115年 - [無官方正解]115 亞洲大學_學士後獸醫學系招生試題：化學#144970

1. In a cathode ray tube (A) electrons pass from the anode to the cathode (B) electrons pass from the cathode to the anode (C) protons pass from the anode to the cathode (D) protons pass from the cathode to the anode

2. Which of the following elements is most likely to be a good conductor of electricity? (A) N (B) S (C) He (D) Fe

3. The scientist who determined the magnitude of the electric charge of the electron was (A) John Dalton (B) Robert Millikan (C) J. J. Thomson (D) Ernest Rutherford

4. Which of the following scientists developed the nuclear model of the atom? (A) John Dalton (B) Robert Millikan (C) J. J. Thomson (D) Ernest Rutherford

5. Which pair of elements would be most likely to form an ionic compound? (A) P and Br (B) Zn and K (C) F and Al (D) C and S

6. Identify the major ionic species present in an aqueous solution of K₂SO₄. (A) K²⁺, S⁶⁺, O₄^8– (B) K²⁺, S⁶⁺, 4O^2– (C) 2K⁺, S⁶⁺, 4O^2– (D) 2K⁺, SO₄^2–

7. Based on the solubility rules, which one of the following compounds should be insoluble in water? (A) AgBr (B) ZnCl₂ (C) MgBr₂ (D) NaCl

8. Based on the solubility rules, which one of the following should be soluble in water? (A) (NH₄)₃PO₄ (B) Ca₃(PO₄)₂ (C) AlPO₄ (D) Ag₃PO₄

9. Based on the solubility rules, which of the following will occur if solutions of CuSO₄(aq) and BaCl₂(aq) are mixed? (A) CuCl₂ will precipitate; Ba²⁺ and SO₄^{2 –} are spectator ions (B) CuSO₄ will precipitate; Ba²⁺ and Cl ^– are spectator ions (C) BaSO₄ will precipitate; Cu²⁺ and Cl^– are spectator ions (D) BaCl₂ will precipitate; Cu²⁺ and SO₄^{2 –} are spectator ions

10. The common constituent in all acid solutions is (A) H₂ (B) H⁺ (C) OH^– (D) H₂SO₄

11. The oxidation number of S in K₂SO₄ is (A) +6 (B) +4 (C) +2 (D) –1

12. In the following redox reaction 4NH₃ + 3Ca(ClO)₂ → 2N₂ + 6H₂O + 3CaCl₂ which element is oxidized and which is reduced? (A) H is oxidized and N is reduced (B) N is oxidized and Cl is reduced (C) N is oxidized and O is reduced (D)Cl is oxidized and O is reduced

13. A 50.0 mL sample of 0.436 M NH4NO3 is diluted with water to a total volume of 250.0 mL. What is the ammonium nitrate concentration in the resulting solution? (A) 21.8 M (B) 0.459 M (C) 2.18 × 10^–2 M (D) 8.72 × 10^–2 M

14. 17.5 mL of a 0.1050 M Na₂CO₃ solution is added to 46.0 mL of 0.1250 M NaCl. What is the concentration of sodium ion in the final solution? (A) 0.205 M (B) 0.119 M (C) 0.539 M (D) 0.148 M

15. A 250. mL sample of 0.0328M HCl is partially neutralized by the addition of 100. mL of 0.0245M NaOH. Find the concentration of hydrochloric acid in the resulting solution. (A) 0.00700 M (B) 0.0164 M (C) 0.0383 M (D) 0.0230 M

16. 1.40 g of silver nitrate is dissolved in 125 mL of water. To this solution is added 5.00 mL of 1.50M hydrochloric acid, and a precipitate forms. Find the concentration of silver ions remaining in solution. (A) 5.7 × 10^–3 M (B) 6.34 × 10^–2 M (C) 5.77 × 10^–2 M (D) 0.121M

17. An exothermic reaction causes the surroundings to (A)warm up (B) become acidic (C) expand (D) decrease its temperature

18. Which of the following processes is endothermic? (A) O₂(g) + 2H₂(g) → 2H₂O(g) (B) H₂O(g) → H₂O(l) (C) 3O₂(g) + 2CH₃OH(g) → 2CO₂(g) + 2H₂O(g) (D) H₂O(s) → H₂O(l)

