CHEMISTRY SEMESTER 1 STUDY GUIDE
Along with the stuff on the review worksheet, students should know the following items.
CH. 1 & 2
 forms of matter
 distinguish between the different forms of matter—pure substances vs. mixtures; elements, compounds,
homogeneous and heterogeneous mixtures
 properties of the different classifications of matter
 given a diagram, determine if it is a pure substance or mixture as well as if it is made up of elements or
compounds and if atoms or molecules
 names and symbols of the elements
 5 evidences of a chemical reaction
 distinguish between physical and chemical properties
 distinguish between physical and chemical changes
 know the 7 diatomic elements
 physical states
 know the names of the physical state changes
 know how the different physical states compare in potential energy
 distinguish between potential energy and kinetic energy, including on a physical state change graph
CH. 3 & 4
 know the 3 different subatomic particles (proton, electron, neutron) and their charges, location, mass
 classification of elements
 metal, nonmetal, metalloid
 representative element, transition metal, inner-transition metal
 alkali metal, alkaline earth metal, halogen, noble gas, lanthanide series, actinide series
 group and period number of the elements
 properties of metals, nonmetals, and metalloids
 reactivity of the different groups of elements, especially alkali metals, halogens and noble gases
 determine the ionic charge of an element from its location on the periodic table
 know your polyatomic ions and the metals that are capable of having more than one charge
NUCLEAR CHEMISTRY
 know the symbols and properties of the different radiation particles
 indicate the type of nuclear decay or reaction given (alpha decay, beta decay, electron capture, fission, fusion,
positron decay)
 determine the missing particle of a nuclear equation
SIGNIFICANT DIGITS AND METRIC SYSTEM
 determine the number of significant digits in a quantity
 correctly round off numbers to the correct number of significant digits
 scientific notation
 write numbers decimal notation in scientific notation and vice versa
 use scientific notation numbers in calculations
 know the 5 fundamental measurements and their base units
 metric prefixes
 know the power of 10 associated with the prefix
 know the abbreviation of the prefixes and the base unit
 convert from one metric unit to another
 use significant digits in calculations
CH. 6
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mole
 define
 know Avogadro’s number
distinguish between empirical and molecular formulas
know the parts of a solution (solute and solvent)
determine the mole ratio and particle ratio of the elements in a compound
CH. 7 & 8 (Reactions Unit)
 know the parts of a chemical equation
 reaction types
 determine the type of reaction given
 distinguish between the properties of different types of reactions
 know solubility rules and what physical state to assign based on the rules
 strong acids
 know the 7 strong acids
 explain the difference between a strong acid and a weak acid
 determine the spectator ions in an ionic equation
CH. 9 (Stoichiometry)
 determine the mole ratio between substances in a chemical equation
 determine the limiting reactant for a reaction
CH. 13 (Gases)
 know the relationship between the volume, pressure, and Kelvin temperature of a gas (directly or inversely
proportional)
 Use the following laws in calculations:
o ideal gas law
o Dalton’s law
o Graham’s law
o Avogadro’s law
 Do calculations involving pressure and moles.
 Given a set of gases, put them in order of their velocities.
 Know the 2 reasons gases are not ideal.
 Know the 2 conditions when gases approach ideal behavior.
 Know what happens to the conditions for gases in a balloon or metal can when one of the conditions changes.
These conditions include:
o volume
o pressure
o temperature
o moles
o velocity
o # of collisions against the surface
 In addition to the relationships between V, P, and T already indicated in the previous study guide, know the
relationship between pressure and moles.
PROBLEMS/WRITTEN PORTION:
 nuclear symbols
 write a nuclear symbol given the needed information
 determine the atomic number, mass number, number of p+, number of n°, number of e−, and the charge
given a nuclear symbol
 write nuclear equations for the decay (alpha, beta, electron capture, or positron decays)
 determining the amount of radioactive material remaining after a given amount of time
 determine the age of a fossil using C-14 dating calculation
 naming compounds—ionic, molecular and acids
 writing formulas—ionic, molecular and acids
 determine the density of a substance given mass and volume
 determine molar mass of substance
 perform mass - moles - # particles conversions
 determine molarity of a solution as well as determine the amount of solute to make a known molar solution
 determine the mass % of the elements in a compound
 determine the mass % of solute in a solution
 determine the empirical and molecular formula of a compound
 English-metric conversions using dimensional analysis
 perform temperature conversions
 write ionic and net ionic equations
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predict products of reactions
balance chemical equations
perform stoichiometry problems
 mass-mass, mole-mass, or mass-mole
 limiting reactant problem
 excess reactant problem
 molar stoichiometry problem
do calculations using the following gas laws: Boyle’s, Charles’, Combined, and Gay-Lussac’s
LAB QUESTIONS
 reading melting/freezing point graph to determine melting/freezing point
 parts of the chloride test—know the name and formula of the precipitate involved in the process
 reactivity of metals in water and acids
 distillation and filtration process
 acid-base indicators: color of phenolphthalein and litmus in acids and bases
VOCAB: (can define these terms for 7 pts extra credit but you must have the
review worksheet done to get the points)
amu
anion
aqueous
atomic number
cation
coefficient
compound
concentration (of a solution)
dissociation
element
empirical formula
endothermic
excess reactant
exothermic
filtrate
group
half-life
heterogeneous mixture
homogeneous mixture
hydrocarbon
hypothesis
inference
insoluble
ion
kinetic energy
law
Law of Conservation of Matter
limiting reactant
mass number
matter
molar mass
molecular formula
molecule
nucleus
oxidation
percent yield
period
potential energy
precipitate
product
reactant
reduction
soluble
solute
solvent
subscripts
theoretical yield
theory