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AP CHEMISTRY
SUMMER ASSIGNMENT
2015
MR. SOLTMANN
Welcome to Advanced Placement Chemistry.
AP Chem is a fast paced course, with higher orders of thinking. You will be expected to pull on
previous knowledge constantly to solve problems. Along the way, we will see some fun demonstrations
and perform some intense chemical experiments.
The attached summer assignment is a recommended assignment, but will not be collected. I will field
questions via email all summer at [email protected]. To aid you, you should read (and
cover) the Brown and LeMay Chemistry the Central Science book. The assignment focuses on all of
chapters 1,2,3 and chapter 10. Also, at the end of the assignment are two important sheets. The first is a
sheet of common ions for reference, you are expected to know these ions for the AP test and thus for this
course. After this page is a sheet of elements; you are expected to know the symbols and names of those
elements.
The packet is important, but more important is that you understand the material on this. As such you
will be tested on these assignments in one big test. The test will occur on the first non-shortened 88
minute block (based on the new schedule); tentatively 9/9/15 or 9/10/15. Of course, these are tentative
dates.
Despite what you are thinking as you look this over, I am not trying to kill you. I am trying to ensure
that you remember enough of your honors Chemistry course so that we can achieve the pace we need to
make the AP Chemistry exam a success for everyone.
Name ___________________________________ AP Chemistry Summer Assignment 2014
SIGNIFICANT FIGURES APPLY TO ALL NUMERIC ANSWERS. ALL NECESSARY WORK
MUST BE SHOWN FOR QUANTITATIVE PROBLEMS.
Unit 1 – Introduction to Matter and Measurement
1) Indicate whether the following substances are heterogeneous Mixtures, or homogeneous Solutions,
Compounds, or Elements.
Seawater ____
sand ____
platinum ____
orange juice ____
Italian salad dressing ____
Epsom salt (magnesium sulfate) ____
methanone _____
Brass alloy ____
europium _____
coca-cola _____
ammonia ____
2) The best way to separate the components of a mixture would be:
a) distillation
b) filtration
c) both distillation and filtration
d) something else
3) The best way to separate the solute from the solvent of a solution would be:
a) distillation
b) filtration
c) both distillation and filtration
d) something else
4) Name these elements (try to do this without a book/periodic table):
Au ________________
Mo ____________________
Sn _____________________
Pb ________________
Sb _____________________
Na _____________________
Fe ________________
K_______________________
W ______________________
5) Write the chemical symbols for these elements (try to do this without a book/periodic table):
fluorine _______
arsenic _______
plutonium _____
krypton _______
mercury _______
silver ______
copper ______
manganese ______
6) Indicate whether the following are Chemical changes or Physical changes.
corrosion of aluminum metal _____
melting of ice _____
pulverizing an aspirin _____
digesting a candy bar _____
7) Write the following without scientific notation, using only metric prefixes.
6.5 x 10-6 m = __________________
6.34 x 10-4 L = ____________________
2.5 x 10-3 L = __________________
4.23 x 10-9 m3 = ___________________
12.5 x 10-8 kg = ___________________
3.5 x 10-11 s = _____________________
8) Convert the following:
25.5 mg = __________________ g
4.0 x 10-10 m = __________________ nm
.575 mm = _________________ m
14.7 km = ______________________ cm
9) A liquid has a mass of 39.73 g and a volume of 25.0 ml. What is its density in g/cm3?
Answer _________________________
10) The density of platinum is 21.45 g/cm at 25 C. What is the mass of 75.00 ml of platinum at this
temperature?
3
o
Answer _________________________
11) The density of titanium is 4.51 g/cm at 25 C. What is the volume of 175 g of titanium at this
temperature?
3
o
Answer _________________________
12) Convert the following temperatures:
62 oF = _______ oC
216.7 oC = __________ oF
233 oC = __________ K
315 K = _______ oF
12.5 K = __________ oC
2500 oF = ___________ K
13) Perform the following conversions indicated. SHOW ALL WORK!
