terminator812>試卷(2019/06/19)

# 106 年 - 高雄醫學大學 106 學年度學士後醫學系招生考試試題-化學#77049

1.16. Select the answer with the correct number of decimal places for the following sum: 13.914 cm + 243.1 cm + 12.00460 cm =
(A) 269.01860 cm
(B) 269.0186 cm
(C) 269.019 cm
(D) 269.02 cm
(E) 269.0 cm

2.17. The difference between a student's experimental measurement of the density of sodium chloride and the known density of this compound reflects the ___________ of the student's result.
(A) accuracy
(B) precision
(C) random error
(D) systematic error
(E) indeterminate error

3.18. The average mass of a carbon atom is 12.011. Assuming you were able to pick up only one carbon unit, the chances that you would randomly get one with a mass of 12.011 is ___________.
(A) 0%
(B) 0.011%
(D) 12.011%
(E) greater than 50%

4.19. A catalyst ___________.
(A) changes the enthalpy of the reaction
(B) does not change the activation energy
(C) provides an alternate pathway to the reaction
(D) does not change the effective collisions
(E) is consumed when more reacting molecules are added

5.20. For a gas sample, which conditions of P (pressure), T (temperature), and n (molar number), respectively, are most ideal?
(A) high P, high T, high n
(B) low P, low T, low n
(C) high P, low T, high n
(D) low P, high T, high n
(E) low P, high T, low n

6.

21. One mole of an ideal gas at 20 °C is expanded isothermally and reversibly from 100 L to 200 L. Which statement is correct?
(A)△ Sgas = 0
(B) △ Ssurr = 0
(C) △ Suniv = 0
(D) △ Sgas = Rln2
(E) △ Sgas = △Ssurr

7.22. Which of the following ionic compounds has the largest lattice energy?
(A) LiF
(B) NaCl
(C) MgO
(D) KBr
(E) BaCl2

8.23. Which of the following species has a trigonal bipyramid structure?
(A) IF5
(B) I3
(C) NH3
(D) PCl5
(E) All of the above.

9.24. Naturally occurring copper exists in two isotopic forms: 63Cu and 65Cu. The atomic mass of copper is 63.55 amu. What is the approximate natural abundance of 63Cu?
(A) 70%
(B) 63%
(C) 90%
(D) 50%
(E) 30%

10.25. Mixing 20 mL of a 4.0 M sodium chloride solution with 40 mL of a 2.0 M calcium chloride solution results in a solution with a chloride ion concentration of  M.
(A) 2.67
(B) 3.33
(C) 4.00
(D) 4.33
(E) 5.00

11.26. How many electrons in an atom can have the quantum numbers n = 4, l = 1?
(A) 2
(B) 6
(C) 10
(D) 18
(E) 32

12.27. The following reaction takes place at 120 °C: H2O(l) → H2O(g) , ΔH = 44.0 kJ/mol, ΔS = 0.119 kJ/mol·K. Which of the following must be true?
(A) The reaction is not spontaneous.
(B) The reaction is spontaneous.
(C) ΔG < 0
(D) Two of these.
(E) None of the above.

13.28. How many σ bonds and π bonds are there in H3C–CH2–CH CH–CH2–C CH ?
(A) 16, 3
(B) 13, 2
(C) 10, 2
(D) 10, 3
(E) 14, 3

14.29. ________________ is a method of separation that employs a system with two phases of matter, including a mobile phase and a stationary phase.
(A) Chromatography
(B) Distillation
(C) Homogenization
(D) Vaporization
(E) Filtration

15.30. Which of the following is an example of nitrogen fixation?
(A) Absorption of NH3 and its transformation into to N2.
(B) Absorption of NH3 and its transformation into to NO2.
(C) Absorption of N2 and its transformation into elemental nitrogen.
(D) Absorption of N2 and its transformation into NH3.
(E) Absorption of nitric acid and its transformation into N2.

