7. Which of the following diatomic species is paramagnetic, has a bond order of 1.5, and is classified as a radical?
(A)
(B)
(C) B₂
(D) CN
(E) NO

8. What is the hybridization of the bolded atoms NNC, from left to right, in azodicarbonamide, H2NC(O)NNC(O)NH2? (A) sp³, sp, sp² (B) sp², sp, sp³ (C) sp², sp, sp² (D) sp, sp, sp² (E) sp², sp², sp²

9. A solid is found to be extremely hard, has a very high melting point, is insoluble in water, and does not conduct electricity in any state. Based on these properties, which of the following solids does it most likely represent? (A) CaCl2 (B) I2 (C) graphite (D) Pb (E) SiC

10. A metal Z with atomic radius r forms a cubic close-packed structure. Which formula correctly calculates the radius of the largest sphere that can fit in an octahedral hole without pushing any atom Z apart? (A) r(√2-1) (B) r(2√2-1) (C) r(√3-1) (D) r(3/√3-1) (E) r/(2√2-1)

11. There are several resonance structures of sulfate ions. Which statement about the most stable Lewis structure of the sulfate ion is invalid? (A) The sulfate ion has a tetrahedral geometry. (B) The sulfate ion is nonpolar. (C) The overall charge of the sulfate ion is 0 in the most stable Lewis structure. (D) All sulfur-oxygen bonds are equivalent. (E) The sulfur atom has an expanded octet.

12. Why is CO slightly polar, but not strongly polar, despite the significant electronegativity difference between carbon and oxygen? (A) The triple bond between carbon and oxygen is highly polar, but the molecule's symmetry reduces the overall polarity. (B) The triple bond in CO eliminates any dipole moment, as it localizes electrons equally between the two atoms. (C) Both carbon and oxygen have formal charges of zero, making the molecule nonpolar despite the electronegativity difference. (D) The electronegativity difference between carbon and oxygen is large, but the formal charge distribution reduces the effective dipole moment. (E) The molecule has a linear geometry, causing the bond dipoles to cancel each other out.

13. One ionic crystal structure contains two ions, . ions occupy the face-centered cubic lattice points, and ions occupy all the tetrahedral holes. Which statement is invalid? (A) The ionic radius of is larger than the ionic radius . (B) The coordination numbers of and F- are 12 and 8 respectively. (C) The relation between the edge length a of the unit cell and is equivalent to a * √3/4 = . (D) There are 4 ions and 8 F- ions in a unit cell. (E) The empirical formula of the ionic crystal structure is CaF2.

14. Which is not the valid statement? (A) 2SO3(g) → 2SO2(g) + O2(g) ＞ 0, the reaction is spontaneous at high temperatures and is entropy driven. (B) 2C(s) + 2H2(g) → C2H4(g) ＞ 0, the reaction will be spontaneous at low temperatures and is entropy driven. (C) 2NO(g) + O2(g) → 2NO2(g) ＜ 0, the reaction will be spontaneous at low temperatures and is enthalpy driven. (D) N2H4(l) + O2(g) → N2(g) + 2H2O(g) ＜ 0, the reaction will be spontaneous at all temperatures. (E) Water slowly evaporates at 25°C. This is a spontaneous reaction that is entropy driven.

15. A real gas behaves non-ideally under certain conditions and can be described by the van der Waals equation of state. Which of the following statements best explains the relationship between the compression factor Z, van der Waals' coefficients a and b, and deviations from ideal gas behavior? (A) For a gas with large a and small b, Z is always greater than 1, indicating the dominance of repulsive forces over attractive forces. (B) At low pressures, the effect of b dominates, causing Z to decrease below 1 due to volume corrections. (C) For a gas with large a, Z decreases below 1 at moderate pressures due to the strong attractive interactions between molecules. (D) At high pressure, the influence of both a and b diminishes, and Z becomes independent of these coefficients, matching ideal gas behavior. (E) Z is always less than 1 for any gas described by the van der Waals equation, regardless of the values of a and b.

16. Consider a gas in thermal equilibrium at two different temperatures, T₁ and T2, where T2 ＞ T1. Which of the following statements best explains the interplay between the Maxwell-Boltzmann distribution, temperature, and entropy for this system? (A) At T2, the Maxwell-Boltzmann distribution shifts to lower particle speeds, and entropy decreases because there are fewer accessible microstates. (B) At T2, the Maxwell-Boltzmann distribution becomes broader, indicating a greater range of particle speeds and an increase in entropy due to more accessible microstates. (C) The Maxwell-Boltzmann distribution remains unchanged between T1 and T2 because the distribution depends only on the mass of the particles, not the temperature. (D) At T1, the narrower Maxwell-Boltzmann distribution corresponds to higher entropy, as lower temperatures increase the uniformity of particle speeds. (E) Entropy remains constant between T1 and T2 because it is a state function independent of temperature changes.

17. Consider the thermodynamic properties, U, , T, H, w, , how many of them are not state functions? (A) 6 (B) 5 (C) 4 (D) 3 (E) 2

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