Congratulations on signing up to take AP chemistry for the 2013-‐ ... Princeton
Review “Cracking the AP Chemistry Exam” workbook for further help. This book ...
Dear Prospective AP chemistry students and parents, Congratulations on signing up to take AP chemistry for the 2013-‐ 2014 school year! AP chemistry is a rigorous yet rewarding course. I wanted to make sure you were aware in advance of the requirements and expectations of this course. First, you will be required to complete a summer assignment (see attached). It is comprised of 50 multiple choice questions and 10 free response questions covering material you should be familiar with from honors chemistry. You should work on it over the summer and be prepared to take a test over this material during the second week of school. I would highly recommend that you WAIT to work on this assignment until the middle of July or later (but just don’t wait until the week before school starts). If you do it too quickly, it won’t serve as a very good review because the material will still be fresh in your mind. Just give yourself 2-‐3 weeks to complete the assignment. Secondly, I want to make sure you understand the commitment that comes with this course. 1.) This course is extremely self-‐directed. It will be up to you to pace yourself and stay current on material, listening to lessons on time and seeking help as you need it. 2.) As the AP test approaches, you will be expected to attend at least one weekend review session in order to participate in a full-‐length practice test (3.5 hrs). 3.) Also as the test approaches, you will be expected to do between 30 minutes and 1 hour of independently study EVERY DAY outside of class to prepare yourself for the test. Feel free to email me if you have any questions or concerns regarding the expectations or summer assignment. Good luck and have a wonderful summer. I look forward to having you in class next fall! Ms. Katie Parks
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Christ Presbyterian Academy AP CHEMISTRY Summer Assignment 2013-‐2014
The following assignment covers material you should have learned in Honors Chemistry. You should complete the assignment before coming to school in August. If there are ones you have trouble with, mark them and we will go over them during the first few days of school. You will have a test over this material during the second week of school. You may refer to your notes and tests from Honors chemistry and your textbook for help with the assignment. Also, you may wish to purchase the Princeton Review “Cracking the AP Chemistry Exam” workbook for further help. This book will also be a great help to you throughout the year in AP chemistry and is highly recommended for you to have before August. It can be purchased in either paperback (around $20) or as an iBook for the iPad (around $15). Email Ms. Parks if you have questions
[email protected]
Multiple Choice 1.) 5.50 grams of gas A and 5.50 grams of gas B are sealed in a rigid container at a constant temperature. The total pressure of the system is 9.00 atm. Which of the following about the partial pressure of gas B is correct? a. The partial pressure of gas B is equal to ½ the total pressure. b. In addition to the information given, one needs to know the relative molecular mass of B in order to determine the partial pressure of gas B. c. In addition to the information provided, one needs to know the total volume of the container in order to calculate the partial pressure of gas B. d. In addition to the information provided, one needs to know the temperature of the gas mixture in order to calculate the partial pressure of gas B. e. In addition to the information provided, one needs to know the average distance traveled between molecular collisions. 2.) The density of an unknown gas is 4.00 grams per liter at 4.00 atm and 127oC. What is the molecular weight of this gas? R=0.0821 L(atm)/mole(K). a. 11.8 g/mol b. 32.8 g/mol c. 88.0 g/mol d. 94.1 g/mol e. 138 g/mol 3.) A sample of neon has a volume of 250 cm3 at 2.00 atm of pressure. At constant temperature, what would the pressure have to be in order for the gas to have a volume of 5.00 x 102 cm3? a. 1.00 atm b. 3.33 atm c. 15.7 atm d. 21.5 atm e. 43.0 atm 4.) A sample of nitrogen gas is sealed in a closed container with a constant volume. The container is heated until the absolute temperature is tripled. Which of the following is also tripled? a. Volume of the gas molecules b. Density of the gas c. The molecular mass of the gas d. The velocity of the gas molecules e. none of the above
