CHEM 1210 Exam #1 Study Guide

The following concepts will be covered on the first exam, which covers Chapters 1-4.

Section 1.5
Significant Figures
Use significant figures, scientific notation, SI units and dimensional analysis in calculations.

Section 1.6
Dimensional Analysis
Know common metric unit and SI units and prefixes, and be able to convert between units in calculations.

Empirical Information you are expected to know:
The volume relationship 1 cm3 = 1 mL
The meaning of the prefixes: kilo-, deci-, centi-, and milli- (Table 1.4)

Empirical Information you are not expected to memorize:
Conversions between metric and english units.
Prefixes other than those listed above.

Lab #1: Scientific Measurements
Know definition of density and be able to calculate quantities using it.
Know difference between accuracy and precision, and be able to distinguish between determinate and indeterminate errors and be able to apply these terms when analyzing a data set.

Lab #2: Separation of the Components of a Mixture
Distinguish among elements, compounds and mixtures (including separation methods for mixtures).
Distinguish between molecular substances and ionic substances in terms of their composition.
Describe the organization of the periodic table including the locations of metals and nonmetals.

Section 2.1-2.3
Atomic Structure
Describe the structure of the atom in terms of protons, neutrons, and electrons.
Describe the electric charge and relative masses of protons, neutrons, and electrons.
Express the subatomic composition of isotopes/ions using chemical symbols together with atomic number and mass number.
Write the complete atomic symbol for ions (including atomic number, mass number, and charge).

Section 2.4
Atomic Weight
Relate atomic weights to the masses of individual atoms and to their natural abundances.

Section 3.4
Avogadro’s Constant and the Mole
Convert grams to moles and moles to grams using molar masses, and convert number of molecules to moles and moles to number of atoms or molecules using Avogadro’s number.

Section 2.8
Common Cations and Anions
Know all the ions and charges on Table 2.4 and 2.5
Use the periodic table to predict the charges of common ions.

Section 2.8
Write the empirical formulas of ionic compounds, given the charges of their component ions.
Write the name of an ion given its chemical formula, or write the chemical formula given its name.
Write the name of an ionic compound given its chemical formula, or write the chemical formula given its name.
Name or write chemical formulas for binary inorganic compounds and for acids.

Section 3.1
Chemical Equations
Balance chemical equations.

Section 3.1
Chemical and Physical Changes
Distinguish between chemical and physical change.

Section 3.2
Chemical Reactions
Identify simple combination, decomposition, and combustion reactions, predict their products, and write their balanced chemical equations.
Law of Conservation of Mass in chemical reactions.

Section 3.7
Limiting Reactants and Theoretical Yield
Determine the limiting reactant in a reaction and use it to determine the amounts of products formed.

Section 3.7
% Yield
Calculate the percent yield of a reaction.

Section 3.5
Empirical and Molecular Formulas
Calculate the empirical and molecular formula of a compound from percentage composition and molecular weight.

Section 3.6
Quantitative Information From Chemical Equations
Be able to relate particle level diagrams to a balanced chemical equation and vice-versa.

Section 4.1
Classify substances as either strong electrolytes, weak electrolytes or non-electrolytes. Demonstrate an understanding of the differences between the three.
Recognize and differentiate between strong acids, weak acids, strong bases and weak bases.

Section 4.2-4.3
Reactions in Aqueous Solution
Identify simple acid-base, precipitation and redox reactions and be able to predict the products of such reactions.

Interpreting the Solubility Guidelines
You do not have to memorize these. They will be attached to the exam.

Net Ionic Equations
Given the molecular equation for a reaction be able to identify spectator ions and write the full ionic equation and/or the net ionic equation for the same reaction.

Section 4.4
Oxidation-Reduction Reactions
Assign oxidation numbers to individual atoms in neutral substances and ions, and use these assignments to determine which substance is reduced which substance oxidized in a redox reaction.

Interpreting the Activity Series
You do not have to memorize this series. It will be attached to the exam.

Reactions Involving Gaseous Products
Be able to predict which reactions will produce a gaseous product.

Section 4.5
Calculate the molarity of a solution, and be able to convert between molarity, the number of moles present in a solution, and the volume of the solution.

Know how to prepare a dilute solution with a specific concentration and volume from a more concentrated solution.

Stoichiometry in Solution and Lab #3: Development of an Equation
Determine limiting reactants and/or calculate theoretical yields of reactions involving aqueous solutions. Use the results of a titration to determine the concentration of an unknown solution.

Section 4.6
Know what an equivalence point/end point of a titration is and be able to use it to perform calculations based on titration data.

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