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Ms. Brasington [email protected] Welcome to AP Chemistry! AP Chemistry is probably the most difficult AP course offered in high school. By signing up for this class, you are agreeing to (1) have a solid work ethic, (2) put in 1 – 2 hours per day on chemistry outside of the classroom, (3) have a secure working knowledge base of general chemistry prior to taking the course, (4) stay after school for help where your knowledge base is weak or the subject area is difficult, (5) minimize absences (whether they are an approved school activity, vacation or illness) as they will greatly affect your work load and understanding, (6) take the AP Chemistry exam, (7) go into the AP Chemistry exam with the expectation of passing with a 3 or higher, and (8) respect that this is a college level course and will be taught as such. Much is expected of you; much is expected of me. With this mutual respect, these expectations can be accomplished. The use of a calculator will be kept to a minimum. The AP exam only allows you to use the calculator on certain sections. Thus, your expertise in math is a necessity. You can expect to utilize basic math skills that you began to learn in elementary school. Addition, subtraction, multiplication and division should be second nature when you walk into the room and you should be able to do these in your head. Practice these skills using simple flash cards. Build the numbers as you go. Do not just stick to the basics. Expand your horizons and work with larger numbers. You also need to be competent with using scientific notation in the above mathematical applications. Utilize the internet to help you find ways to improve your skills. If you do not practice these skills you lose the ability to perform them quickly, confidently and competently. Flash cards will help you throughout this course. It is good practice to begin using now with these basic math skills. Supplemental Text We will be utilizing the following book along with our text. Please purchase this before the new school year begins! I found mine on Amazon for $8.51! There are many different books out there that appear similar. This is the specific one you need. 5 Steps to a 5 AP Chemistry by John T. Moore, Richard H. Langley Published by McGraw/Hill 1 Memorization of Polyatomic Ions Many of these you already know. Many of these you do not. Be sure to have the following polyatomic ions given in the table below memorized by day 1. Common Polyatomic Ions +1 CHARGE ion -1 CHARGE name ion -2 CHARGE name ion name -3 CHARGE ion name NH4+ ammonium H2PO3- dihydrogen phosphite HPO32- hydrogen phosphite H3O+ hydronium H2PO4- dihydrogen phosphate HPO42- hydrogen PO43- phosphate phosphate Hg22+ mercury(I) HCO3- hydrogen carbonate CO32- carbonate PO23- hypophosphite HSO3- hydrogen sulfite SO32- sulfite AsO33- arsenite HSO4- hydrogen sulfate SO42- sulfate AsO43- arsenate NO2- nitrite S2O32- thiosulfate NO3 nitrate SiO3 2- OH- hydroxide C22- - - CH3COO acetate CrO2 - oxalate 2- C2O4 chromate CN cyanide Cr2O72- dichromate CNO- cyanate C4H4O62- tartrate CNS- thiocyanate MoO42- O2 superoxide 2- peroxide MnO4- permanganate S22- disulfide - ClO chlorite ClO3- chlorate ClO4 - - BrO molybdate perchlorate