16.61. A solution contains the ions Ag+ , Ba2+, and Ni2+. Dilute solutions of NaCl, Na2SO4, and Na2S are available to separate the positive ions from each other. In order to effect separation, the solutions should be added in which order?
(A) Na2S, NaCl, Na2SO4
(B) Na2SO4, NaCl, Na2S
(C) Na2SO4, Na2S, NaCl
(D) NaCl, Na2S, Na2SO4
(E) NaCl, Na2SO4, Na2S

17.重新載圖

62. Which of the statements below correctly describes the combustion of glucose, shown below?
(A) Hydrogen in C6H12O6 is being reduced.
(B) Oxygen in O2 is being oxidized.
(C) Hydrogen in C6H12O6 is the reducing agent.
(D) Oxygen in C6H12O6 is the oxidizing agent.
(E) Carbon in C6H12O6 is being oxidized.

18.63. Reaction intermediates differ from activated complexes in that ________.
(A) they are stable molecules with normal bonds and are frequently isolated
(B) they are molecules with normal bonds rather than partial bonds and can occasionally be isolated
(C) they are intermediate structures which have characteristics of both reactants and products
(D) they are unstable and can never be isolated
(E) all reactions involve reaction intermediates, but not all have activated complexes

19.重新載圖

64. Select the Lewis structure for XeO2F2 which correctly minimizes formal charges.
(A)
(B)
(C)
(D)
(E)

20.65. Which species has the highest bond order?
(A) NO+
(B) O2
(C) O2
(D) O2 2−
(E) NO

21.66. What hybridization is present in the phosphorus atom in PCl3 and PCl5, respectively?
(A) sp 2 , d 2 sp 3
(B) sp 2 , dsp3
(C) dsp, dsp3
(D) sp 3 , d 2 sp 3
(E) sp 3 , dsp3

22.67. The spectrochemical series is I < Br< Cl < F < OH< H2O < NH3 < en < NO2 < CN . Which of the following complexes will absorb visible radiation of the highest energy?
(A) [Co(H2O)6] 3+
(B) [CoI6] 3–
(C) [Co(OH)6] 3–
(D) [Co(en)3] 3+
(E) [CoCl6] 3–

23.重新載圖

68. A diprotic acid H2A has Ka1 = 1 x 10–4 and Ka2 = 1 x 10–8 . The corresponding base A2– is titrated with aqueous HCl, both solutions being 0.1 mol/L. Which one of the following diagrams best represents the titration curve which will be seen?
(A)
(B)
(C)
(D)
(E)

24.69. Which of the following coordination compounds will form a precipitate (AgCl) when treated with an aqueous solution of AgNO3?
(A) [Cr(NH3)3Cl3]
(B) [Cr(NH3)Cl]SO4
(C) Na3[Cr(CN)6]
(D) [Cr(NH3)6]Cl3
(E) None of the above.

25.70. If a complex ion is square planar, which d-orbital is highest in energy?
(A) dx2-y2
(B) dx2
(C) dxy
(D) dyz
(E) dxz

26.71. Which of the following statement is incorrect about hydrocarbons?
(A) Breaking the C─H bonds separately of CH4 requires different energies.
(B) The average C─H bond energy of CH4 is higher than that of H─H.
(C) Hydrocarbons are hydrophobic.
(D) Longer alkanes are with higher viscosities than shorter ones.
(E) Branched alkanes are with lower boiling points than their corresponding straight isomers.

27.重新載圖

72. Which of the following molecules is an optically active molecule?
(A)
(B)
(C)
(D)
(E) None of the above.

28.重新載圖

73. The structure below is the repeating unit of a
(A) homopolymer formed by an addition reaction.
(B) homopolymer formed by a condensation reaction.
(C) copolymer formed by an addition reaction.
(D) copolymer formed by a condensation reaction.
(E) polyester formed by an addition reaction.

29.重新載圖

74. Identify the products of the reaction of 3-octene with chlorine.
(A)
(B)
(C)
(D)
(E)

30.75. Which of the following statements about molecular spectroscopies is incorrect?
(A) Ultraviolet-visible (UV-vis) spectra provides information about HOMO-LUMO gap.
(B) Infrared (IR) spectra gives information on bond vibrational transitions.
(C) Rotation transitions occur in the microwave region.
(D) Nuclear magnetic resonance (NMR) spectra provides information about the electronic transitions.
(E) UV-vis spectra involves both the molecular ground state and the excited state.