5.) 5.00 L of a gas is known to contain 0.300 mol. If the amount of the gas is increased to 1.80 mol, what new volume will result (temperature and pressure are held constant)? a. 0.108 L b. 0.833 L c. 8.98 L d. 22.4 L e. 30.0 L
6.) Which of the following has a zero dipole moment? a. CH2Cl2 b. CO c. SO2 d. ClF e. CCl4 7.) The structural isomers C2H5OH and CH3OCH3 would be expected to have the same values for which of the following? (assume ideal behavior) a. Gaseous densities at the same temperature and pressure b. Vapor pressures at the same temperature c. Boiling point d. Melting point e. Sublimation point 8.) In a molecule in which the central atom exhibits d2sp3 hybrid orbitals, the electron pairs are directed toward the corners of a. A tetrahedron b. A square c. A square-‐based pyramid d. An octahedron e. A trigonal bipyramid 9.) Consider the following 3 molecules: X= CH3CH2CH2CH2CH3 Y= CH3CH2CH2CH2OH Z= HO-‐CH2CH2CH2-‐OH Based on the concepts of polarity and hydrogen bonding, which of the following sequences correctly lists the compounds above in the order of their decreasing solubility in water? a. Z < Y < X b. Y < Z < X c. Y< X < Z d. X < Z < Y e. X < Y < Z
10.) Types of hybridization exhibited by the carbon atoms in propene, CH3CHCH3, include which of the following? i. sp ii. sp2 iii. sp3 iv. dsp3 a. i only b. iii only c. i and ii only d. ii and iii only e. ii and iv
11.) Which element is most electronegative? a. He b. F c. Fr d. H e. Na 12.) Which of the following is the electron configuration for Mg? 2 a. 1s 2s2 2p8 b. 1s22s22p4 3s2 c. 1s22s22p73s1 d. 1s22s22p3 3s2 e. 1s22s22p63s2
13.) Which of the following elements would have the lowest first ionization energy? a. Na b. Al c. N d. Cl e. Ar 14.) Rutherford’s gold foil experiment was instrumental in: a. the discovery of the electron b. the discovery of an alpha particle c. the discovery that an atom is mostly empty space d. both A and C e. the discovery of a neutron
15.) What causes high surface tension in water? a. the high boiling point of water b. the bent shape of the water molecule c. hydrogen bonding d. the low density of ice e. none of the above 16.) The Heisenburg Uncertainty Principle says: a. As protons are added to an atom, electrons are added. b. No two electrons can have the same 4 quantum numbers. c. Maximum number of unpaired electrons has the lowest energy configuration. d. It’s impossible to know the location and momentum of an electron at the same time. e. The frequency of an atom depends purely on its velocity. 17.) Consider the reaction: C2H6(g) + O2(g) CO2(g) + H2O(g). If 6.0g of ethane burns, what volume of CO2(g) will be formed at STP? a. 0.2 L b. 0.4 L c. 2.2 L d. 9.0 L e. 22.4 L 18.)
a. b. c. d. e.
19.) a. b. c. d.
e.
Which is NOT true according to the kinetic molecular theory of gases? gas particles are somewhat large in size gas particles exert no real force on each other gases are in constant, random motion average kinetic energy of gas particles depends temperature molecules in gases have no volume Charles's law states that: the pressure of a gas is directly proportional to its temperature in Kelvin the pressure of a gas is inversely proportional to its temperature in Kelvin the volume of a gas is directly proportional to its temperature in Kelvin the volume of a gas is inversely proportional to its temperature in Kelvin none of these
20.) a. b. c. d. e.
Why is a gas easier to compress than a liquid or a solid? the volume of a gas's particles is small compared to the overall volume of the gas the space between gas particles is much less than the space between liquid or solid particles its volume increases more under pressure than an equal volume of liquid does its volume increases more under pressure than an equal volume of liquid does c and d
21.) When a container is filled with 3.00 moles of H2, 2.00 moles of O2, and 1.00 mole of N2, the pressure in the container is 768 kPa. What is the partial pressure O2? a. 128 kPa b. 192 kPa c. 256 kPa d. 213 kPa e. 234 kPa
22.) Which of the following aqueous solutions has the highest boiling point? a. 0.2m KCl b. 0.2m NaBr c. 0.2m BaCl2 d. 0.2m C6H12O6 e. 0.2m NaNO3 23.) Which of the following is (are) colligative properties? 1. Freezing point depression 2. Vapor pressure lowering 3. Boiling point elevation a. 1 only b. 1 and 2 c. 1 and 3 d. 2 and 3 e. 1, 2, and 3 24.) a. b. c. d. e.
