Download AP Chemistry

Advanced Placement
Chemistry Summer Packet
Dear AP Chemistry Students,
I have taught AP Chemistry for 10 years and am very excited about next year. AP Chemistry is designed
to prepare you to be successful in college chemistry as well as to pass the AP Chemistry test. Attached is the
summer work placket to prepare you. Expect a test on this material the second day of school. You should have
all of the polyatomic ions memorized by the first day of school. All of this material should be review. AP
Chemistry is a second year course for a reason. If there are problems in the packet that you are having difficulty
with, do not panic. Contact me through email or some fellow classmates, so that on the first day of school you are
able to do the required problems.
Thank You,
Mrs. Hampton
[email protected]
Material that was Covered in Honors Chemistry
Chapter 1 Intro
The Scientific Method
Chapter 3 Scientific Measurement
Metric Conversions
Significant Figures
Scientific Notation
Chapter 4 Atomic Structure
Dalton, Thomson, Rutherford, Bohr experiments and models of the atom
Isotopes and average mass calculations
Ions
Chapter 5 Electrons in the Atom
Schrodingers model (quantum mechanics)
Shapes of s, p, d and f orbitals
Electron configurations
Electron configurations of ions
Electromagnetic Radiation (calculation of wavelength, frequency and energy)
Absorption and Emission of Light and Emission Spectra
Flame Test
Chapter 6 Periodic Table\
Trends in
Radius
Ionization energy
Electrogenativity
Ion size
Chapter 7 Ionic and Metallic Bonding
Lewis drawings of elements and ions
Characteristics of ionic and metallic bonds
Chapter 8 Covalent Bonding
Draw Lewis structures for molecules
Molecular Geometry : Name VSEPR shapes for molecules
Hybridization (sp, sp2, sp3, sp3d and sp3d2)
Polar bonds
Polarity based on molecular geometry
Intermolecular forces: Hydrogen bonds, London dispersion, Dipole-Dipole, Ion- Dipole,
Covalent Network Solids
Chapter 9 Named and Formula
Memorize polyatomic ions
Write names and formula for A salts, B salts, and molecules
Write names and formula for acids
Chapter 10 Chemical Quantities
Dimensional Analysis
Mole/mass/volume/particle conversions
Empirical and Molecular Formula
Chapter 11 Reactions
Types of Chemical Reactions
Double Displacement
Single Displacement (oxidation and reduction concepts)
Synthesis
Decomposition
Combustion
Acid Base Reactions
Chapter 12 Stoichiometry
Mole/mass/volume/particle conversions with balanced reactions
Limiting Reactants
Chapter 13 and 14 Matter and Gases
Standard Temperature and Pressure
Phase Diagrams
Boyles, Charles, Gay-Lussac, Avogardro’s Gas Laws
Ideal Gas Law
Gas Stoichiometry
Dalton’s Law
Graham’s Law
Kinetic Molecular Theory
Chapter 15 and 16 Solutions
Characteristics of water (specific heat, surface tension, hydrogen bonding)
Solute vs. Solvent
Factors that effect solubility (heat, agitation, particle size)
Vapor Pressures of Solutions
Colligative Properties (including the math!)
Molarity
Dilution Problems
Solution Stoichiometry
Chapter 17 Thermochemistry
Specific Heat Capacity
Enthalpy or reactions
Hess’s Law
Calorimetry
Chapter 18 Reactions Rates and Equilibrium
Reaction Rates (temperature, concentration, particle size, catalysts)
Equilibrium Constant (including the math!)
Equilibrium Expression
Le Chatelier’s Principle
Thermodynamics – spontaneous reactions, entropy and enthalpy
Free Energy
Chapter 19 Acids and Bases
Concepts behind acid strength
Calculation of pH (including logarithmic problems)
Properties or acids and bases
Titrations (math!)
Chapter 22 Organic Chemistry
Alkanes, alkenes, alkynes
Functional Groups
Chapter 25 Nuclear Chemistry
Nuclear Stability and Radioactive Decay
Nuclear Reactions
Half life problems
-
Polyatomic Ions
Nitrate
Nitrite
Oxalate
Peroxide
Permanganate
Phosphate
Hydrogen Phosphate
Dihydrogen Phosphate
Phosphite
Sulfate
Hydrogen sulfate
Sulfite
Silicate
Thiocyanate
Thiosulfate
Acetate
C2H3O2
NO3Ammonium
NH4+
NO2Arsenate
AsO43C2O42Borate
BO33O22Carbonate
CO32MnO4Hydrogen carbonate
HCO3PO43Hypochlorite
ClOHPO42Chlorite
ClO2H2PO4Chlorate
ClO3PO33Perchlorate
ClO4SO42Chromate
CrO42HSO4Dichromate
Cr2O72SO32Cyanide
CNSiO44Hydroxide
OHSCN+
Hydronium
H3O
S2O32Iodate
IO3Molecule Prefixes (nonmetals bonded to nonmetals only!!)