hypobromite - bromite BrO3- bromate BrO2 BrO4 - - IO perbromate hypoiodite IO2- iodite - iodate IO3 - IO4 AlO2 N3- P2O74- pyrophosphate hypochlorite - ClO2 O2 name carbide 2- CrO4 - ion silicate chromite - PO33- phosphite -4 CHARGE periodate - aluminate azide 2 A bit of creativity before you get to the nitty gritty: Create a collage that shows what success means to you regarding AP Chemistry. These are to be on ( 14in x 22 in ) poster board only. The board needs to be completely covered. Write an explanation on the back of your collage. They will be displayed. Remember that success is different for each individual. No two people should have the same collage with the same explanation. How to Make a Collage A collage (From the French: coller, to glue) is a work of formal art, primarily in the visual arts, made from an assemblage of different forms, thus creating a new whole. A collage may include newspaper clippings, ribbons, bits of colored or hand-made papers, portions of other artwork, photographs and other found objects, glued to a piece of paper or canvas. The term collage derives from the French "coller" meaning "glue".This term was coined by both Georges Braque and Pablo Picasso in the beginning of the 20th century when collage became a distinctive part of modern art. Making a collage is fun, easy, and creative! You are going to make a collage to represent who you are. The following link gives step by step details: http://www.wikihow.com/Make-a-Collage The following problems should be review. Please complete and turn in the first day of school. 3 Kellam High School • AP Chemistry Name_____________________________________ Period _____ Date ___/___/___ 1•Matter and Measurement PRACTICE TEST Which physical state of matter exhibits the greatest change in volume with changes in temperature or pressure? 1. a) 2. solid b) liquid c) gas According to the Kinetic Molecular Theory particles of a solid a) are bound in a regular array and do not move. b) float freely within an array occupying various positions relative to neighbors. c) have no relationship to the microscopic structure of the solid. d) vibrate back and forth but do not move past immediate neighbors. e) 3. float freely in the inside but do not move on the surface. What volume of a liquid having a density of 1.48 g/cm3 is needed to supply 5.00 grams of the liquid? a) 0.296 cm3 b) 1.48 cm3 c) 4. d) 3.38 cm3 e) 7.40 cm3 2.26 cm3 The density of aluminum is 2.70 g/cm3. If a cube of aluminum weighs 13.5 grams, what is the length of the edge of the cube? a) 5.00 cm b) 1.71 cm c) 5. e) 0.200 cm 1.25 cm Which temperature change is the smallest? a) 10°C to 20°C b) 10 K to 20°C c) 6. d) 0.312 cm d) 10°F to 20°C e) 10°F to 20°F 10 K to 20 K The number of significant figures in 0.06060 x 10 -5 is a) 2 b) 3 c) d) 5 e) 6 4 4 7. The number, three hundred and fifty thousand, written in scientific notation is best written as a) 350 b) 3.5 x 106 c) 8. d) 3.50 x 105 e) 3.50 x 10-5 3.5 x 105 The mass of a sample weighted on an electronic balance that is sensitive to ±0.3 mg is 1.2300 g. The number of significant figures in this measurement is a) 1 b) 2 c) 9. d) 4 e) 5 3 What is the numerical value of: 1.5 cm – 7.222 x 10-1 cm? a) 0.7778 cm b) 0.778 cm c) d) 0.8 cm e) 