The Chemistry 1220 Final Exam consists of 40 questions and covers Chapters 13-23 in the 12th Edition of “Chemistry the Central Science” by Brown, LeMay, Bursten, Murphy, and Woodward.
To assist you on the exam you will be given a periodic table and the following Chem 1220 Final Exam Useful Information.
In order to prepare yourself for the final I would suggest the following:
•Work through the graded homework problems from Mastering Chemistry
Re-work these problems so you are able to complete them on your own on the exam.
•Work through the lecture problems, which are posted on Carmen.
Re-work these problems so you are able to complete them on your own on the exam.
•Read the textbook sections listed below.
Reading the book before the exam is the best way to “cram” for the exam, especially for the conceptual questions.
•Use any other resources you have to understand the following learning objectives listed below:
Section 13.1
Properties of Solutions, The Solution Process, Energetics of Solution Formation, and Dissolution of NaCl in Water
Describe how enthalpy and entropy changes affect solution formation. Be able to interpret Figures 13.3 and 13.4 and determine how the change in enthalpy of the solvent, solute, and mixture influence whether the solution process is endothermic or exothermic.
Section 13.2
Saturated Solutions and Solubility
Describe the role of equilibria in the solution process and its relationship to the solubility of a solute.
Section 13.3
Factors Affecting Solubility, Miscibility
Describe the relationship between intermolecular forces and solubility, including use of the “like dissolves like” rule.
Pressure Effects on Gas Solubility and Henry’s Law
Describe the relationship between the partial pressure of a gas and its solubility.
Lab #14: Variation of Solubility with Temperature and Solvent
Section 13.4
Expressing Solution Concentration and Units of Concentration
Calculate the concentration of a solution in terms of molarity, molality, mole fraction, percent composition, and parts per million and be able to interconvert between them.
Section 13.5
Colligative Properties
Describe what a colligative property is and explain the difference between the effects of nonelectrolytes and electrolytes on colligative properties.
Boiling Point Elevation and Freezing Point Depression, Vapor Pressure Lowering, Osmosis and Osmotic Pressure, and Molar Mass from Colligative Properties
Be able to calculate the vapor pressure of a solvent over a solution, the boiling point elevation and freezing point depression of a solution, and the osmotic pressure of a solution. Also be able to use these colligative properties to determine molar mass.
Lab #15: Freezing Point Depression
Section 14.1
Factors That Affect Reaction Rates
Understand the factors that affect the rate of chemical reactions.
Section 14.2
Reaction Rates and Reaction Rates and Stoichiometry
Determine the rate of a reaction given time and concentration.
Section 14.3
Concentration and the Rate Law
Relate the rate of formation of products and the rate of disappearance of reactants given the balanced chemical equation for the reaction.
Using Spectroscopic Methods to Measure Rates
Given Beer’s law, be able to calculate concentration in order to determine the rate.
Section 14.4
Change in Concentration with Time
Understand the form and meaning of a rate law including the ideas of reaction order and rate constant.
1st and 2nd Order Integrated Rate Law, and Half Life for 1st and 2nd order Reactions.
Determine the rate law and rate constant for a reaction from a series of experiments given the measured rates for various concentrations of reactants. Use the integrated form of a rate law to determine the concentration of a reactant at a given time and to determine the half life and/or rate constant.
Lab #16: Determining a Rate Law and Rate Constant
Section 14.5
Temperature and Rate, The Collision Model , The Orientation Factor, Transition State Theory, The Arrhenius Equation, and Activation Energy
Explain how the activation energy affects a rate and be able to use the Arrhenius equation.
Lab #17: Variation of Reaction Rate with Temperature
Section 14.6
Reaction Mechanisms, Proposing a Reaction Mechanism, and Mechanisms and Molecularity
Predict a rate law for a reaction having a multistep mechanism given the individual steps in the mechanism.
Section 14.7
Catalysis
Explain how a catalyst works and be able to distinguish between a catalyst and an intermediate.