How many grams of H2SO4 are in 75mL of a 4.00M solution? 14.2g 29.4g 36.7g 44.7g 55.2g
25.) A chemist wants to make 500mL of 0.050M HCl by diluting 6.0M HCl. How much 6.0M HCl would he need to use? a. 4.2mL b. 5.0mL c. 6.0mL d. 8.0mL e. 9.0mL 26.) What is the boiling point of a solution of 7.50g of naphthalene (C10H8) in 50.0g of benzene (C6H6)? Kb of benzene is 2.53 and the normal boiling point of benzene is 80°C. a. 80.3°C b. 81.5°C c. 83.0°C d. 85.0°C e. 273°C 27.)
Which of the following cannot hydrogen bond? a. H2S b. HCl c. NH3 d. HF e. H2O 28.) Why are diamonds so stable? a. Metallic bonding b. Network covalent bonding c. Ionic bonding d. London dispersion forces e. Dipole-‐dipole forces 29.) Which of the following compounds contain both ionic and covalent bonds? a. H2O2 b. CH4 c. NaNO3 d. NH2OH e. C6H12O6 30.) When solid carbon dioxide (dry ice) sublimes, what are the chemical forces that must be overcome? a. Intramolecular covalent bonds b. Hydrogen bonds c. London dispersion forces d. Dipole dipole forces e. Intermolecular covalent bonds
31.) In which of the following compounds is the mass ratio of oxygen to nitrogen closest to 2.86:1.00? a. NO b. NO2 c. N2O d. N2O3 e. N2O5 32.) An unknown hydrocarbon was burned in excess oxygen to form 176.04g of carbon dioxide and 54.06g of water. What is a possible molecular formula of the hydrocarbon? a. CH4 b. C2H2 c. C4H3 d. C4H6 e. C4H10 33.) When the equation below is balanced and all coefficients are reduced to their lowest whole-‐number terms, what is the coefficient for O2? C4H8O3S + O2 CO2 + SO2 + H2O a. 6 b. 7 c. 11 d. 22 e. 28 34.) Hemoglobin is the oxygen-‐carrying protein of most mammals. Each molecule of hemoglobin contains 4 atoms of iron. The molar mass of hemoglobin is about 64,000 g/mol. How many iron atoms are in 0.128g of hemoglobin? a. 7.00x103 b. 7.99x1010 c. 4.82x1018 d. 8.03x1020 e. 6.022x1023 35.) When a hydrate of LiClO4 is heated until all of the water is removed, it loses 33.7% of its mass. The formula of the hydrate is a. LiClO45H2O b. LiClO44H2O c. LiClO43H2O d. LiClO42H2O e. LiClO4H2O
36.)
Consider the reaction below A(g) + B(g) C(g) + D(g) In order to increase the amount of D, you could a. add more C for D to react with b. remove some C c. decrease the volume of the container d. increase the volume of the container e. add a catalyst to spped up the reaction to make more D 37.) Given 2NOCl(g) 2NO(g) + Cl2(g), Kc=4.4x10-‐6 at 323K, what is the equilibrium constant for 6NO(g) + 3Cl2(g) 6NOCl(g) at the same temperature? a. 2.2x103 b. 4.4x106 c. 1.2x1016 d. 8.8x1018 e. 1.32x1019 38.) The equilibrium constant Kc for the reaction COCl2(g) CO(g) + Cl2(g) is 1.67x102 at 1123K. The initial pressure of each gas are as follows: COCl2 = 0.500atm, CO = 0.25atm, Cl2 = 0.75atm. Which of the following are true? a. The system will change such that the pressure of CO and Cl2 will decrease while that of COCl2 will increase. b. The system will change such that the pressure of CO and Cl2 will increase while that of COCl2 will decrease. c. The system will not change. All pressures will remain constant and in equilibrium. d. The system will change such that only the pressure of COCl2 will increase while all other gases will maintain the same pressure. e. None of the above are true 39.) a. b. c. d. e.
