MULTIPLE CHOICE SECTION: The May of 2011 ACP Chemistry final exam is made up of  50 multiple choice questions.  This ACP exam is given to ALL chemistry students throughout the state of Indiana who are enrolled in ACP Chemistry.  It is the Indiana University cxam for CHEM 101 (this is the IU Bloomington chemistry course for non-science majors and nursing students).  (NOTE: Students taking this course for ACP credit through IU may NOT skip the final exam.)  This exam covers only the lecture material (no lab component).

For the review, each student will have access to a PACKET of questions which include a review of ALL of the Chemistry Standards.  There are a total of 47 Indiana Chemistry Standards so you can assume that you will have one question for each standard.  

You will also have a "short answer" review packet given to you each day.

• Part I: Chapters 1-5 Short Answer Review

• Part II: Chapters 6-9 Short Answer Review

• Part III: Chapters 10-13 Short Answer Review

• Part IV: Chapters 14-19, 20, 22 Short Answer Review

SOLUTIONS: As you complete the review process, you will be given solution sets to the work you've done.  These will be given out in class. In addition to the answers, each question has a specific page reference.

PROBLEMS SECTION:  

In addition to the ACP chemistry final, you will have a problems section (designed by us).

• These are problems which test your fundamental understanding of the nature of matter and test whether you can utilize appropriate math skills to solve mathematics-based chemistry problems. 
• BRING YOUR NON-GRAPHING CALCULATOR TO CLASS EVERY DAY AND FOR THE FINAL EXAM.
• For the exam, students will be receiving a stapled set of "reference sheets". 

See helpful hints below:

1. Substances (elements and compounds) and the fundamental characteristics of the phases of matter.  

Hint: This concept tested will also include:

• knowing the difference between a solid, liquid and gas (in terms of particles)
• knowing the difference between an atom and an ion
• knowing the difference between covalent and ionic compounds
• knowing the difference between homogeneous mixtures and heterogeneous mixtures
• knowing the difference between physical changes and chemical changes

2. Reaction prediction and balancing chemical equations.

Examples:
Aluminum plus nitrogen ®
Sodium carbonate ®
Nickel (II) chloride plus ammonium sulfide ®
Scandium plus hydrochloric acid ®

Hint: Be sure to have memorized all the types of reaction prediction types. In addition, you'll need to be able to write formulas correctly and balance equations in order to receive full credit for these problems.

Hint: It is also likely that you will have stoichiometry problems which ALSO involve first writing the balanced chemical equation (like above).

3. Stoichiomentry (including limiting reactants and solution chemistry stoichiometry) - FOCUS ON THESE TYPES OF PROBLEMS.

Example: Calcium reacts completely with 100 mL of a .20 M aqueous solution of HCl to produce hydrogen gas and an aqueous solution. How many grams of calcium was consumed?

Example: 25 g of magnesium nitrate reacts with an excess of calcium carbonate.  Find how much magnesium carbonate is produced.

Hint: Be sure to write and balance the chemical reaction first. Then, use the molar connection in your dimensional analysis.

Example: 17 grams of methane are allowed to react with 20 grams of oxygen. Find the mass of water produced.  What is the limiting reactant?  What is the excess reactant?

Hint: You'll need to set up two dimensional analyses  in order to determine the correct answer. Pay attention to sig figs.

Example: 25 mL of a 0.25 M solution of potassium hydroxide reacts with 15 g of magnesium chloride.  How many grams of water is produced?  What is the limiting reactant?  What is the excess reactant?

PRACTICE PROBLEMS DURING CLASS