COAM (Online in Carmen):

Safety Statement (Online in Carmen):

Safety & Lab Policies Quiz:

Introduction to Smart Worksheets:

Recitation and Quiz Information:

• Recitation consists of attendance points and quiz points. You can find more detail below and in the syllabus.
  • Recitation attendance is worth 10 points for each recitation. When you go to recitation you will sign an attendance sheet using your firstname lastname.# (e.g. Robert Zellmer.1). If you're late you also have to include the time you arrived. If you're late or leave early an appropriate percentage of points will be deducted. The TA will enter your recitation attendance score each week.

  • Quizzes this semester will be timed quizzes on Carmen. They will be open between 7-10 PM on a Sunday. They are approximately 30 min quizzes for which you will be given 40 min. This means the latest you can start is 9:20 PM if you want the full 40 min.

  • Each quiz is worth 40 pts.

  • If you will have a documented conflict with quizzes on Sunday evenings you need to let me know before the first quiz. If something comes up later in the semester which conflicts with the quiz schedule you need to let me know ASAP. Don't make plans that will conflict with the quizzes after the semester starts. Don't wait until the last minute to tell me about a conflict.

  • You will not see the questions and answers after you've taken the quiz but they will be released later. Sometime after the quiz, I will be posting on my class webpage a sample quiz and an answer key. This will not be indentical to the quiz you'll take in Carmen but very similar.

  • We drop the 2 lowest quiz scores. We will excuse the 2 lowest attendance scores (has the effect of dropping the 2 lowest recitation attendance scores).

Quiz Information:

• Pre-quiz: Chem 1210 material

  This quiz covers some of the material you should have learned in 1210 that is relevant to 1220. The quiz is already on Carmen so you can take it during the first week, before we really get started. It will be due by 11:59 PM on Friday, 1/13. It will be graded and and the result recorded in Carmen. However, your score on this quiz will NOT count toward your final grade. You should use it as a guide to your level of understanding of 1210 material. I will use it for the same purposes.
  After the quiz closes a blank pre-quiz and the solutions will be posted at this link (not Carmen). This may not be exactly the same as the questions in the Carmen quiz since that has some randomly generated numbers. It will be a good representation of the quiz on Carmen. If you missed the due date I suggest you print it and take it (time yourself) and then grade yourself.
  You can find the sections from 1210 which I feel are most important for you to fully understand for 1220 on our class web page under the "Notes" link (at the top of that page). If you do not undertand this minimum subset of material from 1210 and struggle with this quiz you must correct your problems you will likely struggle this semester. The material you will encounter in 1220 is very different than what most of you have seen in the past, even if you've taken AP chemistry. The level of understanding we expect is very different than in high school and perhaps even in 1210. Many of you may not have had problems with the material in 1210 and did not have to work very hard to get a decent grade in 1210. Chem 1220 is very different.
  I've summarized info about the four types of solids and their properties. The types of solids are based on their attractive forces. See the link "Types of Solids and Their Properties" in the "Notes" section of the course web page. I also have another summary on line dealing with IAF, solids and solubility. See the link "Ch. 11/12 & 13 - Review of IAF, Solids and Solubility" in the "Notes" section of the course web page (we haven't covered the solubility stuff yet and you are not responsible for it yet).
  There are also pre-recorded videos on Carmen for chapters 11 and 12 from 1210. You can find them in the "Lecture" module on Carmen.

• Quiz 1: Chapter 13 (13.1-13.4)

  This covers material through last week. For the most part that's how coverage on quizzes will be, material from the previous week and maybe small amount from first lecture of the same week. This quiz covers last week's material, nothing from this week's lectures.
  Chapter 11: While this information is not on the quiz you need to review this chapter. In particular, for this coming quiz section 11.2 and 11.5. A lot of people had trouble with the prequiz given last week.
  Section 13.1:
  Understand the solution process and energy diagrams, how solutions form, ideal, endothermic and exothermic solution formation and the importance of entropy in solution formation. In general, when things mix there is an inc. in entropy (disorder) but this is not always the case. An inc. in entropy is absolutely necessary for an ideal or endothermic solution to form. This is not the case for an exothermic process. An exothermic process already tends to be spont. so an inc. in entropy is not necessary for this type of solution to form. There are cases in which the delta(H)_solution is negative, exothermic, and the entropy decreases (solution is more ordered) and the solution forms. Also, understand the role of attractive forces between particles in solution formation.
  In the 12th-14th editions the delta(H)_solvation is referred to as the the delta(H)_mix. This is step 3 (solute-solvent att. forces step), the exothermic step in the solution process as seen in my figures in the notes and Figure 13.4. The book doesn't show an ideal solution figure but I have it in the notes.
  I have a link showing the solution enthalpy diagrams including a discussion about the attractive forces and entropy, "Ch. 13 - Solution Formation and Solubility Effects" in the "Notes" section of the course web page.
  Section 13.2:
  Solubility, saturated, unsaturated and supersaturated solutions.
  Section 13.3:
  Factors affecting solubility - Att. forces ("like dissolves like"), pressure and temp. affects. You considered temp. effects and "like dissolves like" concepts in exp 1 (SOL).
  I have summary on line about attractive forces and solubility. See the link "Ch. 11 & 13 - Review of IAF, Solids and Solubility" in the "Notes" section of my course web page.
  Section 13.4:
  Concentration units (know definitions, how to calculate them, how to use them as conversion factors in problems and how to convert from one conc. unit to another - see my examples in the notes and on the class web page on the easiest way to approach these types of problems).
  Homework coverage (you should be able to all problems in the given ranges):
  The quiz covers sections 13.1-13.4. You should be able to do EOC exercise 13.1-13.9, 13.13-60, 13.93-13.99, 13.101, 13.107, 13.110
  For the on-line homework:
  The Tutorials and the Homework Review problem sets are for credit. They are due the Friday and Saturday, respectively, the weekend of the quiz. Think of them as a review of the material after you've done end-of-chapter problems.
  For Credit:
  Ch 13a (13.2, 13.4) Tutorials
  Ch 13b (13.1) Tutorials
  Ch 13c (13.3) Tutorials
  Ch 13a (13.2, 13.4) Homework Review
  Ch 13b (13.1) Homework Review
  Ch 13c (13.3) Homework Review
  Make sure you can do the assigned textbook questions, the tutorials and the homework review questions.

