Chem 1201 Sample Final Exam 2007

Chem 1201 Sample Final Exam 2007 - Final Exam, Form 1...

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Unformatted text preview: Final Exam, Form 1 Chemistry 12m Fall 2007 Group Final Exam Instructions: On SIDE TWO of the answer sheet: 1) Print your name LAST NAME FIRST and "bubble it in". 2) Print and bubble in your'LSU student ID number. 3) In the field labeled “GRADE OR EDUCATION”, bubble in "1”. On SIDE ONE: 3) Write your name and the exam "FORM #1". 4) Answers to the test questions should go on side one. There is exactly one best answer for each question and you should NOT leave a question blank. On a numerical question, choose the response closest to the correct answer.. Important Constants R = 0.08206 L atm/ (moi K) m 8.314 ]/ (mol K) Avogadro‘s constant: 1 mole = 6.023 X 1023 Planck’s constant: 11 m 6.626 x 10-3418 Speed of light (vacuum): (2 = 2.998 x 108 m/s 1 atm = 760. torr = 760. mm Hg 2 101.325 kPa 2.54 cm = 1 inch Soluble Ionic Compounds Important Exceptions Compounds containing NOS“ None CZEI3OZ" None Cl_ Compounds of Ag+, ngz‘L, and Pb2+ Bf Compounds of Ag+, Hg”, and Pb2+ I 2“ Compounds of Ag", Hgf‘“, and Pb2+ 804 Compounds of Sr“, Ba”, Hg22+, and Pb2+ Insoluble Ionic Compounds Important Exceptions CO _ . . 2... mponnds contanung 8 Compounds of NH4 ‘1", the alkali metal CO 2_ cations, and Ca”, Sr”, and Ba2+ I 3 Cccgingounds of NH4+ and the alkali metal 1 ns 3"... P04 Compounds of NH4+ and the alkali metal _ canons OH Compounds of the alkali metal cations, and Ca2+, 8332+, and Baza— W Final Exam, Form 1 page 1 1. One type of sunburn occurs on exposure to ultraviolet (UV) light of wavelength in the vicinity of 325 um. What is this wavelength in meters? a) 3.25 x 10“9 In ' b) 3.25 x 10-7 m c) 3.25 x 10~6 m cl) 3.25 x 1011mm 6) 3.25 x 10-8 m 2. How many protons, neutrons and electrons are in the neutral bromine atom, 3031“? a) 35 pt, 80 no, 35 e— b) 35 pt, 55 no, 80 e“ c) 80 pt, 35 n“, 80 e“ d) 80 pt, 55 no, 80 e" e) 35 pt, 45 119, 35 e‘ 3. Which formuia / name pair is incorrect? a) Ca(ClO4)2 / calcium perchlorate b) PCls / phosphorus pentachloride c) HNO2 / nitric acid d) Nat-121304 / sodium dihydrogen phosphate e) FeCiz / ironfll) chloride - 4. A sample of C6H1205 contains 4.38 X 1021 atoms of hydrogen. How many oxygen atoms does ‘ this sample contain? a) 2.19 X 10210 atoms b) 9.05 X 1019 O atoms 6) 7 .22 X 1022 O atoms d) 7.36 x 1022 0 atoms 6) 4.61 X 103‘} O atoms 5. What is the chemical formula of the ionic compound that can term between the two elements, rubidium and sulfur? a) RbS b) Rsz c) szS d) Rb283 c) Rb382 6. What is the mass of 22.1 moles of (CH3)20? a) 21.0g b) 31.0 g c) 102. g d) 686. g e) 1.02 x 193 g Final Exam, Form 1 page 2 V 7. Calculate the percentage by mass of chromium in potassium dichromate, KZCrQO7. a) 40.8% b) 26.6% c) 50.3 % d) 31.2% c) 35.4% 8. Consider the balanced chemical reaction shown below: _ 4 NH3(g) + 5 02(g) —> 4 NO(g) + 6 H20(g) In a certain experiment, 9.85 g of NH3 reacts with 7.04 g of 02. How many grams of H20 are produced, assuming 100% yield? a) 19.0 g b) 4.76 g c) 1.90 g d) 0.952 g c) 14.3 g 9. Write the balanced reaction between calcium oxide and carbon (graphite) to form carbon monoxide and CaCz. What is the ratio of moles of carbon to moles of carbon monoxide in the balanced chemical equation? a) lmolCtlmOICO b) 2moiC:1molCO c) 1molC23molCO d) 3molC21molCO e) 1molC:2molCO 10. Determine the empirical formula of the compound with the following composition by mass: 6.7% C, 53.7% S, and 39.6% C1. a) CSsClz b) C23Clz c) CsSsCla 'd) .CSCi __ e) CesaCl ‘ 11. An exchange reaction (metathesis reaction) is carried out with 5.00 grams of barium nitrate and excess sodium phosphate. Assuming complete reaction, What mass of solid barium phosphate is produced? a) 3.84 g b) 5.15 g c) 7.34 g d) 4.72 g c) 9.18 g Final Exam, Form 1 page 3 12. Choose the statement from below which is correct. a) 81904 is insoluble in water. 