Download AP Chemistry Summer 2009

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 [email protected] 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
Name_______________________________________
1. Indicate the number of protons, neutrons, and electrons for each symbol.
1)
40
20
Ca
5) Carbon-14
12
6
C
2) 127
3)
6) Uranium-235
7) Uranium-238
53 I
4)
36
17
Cl
8) Xenon-131
2. Memorize these polyatomic ions. Make flashcards if necessary! Go to
http://wps.prenhall.com/wps/media/objects/4974/5093961/emedia/ch03/PolyatomicIons.html and practice.
Ammonium
NH4+
Acetate
C2H3O2Nitrate
NO3Nitrite
NO2Hydroxide
OH Hypochlorite
ClO Chlorite
ClO2-
Carbonate
Peroxide
Sulfate
Sulfite
Thiosulfate
Chromate
Dichromate
CO3 2O2 2SO4 2SO3 2S2O3 2CrO4 2Cr2O7 2-
Chlorate
ClO3 Perchlorate
ClO4 Permanganate MnO4Bicarbonate
HCO3 Cyanate
CNThiocyanate
SCN 2+
Cobalt
Co Co3+
Phosphate
PO4 3Arsenate
AsO4 3Borate
BO3 3iron
Fe2+ Fe3+
copper
Cu+ Cu2+
tin
Sn2+ Sn4+
lead
Pb2+ Pb4+
3. Inorganic Nomenclature Review (Ionic and Covalent compounds)
Write the formulas/names for the following ionic compounds. Then go to
http://wps.prenhall.com/wps/media/objects/4974/5093961/emedia/ch03/IonicCompounds.html to check your answers
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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 http://wps.prenhall.com/wps/media/objects/4974/5093961/emedia/ch03/AAEDKKE0.html 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 1020 atoms of O2 = ____ mol
9.98 x 10-3 mol carbon monoxide = ____ grams
0.25 mol silver acetate = _______ particles
2.35 mol disulfur trinitride = ______ grams
3.80 Kg of copper (II) phosphate =______ particles
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1.378 x 10-3 grams Ar gas = ______ Liters
5.989 x 1030 molecules sulfuric acid = ________ grams
2.1 x 103 liters oxygen = ____ particles
50.0 g sodium hydrogen carbonate = ____ mol
5. Percent Composition
Show your work formally for the formulas below. Go to
http://wps.prenhall.com/wps/media/objects/4974/5093961/emedia/ch03/MWweightPercent/j2bl/MWweightPercent.html
to review and to check your answers. Other sites for more review include http://www.shodor.org/UNChem/basic/stoic/ .
NH3
CH4
Pb(NO3)2
6. Empirical & Molecular Formulas For review go to
http://wps.prenhall.com/wps/media/objects/4974/5093961/emedia/ch03/EmpFormulaDetermin.html . 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.
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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.
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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
packet.
1. Stoichiometry refers to _____________________________________.
_____________2. Given the following reaction: GeH4 + 3GeF4 4 GeF3H
this reaction, how many moles of GeF4 are needed?
In order to product 8.00 mol of GeF3H with
_____________3. Given the following reaction: AgNO3 + AlCl3Al(NO3)3 + AgCl
be produced by 2.75 mol aluminum chloride?
How many moles of silver chloride can
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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