• Quiz 2: Sections 13.5-13.6, 14.1-14.2

  Sections 13.5-13.6:
  Make sure you can do colligative property calculations, including for ionic substances or ionizing molecular substances (things that dissociate or ionize to give multiple particles, NaCl, HCl, etc.). Know what the van't Hoff factor is (effective # particles or observed "i" - see "A Closer Look - The van't Hoff Factor" in section 13.5 (on page 551, 14th ed., of the paper book and my notes). Look at the link I have about colligative properties under the "Helpful Tidbits" link, "Colligative Properties" which was e-mailed earlier.
  An "ideal" ionic solution is one in which "i" (van't Hoff factor) equals the # of ions one gets from the formula when something dissocitates or ionizes. For NaCl the ideal "i" would be 2. For HCl the ideal "i" would be 2 (HCl is a molecular cmpd and when put in water it completly ionizes to produce H+ & Cl-). For a weak acid such as acetic acid, CH3CO2H, it doesn't completely ionize thus it's not possible to determine exactly what "i" is but it would be between 1, no ionization, and 2, completely ionized.
  You should understand how osmosis affects cells and what the terms isotonic, hypotonic and hypertonic mean.
  Finally, you should understand what colloids are and how you tell whether you have a colloid or a solution (Tyndall effect). Also, you should know the difference between hydrophilic and hydrophobic colloids.
  You should review section 2.7-2.8 on ions, their charges and polyatomic ions, which stay together as a single unit when an ionic compound dissolves. Also, review sections 4.1-4.3 which deal with electrolytes and nonelectrolytes in solution and acid/base reactions. Look at tables 4.2 and 4.3 in relation to strong and weak acids and bases.
  Homework coverage (you should be able to all problems in the given ranges):
  The quiz covers sections 13.5-13.6. You should be able to do EOC exercises 13.10-13.12, 13.61-13.92, 13.102-13.106, 13.108
  For the on-line homework:
  The Tutorials and the Homework Review problem sets are for credit. They are due the Friday and Saturday, respectively, the weekend of the quiz. Think of them as a review of the material after you've done end-of-chapter problems.
  For Credit:
  Ch 13d (13.5, 13.6) Tutorials
  Ch 13d (13.5, 13.6) Homework Review
  Make sure you can do the assigned textbook questions, the tutorials and the homework review questions.
  Section 14.1:
  Know what rate is and how it is related to concentration (rate law). Know what a rate law is and how you can use it, what the order is, rate constant, etc. Know how reaction rates and stoichiometry are related and how the rates of disappearance of reactants and appearance of products can be related to each other and the rate of the reaction (using the balanced equation).
  Section 14.2
  Know how to obtain a rate from data and how to use rate data to determine the rate law using the method of initial rates. This is shown in the book in sample ex 14.6 (and the practice exercise) and my notes. You really need to learn how to do this using the second example I used in lecture (the long one). If you don't you will have problems with some of the end-of-chapter exercises (especially the last one, 14.37, for section 14.2).
  Remember, rate laws can depend on concentration of reactants, products and catalysts. The orders of substances in the rate law can be whole numbers, simple fractions, negative (usually seen for products and inhibitors). To get the overall order you simply add the orders for everything in the rate law. Also, remember in general you can't write the rate law from the balanced chemical equation. It must be determined experimentally. The ONLY time you can write a rate law from a balanced eqn is if you know the reaction is an elementary reaction (a single-step mechanism) and you don't know this by simply looking at the reaction.
  Homework coverage (you should be able to all problems in the given ranges):
  The quiz covers sections 14.1-14.2. You should be able to do EOC exercises 14.1-14.5, 14.17-14.38, 14.90-14.94
  For the on-line homework:
  The Tutorials and the Homework Review problem sets are for credit. They are due the Friday and Saturday, respectively, the weekend of the quiz. Think of them as a review of the material after you've done end-of-chapter problems.
  For Credit:
  Ch 14a (14.1) Tutorials
  Ch 14b (14.2) Tutorials
  Ch 14a (14.1) Homework Review
  Ch 14b (14.2) Homework Review
  Make sure you can do the assigned textbook questions, the tutorials and the homework review questions.

• Quiz 3: Chapter 14 (14.3-14.6)

