109年 - 109 高雄醫學大學_學士後醫學系招生考試：化學#87230

16. For 1.0 M of the following solution, which chemical gives the highest pH value? (A) NaF (B) Na₂S₂O₃(C) NH₄Cl (D) Al(NO₃)₃ (E) Ethanol

17. Which of the following complex is diamagnetic? (A) [Ni(CN)₆]^4– (B) [Ti(CN)₆]^3– (C) [Cr(CN)₆]^3– (D) [Co(CN)₆]^3– (E) All of these

18. Which of the following molecule doesn’t exhibit the behavior of s-p mixing of molecular orbitals? (A) N₂(B) B₂ (C) O₂ (D) NO (E) All of these

19. Which of the following substrate is most likely to exhibit liquid crystalline behavior? (A) (B) (C) (D) (E) C₂₅H₅₁OH

20. What is the net number of tetrahedral holes contained in the close packing of spheres unit cell like face-center cubic? (A) 8 (B) 4 (C) 12 (D) 6 (E) 3

21. Which of the following active ingredient is most commonly used in liquid bleaches (Sanitizers)? (A) NaCl (B) NaClO (C) NaClO₂ (D) NaClO₃ (E) NaClO₄

22. Natural copper contains two isotopic forms. The most common isotope is ⁶³Cu (atomic mass 62.93 amu), which is 69.09% abundant. The average atomic mass of Cu is 63.55 amu. What is the mass of the other isotope? (A) 61.90 amu (B) 63.10 amu (C) 64.93 amu (D) 65.90 amu (E) 67.10 amu

23. 0.2 g of FeCl₃(s) is dissolved in 20 mL water. The pH of this aqueous solution at 25 o C will be (A) pH ＞ 7 (B) pH ＜ 7 (C) pH = 7 (D) no effect on pH (E) this cannot be determined

24. Several possible combinations of ΔH and ΔS for a reaction are listed as below. Which of the following case is spontaneous for this reaction at all temperatures? (A) ΔH is positive, ΔS is positive (B) ΔH is negative, ΔS is positive (C) ΔH is negative, ΔS is negative (D) ΔH is positive, ΔS is negative (E) None of these

25. First-row transition metals play significant roles in biological system. Which of the following transition metal is a component of vitamin B12? (A) Cr (B) Zn (C) Fe (D) Cu (E) Co

26. What is the charge of NO molecule if the bond order is 2? (A) +1 (B) –1 (C) 0 (D) +2 (E) –2

27. What is the range of wave number (cm⁻¹ ) for an organic molecule containing a carbonyl group in the infrared spectrum? (A) 3610−3640 (B) 2850−3300 (C) 2100−2300 (D) 1690−1760 (E) 1080−1300

28. The complex cis-Pt(NH3)2Cl2 showed high anti-tumor activity, but trans-Pt(NH3)2Cl2 showed no effect on tumor therapy. These two complexes can be classified into which type of isomerism. (A) linkage isomerism (B) optical isomerism (C) coordination isomerism (D) ionization isomerism (E) geometric isomerism

29. The decay of strontium-90 follows a first-order process and the rate constant is 0.02406 year⁻¹ . How much of 2 mg sample of strontium-90 remains after 144 years? (A) 0.250 mg (B) 0.062 mg (C) 0.031 mg (D) 0.125 mg (E) 0.500 mg

30. Which compound yields the largest van’t Hoff factor (i) when dissolved in water? (A) NaCl (B) MgCl₂(C) MgSO₄ (D) FeCl₃ (E) Glucose

61. Which is an incorrect statement for heat capacity of ideal gases? (A) C_v is identical for monatomic ideal gases (B) Molecular motion of monatomic ideal gas is zero (C) C_v of polyatomic ideal gas is larger than C_vof monatomic ideal gas (D) C_p ＞ C_vin all ideal gases (E) C_p= R for monatomic ideal gas

62. C_diamond (s) → C_graphite (s) ΔG^o = −2.9 kJ Which of the following is an incorrect statement? (A) The process is spontaneous (B) It occurs very slowly at 25℃ and 1atm (C) Smaller ΔS^o for diamond (D) Smaller ΔH^o for diamond (E) The process become reversible at high temperature and pressure

