Download 2012-2013 CHEMISTRY REVIEW: Organize your NOTEBOOK to

2012-2013 CHEMISTRY REVIEW: Organize your NOTEBOOK to refresh your memory. Review the CHAPTER 1-7 HIGHLIGHTS
from the text. Use the Review Questions to identify areas on which you need to spend more study time. For those areas go
back to your homework assignments, text, and study guides, and notes. The questions on the test will be similar to those on
the chapter tests. The test includes multiple choice questions and one essay from those given on the Review Questions. You will
be given a periodic table and you may use a calculator. You may use your HANDWRITTEN NOTECARD for the test. I will collect
it.
Include information on the following topics on your note card, as needed:
Chapter 1: Matter and Change
o Classes of Matter
o Physical and chemical properties and changes
o General Periodic Table Information
Chapter 2: Measurements and Calculations:
o Qualitative and quantitative observations
o Scientific notation and calculations
o Significant digits and calculations
o Metric system and conversions using DRUL
o Factor-label method of solving conversion problems
o Scientific method and proper experimental procedures
o Derived units and density calculations
Chapter 3: The Building Blocks of Matter
o Laws of conservation of mass, definite proportions, and multiple proportions
o History of atomic theory: Dalton, Thomson, Rutherford…experiments and resulting models
o Parts of an atom
o Nuclear representation (atomic notation)
o Isotopes and average atomic mass calculations
o Mole calculations, Avogadro’s number, molar mass
Chapter 4: Arrangement of Electrons in Atoms
o Electromagnetic spectrum and vocabulary and relationship of wavelength and frequency to energy
o Dual nature of light and electrons
o Bohr’s model of the atom and explanation
o Heisenberg uncertainty principle and Schroedinger’s contribution
o Today’s modern quantum model of the atom and explanation
o Levels, sub-levels, and orbitals, quantum numbers
o Electron configurations (arrow, spectroscopic, noble gas) and the guides (Aufbau Principle, Hund’s Rule, Pauli
Exclusion Principle)
Chapter 5: The Periodic Law
o Periodic Law and historical background: Mendeleev
o Groups, periods, blocks, families, metals, non-metals, metalloids, valence electrons, oxidation numbers (charges)
o Identify trends of atomic and ionic radii, electronegativity, ionization energy, and electron affinity
o Explain trends by groups ( # of energy levels) or periods (# of protons/nuclear charge)
Chapter 6 and 7: Chemical Bonding
o Ionic, polar covalent, non-polar covalent and metallic bonding
o Octet Rule, cations, and anions
o Chemical formulas
o Lewis Dot structures of ionic and covalent compounds
o Single, double, and triple bonds
2012-2013 CHEMISTRY REVIEW: Organize your NOTEBOOK to refresh your memory. Review the CHAPTER 1-6 HIGHLIGHTS
from the text. Identify areas on which you need to spend more study time. For those areas go back to your homework
assignments, text, and study guides, and notes. The questions on the test will be similar to those on the chapter tests. The test
includes multiple choice questions and one essay. You will be given a periodic table and you may use a calculator. You may use
your HANDWRITTEN NOTECARD for a portion of the test. The notes will be on an index card which you may work on in class. It
must be clear, accurate, organized, and handwritten. I will collect it.