  Section 14.3
  Know what an integrated rate equation is for zero-order, 1st-order and 2nd-order reactions and be able to use them. Know what the half-life is for zero-order, 1st-order and 2nd-order reactions. This is in section 14.4. The equations for zero-order are in the notes and there are a couple of questions in the chapter 14 "handouts" discussed in class and on the web (see "notes" link) about zero and 2nd order. Be able to do the special problem discussed in class and sent via e-mail.
  Section 14.4
  Understand the relationship between temp., activation energy (Ea) and rate constant (Arrhenus eqn.) and the rate of the reaction. Understand how all this relates to collision theory and transition state theory.
  Section 14.5:
  Understand mechanisms and how to obtain a rate law from a mechanism, rate laws for elementary reactions, recognize intermediates, and what molecularity means.
  Remember, steps in a mechanism are always written as elementary processes, which means the rate law for a step can be written from the balanced eqn for that step. This is the ONLY time you can write the rate law from a balanced eqn., if you know it's an elementary reaction.
  Section 14.6:
  Know what catalysts are and the four common characteristics of catalysts, homogeneous and heterogeneous catalysis, how catalysts work and be able to recognize a substance as a catalyst or intermediate in a mechanism. Know how a catalyst affects rate and how this can be seen using the Arrhenus eqn.
  You can find the "handouts" mentioned above at Chapter 14 - Chemical Kinetics - Handouts .
  Homework coverage (you should be able to all problems in the given ranges):
  The quiz covers sections 14.3-14.6. You should be able to do EOC exercises 14.6-14.16, 14.39-14.88, 14.95-14.124
  Don't forget the extra homework problems discussed in class. They can be found on my web page at the Notes link (see above) or Homework link where you will also find the solutions, CH 14 - Kinetics, Extra Problems and Solutions .
  You will get the integrated rate equations and half-life eqns. on the quiz. They will not be in any particular order nor will the half-life eqns necessarily be in the same order as the integrated rate equations.
  For the on-line homework:
  The Tutorials and the Homework Review problem sets are for credit. They are due the Friday and Saturday, respectively, the weekend of the quiz. Think of them as a review of the material after you've done end-of-chapter problems.
  For Credit:
  Ch 14c (14.3) Tutorials
  Ch 14d (14.4) Tutorials
  Ch 14e (14.5-14.6) Tutorials
  Ch 14c (14.3) Homework Review
  Ch 14d (14.4) Homework Review
  Ch 14e (14.5-14.6) Homework Review
  Make sure you can do the assigned textbook questions, the tutorials and the homework review questions.

• Quiz 4: Chapter 15 (15.1-15.6)

  There could be a problem or two related to material from Ch 14. That shouldn't be a problem since you were just tested on it.
  Sections 15.1-15.4:
  You need to understand how to set up an expression for the equilibrium constant, K and how to use it. Understand how to set up K for heterogeneous equilibria (when you have pure solids and liquids involved in the equilibrium). What substances appear in the equilibrium constant expression? Gases and solutes in solution but not pure solids or liquids. How do you know if something is a pure solid or liquid? If there's and (s) or (l) for the state symbol in the balanced equation.
  What does the magnitude of K tell you? Does the reaction go to completion and by how much (mostly products or "essentially only" products)? Does the reaction "not occur to any great extent" and how little reaction occurs (mostly reactants or "essentially only" reactants)? Are there appreciable amounts of reactants and products at equilibrium?
  Remember K depends on the form of the balanced equation and you can relate the K for one form of the balanced equation to another. When you multiply an eqn by some factor the K for the new reaction equals the old K RAISED to that factor (you do NOT multiply the K by that factor). (e.g. K_rev = 1/K_for or K_for^-1 which makes sense since to get the reverse rxn you are essentially multiplying the forward rxn by -1).
  Know the relationship between equilibrium constants when you add several balanced equations to get a new balanced equation (the K's of the eqns being added are multiplied together to get the K for the resulting new rxn).
  Know how to relate K_p and K_c.
  Section 15.5:
  Know how to calculate K from conc. or pressures and vice versa using an ICE table.
  Section 15.6: Applications of Equilibrium Constants
  Understand the reaction quotient, Q, and how you use it with K to predict whether the reaction is at equilibrium or not and if not which direction does it proceed to reach equilibrium.
  Know how to use an ICE table to calculate equilibrium conc. starting with initial conc. and the equilibrium constant, K.
  I have some links to help you understand this material, especially using ICE tables.
  CH 15 - Chem. Equil. - Equil. Constant when Adding Eqns - Proof
  CH 15 - Chem. Equil. - ICE Table Example 1 from Notes (video presentation)
  CH 15 - Chem. Equil. - ICE Table Example 2 from Notes (rxn going in reverse)
  Homework coverage (you should be able to all problems in the given ranges):
  The quiz covers sections 15.1-15.6. You should be able to do EOC exercises 15.1-15.9, 15.13-15.60, 15.71-15.89
  Don't forget the extra ICE table problems: CH 15 - Extra Ice Table Problems and Solutions
  For the on-line homework:
  The Tutorials and the Homework Review problem sets are for credit. They are due the Friday and Saturday, respectively, the weekend of the quiz. Think of them as a review of the material after you've done end-of-chapter problems.
  For Credit:
  Ch 15a (15.1-15.2) Tutorials
  Ch 15b (15.3-15.4) Tutorials
  Ch 15c (15.5) Tutorials
  Ch 15d (15.6) Tutorials
  Ch 15a (15.1-15.2) Homework Review
  Ch 15b (15.3-15.4) Homework Review
  Ch 15c (15.5) Homework Review
  Ch 15d (15.6) Homework Review
  Make sure you can do the assigned textbook questions, the tutorials and the homework review questions.

