AP Chemistry Summer Study Guide
AP Chemistry – Summer Study Guide
Future AP Chemistry Student:
Attached you will find summer work which will review the stoichiometry that were learned in Honors Chemistry. It is imperative that you review during the summer. We will begin by applying the concepts you have already mastered this past year and begin looking at problems in a new and exciting way. You may use any resource needed to complete this review packet. You may work with your peers; in fact, I encourage you to do so. Keep in mind that copying from your peers will do you no good, as you will ultimately be responsible for knowing this material.
It is expected that ALL work is shown and completed on notebook paper, NOT on these worksheets. The solutions to these problems will be collected** on August 19, 2016. We will spend approximately one week reviewing this content before your first AP Chemistry test, which is scheduled for Monday Aug 29, 2016. Mastering these problems will ensure you perform well on this test.
There is also a vocabulary list attached. You will be tested on these words during the first two weeks of school. Flash cards make this process very easy.
If you have any questions, please e-mail me at Sfiligok@hudson.edu and I will get back to you. If you would like to check out a text book to use over the summer, please stop by C100, as you will have to turn in your Honors Chemistry textbook at the end of this year.
Enjoy your summer,
Mrs. Sfiligoj
** This is your first summative grade!
Directions: Below you will find topics that are a review of material you learned in Chemistry. Beneath each topic are a series of questions pertaining to the topic. Answer each of the questions with the following in mind: show all work, label all numbers with units and species (ex: 3 grams of NaCl), and provide your answer with correct units and significant figures…On another sheet of paper…i.e. not in this packet!
AP Chemistry Summer Study Guide
1. For the combustion of sucrose: C12H22O11 + O2 ---> CO2 + H2O there are 10.0 g of sucrose and 10.0 g of oxygen reacting. Which is the limiting reagent?
2. Calculate the mass of NaBr formed when 50.0 grams of NBr3 and 57.0 grams NaOH react according to the unbalanced reaction:
NBr3 + NaOH ---> N2 + NaBr + HOBr
3. Aluminum reacts with chlorine gas to form aluminum chloride via the following reaction: Al + Cl2 ---> AlCl3
How many grams of aluminum chloride could be produced from 34.0 g of aluminum and 39.0 g of chlorine gas?
4. Interpret reactions in terms of representative particles, then write balanced chemical equations and compare with your results. Determine limiting and excess reagent and the amount of unreacted excess reactant.
a) 3 atoms of carbon combine with 4 molecules of hydrogen to produce methane (CH4)
b) 7 molecules of hydrogen and 2 molecules of nitrogen gases react to produce ammonia
c) 4 molecules of hydrogen and 5 molecules of chlorine react.
5. 950.0 grams of copper (II) sulfate are reacted with 460.0 grams of zinc metal.
a) What is the theoretical yield of Cu?
b) If 295.8 grams of copper are actually obtained from this reaction, what is the percent yield?
6. What weight of each substance is present after 0.4500 g of P4O10 and 1.5000 g of PCl5 are reacted completely?
P4O10 + PCl5 ---> POCl3
7. The equation for the reduction of iron ore in a blast furnace is given:
Fe2O3 + CO ---> Fe + CO2
a) How many grams of iron can be produced by the reaction of 7.00 grams of Fe2O3 and 3.00 grams of CO?
b) How many grams of the excess reagent remains after the reaction has ceased?
8. 35.5 g SiO2 and 66.5 g of HF react to yield 45.8 g H2SiF6 in the following reaction:
SiO2(s) + HF(aq) ---> H2SiF6(aq) + H2O(l)
a) How much mass of the excess reactant remains after reaction ceases?
b) What is the theoretical yield of H2SiF6 in grams?
c) What is the percent yield?
9. The reaction of 15.0 g C4H9OH, 22.4 g NaBr, and 32.7 g H2SO4 yields 17.1 g C4H9Br in the reaction below:
C4H9OH + NaBr + H2SO4 ---> C4H9Br + NaHSO4 + H2O
Determine:
a) the theoretical yield of C4H9Br
b) the actual percent yield of C4H9Br
c) the masses of leftover reactants, if any
10. A 0.972-g sample of a CaCl2 ⋅ 2H2O and K2C2O4 ⋅ H2O solid salt mixture is dissolved in 150 mL of deionized water, previously adjusted to a pH that is basic. The precipitate, after having been filtered and air-dried, has a mass of 0.375 g. The limiting reactant in the salt mixture was later determined to be CaCl2 ⋅ 2H2O
a) How many grams of the excess reactant, K2C2O4 ⋅ H2O, reacted in the mixture?
b) What is the percent by mass of CaCl2 ⋅ 2H2O?
c) How many grams of the K2C2O4 ⋅ H2O in the salt mixture remain unaffected?
