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AP Chemistry – Summer Study Guide Future AP Chemistry Student: Attached you will find summer work which will review topics 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. I will be collecting your work during the first week of school and it will be graded. If you have any questions, please e-mail me at [email protected] 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 Help Sessions this summer: Please attend any or all of these to help you work through this study guide. Where: Panera Hudson When: Tues, June 16th Tues, July 7th Tues, Jul 28th Time: 10:00am- 12:00pm 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. Measurement (Zumdahl-Zumdahl Section 1.3-1.8) A. Write the appropriate symbol in the blank, <, =, > 1. 303m_____303 X 103km 2. 500g_____0.500kg 3. 1.50cm3_____1.50 X 103 nm3 B. Explain how a volume measurement is made when measuring water in a graduated cylinder. C. Identify the best piece of lab equipment and process that would be used to measure the following: 1. Mass of a solid crystal reagent which is in excess. 2. Mass of a solid precipitate 3. Create 500ml of a 1M HCl solution from 2M stock 4. Volume of 15ml of a 0.05M NaCl solution 2. Significant Figure (Zumdahl-Zumdahl Section 1.5) A. Round off the following quantities to the indicated number of significant figures. 1. 7.4855 grams (3 significant figures) 2. 298.693 cm (5 significant figures) 3. 11.968 lbs. (1 significant figure) 4. 345 oz. (2 significant figures) B. Calculate the following to the correct number of significant figures. 1. X = 128.5 + 2116.44 – 2244.47 2. X = 0.004010 X 2.0000 X 50054 3. X = 12.6 + 0.3 + 256.5/ 1003.7 4. X = 12.20 – (1.60 + 4(0.36))1/2/ 1.3409 3. Dimensional Analysis (Zumdahl-Zumdahl Section 1.6) A. A metal slug weighing 25.17 grams is added to a flask with a volume of 59.7mL. It is found that 43.7 grams of methanol (density = 0.791 g/mL) must be added to the metal to fill the flask. What is the density of the metal? B. A solid with an irregular shape and a mass of 11.33 grams is added to a graduated cylinder filled with water (density = 1.00 g/mL) to the 35.0mL mark. After the solid sinks to the bottom, the water level is read to be at the 42.3mL mark. What is the density of the solid? C. Air is 21% oxygen by volume. Oxygen has a density of 1.31 g/L. What is the volume, in liters, of a room that holds enough air to contain 55 kilograms of oxygen? 4. Periodic Table & Atom: Protons, Neutrons, Electrons (Zumdahl-Zumdahl Sections 2.1-2.5, 3.1, 7.8, 7.11-7.13) A. Who discovered the electron? Describe the experiment that led to the deduction that electrons are negatively charged. B. Selenium is widely sold as a dietary supplement. It is advertised to “protect” women from breast cancer. Write the nuclear symbol for naturally occurring selenium. It has 34 protons and 46 neutrons. C. Complete the following table using the periodic table if necessary. Nuclear Charge Number of Number of Number of Symbol Protons Neutrons Electrons 79 0 35Br -3 7 7 +5 33 42 90 4+ 40Zr D. Strontium has four isotopes with the following masses: 83.9134 (0.56%), 85.9094 (9.86%), 86.9089 (7.00%), and 87.9056 (82.58%). Calculate the atomic mass of strontium. E. Define an isotope. What is the same and what is different? F. Complete the table below. Element Electron Configuration Mg 1s22s22p63s23p64s23d104p65s24d3 Br 1s22s22p63s23p64s23d104p65s24d105p66s25d106p1 G. Complete the table below. Element Orbital Diagram Ti Xe C Sc H. Define ionization energy. Arrange the following elements in order based on increasing ionization energy: Na, Mg, K I. Define atomic radius. Arrange the following elements in order based on decreasing atomic radii: Cl, S, Ca J. Define electronegativity. Arrange the following elements in order based on increasing electronegativity: Be, Mg, Ca. 5. Nomenclature (Zumdahl-Zumdahl Section 2.8) A. Complete the table below Name ICl3 N2O5 PH3 HNO2 HNO3 HCl K2Cr2O7 Fe2(SO3)3 NaClO MgCl2 B. Complete the table below. Name Iron (III) carbonate Sulfur hexafluoride Silicon dioxide Hypochlorous acid Oxalic acid Carbon monoxide Sulfur trioxide Copper (II) sulfate Barium oxide Titanium (IV) oxide Formula Formula C. Criticize each of the following statements. 