Mono-1
hexa - 6
di- 2
hepta - 7
tri- 3
octa - 8
tetra- 4
nona- 9
penta-5
deca - 10
Strong Acids
Hydrobromic acid
Nitric acid
Sulfuric acid
Hydrochloric acid
Hydroiodic acid
Chloric Acid
Perchloric Acid
Iodic Acid
HBr
HNO3
H2SO4
HCl
HI
HClO3
HClO4
HIO3
Strong Bases
Alkali, alkali earth hydroxides
LiOH
NaOH
KOH
Mg(OH)2
Ca(OH)2
Weak Acids
Hydrofluoric Acid
Nitrous Acid
Sulfurous Acid
Carbonic acid
Acetic acid
Chlorous Acid
Hypochlorous Acid
Phosphoric acid
Hydrocyanic
HF
HNO2
H2SO3
H2CO3
HC2H3O2
HClO2
HClO
H3PO4
HCN
Weak Bases
Ammonia
Methyl amine
Aniline
Bicarbonate
Carbonate
NH3
CH3NH2
C6H5NH2
HCO3CO32-
Practice Problems:
Name the following compounds, using Roman numerals when necessary.
1. NH4NO3
26. BaCl2
2. CsClO4
27. KCl
3. NaOH
28. BaCO3
4. Na3PO4
29. K2CO3
5. Hg2I2
30. KOH
6. Cu(OH)2
31. BaO
7. BaO
32. Fe3(PO4) 2
8. Al(C2H3O2)3
33. SnBr2
9. SrCl2
34. (NH4)2CO3
10. MgSO3
35. SrCO3
11. FeCl2
36. NH4Br
12. Pb(ClO3)2
37. Ag2SO4
13. PbO
38. AlCl3
14. Sr(ClO3)2
39. ZnCl2
15. V(NO3)2
40. Al2(SO4)3
16. CO
41. KSCN
17. H2O
42. N2O
18. SO3
43. NiO
19. CoCl
44. P4O10
20. NaCN
45. Cl2O8
21 Cu3N
46. NaCN
22. CoO
47. HF
23. NaHSO4
48. NiClO4
24. N2H4
49. PbCr2O7
25. Mg(MnO4)2
50. LiNO2
Chemical Formula Practice
For each of the following compounds give the correct chemical formula. The compounds fall into different
categories:
Molecules
:
prefixes indicate the number of each element
A Group Salts :
charges used to balance formula
B Group Salts :
Roman Numerals show charge of transition metal, charges used to balance formula
Silver, cadmium and zinc are exceptions. (Ag+, Cd2+ and Zn2+)
1. Aluminum hydrogen carbonate
23. Ammonium acetate
2. Potassium perchlorate
24. Nickel (II) nitrite
3. Calcium carbonate
25. Copper (I) carbonate
4. Chromium (II) nitrite
26. silver cyanide
5. Boron trichloride
27. Ammonium chlroate
6. Dichlorine heptachloride
28. Silver nitride
7. Stannic phosphate
29. Magnesium sulfide
8. Lithium fluoride
30. Iron (III) sulfate
9. Zinc oxide
31. Silver chromate
10. Sulfur hexafluoride
32. Sodium fluoride
11. Iron (III) sulfide
33. Copper (II) thiocyanate
12. Vanadium (IV) phosphide
34. Tetraiodine nonoxide
13. Mercury (II) iodide
35. Tin (II) oxalate
14. Zinc sulfite
36. Aluminum oxalate
15. ammonium sulfide
37. Manganese (II) hydroxide
16. nickel (III) hypochlorite
38. Aluminum oxide
17. Lithium nitride
39. Calcium perchlorate
18. Aluminum carbonate
40. Magnesium sulfite
19. Nitrogen monoxide
41. Zinc sulfide
20. Lead (II) phophite
42. Mercury (II) perchlorate
21. Manganese (III) acetate
43. Vanadium (I) hydrogen phosphate
22. Antimony (IV) hydroxide
44. NaC2H3O2
Balancing Reactions Review
Vocabulary: The following are terms that you should be comfortable with using in daily practice.