11. Disulfide dichloride, S2Cl2, is used in the vulcanization of rubber, a process that prevents the slippage of rubber molecules past one another when stretched. It is prepared by heating sulfur in an atmosphere of chlorine:
S8(s) + 4Cl2(g) 4S2Cl2(l)
a. What is the theoretical yield of S2Cl2 in grams when 4.06 grams of S8 are heated with 6.24 grams of Cl2? If the actual yield of S2Cl2 is 6.55 grams.
b. What is the percent yield?
12. When tin comes in contact with the oxygen in the air, tin (IV) oxide, SnO2, is formed.
Sn(s) + O2(g) SnO2(s)
A piece of tin foil, 8.25cm x 21.5cm x 0.600mm (d=7.28g/cm3) is exposed to oxygen.
a. Assuming that all the tin has reacted, what is the mass of the oxidized tin foil?
b. Air is about 21% oxygen by volume (d=1.309g/L at 25C and 1 atm). How many liters of air are required to completely react with the tin foil?
13. Oxygen masks for producing O2 in emergency situations contain potassium superoxide, KO2. It reacts with CO2 and H2O in exhaled air to produce oxygen:
4KO2(s) + 2H2O(g) + 4CO2(g) 4KHCO3(s) + 3O2(g)
If a person wearing such a mask exhales 0.702 grams CO2/min, how many grams of KO2 are consumed in 25 minutes?
14. When iron and steam react at high temperatures, the following reaction takes place:
3Fe(s) + 4H2O(g) Fe3O4(s) + 4H2(g)
How much iron must react with the excess steam to form 897 grams of Fe3O4 if the reaction yield is 69%.
15. Oxyacetylene torches used in welding reach temperatures near 2000C. The reaction involved in the combustion of acetylene is:
2C2H2(g) + 5O2(g) 4CO2(g) + 2H2O(g)
a. Starting with 175 grams of both acetylene and oxygen, what is the theoretical yield, in grams of carbon dioxide?
b. If 68.5L (d=1.85g/L) of carbon dioxide is produced, what is the percent yield at the same conditions of temperature and pressure?
16. The Space Shuttle uses aluminum metal and ammonium perchlorate in its reusable booster rockets. The products of the reaction are aluminum oxide, aluminum chloride, nitrogen monoxide gas, and steam. The reaction contains 7.00 grams of aluminum and 9.32 grams of ammonium perchlorate.
c. Write the balanced equation for the reaction.
d. What is the theoretical yield of aluminum oxide?
e. If 1.56 grams of aluminum oxide is formed, what is the percent yield?
f. How many grams of excess reactant are unused?
17. Aspirin, C9H8O4, is prepared by reacting salicylic acid, C7H6O3, with acetic anhydride,C4H6O3, in the reaction:
C7H6O3 + C4H6O3 C9H8O4 + C2H4O2(l)
A student is told to prepare 45.0 grams of aspirin. She is also told to use a 55.0% excess of acetic anhydride and to expect to get an 85.0% yield in the reaction. How many grams of each reactant should she use?
18. A student prepares phosphorus acid, H3PO3, by reacting solid phosphorus triiodide with water.
PI3(s) + 3H2O(l) H3PO3(s) + 3HI(g)
The student needs to obtain 0.250L of H3PO3 (d=1.651 g/cm3). The procedure calls for 45.0% excess of water and a yield of 75.0%. How much phosphorus triiodide should be weighed out? What volume of water (d=1.00 g/cm3) should be used
19. A 4.000 g sample of M2S3 is converted to MO2 and loses 0.277 g. What is the atomic weight of M? The reaction that takes place is: M2S3 + O2 ---> MO2 + SO2
20. A salt contains only barium and one of the halide ions. A 0.1480 g sample of the salt was dissolved in water and an excess of sulfuric acid was added to form barium sulfate, which was filtered, dried and weighed. Its mass was found to be 0.1660 g. What is the formula for the barium halide?
