13. Consider the following orderings. I. Na⁺ < Mg²⁺ < Al³⁺ < Si⁴⁺ II. Be < Mg < Ca < Sr III. I < Br < Cl < F IV. Al < Si < P < Cl Which of these give(s) a correct trend in ionization energy?
(A) III
(B) II, IV
(C) I, IV
(D) I, III, IV
(E) none of them

14. Consider the following molecules. Select the molecule(s) that violate the octet rule. (A) I, II, IV (B) I, III, IV, VI (C) III, V, VI (D) I, IV, VI (E) I, II, IV, VI

15. Which of the following statements is true? (A) Tetrahedral molecules (four identical bonds equally spaced) always has a dipole moment. (B) Both HF and CO₂ are linear molecules and therefore polar. (C) The correct order for molecules from most to least polar is CF₂H₂ > CCl₂H₂ > CF₂Cl₂ > CH₄ = CCl₄. (D) The molecular structure of SOCl₂ is trigonal planar. (E) The molecular structure of XeF₅⁺ is trigonal bipyramidal.

16. Consider the molecule:Specify the hybridization of each carbon atom.

17. Which of the following statements is false?(A) The bond length of $\text{N}2$ is shorter than $\text{N}2^+$.(B) The bond in of $\text{N}2$ is stronger than $\text{N}2^-$.(C) The bond dissociation energy of $\text{N}2$ is higher than $\text{N}2^-$.(D) The bond order of $\text{N}_2$ is 2.5.(E) All of above are true.

18. Which one of the following decreases as the strength of the attractive intermolecular forces increases? (A) the heat of vaporization (B) the normal boiling temperature (C) the extent of deviations from the ideal gas law (D) the sublimation temperature of a solid (E) the vapor pressure of a liquid

19. Determine the osmotic pressure of a solution that contains 0.048 g of a hydrocarbon solute (molar mass = 340 g/mol) dissolved in benzene to make a 350-mL solution. The temperature is 20.0°C. (A) 0.50 torr (B) 2.5 torr (C) 3.3 torr (D) 7.4 torr (E) 6.9 torr

20. For a reaction: aA → Products, $[\text{A}]_0 = 6.0 \text{ M}$, and the first two half-lives are 56 and 28 minutes, respectively. Calculate $[\text{A}]$ at $t = 105.9$ minutes. (A) 5.7 M (B) 12 M (C) 0.68 M (D) 0.33 M (E) none of these

21. Consider the following reaction: $\text{CS}2(g) + 4\text{H}2(g) \rightleftharpoons \text{CH}4(g) + 2\text{H}2\text{S}(g)$. The equilibrium constant $K$ is about 0.31 at 900°C. What is the $K_p$ at this temperature? (A) $2.9 \times 10^3$ (B) $3.2 \times 10^{-3}$ (C) $3.3 \times 10^{-5}$ (D) $3.0 \times 10^1$ (E) $1.1 \times 10^{-3}$

22. The questions below refer to the following system: $$\text{Co}(\text{H}2\text{O}){6}^{2+} + 4 \text{Cl}^- \rightleftharpoons \text{CoCl}4^{2-} + 6\text{H}2\text{O}$$ When cobalt(II) chloride is added to pure water, the $\text{Co}^{2+}$ ions hydrate. The hydrated form then reacts with the $\text{Cl}^-$ ions to set up the equilibrium shown here. Which statement below describes the change that the system will undergo if silver nitrate is added? (A) It should become more blue. (B) It should become more pink. (C) Water will be produced. (D) The silver ion will react with the $\text{CoCl}_4^{2-}$. (E) Nothing will change.

23. Using the following $K_a$ values, indicate the correct order of base strength. $$\text{HNO}_2 \text{ Ka} = 4.0 \times 10^{-4} \quad \text{HF Ka} = 7.2 \times 10^{-4} \quad \text{HCN Ka} = 6.2 \times 10^{-10}$$ (A) $\text{CN}^- > \text{NO}2^- > \text{F}^- > \text{H}2\text{O} > \text{Cl}^-$ (B) $\text{Cl}^- > \text{H}2\text{O} > \text{F}^- > \text{NO}2^- > \text{CN}^-$ (C) $\text{CN}^- > \text{F}^- > \text{NO}2^- > \text{Cl}^- > \text{H}2\text{O}$ (D) $\text{H}2\text{O} > \text{CN}^- > \text{NO}2^- > \text{F}^- > \text{Cl}^-$ (E) none of these

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