Practicefinal-Troger

Practicefinal-Troger - Name: __________________________...

Info iconThis preview shows page 1. Sign up to view the full content.

View Full Document Right Arrow Icon
This is the end of the preview. Sign up to access the rest of the document.

Unformatted text preview: Name: __________________________ Date: _____________ 1. The maximum oxidation states for chromium and manganese are A) both +7. B) +7 and +8, respectively. C) +3 and +4, respectively. D) +5 and +6, respectively. E) +6 and +7, respectively. 2. What is the formula of the compound formed when potassium dichromate is dissolved in aqueous potassium hydroxide? A) K2CrO4 B) K2Cr2O7 C) CrO3 D) Cr(OH)3 E) Cr2O3 3. All of the following ligands are monodentate except A) ammine. B) cyano. C) aqua. D) carbonyl. E) oxalato. 4. What is the oxidation number of cobalt in [CoCl(NH3)5]Cl2? A) +4 B) +1 C) +6 D) +2 E) +3 5. What is the name of the complex [Cr(en)2(OH2)Cl]Cl2? A) diethylenediaminebis(aquachloro)chromium(III) chloride B) aquachlorobis(ethylenediamine)chromium(III) chloride C) chloroaquabis(ethylenediamine)chromate(III) chloride D) aquachlorobis(ethylenediamine)chromium(II) dichloride E) aquachloridebis(ethylenediamine)chromium(III) chloride Page 1 6. How many geometric isomers are possible for the complex ion [Co(NH3)3(OH2)3]3+? A) 4 B) 1 C) 0 D) 2 E) 3 7. Which of the following complexes is chiral? A) trans-[Cr(en)2Cl2]+ B) cis-[Cr(en)2Cl2]+ C) cis-[Cr(NH3)4Cl2]+ D) trans-[Cr(en)2(NH3)Cl]2+ E) [Co(OH2)3(NH3)3]3+ 8. Which of the following is expected to be the best oxidizing agent? A) Cu+(aq) B) Ti3+(aq) C) CrO42-(aq) D) VO2+ E) Cr2+(aq) 9. Which of the following would be the strongest acid in aqueous solution? A) Mg(OH2)62+(aq) B) V(OH2)62+(aq) C) Ni(OH2)62+(aq) D) Sc(OH2)63+(aq) E) Fe(OH2)62+(aq) 10. Which of the following complex ions has the largest d-orbital splitting energy? A) [Co(NH3)6]3+ B) [Co(CN)6]3C) [Co(ox)3]3D) [CoCl6]3E) [Co(OH2)6]3+ Page 2 11. Which of the following complex ions is colorless? A) [Cr(OH2)6]3+ B) [Ti(OH2)6]3+ C) [Ni(OH2)6]2+ D) [V(OH2)6]2+ E) [Zn(OH2)6]2+ 12. How many unpaired electrons are predicted for [Mn(CN)6]4-? A) 1 B) 2 C) 3 D) 5 E) 0 13. How many nucleons does boron-11 contain? A) 6 B) 10 C) 5 D) 11 E) 16 14. When an b particle is emitted, the atomic number A) increases by 4. B) decreases by 1. C) increases by 1. D) decreases by 4. E) increases by 2. 15. What nuclide undergoes a decay to produce the daughter nuclide radon-222 (Z = 86)? A) radium-226 B) thorium-230 C) polonium-222 D) protactium-230 E) uranium-236 Page 3 16. The nuclear equation for the disintegration of In-116 produces Sn-116 and A) a positron. B) helium-4. C) a neutron. D) gamma rays. E) an electron. 17. Bombarding 54Fe with a neutron results in emission of a proton and formation of A) 55Fe. B) 54Cr. C) 54Co. D) 54Mn. E) 49Ti. 18. Which of the following is most likely to undergo a decay? A) 24Na B) 47K C) 14C D) 232Th E) 3H 19. What is the element produced when 44Ti undergoes electron capture? A) Ar B) K C) Sc D) V E) Ca 20. Which of the following is most penetrating? A) a B) b C) b+ D) p E) n Page 4 21. When 214Pb decays as part of the 238U decay series, there are two a particles and four b particles lost starting with b emission from 214Pb. What is the final product? A) 207Pb B) 206Pb C) 210Bi D) 210Po E) 210Pb 22. The half-life of strontium-90 is 28.1 years. Calculate the percent of a strontium sample left after 100 years. A) 76% B) 0.34% C) 63% D) 82% E) 8.5% 23. A sample of a dish from an archaeological dig gave 18,500 disintegrations