21. For the reaction below, when 0.5000 g of XI3 reacts completely, 0.2360 g of XCl3 is obtained. Calculate the atomic weight of element X and identify it. XI3 + Cl2 ---> XCl3 + I2
22. A 12.5843 g sample of ZrBr4 was dissolved and, after several steps, all of the combined bromine was precipitated as AgBr. The silver content of AgBr was found to be 13.2160 g. Assume the atomic masses of silver and bromine to be 107.868 and 79.904. What value was obtained for the atomic mass of Zr from this experiment?
23. A 75.35g sample of an unknown base, which consist of 19.99% C, 26.64% O, 46.65% N and 6.73% H reacts with a 62.55g sample of an unknown molecular compound which consists of 30.45% N and 69.55% O. Calculate the mass of each of the three resulting products, carbon dioxide, water and nitrogen gas.
24. Three compounds, silver oxide, ammonium hydroxide and ammonium nitrate react to for a complex silver compound and water. The silver complex is found to contain 52.89% Ag, 20.61% N, 2.97% H and 23.53% O. Calculate the mass of each reactant needed to produce 45.35g of the complex silver compound.
25. A 9.25g sample of an unknown hydrate is heated. After repeated heatings, the mass stabilizes at 5.03g. The anhydrous salt is analyzed and found to contain .762g of potassium, .526g aluminum, 1.25g sulfur and 2.49g of oxygen. How many grams of aluminum are needed to produce the 9.25g of the unknown hydrate if the reaction requires aluminum, potassium hydroxide, sulfuric acid and water and hydrogen gas is liberated during the production of the hydrate.
26. Two salts, 50.0 grams of each, are dissolved in water and then mixed together to produce a precipitate. The first salt contains 14.09g N, 4.06g H, 10.385g P and 21.46g O. The second salt contains 16.06g Ni, 7.67g N, and 26.27g of O. In grams, what is the maximum mass of precipitate that can be formed? If 29.5g were actually formed during an experiment, calculate the percent yield.
27. An unknown organic base is combusted. In addition to the usual products of the combustion of a hydrocarbon, nitrogen dioxide is also produced. The organic base is 68.87% C, 15.06% H and the remainder is N. If 100.00g of the unknown organic base is combusted in 145.00g of oxygen gas, calculate the mass of each of the products and calculate the mass of excess reactant remaining.
VOCABULARY: In order to expand your chemistry vocabulary, you will find numerous terms and definitions that you need to have memorized for the first day of school. You will be tested on 20 terms, randomly chosen. This will be a summative quiz. I would recommend making flash cards and practicing until you show mastery of all terms.
Absorbance: Light that does not pass through a solution A = abc
Activation Energy: Minimum energy needs to be added to a system in order for the chemical reaction to occur
Alpha Particle: He2+ 2 protons, mass number = 4, 2+ charge Highly ionizing particle; Low energy
Anion: Negatively charge ion
Arrhenius Acid: Donates a H+ ion
Arrhenius Base: Donates a OH- ion
Atom: Smallest constituent unit of ordinary matter that has the properties of a chemical element
Atomic Mass: Average of all naturally occurring isotopes
Atomic Number: Number of protons; defines the atom
Beta Particle: -1 proton, mass number =0; medium ionizing ability, medium energy
Boiling: Phase change from a liquid to a gas
Bronsted-Lowry Acid: Donates a proton, H+
Bronsted-Lowry Base: Accepts a proton, H+
Calorimetry: Means of measuring the heat gained/ lost by a system during a chemical reaction
Catalyst: Lowers the activation energy. Not a reactant. Not a product
Cation: Positively charged ion
Chemical Equilibrium: Rate of the forward reaction equals the rate of the reverse reaction
Condensation: Phase change from a gas to a liquid
Conversion Factor: Allows for the conversion from one unit of measure to another
Covalent Bond: Bond formed by the sharing of electrons between atoms.