Section 15.1
The Concept of Chemical Equilibrium and Visual Representation of Equilibrium
Understand what is meant by chemical equilibrium and how it relates to reaction rates. Be able to visualize dynamic equilibrium a tthe atomic level.
Section 15.2
The Equilibrium Constant
Write the equilibrium-constant expression for any reaction.
Equilibrium Expressions Involving Gases
Relate the equilibrium constant expressed using molar concentrations to that using presssures.
Section 15.3-15.5
Magnitude of Equilibrium Constants
Relate the magnitude of an equilibrium constant to the relative amounts of reactants and products present in an equilibrium mixture.
Determining Equilibrium Constants from Experimental Data and Combining Equilibrium Constants
Manipulate the equilibrium constant to reflect changes in the chemical equation and be able to calculate the equilibrium constant from concentration measurements.
Heterogeneous Reactions
Write the equilibrium-constant expression for a heterogeneous reaction.
Linking Equilibrium and Kinetics
Section 15.6
The Reaction Quotient Q
Predict the direction of a reaction given the equilibrium constant and the concentrations of reactants and products.
Fundamentals of Equilibrium Concentration Calculations
Calculate equilibrium concentrations given the equilibrium constant and all but one equilibrium concentration and Calculate equilibrium concentrations, given the equilibrium constant and the starting concentrations.
Section 15.7
Le Chatlier’s Principle and Disturbing Equilibrium: The Effect of Changing Concentration on Equilibrium, The Effect of Pressure Changes on Equilibrium, The Effect of an Inert Gas, Temperature, and Catalysis on Equilibrium
Understand how changing the concentrations, volume, or temperature of a system at equilibrium affects the equilibrium position.
Lab #18: Equilibrium and Le Chatelier’s Principle
Section 16.1
Acid-Base Equilibria
Define and identify acids and bases using the Arrhenius, Bronsted-Lowry and Lewis descriptions.
Section 16.2
Bronsted-Lowry Acids and Bases and Conjugate Acid-Base Pairs
Identify conjugate acid-base pairs and relate the strength of an acid to the strength of its conjugate base.
Relative Strengths of Acids and Bases
Write the appropriate equilibrium constant and proton transfer reaction for acid-base reactions, and use this relationship to evaluate the strength of acids and bases.
Section 16.3
Acid-Base Relationships in Water and The Autoionization of Water
Describe the autoionization of water and calculate pH from the concentration ofhydronium ion or the concentration of hydroxide ion.
Section 16.4
The pH Scale
Use the pH scale to identify acidic and basic solutions. Identify pH ranges from the color of indicator solutions.
Section 16.5
pH of Strong Acids, Calculations involving Concentrations and pH of Strong Acids
Identify strong acids and bases. Calculate the pH of a strong acid or strong base from its empirical formula and concentration.
Section 16.1
Acid-Base Equilibria
Define and identify acids and bases using the Arrhenius, Bronsted-Lowry and Lewis descriptions.
Section 16.2
Bronsted-Lowry Acids and Bases and Conjugate Acid-Base Pairs
Identify conjugate acid-base pairs and relate the strength of an acid to the strength of its conjugate base.
Relative Strengths of Acids and Bases
Write the appropriate equilibrium constant and proton transfer reaction for acid-base reactions, and use this relationship to evaluate the strength of acids and bases.
Section 16.3
Acid-Base Relationships in Water and The Autoionization of Water
Describe the autoionization of water and calculate pH from the concentration ofhydronium ion or the concentration of hydroxide ion.
Section 16.4
The pH Scale
Use the pH scale to identify acidic and basic solutions. Identify pH ranges from the color of indicator solutions.
Section 16.5
pH of Strong Acids, Calculations involving Concentrations and pH of Strong Acids
Identify strong acids and bases. Calculate the pH of a strong acid or strong base from its empirical formula and concentration.
Section 16.6
Weak Acids
Identify weak acids and bases.