• Quiz 5: Ch 15 (15.7), Ch 16 (16.1-16.5)

  There may be some overlap with section 15.6 (ICE table calculations).
  Section 15.7: Le Chatelier's Principle
  Understand how changing conc. shifts a reaction (AWAY from ADDED, TOWARD REMOVED). Remember adding or removing (small amounts, but not all) of a pure solid or pure liquid will not shift a reaction. Removing all of a pure solid or pure liquid will shift the reaction (toward the removed substance - you have to have some of the solid or liquid to be at equilibrium when they are present). Adding or removing a pure liquid which is also the solvent will cause a shift due to an indirect effect (e.g. adding solvent decreases the conc. of the solutes causing the reaction to shift toward more moles in solution, similar to what happens for gases when the volume is inc.). Conc. changes do NOT affect the numerical value of K.
  Know how changing pressure (due to volume changes) effects a reaction. Increasing pressure (by reducing the volume, which increases the conc. of all gases in the gas solution and thus inc. pressure) shifts the reaction toward fewer moles of gase. Decreasing pressure (by inc. the volume, which decreases the conc. of all gasses in the gas solution and thus dec. pressure) shifts the reaction toward more moles of gas. Changing volume for a gas is essentially changing the concentration of the gases. Decreasing volume increases the conc. of the gases and shifts the reaction to the side with fewer moles in solution (remember, a gas mixture is a solution). Pressure changes do NOT affect the numerical value of K.
  Remember, adding an inert (non-reacting) gas to a reaction involving gases will increase the total pressure but will NOT cause a shift in the reaction because the partial pressures of the gases involved in the reaction do not change.
  Something similar also occurs in reactions taking place in a liquid solution environment. When the volume of solution changes the reaction will shift if there is a change in moles of dissolved solutes. If the volume is increased by adding solvent the conc. of solutes in solution dec. and at that moment the reaction shifts toward more moles of solutes (and the comes back to a new equil.). This is like decreasing pressure by inc. volume for gases, the reaction shifts toward more moles of gas. If the volume is decreased by removing solvent (allowing some to evaporate) the conc. of solutes in solution inc. and at that moment the reaction shifts toward fewer moles in solution (and then comes back to a new equil.).
  Also, know how changing temperature shifts a reaction AND changes the numerical value of the equilibrium constant, K (changing conc. and pressures do not affect the numerical value of K). Treat heat as a reactant or product. How does the change in the forward and reverse rate constants (rates) cause the shift in the equilibrium and affect K for both exothermic and endothermic reactions? Remember, temperature changes have a bigger affect on reactions with bigger E_a.
  Homework coverage (you should be able to all problems in the given ranges):
  The quiz covers sections 15.7. You should be able to do EOC exercises 15.10-15.12, 15.61-15.70, 15.90-15.97
  For the on-line homework:
  The Tutorials and the Homework Review problem sets are for credit. They are due the Friday and Saturday, respectively, the weekend of the quiz. Think of them as a review of the material after you've done end-of-chapter problems.
  For Credit:
  Ch 15e (15.7) Tutorials
  Ch 15e (15.7) Homework Review
  Make sure you can do the assigned textbook questions, the tutorials and the homework review questions.
  Chapter 16 (16.1-16.5)
  Sections 16.1-16.2
  Acids and bases (Arrhenius and Bronsted-Lowry theory), conjugate acid/base pairs, relative strengths of acids and bases, predicting whether the acid-base reaction lies to the left or right at equilibrium.
  Lewis acid-base theory in this section is NOT on this quiz. We haven't covered it. We will cover it next week and it would be on Quiz 6.
  Sections 16.3-16.4
  Autoionization of water, K_w, pK_w, pH, pOH, pH scale. What does it mean for a solution to be neutral, acidic or basic, at any temperature.
  Section 16.5
  Strong acids and bases and weak acids and bases. You MUST know the 7 common strong acids and the strong bases (those discussed in the book, notes, class and on the class web page). All other acids or bases you see will be weak acids or bases (unless told otherwise). You need to be able to do calculations for strong acids and bases.
  There are 5 links concerning acids and bases on my class web page. Go to the "Helpful Tidbits" link and you will find them at the bottom. These came about from answering e-mail questions from students over the years. The first four acid-base links apply to the material covered by this quiz.
  Homework coverage (you should be able to all problems in the given ranges):
  The quiz covers sections 16.1-16.5. You should be able to do EOC exercises 16.1(a), 16.3-16.5, 16.13-16.52, 16.100, 16.102, 16.103, 16.105, 16.115-16.119
  For the on-line homework:
  The Tutorials and the Homework Review problem sets are for credit. They are due the Friday and Saturday, respectively, the weekend of the quiz. Think of them as a review of the material after you've done end-of-chapter problems.
  For Credit:
  Ch 16a (16.1-16.2) Tutorials
  Ch 16b (16.3-16.4) Tutorials
  Ch 16c (16.5) Tutorials
  Ch 16a (16.1-16.2) Homework Review
  Ch 16b (16.3-16.4) Homework Review
  Ch 16c (16.5) Homework Review
  Make sure you can do the assigned textbook questions, the tutorials and the homework review questions.

• Quiz 6: Chapter 16 (16.6-16.9)

  Sections 16.6-16.7:
  You need to be able to do calculations for weak acids and bases (using ICE tables). You should understand what polyprotic acids are and how to do calculations for them.
  Sections 16.8-16.9:
  Relationship between K_a, K_b and K_w, pK_a, pK_b and pK_w for a conjugate acid-base pair.
  You need to understand hydrolysis problems (acid-base properties of salt solutions). Know how the relationship between K_a, K_b and K_w for a conjugate acid-base pair is used for these problems. Be able to do calculations for salt solutions to determine pH, etc. This means setting up an equilibrium (ICE) table. You need to understand what the controlling equilibrium reaction is in order to set up the proper ICE table.
  There are 5 links concerning acids and bases on my class web page. Go to the "Helpful Tidbits" link and you will find them at the bottom. These came about from answering e-mail questions from students over the years. The first four acid-base links apply to the material covered by this quiz.
  Homework coverage (you should be able to all problems in the given ranges):
  The quiz covers sections 16.6-16.9. You should be able to do EOC exercises 16.6-16.11, 16.53-16.92, 16.101, 16.104, 16.106-16.112, 16.117, 16.119
  For the on-line homework:
  The Tutorials and the Homework Review problem sets are for credit. They are due the Friday and Saturday, respectively, the weekend of the quiz. Think of them as a review of the material after you've done end-of-chapter problems.
  For Credit:
  Ch 16d (16.6-16.7) Tutorials
  Ch 16e (16.8-16.9) Tutorials
  Ch 16d (16.6-16.7) Homework Review
  Ch 16e (16.8-16.9) Homework Review
  Make sure you can do the assigned textbook questions, the tutorials and the homework review questions.