Which molecule ahs the greatest bond energy? CO Cl2 NO F2 H2
40.) Which of the following chlorine-‐oxygen species has a pyramidal structure? a. ClO2 b. ClO2-‐1 c. ClO3-‐1 d. ClO4-‐1 e. Cl2O 41.) Which pair of substances will have the most similar geometry? a. SO3 and ICl3 b. SO3 and CO3-‐2 c. SO3 and SO4-‐2 d. SO4-‐2 and CO3-‐2 e. CH4 and SF4
42.) Which of the following would represent a non-‐polar molecule containing polar bonds? a. I2 b. CO2 c. PF3 d. SO2 e. H2O 43.) How many resonance forms are possible for SO3? a. 1 b. 2 c. 3 d. 4 e. 5 44.) How many valence electrons are present in the SCN-‐1 ion? a. 14 b. 15 c. 16 d. 17 e. 18 45.) The intermolecular force that is common for all molecules is a. Covalent bonding b. Dipole-‐dipole forces c. Hydrogen bonds d. Dipole-‐induced dipole forces e. London dispersion forces
46.) When the equation below is balanced, the sum of all coefficients is what? C2H3F + O2 CO2 + H2O + HF a. 9 b. 11 c. 12 d. 15 e. 19 47.) 5.00L of a gas is known to contain 0.300mol of the gas. If the amount of gas is increased to 1.80mol, what new volume will result if temperature and pressure are held constant? a. 108mL b. 833mL c. 8.98L d. 22.4L e. 30.0L
48.) What is the mole fraction of ethanol, C2H5OH, in an aqueous solution that has a density of 0.798g/mL and in which the ethanol concentration is 4.50m? a. 0.0046 b. 0.090 c. 0.15 d. 0.35 e. 0.72
49.) What is the vapor pressure of a mixture of 9.01g water and 0.500mol sugar at 29°C? The vapor pressure of pure water at 29°C is 30.0torr. a. 3.75torr b. 7.50torr c. 15.0torr d. 30.0torr e. 60.0torr 50.)
a. b. c. d. e.
The ground state electron configuration for an arsenic atom is 1s22s22p63s23p64s13d104p4 1s22s22p63s23p64s23d104p3 1s22s22p63s23p64s13d104p3 1s22s22p63s23p64s23d94p4 none of the above are correct
Free Response 1.) Explain the following in terms of atomic/molecular structure and intermolecular forces. a. Neon has a lower boiling point than xenon. b. Fluorine and chlorine are gases at room temperature, while bromine is a liquid and iodine is a solid. c. H2O is a liquid at room temperature while H2S is a gas. d. Solid magnesium has a higher melting point that solid sodium. e. PCl3 has a measureable dipole moment whereas PCl5 does not. 2.) Iron metal reacts with hydrochloric acid to produce hydrogen gas and iron (II) chloride. 0.0035M hydrochloric acid is used. This reaction takes place in 2.5 L of water. a. Write the balanced equation for the reaction described above. b. Determine the number of moles produced in the solution. c. Determine the pressure of the system, in mmHg. d. If an inert gas was added to the system, which way would the equilibrium shift? e. If the reaction is exothermic, which way would the equilibrium shift if the temperature was to increase? 3.) A solution of camphor (C10H16O = 152.23g/mol, density = 0.99g/mL) is prepared by mixing 50.0g of camphor with 1.50L of chloroform (CHCl3 = 119.40g/mol, density = 1.48g/mL). Assume volume are additive. a. Determine the mass percent of camphor in the solution. b. Determine the molarity of the solution. c. Determine the molality of the solution. d. The vapor pressure of pure chloroform is 159mmHg at 293K. Determine the vapor pressure of the solution at this temperature. e. Determine the osmotic pressure of the solution at 293K. f. Determine the boiling point of this solution. The normal boiling point for chloroform is 62°C and the Kb is 3.63. 4.) For sulfur, a. Write the extended electron configuration. b. Write the abbreviated electron configuration. c. Tell how many valence electrons it has. d. Write the abbreviated orbital diagram. e. Tell how many unpaired electrons it has. f. Write a possible set of quantum numbers (n, l, ml, ms) for a valence electron of sulfur. g. Is sulfur paramagnetic or diamagnetic? h. Name two atoms/ions that are isoelectronic with sulfur. i. In terms of atomic structure, explain why the atomic radius of sulfur is smaller than that of phosphorus.