19. To which one of the following reactions occurring at 25°C does the symbol △H°f[H₂SO₄(l)] refer? (A) 2H(g) + S(g) + 4O(g) → H₂SO₄(l) (B) H₂(g) + S(g) + 2O₂(g) → H₂SO₄(l) (C) H₂SO₄(l) → H₂(g) + S(s) + 2O₂(g) (D) H₂(g) + S(s) + 2O₂(g) → H₂SO₄(l)

20. When 0.560 g of Na(s) reacts with excess F₂(g) to form NaF(s), 13.8 kJ of heat is evolved at standard-state conditions. What is the standard enthalpy of formation (△H°_f) of NaF(s)? (A) 24.8 kJ/mol (B) 570 kJ/mol (C) –24.8 kJ/mol (D) –570 kJ/mol

21. Find the standard enthalpy of formation of ethylene, C₂H₄(g), given the following data: heat of combustion of C₂H₄(g) = –1411 kJ/mol; △H°f[CO₂(g)] = –393.5 kJ/mol; △H°f[H₂O(l)] = –285.8 kJ/mol. (A) 52 kJ/mol (B) 87 kJ/mol (C) 731 kJ/mol (D) 1.41 × 10³ kJ/mol

22. Calculate the standard enthalpy change for the reaction 2C₈H₁₈(l) + 17O₂(g) → 16CO(g) + 18H₂O(l).
Given:
2C₈H₁₈(l) + 25O₂(g) → 16CO₂(g) + 18H₂O(l)  △H° = –11,020 kJ/mol
2CO(g) + O₂(g) → 2CO₂(g)   △H° = –566.0 kJ/mol (A) 10,450 kJ/mol (B) 6,492 kJ/mol (C) 15,550 kJ/mol (D) –6,492 kJ/mol

23. Given the thermochemical equation 2SO₂ + O₂ → 2SO₃, △H°_rxn = –198 kJ/mol, what is the standard enthalpy change for the decomposition of one mole of SO₃? (A) 198 kJ/mol (B) –99 kJ/mol (C) 99 kJ/mol (D) 396 kJ/mol 

24. Which of the following processes always results in an increase in the energy of a system? (A) The system loses heat and does work on the surroundings. (B) The system gains heat and does work on the surroundings (C) The system loses heat and has work done on it by the surroundings. (D) The system gains heat and has work done on it by the surroundings.

25. For which of these reactions will the difference between △H° and △E° be the greatest? (A) 2H₂O₂(l) → 2H₂O(l) + O₂(g) (B) CaCO₃(s) → CaO(s) + CO₂(g) (C) NO(g) + O₃(g) → NO₂(g) + O₂(g) (D) 2C₂H₆(g) + 7O₂(g) → 4CO₂(g) + 6H₂O(l)

26. The elements in Group 2A are known by what name? (A) transition metals (B) halogens (C) alkali metals (D) alkaline earth metals

27. The general electron configuration for atoms of all elements in Group 5A is (A) ns²np⁶ (B) ns²np⁵ (C) ns²np⁴ (D) ns²np³

28. In what row and group of the periodic table would you find the element with the electron configuration [Kr]5s²4d¹⁰5p²? (A) row 4, group 4A (B) row 4, group 5A (C) row 5, group 4A (D) row 5, group 5A

29. Which of the following make an isoelectronic pair: Cl^– , O^2–, F, Ca²⁺, Fe³⁺? (A) Ca²⁺ and Fe³⁺ (B) O^2– and F (C) F and Cl^– (D) Cl^– and Ca²⁺

30. Which one of the following pairs are isoelectronic? (A) Mn²⁺ and Ar (B) Zn²⁺ and Cu²⁺ (C) Na⁺ and K⁺ (D) K⁺ and Cl^–

31. The cobalt(III) ion, Co³⁺, has how many 3d electrons? (A) 0 (B) 7 (C) 6 (D) 5

32. The successive ionization energies of a certain element are I₁ = 589.5 kJ/mol, I₂ =1145 kJ/mol, I₃= 4900 kJ/mol, I₄ = 6500 kJ/mol, and I₅ = 8100 kJ/mol. This pattern of ionization energies suggests that the unknown element is (A) K (B) Si (C) As (D) Ca

33. Which of the following elements has the greatest electron affinity (largest positive value)? (A) Mg (B) Al (C) Si (D) P

34. Consider the following reaction 2A + 3F₂ → 2AF₃. What is the formula for the reaction product if we substitute iodine for fluorine? (A) A₂I₃ (B) A₃I₂ (C) AI₃ (D) A₃I