• Quiz 7: Ch 16 (16.1 & 16.10) & Ch 17 (17.1-17.2)

  Sections 16.1 & 16.10:
  Acid-base behavior and structure, Lewis acid-base theory (in section 16.1) and how this theory encompasses Arrhenius and B-L theories. Remember, every Arrhenius acid or base is a B-L acid or base and every B-L acid or base is a Lewis acid or base. However, it doesn't necessarily go back the other way (BF3 is a Lewis acid but not a B-L or Arr. acid).
  Homework coverage (you should be able to all problems in the given ranges):
  The quiz covers sections 16.1 & 16.10. You should be able to do homework problems 16.1-16.2, 16.12, 16.17-16.18, 16.93-16.98, 16.99, 16.113, 16.120
  For the on-line homework:
  The Tutorials and the Homework Review problem sets are for credit. They are due the Friday and Saturday, respectively, the weekend of the quiz. Think of them as a review of the material after you've done end-of-chapter problems.
  For Credit:
  Ch 16f (16.10 & 16.1) Tutorials
  Ch 16f (16.10 & 16.1) Homework Review
  Make sure you can do the assigned textbook questions, the tutorials and the homework review questions.
  Section 17.1
  Common-ion effect. Know what is meant by a CI effect. Be able to do a CI problem to determine pH.
  Section 17.2
  Buffer systems are just a special type of CI problem. You should be able to recognize when you have a buffer system as compared to a "normal" CI problem. Why? If it's a buffer system you can use the Henderson-Hasselbalch eqn. to calculate the pH of a solution. Remember, to be a buffer you have to have some of each member of a conjugate acid-base pair of a weak acid or weak base (e.g. HF/F-, NH3/NH4+). To be a good buffer system the ratio of the base component to the acid component (or vice versa) should be between 10 and 0.1. Also, the conc. of each component should be relatively large, usually 0.001 M or larger. This has to do with something called buffer capacity, how much strong acid or base can be neutralized ("absorbed") by the buffer so the pH doesn't change much.
  Homework coverage (you should be able to all problems in the given ranges):
  The quiz covers sections 17.1-17.2. You should be able to do EOC exercises 17.1-17.4, 17.13-17.32, 17.84-17.89
  For the on-line homework:
  For Credit:
  Ch 17a (17.1-17.2) Tutorials
  Ch 17a (17.1-17.2) Homework Review
  Make sure you can do the assigned textbook questions, the tutorials and the homework review questions.

• Quiz 8: Chapter 17 (17.3-17.5)

  The quiz covers titrations (17.3) and solubility (17.4-17.5). They are closely related. You need to know about common-ion problems and buffers since these are encounterd during a titration and Ksp calculations. Make sure you understand common-ion systems and buffers as you need this for titrations. They were covered on quiz 7 and MT2. Titrations are essentially putting things together from Ch 16 and 17.1-17.2 into one comprehensive problem.
  Section 17.3:
  Acid-base titrations. Understand titrations and be able to calculate the pH at any point on a titration curve. This can cover all aspects of titrations, SA-SB, SB-SA, WA-SB, WB-SA, polyprotic acid titrations, polyprotic (polybasic) base titrations. You should understand the differences between SA-SB, SB-SA, WA-SB, WB-SA titration (e.g. Is the pH equal to 7, above 7 or below 7 at the equiv. pt.?).
  Section 17.4:
  Solubility equilibria, solubility and molar solubility, solubility-product constant (Ksp), calculating Ksp from solubility, calculating solubility from Ksp.
  Section 17.5:
  Factors affecting solubility (common-ion effect, pH effects, complex-ion formation, amphoterism).
  Homework coverage (you should be able to all problems in the given ranges):
  The quiz covers section 17.3-17.5. You should be able to do EOC exercises 17.5-17.11, 17.33-17.68, 17.90-17.93, 17.97-17.100, 17.102-17.109, 17.111, 17.113-17.116
  For the on-line homework:
  The Tutorials and the Homework Review problem sets are for credit. They are due the Friday and Saturday, respectively, the weekend of the quiz. Think of them as a review of the material after you've done end-of-chapter problems.
  For Credit:
  Ch 17b (17.3) Tutorials - due before spring break
  Ch 17c (17.4) Tutorials
  Ch 17d (17.5) Tutorials
  Ch 17b (17.3) Homework Review - due this past Monday
  Ch 17c (17.4) Homework Review
  Ch 17d (17.5) Homework Review
  Make sure you can do the "assigned" textbook questions, the tutorials and the homework review questions.

• Quiz 9: Ch 17 (17.6), Ch 5 (review) and Ch 19 (19.1-19.5)

