12. Calcium has a cubic closest packed structure as a solid. Assuming that calcium has an atomic radius of 197 pm, please calculate the density of solid calcium to be ______ g/cm³
(A) 11.6
(B) 1.54
(C) 4.5
(D) 3.38
(E) 22.68

8. Which of the following statements is correct? (A) Argon has ionization energy higher than bromine. (B) Among has the smallest radius. (C) For Rb, Na, and Be, the order of increasing atomic size is Rb ＜ Na ＜ Be. (D) In the ground state of mercury, Hg, its electron configuration is . (E) In the ground state of element 115, Uup, it has 24 electrons occupying atomic orbitals with l = 3.

9. Please use the following data to estimate for potassium chloride to be _________ kJ/mol. K(s) + (1/2)Cl2(g) → KCl(s)； lattice energy, -690. kJ/mol； ionization energy for K, 419 kJ/mol； electron affinity of Cl, -349 kJ/mol； bond energy of Cl2, 239 kJ/mol； ethalpy of sublimation for K, 90. kJ/mol. (A) -161 (B) -1085 (C) 161 (D) 1085 (E) -411

10. Which of the following statements is correct? (A) F2 + has its bond order of 1.5. (B) CN- is paramagnetic. (C) Between would most likely gain an electron. (D) The predicted molecular structure and expected hybrid orbitals on the central atom of TeF4 are see-saw and d2 sp 3 , respectively. (E) The predicted molecular structure and expected hybrid orbitals on the central atom of IF4 is trigonal bipyramid and d2 sp 3 , respectively.

11. Which of the following statements is correct? (A) CO2 has intermolecular forces greater than that of OCS. (B) LiF has its freezing point lower than those of F2 and HCl. (C) CaO has its enthalpy of fusion smaller than those of I2 and CsBr. (D) H2O2 has its viscosity greater than those of HF and H2S. (E) H2CO has intermolecular forces greater than that of CH3OH.

13. In order to prepare a solution with a freezing point of -1.50°C, 200.0 g water has to be added glycerin (C3H8O3), a nonelectrolyte, with mass of _______g to attain the desired aqueous solution. (A) 0.018 (B) 36.46 (C) 18.1 (D) 26.0 (E) 14.8

14. Consider the reaction 3A + B + C⇌D + E where the rate law is defined as –(∆[A]/∆t) = k[A]2 [B][C]. An experiment is carried out where [B]0 = [C]0 = 1.00 M and [A]0 = 1.00 × M. We also know that after 3.00 min of the reaction, [A] is 3.26 × M. What will be the concentration of A after 10.0 min? (A)M (B)M (C) 1.00 M (D)M (E)M

15. Ea for the uncatalyzed reaction O3(g) + O(g) → 2O2 is 14.0 kJ. Ea for the same reaction when catalyzed is 11.9 kJ. What is the ratio of the rate constant for the catalyzed reaction to that for the uncatalyzed reaction at 25℃? Assume that the frequency factor A is the same for each reaction. (A) 215 (B) 51 (C) 2.3 (D) 532 (E) 0.25

16. Consider the decomposition equation of a compound: C5H6O3(g)⇌C2H6(g) + 3CO(g). When a 5.63-g sample of pure C5H6O3(g) was sealed into an otherwise empty 2.50-L flask and heated to 200℃, the pressure in the flask gradually rose to 1.63 atm and remained at that value. The K value for this reaction is _____ . (A) (B) (C) (D) (E)

17. Which of the following 0.10 M solutions are correctly arranged in order of most acidic to most basic? (A) HCl ＞ KCl ＞ NH4Cl ＞ KCN ＞ KOH (B) NH4Cl .＞ HCl .＞ KCl ＞ KCN ＞ KOH (C) NH4Cl .＞ HCl .＞ KCN ＞ KCl ＞ KOH (D) HCl ＞ NH4Cl ＞ KCl ＞ KCN ＞ KOH (E) HCl ＞ NH4Cl ＞ KCN ＞ KCl ＞ KOH

18. A 0.15 M solution of a weak acid is 3.0% dissociated. The Ka of the acid is calculated to be _______ . (A) (B) (C) (D)(E)