7.072 x 10-1 cm 0.78 cm 10. Four samples were weighed using three different balances. (All are as accurate as the precision below indicates.) The masses are 0.94 kg, 58.2 g, 1.55 g, and 250 mg. This total mass should be reported as a) 1000.000 g b) 1000.0 g c) d) 1.00 x 103 g e) 1.0 x 103 g 1.000 x 103 g 11. The temperature of the room is 75°F. What is its temperature in Celsius degrees? a) 24°C b) 27°C c) d) 43°C e) 43°C 30°C 12. The symbols for a metal, a non-metal and a noble gas in that order are a) Ag, Ga, Xe b) Ce, Ge, Ne c) d) Ba, P, Ar e) P, Pb, Kr Ca, Sn, Ks 13. Which of the following elements is a non-metal? a) Ca b) Cr c) d) Cl e) Cs Co 5 14. A good example of an ionic compound is a) water b) sugar c) d) sodium chloride e) natural gas dry ice 15. When a pure solid substance was heated, a student obtained another solid and a gas, each of which was a pure substance. From this information which of the following statements is ALWAYS a correct conclusion? a) The original solid is not an element. b) Both products are elements. c) The original solid is a compound and the gas is an element. d) The original solid is an element and the gas is a compound. e) Both products are compounds. 16. Classify each observation as a physical or a chemical property and tally them. Observation 1: Bubbles form on a piece of metal when it is dropped into acid. Observation 2: The color of a crystalline substance is yellow. Observation 3: A shiny metal melts at 650°C. Observation 4: The density of a solution is 1.84 g/cm3 a) 2 chemical properties and 2 physical properties b) 3 chemical properties and 1 physical properties. c) 1 chemical properties and 3 physical properties d) 4 chemical properties e) 4 physical properties 17. To convert a value in kilograms to centigrams one should a) multiply by 105 b) multiply by 103 c) d) divide by 105 e) divide by 10-1 multiply by 10-3 18. How many cm2 are in an area of 4.21 in2? a) 10.7 cm2 b) 114 cm2 c) d) 1.66 cm2 e) 1.14 cm2 27.2 cm2 19. When the prefix micro (µ) is used in the metric system, a fundamental unit of measurement is multiplied by a factor of a) 10-9 b) 10-6 c) d) 103 e) 109 10-3 6 20. Of the masses 86.30 g, 0.0863 kg and 8.630 x 10 5 mg, which (if any) is the largest? a) 86.30 d) they are the same b) 0.0863 kg c) e) 5 8.630 x 10 mg two are the same, one is smaller 21. The element chlorine is obtained for commercial use by the following method: a) Isolation from gas pockets in the earth’s crust. b) Separation from air by a high pressure technique. c) Filtration of brine (NaCl) solutions. d) Electrolysis of aqueous NaCl solutions. e) Mixing sulfur and argon in equal quantities. 22. Consider a brass alloy which contains 66% copper and 34% zinc. How many grams of zinc are present in 125 kg of the alloy? a) d) 2.4 x 104 g 2.4 g b) 42 g c) e) 4.2 x 104 g 83 g 23. The density of a sodium sulfate solution is 1.07 g/cm3. The solution is 8.00% sodium sulfate by mass. How many cm3 of the solution are needed to supply 4.28 g of sodium sulfate? a) 30.0 cm3 b) 35.0 cm3 c) d) 45.0 cm3 e) 50.0 cm3 40.0 cm3 24. Which of the following is NOT an SI base unit? a) mass d) time b) volume c) e) temperature length 2 Atoms and Elements 1. Certain properties are characteristic of metals. Which