Name: ______________________________ AP Chemistry Exam #2 1. ___ 2. ___ 3. ___ 4. ___ 5. ___ 6. ___ 7. ___ 8. ___ 9. ___ 10. ___ 11. ___ 12. ___ 13. ___ 14. ___ 15. ___ 16. ___ 17. ___ 18. ___ 19. ___ 20. ___ 21. ___ 22. ___ 23. ___ 24. ___ 25. ___ Question 1-3 refer to the following pairs of elements. A. Be and B B. P and S C. Cl and F D. Cr and Mo E. Au and Ag 1. Show a reversal in the trend for first ionization energy because of electronelectron repulsion. 2. Show a reversal in the trend for first ionization energy because of shielding by full orbitals. 3. Exhibit an anomaly in the outer electron configuration due to filling of d orbitals. Questions 4-8 refer to the following elements: A. B. C. D. E. 4. 5. 6. 7. 8. Na Mg O S N Is the most electronegative. exhibits the most number of oxidation states. has the largest atomic radius. has the smallest atomic radius for its most common ion. has the largest difference between first and second ionization energy. For each, select the best answer from the choices immediately below each question. 9. Which of the following intermolecular forces are found in all substances? (A) dipersion (B) dipole-dipole (C) hydrogen bonding (D) ion-dipole (E) covalent 10. Which of these substances can form hydrogen bonds within their pure liquids? I. CH3NH2 II. (CH3)2C = O III. CH3OH IV. CH3OCH3 (A) I, II, III, IV (B) I, II, III only (C) II only (D) I, II only (E) I, II, IV only 11. What is the correct order of boiling points, lowest to highest, for these liquids? (A) CH3CH2CH3 < CH3CH2OH < H2O (B) CH3CH2OH < CH3CH2CH3 < H2O (C) H2O < CH3CH2CH3 < CH3CH2OH (D) CH3CH2CH3 < H2O < CH3CH2OH (E) CH3CH2OH < H2O < CH3CH2CH3 12. What volume of 0.500 M AlCl3 solution is needed to prepare 300 ml of a solution that has a chloride concentration of 0.300 M? (A) 30.0 ml (B) 50.0 ml (C) 60.0 ml (D) 120 ml (E) 180 ml 13. Formulas of five compounds of a particular ion “X” are listed below. Which of them must be incorrect? (A) X2O3 (B) X2(CO3)3 (C) XPO4 (D) XCl3 (E) X3N 14. How many unpaired electrons are found in the most stable electronic state of a sulfur atom? (A) 0 (B) 1 (C) 2 (D) 4 (E) 6 15. Which molecule has the strongest bond? (A) CO (B) O2 (C) NO (D) F2 (E) Cl2 16. Which molecule has the shortest bond length? (A) N2 (B) O2 (C) Cl2 (D) Br2 (E) F2 17. Which molecule has the longest bond length? (A) F2 (B) Cl2 (C) Br2 (D) I2 (E) N2 18. For SF4, the molecular geometry is: (A) trigonal planar (B) trigonal bipyramidal (C) see-saw (D) T-shape (E) Tetrahedral 19. Which is (are) planar? I. NO3- II. SO3 III. CO32- IV. SO32(A) I only (B) III only (C) I, II, III only (D) I, III, IV only (E) All are planar 20. A bond angle commonly found in molecules having a central atom that is sp3 hybridized is: (A) 180 (B) 120 (C) 109.5 (D) 90 (E) 75 21. Which molecule would have a bond angle that deviates most from that predicted by VSEPR? (A) CH4 (B) NH3 (C) H2O (D) CH3F (E) CO2 22. Which substance will have the highest melting point? (A) HBr (B) LiBr (C) CaBr2 (D) SBr4 (E) Br2 23. Which substance will have the highest boiling point? (A) CH3CH2CH2CH3 (B) CH3CH2CH2CH2F (C) CH3CH2CH2CH2Cl (D) CH3CH2CH2CH2Br (E) CH3CH2CH2CH2I 24. Which atom is least likely to covalently bond? (A) Na (B) Al (C) C (D) Cl (E) S 25. If 1.0 ml of a stock solution that is 1.0 M Na+ is added to a flask and then water is added to reach a total volume of 100.0 ml, what is the Na+ concentration of the resulting solution? (A) 0.0010 M (B) 0.010 M (C) 0.10 M (D) 1.0 M (E) 10.0 M