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ap chemistry summer 2009 assignment by ashrafp


									AP Chemistry Summer 2009-2010 Assignment
Posted June 2009

Thinking about next year already? Yes, we are! Because this is a test-driven course, and because this test is administered in
early May, you need to come already warmed up and ready to go on day one in August! This summer assignment serves as a
review of a select few basic skills as well as a list of some items that you need to have ready at your fingertips. (Note: former
students have indicated this served as a tremendous help!)

Download this assignment so that you may click on the hyperlinks provided. Follow the website links and instructions below.
You will get immediate feedback on some of your answers as you progress. Setups, labels, sig figs, canceling all count! Have
this ready for submission on your first day back to school. Your first test will be the second day of school and will cover the
information included in this assignment. If you need a refresher you should consult last year’s notes and/or check the
website links. If a problem arises this summer with one of the websites, I have included many different websites as
alternative references.

Please send me a confirmation email ASAP to indicating that (1) you have received this assignment,
and (2) you can access these websites. If you have any questions, please email me before August 12.

Enjoy your summer! I look forward to seeing you all again this fall!

Mrs. Zebris
Rocky River High School/AP Chemistry Instructor


1. Indicate the number of protons, neutrons, and electrons for each symbol.
              40                                                               12                                     36
              20 Ca                 2) 127
                                        53 I
                                                                                6 C                             4)     Cl

         5) Carbon-14               6) Uranium-235                       7) Uranium-238                         8) Xenon-131

2. Memorize these polyatomic ions. Make flashcards if necessary! Go to and practice.
                            +                              2-                          -                        3-
       Ammonium        NH4          Carbonate         CO3       Chlorate       ClO3         Phosphate      PO4
                           -                              2-                        -                           3-
       Acetate      C2H3O2          Peroxide           O2       Perchlorate    ClO4         Arsenate      AsO4
                           -                               2-                           -                       3-
       Nitrate        NO3           Sulfate           SO4       Permanganate MnO4           Borate          BO3
                           -                               2-                         -                    2+    3+
       Nitrite        NO2           Sulfite           SO3       Bicarbonate   HCO3          iron        Fe Fe
                           -                               2-                       -                      +    2+
       Hydroxide       OH           Thiosulfate      S2O3       Cyanate          CN         copper     Cu Cu
                            -                             2-                          -                   2+    4+
       Hypochlorite    ClO          Chromate         CrO4       Thiocyanate     SCN         tin        Sn Sn
                           -                              2-                  2+    3+                   2+    4+
       Chlorite       ClO2          Dichromate      Cr2O7       Cobalt      Co Co           lead      Pb Pb

3. Inorganic Nomenclature Review (Ionic and Covalent compounds)
Write the formulas/names for the following ionic compounds. Then go to to check your answers

        Barium hydroxide              _____________                 NH4OH            __________________________

        Calcium sulfide               _____________                 NaOH             __________________________

        Silver chloride               _____________                 AgNO3            __________________________

        Iron (II) nitrate             _____________                 FeS              __________________________

        Lead (II) sulfate             _____________                 LiClO3           __________________________

        Aluminum hydroxide            _____________                 FeCl3            __________________________

        Ammonium phosphate            _____________                 Na2S             __________________________

        Sodium perchlorate            _____________                 Na2SO4           __________________________

        Calcium carbonate             _____________                 Pb(NO3)2         __________________________

        Sodium carbonate              _____________                 LiOH             __________________________

Go to and write the name and
formulas for 10 items.

        1.__________________________________________                6. .__________________________________________

        2. .__________________________________________              7. .__________________________________________

        3. .__________________________________________              8. .__________________________________________

        4. _________________________________________                9..__________________________________________

        5.__________________________________________                10. _________________________________________

4. Mole/Mass/Particles Conversions Show your factor-labeling work formally for the following. Round all molar masses
from the periodic table to the hundredths place. Be sure to watch your units and sig figs!

2.4 mol H2O = ____ particles of H2O                                 5.9 x 10 atoms of O2 = ____ mol

9.98 x 10 mol carbon monoxide = ____ grams                          0.25 mol silver acetate = _______ particles

2.35 mol disulfur trinitride = ______ grams                         3.80 Kg of copper (II) phosphate =______ particles

            -3                                                                     30
1.378 x 10 grams Ar gas = ______ Liters                                  5.989 x 10 molecules sulfuric acid = ________ grams

2.1 x 10 liters oxygen = ____ particles                                  50.0 g sodium hydrogen carbonate = ____ mol

5. Percent Composition      Show your work formally for the formulas below. Go to
to review and to check your answers. Other sites for more review include .

           NH3                                 CH4                                        Pb(NO3)2

6. Empirical & Molecular Formulas For review go to . Also check out the
hint cards. Then show your work to calculate the formulas.