1. In an ionic compound the number of cations is always equal to the number of anions. 2. The molecular formula for strontium bromide is SrBr2. 3. The mass number is always equal to the atomic number. 4. For any ion, the number of electrons is always more than the number of protons. 6. Molar Mass (Zumdahl-Zumdahl Section 3.3-3.4) A. Complete the following table for TNT, C7H5(NO2)3. Number of Grams Number of Moles Number of Molecules 127.2 1.248 4.32 X 1022 Number of N Atoms 5.55 X 1019 B. Calculate the molar mass of the following: 1. cane sugar, C12H22O11 2. laughing gas, N2O 3. vitamin A, C20H30O 7. Percent Composition (Zumdahl-Zumdahl Section 3.6) A. Turquoise has the following chemical formula: CuAl6(PO4)4(OH)8*4H2O. Calculate the mass percent of each element in turquoise. B. A tablet of Tylenol has a mass of 0.611 grams. It contains 251mg of its active ingredient, acetaminophen, C8H9NO2. 1. What is the mass percent of acetaminophen in a tablet of Tylenol? 2. Assume that all the nitrogen in the tablet is in the acetaminophen. How many grams of nitrogen are present in a tablet of Tylenol? 8. Simplest & Molecular Formulas (Zumdahl-Zumdahl Section 3.7) A. Determine the simplest formula of the following compounds: 1. the food enhancer MSG which has the composition 35.51%C, 4.77% H, 37.85% O, 8.29% N, and 13.6% Na. 2. Zircon, a diamond like mineral, which has the composition 34.91% O, 15.32% Si, and 49.76%Zr. 3. Nicotine which has the composition 74.0% C, 8.65% H, and 17.4% N. B. Explain how you would find the molecular formula given the simplest formula and the molar mass. 9. Balancing Equations (Zumdahl-Zumdahl Section 3.9) A. Balance the following equations: 1. H2S + SO2 S + H2O 2. CH4 + NH3 + O2 HCN + H2O 3. Fe2O3 + H2 Fe + H2O 10. Stoichiometry (Zumdahl-Zumdahl Section 3.10) A. Diborane, B2H6, can be prepared by the following reaction: 3NaBH4 + 4BF3 2B2H6 + 3NaBF4 1. How many moles of NaBH4 react with 1.299 moles of BF3? 2. How many moles of B2H6 can be obtained from 0.893 moles of NaBH4? 3. If 1.987 moles of B2H6 is obtained, how many moles of NaBF4 are produced? 4. How many moles of BF3 are required to produce 4.992 moles of NaBF4? 11. Limiting Reagents & Theoretical Yield (Zumdahl-Zumdahl Section 3.10) A. 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 mixture contains 7.00 grams of aluminum and 9.32 grams of ammonium perchlorate. 1. Write the balanced equation for the reaction. 2. What is the theoretical yield of aluminum oxide? 3. If 1.56 grams of aluminum oxide is formed, what is the percent yield? 4. How many grams of excess reactant remain? B. Oxyacetylene torches used for welding reach temperatures near 2000oC. The reaction involved in the combustion of acetylene is 2C2H2 + 5O2 4CO2 + 2H2O 1. Starting with 175 grams of both acetylene and oxygen, what is the theoretical yield, in grams, of carbon dioxide? 2. If 68.5L (density = 1.85 g/L) of carbon dioxide is produced, what is the percent yield at the same conditions of temperature and pressure? 3. The following equation describes the oxidation of ethanol to acetic acid by potassium permanganate: 3C2H5OH + 4KMnO4 4. 5. 6. 7. 8. 3HC2H3O2 + 4MnO2 + 4KOH + H2O 5.00 grams of ethanol and an excess of aqueous potassium permanganate are reacted and 5.98grams of acetic acid results. What is the percent yield? If 45ml of a 1.50M AgNO3 solution is added to 25.0grams of NaCl, how many grams of AgCl can be produced? How many liters of a 3.0M phosphoric acid solution are required to react with 4.50 grams of zinc metal? How many grams of aluminum metal are required to react with 35ml of 2.0M hydrochloric acid? Determine the percent yield for the reaction in which 15.8 grams of NH3 and excess oxygen gas produce 21.8grams of NO gas and some water. Determine the percent yield for the reaction between 15.0 grams of N2 and 15.0grams of H2 if 10.5 grams of NH3 is produced? 