35. Give the number of lone pairs around the central atom and the molecular geometry of XeF₄. (A) 0 lone pairs, tetrahedral (B) 1 lone pair, distorted tetrahedron (seesaw) (C) 1 lone pair, square pyramidal (D) 2 lone pairs, square planar

36. According to the VSEPR theory, the geometry of the _SO3 molecule is (A)pyramidal (B)tetrahedral (C)trigonal planar (D)distorted tetrahedron (seesaw)

37. According to VSEPR theory, which one of the following species has a tetrahedral geometry? (A) IF₄⁺ (B) IF₄^– (C) PCl₄⁺ (D) PCl₄^–

38. The bond angle in Cl₂O is expected to be approximately (A) 90°. (B) 109.5° (C) 120° (D) 145°

39. Indicate the type of hybrid orbitals used by the central atom in BrF₃. (A) sp (B) sp² (C) sp³ (D) sp³d

40. The number of pi bonds in the oxalate ion (C₂O₄^2–) is (A) 1 (B) 2 (C) 3 (D) 4

41. Which of the following molecular changes is necessary for mass spectrometry to occur? (A) excitation of an electron from the ground state to higher energy state (B) change of alignment of an electron in a magnetic field (C) change of alignment of a proton in a magnetic field (D) loss of an electron

42. Which of the following m/z values is the molecular ion for 2-butanone?
(A) 29 (B) 43 (C) 57 (D) 72

43. Which of the following statements best explains the information we can gain from mass spectrometry? (A) It allows us to determine the number of protons in a compound. (B) It allows us to determine the kinds of functional groups in a compound. (C) It allows us to determine the molecular weight and the mass of some fragments of a compound. (D) It allows us to determine the presence and nature of a carbocation in the compound.

44. What m/z value would you predict for the most stable fragment peak in the mass spectrum of 4-ethylheptane? (A) 128 (B) 127 (C) 113 (D) 99

45. Which of the following is not a major peak in the MS of isopentane? (A) 29 (B) 43 (C) 57 (D) 60

46. Which of the following statements best explains how a hydrocarbon can show an M+2 peak in mass spectrometry? (A) from ¹³C and 1H (B) from ¹²C and ²H (C) from a single ³H (D) from two ¹³C's

47. Which of the following characterizes the      unusually      intense peak of alkyl chlorides in MS spectrometry? (A) M + 1 peak (B) M + 2 peak (C) base peak (D) parent peak

48. Which compound's mass spectrum shows peaks at M, M+2, and M+4 whose abundances are in a ratio of 1:2:1? (A) chlorocyclohexane (B) 1,2-dichlorocyclohexane (C) 1-bromopentane (D) 1,5-dibromopentane

49. Which of the following m/z values is the base peak for benzyl alcohol? (A) 77 (B) 108 (C) 91 (D) 17

50. Which of the following compounds exhibits the pattern of m/z values shown below? 41, 43, 57, 87, 101, 116 (A) propyl bromide (B) isopropyl bromide (C) sec-butyl isopropyl ether (D) 2-hexanol

51. Which of the following is the base peak for the compound below?
(A) 92 (B) 77 (C) 57 (D) 43

52. The mass spectra of alcohols often fail to exhibit detectable M peaks but instead show relatively large ________ peaks. (A) M+1 (B) M+2 (C) M-17 (D) M-18

53. An acylium ion is often produced as a fragment in the MS of which of the following class of organic compounds? (A) ketones (B) ethers (C) alkyl halides (D) alcohols

54. Give the ion that corresponds a m/z ratio of 31 in a mass spectrum of 1-butanol. (A) (B) (C) (D)

55. Give the ion that corresponds to a m/z ratio of 56 in a mass spectrum of 1-butanol. (A) (B) (C) (D)

56. Which of the following normally occurs in a molecule when a photon of infrared light is absorbed? (A) An electron moves to an orbital of higher potential energy (B) The vibration energy increases (C) An electron changes alignment in a magnetic field (D) The molecule gains an electron

57. In the electromagnetic spectrum, ________ frequencies, ________ wavenumbers, and ________ wavelengths are associated with high energy. (A) high, small, long (B) low, large, short (C) low, small, short (D) high, large, short

58. Which of the infrared regions is considered to be the      fingerprint      region? (A) 4000cm-1 - 1000cm-1 (B) 4000μm - 1000μm (C) 2200μm - 1000μm (D) 1000cm-1 - 400cm-1

59. Which of the infrared regions is considered to be the      fingerprint      region? (A) 4000cm-1 - 1000cm-1 (B) 1000cm-1 - 400cm-1 (C) 2200μm - 1000μm (D) 4000μm - 1000μm