  Section 17.6:
  Precipitation and separation of ions. Section 17.7 is just for your information about separation of ions. There will be no specific questions from 17.7. However, reading through this section may help you understand precipitation reactions and what types of compounds are usually insoluble and to what degree. There are a couple of homework problems to aid in this. Also, there is a Sample Integrative Exercise in this section you should be able to do.
  Section 17.7: This section is NOT on the quiz. We did NOT cover this material. You are not responsible for it. It will NOT be on Midterm 3.
  Homework coverage (you should be able to all problems in the given ranges):
  The quiz covers section 7.6. You should be able to do EOC exercises 17.10, 17.69-17.76, 17.116
  For the on-line homework:
  The Tutorials and the Homework Review problem sets are for credit. They are due the Friday and Saturday, respectively, the weekend of the quiz. Think of them as a review of the material after you've done end-of-chapter problems.
  For Credit:
  Ch 17e (17.6) Tutorials
  Ch 17e (17.6) Homework Review
  Make sure you can do the assigned textbook questions, the tutorials and the homework review questions.
  Chapter 5 (review) - no direct questions from this chapter:
  Understand first law of thermodynamics (conservation of energy and E=q+w from ch 5), state functions, Hess's Law, Enthalpy of Formation and how to use these to obtain enthalpies of reaction. There are questions in chapter 19 which refer to things from chapter 5 and enthalpy is used extensively in ch 19.
  See my chapter 19 notes (pages 1-17 to get an idea of what sorts of things you need to review from chapter 5).
  Section 19.1:
  Understand what a spontaneous process is. Understand the diff. between reversible and irreversible processes and how this is all related to spontaneous processes.
  Section 19.2:
  Entropy and the 2nd law of thermodynamics. Relationship between entropy and heat. Entropy for phase changes. Should be able to calc. entropy changes for both system and surroundings for reversible (equilibrium) and irreversible processes and relate this to the entropy of the universe.
  Section 19.3:
  Understand the molecular interpretation of entropy and microstates as well as Boltzmann's eqn (eqn 19.5). Molecular motions and energy and the relation to entropy (translational, rotational and vibrational motions, also called degrees of freedom - see the notes for more a more detailed explanation of these). Be able to make qualitative predictions about changes in entropy. Third law of thermodynamics.
  Section 19.4:
  Entropy changes in chemical reactions. Temperature variation in entropy. Standard molar entropies. Calculating the standard entropy for a reaction using standard molar entropies (eqn. 19.8). Entropy changes in the surroundings.
  Section 19.5:
  Understand free energy and how it relates to enthalpy, entropy, temp. and spontaneity. Know how to use std. free energies of formation to calc. std. free energy changes for a rxn (eqn 19.14).
  Homework coverage (you should be able to all problems in the given ranges):
  The quiz covers section 19.1-19.5. You should be able to do EOC exercises 19.1-19.6, 19.11-19.62, 19.85-19.92
  For the on-line homework:
  The Tutorials and the Homework Review problem sets are for credit. They are due the Friday and Saturday, respectively, the weekend of the quiz. Think of them as a review of the material after you've done end-of-chapter problems.
  For Credit:
  Ch 19a (19.1-19.2) Tutorials
  Ch 19b (19.3-19.4) Tutorials
  Ch 19c (19.5) Tutorials
  Ch 19a (19.1-19.2) Homework Review.
  Ch 19b (19.3-19.4) Homework Review.
  Ch 19c (19.5) Homework Review.
  Make sure you can do the assigned textbook questions, the tutorials and the homework review questions.

• Quiz 10: Ch 19 (19.5-19.7), Ch 20 (20.1-20.5)

  Section 19.5:
  There's some overlap with this section from Quiz 9. Understand free energy and how it relates to enthalpy, entropy, temp. and spontaneity. Understand the free-energy diagrams and how it relates to the relationships between del(G), del(G^o), the reaction quotient (Q) and the equil. constant. This is explained below under Section 19.7.
  Section 19.6:
  Understand how free energy varies with temp and how to predict under what temp conditions whether a reaction is spont or nonspont and how to calculate this as well.
  Section 19.7:
  Understand how free energy under nonstandard conditions relates to standard free energy and the reaction quotient. Understand the relationship between std. free energy and the equilibrium constant. Understand what the free energy change under nonstandard conditions (deltaG) means and what the free energy change under standard conditions (deltaG^o) means (i.e. deltaG tells you whether a rxn is spont or nonspont under any conditions and related to the slope of the free-energy curve under any conditions and deltaG^o tells you about the diff. in free energy between the products and reactants and tells you where the position of the minimum in the free-energy curve is, where the position of equilibrium lies) - see section 19.5 and the last few pages in the notes.
  Understand how to use the realtionship between K and deltaG^o to explain how K changes with temp. Also, look at the van't Hoff eqn I gave in the notes. It looks like the Arrhenius eqn but instead of the rate constant, k, it has the equil. constant, K, and instead of Ea it has delta(H^o_rxn). I used this to explain why K inc as T inc for endothermic rxns and why K dec as T inc for exothermic rxns. This was something we just kind of stated in Ch 15 and can now be explained.
  Homework coverage (you should be able to all problems in the given ranges):
  The quiz covers sections 19.5-19.7. You should be able to do EOC exercises 19.7-19.10, 19.61-19.84, 19.93-19.105
  For the on-line homework:
  The Tutorials and the Homework Review problem sets are for credit. They are due the Friday and Saturday, respectively, the weekend of the quiz. Think of them as a review of the material after you've done end-of-chapter problems.
  For Credit:
  Ch 19c (19.5) Tutorials (due last weekend)
  Ch 19d (19.6) Tutorials
  Ch 19e (19.7) Tutorials
  Ch 19c (19.5) Homework Review (due last weekend)
  Ch 19d (19.6) Homework Review
  Ch 19e (19.7) Homework Review
  Make sure you can do the assigned textbook questions, the tutorials and the homework review questions.
  Section 20.1:
  Understand oxidation states (oxidation numbers), redox reactions, what is oxidized and reduced and what are oxidizing and reducing agents (oxidant and reductant).
  Review section 4.4 (Oxidation Numbers and Redox Reactions).
  It would also be a good idea to do homework problems 4.8-4.9, 4.45-4.58. Also, see the following worksheet for additional practice on oxidation numbers:
  Oxidation Numbers Worksheet - Review of oxidation numbers
  Sections 20.2:
  Be able to balance redox reactions using the half-rxn method. When balancing in base, balance the reaction as if in acid first (adding H+ to the side which needs H atoms) and then "neutralize" the H+ by adding the appropriate number of OH- to the side with the H+ and ALSO the other side, as if it's a math eqn. The H+ and OH- will add up to give H2O. Then cancel H2O if they're on both sides. Don't forget, the H+ or OH- can wind up on the same side as the H2O.
  Sections 20.3:
  Understand voltaic cells, how they work, what occurs at the anode (oxidation) and the cathode (reduction), what the charges are on the anode (-) and cathode (+), etc. Understand the shorthand notation for a cell as given in lecture and the notes (and homework exercise 20.100).
  Sections 20.4:
  Understand cell potentials and standard cell potentials and how the two are related. Understand how to calculate cell pot. from reduction potentials for reduction half reactions. Understand how standard reduction potentials relate to the strengths of oxidizing and reducing agents. You need to know what is meant by standard conditions (1 M for conc of things in soln and 1 atm partial pressures for gases).
  Section 20.5:
  Understand how E and delta(G) are related and how E^o and delta(G^o) and the equilibrium constant are related and that a negative delta(G^o) and positive E^o indicate a spontaneous rxn and a K > 1.
  Homework coverage (you should be able to all problems in the given ranges):
  The quiz covers sections 20.1-20.5. You should be able to do EOC exercises 20.1-20.7, 20.13-20.64, 20.99-20.103
  For the on-line homework:
  The Tutorials and the Homework Review problem sets are for credit. They are due the Friday and Saturday, respectively, the weekend of the quiz. Think of them as a review of the material after you've done end-of-chapter problems.
  For Credit:
  Ch 20a (20.1-20.2) Tutorials
  Ch 20b (20.3-20.4) Tutorials
  Ch 20c (20.5) Tutorials
  Ch 20a (20.1-20.2) Homework Review
  Ch 20b (20.3-20.4) Homework Review
  Ch 20c (20.5) Homework Review
  Make sure you can do the assigned textbook questions, the tutorials and the homework review questions.