50.0 days = _____________ s
43 miler per hour = _______________ meters per second
13.8 g/cm3 = ______________ kg/m3
22.50 gal/min = _____________ liters/second
14) A certain silver dollar as a mass of 26.73 g and is 90.0% silver. If the value of silver is $5.30 per
troy ounce, what is the current value of a dozen silver dollars?
Answer _________________________
15) A sample of ascorbic acid contains 1.50 grams of carbon and 2.00 grams of oxygen. Another
sample of ascorbic acid contains 6.35 grams of carbon. How many grams of oxygen would this sample
have?
Answer _________________________
16) The density of silver is 10.5 g/cm and the density of aluminum is 2.70 g/cm3. Two spheres of equal
mass are constructed, one of silver and one of aluminum. The silver sphere has a radius of 12.0 cm.
What is the radius of the aluminum sphere? Vsphere = 4/3r3
3
Answer _________________________
17) Complete the following math using appropriate significant figures:
12.34 cm x 8.4 cm x 13.1 cm = ______________________
187.245 ml + 43.1 ml + 391.55 ml = _____________________
(37 + 273.15 K) * 321 J/K = _______________________
18) What is the difference between metric units and SI units?
The test for unit one will include naming and writing symbols for elements.
Unit 2 –Atoms, Molecules, and Ions
19) The radius of a krypton atom is about 1.9 Angstroms.
a) How many krypton atoms would have to be lined up to span 1.0 mm? _____________
b) What is the volume of this spherical atom (in cm3)? ___________
20) Complete the chart below: (only mass #s are given, you must look up the atomic #s)
# of protons # of neutrons # of electrons
28
Si
60
Ni
195
Pt
238
U
21) Complete the chart for neutral atoms:
121
Symbol
Sb
Protons
38
94
Neutrons
50 108
Electrons
74 57
Mass #
139 239
22) From the data below, determine the average atomic mass of the given element.
Isotope (Mass #)
203.97302
204.97444
206.97587
Abundance by %
1.40000%
24.10000%
22.10000%
207.97663
52.40000%
23) Indicate the formal family name to which each of the indicated elements belong:
iodine _______________________
potassium _____________________
argon _______________________
strontium ______________________
tellurium _______________________
24) Of the elements listed in question 21: (list them by their chemical symbols)
a) which elements are metals? _____________________________________
b) which elements are nonmetals? ___________________________________
c) which elements are metalloids? ___________________________________
25) A compound has two boron atoms and six hydrogen atoms.
a) what is its empirical formula? ___________________
b) what is its molecular formula? ___________________
26) How many hydrogen atoms are present in one molecule of:
a) ethanol? _______
b) calcium acetate? ________
c) ammonium phosphate? _______
27) Write the empirical formula for:
a) Al2Br6 _____________
b) C8H10 _____________
d) P4O10 ______________
c) C4H8O2 _______________
e) C6H4Cl2 _____________ f) B3N3H6 _______________
28) Based on its location in the periodic table, what is the most stable ion for:
a) Al _______
b) Ca _______
c) S ________
d) I _________
e) Cs ______
29) Based on their locations in the periodic table, write the formula of the ionic compounds formed
between:
a) gallium and fluorine ____________
b) lithium and iodine ____________
c) aluminum and oxygen ____________
d) magnesium and nitrogen ___________
30) Name the following ionic compounds:
a) AlF3 _______________________________
b) Fe(OH)2 ________________________________
c) Cu(NO3)2 ____________________________
d) Ba(ClO4)2 ______________________________
e) Li3PO4 _______________________________
f) Hg2S ___________________________________
g) Ca(C2H3O2)2 __________________________
h) Cr2(CO3)3 _______________________________
i) K2Cr2O7 _______________________________ j) NH4MnO4 _______________________________
31) Write the chemical formulas for the following ionic compounds
a) potassium chromate ___________________
b) magnesium chlorate __________________
c) iron (III) carbonate ___________________
d) tin (IV) sulfate ____________________
e) lead (IV) arsenate ____________________
f) antimony (V) perchlorate ________________
g) silver sulfide _____________________
h) barium nitrite _____________________
i) manganese (II) oxalate _________________
j) aluminum cyanide ___________________
32) Name the following acids:
a) HBr __________________________
b) HClO __________________________
c) H2CO3 _________________________
d) HCN ___________________________
e) H3AsO4 __________________________
f) HI ______________________________
33) Write the formulas for the following acids:
a) hydrofluoric _______________________
b) nitrous _________________________
c) bromic ___________________________
d) oxalic _________________________
e) phosphous ________________________
f) hydrochloric ______________________
34) Write the formulas of the following binary covalent compounds:
a) tetraphosphorus decoxide ______________
b) dinitrogen tetroxide __________________
c) sulfur trioxide _____________________
d) trinitrogen monoxide _________________
35) Write the names of the following binary covalent compounds:
a) SCl6 _____________________________
b) IBr5 _______________________________
c) XeF4 _____________________________
d) NO _______________________________
For the test on unit two, you will have to know your common
ions. No charts will be provided.