property means that you can pound the substance into a foil? a) ductility b) conductivity 2. c) sectility d) malleability Which of the following is a metalloid? a) As b) Ag c) S d) Pb e) He 7 3. Which of the following is a transition metal? a) Cl 4. e) C b) Kr c) K d) Al e) H b) Eu c) Cd d) P e) W Which element has the highest melting point? a) Pb 7. d) Ca Which of the following is an lanthanide? a) Xe 6. c) P Which of the following is an alkali metal? a) Mg 5. b) Ni b) Au c) Os d) W e) Hg Pictured below is a schematic of the Rutherford experiment. Which scattered -particle gives the best evidence for the nuclear atom? a b c e a) a 8. b) b c) c d) d e) e Which of the following is an isotope of the element with 20 protons (p=20) and 22 neutrons (n=22)? a) titanium-22 b) zirconium-40 9. d c) calcium-40 d) titanium-48 The imaginary element X has the following natural abundances and isotopic masses. What is the atomic weight of X? 24 24.02 amu 40.0% 12 X 26 26.10 amu 60.0% 12 X For questions 13 - 16, use the following key: (each answer may be used once, more than once, or not at all.) a) John Dalton b) Ernest Rutherford c) J.J. Thomson d) Democritus 13. His model of the atom has been called the “billiard ball” model. 14. He studied matter in cathode ray tubes. 8 15. His philosophical idea included the term “atomos”. 16. He added to the atomic theory the idea that atoms had positive and negative parts. 220 17. Consider the following notation: 86 Rn Which statement below is correct? a) This particle contains 86 protons b) This particle has a mass number of 86 c) This particle has an atomic number of 220 d) This particle contains 220 neutrons 18. If copper metal is a mixture two isotopes, Cu-63, mass = 62.9298 u and Cu-65, mass = 64.9278 u. The molar mass of copper is 64.546 g/mole. Calculate the % abundances of the two isotopes of copper. 3 • Molecules and Compounds 1. What is the formula of the ionic compound formed between Mg and Br? a) MgBr b) Mg2Br c) 2. e) Mg2Br3 MgBr2 What is the formula of the ionic compound formed between Ca and P? a) Ca2P3 b) CaP c) 3. d) Mg2Br2 d) Ca2P e) Ca3P2 Ca5P10 What is the name of the SO32– ion? a) sulfate b) nitrate c) d) sulfur trioxide e) hydrogen sulfate sulfite 4. What is the correct formula and charge for the chromate ion? a) CrO42– d) Cr2O7– b) CrO4– e) Cr3+ c) Cr2O72– 5. Which one of the following elements forms ions with two different valences? a) calcium b) arsenic c) iron d) fluorine 9 6. The correct name for CCl4 is a) carbon(I) chloride b) carbon chloride c) carbon tetrachloride d) monocarbon chloride(IV) e) 7. carbochlorinate The correct formula for hydrogen telluride is a) HTe b) H2Te 8. H3Te d) HTe2 The correct formula for dinitrogen tetroxide is a) NO2 d) NO3– b) N2O4 c) 9. c) e) (N2O)4 N2 O 5 The correct name for S2Cl2 is a) sulfur dichloride b) sulfur(I) chloride c) sulfur(II) chloride d) disulfur dichloride e) sulfur chloride 10. The correct name for H3P is a) hydrogen phosphide b) trihydrogen phosphide c) hydrogen phosphate d) phosphorus trihydride e) hydrogen triphosphate 11. The molar mass of (NH4)2S is closest to: a) 50 g/mol b) 82 g/mol c) 68 g/mol d) 100 g/mol 12. How many atoms are in 12 molecules of glucose, C6H12O6? a) 24 b) 288 c) 2160 d) 7.22 x 1024 