• Quiz 11: Chapter 20 (20.6-20.9) and Chapter 23 (23.1-23.3)

  There will be some overlap with Midterm 3 material (section 20.6-20.9).
  Sections 20.6-20.9: on MT 3
  Section 20.6:
  Nernst Eqn. You should be able to use this eqn. to calculate the E for a cell under nonstandard conditions. Understand concentration cells.
  Sections 20.7-20.8:
  Applications of voltaic cells. Understand what batteries and fuel cells are (in terms of being spontaneous and how to deal with the reactions - which are no different than what you do for voltaic cells. I won't ask you to draw or list equations for specific batteries). Understand corrosion and how to prevent it.
  Sections 20.9:
  Electrolysis, quantitative aspects of electrolysis (stoichiometry). Know the similarities and differences between voltaic and electrolytic cells.
  Understand how E and delta(G) are related and how E^o and delta(G^o) and the equilibrium constant are related and that a negative delta(G^o) and positive E^o indicate a spontaneous rxn and a K > 1 and a positive delta(G^o) and negative E^o indicate a nonspontaneous rxn and a K < 1. You still need to know this for electrolysis.
  Homework coverage (you should be able to all problems in the given ranges):
  The quiz covers sections 20.6-20.9. You should be able to do EOC exercises 20.8-20.12, 20.63-20.98, 20.106, 20.108-20.115
  For the on-line homework:
  The Tutorials and the Homework Review problem sets are for credit. They are due the Friday and Saturday, respectively, the weekend of the quiz. Think of them as a review of the material after you've done end-of-chapter problems.
  For Credit:
  Ch 20d (20.6) Tutorials - due before MT3 but still available for review
  Ch 20e (20.7-20.9) Tutorials
  Ch 20d (20.6) Homework Review - due before MT3 but still available for review
  Ch 20e (20.7-20.9) Homework Review
  Make sure you can do the assigned textbook questions, the tutorials and the homework review questions.
  Sections 23.1:
  Transition metals, properties of transition metals, lanthanide contraction, electron configurations and oxidation states (electrons come out of the s orbitals first), magnetism (understand the different types).
  Section 23.2:
  Transition-metal complexes (ligands, complex ions, coordination cmpds), Werner's Theory, coordination number, coordination sphere, metal-ligand bonding (Lewis acid-base rxns), be able to determine oxidation number and coord. number of the metal in a complex or coord. cmpd., geometries (often depend on the ligand - ligands which carry substantial negative charge reduce the the coord. number, i.e. # atoms directly bonded to metal atom)
  Section 23.3:
  Know what ligands are and the difference between monodentate, bidentate and polydentate ligands. Know the names and structures of the most common ligands (tables 23.4 and 23.5, for the 11th ed tables 24.2 and 24.3). For the bidentate ligands know oxalate, carbonate and ethylenediamine (en). For the polydentate ligands the most commonly seen are triphosphate ion and ethylenediaminetetraacetate ion (EDTA^4-). Know what chelation is.
  Homework coverage (you should be able to all problems in the given ranges):
  The quiz covers sections 23.1-23.3. You should be able to do EOC exercises 23.1-23.3, 23.11-23.34, 23.67-23.71. If a question asks you to give a name don't worry about that part.
  For the on-line homework:
  The Tutorials and the Homework Review problem sets are for credit. They are due the Friday and Saturday, respectively, the weekend of the quiz. Think of them as a review of the material after you've done end-of-chapter problems.
  For Credit:
  Ch 23a (23.1-23.2) Tutorials
  Ch 23a (23.1-23.2) Homework Review
  Ch 23c (23.3-23.4) Tutorials - due next weekend but do 1-3, 5 for this quiz.
  Ch 23c (23.3-23.4) Homework Review - due next weekend but do 1-10 for this quiz.
  Make sure you can do the assigned textbook questions, the tutorials and the homework review questions.

