Total points: 27	[Plus bonus problems, 9 pts.]

Take home test. Test 2 covers Ch 6 through Ch 10. Much of the test is on material from the two written assignments. 

DUE: Wednesday, 11/9/05, start of class. 

Test is closed book. You may use a note page (one page, 8.5 x 11), plus a periodic table. Calculators “required”. You may supply scratch paper. (You may need some extra paper for the bonus questions.) You may NOT use books, handouts, models, other class or reading notes, other outside sources, etc (except for the specific items listed above).

The general idea is that a take home test is just like a test in class, except that you determine the time and place to take it.

Do not open the test until you are ready to start taking it. Opening the test marks the end of your study time and the beginning of test time. Prior to beginning the test, you may study as much as you wish, and in any way. You may study with others, so long as no one involved has yet opened the test. You may not discuss the test with others (except me) until after the test has been turned in.

This test is similar to other tests in this course (including the samples). Try to resolve doubts about the meaning of test questions by considering them in the context of this course. If you feel there are ambiguities in a question, state any assumptions you make.

Estimated time: 1-2 hours (plus bonus section). It is not a timed test. Take the time you need to do it well. As long as you feel you are being productive, you are welcome to continue. (That also means you need to know when to stop.) I would appreciate it if you would note how long you took.

You should take the test “straight through” in one session (except for the rather long and optional bonus section; see note there). However, you may seek clarification of test questions at a reasonable time after your primary session. This may include asking me about test questions before class.

Feel free to contact me (<contact information>), either in preparation for the test or if you need clarification of questions during the test. I will “guarantee” phone availability Tuesday evening 7-9 pm. I will send any test clarifications/corrections that come up to the class e-mail list.

For “emergency use only” You may return the test by mail (postmarked by the due date): <address>. (Do NOT send by any method that requires my signature to pick it up.)

•	Please sign the “Honor System pledge” (next page).

Total points: 27	[Plus bonus problems, 9 pts.]

General
•	Closed book. You may use a note page, plus a periodic table. 
•	Calculator “required”.
•	If a question isn’t clear, please ask me about it.
•	Some questions request a simple answer and an explanation. It’s the explanation that is important. No credit for answer without a requested explanation. 
•	Show phases in all equations.
•	Show work and show units on all calculations. Try to show correct number of significant figures (SF) in final results. I will grade on this in most problems.

N = 6.02x1023; density of water = 1.0 g/mL; 3.785 L = 1 gallon; molar volume of any ideal gas, at STP: 22.4 L. 1 pound = 454 g. Pico = 10-12; nano = 10-9; micro = 10-6.

Please SIGN the following agreement (often referred to as an Honor System pledge).

	I agree to take this test according to the rules established for it.

								(-signature)

Reminder Show phases in all equations you write; use clear dimensional analysis on all conversions; show proper SF in answers.

1. (1 pt.; no credit without explanation) Consider the compound Cu2Se. One of the ions in this compound could be easily predicted by looking at the PT. Which one, and why (or how)?

2. (1 pt.; no credit without explanation) The formula for sodium tungstate is Na2WO4. Knowing that what would you expect the formula for calcium tungstate to be? Briefly explain how you can figure it out.

3. (2 pts.) Calculate the formula mass (molar mass) of iron(III) chloride hexahydrate. (Show what numbers you use.) Units???

4. (2 pts.; 1 pt. per part) 

a. Write the formula of lithium sulfate.

b. Write the formula of lithium sulfide.

5. (2 pts.) You have 218 g of potassium carbonate. How many moles is this? (As on all problems, show clear work, with clear units.) (Carbonate is CO32-, which you should know.)

6. (2 pts.) Balance the following equation:

    B2O3 (s) +     HF (l)        BF3 (g) +      H2O (l)

7. (6 pts.; 2 pts. per part) Butane is a hydrocarbon fuel similar to gasoline, but lighter. It is sold as “bottled gas”, and is used in cigarette lighters. The chemical formula of butane is C4H10. Consider the complete combustion of butane. (Parts a and b are independent.)

a. H for the reaction is -2.89x103 kJ/mol of butane. How much heat would be obtained by burning 850 g of butane? Show clear work.

b. Write a balanced equation for the complete combustion of butane. Show phases.

c. Using your equation from part b, calculate the mass of any one product obtained from burning 1.00 kg of butane.