Unit 3 – Calculations with Chemical Formulas and Equations
36) Balance the following equations
a) ____ P2O5 (s) + ____ H2O (l)  ____ H3PO4 (aq)
b) ____ CH4 (g) + ____ Cl2 (g)  ____ CCl4 (l) + ____ HCl (g)
c) ____ Al4C3 (s) + ____ H2O (l)  ____ Al(OH)3 (s) + ____ CH4 (g)
d) ____ C4H10O (l) + ____ O2  ____ CO2 + ____ H2O
e) ____ Fe(OH)3 (s) + ____ H2SO4 (aq) ____ Fe2(SO4)3 (aq) + ____ H2O (l)
37) Write out the complete balanced equation for the reaction indicated. INCLUDE PHASES.
a) Solid zinc metal reacts with sulfuric acid to produce hydrogen gas and a solution of zinc sulfate.
b) When liquid phosphorus trichloride is added to water it reacts to form phosphous acid
(sometimes called phosphorous acid) and hydrochloric acid.
c) When gaseous phosphorus trihydride is combusted in air, water is formed as well as an insoluble
solid tetraphosphorus decoxide.
d) When solid mercury (II) nitrate is heated, it decomposes into solid mercury (II) oxide, gaseous
nitrogen dioxide and oxygen.
e) Copper metal reacts with sulfuric acid to form solid copper (II) sulfate, sulfur dioxide gas, and
water.
38) Balance the following reactions, then indicate whether they are synthesis (S), decomposition (D),
single replacement (SR), double replacement (DR), or combustion(C).
a) ___ Mg + ___ AlF3  ___ MgF2 + ___ Al
____
b) ___ Cu(ClO3)2  ___ CuCl2 + ___ O2
____
c) ___ NH3 + ___ O2  ___ NO2 + ___ H2O
____
d) ___ N4O10 + ___ H2O  ___ HNO3
____
e) ___ KI + ___ Fe2S3  ___ K2S + ___ FeI3
____
39) Determine the molar mass of:
a) H2S _____________________
b) NiCO3 ______________________
c) (NH4)3AsO3 _____________________
d) Sb2(S2O3)5 ______________________
40) Calculate the percentage (by mass) of oxygen in:
a) sulfur dioxide ________________
b) ethanoic acid _________________
c) potassium phosphate _________________
d) aluminum nitrate ________________
e) dinitrogen pentoxide _______________
41) Rank the following quantities from the one with the most atoms to the one with the least atoms:
.500 mol of water
23.0 g of sodium
6.02 x 1023 nitrogen molecules
________________
most atoms
__________________
___________________
least atoms
42) Calculate the following quantities
a) the mass, in grams, of 1.73 mol of calcium hydroxide __________________
b) the number of moles of magnesium nitrate in 6.50 grams of the substance ________________
c) the number of molecules in .775 moles of methanol _____________________
d) the number of hydrogen atoms in 1.24 mol butane _____________________
e) the number of electrons in 88.0 grams of carbon dioxide ______________________
43) A sample of glucose, C6H12O6, contains 5.77 x 1020 atoms of carbon.
a) How many atoms of oxygen are present? ___________________
b) What mass, in grams, of glucose does it contain? _________________
44) Determine the empirical formula of a compound that contains:
a) .0130 mol carbon, .0390 mol hydrogen, and .0065 mol oxygen
___________________
b) 11.66 g of iron and 5.01 g of oxygen
____________________
c) 40.0 % carbon, 6.7% hydrogen and 53.3% oxygen
____________________
d) 53.3% potassium, 14.6% phosphorus and 30.1% oxygen
____________________
e) 62.1% carbon, 5.21% hydrogen, 12.1% nitrogen, 20.7% oxygen
____________________
45) Determine the empirical and molecular formula of a compound that contains:
a) 49.5 % carbon, 5.15% hydrogen, 28.9% nitrogen and 16.5 % oxygen with a molar mass of 195
g/mol.