Deposition: Phase change from a gas to a solid
Dipole-Dipole: Permanent IMF present in polar molecules
Direct Relationship: Relationship between two variables where when one changes, the other changes in the same manner
Dissociate: To break into ions
Dissolve: To break into smaller pieces
Distillation: Process of separating liquids based on differences in boiling temperatures
Double Bond: Two shared pairs of electrons
Electrolyte: Dissociates into charge particles which are capable of conducting electricity
Electrolytic Cell: Redox reaction that is spontaneous
Electron Affinity: Energy released when an atom gains an electron
Electron: Negatively charged particle. Charge = -1, Mass ~0amu. Located in the orbitals surrounding the nucleus
Electronegativity: The ability of an atom to attract electrons from another atom
Empirical Formula: Lowest whole number ratio of atoms in a compound
Endothermic: Energy is gained by the system
Evaporation: Process of removing water from an aqueous solution. Solute is left behind
Exothermic: Energy is released by the system
Filtrate: Liquid that passes through the filter paper
Filtration: Process of separating a precipitate from its aqueous solution
Formula Unit: Ionically bonded atoms
Freezing: Phase change from a liquid to a solid
Galvanic / Voltaic Cell: Redox reaction that is spontaneous
Gamma Ray: 0 protons, mass number = 0, Low ionizing ability, high energy
Halogen: Elements in group 17. Form halides as ions
Hydrogen Bonding: Strong dipole that results when H is bonded to F, O, or N
Indirect relationship: Relationship between two variables where when one changes, the other changes in the opposite manner
Insoluble: Does not dissolve in water
Intermediate: Species produced in one step and consumed in another step
Intermolecular Forces, IMF: Attractive forces between molecules
Ion: Charge particle
Ionic Bond: Bond formed by the transfer of 1 or more electrons from the least electronegative atom to the more electronegative atom
Ionization Energy: Energy required to remove the outer electron
Kinetic Energy: Energy of motion, temperature is a measure of KE
Limiting Reactant: Reactant to runs out first thus limiting the amount of product that can be formed
London Dispersion Forces: Temporary IMF caused by the movement of electrons
Lone Pair: Unbonded electrons
Mass Number: Mass of all protons and neutrons
Melting: Phase change from a solid to a liquid
Molar Mass: grams per 1 mol
Molarity: moles of solute per liter of solution
Molecular Formula: actual number of moles of each atom in a compound
Molecule: Covalently bonded atoms
Neutron: Neutral particle. No charge. Mass = 1amu, Located in the nucleus
Noble Gas: Group 18 on the PT. Each has 8 valence electrons. Nonreactive
Orbital: Regions of probability where electrons are located. Each orbital can contain up to 2 electrons
Oxidation Number: A charge assigned to an atom that represents that charge it would have if it contained and ionic bond. Oxidation numbers are written as charge value, +4, -6, +2
Oxidation: Process of losing electrons which increases the oxidation number
Percent Error: Absolute value (Theoretical – Experimental) / Theoretical) x 100%
Percent Yield: (Quantity produced / Theoretical Amount) x 100%
Precipitate: Solid matter that forms from the reaction of two aqueous solutions
Principle Energy Level: n= 1 means first energy level. Energy levels contain sublevels
Proton: Positively charged particle. Charge = +1, Mass = 1amu, Located in the nucleus
Reduction: Process of gaining electrons which reduces the oxidation number
Significant Figures: Those digits that carry meaning contributing to its precision
Single Bond: One shared pair of electrons
Soluble: Dissolves in water
Solute: The species that gets dissolved to form a solution
Solution: Solute and solvent
Solvent: The species that does the dissolving to form a solution
Sources of Error: These are errors that you make in the lab which result in either increased or decreased yields. These do not include Human Error, Calculations, Massing…..
Specific Heat: Energy required to raise 1 gram of a substance 1C
Strong Acid: Dissociates 100%
Strong Base: Dissociates 100%
Sublevel: s, p, d, and f. defines the shape
Sublimation: Phase change from a solid to a gas
Surroundings: This refers to everything outside of the system
System: This refers to the reaction
Transmittance: Light that passes through a solution
Triple Bond: Three shared pairs of electrons
Valence electrons: Outer electrons which are available for bonding
Weak Acid: Dissociate very little. Remains mostly in its molecular form
Weak Base: Dissociates very little. Remains mostly in its molecular form
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