Chemistry 110, Spring 2005, Section 3

Dr. Petr Vanýsek, Instructor

     Q: When do I see the results of my test?
     A: You will be able to pick up a printed slip with your score, correct answers and your answers the very next class after the test. If you do not get it there, then you can get it during the regular office hours.

Results for Test I were available in class on Thursday, February 3rd. If you did not pick them up, see me during my office hours.
Results for Test II were available in class on Tuesday, February 22nd. If you did not pick them up, see me during my office hours.
Results for Test III were available in class on Thursday, March 20th. If you did not pick them up, see me during my office hours.
Results for Test IV were available in class on Thursday, April 7th. If you did not pick them up, see me during my office hours.
Results for the Final are not printed on the invidiual slips by the Testing Service, thus, I cannot give you back invidual reports. Note on your test forms what answers you chose.

The answers for the final are posted on my office door.

 

The following is recommended study material for the upcoming tests and quizzes

 

Note on the sample problems: (The following is an example from a 2003 test.) They are rephrased questions from the test, made more generic than the actual questions. Part of your learning experience, if you want to use this guide, is to figure out the clues. Example:
The test question looks like this:
How many grams of NaOH will be needed to prepare 250 ml of 3.0 mol/l solution of NaOH. Assume molecular mass of NaOH to be 40.0 g/mol.
        a)    30.0 g
        b)    30000 g
        c)    18000 g
        d)    18.75 g
        e)    33.3 g

However, the guide question looks like this:
Given the volume and desired concentration of NaOH solution, how many grams of NaOH have to be taken to prepare such solution?

 

 

 

Past tests:

Test I - 1 February 2005

50 questions (multiple choice, 5 choices, one correct)

[The following 12 subjects areas will be covered by more than just one question in the test.]

1.       Determine how many significant figures are in a given number. Example: 20.130, 2005, 340.

2.      Report a number (e.g., 0.0054354) using exponential form and using a requested number of significant figures.

3.       Know how to solve problem 1.85 

4.      Perform calculation (addition, division, subtraction, multiplication) and report the result using correct number of significant figures.

5.      Know the names (including the Latin forms) and symbols for chemical elements from Table 2.2. Pay also attention to the correct spelling.

6.     Know the definition of density and be able to perform a density related calculation.

7.     Know how to predict from density whether an object will float in a liquid, or whether it will sink.

8.     Know prefixes used to change magnitude of units, know the corresponding values and know how to convert between units. For example: how many kg is 3.48 mg?

 9.    Orient yourself in the periodic table. Know the alkali metals, alkaline earth elements, halogens, noble gases, metals, non-metals.

10. Know the basic composition of an atom (electrons, protons, neutrons, nucleus). Know what is the mass number, atomic number and know how to figure out from various clues the number of electrons, protons and neutrons in an atom.

11. Know what is an isotope. 

12. Know some of the properties of the elements mentioned in class.

 

Test II - 17 February 2005
(posted 8 February 2005)

Material from Chapters 1, 2, 3, and early part of 4 covered.

 

bullet

   Report given number (e.g. 0.030016) in the exponential notation using given number (e.g., four) significant figures:

bullet

   Know how to perform direct and inverse proportions calculations.

bullet

   Know the symbols, names, Latin names and correct spelling of the previously assigned elements.

bullet

    Know metric prefixes, their values, conversion between units with different prefixes. Know the conversions between units of length, area, and volume. 

bullet

How many cubic centimeters of olive oil have the same mass as 0.500 liter of ethylalcohol? (Densities given on page 29. If such question is given on the test, the densities would be provided.)

bullet

Calculate average atomic mass of an element, if percent composition by individual isotopes is given.

bullet

What is the largest number of electrons that can be present in the first, second, third and fourth electron shell?

bullet

Know what it fusion and fission.

bullet

Know what is alpha and beta emission and what is gamma radiation.

bullet

For a given reaction, e.g.,

                                         Th    ŕ   Rn  +  He

       name the process that is described by the reaction.

 

bullet

Write the correct electron configurations for some simple atoms? (e.g. Li, Be, B, C, Na, Si, S, Al)

bullet

Know how to perform calculations with half-life concept. E.g., A radioactive element has half-life of 6.0 hours.  How much time has lapsed, if from the original sample weighing 96 mg all what is left are 2 mg of the element?

bullet

Know what are valence electrons. Know how to determine how many valence electrons a given element has.

bullet

Know how to use (draw) the electron dot structure.

bullet

Know what is a cation, what is an anion.

bullet

Know the rules for naming ionic compounds

bullet

     What are the radioactive particles released in the following nuclear equations?