Calculating Ka from pH
Calculate the acid-dissociation constant for a weak acid or base-dissociation constant for a weak base given its concentration and the pH of the solution.
Percent Ionization
Calculate the percent ionization of a weak acid/base.
Using Ka to Calculate pH
Calculate the pH of a solution of a weak acid/base given its concentration and the appropriate dissoication constant.
Polyprotic Acids
Be able to analyze successive ionization constants and interpret titration curves of polyprotic acids.
Section 16.7
Weak Bases
Calculate Kb for a weak base given Ka of its conjugate acid.
Section 16.8
Relationship Between Ka and Kb
Calculate Ka for a weak acid given Kb of its conjugate base.
Laboratory #19: Analysis of a Solution of Two Acids
Section 16.9
Acid-Base Properties of Salt Solutions
Predict whether an aqueous solution of a salt will be acidic, basic or neutral and calculate the pH of salt solutions.
Section 16.10
Acid-Base Behavior and Chemical Structure
Be able to predict the relative strength of a series of acids based on chemical structure. For carboxylic acids, be able to identify how acid strength relates to the resonance stability associated with its conjugate base.
Section 16.11
Lewis Acids and Bases
Be able to define and identify Lewis Acids and Bases
Section 17.1
Common Ion Effect
Describe the common ion effect and use it to make qualitative predictions of how the presence of salts can alter pH or solubility equilibria.
Section 17.2
Buffer Solutions
Explain how a buffer functions and calculate the pH of a buffered solution, including its response to additions of acid or base.
Section 17.3
Acid-Base Titrations
Identify various types of acid-base titrations (strong acid-strong base, weak acid-strong base, weak base-strong acid, etc.) from their titration curves. Calculate the pH at any point in a titration, and determine the appropriate indicator for a given acid-base titration.
Laboratory #20: Acid-Base Titration Curves: Determining pKa
Section 17.4
Solubility Equilibria
Given either solubility-product constant, molar solubility or mass solubility for a substance calculate the other two quantities.
Laboratory #21: Determining a Solubility Product Constant
Section 17.5
Factors That Affect Solubility
Calculate molar solubility in the presence of a common ion. Predict the effect of pH on solubility of an ionic compound. Explain the effect of complex-ion formation and amphoterism on solubility.
Section 17.6
Solubility Equilibria
Use solubility-product constant and the reaction quotient to predict the concentration of ions needed to form a precipitate, and use such calculations to predict the order of precipitation and best separation in a solution containing multiple ions.
You are not responsible for Chapter 17.7 on the SP2013 exam.
Section 17.7
Factors That Affect Solubility
Interpret the results of qualitative analysis schemes to determine the identity of cations in a sample of unknown composition.
Section 19.1
Spontaneous Processes
Be able to distinguish between a spontaneous process, reversible process, irreversible process, and isothermal process.
Section 19.2
Entropy and the Second Law of Thermodynamics
State the second law of thermodynamics and describe the notion of entropy. Be able to justify how/why the entropy of the universe increases in a spontaneous process.
Section 19.3
Molecular Interpretation of Entropy
Explain how the entropy of a system is related to the number of possible microstates and describe the kinds of molecular motion that a molecule can possess. Be able to use the concepts of microstates and molecular motion to make qualitative predictions about entropy.
Section 19.4
Entropy Changes in Chemical Reactions
Predict the sign of the entropy change for physical and chemical processes.
19.3, 19.4, 19.43, 19.47, 19.48, 19.49
Section 19.5
Gibbs Free Energy
Be able to calculate changes in entropy, or changes in Gibbs free energy, for chemical reactions to determine if a reaction is spontaneous.
19.53, 19.54, 19.59, 19.61
Section 19.6
Free Energy and Temperature
Recognize how changing the temperature influences the spontaneity of a reaction and predict which temperatures a reaction will be spontaneous given the change in enthalpy and the change in entropy.
