Exam2-S01 - Chemistry 12 Exam II Form A February 28, 2001...

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Unformatted text preview: Chemistry 12 Exam II Form A February 28, 2001 Name ____________________ Section ____________________ Student No. ____________________ IMPORTANT: On the scantron (answer sheet), you MUST clearly fill your name, your student number, section number, and test form (white cover = test form A; yellow cover = test form B). Use a #2 pencil. 1. From the following heats of reaction: 2SO2 (g) + O2 (g) ! 2SO3 (g) 2S (s) + 3O2 (g) ! 2SO3 (g) ∆H = −196 kJ ∆H = −790 kJ calculate the heat of reaction to form SO2 from sulfur and oxygen according to the following equation: S (s) + O2 (g) ! SO2 (g) a. + 395 kJ b. + 202 kJ c. −297 kJ d. −398 kJ e. −594 kJ ___________________________________________________________________________ 2. Calculate ∆Horxn for neutralization reaction that occurs between NaOH and HCl. ∆Hof (NaOH) (aq) = −469.6 kJ/mol ∆Hof (NaCl)(aq) = −407.1 kJ/mol ∆Hof (HCl) (aq) = −167.2 kJ/mol ∆Hof (H2O) (l) = –285.8 kJ/mol There are 25 questions on this exam. Check that you have done all of the problems and filled in the first 25 bubbles on the scantron. The maximum score on this exam is 20 points. • • Calculators with text-programmable memory are not allowed. Relevant data and formulas, including the periodic table, are attached at the end of this exam. Your grade will be based only on what is on the scantron form. The answer key will be posted on the web after the exam (under "News"). Hints • • +515.5 kJ –390.5 kJ –1329.7 kJ +29.1 kJ –56.1 kJ _____________________________________________________________________________ Exam policy • • a. b. c. d. e. As you read the question, underline or circle key words to highlight them for yourself. Avoid errors from "mis-reading" the question. There is no penalty for guessing. 1 3. Which of the following is the ground-state electron configuration of K+? a. b. c. d. e. [Ar]4s1 [Ar]3d10 [Ar]4s2 [Ar] [Ar]4s13d1 ______________________________________________________________________________ 2 4. How much energy is required to heat 20 g of water from 22 oC to 37 oC? The specific heat of water is 4.18 J/(gK). a. b. c. d. e. 8. The first four ionization energies (I) for an atom are given below. I1: 578 1839 J 1254 J 3093 J 177 J 105 J I2: 1820 I3: 2750 I4: 11,600 (all in kJ/mol) What is the atom represented? ______________________________________________________________________________ a. b. c. d. e. sodium aluminum chlorine silicon neon 5. How many unpaired electrons are there in the ground-state of Cu? ___________________________________________________________________________ a. b. c. d. e. 0 1 2 3 4 9. Which of the following atoms is the most electronegative? ______________________________________________________________________________ 6. Which of the following ionic solids has the largest lattice energy? a. b. c. d. e. LiCl KCl RbCl BaO SrO a. francium b. lithium c. chlorine d. oxygen e. fluorine ___________________________________________________________________________ 10. Which of the following species has the smallest radius? ______________________________________________________________________________ 7. A Lewis structure of SO3 is shown below. How many additional resonance structures equivalent to the one shown can be drawn for this molecule? a. b. c. d. e. Ne F– O2– Cl Cl– ____________________________________________________________________________ 11. Which of the following bonds will be non-polar? O O a. b. c. d. e. S O none one two three four a. b. c. d. e. Li─H H─F H─Cl O─O O─H _____________________________________________________________________________ ______________________________________________________________________________ 3 4 12. The following pictures present s (I), p (II), d (III), and f (IV) orbitals. Which of these orbitals can have the quantum number ml = −2? I) 15. Which of the following is a permissible set of quantum numbers? a. b. c. d. e. II) n 2 3 2 3 2 l −1 2 −3 2 3 ml +2 −3 −2 −2 0 ms +1/2 −1/2 −1/2 +1/2 +1/2 __________________________________________________________________________________________ III) IV) 16. Which of the following orderings of atom/ion radii is incorrect? a. I– > I > I+ b. Ca2+ > Mg2+ > Be2+ c. Fe > Fe2+ > Fe3+ d. K+ > Cl– > S2– e. Br > Cl > F ____________________________________________________________________________ a. III only b. II and III only c. IV only d. III and IV only e. I, II, III and IV ____________________________________________________________________________ 13. Which of the following photons of the electromagnetic radiation has the highest energy? a. orange light with λ = 645 nm b. radio-wave with frequency of 700 MHz (λ = 43 cm) c. microwave with λ = 2 cm d. ultraviolet light with frequency of 3 x 1015 s-1 (λ = 100 nm) e. infrared light with λ = 6 µm (= 6 x 10-6 m) __________________________________________________________________________ 14. Of the following isoelectronic species, which one has the smallest size? a. S2– b. Cl– c. Ar d. K+ e. Ca2+ ______________________________________________________________________________ 