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Chemistry I
Final Exam review topics – Semester 1
Probable format:
December 2008
80 multiple choice, no written problems or questions.
1 – The Chemical World
 Scientific method, terms
 Law of conservation of mass, application of
2 – Measurement and Problem Solving
 Sig figs, add/sub rule, mult/div rule, apply them, from a picture
 SI unit system; base units, derived units
 Prefixes (micro, milli, centi, kilo)
 Conversion problems; single to multistep problems
 Density; know its meaning, apply the equation
3 – Matter and Energy
 States of matter; solid, liquid, gas – properties of , id from a picture
 Amorphous vs crystalline
 Matter classification; pure sub (element compound), mixture (homo, hetero); id from a picture
 Physical vs. chemical properties, changes
 Methods of separation (distillation, filtration, chromatography)
 Law of conservation of energy, converting to different forms
 Energy unit conversion problems
 Temperature scales, conversions (°C ↔ K)
 Heat calculations – calorimeter, q = mcT
4 – Atoms and Elements
 Democritus
 Dalton’s atomic theory
 Thomson – cathode ray tube work; what did it show
 Rutherford – gold-foil experiment; how was it done, what did it show
 Structure of the atom; nucleus, protons, neutrons, electrons
 Notation for an element; atomic number, mass number, charge
 Periodic table arrangement; based on what; zig-zag line
 Group names; Alkali, alkaline earth, halogens, noble gases
 Charges for those elements with a fixed charge
 Isotopes
 Average atomic mass; conceptual idea; calculate one
5 – Molecules and Compounds
 Law of constant composition
 Diatomic molecules (7 of them)
 Ionic vs. covalent compounds; how do you know
 Naming compounds and writing formulas
o Ionic compounds – know those ions and charges
o Molecular compounds – know those prefixes
o Acids – three types
6 – Chemical Composition
 Mole conversions
 Avogadro’s number
 Molar mass
 Conversions from a chemical formula (formula ratio)
 Percent composition (by mass); from data; from chemical formula
 Empirical formula; molecular formula problems
7 – Chemical Reactions
 Evidences of a chemical reaction
 Writing and balancing chemical equations
 Aqueous, what does it mean
 Solubility, (sol. table (p. 200)) will be provided, be able to use it
 Precipitation reactions
 Molecular, ionic, and net ionic equations (spectator ions)
 Acid base reactions; what are the products, …
 Gas evolution reactions; 4 gases you will need to predict
 Oxidation- reduction reaction; yes or no
 Combustion reactions
 Identify types of reactions (Syn, Dec, SR, DR, Comb)
 Identify if a reaction is redox or not
8 – Quantities in Chemical Reactions
 Calculations involving balanced equations
o Mass – mass
o Mole - mole
o Molar volume
o Molarity
o Thermochemical equations (involving heat)
 Limiting reactant concept
 Theoretical yield
 Percent yield
17 – Radioactivity & Nuclear Chemistry
 Becquerel – discovered radioactivity
 Curies – coined the term radioactivity and researched it for years
 Types of radioactive emissions; alpha, beta, gamma
 Write and balance nuclear equations
 Alpha; what’s an alpha particle like; write a decay equation; what happens to alpha particles once they leave
 Beta decay; what’s a beta particle like; write a decay equation, where does a beta particle come from
 Gamma decay; …
 Positron emission; what’s a positron like; write a decay equation, where does a positron come from
 Half-life problems (whole number of half-lives)
 Decay series
 Fission, nuclear reactors – basic components, finish an equation
 Fusion, stars (including our sun), finish an equation
18 – Organic Chemistry
 Vitalism; what is it
 Wohler; what did he do?
 Hydrocarbons, names and structures, straight, branched
o Saturated, unsaturated
o Alkanes, alkenes, alkynes
o Aromatics (benezene); ortho, meta, para
 Functional groups; recognize them; (name the underlined types)
o Alcohols, ethers, aldehydes, ketones, carboxylic acids, esters, amines
 Polymers; two types – addition, condensation
o monomer