per gram of carbon per day. A 1.00-g sample of carbon from a modern source gave 22,080 disintegrations per day. If the decay constant of carbon-14 is 1.2 10-4 y-1, what is the age of the dish? A) 1500 y B) 8300 y C) 68000 y D) 640 y E) 30000 y 24. The nuclear binding energy for lithium-7 is the energy released in the nuclear reaction A) 31H + 7n 7Li B) 6Li + n 7Li C) 31H + 4b 7Li D) 31H + 4n 7Li E) 71H 7Li Page 5 25. Calculate the energy change when one 235U nucleus undergoes the fission reaction 235 U + n 142Ba + 92Kr + 2n The masses needed are 235U, 235.04 u; 142Ba, 141.92 u; 92Kr, 91.92 u; n, 1.0087 u. And there are 1.6605 x 10-27 kg/u. A) -3.2 10-28 J B) +1.8 10-10 J C) -1.7 10-10 J D) +2.9 10-11 J E) -2.8 10-11 J 26. What is the d-electron configuration of the tetrahedral complex ion [FeCl4]-? A) e2t3 B) e4t1 C) e5 D) e1t4 E) e3t2 27. A galvanic cell has in one compartment an aqueous solution of Cd+2 in contact with a Cd electrode. In the other compartment there is a 1.00M solution of Ni+2 in contact with a Ni electrode. The cell has an electromotive force of 0.240V at 25C. What is the concentration of Cd+2? The standard reduction potential of Ni2+ is -0.23 V and for Cd2+ it is -0.4V. A) 2 x 10-4 M B) 4 x 10-4 M C) 2 x 10-3 M D) 4 x 10-3 M E) none of the above 28. S2O8- (aq) + 3I- (aq) _ 2 SO4-2 (aq) + I3- (aq) This reaction has a rate constant of 4.79 M-1s-1. How long does it take for the reactant concentration to drop from 0.0720M to 0.0290M? A) 3.5 sec B) 4.3 sec C) 5.4 sec D) 6.8 sec E) 1.9 sec Page 6 29. What is the product that forms from the reaction K2O + P4O6 _ A) KPO2 B) KPO3 C) K2PO4 D) K3PO3 E) K3PO4 30. The standard reduction potential for the I2/I- electrode is +0.54 V, and the standard emf of the cell Pt(s)|I2(s)|I-(aq)|Ag+(aq)|Ag(s)| is +0.26 V at the same temperature. What is the standard reduction potential of the Ag+/Ag couple? A) +0.80 V B) -0.80 V C) +0.28 V D) -0.28 V E) none of these 31. The mechanism proposed for the reaction between nitric oxide and bromine is: Step 1: NO + Br2 NOBr2 (slow) (fast) Step 2: NOBr2 + NO NOBr + NOBr Write the rate law for the formation of NOBr A) Rate=k[NO][NOBr2] B) Rate=k[NO][Br2] C) Rate=k[NO]2[Br2] D) Rate=k[NOBr2]2 E) Rate=k[NO]2 32. Sodium azide is used to inflate protective air bags in automobiles. What mass of solid sodium azide is needed to provide 50.0L of N2 at 1.5 atm and 25C? MW sodium azide = 65.02 g/mol A) 133 g B) 138 g C) 289 g D) 298 g E) 66 g Page 7 33. The activity of a sample containing Carbon-14 is 4.7 Bq. Express this activity in millicuries. A) 1.27 x 10-5 MCi B) 1.74 x 1016 MCi C) 3.41 x 10-4 MCi D) 5.76 x 105 MCi E) 5.76 x 10-5 MCi 34. What are the decay products of 146C A) 146C + g B) 147N + 42He2+ C) 137N + 01e D) 147N + 0-1e E) It doesn't decay. 35. Which of the following reactions is the first step in forming plutonium in a nuclear reactor? A) 23892U + 10n ---> 23992U B) 23592U + 10n ---> 23692U C) 23892U ---> 23490Th + 42He D) 23892U ---> 23893Np + 0-1e E) 23592U ---> 23593Np + 0-1e 36. What is the following reaction called? 3H2 + N2 2NH3 A) Haber Process B) Ostwald Process C) Shift Reaction D) Rauschig Process E) Claus Process Page 8 37. Which of the following might be an initiation step in a chain reaction? A) Br2 + heat or light 2Br B) Br + H2 HBr + H C) H + Br2 HBr + Br D) Br + Br Br2 E) H + Br HBr . . . . . . . . . 