Chapter 6-9 Review PDF

Name: __________________________ Date: _____________ 1. Given the reaction, 4B + 3A → 4C + 7D, and some standard enthalpies of H of formation, : A: +15.7 kJ mol -1 B: −86.4 kJ mol-1 C: −52.7 kJ mol-1 D: −71.6 kJ mol-1 What is the standard...

Name: __________________________ Date: _____________ 1. Given the reaction, 4B + 3A → 4C + 7D, and some standard enthalpies of H of formation, : A: +15.7 kJ mol -1 B: −86.4 kJ mol-1 C: −52.7 kJ mol-1 D: −71.6 kJ mol-1 What is the standard enthalpy of reaction, in kJ for the reaction shown? A) −53.6 kJ B) −413.5 kJ C) −515.6 kJ D) −853.6 kJ E) −908.4 kJ 2. Complete combustion of hydrocarbons, or compounds with C,H, and O as the only elements, gives CO 2 and H2O as the only products. If carried out under standard conditions, the CO 2 is a gas while the H2O is a liquid. Given these standard enthalpies of combustion: C2H4(g) = −1411.08 kJ mol-1 C2H2(g) = −1299.65 kJ mol-1 H2(g) = −285.90 kJ mol-1 C(s) = −393.50 kJ mol-1 Calculate the standard enthalpy of reaction for the process, C 2H2(g) + H2(g) → C2H4(g) A) −174.47 kJ B) +397.33 kJ C) −961.47 kJ D) −2424.83 kJ E) −2996.63 kJ 3. H of The thermochemical equation which is associated with , the standard enthalpy of formation, for acetic acid, C 2H4O2(l), is A) C2(s) + 4 H(g) + O2(g) → C2H4O2(l) B) 2 C(g) + 4 H(g) + 2 O(g) → C2H4O2(l) C) C2(s) + 2 H2(g) + O2(g) → C2H4O2(l) D) 2 C(s) + 2 H2(g) + O2(g) → C2H4O2(l) E) C(s) + H2(g) + O2(g) → C2H4O2(l) 4. A 350.0 gram sample of copper is initially at 25.0 °C. It absorbs 12.50 kJ of heat from its surroundings. What is its final temperature, to the nearest tenth of a degree? (specific heat = 0.3874 J g− 1 °C-1 for copper) A) 38.8 °C B) 67.2 °C C) 92.2 °C D) 117.2 °C E) 156.7 °C Page 1  5. 500.0 ml of 0.220 molar HCl(aq) was added to a high quality insulated calorimeter containing 500.0 ml of 0.200 molar NaOH(aq). Both solutions have a density of 1.000 g ml-1 and a specific heat of 4.184 J g− 1 °C-1. The calorimeter had a heat capacity of 850.0 J °C-1. The temperature of the entire system rose from 25.60 °C to 26.70 °C. Calculate the heat of reaction, in kJ, per mole of NaOH(aq). ______ 6. The standard enthalpy of combustion for ethylene glycol, C 2H6O2(l), is −1179.5 kJ H of mol-1. Using this data and the standard enthalpies of formation, : H2O(l) = −285.9 kJ mol-1; CO2(g) = −393.5 kJ mol-1 calculate the standard enthalpy of formation of C 2H6O2(l), in kJ mol-1. ______ 7. Calculate the frequency of visible light having a wavelength of 464.1 nm A) 139.1 s− 1 B) 1.548 x 10 − 6 s− 1 C) 1.548 x 10 − 15 s− 1 D) 6.460 x 10 14 s− 1 E) 6.460 x 10 5 s− 1 8. What is the wavelength of electromagnetic radiation which has a frequency of 4.464 x 10 14 s− 1? A) 1.338 x 10 23 m B) 1.489 x 10 − 6 m C) 6.716 x 10 − 7 nm D) 671.6 nm E) 7.472 x 10 − 15 nm 9. What is the energy, in joules, of one photon of visible radiation with a wavelength of 464.1 nm? A) 1.026 x 10 − 48 J B) 2.100 x 10 35 J C) 2.341 x 10 11 J D) 4.280 x 10 − 19 J E) 4.280 x 10 − 12 J 10. What is the energy, in joules, of one mole of photons whose wavelength is 5.461 x 10 2 nm? A) 2.191 x 10 − 4 J B) 2.437 x 10 − 12 J C) 2.191 x 10 5 J D) 1.376 x 10 6 J E) 4.06 x 10 − 19 J Page 2 11. Calculate the frequency of the light emitted by a hydrogen atom during a transition of its electron from the energy level with n = 6 to the level with n = 3. Recall that the quantized energies of the levels in the hydrogen atom are given by: 21.79 x 10 −19 En = − joule n2 A) 1.665 x 10 − 26 s − 1 B) 1.824 x 10 − 15 s− 1 C) 2.740 x 10 14 s− 1 D) 3.649 x 10 − 15 s− 1 E) 9.132 x 10 13 s− 1 12. Given the following sets of quantum numbers for n l ml ms, which one of these sets is not a possible set for an electron in an atom? n l ml ms A) 4 2 2 −½ B) 3 