16. One can safely assume that the 3s- and 3p-orbitals will form molecular orbitals similar to those formed when 2s- and 2p-orbitals interact. According to molecular orbital theory, what will be the bond order for the Cl₂⁺ ion?
(A) 0.5
(B) 1
(C) 1.5
(D) 2
(E) None of these choices is correct.

17. Consider three 1-L flasks at STP. Flask A contains NH3 gas, flask B contains NO2 gas, and flask C contains N2 gas. Which contains the largest number of molecules? (A) Flask A (B) Flask B (C) Flask C (D) All are the same (E) None of these choices is correct.

18. In which flask are the molecules least polar and therefore most ideal in behavior? (A) Flask A (B) Flask B (C) Flask C (D) All are the same (E) None of these choices is correct.

19. For which of the following species are the intermolecular interactions entirely due to dispersion forces? (A) C2H6 (B) CH3OCH3 (C) NO2 (D) H2S

20. Which of the following liquids would have the highest viscosity at 25°C? (A) CH3OCH3 (B) C2H5OH (C) CH3Br (D) HOCH2CH2OH

21. A 15.00 % by mass solution of lactose (C12H22O11, 342.30 g/mol) in water has a density of 1.0602 g/mL at 20°C. What is the molarity of this solution? (A) 0.03097 M (B) 0.4133 M (C) 0.4646 M (D) 1.590 M (E) 1.379 M

22. Which of the following systems possesses the lowest freezing point? (A) 0.1 M FeCl3(aq) (B) 0.1 M K2SO4(aq) (C) 0.1 M CaCl2(aq) (D) 0.3 M C6H12O6, glucose (E) 0.1 M NaCl

23. For a particular process q = 20 kJ and w = 15 kJ. Which of the following statements is true? (A) Heat flows from the system to the surroundings. (B) The system does work on the surroundings. (C) E = 35 kJ (D) All of the above are true. (E) None of these choices is correct.

24. Which of the following results in a decrease in the entropy of the system? (A) O2(g), 300 K→O2(g), 400 K (B) H2O(s), 0°C→ H2O(l), 0°C (C) N2(g), 25°C→N2(aq), 25°C (D) NH3(l), -34.5°C→ NH3(g), -34.5°C (E) 2H2O2(g)→ 2H2O(g) + O2(g)

25. Given the following acids and Ka values:What is the order of increasing base strength? (A) CN–, F–, OAc–, ClO4– (B) CN–, OAc–, F–, ClO4– (C) CN–, ClO4–, F–, OAc– (D) ClO4–, OAc–, CN–, F– (E) ClO4–, F–, OAc–, CN–

26. According to the first law of thermodynamics, the energy of the universe is constant. Does this mean that ΔE is always equal to zero? (A) Yes, ΔE = 0 at all times, which is why q = -w. (B) No, ΔE does not always equal zero, but this is only due to factors like friction and heat. (C) No, ΔE does not always equal zero because it refers to the system's internal energy, which is affected by heat and work. (D) No, ΔE never equals zero because work is always being done on the system or by the system. (E) None of these

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