10 13. Calculate the number of atoms in 4.0 x 10-5 g of aluminum. a) 8.9 x 1017 b) 4.6 x 1019 c) 6.5 x 1020 d) 3.8 x 1023 14. Which of the following samples contains the smallest number of atoms? a) 1 g H2 b) 1 g O2 c) 1 g O3 d) 1 g Cl2 15. What is the mass of one molecule of octane, C8H18? a) 114 g b) 1.89 x 10-22 g c) 1.10 x 10-22 g d) 4.32 x 10-23 g 16. What is the percent nitrogen (by mass) in ammonium carbonate, (NH 4)2CO3? a) 14.53% b) 27.83% c) 29.16% d) 33.34% 17. Of the following, the only empirical formula is a) N2F2 b) N2F4 c) H2C2 d) HNF2 18. A compound consists of the following elements by weight percent: carbon - 40.0% oxygen - 53.3% hydrogen - 6.7% The ratio of carbon : oxygen : hydrogen in the empirical formula is a) 1:2:1 b) 1:1:1 c) 1:1:2 d) 2:1:2 19. An organic compound which has the empirical formula CHO has a molar mass of 232. Its molecular formula is: a) CHO b) C2H2O2 c) C4H4O4 d) C8H8O8 20. When CaSO4·y H2O is heated, all of the water is driven off. If 34.0 g of CaSO4 [molar mass = 136] is formed from 43.0 g of CaSO4·y H2O, what is the value of y? a) 1 b) 2 c) 3 d) 4 11 4 • Chemical Equations and Stoichiometry 1. Balance the following equation: ___NH3 + ___O2 ___NO2 + ___H2O The balanced equation shows that 1.00 mole of NH3 requires ___ mole(s) of O2. a) 0.57 c) 1.33 b) 1.25 d) 1.75 2. Write a balanced equation for the combustion of acetaldehyde, CH 3CHO. When properly balanced, the equation indicates that ___ mole(s) of O 2 are required for each mole of CH3CHO. a) 1 c) 2.5 b) 2 d) 3 3. Balance the following equation with the SMALLEST WHOLE NUMBER COEFFICIENTS possible. Select the number that is the sum of the coefficients in the balanced equation: ___KClO3 ___KCl + ___O2 a) 5 b) 6 c) 7 d) 8 4. Write a balanced equation for the combustion of propane, C3H8. When properly balanced, the equation indicates that ___ moles of O 2 are required for each mole of C3H8. a) 3 b) 3.5 c) 5 d) 8 5. What is the total mass of products formed when 16 grams of CH4 is burned with excess oxygen? a) 80 g c) 36 g b) 44 g d) 32 g 6. Calculate the mass of hydrogen formed when 25 g of aluminum reacts with excess hydrochloric acid. 2Al + 6HCl 2 AlCl3 + 3 H2 a) 0.41 g c) 1.2 g b) 0.92 g d) 2.8 g 7. How many grams of the mixed oxide, Fe3O4, are formed when 6.00 g of O2 react with Fe according to 3Fe + 2O2 Fe3O4 a) b) 8. 43.4 86.8 c) d) 174 21.7 For the reaction: 2MnO2 + 4KOH + O2 + Cl2 2KMnO4 + 2KCl + 2H2O there is 100. g of each reactant available. Which reagent is the limiting reagent? [Molar Masses: MnO2=86.9; KOH=56.1; O2=32.0; Cl2=70.9] a) MnO2 c) O2 b) KOH d) Cl2 12 9. How many grams of nitric acid, HNO3, can be prepared from the reaction of 92.0 g of NO 2 with 36.0 g H2O? 3NO2 + H2O 2HNO3 + NO a) b) 10. 64 76 c) d) 84 116 The reaction of 25.0 g benzene, C6H6, with excess HNO3 resulted in 21.4 g C6H5NO2. What is the percentage yield? C6H6 + HNO3 C6H5NO2 + H2O a) 100% c) 54.3% b) 27.4% d) 85.6% 5 • Reactions In Aqueous Solution 1. When H2SO4 and Ba(OH)2 are reacted in a double replacement reaction, one of the products of the reaction is… a) H2 d) BaH2 b) H2O c) 2. e) BaS Which of the following is a base? a) KOH d) CH3OH b) C2H5OH c) 3. e) Br– H2CO3 d) HClO3 b) HF c) e) H3PO4 HNO3 d) H2S b) H2SO3 c) e) HNO2 