MASTERY OBJECTIVES FOR CHEMISTRY:
SECOND SEMESTER - 2008

The following are a summary of the essential objectives you need to know for the final exam.  The exam questions will be testing your mastery of these areas.  By way of studying for the final, I suggest that you review your unit documents, self-tests, old tests and quizzes and your textbook, of course.  You can see sample exam questions from past year’s exam on the website.

Unit 6: Reactions and Stoichiometry – Chapter 12

  1. Calculate chemical quantities from balanced chemical equations using units of moles, mass, representative particles and volume (gases at STP).  (12.2)

  2. Draw atomic level pictures that represent chemical reactions in terms of proportions of reactants and products including states, types and formulas of compounds. (GIAs)

  3. Identify the limiting reactant in a reaction and to quantify the amount of excess reactant(s) using either atomic level pictures or numerical stoichiometric quantities.  (12.3 and GIAs)
  4. Derive the empirical and/or molecular formula of a compound from experimental data.  (10.3 and lab practical)

UNIT 7: States of Matter Chapters 13 & 14

  1. Describe the kinetic-molecular theory, and explain how it accounts for observed physical behavior in solids, liquids and gases. (Chapter 13 and 14.1)

  2. Explain what gas pressure means, describe how gas particles cause pressure, and be able to convert between different units of pressure. (13.1)

  3. Describe the nature of liquids and the intermolecular forces that determine their physical properties. (13.2)

  4. Identify the features of a phase diagram of a pure substance. (13.4, essay assignment)

  5. State the gas laws, give their mathematical relationships and describe the relationships in terms of the kinetic molecular theory.  (Boyle’s Law, Charles’ Law, Gay-Lussac’s Law, the Combined Law, Dalton's Law of Partial Pressures) (14.2)

  6. Discuss the significance of the ideal gas law, pointing out the assumptions behind the law.  Compare ideal and real gases. (14.3)

  7. Calculate an unknown quantity using the Ideal Gas law. (14.3)

  8. Be able to do stoichiometric calculations involving gases. (worksheet and lab)

UNIT 8: Solutions, Equilibrium and Solubility - Chapters 15, 16 & 18

  1. Explain why all soluble ionic compounds are electrolytes.  (15.2)

  2. Differentiate among saturated, unsaturated, and supersaturated solutions.  (16.1)

  3. Explain how solutions form and describe the factors that affect the rate at which a solute dissolves. (16.1)

  4. Define solubility and describe the factors that affect solubility.  (16.1)

  5. Measure and calculate the concentration of a solution in terms of molarity, and apply calculations to stoichiometry problems involving solutions. (16.2 and GIAs)

  6. Define a colligative property of a solution and describe three such properties.  (16.3)

  7. Define chemical equilibrium and explain how it is achieved in relation to reversible reactions.  (18.2)

  8. Write the equilibrium constant, Keq, expression from a balanced chemical equation.  (18.2)

  9. Analyze the extent of the reaction or position of the equilibrium based upon the size of the equilibrium constant, Keq.  (18.2)

  10. Distinguish between exothermic and endothermic reactions in terms of enthalpy change and how energy moves between a system and its surroundings.  (17.1)

  11. Explain Le Chatelier’s Principle and describe how changes in concentration, pressure and temperature affect a reaction at equilibrium.  (18.2)

  12. Predict whether or not a precipitate will form when two solutions are mixed, based on a solubility table or the table of general solubility rules for ionic compounds.  (18.3)

  13. Write the Ksp expression for a dissolution/precipitation equilibrium and calculate the equilibrium ion concentrations for a slightly soluble salts. (18.3)

UNIT 10: Acids and Bases - Chapter 19

  1. Identify common physical and chemical properties of acids and bases.  (19.1)

  2. State the Bronsted-Lowry definition of acids and bases, and identify conjugate acid-base pairs in acid-base reactions using the Bronsted-Lowry theory.  (19.1)

  3. Describe the auto-ionization equilibrium of water with a chemical equation and a Kw expression. (19.2)

  4. Describe the pH scale.  (19.2)

  5. Inter-convert between the pH of a solution and the hydronium-ion or hydroxide-ion concentration.  (19.2)

  6. Explain how equilibrium constants are related to the dissociation constants of acids and bases.  (19.3)

  7. Explain what dissociation constants indicate about an acid’s or base’s strength. (19.3)

  8. Calculate Ka’s or equilibrium concentrations of ions using the ICE method. (19.4 and GIA)
  9. Demonstrate how certain salts can exhibit acidic or basic properties.  (19.5)
  10. Identify a buffer, and with chemical equations explain how buffers work. (19.5)

Unit 11: “The Chemistry of Life” Chapters 22-24

  1. Identify the source of complexity and diversity in organic molecules as the existence of isomers, structural, geometric and optical.  (22.3)

  2. Identify the following functional groups by the characteristic atom groups: alcohols, ketones, aldehydes, carboxylic acids, esters, amines and amides.  (Table 23.1, p. 726)

  3. Identify some basic properties of the following classes of compounds: alcohols, ketones, aldehydes, carboxylic acids, esters, amines and amides.  These properties would include water solubility, boiling points and whether the molecules can hydrogen bond or not. (23.2-3)

  4. Describe the structure and functions of carbohydrates. (24.2)

  5. Describe the structure and functions of lipids.  (24.4)

  6. Describe the structure and functions of proteins.  (24.3)

  7. Describe the structure and functions of nucleic acids.  (24.5)

  8. Discuss in a short answer or essay format the interrelated functions of carbohydrates and proteins, lipids and proteins, and proteins and nucleic acids. 

  9. Articulate what it means to say that polysaccharides, proteins and nucleic acids can all be called “biopolymers.” (23.4)

 

Suggested Activities and Timetable for Preparing for Exams.

1)      Week of May 19: Get organized and Work on Review Labs for Empirical Formula and Gases.

a)      Collect materials from each unit of the 2nd semester (units 6-11).  This would include: self-tests, quizzes, tests, relevant worksheets and labs.

b)      Determine what you are missing and get copies of what you need from the internet, from friends or from me, Mr. Ause.

Reviewing Units:

c)      Look over the objectives, refreshing your vocabulary and the components of this unit.

d)      Review your quizzes and tests, especially looking at those questions you missed.

e)      Write an outline of the units using your notes, book and other sources.

f)        Bring your questions to me during tutorials in the following week.

2)      Weekend of May 24-26: Review Units 6- 8 (as suggested above)

3)      During exam week attend tutorials Tues & Wed 1:00 pm – 3:30

a)      Go over the exam questions available on the Chemistry class website.

b)      Bring in your specific questions for review during tutorial and class during the next week.

4)      General Reminders:

a)      Focus on the Mastery Objectives; regularly refer to these.

b)      Spread out your studying.

c)      Ask your questions of your classmates and me.

d)      Use your old tests and quizzes to test your studying.