16. What is the hybridization of the central atom in SF₆?
(A) sp
(B) sp²
(C) sp³
(D) dsp³
(E) d²sp³

17. The molecular orbital configuration (σ₂s)²(σ₂s*)²(π₂py)¹(π₂px)¹ corresponds to the ground state of which species? (A) Be₂ (B) Li₂⁺ (C) B₂ (D) B₂²⁻ (E) C₂

18. Most valence electron transitions occur in the _ region of the electromagnetic spectrum. Rotational transitions are typically induced by radiation in the region, and vibrational transitions are typically induced by radiation in the _ region. (A) X-ray, UV-vis, IR (B) UV-vis, IR, microwave (C) IR, microwave, UV-vis (D) Microwave, X-ray, UV-vis (E) UV-vis, microwave, IR

19. Raw milk sours in 4.0 h at 28°C but takes 48 h to sour in a refrigerator at 5°C. Calculate the activation energy for the souring of milk. (A) 8.87 kJ/mol (B) 4.00 kJ/mol (C) 12.0 kJ/mol (D) 75.2 kJ/mol

20. In a cubic closest-packed solid, what percentage of the space is occupied by the spheres? (A) 43.8% (B) 52.4% (C) 68.0% (D) 74.0% (E) 84.0%

21. In the unit cell of sphalerite, Zn²⁺ ions occupy half of the tetrahedral holes in a face-centered cubic lattice of S²⁻ ions. How many formula units of ZnS are present in one unit cell? (A) 1 (B) 2 (C) 3 (D) 4 (E) 5

22. A 4.0 g sample of solid NaOH is dissolved in enough water to prepare 1.0 L of aqueous solution. What is the approximated osmotic pressure of this solution at 25°C? (A) 2.1 atm (B) 2.4 atm (C) 3.6 atm (D) 4.4 atm (E) 4.9 atm

23. Arrange the following compounds in order of increasing boiling point: SnCl₄, SnBr₄, and SnI₄. (A) SnCl₄ < SnBr₄ < SnI₄. (B) SnI₄ < SnBr₄ < SnCl₄. (C) SnBr₄ < SnI₄ < SnCl₄. (D) SnCl₄ < SnI₄ < SnBr₄. (E) SnI₄ < SnCl₄ < SnBr₄.

24. Which of the following coordination compounds forms a precipitate when treated with aqueous AgNO₃? (A) Na₃[CrCl₆] (B) [Cr(NH₃)₃Cl₃] (C) Na₃[Cr(CN)₅Cl] (D) [Cr(NH₃)₆]Cl₃

25. How many isomers does C₃H₆Br₂ have? Count enantiomers separately. (A) 2 (B) 3 (C) 4 (D) 5 (E) 6 

26. Which of the following statements about isotopes are correct? (A) Different isotopes of the same element contain different numbers of electrons. (B) The mass number of an isotope equals the total number of protons and neutrons in its nucleus. (C) The atomic masses of carbon-12 and carbon-13 are exactly 12 u and 13 u, respectively. (D) The atomic mass listed for an element in the periodic table is a weighted average of the masses of its naturally occurring isotopes. (E) Isotopes are represented by a subscript mass number to the left of the element symbol, for example, ²³⁵U.

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