63. Determine the number of nodal surfaces for a 3s orbital. (A) 3 (B) 2 (C) 1 (D) 0 (E) None of these

64. Which molecule has only one resonance structure that obeys the Octet rule? (A) NO⁺ (B) NO₂⁻(C) NO₃⁻ (D) O₃ (E) CO₃²⁻

65. What is the resonance frequency (MHz) for¹³C nuclei operated in a nuclear magnetic resonance spectrometer of 400 MHz? (gyromagnetic ratio of 1 H and¹³C is ~4) (A) 100 (B) 200 (C) 400 (D) 800 (E) 1600

66. The color difference between [CoCl₄]²⁻and [Co(H₂O)₆]²⁺can be supported by which concept? (A) Redox process (B) Spectrochemical series (C) Disproportionation reaction (D) van’t Hoff factor (E) Hard-Soft Acid-Base

67. How many net numbers of spheres are occupied in a face-centered cubic (f.c.c.) unit cell? (A) 1 (B) 2 (C) 4 (D) 6 (E) 8

68. For a reaction involving changes of reactant concentrations ([A]), what is the reaction order (m) when the correlation of ln [A] versus time (t) is a straight line? (A) m=0 (B) m=1/2 (C) m=1 (D) m=2 (E) None of these

69. Consider the reaction Fe³⁺(aq) + SCN^- (aq) FeSCN²⁺(aq). Which one of the following statements is correct? (A) The equilibrium position shifts to the right after water is added to double the volume (B) The equilibrium position shifts to the right after AgNO₃(aq) is added (C) The equilibrium position shifts to the left after NaOH(aq) is added (D) The equilibrium position shifts to the left after Fe(NO)₃(aq) is added (E) None of the above is correct

70. Which “P” in the following compounds has the lowest oxidation state? (A) Phosphoric acid (B) Phosphorous acid (C) Hypophosphorous acid (D) Sodium phosphide (E) Black phosphorus

71. How many π electrons are delocalized in 1,4-diphenyl-1,3-butadiene? (A) 4 (B) 8 (C) 16 (D) 24 (E) 32

72. Based on MO theory, which molecule is not paramagnetic? (A) O₂⁻ (B) O₂⁺ (C) O₂ (D) N₂ (E) N₂⁺

73. Consider mixing equal volume of 0.1 M Na₂CO₃ solution and 0.1 M H₂SO₄ solution. Which statement is correct? (A) [H⁺] is less than 0.05 M (B) [H⁺ ] is between 0.1 M and 0.05 M (C) [H⁺ ] is 0.1 M (D) [H⁺ ] is 0.2 M (E) pH ＞ 7

74. Which is the major specie for a carbonate-containing solution at pH 8.5? (K_a1 = 4.3 × 10^–7, K_a2 = 4.8 × 10^–11 for carbonic acid) (A) CO₂ (B) H₂CO₃ (C) HCO₃⁻ (D) CO₃²⁻(E) C₂O₄²⁻

75. What is the main contribution for the negative entropy value (ΔSo soln ＜ 0) when formation of LiF(aq) in water? (A) Random dispersal of water (B) Breaking ordered bonding of solids (C) Interaction of Li⁺ and F⁻ with water molecules (D) Dispersion of Li⁺ and F⁻ into solution (E) Fast equilibrium

76. The energy required to remove the electron from a hydrogen atom in its ground state is 2.178 × 10^–18J. What is the energy required to excite the electron in the He⁺ ion from the n = 1 level to the n = 2 level? (A) 1.634 × 10^–18 J (B) 2.178 × 10^–18 J (C) 3.268 × 10^–18 J (D) 8.712 × 10^–18 J (E) None of these

77. To increase the value of K for the endothermic reaction as mentioned below, a chemist should__________ . (A) decrease the temperature (B) decrease the container volume (C) increase the total pressure (D) increase the temperature (E) None of these

78. Two moles of an ideal gas undergo isothermal expansion from a volume of 1.0 L to a volume of 10.0 L against a constant external pressure of 1.0 atm. Calculate the changes of internal energy (ΔE). (1 L·atm = 101.3 J) (A) 9.12 × 10² J (B) 1.82 × 10³ J (C) –9.12 × 10² J (D) –1.82 × 10³ J (E) 0 J

