Chemistry I Final Exam Topics – Spring 2013

Unit 1

·         Lab safety

Unit 2

·         Physical vs. chemical properties

Unit 3

·         Aspects of Dalton’s experiments

·         Results of gold foil experiment

·         Differences in isotopes of elements

·         # of protons, neutrons, electrons in neutral atoms vs. ions

·         How average atomic mass is determined

·         Determine # of atoms given number of moles

·         Mole ŕ gram conversion

·         Grams ŕ mole conversion

Unit 4

·         Location of electrons in quantum mechanical model

·         How atoms emit light

·         Use diagram of Bohr model of hydrogen atom

·         Determine number of valence electrons given an electron configuration

·         Orbital notation for HOEL

·         Electron dot diagrams for elements

Unit 5

·         Definition and trend for ionization energy

·         Trends in atomic radius

·         Trends in electronegativity

·         Extrapolate periodic trends using given information

Unit 6

·         Bond polarity vs. molecular polarity

·         Bond types vs. electron transfer/share, based on elements involved

·         Bond types vs. properties of compounds

·         Molecular geometry (shapes based on surrounding atoms and lone pairs)

·         IMFs in samples of different types of compounds

Unit 7

·         Write formula for compound given the name.

·         Name compound given formula.

·         Given formula, determine placement of unknown element on P.T.

·         Determine oxidation number of element in a cmpd, in polyatomic ion

·         % by mass of element in compound

·         Calculate empirical formula of a compound given data.

·         Determine molecular formula when given molar mass.

Unit 8

·         Balance equations

·         Types of chemical reactions

·         Use Activity Series to predict outcome of single replacement reactions

Unit 9

·         Meaning of mole ratios

·         Mole ŕ mole stoichiometry

·         Mole ŕ mass stoichiometry

·         Mass ŕ mole stoichiometry

·         Mass ŕ mass stoichiometry

·         % yield calculation

Unit 10

·         Assumptions of the Kinetic-Molecular Theory

·         Conditions when gases behave most/least ideally

·         Combined gas law problem

·         Ideal gas equation problem

·         Volume ŕ volume stoichiometry

·         Compare rates of effusion

·         Factors that affect rate of effusion

Unit 11

·         Phase diagram – identify important points & know definitions (critical point, triple point, normal boiling & melting point, etc.)

·         Phase diagram – determine state(s) of matter at certain temperature and pressure

·         Heat calculation with change in temperature

·         Heat calculation with change in phase/state

·         Heating curve vs. state of matter

Unit 12

·         Solubility curve graphs

·         Molarity by dilution

·         Molarity problem

·         Determine highest BP, lowest FP given concentration of different substances in water

·         Using rules in Reference Tables, determine solubility of compounds

·         Net ionic equations

Unit 13

·         Characteristics of an equilibrium system

·         Writing a Keq expression

·         LeChatelier’s Principle equilibrium shift

Unit 14

·         Characteristics of strong/weak acids & bases

·         Arrhenius acid-base definitions & neutralization reactions

·         Identify Bronsted-Lowry acids & bases and explain their role in proton (H+) transfer

·         pH/pOH calculation for strong acid/base

·         [H+]/[OH-] calculation for strong acid/base

·         Titration problem

Unit 15

·         Endothermic vs. exothermic reactions in terms of amount of PE for reactants/products & sign of DH

·         Heat transfer between objects at different temperatures

·         How does a catalyst increase the rate of a reaction?

·         Potential energy diagram interpretation

·         Reaction rates using collision theory explanations

·         Entropy

Unit 16

·         Balancing a nuclear equation

·         Half-life problems


·         Light calculations (c = ln and E=hn)

·         Oxidation and reduction half-reactions

·         Quantum numbers

·         Limiting Reactant

·         Ka problem

·         BP/FP problem

·         Predict products of reaction