8. (3 pts.) Consider the element with electron configuration 1s22s22p63s23p5.

a. (1 pt.) What element is this? How do you know?

b. (1 pt.) What charge do you expect for a simple ion from this element? How can you tell -- based on the electron configuration?

c. (1/2 pt.) Which of the electrons are the valence electrons?

d. (1/2 pt.) Give one example of another element with the same number and type of valence electrons.

9. (2 pts.) The explosion of nitroglycerin is described by the following balanced equation:

4 C3H5(NO3)3 (s)  12 CO2 (g)+ 10 H2O (g) + 6 N2 (g) + O2 (g)

a. (1 1/2 pts.) If 8.7 moles of nitroglycerin react, how many moles of water vapor will be produced? Show clear work, with a clear conversion factor. The purpose of the question is to see the relationship. Show proper SF.

b. (1/2 pt.) How would you classify this reaction, using one of the common terms for describing types of reactions? A 1-2 word standard term is preferred (e.g., double replacement.)

10. (2 pts.; 1 pt. per part) “Calcium chloride” is CaCl2.

a. When we say that a mole of calcium chloride contains twice as much chlorine as calcium, what do we mean? (For example, does this statement mean that the mass of chlorine is twice the mass of calcium in this compound?)

b. Make a sketch to show what calcium chloride is composed of at the particulate level. (Show each atom or ion, with its proper formula.)

11. (2 pts.) You mix aqueous solutions of magnesium nitrate and sodium hydroxide, and observe a white precipitate. Write a balanced equation for the reaction. Show phases. (Hydroxide is OH-, which you should know.)

12. (2 pts.) A useful reaction in the processing of an ore of titanium is the following: The ore consists largely of FeTiO3; it is reacted with carbon monoxide, which helps remove O from the mineral. The products are metallic iron, titanium(IV) oxide, and a common gas. Write a balanced equation for this reaction. Include phases.

BONUS QUESTIONS: 9 pts. (Reminder The bonus questions are intended as an extra challenge; they are not an important part of your score. Focus on the main set of questions. However, each of the bonus questions deals with some interesting issue, probably a little more advanced than the main coverage in the course. I hope that most of you will at least try most of these.)

This is a rather long bonus section. I did that because I wanted to be able to offer some significant range of more challenging questions, for those who want such a challenge. Because of the length, it is ok if you want to take a break and do this at a second sitting, even the next day. However, except for that, please follow general test procedures here. You might need more space for a couple of these; just attach an extra page, labeled.

B1. (1 pt.) We indicated that the common aluminum ion is Al3+. But in fact, this is an oversimplification. Aluminum tends to form complexes with other ions and water molecules. One particular ionic form of aluminum is AlO4Al12(OH)24(H2O)12. What charge would you expect on this complex structure, assuming that each atom (or group) individually is in its common ionic form? Explain (or show clear work).

B2. (1 pt.) Consider the sample from question #5. How many grams of oxygen are in this sample? Show clear work.

B3. (2 pts.) The concentration of gold in the oceans is about 10 parts per trillion (10 g gold/1012 g ocean). The volume of the Pacific Ocean is about 1 ZL (Z = zetta = 1021.) What is the value of the gold in the Pacific Ocean, assuming that the price of gold is about $450/ounce? That is the troy ounce (used for precious metals); 31 g per troy ounce. Show clear dimensional analysis setup and show appropriate SF; state any assumptions you make.

Think about Why, then, don’t we harvest the gold from the ocean?

B4. (3 pts.) 
a. (1 pt.) Sulfur dioxide, water and calcium sulfide react to produce calcium hydroxide and sulfur. Write a balanced equation for this reaction. (You can write sulfur as S.) Show the phase for each chemical.

b. (1 1/2 pts.) If you react 6.00 moles of sulfur dioxide and 9.00 moles of calcium sulfide, how many moles of sulfur could be made? Explain. Show work as appropriate.

c. (1/2 pt.) We have discussed several “types” of reactions. How would you classify this reaction? Explain. (Careful. This is something of a trick question.)

B5. (2 pts.) The maximum level of lead allowed in drinking water is about 1.5x10-5 g/L. How many lead atoms (or ions) would be allowed in a glass of water? State any assumptions you make, and show clear work.

cq\pq2
10/31/05