Empirical formula = ___________________
Molecular Formula = _______________________
b) 57.14 % carbon, 6.16% hydrogen, 9.52% nitrogen, and 27.18 % oxygen with a molar mass of
276 g/mol.
Empirical formula = ___________________
Molecular Formula = _______________________
c) 59.0 % carbon, 7.1% hydrogen, 7.7% nitrogen, and 26.2 % oxygen with a molar mass of 180
g/mol.
Empirical formula = ___________________
Molecular Formula = _______________________
46) Given the reaction: ___ Na2SiO3 + ___ HF  ____ H2SiF6 + ____ NaF + _____ H2O
a) how many moles of HF are needed to react with .300 mol of Na2SiO3? _______________________
b) How many grams of NaF form when .500 mol of HF are completely consumed? _________________
c) How many grams of water form if 125 g of NaF formed? ______________________
47) Given the reaction: ___ C6H12O6  ___ C2H5OH + ___ CO2
a) How many moles of carbon dioxide are produced when .400 mol of glucose (C6H12O6) reacts
completely? _____________________________
b) How many grams of glucose are needed to form 7.50 g of ethanol? _____________________
c) how many grams of carbon dioxide form when 7.50 g of ethanol are produced? _________________
48) Given the reaction: ____ C6H14 + ____ O2  ____ CO2 + ____ H2O
a) 42.0 grams of hexane are combined with 80.0 of oxygen at STP. What is the limiting
reagent(reactant) ? ________________
b) what mass of carbon dioxide is produced? _________________
c) what mass of water vapor is produced? _________________
d) What mass of the excess reagent is left over? ________________
e) If the actual yield of water vapor is 20.6 grams, then what is the percent yield? _____________
49) A simple hydrocarbon (no oxygen) is combusted completely, producing 6.28 grams of carbon
dioxide and 2.57 grams of water vapor. What is the empirical formula of this hydrocarbon?
50) 2.78 grams of an oxy-hydrocarbon is combusted completely, producing 6.32 grams of carbon
dioxide and 2.58 grams of water vapor. If its molar mass is about 116 g/mol, what is its molecular
formula?
51) One student measures the volume of a gas at 216 mL when the pressure was 1.25 atm. Another
student comes in and lowers the pressure to 87900 Pa. If the temperature remained the same, what is the
new volume of the same sample of gas?
52) On a hot day, 104 oF, the volume of gas in a tire is 3.46 liters. What is the volume of the gas on a
cold winter day, -13.0 oF, if the pressure and amount of gas have not changed?
53) On a warm day, .0500 moles of neon would have a volume of about 1.27 liters. On the same day,
given the same temperature and pressure, what would the volume be for 1.33 moles of neon?
54) A fixed metal tank has a volume of 52.4 liters. The tank is filled on a cold day (0.00 oC) with
hydrogen gas under a pressure of 2.00 atm. The tank exploded on a hot day (100.0 oC). Assuming the
volume of the tank didn’t change (until it exploded) what was the pressure in the tank just before it
exploded?
55) A latex balloon was filled with exactly 1.000 liters of helium when the temperature was 32.50 oC
and the air pressure was 1.17 atm. Later on a storm comes in, dropping the air pressure to 720. Torr and
dropping the temperature to 25.80 oC. What is the new volume of the balloon?
56) A .275 mole sample of helium is kept under a pressure of 2.00 atm and at a temperature of 75 oC.
What is the volume of the gas?
57) A 6.125 gram sample of neon is used in a sign. The neon is kept under a pressure of 75,330 Pa.