Coefficient
Synthesis/Combination
Products
Gas
Subscript
Decomposition
Reactants
Liquid
Precipitate
Single Displacement
Yields
Solid
Aqueous
Double Displacement
Soluble
Balanced equation
Diatomic elements
Combustion
Insoluble
Law of conservation of Mass
word equation
Chemical equation
Translate the following descriptions into balanced reactions.
Reaction Types
A) Synthesis (Combination) Two reactants combine to give one product.
a) Metal oxide + water  base
(basic anhydrides)
CaO(s) + H2O(l)  Ca(OH)2(aq)
Na2O(s) + H2O (l)  2 NaOH (aq)
b) Nonmetal oxide + water  acid
(acid anhydrides)
SO2(g) + H2O(l)  H2SO3(aq)
SO3(g) + H2O(l)  H2SO4(aq)
N2O5(g) + H2O(l) → 2 HNO3(aq)
P2O5(g) + 3 H2O(l) → 2 H3PO4(aq)
d) Metal + oxygen → metal oxide
2 Mg(s) + O2(g) → 2 MgO(s)
4 Al(s) + 3 O2(g) → 2 Al2O3(s)
e) Metal + nonmetal → Salt
2Al(s) + 3 Cl2(g) → 2 AlCl3(s)
2 Al(s) + 3Br2(l) → 2 AlBr3(s)
3 Ca(s) + N2(g) → Ca3N2(s)
B) Decomposition: a single substance is decomposed or broken down to give two or more different products.
a) Hydrolysis of water
2H2O(l) → 2H2(g) + O2(g)
b) Hydrogen Peroxide
(with either a catalyst or heat)
2 H2O2(g) → 2 H2O(g) + O2(g)
c) Chlorates
2KClO3(s) Δ → 2KCl(s) + 3O2(g)
d) Carbonates
(NH4)2CO3(s) Δ → H2O(g) + CO2(g) + 2NH3(g)
CaCO3(s) Δ → CaO(s) + CO2(g)
NaHCO3(s) Δ → Na2CO3(s) + H2O(g) + CO2(g)
C) Single Displacement (Redox) An element reacts with a compound totake the place of one of the elements of
that compound. A new element is formed along with a new compound.
a) Metal and Acid  hydrogen + salt
H2SO4(aq) + Fe(s) → FeSO4(aq) + H2(g)
b) Metal and Water hydrogen + metal hydroxide OR metal oxide
2Na(s) + 2H2O (l) → NaOH(aq) + H2(g)
Ca(s) + 2H2O(l) → Ca(OH)2(aq) + H2(g)
Mg(s) + H2O(l) → MgO(s) + H2(g)
(water must be hot for this one!)
c) Metal + salt  metal + salt
CuSO4(aq) + Fe(s) → FeSO4(aq) + Cu(s)
AgNO3(aq) + Cu(s) → Cu(NO3)2(aq) + Ag(s)
d) Halogens + Halogen salt  halogen + halogen salt
Elements higher up on the halogens will replace element lower on the table
Cl2(g) + 2 KBr(aq) → Br2(l) + 2 KCl(aq)
D) Double Discplacement (Metathesis) Two compounds exchange partners to produce two different compounds.
Neutralization
H3PO4(aq) + 3NH4OH(aq) → 3H2O(l) + (NH4)3PO4(aq)
E) Combustion: a carbon compound is burned in oxygen to create carbon dioxide and water.
CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(g)
C6H12O6(s) + 6O2(g) → 6CO2(g) + 6H2O(g)
A) Synthesis (Combination)