31.重新載圖

76. Consider the following reaction: . The equilibrium constant K is about 0.0196 at 115 °C. Calculate Kp at this temperature?
(A) 0.196
(B) 0.624
(C) 0.285
(D) 22.9
(E) 2.9

32.重新載圖

77. The equilibrium constant for reaction
(A) K 4
(B) 4K
(C) 1/4 K
(D) 1/K4
(E) - K 4

33.78. The pH of a 0.005 M K2O aqueous solution should be ________.
(A) 11.7
(B) 7.0
(C) 2.3
(D) 12.0
(E) 5.0

34.

79. How long will it take to produce 18.2 g of Ag (atomic mass = 107.87 amu) from a solution of AgNO3 using a current of 10.00 amp? (F = 96500 C/mol)
(A) 3.26✖103 s
(B) 8.14✖102 s
(C) 4.88✖103 s
(D) 1.63✖103 s
(E) 5.43✖103 s

35.80. Given Cu2O(s) + 1/2O2(g) → 2CuO(s) , ΔH° = −144 kJ and Cu2O(s) → Cu(s) + CuO(s) , ΔH° = +11 kJ Calculate the standard enthalpy of formation of CuO(s) .
(A) −155 kJ
(B) +299 kJ
(C) +155 kJ
(D) −299 kJ
(E) −166 kJ

36.重新載圖

81. Calculate E°cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous.   Overall reaction: MnO4(aq) + 2H2O(l) + 3Co2+ (aq) MnO2(s) + 3Co3+(aq) + 4OH(aq)
(A) E°cell = –1.23 V, spontaneous
(B) E°cell = –1.23 V, nonspontaneous
(C) E°cell = 1.23 V, spontaneous
(D) E°cell = 1.23 V, nonspontaneous
(E) E°cell = –0.05 V, nonspontaneous

37. 82. The successive packing pattern for a hexagonal closest packed structures is which of the following?
(A) ABCABC
(B) ABCCBA
(C) ABABAB
(D) ABAABA
(E) AABBAA

38.重新載圖

83. Identify the missing particle in the following equation:
(A)
(B)
(C)
(D)
(E) None of the above.

39.84. How many valence electrons are there in an atom with the electron configuration [noble gas]ns 2 (n – 1)d 10 np 3 ?
(A) 2
(B) 3
(C) 5
(D) 10
(E) 15

40.85. For the process CHCl3(s) → CHCl3(l) , ΔH° = 9.19 kJ/mol and the melting point of chloroform is –64 °C. Calculate ΔS° ?
(A) 43.9 J/mol/K
(B) 53.9 J/mol/K
(C) 26.3 J/mol/K
(D) 75.2 J/mol/K
(E) None of the above.

41.86. Atomic orbitals developed using quantum mechanics ________.
(A) describe regions of space in which one is most likely to find an electron
(B) describe exact paths for electron motion
(C) give a description of the atomic structure which is essentially the same as the Bohr model
(D) allow scientists to calculate an exact volume for the hydrogen atom
(E) are in conflict with the Heisenberg Uncertainty Principle

42.87. Which of the following species requires the highest energy to remove an electron from its valence shell?
(A) Na+
(B) F
(C) K
(D) Cl
(E) Mg2+

43.88. A reaction was found to be zero order in X. Increasing the concentration of X by a factor of 5 will cause the reaction rate to ________.
(A) remain constant
(B) increase by a factor of 25
(C) increase by a factor of 5
(D) increase by a factor of 10
(E) decrease by a factor of the cube root of 5

44.89. Which of the following is not a factor determining the energy of activation according to the Arrhenius equation? (ABCDE皆送分)
(A) temperature
(B) frequency of collision of reacting molecules
(C) fraction of collisions with effective orientations
(D) frequency factor
(E) None of the above.

45.90. A student needs a solution buffered at pH 4.30 ([H+ ] = 5.0×10−5 M). This student can choose from the following weak acids and their salts to prepare the buffer. Which system will own the best buffering capacity?
(A) Benzoic acid (Ka = 6.4 × 10-5 )
(B) Chloroacetic acid (Ka = 1.35 × 10-3 )
(C) Propanoic acid (Ka = 1.3 × 10-5 )
(D) Hypochlorous acid (Ka = 3.5 × 10-8 )

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