AP Chemistry Summer Assignment 2014
1. This year’s summer assignment consists of two portions. The first portion is the
attached review packet. The second portion is the online blackboard modules portion.
2. Review Packet – the attached review packet must be completed over the summer and is
due on the first day you have AP Chemistry class when we return in September. 20%
will be taken off for each day it is late. This packet is graded for correctness…not just
completion…so take your time, review the concepts and answer questions correctly. Be
sure to show work when it is specified. Be sure to include proper units in your final
answers.
3. Blackboard Quizzes – Over the summer you must sign onto blackboard and check out
the AP Chemistry blackboard site. This site will contain a discussion board, where you
and the other AP Chemistry students should feel free to discuss summer assignment
questions together, and Blackboard Modules that must be completed before the start of
the school year.
4. Reference Material – The first 3 chapters of the AP Chemistry Textbook will be
available online posted on the blackboard site. Be sure to keep all of your notes from
your first year chemistry course...these will surely help. Feel free to discuss questions
with classmates on the discussion board. Google is always a good tool.
5. Troubleshooting – If you lose your summer assignment packet…there will be a copy
posted on the blackboard site and there is a copy posted on the Centreville High School
website. If you are not enrolled to the blackboard site – Email Mr. Fox,
srfox@fcps.edu and Mrs. Neer, mlneer@fcps.edu . We should have you enrolled in a
couple of days.
6. Due Dates –
a. Blackboard Modules…September 1st by 7:00 pm
b. Review Packet…September 2rd (1st, 3rd, 5th 7th ) September 3th (2nd, 4th, 6th)
AP Chemistry Summer Assignment (2014): This assignment is due they day of your first AP Chemistry
class. This packet will be graded for correctness. Use any source to help you complete this packet. All
concepts are from your first year chemistry course.
I. Units of measurement
Fill in the following chart for the Fundamental SI Units
Physical Quantity
Name of Unit
Abbreviation
Mass
Length
m
s
Temperature
K
Ampere
Pressure
Pa
mol
Luminous Intensity
Fill in the following chart of metric system prefixes
Prefix
Symbol
Mega
Meaning
Exponential
Notation
1,000,000
103
k
hecto
___
da
10
____
1
100
10-1
cm
10-3
micro
nano
0.000001
10-9
Make the following conversions…set up using dimensional analysis (train track method)
1. 500 grams to kilograms
2. 15.25 mL to liters
3. 1.75 meters to nanometers
4. 0.045 mol to mmol
5. 5,000 grams to pounds (1 kg = 2.2 pounds)
Significant Figures (Digits)
Identify the number of significant figures in the following measurements
0.001 m ___________
2.153 X 10-3 L __________
1000 K __________
1,000,000 kg ____________
10. mol _____________
0.0060740 nm ____________
Preform the following calculations, your answers must have the correct # of significant figures
1. 1.50 X 17 =
2. 1.563 + 15.0247 + 17.1 =
3. 19.12346 ÷ 3 =
4. Given the following data table from a lab notebook calculate the density of the metal…answer must be
with correct significant figures.
Measurement
Value
Mass of Metal
10.15 g
Volume of Water
15.15 mL
Volume of Water & Metal
20.16 mL
Mass of Graduated Cylinder
25.18 g
Density of metal _______________
Temperature: In AP Chemistry you are responsible to know about the Kelvin Scale, the Celsius Scale and the
Fahrenheit Scale
Kelvin = Celsius + 273
Celsius = Kelvin – 273
Fahrenheit = Celsius X 9/5 + 32
Celsius = (Fahrenheit – 32) 5/9
1. The boiling point of water is 100̊C, what is this in Kelvin and Fahrenheit?
2. Convert 315 K to Celsius.
3. Convert 500.5 K to Fahrenheit
4. Convert -273 Celsius to Kelvin
II. Atomic Structure
Define the following
1. Atom –
2. Proton –
3. Neutron –
4. Electron –
5. Atomic Number –
6. Mass Number –
7. Average Atomic Mass –
8. Isotope –
9. Ion –
Average atomic mass
1. Magnesium has three natural isotopes. Magnesium – 24, which is 78.99% abundant, Magnesium – 25,
which is 10.00% abundant, and Magnesium – 26, which is 11.01% abundant. Calculate the average
atomic mass of magnesium.