13) Be(OI~I)2 is soluble in water. 0) NaNOa. is insoluble in water. 6) HgQCEZ is soluble in water. 6) MgSO4 is insoluble in water. 13. Choose the correct balanced net ionic equation for the reaction which occurs when Fe(N03)2(aq) and NagPO4(aq) are mixed. a) FeZ+(aq) + P0421219 ——> FePO4(S) b) Na+(aq) + NO3—(aq) —> NaNO3(s) c) 3 Fe2+<ao + 2 P0437an —> Fageoms) d) 3 Fe+(aq) + P043”(aq) w» Fe3PO4(s) e) 2 Fe+(aq) + P042“(aq) m» Fe2P04(s) 14. How many grams of solute are present in 39.4 ml; of 0.729 M CaBrz? a) 5.74x103g b) 5.74g c) 1.44 x 102 g d) 0.144 g e) 2.87 x 10‘2 g 15. A 350. mL of an aqueous solution of Ca(OH)2 was titrated with 0.337 M HNOg. It required 55.8 ml. of the acid solution to neutralize the Ca(OH)2 solution. What was the concentration of the Ca(OH)2 solution in moles/liter? a) 4.90 x 1045 M b) 5.37 x 10“2 M c) 3.85 x 10""4 M a) 0.0269M e) 7.71 x 104M 16. A 50.0 mL sample of 1.00 M NaCl and a 100.0 ml. sample of 0.500 M NaCl are mixed. What is the final concentration? a) 4.00 M NaCl 13) 3.00 M NaCl c) 2.00 M NaCl d) 1.00 M NaCl e) 0.667 M NaCl Final Exam, Form 1 page 4 17. What is the energy of a photon with frequency 5.36 x 1013 8‘1? 21) 3.55 x10”20J b) 4.87x10'20f 0) 6.928104% :1) 8.81x10'293 e) 1.83 810401 18. The emission spectrum of a hydrogen atom consists of certain colors of iight. Which is the correct interpretation? a) No more than two 53‘ can occupy one orbitai. I b) The e‘ in a hydrogen atom has quantized energy ievels. c) The momentum and position of an e- cannot be simuitaneously measured. d) The wavelength of light is inversely proportional to its frequency. e) The photoelectric effect describes the kinetic energy of an ejected electron. 19. Which of the foilowing is an allowed combination of quantum numbers for an electron in a Cl orbital a) nfl2,£=2,rn.gwl b) nu3,,€m—1,m,g=—-i c) n=4,£=2,m,g=3 d) n=5,£=5,m,g:-3 e) n=6,£=2,m,g=0 20. Consider an electron with these quantum numbers: n = 3, fl = 2, 111 ,g = 0, m3 = +1/ 2 Identify a valid set of quantum numbers for a second, paired electron in the sarne orbital. a) nm3,£ =2,znrg7 =0,rns=—l/2 b) n=3,£ :2,m£ =1,rnsw+I/2 c) n=»3,£ =2,m,g m—lgms=+l/2 ($113143 =2,m_,g flw1,m5:~l/2 e) n=4,£ "—“2,rn,g zLrnsfli’l/Z Final Exam, Form 1 page 5 21. Which of the foilowing is the correct eiectronic configuration for neutrai Ge? a) [Ar] 452 3p3 b) [Ar} 352 3d10 3p2 0) [Ar} 432 4133 d) [Ar] 432 Balm 4p2 6) [Ar] 432 46.10 4133 22. Arrange the foilowing atoms in order of increasing size: P, S, C1, N, O a) P<S<C1<N<O b) O<N<Cl<S<P c) O<N<P<S<Cl d) CE<S<P<O<N e) N<O<P<S<Cl 23. What is the correct electron configuration for 1613+? a) [Kr] 4d6 b) {Kr} 531 4&5 o) {Kr} 5524(17 d) [KI] 552 4d”? 8) [K1] 5334(110 24. Which species is isoeiectronic with N3“? a) B32+ b) Se2+ c) 3212+ d) Ca2+ e) Mg2+ 25. What is the key reason Why most metals form cations relatively easily? a) Metals have small electron affinity b) Metals haVe small ionization energies e) Metals have small electronegativity d) Metals are typically smaller in radius than nonmetais e) Metals have short Bragg scattering angies Final Exam, Form 1 page 6 26. How many nonboncling electrons are if} the Lewis electron dot for phosgene, COClz. The atom arrangement has the oxygen and both chlorines attached to a ceatral carbon, like this. a) 12 e" b) 14 e“ c) l6 6"“ d) 18 e“ e) 20 e" 27. How many resonance structures are there for ozone, 03? a) 0 b) l c) 2 d) 2.5 e) 3 28. Which of these molecules contains the most polar covalent bond(s)? a) SiF4 b) F2 0) OF2 d) NF3 e) CF4 29. Below are three pictures of different types of hybrid orbitals. Each picture shows only two of the possible hybrid orbitals. Which statement is true? Copylfigbl @2055 Pearson Prentice Hall, inc. (1) (II) (III) a) The orbitals in picture I are sp hybridized. b) The orbitals in picture I could be found in a tetrahedral geometry. 