           A. A 100. gram sample of compound of sodium contains 36.5 grams of sodium, 25.4 grams of sulfur, and 38.1 grams
           of oxygen. What is the empirical formula for the compound?

           B. Fat makes up a major portion of all soaps. A fat used in many soaps is 76.5% carbon, 12.2% hydrogen, and 11.3%
           oxygen. What is its empirical formula?

                 What is the molecular formula of a fat with a molecular mass of 705 g/mol?

           C. A sample of a substance is determined to be composed of 0.89 g of potassium, 1.18 g of chromium, and 1.27 g
           of oxygen. Calculate the empirical formula.

     D. Strychnine, a deadly poison, has a molecular mass of 334 g/mol and a percentage composition of 75.42% carbon,
     6.63% hydrogen, 8.38% nitrogen, and the balance oxygen. What is the molecular formula of strychnine? (Hint:
     DO NOT round up the number found for carbon in the empirical formula.)

     E. A 10. gram sample of a compound contains 7.22 grams of magnesium and 2.78 grams of nitrogen. What is its
     empirical formula?

    F. An organic compound with a molecular mass of 140 g/mol is 68.54% carbon, 8.63% hydrogen, and 22.83% oxygen.
    What is the molecular formula of the compound?

     G. To find the experimental empirical formula of a compound, a student heats a coil of magnesium ribbon (0.25 g)
     in a crucible. Oxygen combines with the magnesium when heated to form magnesium oxide. Data recorded:

            Mass of empty crucible and cover - 20.74g
            Mass of magnesium ribbon - 0.25g
            Mass of crucible, cover, and final product - 21.17g
             What is the empirical formula for magnesium oxide that was the final product? Show EVERY mathematical
             step fully.

     H. What is a hydrate?______________________________________________
     Name the following hydrates:

     CuSO4 * 5H2O ________________                MgSO4 * 7H2O________________         Na2CO3*10H2O_______________

     I. Cerium iodide (CeI3) occurs as a hydrate with the composition 76.3% CeI3 and 23.7% H2O. Calculate the formula of
     this hydrate.

        II. Cobalt (II) nitrate, Co(NO3)2, is used in ceramic glazes. The compound exists as a hydrate that is 37.1% water and
        62.9% cobalt (II) nitrate. What is the formula for this hydrate?

9. Stoichiometry: For a review of the topics below, you can refer to your honors chemistry notes or check the index on the
prior sites in this assignment. Show your work on your own paper for each problem below. Circle your final answer. Then
write your final answer on the line provided on this sheet with sig figs and units. Staple your work to the back of this

1. Stoichiometry refers to _____________________________________.

_____________2. Given the following reaction: GeH4 + 3GeF4 4 GeF3H            In order to product 8.00 mol of GeF3H with
this reaction, how many moles of GeF4 are needed?

_____________3. Given the following reaction: AgNO3 + AlCl3Al(NO3)3 + AgCl          How many moles of silver chloride can
be produced by 2.75 mol aluminum chloride?

4. Write the balanced reaction for the complete combustion of propane (C3H8) _____________________________________
         ______________The reaction of 2.5 mol of O 2 will produce how many mol of H2 0?

5. Under appropriate conditions, nitrogen and hydrogen combine to yield ammonia.           ___Mg + ___N2 ___Mg3N2

        _____________a. A 7.1 g sample of N2 requires ____ g of Mg for a complete reaction?
        _____________b. 100.0 g of N2 gas will theoretically yield how many grams of Mg3N2?
        _____________c. If the actual yield from an experiment is only 300.0 g, what is the percent yield of this reaction?
        _____________d. If 25.0 g of Mg are react with 14.0 g N2, which is the limiting reactant and how many grams of
        Mg3N2 will form?

6. Balance first: __LiOH + __KCl __ LiCl + __KOH

        _____________a. If you begin this with 20.00 grams of lithium hydroxide, what is your theoretical yield of LiCl?
        _____________b. If you actually produced 6.00 grams of lithium chloride, what is your percent yield?

7. Balance first: __C3H8 + __O2 __CO2 + __ H2O

        _____________a. If 5 grams of C3H8 is used what is the theoretical yield of water?

        _____________b. If you produced a percent yield of 75%, how many grams of water did you make?

8. Aluminum reacts with chlorine as described: ___Al s + ___Cl2 g___AlCl3 s

        _____________a. If you begin with 4.599 x 10-3 g Al and 2.332 x 10-2 g of chlorine gas, which is the limiting reactant?
        _____________b. How many grams of aluminum chloride can be produced from this reaction?
        _____________c. Calculate the mass of excess reactant that remains after the reaction is complete.
        _____________d. If you needed to make 100.0 g of AlCl3, how many liters of Cl2 do you need?


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