H2SO4 What is the oxidation number of C in CO32–? a) +6 d) +1 b) +4 c) 6. HNO3 SO2 turns into which acid in solution? a) 5. CO2 Which of the following is a strong acid? a) 4. SO2 e) –1 +2 What is the oxidation number of Br in KBrO4? a) +1 b) –1 c) +5 d) +7 e) +8 13 7. For each change below, label the change of the underlined element as Oxidation, Reduction, or Neither ___ Cu2+ Cu ___ CH4 CO2 ___ H2O2 H2O ___ CO2 H2CO3 8. How many milliliters of 0.123 M NaOH solution contain 25.0 g of NaOH (molar mass = 40.00 g/mol)? a) 5.08 mL b) 50.8 mL c) 9. d) 625 mL e) 5080 mL 508 mL If you need 1.00 L of 0.125 M H2SO4, how would you prepare this solution? a) Add 950. mL of water to 50.0 mL of 3.00 M H2SO4. b) Add 500. mL of water to 500. mL of 0.500 M H2SO4. c) Add 750 mL of water to 250 mL of 0.375 M H2SO4. d) Dilute 36.0 mL of 1.25 M H2SO4 to a volume of 1.00 L. e) Dilute 20.8 mL of 6.00 M H2SO4 to a volume of 1.00 L. 10. What is the molarity of the solution that results when 60.0 g NaOH is added to enough water to make 500. mL solution? a) 1.33 M b) 12.0 M c) d) 8.0 M e) 1.50 M 3.00 M 11. What is the molarity of the solution that results when 45.0 g HCl is dissolved in enough water to make 250. mL solution? a) 4.94 M b) 4.50 M c) d) 1.80 M e) 1.46 M 3.24 M 12. How many grams of Na2CO3 (molar mass = 106.0 g/mol) are required for complete reaction with 25.0 mL of 0.155 M HNO3? Na2CO3 + 2HNO3 2NaNO3 + CO2 + H2O a) 0.122 g b) 0.205 g c) d) 20.5 g e) 205 g 0.410 g 14 13. What volume of 0.150 M NaOH is needed to react completely with 3.45 g iodine according to the equation: 3 I2 + 6 NaOH 5 NaI + NaIO3 + 3 H2O a) 181 mL b) 45.3 mL c) d) 2.04 mL e) 1.02 mL 4.08 mL 14. What is the concentration of an NaOH solution if it takes 16.25 mL of a 0.100 M HCl solution to titrate 25.00 mL of the NaOH solution? a) 0.0165 M b) 0.151 M c) d) 0.100 M e) 0.413 M 0.0650 M 15. A 4.00 M solution of H3PO4 will contain ___g of H3PO4 in 0.250 L of solution. a) 196 g b) 98.0 g c) d) 24.0 g e) 12.0 g 49.0 g 6 • Energy and Chemical Reactions 1. How many joules are equivalent to 37.7 cal? a) 9.01 J b) 4.184 J 2. 1.51 J d) 158 J The quantity of heat that is needed to raise the temperature of a sample of a substance 1.00 degree is called its a) heat capacity b) specific heat 3. c) c) enthalpy d) kinetic energy If 25 J are required to change the temperature of 5.0 g of substance A by 2.0C, what is the specific heat of substance A? a) 250 J/gC b) 63 J/gC 4. c) 10. J/gC d) 2.5 J/gC How much energy is required to change the temperature of 2.00 g aluminum from 20.0C to 25.0C? The specific heat of aluminum is 0.902 J/gC. a) 2.3 J b) 9.0 J c) 0.36 J d) 0.090 J 15 5. Consider the thermal energy transfer during a chemical process. When heat is transferred to the system, the process is said to be _______ and the sign of H is ________. a) exothermic, positive b) endothermic, negative c) exothermic, negative d) endothermic, positive 6. When two solutions react the container “feels hot.” Thus, a) the reaction is endothermic. b) the reaction is exothermic. c) the energy of the universe is increased. d) the energy of both the system and the surroundings is decreased. 