0) The orbitals in picture II are Sp2 hybridized. d) The orbitals in picture III are sp3 hybridized. e) The orbitals in picture III could be found in a trigonal planar geometry. Final Exam, Form 1 page 7 30. What are the eieetron domain and moiecular geometries of the ion, CIFf ? a) trigonai planar, bent ' b) trigonal bipyramid, linear c) trigonal bipyramid, T—shaped (1) linear, linear e) tetrahedral, beat 31. What is the formal charge on phosphorus in the hexafluorophosphate anion, PFs”? a) +2 13) +1 0) 0 d) —1 e) m2 32. Determine the temperature, in Celsius, for 50.0 g of water vapor in a sealed 22.4 L tank with a pressure of 1.00 MPa. 1 atm = 101,325 Pa a) 273 °C b) 288 °C o) 350 °C ' d) 698 8C e) 723 °C 33. What is the partial pressure of oxygen in the Earth’s atmosphere at sea level. The moie fraction of oxygen is 0.2095. Assume a totai pressure of 760. torr. a) 601 torr 1)) 15,922 torr c) 209.5 torr d) 159 torr e) 760 torr 341. The density of air at sea 1eve1 at 20.0 °C is 1.212 g/ L. What is the density of hydrogen gas at the same temperature and pressure? The average molar mass of air is 29.1466 55/ mol. a) 1.212 g/L ' 13) 0.0419 g/L o) 1.23 g/L (:1) 0.0838 g/L 6) 0.000827 g/L Final Exam, Form 1 page 8 35. A balloon with a 1.73 L volume at 270 GC is heated to 52.0 0C at constant pressure. What volume does the gas oocupy at the higher temperature? The number of moles is constant. a) 1.24 L b) 187 L e) 3.46 L d) 2.41 L e) 3.33 L 36. What is/are the physical states present at T m 200 K and P = 1.0 atm? 10 E :2 3 a 0.5_; a 9—: 0 too 200 300 400 Temperature (K) Copyfighl o 2005 Pearson firenliea Mail Inc. a) both solid and liquid states b) both solid and gas states 0) liquid state (1) solid state e) gas state 37. Which species is predicted to have the highest boiling point? a) GeBm b) GeClz; c) CH4 6) CC14 e) SiClz; 38. Which of the following molecules can form hydrogen bonds? a) CH3CN b) £1202 c) CH30CHs d) HzS e) CH4 Final Exam, Form 1 page 9 39. 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What is the wavelength (9») of the radio waves, and what is the energy (E) of one of the associated photons? a) l=3.36m E=5.92><10'26I b) Awassuo‘ém E21.12xi0"81 c) l=3.36x106m. E=5.92x10‘321 d) am2.58x1o“m Emmzx 10421 e) a=298~x 104131 E=6.68x10'251 2) The molecule H200 contains a) 3 sigma bonds and 0 pi bonds 1)) 3 sigma and 1 pi bond c) 2 sigma and 1 pi bond d) 1 sigma and 2 pi bonds e) 3 pi and 0 sigma bonds 3) Choose which intermolecular forces are present in a solid sample-of CH‘gF? (i) London dispersion force (ii) dipole—dipole force (iii) hydrogen bonding force a) only b) (ifi) only c) (i) and (ii) (1) (iii) only 6) (i): (ii) and (iii) 4) What is the mass of a sample of carbon dioxide that contains 6.00 X 103‘ molecules?! a) 4.38 x 10"9 g b) 9.96 x 10'21 g c) 1.59 x1029g s) 4.53 >< 1022 g e) 2.26 x 10“22 g Page 1 Chemistry 1201, Fall 2008 Final Exam, Form 4 5) Which one of the following is an approximate bond angle in‘a molecuie with trigonal planar electron domain geometry and bent molecular geometry? a) 1095" b) 90° c) 120° (1) 180° e) 60° 6) Which one of the following statements correctly describes the polarity of dibromodichlorosilane, SiBrZClz? a) SiBr2012 is expected to be nonpolar even though it has polar bonds. b) SiBl‘zClg is expected to be polar because it has polar bonds and is not perfectly symmetrical. c) SiBr2C12 is expected to be nonpolar because it has nonpolar bonds. (1) SiBl'zClz is expected to be polar due to the presence of a non—bonding (lone) pair on Si. e) 8113mm; is expected to be nonpoiar because the bond dipoles cancel. 