1 −1 −1 C) 4 3 2 ½ D) 4 3 −2 −½ E) 5 2 2 ½ 13. The maximum number of electrons that would be required to fill all the energy levels having a value of 4 for n, the principal quantum number, is A) n B) n+1 C) 2n D) n 2 E) 2n 2 14. The spectroscopic notation (number + letter designation) for the subshell with n = 4 and l = 2 is A) 4d subshell B) 4p subshell C) 4f subshell D) 4s subshell E) there is no subshell fitting this description Page 3 15. The three quantum numbers which characterize the solutions to the wave equation describing the behavior of the electron in the H atom are usually designated as A) 1s 2s 2p B) n l ms C) ml ms mp D) n l ml E) l ml ms 16. The number of orbitals in a shell with n = 3 is ______ 17. Which one of the species below should have the smallest value for its first ionization energy? A) Ba B) C C) Cs D) K E) Mg 18. The atoms in the nitrogen molecule, N 2, are held together by A) a single covalent bond B) a double covalent bond C) a triple covalent bond D) an ionic bond E) a magnetic dipole bond 19. The atoms in the hydrogen fluoride molecule are held together by A) a single covalent bond B) a double covalent bond C) a triple covalent bond D) an ionic bond E) a magnetic dipole bond 20. Draw the Lewis structure for the F2CO molecule. Based on this structure, the correct number of polar bonds and non-polar bonds is A) 3 polar bonds and no non-polar bonds B) 2 polar bonds and 1 non-polar bond C) 1 polar bonds and 2 non-polar bonds D) no polar bonds and 3 non-polar bonds E) 2 polar bonds and 2 non-polar bonds Page 4 21. The metaphosphate ion, PO 3-, is the structural analog of the NO 3- ion with respect to the geometric arrangement of the atoms in the ion. After drawing the "best" Lewis structure for the metaphosphate ion based on formal charge considerations, what is the formal charge on the phosphorus atom? A) -1 B) 0 C) +1 D) +2 E) +5 22. Complete the Lewis structure for H 2SeO4 from the skeletal template presented below by filling in the bonds and the remaining valence electrons (those which are not in the bonds). If the valence shells are filled to the usual limit (maximum of 8), what is the sum of the absolute values of all the formal charges in the molecule? A) 0 B) 1 C) 2 D) 3 E) 4 23. Based on conclusions from application of the VSEPR theory, which one of the following molecules or ions is bent (nonlinear)? A) Cl2O B) CO2 C) HCN D) CO E) NO2+ 24. Which one of the molecules below is a polar molecule? A) Br2 B) BF3 C) CO2 D) CS2 E) IBr Page 5 25. Draw a Lewis structure for the C 2H4 molecule. What is the hybrid orbital set used by either of the carbon atoms for bonding? A) sp 3d 2 B) sp C) sp 3d D) sp 3 E) sp 2 26. Which one of the following hybrid orbital sets is used by the central atom for −bonding in the AsF5 molecule? A) sp B) sp 2 C) sp 3 D) sp 3d E) sp 3d 2 27. How many -bonds and -bonds, respectively, are there in an N 2H2 molecule? A) 2 -bonds and 2 -bonds B) 4 -bonds and 0 -bonds C) 3 -bonds and 0 -bond D) 3 -bonds and 1 -bond E) 2 -bonds and 1 -bond 28. The PCl3 molecule employs hybrid orbitals centered on the phosphorus atom in its bonding scheme, according to valence bond theory. What is the name of the hybrid orbital set used by the phosphorus atom in this molecule? ________ 29. A comparison of the two molecules, SbF5 and IF5, using VSEPR theory reveals that A) the IF5 is polar and the SbF5 is non-polar B) both molecules are non-polar C) the SbF5 is polar and the IF5 is non-polar D) both molecules are polar E) both molecules have lone pairs in the valence shell of the central atom Page 6 Answer Key 1. B 2. A 3. D 4. D 5. 55.4 kJ 6. −465.2 kJ 7. D 8. D 9. D 10. C 11. C 12. B 13. E 14. A 15. D 16. 9 17. C 18. C 19. A 20. A 21. B 22. E 23. A 24. E 25. E 26. D 27. D 28. sp 3 29. A Page 7