When the temperature is 27 oC, what is the volume of the gas?
58) What is the density of fluorine gas when the pressure is 125, 000 Pa and the temperature is 95 oF?
59) A 2.0 L tank of nitrogen gas at 1.0 atm and 25 oC is connected to a 3.0 L tank of oxygen at 2.0 atm
and 25 oC. When the valve is opened, allowing the gases to mix, but not react:
a) What is the new pressure of the nitrogen?
b) what is the new pressure of the oxygen?
c) What is the total pressure of the system?
d) What is the mole fraction of nitrogen in this system?
60) A 10 liter tank contains oxygen at 1.00 atm and 298 K. A 12 liter tank contains helium at .75 atm
and 298 K. The valve that connects the two tanks is opened, allowing the gases to mix, but obviously
they do not react. What is the mole fraction of the helium in the system after mixing has occurred?
61) What are the densities of CO2, N2O, and Cl2 at STP?
62) A neon sign is made from cylindrical glass tubing with a diameter of 4.5 cm and whose length is 5.3
m. If the sign contains neon at 2.03 Torr and 35 oC, what mass of neon is in the tube? Remember that 1
liter is the same as 1 dm3.
63) A gas with an empirical formula of CH3 has a density of 1.218 g/L at 27oC and 1 atm. What is its
molecular formula?
64) A mixture containing 3.15 g each of CH4, C2H4 and C4H10 is contained in a 2.00 liter flask at a
temperature of 64 oC.
a) Calculate the partial pressure of each gas.
b) Calculate the total pressure of the mixture.
65) A mixture of gases contains .75 mol N2, .30 mol O2, and .15 mol CO2. If the total pressure of the
mixture is 1.56 atm, what is the partial pressure of each component?
66) 6.05 g of O2, 4.92 g of N2, and 1.32 g of H2 are mixed in a container.
a) what are the mole fractions of each component?
b) What is the partial pressure of each component if it is held in a 12.40 liter vessel at 15 oC?
67) Zinc metal is placed in sulfuric acid. If 159 ml of wet H2 gas is collected over water at 24 oC and the
manometric pressure of 738 Torr, how many grams of zinc have been consumed? Hint -You will need
to look up a water vapor table.
68) Acetylene gas, C2H2 , can be prepared by the reaction:
CaC2 (s) + 2 H2O (l)  Ca(OH)2 (s) + C2H2 (g)
Calculate the volume of C2H2 that is collected over water at 21 oC by reaction of 3.26 g CaC2 if the
manometer reads 748 Torr? Hint -You will need to look up a water vapor table.
69) Given the reaction: ___ C3H8 (g) + _ O2 (g)  ___ CO2 (g) + ___ H2O (g)
a) If 2.50 L of propane reacts completely with excess oxygen, what volume of carbon dioxide will be
produced at a constant temperature of 86.0 oF and a constant pressure of 1.75 atm?
b) If 4.44 L of propane are mixed with 11.1 L of oxygen at constant STP ,
i) what is the limiting reagent? ______________________
ii) what volume of the excess reagent is left after the reaction?
______________________
iii) what mass of water vapor is produced? ______________________
c) If 15.0 grams of propane reacts completely, what volume of carbon dioxide is produced? Assume
constant STP.
70) Calculate and compare the average kinetic energy of H2 and CO2 at 300 K.
71) Calculate and compare the rms speeds of H2 and CO2 at 300 K.
72) List the following gases in order of increasing molecular speed: CO2, N2O, HF, F2, H2.
73) Vessel A contains CO (g) at STP. Vessel B contains SO2 (g) at 20 oC & .50 atm.
Assume that the two vessels have the same volume!
a) Which vessel contains more molecules?
____
b) Which vessel contains more mass?
____
c) In which vessel will the molecules have a higher average kinetic energy?
____
d) In which vessel will the molecules have the higher rms speeds?
____
74) Under one set of conditions, oxygen effused at 2.00 liters/second. Under the same conditions, at
what rate should hydrogen effuse?
75) A gas is found to diffuse at a rate 4x that of oxygen. What is the molar mass of this gas?
