in Kelvin (be able to convert
temperature from °C)
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Relate number of particles and volume using
Avogadro’s principle (molar volume)
Solutions
Types of Mixtures
 Compare the properties of solutions, suspensions and colloids
◦ Brownian motion
◦ Tyndall effect
Electrolytes versus Nonelectrolytes
Factors Affecting Solvation
 Understand/define solvation
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◦ Factors affecting rate of dissolution
◦ Solubility of liquids and gases
◦ Role of polarity in dissolution
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Define/recognize solubility
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Unsaturated solutions
Saturated solutions
Supersaturated solutions
Precipitate
Concentrations of Solutions
 Molarity (know this formula)
Colligative Properties
 Explain/define
 Discuss how colligative properties affects the freezing-point and
boiling point of a substance
Acids and Bases
Properties of Acids and Bases
 Characteristics of acids and
bases
 Strong vs. weak acids and
bases
 Definitions
◦ Arrhenius
◦ Bronsted-Lowry
◦ Lewis
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Explain amphoteric
Discuss self-ionization of
water
Calculate
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Meaning of Kw
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◦ pH
◦ pOH
◦ Concentration
Thermodynamics
 Energy
 Define energy
 Understand the First Law of
Thermodynamics
 Heat
◦ Define
◦ Know the equation for calculating
heat
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Recognize thermochemical
equations
Describe enthalpy
Chemical Kinetics and Equilibrium
Energy Diagram
 Identify parts of an energy diagram
 Recognize if energy diagram represents an exo- or endothermic
reaction
Reaction Rates
 Understand reaction rates
 Know the factors that affect rates (temperature, size, concentration,
catalyst)
Equilibrium
 Meaning of equilibrium conditions
 Equilibrium constant (Keq)
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Define
Know that Keq varies with temperature
Understand magnitude---favors products or reactants
Write an expression
Calculate Keq and/or unknown concentration
Apply Le Chatelier’s Principle – how temperature, pressure,
concentration change equilibrium position
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Hopefully you worked hard and wrote
everything down in your booklet
You WILL be able to use this book on the
final!
1. You’re welcome.
2. Don’t forget it on Monday – I will not feel sorry for
you.
3. If you slacked – you can still add to it this
weekend – the PowerPoint will be posted to the
school website today.