2. Europium has two natural isotopes, Europium – 151 & Europium – 153. The average atomic mass of
Europium is 151.96 amu. Based on this information answer the following.
a. Which isotope is more naturally abundant…justify your answer
b. Calculate the % abundance of both isotopes
Complete the Chart
Name
Symbol
Atomic #
Mass #
# of Protons
# of Electrons
# of Neutrons
Carbon
C
6
12
6
6
6
Zinc ion
Zn2+
17
18
20
65
Chloride
S2Radium - 226
16
32
III. Ionic Compounds (It would be wise to have these memorized)
Common Metal Ions with More than One Ionic Charge (MOM)
Symbol
Stock Name
Classical Name
+
Cu
Copper(I) ion
Cuprous ion
Cu2+
Copper(II) ion
Cupric ion
2+
Fe
Iron(II) ion
Ferrous ion
3+
Fe
Iron (III) ion
Ferric ion
Hg2+
Mercury(II) ion
Mercuric ion
Pb2+
Lead(II) ion
Plumbous ion
Pb4+
Lead(IV) ion
Plumbic ion
2+
Sn
Tin(II) ion
Stannous ion
Sn4+
Tin(IV) ion
Stannic ion
2+
Cr
Chromium(II) ion
Chromous ion
3+
Cr
Chromium(III) ion
Chromic ion
Mn2+
Manganese(II) ion
Manganous ion
Mn3+
Manganese(III) ion
Manganic ion
Co2+
Cobalt(II) ion
Cobaltous ion
Co3+
Cobalt(III) ion
Cobaltic ion
***Note Silver ion and Zinc ion and Cadmium ion are all transition metal ions, but they only have 1
charge (1 oxidation state) so they do NOT need a roman numeral. (Ag1+ and Zn2+ and Cd2+)
Common Polyatomic Ions
Name
Ammonium
Nitrite
Nitrate
Hydrogen Sulfate
Hydroxide
Cyanide
Permanganate
Hydrogen Carbonate
Hypochlorite
Chlorite
Chlorate
Perchlorate
Bromate
Hydronium
Formula
NH4+
NO2NO3HSO4OHCNMnO4HCO3ClOClO2ClO3ClO4BrO3H3O+
Name
Iodate
Periodate
Acetate
Dihydrogen Phosphate
Carbonate
Sulfite
Sulfate
Thiosulfate
Peroxide
Chromate
Dichromate
Hydrogen Phosphate
Phosphite
Phosphate
Formula
IO3IO4C2H3O2H2PO4CO32SO32SO42S2O32O22CrO42Cr2O72HPO42PO33PO43-
The old way to say “hydrogen carbonate” was “bicarbonate”…if you see the prefix “bi” in front of a polyatomic
ion name, then you are adding an H+ to the formula…note that when you add an H+ to the formula the net
charge of the ion goes down one…Carbonate = CO32-….Bicarbonate = HCO31Bisulfate = HSO4-
Write the formula for the following compounds
1. Sodium Sulfate _________________________________________________
2. Iron (III) carbonate ______________________________________________
3. Cesium sulfide _________________________________________________
4. Ammonium dichromate _________________________________________
5. Zinc hydroxide ________________________________________________
6. Vanadium (V) nitrate ___________________________________________
7. Potassium permanganate ________________________________________
8. Aluminum thiosulfate __________________________________________
9. Lead(II) Chloride _____________________________________________
10. Gold(III) phosphite ____________________________________________
11. Sodium acetate _______________________________________________
12. Calcium oxide _______________________________________________
13. Sodium chloride ______________________________________________
14. Magnesium thiosulfate _________________________________________
Write the name for the following compounds
1. FeO ______________________________________________________
2. Pb(SO4)2 _________________________________________________
3. Ca(OH)2 __________________________________________________
4. Na2CO3 __________________________________________________
5. LiHCO3 __________________________________________________
6. (NH4)2CrO4 ______________________________________________
7. Fe2O3 ___________________________________________________
8. AlN
___________________________________________________
9. Cr(NO3)3 _________________________________________________
10. KClO4 ___________________________________________________
11. CrO3 _____________________________________________________
12. Sr(ClO)2 __________________________________________________
IV. Molecular Compounds (Two non-metals)
Prefixes used in naming binary molecular compounds
Prefix Mono- DiTri- Tetra- Penta- Hexa- Hepta- Octa- Nona- DecaNumber
1
2
3
4
5
6
7
8
9
10
The steps to identifying and naming binary molecular compounds
1. First confirm that the compound is a binary molecular compound a compound composed of two
nonmetals.