38. Given: Ag+(aq) + e- Ag(s) Fe3+(aq) + e- Fe2+(aq) Cu2+(aq) + 2e- Cu(s) Which is the strongest reducing agent? A) Ag B) Cu2+ C) Cu D) Ag+ E) Fe2+ E = 0.80 V E = 0.77 V E = 0.34 V 39. If the standard potential for Ti3+(aq)/Ti2+(aq) is -0.37 V and the standard potential for Ti2+(aq)/Ti(s) is -1.63 V, calculate the standard potential for Ti3+(aq) + 3e- Ti(s). A) -1.19 V B) -0.40 V C) -2.00 V D) -1.26 V E) -1.21 V Page 9 40. Consider the following cell: Zn(s)Zn2+(aq, 0.100 M) m Cl-(aq, ? M)Cl2(g, 0.500 atm)Pt For this cell, E = 2.12 V and E = 2.27 V at 25C. Calculate the Cl-(aq) concentration in the cathode compartment. A) 1.2 10-1 M B) 4.3 10-5 M C) 2.9 10-3 M D) 1.5 10-3 M E) 6.5 10-3 M 41. For the reaction S2O82-(aq) + 3I-(aq) 2SO42-(aq) + I3-(aq), rate = k[S2O82-][I-]. When the reaction is followed under pseudo-first-order conditions with [S2O82-] = 200 mM and [I-] = 1.5 mM, the rate constant was 1.82 s-1. The second order rate constant, k, for the reaction is A) 1.21 103 M-1s-1. B) 6.07 103 M-1s-1. C) 9.10 M-1s-1. D) 1.37 10-2 M-1s-1. E) 1.82 M-1s-1. 42. The activation energy of a reaction is given by A) +(slope of a plot of lnk vs 1/T) R. B) -(slope of a plot of lnk vs 1/T) R. C) -R (slope of a plot of lnk vs 1/T). D) +(slope of a plot of lnk vs 1/T) R. E) -(slope of a plot of lnk vs 1/T) R. 43. Consider the following possible reactions: 1. B(OH)3(aq) + H2O(l) 2. SiH4(g) + H2O(l) (trace OH-(aq)) 3. CCl4(l) + H2O(l) 4. SiCl4(l) + H2O(l) Which of the reactions that occur are Lewis acid-base reactions? A) (3) and (4) B) (2) C) (1), (3), and (4) D) (1) E) (1) and (4) Page 10 44. What occurs when beryllium is added to aqueous sodium hydroxide? A) Be(OH)2(s) precipitates. B) Beryllium reacts to evolve hydrogen gas and form [Be(OH)4]2-(aq). C) Beryllium reacts to evolve hydrogen gas form [Be(OH2)6]2+(aq). D) O2(g) is produced. E) No reaction occurs because beryllium does not react in aqueous sodium hydroxide. 45. Calculate the emf for a Daniell Cell (E0 = 1.1 V ) with a Zn2+ concentration of 0.1M and a Cu2+ concentration of 0.1M. A) -2.2 V B) 0 V C) 1.1 V D) 2.0 V E) 2.2 V 46. Magnesium nitride dissolves in water to produce A) HNO3(aq) and MgO(s). B) N2(g) and MgO(s). C) NH3(g) and Mg(OH)2(s). D) Mg(NO3)2(aq). E) N2H4(l) and Mg(OH)2(s). 47. The geometry of PCl4+ is A) T-shaped. B) tetrahedral. C) seesaw. D) trigonal bipyramidal. E) trigonal pyramidal. 48. The oxoacids of Group 17 have the general formula HXOn where X is a halogen and n = 1 to 4. Which of the following is true? A) As the oxidation number of X increases, the strength of the acid decreases. B) As the oxidation number of X increases, the oxidizing strength of the acid increases. C) Only the oxoacids with oxidation number +1 are strong acids. D) The oxoacids with oxidation number +1 are reducing agents. E) The oxoacids with oxidation number +7 are weak oxidizing agents. Page 11 49. The products of the disproportionation of chlorine in water are A) HClO and O2 B) HClO and HCl C) ClO2 and H2 D) OH- and HCl E) HClO4 and HClO 50. The anhydride of phosphoric acid is produced by the reaction A) H3PO4(aq) HPO3(aq) + H2O(l). B) 2H3PO4(l) H4P2O7(l) + H2O(l). C) P4(s) + 3O2(g) P4O6(s). D) P4(s) + 5O2(g) P4O10(s). E) P4(g) + 3OH-(aq) + 3H2O(l) 3H2PO2-(aq) + PH3(g). Page 12 Answer Key 1. 2. 3. 4. 5. 6. 7. 8. 9. 10. 11. 12. 13. 14. 15. 16. 17. 18. 19. 20. 21. 22. 23. 24. 25. 26. 27. 28. 29. 30. 31. 32. 33. 34. 35. 36. 37. 38. 39. 40. 41. 42. 43. 44. E A E E B D B C D B E A D C A E D D C E B E A D E A D B D A C A A D A A A C E E C E E B Page 13 45. 46. 47. 48. 49. 50. C C B B B D Page 14 ...
View Full Document

This note was uploaded on 08/31/2008 for the course CHEM 21523 taught by Professor Trogler during the Spring '08 term at UCSD.

Ask a homework question - tutors are online