• Quiz 12: Ch 23 (23.3-23.6) and Ch 21 (21.1-21.4)

  There's some overlap with quiz 11 material. You need to understand 23.2 before you can do things in the other sections. I won't repeat the EOC exercises here since you can find those above in the homework list for quiz 11.
  Section 23.2:
  Transition-metal complexes (ligands, complex ions, coordination cmpds), Werner's Theory, coordination number, coordination sphere, metal-ligand bonding (Lewis acid-base rxns), be able to determine oxidation number and coord. number of the metal in a complex or coord. cmpd., geometries (often depend on the ligand - ligands which carry substantial negative charge reduce the the coord. number, i.e. # atoms directly bonded to metal atom)
  Section 23.3:
  Know what ligands are and the difference between monodentate, bidentate and polydentate ligands. Know the names and structures of the most common ligands (tables 23.4 and 23.5, for the 11th ed tables 24.2 and 24.3). For the bidentate ligands know oxalate, carbonate and ethylenediamine (en). For the polydentate ligands the most commonly seen are triphosphate ion and ethylenediaminetetraacetate ion (EDTA^4-). Know what chelation is.
  Section 23.4:
  Do NOT worry about naming transition-metal (coordination) compounds in this section.
  Isomerism. Know what isomers are. Know the two main groups (structural and stereoisomers) and the 4 specific branches from these two main groups: coord. sphere, linkage, geometric and optical (enantiomers). You need to be able to draw the cmpds from the formula and the description given (for a coordination number of 4 I would tell you whether it's tetrahedral, or sq. planar). You should realize when the coord. # is 6 it has to be octahedral. Understand what enantiomers are (nonsuperimposable mirror images). Know these are chiral and optically active and one is dextrorotatory (d) and the other would be levorotatory (l). There's no way to tell which is which simply by looking at them. However, if I tell you one is (d) then it's enantiomer has to be (l).
  Section 23.5 (Color and Magnetism in Coordination Chemistry):
  Color and magnetism. Understand the color wheel (which will be given) and complementary colors and how this is related to the crystal-field splitting (size of splitting, energy, wavelength, etc.).
  Section 23.6 (crystal field theory, CFT):
  Remember in CFT we are looking at the metal-centered d orbitals and the electrons in those orbitals from the metal itself. We are not considering any of the electrons from the ligands when it comes to the diagrams we use because these electrons are in molecular orbitals which are primarily ligand centered (located on the ligands) and are much lower in energy and filled. The electron transitions we are considering are from one d-orbital on the metal to another d-orbital on the metal.
  You should know how the metal "d" orbitals are split (arranged) for linear, tetrahedral, square planar and octahedral complexes.
  For an octahedral crystal field energy diagram the t₂ (or t_2g) set of orbitals (d_xy, d_xy, d_xy) are lower in energy than the e (or e_g) set of orbitals (d_z^2, d_x2-y2).
  You should know what is meant by weak-field and strong-field ligands and how this effects the splitting of the e and t₂ orbitals on the metal ion. You should know what are crystal-field splitting and spin-pairing energies and how to determine if something will be a high-spin complex or low-spin complex. This depends on whether the ligand is a weak-field or strong-field ligand (strength
  Homework coverage (you should be able to all problems in the given ranges):
  The quiz covers sections 23.2-23.6. You should be able to do EOC exercises 23.2-23.10, 23.21-23.66, 23.69-23.94. Ignore any questions that ask you to name complexes.
  For the on-line homework:
  The Tutorials and the Homework Review problem sets are for credit. They are due the Friday and Saturday, respectively, the weekend of the quiz. Think of them as a review of the material after you've done end-of-chapter problems.
  For Credit:
  Ch 23b (23.3-23.4) Tutorials
  Ch 23c (23.5-23.6) Tutorials
  Ch 23b (23.3-23.4) Homework Review
  Ch 23c (23.5-23.6) Homework Review
  Make sure you can do the assigned textbook questions, the tutorials and the homework review questions.
  Section 21.1:
  Nuclear eqns. Types of radioactive decay and particles (alpha, beta, positron emission, electron capture) and gamma radiation.
  Section 21.2:
  Patterns of nuclear stability (neutron-to-proton ratio, belt of stability, stability based on whether the number of protons and neutrons are even or odd, magic numbers, radioactive series.
  Section 21.3:
  Nuclear transmutations (including the shorthand representation given in section 21.3 for the transmutation reaction), reactions involving neutrons, transuranium elements.
  Homework coverage (you should be able to all problems in the given ranges):
  The quiz covers sections 21.1-21.3. You should be able to do EOC exercises 21.1-21.4, 21.9-21.32, 21.71-21.72, 21.74.
  For the on-line homework:
  For Credit:
  Ch 21a (21.1-21.2) Tutorials
  Ch 21b (21.3-21.4) Tutorials
  Ch 21a (21.1-21.2) Homework Review
  Ch 21b (21.3-21.4) Homework Review
  Make sure you can do the assigned textbook questions, the tutorials and the homework review questions.

Solutions:

• Prequiz
• Quiz 1
• Quiz 2
• Quiz 3
• Quiz 4
• Quiz 5
• Quiz 6
• Quiz 7
• Quiz 8
• Quiz 9
• Quiz 10
• Quiz 11
• Quiz 12

Blank Quizzes:

• Prequiz
• Quiz 1
• Quiz 2
• Quiz 3
• Quiz 4
• Quiz 5
• Quiz 6
• Quiz 7
• Quiz 8
• Quiz 9
• Quiz 10
• Quiz 11
• Quiz 12