60. Which of the following is not a common bending vibration of a CH₂ group? (A) flip (B) rock (C) scissor (D) twist

61. Which molecule below has a significant band in the IR at 3400 cm^-1 (strong and broad)? (A) CH₃CH₂CH₂OH (B) CH₃C≡CCH₂CH₃ (C) CH₃CH₂CH(NH₂)CH₃ (D) (CH₃)₃N

62. Which molecule below has a significant band in the IR at 2220 cm^-1 (medium)? (A) CH₃CH₂CH₂OH (B) CH₃C≡CCH₂CH₃ (C) CH₃CH₂CH(NH₂)CH₃ (D) CH₃CO₂CH₂CH₃

63. Which molecule below has a significant band in the 1720 - 1780 cm^-1 range of its IR spectrum? (A) CH₃CH₂CH₂OH (B) CH₃C≡CCH₂CH₃ (C) CH₃CH₂CH(NH₂)CH₃ (D) CH₃CO₂CH₂CH₃

64. Which of the following carbonyl groups exhibits the highest wavenumber in infrared spectroscopy?
(A) I (B) II (C) III (D) IV

65. Which compound would be expected to show intense IR absorption at 2710 and 1705 cm-1? (A) CH₃COCH₂CH₃ (B) PhCOCH₃ (C) PhCHO (D) CH₂=CHCOCH₃

66. Which of the following functional groups typically exhibits a carbonyl stretch at the lowest frequency? (A) amide (B) ester (C) ketone (D) aldehyde

67. Which of the following species has a characteristic broad absorption at 3200-3500 cm^-1 in its IR spectrum? (A) PhCH₂CN (B) PhCH₂N(CH₃)₂ (C) PhCH₂CO₂CH₃ (D) PhCH₂CH₂OH

68. Which of the following carbon-hydrogen bonds exhibits the lowest wavenumber for a C-H stretch in infrared spectroscopy?
(A) I (B) II (C) III (D) IV

69. Which compound would be expected to show intense IR absorption at 3300 cm^-1? (A) CH₃CCCH₃ (B) butane (C) 1-butene (D) CH₃CH₂CCH

70. Which compound's carbonyl stretch occurs at the greatest wavenumber? (A) CH₃CH₂CH₂CHO (B) CH₃COCH₂CH₃ (C) CH₃CH₂CONH₂ (D) CH₃CH₂CO₂CH₃

71. Which molecule below has two significant bands in the IR at 2720 cm^-1 and 2820 cm^-1 (medium)? (A) CH₃COCH₂CH (B) CH₃CH₂CO₂CH₃ (C) CH₃CH₂CH₂CHO (D) CH₂=CHCH₂CH₃

72. Which of the following compounds exhibits the highest λmax in UV spectra?
(A) I (B) II (C) III (D) IV

73. Which of the following compounds absorbs the longest wavelength of UV-visible light? (A) -2-butene (B) 1-hexene (C) (Z)-1,3-hexadiene (D) -1,3,5-hexatriene

74. In the infrared spectrum, a compound of formula C4H8O gave an absorption band at 1720 cm^-1, but no bands at 2720 - 2830 and 3400 cm^-1. What is the compound? (A) 2-butanone (B) butanal (C) cis-2-butenol (D) trans-2-butenol

75. How many signals would you expect to see in the 1H NMR spectrum of the following compound?
(A) 2 (B) 3 (C) 4 (D) 5

76. How many signals would you expect to see in the 1H NMR spectrum of the following compound?
(A) 3 (B) 4 (C) 5 (D) 6

77. How many signals would you expect to see in the 1H NMR spectrum of the following compound?
(A) 1 (B) 2 (C) 3 (D) 4

78. If a chemical shift of an NMR signal is 7.2 ppm measured in a 60 MHz NMR spectrometer, how many Hz would this signal be from the TMS signal? (A) 8.3 Hz (B) 432 Hz (C) 0.12 Hz (D) 72 Hz

79. Using a 60 MHz spectrometer, the protons in dichloromethane appear at 5.30 ppm. When the same sample is placed in a 100 MHz instrument, where does the signal appear? (A) 8.33 ppm (B) 3.18 ppm (C) 5.30 ppm (D) cannot be determined from information given

80. Which of the following methyl groups will exhibit the most downfield (highest) chemical shift in 1H NMR spectroscopy?
(A) I (B) II (C) III (D) IV