                              

                              

bullet

Know what the electron subhells are, how many electrons can each hold and how are they named.

bullet

Be familiar with the requirements of the class syllabus, know the grading scale of the class, bring with you for the test the required calculator.

bullet

Know what are the groups, periods, isotopes, electron arrangement (configuration).

bullet

Why is it that all of the isotopes of elements with atomic number of 84 and higher are radioactive?

 

 

Test III - 8 March 2005

- Name chemical compounds, e.g., what is the name of FePO4 ?

- Know the names, formulas and charges of the common ions and anions (including the polyatomic ions).

- Know the rules of naming chemical compounds. Know the rules for writing formulas for chemical compounds.

- Know the types of bonds (polar, covalent... etc.). Be able to tell in which compound which bond can be encountered.

- Know what is electronegativity and where it can be used.

- Know how to use the octet rule.

- Know how to decide the shape of a molecule (bond angle).

- Know what is a polar bond; know what is a polar molecule. Understand how the two are related.

- Thermochemistry calculations: E.g.: If 3.5 g of sample are burned and the heat released is 48 kJ, what is the caloric value of this material (in kJ/g)?

- Container is filled with hot water (890 g), at temperature 65 oC. How much heat is released when the water cools down to 25 oC.

- Several more calculations, similar in concept to the two above.

- What types of interactive forces may occur between two atoms?

- Thermochemical calculations related to phase changes: E.g., how much energy is released when 250 g of water at 25 oC cools down to 0 oC and solidifies into ice?

- What is the relationship between temperature and thermal motion of particles?

- Know condensation, evaporation, melting, fusion, sublimation, etc.

- What is kinetic; potential energy. Know examples.

- What are the units of energy, know examples of kinetic and potential energy; how is the dietary unit (in the USA) related to the other energy units?

- What is the ability to do work?

 

 

Test IV - 5 April 2005  
(posted 29 March 2005)

50 questions (multiple choice, 5 choices, one correct)

 

- What is a physical and what is a chemical change? Know examples.

- What is oxidation and reduction. How it this manifested in biological systems?   Know how to find what is oxidized and what is reduced in a chemical equation.

 - Know hot to balance chemical reactions.

 - Know what is a reactant, catalyst, reaction product, solvent.

- Know types or reactions, for example endothermic and exothermic. But there are other          classifications as well.

- Know the meaning of the Le Chatelier's principle.

- Know how to calculated moles, molecules, grams, atoms.

- What is an equilibrum reaction, what is equilibrium?

- Calculate an empirical formula for a compound if mass percentage of its constituents is given.

- Know how to deal with grams and moles if a reaction if given. E.g., you have 1.5 moles of a reactant, how many grams of a product can you get?

- Know how to calculate percentages, especially, a yield of chemical reaction.

- What is a catalyst?

 

The final test 10 May 2005

    It is comprehensive and it will cover chapters 1-10. Chapters 1-7 were already covered in the previous tests, so you should use the previous study guides. Material for  8-10 is here:

1.    Some problems shown in class are specifically pointed out as "being on the test."     Those problems, indeed, will be on the test. You have them in your class notes.

2.   A number of problems related to the ideal gas law, pV=nRT. For example: The temperature of a 500 ml sample of gas increases from 150 to 350 oC. What is the final volume of the sample of the gas, if the pressure in the container is kept constant?

3.  Dilution problems. There are various kinds, one example, a practice problem: If you are diluting  20.0 ml of a 5.5 mol/l HBr solution to 0.50 mol/l HBr, how many milliliters of water will you need to add?

4. Calculations of pH of a buffer. For example:

Nitrous acid has a Ka of 4.5x10-5. What is the pH of a buffer solution containing 0.15 mol/l HNO2 and 0.15 mol/l NO2-?

5. Know what is a buffer - what does it do, how to prepare it, etc.

6. When you know the formula of the compound dissolve, predict whether the solution will be acidic, basic or neutral. For example, solution of sodium carbonate will be basic, solution of ammonium nitrate will be acidic (see p. 346), understand and know Table 10.9.

7. Know what is pH, how to do calculations with pH. How does the logarithmic scale of pH related to hydronium concentration.

8. Know what conjugate acid and base are. For example - Write a conjugate acid for the hydroxide ion.

9.    Know what strong and weak electrolytes are.

10.  Various molarity concentrations. E. g., what is the molarity of solution that has 25.4 g of NaCl dissolved in 350 ml of solution?

11. Know osmosis.

12. Know the precipitation table and know how to use it -- predict which compound will be soluble or insoluble.

13. Know the impact of "like dissolves like" concept

14. Know the impact of the LeChatellier's principle.

15. Know the impact of hydrogen bonds on properties of water.

16. What is STP for an ideal gas, what is the volume of 1 mole of an ideal gas of STP, how large would be a cube that has the volume of 1 mole of gas at STP?

17. Know how exothermic and endothermic process during dissolution affect the solubility vs. temperature dependence.