2. The name must identify the element in the molecule
3. The name must indicate the number each atom of each element in the molecule
4. Name the elements in the order listed in the formula.
5. Use prefixes to indicate the number of each kind of atom.
6. Omit the prefix mono- when the formula contains only one atom of the first element in the name.
7. The suffix of the of the name of the second element is –ide
Name the following
1. CO2 _______________________________
2. PCl3 ________________________________
3. P2O5 ________________________________
4. P4O10 ________________________________
5. SF6
________________________________
6. XeO4 _________________________________
7. S2Cl7 _________________________________
V. Moles/Molarity
Complete each of these calculations, use dimensional analysis…show work
1.
How many grams is 5.30 moles of carbon dioxide?
2. What is the volume of 53.5 grams of oxygen gas at STP? (oxygen is diatomic)
3. How many gold atoms are in a 100.0 gram sample of gold?
4. How much space would 5.6 X 1026 molecules of nitrogen take up at STP?
Molarity (Measurement of concentration of a solution)
1. What is the molarity of a salt water solution that contains 15 moles of NaCl in a 100 liter solution?
2. If 17.0 grams of CaCl2 is dissolved in a 20.0 liter solution. What is the concentration of the calcium
chloride?
3. 25.2 grams of potassium chloride were dissolved in a 80.0 mL solution. What is the molarity of the
potassium chloride solution?
4. How many moles of NaCl would be required to make 25 mL of a 3.5 molar solution?
5. The concentration of CO2 in a can of soda is approximately 0.045 M. If all of the CO2 in a 12 ounce
soda evolves from solution, how many liters would the CO2 gas take up @ STP? (1 oz = 29.6 mL)
6. What mass of Lithium chloride is required to make 500.0 mL of a 0.50 molar solution?
Dilution (M1V1 = M2V2)
1. A student takes 25 mL of a 3.5 molar solution and dilutes it to 100 mL. What is the new concentration
of the solution?
2. What volume of a 12.0 M stock solution is required to make 600.0 mL of a 2.0 M solution?
3. How many milliliters of distilled water should be added to 100.0 mL of a 3.0 M solution to dilute it to
1.5 M?
More Molarity
1. If the concentration of a FeCl3 solution is 2.5 M. What is the concentration of just chloride ions (Cl1-)
2. If the concentration of a 5.0 liter solution of ZnCl2 is 0.010M. How many chloride ions (Cl1-) are in
solution?
3. Given a 2.0 M solution of Aluminum Sulfate. What is the concentration of Al3+? What is the
Concentration of SO42-?
VI. Chemical Reactions & Stoichiometry
Balance the following equations and identify them as one of these (Synthesis, Decomposition, Combustion,
Single Replacement, Double Replacement, Neutralization)
1.
