AP Chemistry Summer Assignment 2010-2011
Greetings New AP Chemistry Students!
It is that time! Because this is a test-driven course, and because the AP Chemistry test will be administered much earlier this
year (note: it is the first ap test on the Monday morning we return from spring break), we will be picking up from where we
left off last year in honors chemistry. 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 your answers as you progress; work toward these
answers. The answers to sections 5 & 6 are given on the last page of this assignment.
Have this assignment ready for submission on your first day back to school—August 31. I will check your work for proper
labels, sig figs, and canceling, but you will be able to check your answers as you go along. Your first test will be the second
day of school and will cover the information included in this assignment. If a problem arises with one of the websites, I have
included alternative references.
Enjoy the rest of your summer! I look forward to seeing you all again this fall!
Mrs. Zebris
Rocky River High School/AP Chemistry Instructor
Topics covered on first test:
 Naming compounds & writing formulas
 Mass-Mole-Particle Dimensional Analysis
 Percent Composition by Mass of a Compound
 Calculating Empirical & Molecular Formulas
 Balancing Equations
 Stoichiometry (Mass-Mole, Limiting Reactants, Percent Yield, Theoretical Yield, Actual Yield)
Step-by-step review of topics: http://www.shodor.org/UNChem/basic/stoic/
1. Memorize these polyatomic ions and special cation charges. Make flashcards if necessary! For practice, go to
http://wps.prenhall.com/wps/media/objects/4974/5093961/emedia/ch03/PolyatomicIons.html
+
Ammonium
NH4
Acetate
C2H3O2
Nitrate
NO3
Nitrite
NO2
Hydroxide
OH
Hypochlorite
ClO
Chlorite
ClO2
Carbonate
Peroxide
Sulfate
Sulfite
Thiosulfate
Chromate
Dichromate
2-
CO3
2O2
2SO4
2SO3
2S2O3
2CrO4
2Cr2O7
-
Chlorate
ClO3
Perchlorate
ClO4
Permanganate MnO4
Bicarbonate
HCO3
Cyanate
CN
Thiocyanate
SCN
2+
3+
Cobalt
Co Co
3-
Phosphate
PO4
3Arsenate
AsO4
3Borate
BO3
2+
3+
iron
Fe Fe
+
2+
copper
Cu Cu
2+
4+
tin
Sn Sn
2+
4+
lead
Pb Pb
2. Be able to name Ionic and Covalent compounds (using the criss-cross method and the prefix method) Practice at:
http://wps.prenhall.com/wps/media/objects/4974/5093961/emedia/ch03/IonicCompounds.html
http://wps.prenhall.com/wps/media/objects/4974/5093961/emedia/ch03/AAEDKKE0.html
3. Mole/Mass/Particles Conversions Show your work formally for the following on your own paper. Round all molar masses
from the periodic table to the hundredths place. Be sure to watch your units and sig figs!
a)
b)
c)
d)
e)
2.4 mol H2O = ____ particles of H2O
-3
9.98 x 10 mol carbon monoxide = ____ grams
2.35 mol disulfur trinitride = ______ grams
-3
1.378 x 10 grams Argon gas = ______ Liters
3
2.1 x 10 liters oxygen = ____ particles
1|Page
20
f) 5.9 x 10 atoms of O2 = ____ mol
g) 0.25 mol silver acetate = _______ particles
h) 3.80 Kg of copper (II) phosphate =______ particle
30
i) 5.989 x 10 molecules sulfuric acid = ________ g
j) 50.0 g sodium hydrogen carbonate = ____ mol
4. Percent Composition
Show your work formally. Go to the link to review and to check your answers.
http://wps.prenhall.com/wps/media/objects/4974/5093961/emedia/ch03/MWweightPercent/j2bl/MWweightPercent.html
NH3
CH4
Pb(NO3)2
NO
NO2
N2O
5. Empirical & Molecular Formulas
Review how to calculate these at:
http://wps.prenhall.com/wps/media/objects/4974/5093961/emedia/ch03/EmpFormulaDetermin.html or
http://www.shodor.org/UNChem/basic/stoic/ Show your work formally on your own paper:
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?
6. Stoichiometry (Limiting Reactant, Excess Reactant, % yield, theoretical yield, actual yield)
a. Define each of the terms on your paper.
b. Given the following reaction: __GeH4 + __GeF4 __ GeF3H
how many moles of GeF4 are needed?
In order to product 8.00 mol of GeF3H with this reaction,
c. Given the following reaction: __ AgNO3 + __AlCl3__Al(NO3)3 +__ AgCl
produced by 2.75 mol aluminum chloride?
How many moles of silver chloride can be
d. Write the balanced reaction for the complete combustion of propane (C3H8)
The reaction of 2.5 mol of O2 will produce how many mol of H2O?
e. Under appropriate conditions, nitrogen and hydrogen combine to yield ammonia.
___Mg + ___N2 ___Mg3N2
i. A 7.1 g sample of N2 requires ____ g of Mg for a complete reaction?
ii. 100.0 g of N2 gas will theoretically yield how many grams of Mg3N2?
iii. If the actual yield from an experiment is only 300.0 g, what is the percent yield of this reaction?
iv. 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?
f. Balance first: __LiOH + __KCl __ LiCl + __KOH
i. If you begin this with 20.00 grams of lithium hydroxide, what is your theoretical yield of LiCl?
ii. If you actually produced 6.00 grams of lithium chloride, what is your percent yield?
g. Balance first: __C3H8 + __O2 __CO2 + __ H2O
i. If 5 grams of C3H8 is used what is the theoretical yield of water?
ii. If you produced a percent yield of 75%, how many grams of water did you make?
h. Aluminum reacts with chlorine as described: ___Al s + ___Cl2 g___AlCl3 s
2|Page
i. If you begin with 40.0 g Al and 40.0 g of chlorine gas, which is the limiting reactant?
ii. How many grams of aluminum chloride can be produced from this reaction?
iii. Calculate the mass of excess reactant that remains after the reaction is complete.
iv. If you needed to make 100.0 g of AlCl3, how many liters of Cl2 do you need?
Answers:
5a Na2SO3
b. Emp formula: C9H17O Molecular formula: C45H85O5
c. K2Cr2O7
d. C12H22N2O2 (EF and MF)
e Mg3N2
f. EF: C4H6O MF: C8H12O2
6b 10.7 mol
c 8.25 mol
d 2 mol
ei 18 g
Ii 360.4 g
Iii 83.2%
Iv 34.6 g will form from LR
fi 35.40 g
ii. 16.9%
gi, 8 g
ii. 6 g
hi.
ii.
iii.
iv.
3|Page
Cl2
50.1 g
29.80 g
25.20 L