Include information on the following topics on your note card, as needed:
Chapter 6 and 7: Chemical Bonding and Molecular Geometry and Chemical Formulas and Chemical Compounds
o Ionic, polar covalent, non-polar covalent and metallic bonding
o Octet Rule, cations, and anions
o Chemical formulas
o Lewis Dot structures of ionic and covalent compounds
o Single, double, and triple bonds
o Explain what VSEPR stands for and how it explains the shapes of molecules
o Intermolecular forces
Chapter 7: Chemical Formulas and Chemical Compounds
o Calculate molar mass
o Convert between moles, grams, # of particles, or volume of a gas
o Calculate the % composition of a compound
o Define and calculate empirical and molecular formulas from either % composition or mass composition
Chapter 8: Chemical Equations and Reactions
o List observations that indicate that a chemical reaction may have occurred
o Write word and formula equations using symbols to include information about the reaction
o Balance chemical equations
o Define and give general equations for 5 types of chemical reactions
o Classify reactions
o Given the reactants, predict products of single-displacement, double-displacement, combustion, and simple synthesis
and decomposition reactions
o Use the activity series fro single-displacement reactions
o Use the solubility chart/guidelines for double-displacement reactions
Chapter 9: Stoichiometry
o Define stoichiometry
o Explain the importance of the mole ratio
o Determine the mole ratio of substances from the chemical equation
o Use the mole map to perform stoichiometric calculations from moles, grams, volume, or # of particles to grams to
moles, grams, volume, or # of particles
o Differentiate theoretical yield and actual yield
o Determine limiting reactant, theoretical yield, percentage yield, and excess reactant
Chapter 10 & 11: States of Matter and Graham’s Law
o State and explain the kinetic molecular theory of matter (KMT) and use it to explain properties of matter
o Define ideal gas and describe the conditions under which real gases deviate from ideal gas behavior
o Describe these properties of gases: expansion, density, fluidity, compressibility, diffusion, effusion
o Use KMT to describe properties of gases, liquids and solids
o Define vaporization, boiling, condensation, melting, freezing, sublimation, deposition
o Distinguish crystalline and amorphous solids
o Recognize that crystals possess symmetry due to the crystal structure
o Describe changes of state in terms of KMT
o Recognize and describe conditions of dynamic equilibrium
o Interpret phase diagrams and heating curves
o Describe equilibrium vapor pressure
o Describe the structure of water and use it to explain its physical properties
o Calculate the amount of heat energy released or absorbed when a quantity of water freezes or melts
o Describe the processes of diffusion and effusion
o Use Graham’s Law to calculate the ratio of effusion/diffusion of two gases based on their molar masses
Chapter 11: Gases
o Define pressure and convert between various pressure units
o State STP
o State and use Dalton’s Law, Charles’ Law, Boyle’s Law, Gay-Lussac’s Law, Avogadro’s Law, combined Gas Law, Ideal
Gas Law
o Explain Gas Laws using KMT
o Understand standard molar volume of a gas = 22.4 L at STP
Chapter 12: Solutions
o Define solution and list different solute-solvent combinations and give examples
o Contrast solutions with suspensions and colloids
o Distinguish electrolytes and non-electrolytes
o Describe the solution process and explain using KMT
o List and explain factors that affect the rate of dissolution in solid/liquid solutions and gas/liquid solutions
o Apply terms exothermic and endothermic to the solution process
o Compare the effect of temperature on solubility
o Interpret solubility curves
o Define %solution, molarity, and molality and perform concentration calculations
o Describe how to prepare a solution
o Calculate dilutions
Chapter 13: Ions in Aqueous Solutions and Colligative Properties
o Write equations for dissolution of ionic compounds in water
o Use solubility chart to predict if precipitate will form when soluble ionic compounds are formed
o Write the total ionic equations and the net ionic equation for precipitation reactions
o Draw and explain the formation of the hydronium ion
o Distinguish strong and weak electrolytes
o List 4 colligative properties and explain
o Calculate boiling point elevation, freezing point depression and solution molality of non-electrolytes and electrolytes
o Discuss difference between expected and actual colligative properties
Chapter 14 Acids and Bases
o List general properties of acids and bases and give examples
o Name common acids
o Define acid and base according to Bronstead-Lowry, Arrhenius, and Lewis definitions
o Explain difference between strong and weak acids and bases
o Describe a conjugate acid and a conjugate base
o Explain acid rain
Chapter 15 Acid-Base Titration and pH
o Describe the self-ionization of water
o Define pH and explain and use the pH scale
o Find pH given hydronium ion concentration or hydroxide concentration
o Find pH given hydronium ion concentration or hydroxide concentration
o Finf hydronium ion concentration or hydroxide concentration given pH
o Describe indicators
o Explain titration procedures
o Calculate molarity from concentration data