H2 + N2 ↔ NH3
2. Zn + HCl ↔ ZnCl2 + H2
3. Ca(OH)2 + H3PO4 ↔ H2O + Ca3(PO4)2
4. C6H6 + O2 ↔ CO2 + H2O
5. C4H10 + O2 ↔ CO2 + H2O
6. Pb(NO3)2 + NaCl ↔ PbCl2 + NaNO3
7. H2O2 ↔ H2O + O2
8. KClO3 ↔ KCl + O2
9. CO2 + H2O ↔ H2CO3
Steps to solving any stoichiometry problem
1. Write the BALANCED equation.
2. Figure out quantity you are given (grams, liters, representative particles, molarity and volume or moles) and
convert them to moles of what you are given….if what you are given is already in moles then you are good
to go.
3. Use mole ratio found from the coefficients in the balanced equation to convert moles of what you are given,
to moles of what you are looking for…(take moles given and multiply it by the mole ratio that has moles of
what you are looking for on top, and moles of what you already have on bottom. This cancels out moles
given and gives you moles of what you are looking for)
4. Now convert moles of what you are looking for to desired units (grams, liters, representative part.) If the
question asks for moles then you are good to go.
Solve the following problems (you must write down the correct balanced equation in your answer)
1. If 15.0 grams of hydrogen gas are added to excess nitrogen gas, how many moles of ammonia (NH3)
will be produced?
2. When hydrogen peroxide (H2O2) decomposes the products are water and oxygen gas. What volume of
oxygen gas will be produced if 3.0 moles of hydrogen peroxide decompose? @ STP
3. When 25 grams of silver nitrate are added to excess sodium chloride. What mass of silver chloride will
precipitate out of solution?
4. When 5.0 X 1024 atoms of zinc are placed in a solution hydrochloric acid (HCl) and completely react,
what volume of hydrogen gas will be produced @ STP?
Solution stoichiometry…follow the same steps!!!
1. If 25 mL of a 2.5 M solution of lithium chloride is added to excess lead(II) nitrate what mass of a
lead(II) chloride will be produced?
2. (Limiting Reactant). If 25 mL of a 2.5 M solution of HCl is added to 40 mL of a 2.0 M solution of
NaOH, how many moles of water will be produced?
3. (Limiting Reactant). If 30.0 mL of a 1.0 M solution of calcium chloride is added to 25.0 mL of a 1.0 M
solution of silver nitrate. What mass of silver chloride will be produced? What will the molarity of the
chloride ion (Cl1-) remaining in solution?
VII.
Gas Laws & Empirical & Molecular Formulas
1. Describe the relationship between Pressure & Volume when temperature is constant (Boyle’s Law)
a. What would a graph of Pressure vs. Volume look like?
2. Describe the relationship between Volume and Temperature when pressure is constant (Charles’s Law)
a. What would a graph of Volume vs. Temperature look like?
3. Describe the relationship between Pressure & Temperature…. volume is constant (Gay-Lussac’s Law)
4. Describe the relationship between moles of gas and volume when pressure is constant (Avogadro’s Law)
5. Write the equations for the combined gas law and ideal gas law
6. What mass of oxygen gas would be required to fill a 20.0 liter container at 2.0 atm and 37ᵒC?
7. Ideal gas law solved to include density in the equation is
P = DRT
MM
Where MM is molar mass.
What would the density of a sample of CO2 gas be, in gram/liter, if the pressure of the sample was 3.5
kPa at 298 K?
Empirical & molecular formulas
1. A compound containing only Carbon and Oxygen is found to be 27.3 % carbon by mass. The molar
mass of the compound is 88 g/mol.
a. What is the empirical formula of the compound?
b. What is the molecular formula of the compound?
Putting it all together
1. The complete combustion of a 35.0 gram sample of an unknown hydrocarbon was found to produce
118.3 grams of carbon dioxide and 24.2 grams of water.
a. What is the empirical formula of the hydrocarbon
b. The hydrocarbon in its gaseous state at 2.0 atm and 400.0 Kelvin is found to have a density
of 4.75 g/L. What is the molar mass of the unknown hydrocarbon
c. What is the molecular formula of the hydrocarbon?
d. Write the balanced equation that shows complete combustion of the hydrocarbon?