7. Which one of the following would have an enthalpy of formation value (Hf) of zero? a) H2O(g) c) b) O(g) 8. H2O(l) d) O2(g) Calculate the standard enthalpy of the reaction for the process 3NO(g) N2O(g) + NO2(g) using the standard enthalpies of formation (in kJ/mol): NO = 90; N2O = 82.1; NO2 = 34.0 a) -153.9 kJ c) b) 206 kJ -26.1 kJ d) 386 kJ 19. Calculate the amount of heat needed to change 25.0 g ice at 0C to water at 0C. The heat of fusion of H2O = 333 J/g; a) 56.5 kJ c) b) 8.33 kJ 7.06 kJ d) 463 kJ 7&8 • Atomic Structure & Periodicity 9. Which quantum number determines the subshell occupied by an electron (s, p, d, f, etc.)? a) n c) b) l ml d) ms 10. What position on the standing wave shown below corresponds to a crest? a) A b) B c) C d) D e) E 16 11. How many orbitals make up the 4d subshell? a) 0 b) 1 c) 3 d) 5 e) 7 12. The value of l that is related to the following orbital is: a) 0 b) 1 c) 2 d) 3 e) 4 13. The correct electron configuration for nitrogen is a) 1s2 2s2 2p6 3s2 3p2 b) 1s2 2s2 2p6 2d4 c) 1s2 2s2 2p3 d) 1s2 2s2 3s2 4s1 e) 1s2 1p5 14. The electron configuration of the indicated atom in the ground state is correctly written for which atom? a) Ga [Ar] 3d12 4s2 b) Ni [Ar] 3d10 c) [Ar] 3s2 3p8 Ni d) Cu [Ar] 3d10 4s1 15. Which of the following sets of quantum numbers is possible for a 3d electron? 1 a) n = 3, l = 3, ml = –2, ms = + 2 1 b) n = 2, l = 1, ml = +1, ms = – 2 1 c) n = 3, l = 1, ml = 0, ms = – 2 1 d) n = 3, l = 2, ml = –2, ms = + 2 1 e) n = 4, l = 1, ml = +1, ms = + 2 16. In what section of the periodic table is the 4f subshell being filled? a) period 4 b) transition elements Y to Cd c) noble gases d) group IA e) lanthanides 17 17. Which one of the following elements has 3 electrons in a p subshell? a) Sb b) Na c) Sc d) V e) Nd 18. Which of the following distributions of electrons is correct for three electrons in p-subshell? a) b) c) d) e) 20. Which of the following correctly represents the ionization of an atom? a) Cl(g) + e– Cl–(g) b) Na(g) Na+(g) + e– c) Na(s) – e– Na+(g) d) Cl2(g) 2 Cl(g) 21. Which of the following is likely to have the largest atomic radius? a) H b) Mn c) Cl d) Rb e) Ag 23. Which of the following has the greatest ionization energy? a) K b) Ca c) Fe d) Ga e) Br 24. Which of the following has the lowest ionization energy? a) Li b) Na c) K d) Rb e) Cs 26. Draw the orbital diagram for a neutral Ag atom: 5s 4s 3s 2s 1s 18 Write the electron configuration for silver: 27. Long form: 28. Short form using noble gases: 9 Bonding & Molecular Structure 1. The correct Lewis symbol for ground state carbon is a) 2. b) b) c) d) e) b) P c) S d) B e) F How many electrons are shown in the Lewis structure of perchlorate ion, ClO4–? a) 30 5. e) Which of the atoms below is least likely to violate the octet rule? a) Be 4. d) The correct Lewis symbol for ground state aluminum is a) 3. c) b) 31 c) 32 d) 50 e) 51 Which of the following is the correct Lewis structure for SOCl2? (Consider formal charge) a) d) b) e) c) 6. In which of the following is the actual compound a resonance hybrid of Lewis structures? a) NO2 b) H2O c) 7. d) CCl4 e) none of these O3 Which of the following bonds is most polar? a) N – Cl b) C – N c) d) Br – Br e) S–O S–S 19 8. 