12. Molarity (Zumdahl-Zumdahl Section 4.1) A. A reagent bottle is labeled 0.450M K2CO3. 1. How many moles of K2CO3 are present in 45.6mL of this solution? 2. How many milliliters of this solution are required to furnish 0.800 moles of K2CO3? 3. Assuming no volume change, how many grams of K2CO3 do you need to add to 2.00L of this solution to obtain a 1.000M solution of K2CO3? 4. If 50.0mL of this solution is added to enough water to make 125mL of solution, what is the molarity of the diluted solution? 13. Ideal Gas Law (Zumdahl-Zumdahl Section 5.3) A. A piece of dry ice, CO2, has a mass of 22.50 grams. It is dropped into an evacuated 2.50L flask. What is the pressure in the flask at -0.4oC? B. Use the ideal gas law to complete the following table, for CO2 Pressure Volume Temperature Moles Grams o 1.75L 19 C 1.66 0.895atm 6oC 14.0 433mmHg 92.4mL 0.395 o 1.1atm 8.66L 25 C 14. Light (speed, frequency, wavelength) (Zumdahl-Zumdahl Section 7.1) A. A photon of violet light has a wavelength of 423nm. Calculate 1. the frequency 2. the energy in joules pre photon 3. the energy in kilojoules per mole B. Describe the relationship between wavelength and frequency. C. Describe the relationship between energy and frequency. D. Explain which color of light in the visible spectrum has the highest energy. E. Explain which color of light in the visible spectrum has the longest wavelength. 15. Lewis Dot Structures (Zumdahl-Zumdahl Section 8.10) A. Complete the table below: Formula Lewis Dot 3-D Shape/ AXE Shape Name Structure Formula CCl4 Angles NCl3 SO2 SO3 Formula Polar Bonds (Y/N) Polar molecule (Y/N) Hybridization Number of / bonds Type(s) of IMF CCl4 NCl3 SO2 SO3 16. Kinetics (Zumdahl-Zumdahl Section (Zumdahl-Zumdahl Section 12.2-12.3) A. The equation for the reaction between iodide and bromate ions in acidic solution is 2A 3B + C Time (min) 0 35.0 44.0 66.2 [A] 1.2 x 10-4 4.00 x 10-5 3.00 x 10-5 1.50 x 10-5 1. Draw and label a graph to show the changes in concentration versus time for all reactants and products (one graph) 2. Draw and label a graph to show what relationship provides a linear relationship ([ ] vs t, ln[ ] vs t, or 1/[ ] vs t) 3. Write the resulting rate law with the value of the rate constant, k, substituted into the equation 17. Equilibrium (Zumdahl-Zumdahl Section 13.1-13.2) (NEW) A. Write the mass action expressions for the following reactions: 1. I2(g) + 5F2(g) 2IF5(g) 2. CO(g) + 2H2(g) CH3OH(l) 3. 2H2S(g) + 3O2(g) 2H2O(l) + 2SO2(g) 4. SnO2(s) + 2H2(g) Sn(s) + 2H2O(l) B. A gaseous reaction mixture contains 0.30 atm SO2, 0.16atm Cl2, and 0.50 atm SOCl2 in a 2.0L flask. Kp = 0.011 for the equilibrium system SO2Cl2(g) SO2(g) + Cl2(g) 1. Is the system at equilibrium? Explain. (Hint: Solve for Q) 2. If it is not at equilibrium, in which direction will the system move to reach equilibrium? (Hint: Compare Q to Kp) 18. Acids and Bases (Zumdahl-Zumdahl Section 14.1-14.3) (NEW) A. Find the pH and pOH of solutions with H+ ion concentrations of: 1. 6.0M 2. 4.6 X 10-8M 3. 7.2 X 10-14M B Write the dissociation equation for each of the following: 1. Hydrocyanic acid 2. Phosphoric Acid 3. Hydrofluoric acid 4. Sulfuric acid 19. Nuclear Reactions (Zumdahl-Zumdahl Section 19.1-19.7) A. Define emission reaction and bombardment reactions B. Write the symbols for the following and explain how the number of protons and mass number changes when the particle is a reactant, and as a product. Alpha, Beta, Gamma, Proton, Neutron C. Write balanced reactions for the following: 1. U-238 undergoes alpha emission 2. Th-185 undergoes beta emission 3. Cl-35 is bombarded with a neutron 4. Ni-63 is bombarded with a proton 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