1. Diphosphorus pentoxide is added to water to form phosphoric acid.
2. Sodium oxide is mixed with water to form the metal base.
3. Aluminum metal burns in oxygen to form a salt.
4. Metallic lithium and oxygen gas produces lithium oxide.
5. Solid potassium oxide salt is dropped into water to produce potassium hydroxide solution.
B) Decomposition
1. Calcium chlorate decomposes into calcium chloride and oxygen gas.
2. Sodium carbonate decomposes into carbon dioxide gas and sodium oxide.
3. Sodium bicarbonate decomposes into sodium carbonate, carbon dioxide and water.
4. When heated solid potassium perchlorate produces potassium chloride and oxygen gas.
5. Hydrogen peroxide is heated to form water vapor and oxygen gas.
C. Single Displacement (Redox)
1. Aluminum is added to hydrochloric acid to produce hydrogen has and aluminum chloride.
2. A piece of nickel is place into silver nitrate forming nickel (II) nitrate.
3. Lead metal is placed in a solution of silver nitate to form lead (II) nitrate and silver metal.
4. Zinc is dropped into hydrochloric acid.
5. Chlorine gas is bubbled through a solution of magnesium bromide displacing liquid bromine and a salt.
D. Double Discplacement (Metathesis)
1. Solutions of aluminum hydroxide and sulfuric acid are mixed.
2. Zinc phosphate solution is mixed with tin (IV) nitrate solution.
3. Ammonium hydroxide is mixed with copper (II) phosphate.
4. Lithium hydroxide solution is poured into nitric acid (HNO3).
5. Potassium phosphate solution reacts with a solution of lead (II) nitrate to produce a lead solid.
E. Combustion
1. Combustion of sucrose (C12H22O11) yields carbon dioxide and water.
Gas Laws, Stoichiometry,
Empirical/Molecular Formula Problems
Solve the following problems. Show all work, round off correctly to the number of significant digits. Use
units in your work and in your answer.
PV = nRT
R = 8.314 L kPa/mol K or R = 0.08206 L atm/mol K
1. What is the volume of 0.813 moles of hydrogen sulfide at 25 °C and 1.10 atm?
2. How many grams of carbon tetrachloride are present in a sample of gas in a 2.50 liter container at 30 °C and 1.0
atm? (Solve for n first)
3. What is the volume of 4.2 x 1022 molecules of ozone, O3, at 31.0 C and 99.4 kPa? (Convert to moles first)
Stoichiometry: Use the following balanced reactions to answer the questions.
4. Alex drips hydrochloric acid onto a 5.9 g piece of magnesium in a single displacement reaction. How many
molecules of HCl are required?
2HCl(aq) + Mg(s) → MgCl2(aq) + H2(g)
5. How many milliliters of NH3, at STP, will react with 5.3 g of oxygen gas to form nitrogen dioxide and water?
4NH3(g) + 7O2(g)  4NO2(g) + 6H2O(g)
Limiting Reactants
Begin with the first reactant given. Use stoichiometry to determine how much of the other reactant is required.
State which reactant is limiting. Then begin with the limiting reactant and answer the question. EXAMPLE:
If the reaction of 3.82 g of magnesium nitride with 7.73 g of water produced
3.60 g of magnesium oxide, what is the percent yield of this reaction?
Mg3N2(s) + 3 H2O(l) → 2 NH3(g) + 3 MgO(s)
3.82 g Mg3N2
mol Mg3N2
100.9 g
3 mol H2O
1 mol Mg3N2
3.82 g Mg3N2
mol Mg3N2
100.9 g
3 mol MgO
1 mol Mg3N2
18.0 g = 2.04 g H2O required
mol H2O
40.3 g = 4.58 g MgO
mol MgO
Mg3N2is limiting.
6. How many molecules of water vapor is produced when 4.393 moles of HNO3 gas reacts with 3.4 grams of solid
hydrogen sulfide?
3 H2S(s) + 2 HNO3(g) → 2 NO(g) + 4 H2O(g) + 3 S(s)
7. DDT, an insecticide harmful to mammals is produced by the following reaction:
2 C6H5Cl + C2HOCl3 → C14H9Cl5 + H2O
(chlorobenzene) (chloral)
(DDT)
In a government lab 1142 g of chlorobenzene were reacted with 485 g of chloral.
a) In grams how much DDT was formed? (limiting reactant problem!)
b) What amount of excess reactant is leftover?
c) If the actual yield of DDT was 200.0 g what was the percent yield?
8. Nitrogen gas can be prepared by passing gaseous ammonia over solid copper (II) oxide at high temperatures.
The other products of this reaction are solid copper and water vapor. If a sample containing 18.1 g of ammonia
reacted with a 90.4 g of copper (II) oxide, how many grams of nitrogen will be formed?
2 NH3(g) + 3 CuO(s) → N2(g) + 3 Cu(s) + 3 H2O(g)
Empirical and Molecular Formula
9. Determine the empirical formula of a compound that is 17.0 % Mg, 38.0% Al and 45.0%O.
10. Determine the empirical formula of a compound that is 27% K, 35% Cr, and 38% O.
11. Determine the empirical formula for 86% C and 14% H. What is its molecular formula if it has a molar mass
of 70.0 g?
12. A white powder and sends it in to be analyzed. It is found to contain 43.64 % phosphorus and 56.36 %
oxygen by mass. Obtaining the empirical formula will be tricky because you will find a fraction in the ratios.
Multiply these numbers by 2 to get two whole numbers. The compound has a molar mass of 283.88 g/mol. What
is the molecular formula?
13. Caffeine, a stimulant found in coffee, tea, and chocolate, contain 49.18% carbon, 5.05 % hydrogen, 28.87
% nitrogen and 16.49 % oxygen by mass. The molar mass is 194.2 g/mol. What is the molecular formula?