76) A gas of unknown molar mass was allowed to effuse through an opening under constant pressure
conditions. It required 105 s for 1.0 liter of the gas to effuse. Under identical conditions it required 31 s
for 1.0 liter of oxygen to effuse. Calculate the molar mass of the unknown gas.
77) Circle the gas in each pair that is more likely to deviate from the ideal gas law:
a) He at STP or C4H20 at STP
b) 1 g of He in a 5 liter tank or 1 g of He in a 2 liter tank
c) 1 g of He at 100 K or 1 g of He at 400 K
d) 1 g of He under 1 atm or 1 g of He under 5 atm
e) N2O at STP or CO2 at STP
78) A gas is determined to have an empirical formula of CH. If the gas diffuses 2.08 times slower than
water vapor under the same conditions, what is the molecular formula of the gas?
79) Two porous containers are filled with hydrogen and neon respectively. Under identical conditions,
exactly 1/2 of the hydrogen escapes in 4 hours. How long will it take for exactly 2/3 of the neon to
escape?
+1
hydrogen, H+
cesium,Cs+
copper (I), Cu+
lithium, Li+
potassium, K+
silver, Ag+
sodium, Na+
Common Monatomic ions
+2
+3
2+
barium, Ba
aluminum, Al3+
2+
calcium, Ca
chromium(III), Cr3+
cobalt(II) Co2+
iron(III), Fe3+
2+
copper(II) , Cu
iron(II) , Fe2+
lead(II), Pb2+
magnesium, Mg2+
manganese(II), Mn2+
mercury(II), Hg2+
nickel(II), Ni2+
strontium, Sr2+
tin(II), Sn2+
Zinc, Zn2+
-1
chloride, Clfluoride, Fbromide, Briodide, Ihydride, H-
-2
oxide, O2sulfide, S2-
+1
ammonium, NH4+
-1
acetate, C2H3O2Acetate, CH3COObicarbonate, HCO3Bisulfate, HSO4bromate, BrO3bromite, BrO2chlorate, ClO3chlorite, ClO2cyanide, CNhydroxide, OHHypobromite, BrOhypochlorite, ClOhypoiodite, IOiodate, IO3Iodite, IO2nitrate, NO3nitrite, NO2permanganate, MnO4perchlorate, ClO4-
+4
lead(IV), Pb4+
tin(IV), Sn4+
-3
nitride, N3phosphide, P3-
Common Polyatomic ions
+2
Mercury(I), Hg22+
-2
carbonate, CO32chromate, CrO42dichromate, Cr2O72oxalate, C2O42peroxide, O22sulfate, SO42sulfite, SO32tartrate, C4H4O62thiosulfate, S2O32-
-1
periodate, IO4Thiocyanate, SCN-
-3
arsenate, AsO43arsenite, AsO33phosphate, PO43phosphite, PO33-
+5
Antimony(V), Sb5+
Elements You Should Know
YOU DO NOT HAVE TO TURN THIS IN. THIS IS JUST TO HELP YOU STUDY!
Al ________________________
H _______________________
Rb ____________________
Sb ________________________
I ________________________
Sc _____________________
Ar ________________________
Ir _______________________
Se _____________________
As ________________________
Fe _______________________
Si _____________________
Ba ________________________
Kr _______________________
Ag _____________________
Be ________________________
Pb _______________________
Na _____________________
Bi _________________________
Li ________________________
Sr _____________________
B _________________________
Mg _______________________
S ______________________
Br _________________________
Mn _______________________
Te _____________________
Cd ________________________
Hg _______________________
Th _____________________
Ca ________________________
Mo _______________________
Sn _____________________
C _________________________
Nd _______________________
Ti _____________________
Cs ________________________
Ne _______________________
W _____________________
Cl _________________________
Ni _______________________
U ______________________
Cr ________________________
N ________________________
V ______________________
Co ________________________
O ________________________
Xe _____________________
Cu ________________________
Pd _______________________
Zn _____________________
F _________________________
P ________________________
Zr _____________________
Fr ________________________
Pt ________________________
Ga _______________________
Pu _______________________
Ge _______________________
K _______________________
Au _______________________
Ra _______________________
He _______________________
Rn _______________________