7. Consider the molecular orbital energy level diagrams for O₂ and NO. Which of the following is true? I. Both molecules are paramagnetic. II. The bond strength of O₂ is greater than the bond strength of NO. III. NO is an example of a homonuclear diatomic molecule. IV. The ionization energy of NO is smaller than the ionization energy of NO+.
(A) I only；
(B) I and II；
(C) I and IV；
(D) II and III；
(E) I, II, and IV

3. The partial pressures of CH4, N2, and O2 in a sample of gas were found to be 135 mm-Hg, 508 mm-Hg, and 571 mm-Hg, respectively. Calculate the mole fraction of nitrogen. (A) 20.4； (B) 0.470； (C) 0.418； (D) 0.751； (E) 0.359

4. A 32.5 g piece of aluminum (which has a molar heat capacity of 24.03 J/°C·mol) is heated to 82.4°C and dropped into a calorimeter containing water (specific heat capacity of water is 4.18 J/g°C) initially at 22.3°C. The final temperature of the water is 24.2°C. Ignoring significant figures, calculate the mass of water in the calorimeter. (Al: 26.98 g/mol) (A) 212 g； (B) 5.72 kg； (C) 6.42 g； (D) 1.68 kg； (E) none of these

5. Which of the following statements is (are) true? I. An excited atom can return to its ground state by absorbing electromagnetic radiation. II. The energy of an atom is increased when electromagnetic radiation is emitted from it. III. The energy of electromagnetic radiation increases as its frequency increases. IV. An electron in the n = 4 state in the hydrogen atom can go to the n = 2 state by emitting electromagnetic radiation at the appropriate frequency. V. The frequency and wavelength of electromagnetic radiation are inversely proportional to each other.(A) II, III, IV； (B) III, V； (C) I, II, III； (D) III, IV, V； (E) I, II, IV

6. Consider the following reaction: A2 + B2  2AB ∆H = -365 kJ The bond energy for A2 is half the amount of AB. The bond energy of B2 = 447 kJ/mol. What is the bond energy of A2? (A) 812 kJ/mol； (B) 630 kJ/mol； (C) 271 kJ/mol； (D) –183 kJ/mol； (E) none of these

8 If equal, rigid spheres are arranged in a simple cubic lattice in the usual way (i.e., in such a way that they touch each other), what fraction of the corresponding solid will be empty space? (A) 0.52； (B) 0.32； (C) 0.68； (D) 0.48； (E) none of these

9 At a given temperature, you have a mixture of benzene (vapor pressure of pure benzene = 745 torr) and toluene (vapor pressure of pure toluene = 290 torr). The mole fraction of benzene in the vapor above the solution is 0.590. Assuming ideal behavior, calculate the mole fraction of toluene in the solution. (A) 0.213； (B) 0.778； (C) 0.641； (D) 0.359； (E) 0.590

10. A 1 L container originally holds 0.4 mol of N2, 0.1 mol of O2, and 0.08 mole of NO. If the volume of the container holding the equilibrium mixture of N2, O2, and NO is decreased to 0.5 L without changing the quantities of the gases present, how will their concentrations change? (A) The concentration of NO will increase； the concentrations of N2 and O2 will decrease. (B) The concentrations of N2 and O2 will increase； and the concentration of NO will decrease. (C) The concentrations of N2, O2, and NO will increase. (D) The concentrations of N2, O2, and NO will decrease. (E) There will be no change in the concentrations of N2, O2, and NO.

11. In titrating 0.20 M hydrochloric acid, HCl, with 0.20 M NaOH at 25°C, the solution at the equivalence point is (Cl: 35.45 g/mol): (A) 0.20 M NaCl； (B) very acidic； (C) slightly acidic； (D) 0.10 M HCl and 0.20 M NaOH； (E) 0.10 M NaCl

12. Consider a solution containing the following cations: Na⁺, and Ag⁺. Treatment of the solution with dilute HCl followed by saturation with H2S results in formation of precipitate(s). Which ions still remain in solution ? (A) Ag⁺ only； (B) Na⁺, ； (C) Ag⁺ and ； (D) Na⁺, , and ； (E) Na⁺ only

13. A mixture of hydrogen and chlorine remains unreacted until it is exposed to ultraviolet light from a burning magnesium strip. Then the following reaction occurs very rapidly:  → ∆G = -45.54 kJ； ∆H = -44.12 kJ； ∆S = -4.76 J/K  Which of the following is consistent with this information? (A) The reactants are thermodynamically more stable than the products. (B) The reaction has a small equilibrium constant. (C) The ultraviolet light raises the temperature of the system and makes the reaction more favorable. (D) The negative value for ∆S slows down the reaction. (E) The reaction is spontaneous, but the reactants are kinetically stable.