79. Which theory, phenomenon or equation can explain redox potential difference on ion concentrations? (A) Disproportionation (B) Electrogenerated chemiluminescence (C) Galvanic displacement (D) Henderson-Hassebalch equation (E) Nernst equation

80. Using the data below, calculate the normal boiling point of liquid Br2 at 1 atm. For the process, Br₂(l) → Br₂(g): ΔH° = 31.0 kJ mol⁻¹ and ΔS° = 93.0 JK⁻¹ mol⁻¹ (A) 300 K (B) 0.33 K (C) 0.30 K (D) 333 K (E) 433 K

81. Using the data shown as follows to calculate ΔG° for the reaction (1 F = 96,485 coulombs):

2Fe³⁺(aq) + Cu(s) → 2Fe²⁺(aq) + Cu²⁺(aq)

The reduction potentials for Fe3+ and Cu2+ are as follows:

Fe³⁺ + e^–→ Fe²⁺ ε° = 0.77 V

Cu²⁺+ 2e^– → Cu ε° = 0.34 V

(A) –8.3 × 10⁴ J (B) –1.2 × 10⁵ J (C) –4.2 × 10⁴ J (D) –6.0 × 10⁴ J (E) –2.4 × 10⁵J

82. For corrosion of iron, which of the following statements is (are) true?

I. Anode reaction: Fe → Fe²⁺ + 2e^–

II. Cathode reaction: O₂+ 2H₂O + 4e^– → 4OH^–

III. Moisture serving as a salt bridge

(A) I (B) III (C) I and II (D) I, II, and III (E) None of the statement is true

83.Above structure is the precursor of the Remdesivir (potential COVID−19 drug), which of the below statements are true? I. It is an aromatic compound II. It has 13 σ bond III. It shows dipole moment IV. It has 11 σ bond V. It contains sp hybridization Please choose one of the answer below, (A) I and IV (B) II and IV (C) I, II, and III (D) I, II, III, and V (E) None of these

84. What is the boiling-point change for a solution containing 18.0 g of glucose in 150.0 g of water at 1 atm? (K_b = 0.51 °C kg/mol for water) (A) 2.2 °C (B) 0.06 °C (C) 0.34 °C (D) 4.3 °C (E) 1.8 °C

85. If the human eye has an osmotic pressure of 8.0 atm at 25˚C, the concentration of solution particles in water will be_________ mmol/L in order to provide an isotonic eyedrop solution, a solution with equal osmotic pressure. (A) 620 (B) 4,110 (C) 0.62 (D) 327 (E) 79

86. The solubility of CaCl2 in cold water is 74.5 g per 100.0 g water. Assuming i = 3.0 for CaCl₂, the freezing point for a saturated solution of CaCl₂ will be________˚C. (K_f= 1.86 °C kg/mol for water) (A) 0 (B) –0.32 (C) –13 (D) –32 (E) –37.4

87. Determine the value of Kc for the reaction (A) 0.001 (B) 0.01 (C) 0.1 (D) 1.0 (E) 10

88. 2-deoxy-2-[¹⁸F]fluoroglucose ( [¹⁸F]FDG ) decays by _______ and [18F] will yield stable _______. (A) alpha emission, ¹⁸O (B) beta emission, ¹⁹F (C) positron emission, ¹⁸O (D) photon emission, ¹⁹F (E) neutron capture,¹⁹O

89. For an unknown molecules A₂, if the dissociation energy is 1204 kJ/mol, what is the maximum wavelength of electromagnetic radiation required to rupture this bond? (Planck constant: 6 × 10^-34 J.s, light of speed: 3 × 10⁸ m/s) (A) 90 nm (B) 120 nm (C) 150 nm (D) 180 nm (E) 210 nm

90. Calculate the ratio of the root-mean-square velocities (μ_rms) of H₂ to SO₂. (A) 1.0 (B) 0.18 (C) 32 (D) 5.6 (E) 180

109年 - 109 高雄醫學大學_學士後醫學系招生考試：化學#87230

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