7) Which one of the following isoelectronic ions has the largest radius? a) N3“ b) A1“ 0) N2?" (1) 02‘ e) F“ 8) When the following equation is balanced with the smallest whole numbers, what is the stoichiometric coefficient of nitric acid? WN205(g) + __H20(l) ——+ ___HN03(aq) a) l b) 5 c) 4 d) 3 e) 2 9) Sulfur trioxide is made from the reaction of sulfur dioxide and oxygen. How many grams of 803 can be made from the reaction of 1.91 g SO; with 1.29 g 03? a) 3.20 g b) 2.39 g c) 3.23 g d) 6.46 g e) 4.77 g Page 2 Chemistry 1201, Fall 2008 Final Exam, Form4 10) This figure shows 10 neon atoms in a 1 mL box at room temperature. What would happen to the partial pressure of neon if l0 oxygen molecules were added to the box (assume there is no change in temperature or volume)? a) The partial pressure of neon would be twice the partial pressure of oxygen. 13) The partial pressure of neon would increase 0) The partial pressure of neon would not change :1) ’E‘he partial pressure of neon would decrease _ e) The partial pressure of neon would be half the partial pressure of oxygen. 11) What is the enthalpy change for the production of dihydroxyacetone, a component in quick—tanning lotions, as shown in the reaction below? i i i i if i eriwc~cmn + 0:0 We» n—-o———-CI:——C—-cl:—o——H H H H H a) +1324k5 b) ~1642k} c) +901<J d) —524kf e) ~318k1 12) Which three elements are likely to have simiiar chemical and physical properties? a) calcium, strontium, and Barium b) nitrogen, oxygen, and neon c) sodium, magnesium, and aluminum (1) nickel, cepper, and zinc e) hydrogen, oxygen, and carbon Page 3 Chemistry 1201, Fa112008 Final Exam, Format 13) Which Lewis structure is preferred for CFClO? .‘3. 00¢ a. i no a) :Fmewcr: flQ ti 18¢ 90: b) up. i so. flame. to: C) I?! 00 :F—HCWW it. to O. :0: d) 'ma of; C .. o". O 0 14) What volume of 0.110 M NaOH(aq) is needed to react completely with 13.8 mL of 0.176 M H3P04(aq)? __ 1-13P04(aq) + _ NaOH(aq) —+ W Na3P04(aq) +_ __ H200) a) 86.3mL b) 22.1mL 0) 7.36m d) 25.9mL e) 66.2mL 15) What is the empirical fonnula of a compound that contains 29% Na, 41% S, and 30% 0 by mass? a) NaSO: b) NaSO C) N32S203 d) NaSO; e) Na28205 16) Given the unidentified isotope 3X ,whieh one of the following is true? a) The atom contains 34 protons. b) The atom contains 61 neutrons. e) The element must be promethium , Pm. d) The neutral atom contains 27 electrons. e) The number of protons plus electrons in the atom equals 61. Page 4 Chemistry 126}, Fall 2008 Final Exam, Formé ' 17) What is the density of air (average moiar mass = 29.0 g/moi) at 2.1.0 “C and a pressure of 741 torr? a) 0.855 g/mL 1)) 0.00117 g/mL 0) 0.0522 g/L d) 1.17 gfL c) 0.855 g/L 159111 the following Lewis structure, G; Q, T, X, Y, and Z represent elements in the first two rows of the periodic table (H through Ne). Identify element G so that its formal charge is zero. .T: X .. II I :jaf—G—IQ-I-Z a) ‘H b) O C) d) F e) C 19) What is the correct answer to the following expression: (49.1 — 42.61) x 13.1? a) 85.02 b) 85 c) 9x102 (1) 85.019 6) 85.0 20) Which atom is got listed with its correct eiectron configuration? 