5 17. Bromine is much more apt to exist as an anion than is potassium. This is because: a. b. c. d. e. Bromine is bigger than potassium. Bromine has greater (more positive) ionization energy than potassium does. Bromine has greater (more negative) electron affinity than potassium does. Bromine is a gas and potassium is a solid. Bromine is more metallic than potassium. ______________________________________________________________________________ 18. Based on the positions of the elements in the periodic table, which of the following bonds is the most polar? a. b. c. d. e. P─N P─O P─Si P─S P─C ______________________________________________________________________________ 6 19. What is the formal charge on phosphorus in the following Lewis structure of PO43─? 3- O O a. b. c. d. e. P O O a. –2 b. –1 c. 0 d. +1 e. +2 _____________________________________________________________________________ 20. Which of the following drawings is the best Lewis structure for nitrate ion (NO3–)? Other structures (that are equally good) may exist, but are not shown here. a. O N O O b. O N O N d. O O N O - O - O c. O - 4s 4p 4d 4f 5s _____________________________________________________________________________ 23. Which quantum number defines the shape of the orbital? a. b. c. d. e. principal (n) azimuthal (l) magnetic (ml) spin (ms) magnetic and spin (ml and ms) _____________________________________________________________________________ - O 22. In a given multielectron atom, which subshell electrons experience the largest effective nuclear charge? e. O N O 24. What is the value of the azimuthal quantum number (l) for the outermost electrons in a ground state oxygen atom? a. b. c. d. e. 0 1 2 3 4 ______________________________________________________________________________ 25. Which of the following transitions in the Bohr hydrogen atom affords emission of the highest-energy photon? O __________________________________________________________________________ 21. Which of the following statements is false? a. Metals tend to have lower ionization energies than nonmetals b. A neutral element that readily accepts electrons, such as F, has an exothermic electron affinity. c. When a neutral atom loses an electron, its radius increases. d. Nonmetals are more electronegative than metals. e. As one goes across a period from left to right, the radii of the neutral atoms generally decrease. _____________________________________________________________________________ 7 a. ni = 1 ! nf = 4 b. ni = 4 ! nf = 1 c. ni = 4 ! nf = 2 d. ni = 2 ! nf = 4 e. ni = 1 ! nf = 2 ______________________________________________________________________________ END OF EXAM 8 PERIODIC TABLE of the ELEMENTS (2001) Constants & Equations 2 -2 MAIN GROUPS 1 J = 1 kg· m ·s RH = 2.18 × 10-18 J c = 3.00 × 108 m·s-1 e = –1.60 × 10-19 C h = 6.63 × 10-34 J·s 23 N = 6.02 × 10 mol 1 D = 3.33 × 10-30 C·m MAIN GROUPS 1A 1 1 H 1.008 3 8A 18 2 Li 9.012 11 E = hν 20 1 1 ∆E = R H 2 − 2 n nf i λ= h mv E = kL Q1Q2 d 7B 7 25 4B 4 22 5B 5 23 V Cr Mn 47.867 50.942 51.996 54.938 Ca Sc 40.078 44.956 4.003 F Ne 12.011 14.007 15.999 18.998 20.180 C N O 10 Ti 14 15 16 S Cl Ar 26.982 28.086 30.974 32.066 35.453 39.948 58.693 Cu Zn Ga Ge As Se Br Kr 63.546 65.39 69.723 72.61 74.992 78.96 79.904 83.80 45 46 35 36 Zr Nb Mo Tc Ru Rh Pd Ag Cd 48 49 In Sn Sb Te 52 53 I Xe 91.224 92.906 95.94 [98] 101.07 102.90 106.42 107.87 112.41 114.82 118.71 121.76 127.60 126.90 131.29 83 84 85 54 Cs Ba La* Hf Ta 73 74 W Re Os 76 77 Ir Pt Au Hg 80 81 Tl Pb Bi Po At Rn 132.91 137.33 138.91 178.49 180.95 183.84 186.21 190.23 192.22 195.08 196.97 200.59 204.38 207.2 208.98 [209] [210] [222] 88 82 51 34 18 Y 79 50 33 17 39 78 47 32 P 88.906 75 44 31 Si 38 72 43 58.933 Al Sr 57 42 Ni 55.845 1B 11 29 87.62 56 41 Co 8B 10 28 Rb 55 40 Fe 8B 9 27 8B 8 26 85.468 87 µ = Qr 6B 6 24 3B 3 21 39.098 37 7A 17 9 13 Mg 24.305 K c = λν 6A 16 8 2B 12 30 12 Na 19 5A 15 7 B TRANSITION METALS 22.990 -1 4A 14 6 10.811 Be 6.941 He 3A 13 5 2A 2 4 86 Fr Ra Ac** 89 104 105 106 107 108 109 110 111 112 114 116 118 [223] [226] [227] [261] [262] [266] [264] [265] [268] [269] [272] [277] [285] [289] [293] Rf Db 58 Sg 59 Bh 60 Hs 61 Mt 62 63 64 65 66 67 68 69 70 71 q = m · c · ∆T Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu 140.12 * LANTHANOIDS 140.91 144.24 [145] 150.36 151.96 157.25 158.92 162.50 164.93 167.26 168.93 173.04 174.97 90 ** ACTINOIDS ∆H°rxn = Σ n ∆H°f (products) − Σ m ∆H°f (reactants) Th Pa 91 92 U Np Pu Am Cm Bk Cf Es Fm Md 101 102 103 232.04 321.04 238.03 [237] 93 [244] 94 [243] 95 [247] [247] [251] [252] [257] [258] [259] [262] 10 9 96 97 98 99 100 No Lr ANSWER KEY Chem 12 Exam II Spring 2001 1. C 2. E 3. D 4. B 5. B 6. E 7. C 8. B 9. E 10. A 11. D 12. D 13. D 14. E 15. D 16. D 17. C 18. B 19. C 20. D 21. C 22. A 23. B 24. B 25. B 11 ...
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This note was uploaded on 05/24/2009 for the course CHEM 110 taught by Professor Hofmann,brucerob during the Fall '08 term at Pennsylvania State University, University Park.

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