5.) Three identical balloons are each filled with equal volumes of three separate gases (H2O, O3, and Xe). All balloons are at 27°C and 1.5atm pressure. a. Which balloon would have the least mass? Explain. b. Which balloon would have the gas with the greatest velocity? Explain. c. Which balloon would have the gas with the greatest kinetic energy? Explain. d. One day later, all of the balloons are appreciably smaller. If all factors are equal, which balloon would be the largest? Explain. 6.) A solution containing 6.30g of an unknown compound dissolved in 100.0g of water freezes at -‐0.651°C. The solute is a nonelectrolyte. Calculate the molar mass of the unknown compound. The Kf for water is 1.86. 7.) Given the molecules xenon difluoride and xenon tetrafluoride. a. Draw a Lewis structure for each. b. Predict the electron pair geometry and molecular geometry for each. c. Predict the ideal bond angle for each. d. Predict the hybridization of the central atom in each molecule. e. Give the number of sigma and pi bonds in each molecule. f. Is xenon tetrafluoride polar or nonpolar? Explain your answer. 8.) Nitric oxide (NO) is a very reactive, poisonous gas with adverse effects on the environment. Produced in internal combustion engines and electrical generating stations, NO has been implicated in depletion of the ozone layer, formation of photochemical smog, and acid rain. In an experiment to investigate ozone-‐depleting compounds, nitric oxide and ozone were mixed at 200°C according to the following equation. NO + O3 NO2 + O2 The following gaseous equilibrium concentrations were measured: [NO]=0.25M [O3]=0.30M [NO2]=[O2]=0.60M a. Write the equilibrium constant Kc expression for this reaction. b. Calculate the value of Kc. c. Calculate the value of Kp. d. When the mixture was cooled to a lower temperature, 25% of the O2 was converted back to O3. Calculate the Kc at this lower temperature. e. IN A DIFFERENT EXPERIMENT, 0.75mol of NO was mixed with 0.75mol of O3 in a 5L flask at 200°C. Calculate [O2] at this temperature for this experiment.
9.) A sample of a pure gaseous hydrocarbon is introduced into a previously evacuated rigid 1.00L vessel. The pressure of the gas is 0.200atm at a temperature of 127°C. a. Calculate the number of moles of the hydrocarbon in the vessel. b. O2(g) is introduced into the same vessel containing the hydrocarbon. After the addition of the O2(g), the total pressure of the gas mixture in the vessel is 1.40atm at 127°C. Calculate the partial pressure of O2(g) in the vessel. The mixture of the hydrocarbon and oxygen is sparked so that a complete combustion reaction occurs, producing CO2(g) and H2O(g). The partial pressure of these gases at 127°C are 0.600atm for CO2(g) and 0.800atm for H2O(g). There is O2(g) remaining in the container after the reaction is complete. c. Use the partial pressure of CO2(g) and H2O(g) to calculate the partial pressure of the O2(g) consumed in the combustion. d. On the basis of your answers above, write the balanced chemical equation for the combustion reaction and determine the formula of the hydrocarbon. e. Calculate the mass of the hydrocarbon that was combusted.
10.) Oxygen is found in the atmosphere as a diatomic gas, O2, and as ozone, O3. Ozone has a dipole moment whereas O2 does not. a. Draw the Lewis structures for both molecules. b. Use the principles of bonding and molecular structure to account for the fact that ozone has a higher boiling point than diatomic oxygen. c. Use the principles of bonding and molecular structure to account for the fact that ozone is more soluble than diatomic oxygen in water. d. Explain why the two bonds in ozone are of equal length and are longer than the bond in diatomic oxygen. e. Elemental oxygen (O) is strongly affected by a magnetic field. Explain why. f. For the equilibrium reaction below at 25°C and 1 atm, Kc = 1x10-‐57. 3O2(g) 2O3(g) Which form of oxygen (O2 or O3) is more abundant under normal conditions? Explain.