19.66, 19.67, 19.69, 19.71
Section 19.7
Free Energy and Temperature
Be able to calculate ΔG under non-standard conditions and recognize how ΔG changes when the partial pressures of gases are not equal to one atmosphere and the concentration of solutions are not one molar.
Relate Gibbs free energy to the equilibrium constant and understand how the magnitude of K relates to spontaneity.
19.77, 19.81, 19.99
Understand the molecular interpretation of entropy, and how it relates to the 2nd law of thermodynamics.
19.27, 19.37, 19.43
Laboratory experiment #22 Solubility and Determination of ΔG, ΔH and ΔS of Ca(OH)2
Understand calculations & concepts.
Section 20.1
Oxidation States and Oxidation-Reduction Reactions
Be able to determine the oxidation states of all species in an electrochemical reaction in order to identify the species oxidized, the species reduced, the oxidizing agent, and the reducing agent based on standard reduction potential data or reactivity.
20.6, 20.43, 20.47
Section 20.2
Balancing Redox Reactions
Complete and balance redox equations using the method of half-reactions in both acidic and basic solutions.
20.21, 20.23
Section 20.3
Voltaic Cells
Sketch a voltaic cell and identify its cathode, anode, and the directions that electrons and ions move.
Be able to visualize the change in mass at the anode/cathode and the change in concentrations in the anode/cathode compartment at the molecular level.
20.8, 20.27, 20.37, 20.39
Section 20.4
Cell Potentials Under Standard Conditions
Calculate standard cell potentials (emfs) from standard reduction potentials.
Use reduction potentials to predict whether a redox reaction is spontaneous and to determine the relative strengths of oxidizing and reducing agents.
Understand the terms standard reduction potential and the operation of a standard hydrogen electrode.
20.33, 20.34
Section 20.5
Free Energy and Redox Reactions
Related the standard cell potential to the standard free energy change and the equilibrium constant.
Section 20.6
Cell Potentials Under Nonstandard Conditions
be able to apply the Nernst equation to determine the cell potential under non-standard conditions and relate the standard cell potential to the standard free energy change and the equilibrium constant.
20.65, 20.69, 20.72
Section 20.6
Cell Potentials Under Nonstandard Conditions
Electrolysis in non-aqueous and aqueous systems.
20.89, 20.90, 20.109
Section 20.8
Corrosion
Be able to apply concepts of spontaneous electrochemical processes to explain how corrosion is prevented by cathodic protection.
20.84, 20.85
Section 20.9
Electrolysis
Describe the reactions in electrolytic cells and relate amounts of products and reactants in redox reactions to electrical charge.
Laboratory experiment #23 Electrochemistry
Understand calculations & concepts.
Section 23.1-23.2
Transition Metal Complexes
Determine the oxidation number and number of d electrons for metal ions in complexes and determine the coordination number about the central atom and geometry of the transition metal complex.
23.15, 23.23, 23.25, 23.29
Section 23.4
Isomerization in Coordination Chemistry
Recognize and draw the structural and stereoisomers in a transition metal complex.
23.5, 23.6, 23.39, 23.40
Section 23.4
Isomerization in Coordination Chemistry
Section 23.6
Crystal-Field Theory
Be able to interpret crystal-field splitting diagrams for octahedral, square-planar & tetrahedral geometries, and for weak and strong field ligands. Understand the terms high spin and low spin.
23.8, 23.47, 23.59, 23.63.
Use crystal-field theory to explain color in coordination compounds.
23.51, 23.53, 23.54
Section 21.1
Nuclear Equations
Determine numbers of protons and neutrons in a nucleus, and write balanced nuclear equations for nuclear decay processes.
Section 21.2
Patterns of Nuclear Stability
Predict nuclear stability and by using the belt of stability, predict the expected type of nuclear decay for radioactive nuclei.
Section 21.4
Rates of Radioactive Decay
Use the half-life of an isotope to calculate the percent of a radionuclide that remains after a given time has passed and vice versa. Calculate the age of an object containing a radionuclide from its isotope ratio.
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