9. Which one of the following molecules is a polar molecule? a) c) b) d) Which molecular shape has bond angles which are not all the same? a) linear d) planar triangular b) tetrahedral c) e) trigonal bipyramid octahedral 10. The molecule BrF3 has how many lone pairs of electrons on the central atom? a) 0 b) 1 c) 2 d) 3 11. What is the geometrical arrangement of electron pairs in H2O? a) linear b) bent c) d) trigonal bipyramidal e) tetrahedral octahedral 12. What is the shape of BrI3? a) square planar b) T-shaped c) d) pyramidal e) bent distorted tetrahedral 13. Which of the following is a polar species? a) CO2 b) PCl5 c) ICl2– d) TeCl4 e) CCl4 20 14. Among those listed below, which element will have the strongest tendency to form double bonds? a) S b) B H 2.1 Li 1.0 Na 0.9 K 0.8 Rb 0.8 Cs 0.7 Fr 0.7 c) Al d) O Electronegativity Values Be 1.5 Mg 1.2 Ca 1.0 Sr 1.0 Ba 0.9 B 2.0 Al 1.5 Ga 1.6 In 1.7 Tl 1.8 C 2.5 Si 1.8 Ge 1.8 Sn 1.8 Pb 1.8 N 3.0 P 2.1 As 2.0 Sb 1.9 Bi 1.9 O 3.5 S 2.5 Se 2.4 Te 2.1 Po 2.0 F 4.0 Cl 3.0 Br 2.8 I 2.5 At 2.2 He --Ne --Ar --Kr --Xe --Rn --- 12 • Gases and Their Properties 1. A pressure of 745 mmHg corresponds to ___ kPa. a) 55.89 kPa b) 0.980 kPa 2. 3. a) - 469 K b) 77 K d) 745 kPa c) 153 K d) 469 K 1.20 atm is the same pressure as: 1.2 mmHg b) 760 mmHg c) d) 850 mmHg e) 358 mmHg 912 mmHg For an ideal gas, which pair of variables are inversely proportional to each other (if all other factors remain constant)? a) P, V b) P, T 5. 99.3 kPa Liquid nitrogen has a boiling point of -196 °C this corresponds to… a) 4. c) c) V, T d) n, P A real gas would act most ideal at a) 1.0 atm and 273 K b) 10 atm and 546 K c) 10 atm and 273 K d) 0.5 atm and 546 K e) 0.5 atm and 273 K 21 7. A 31.0 mL sample of gas is collected at a temperature of 37 °C and pressure of 720 mmHg. What is its volume at 17 °C and 580 mmHg. a) 23 mL b) 27 mL c) d) 41 mL e) 58 mL 36 mL 11. What is the pressure exerted by some nitrogen gas collected in a tube filled with water on a day when the room temperature is 18.0 °C and the room pressure is 750.0 mmHg? [The partial pressure of water at 18 °C is 15.5 mmHg.] a) 15.5 mmHg b) 750.0 mmHg c) d) 760.0 mmHg e) 732.0 mmHg 734.5 mmHg 12. As the average kinetic energy of the molecules of a sample increases, the temperature of the sample a) decreases c) remains the same b) increases 13. If a gas that is confined in a rigid container is heated, the pressure of the gas will… a) increase c) remain the same b) decrease 14. A mixture of gases at 810 kPa pressure contains: 3.0 moles of oxygen gas, 2.0 moles of helium gas, and 4.0 moles of carbon dioxide gas. What is the partial pressure of helium gas, P He. a) 405 kPa b) 1620 kPa c) d) 81.0 kPa e) 180 kPa 810 kPa 18. At STP, it was found that 1.12 L of a gas had a mass of 2.78 g. Its molar mass is a) 2.78 g/mol b) 27.8 g/mol c) 55.6 g/mol d) 111 g/mol 17 Acid-Base Equilibria 1. What is the [H+] when [OH-] = 8.1 x 10-5? a) 8.1 x 10-5 M b) 1.0 x 10-7 M c) d) 3.6 x 10-6 M e) 8.1 x 10-5 M 1.2 x 10-10 M 22 2. What is the [H+] when [OH-] = 3.3 x 10-9? a) 3.0 x 10-6 M b) 1.0 x 10-7 M c) 3. e) 3.3 x 10-9 M 3.3 x 10-5 M What is the [H+] in a 0.0025 M HCl solution? a) 1.0 x 10-7 M b) 4.0 x 10-12 M c) 4. d) 6.6 x 10-5 M d) 3.6 x 10-5 M e) need more info -3 2.5 x 10 M What is the [OH-] in a 0.0050 M HCl solution? a) 5.0 x 10-3 M b) 1.0 M c) d) 6.6 x 10-5 M e) 2.0 x 10-12 M 1.0 x 10-7 M 23