5.) Fe: [Ar] 432 3d6 b) Hg: {Xe16325d10 6) Ge: [Ar]4s23d1°4p2 (1) Ti: [Ar}4s23d2 6) Be: [He] 232 210111 an atom, what is the maximum number of electrons that can have the three quantum numbers n=4, l=2,m;=~1? a) 32 b) 4 c) 1 d) 1 0 e) 2 Page 5 Chemistry 1201, Fall 2008 Final Exam, Forms ' 22) What is the hybridization of the central atom in a molecule with see-saw'molecular geometry? a) Sps b) Alpsd2 0) S}? d) spsd 6) spz 23) Which one of the following is a description of a compound which, when added to water, becomes a strong electrolyte? a) A weak base which exists as a mixture of molecules and ions in solution. ‘ b) A molecular compound which exists entirely as molecules in solution. e) A weak acid which exists as a mixture of molecules and ions in solution. (1) A strong acid which exists entirely as ions in solution. ' ‘ e) An insoluble salt which doesn’t dissolve in solution. 24) Choose the phrase which "best describes the NwO bonds of N02" , the nitrite ion: a) one bond is a single bond and the other is a double bond. b) each bond is a single bond. 0) one bond is a single bond and the other is a triple bond. cl) each bond has an intermediate bond order between a single and double bond. 6) each bond is a double bond. 25) Barium reacts with polyatomic ion X to form a compound with the fonnula Ba3X2. What would be the most likely formula for the compound formed between sodium and X? a) NagX b) NaX' c) NagX (1) Nang e) N32X2 Page 6 Chemistry 1201, Fall 2008 Final Exam, Form‘é' ' 26) Consider the following diagram: rm: added {3) Which one of the following best describes Why the temperature does not increase during phase change D "e E even though heat is being added to the system during these steps? a) The added heat only causes atoms Within molecules to rearrange. b) The added heat only increases the velocity of the molecules. ' c) The added heat only breaks bonds Within molecules. d) The added heat only overcomes intermolecular forces. e) The added heat only increases the density of the sample. 27) Consider the elements in group 2A. Which of the following statements is/are not correct? (i) 2A elements form ions with +2 charges. a ' (ii) 2A elements generally have larger radii than 1A elements in the-same row. (iii) 2A elements have the general valence shell electron configuration nsz. (iv) 2A elements have very high third ionization energies. a) (ii), (iii) and (iv) b) (ii) only c) (ii) and (iii) (1) (i) only eowwmw 28) The neutralization reaction between HCl(aq) and KOH£aq) produces a) potassium oxide b) hydrogen gas c) oxygen gas d) potassium hydroxide e) water and a salt Page 7 Chemistry 1201, Fall 2008 Final Exam, Form _4 ' 29) A pressurized steel cylinder of helium has an internal pressure of 1.08 atm at 250 °C. If the cylinder is placed in a freezer at —10.0 °C, what is the new value of its internal pressure? a) 1.08 atm b) 3.20 atm c) 0.697 atm d) 1.47 atm e) 0.953 atm 30) Which one of the following molecules is polar? a) 302 r 13) C02 C) SE5 (1) BF; e) XeF4 3 1) What is the molarity of CH30H in a solution prepared by dissolving 11,7 g of CH30H in enough water to make 230. mL of solution? a) 11.7M b) 0.0513M c) 1.59M d) 0.627M e) 3.22M 32) In this diagram, all of the gases are at the same temperame: z . . .9 " 5%102 mile- ,25 0x103 m? Speed (Hi/Si.) Fraction of molecules within 30 sin/’3 of indicated speed The diagram illustrates that a) gases with lower masses have higher rms speeds. in) there is no correlation between mass and rms Speed. 6) gases with higher masses have higher rms speeds. d) polar molecules have higher rms Speeds. e) nonpolar molecules have higher rms speeds. Page 8 Chemistry 1201, Fall 2008 Final Exam, Form4 33) Which one of the following has 3 unpaired electrons in its ground electronic state? a) B b) V" c) 0 d) Co 6) N“ Page 9 ...
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Chem 1201 Sample Final Exam 2007 - Final Exam, Form 1...

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