1. An exothermic reaction causes the surroundings to A. warm up. B
CHAPTER 6 1. An exothermic reaction causes the surroundings to A. warm up. B. become acidic. C. expand. D. decrease its temperature. E. release CO2 . Answer: A 2. Copper metal has a specific heat of 0.385 J/g·°C. Calculate the amount of heat required to raise the temperature of 22.8 g of Cu from 20.0°C to 875°C. A. B. C. D. E. 3. 1.97 105 J 1.0 102 J 329 J 7.51 kJ 10.5 kJ Answer: D Calculate the amount of heat necessary to raise the temperature of 12.0 g of water from 15.4°C to 93.0°C. The specific heat of water = 4.18 J/g·°C. A. 0.027 J B. 324 J C. 389 J D. 931 J E. 3,890 J Answer: E 4. How much heat is required to raise the temperature of 1,500 g of water from 25°C to 52°C? The specific heat of water is 4.184 J/g·°C. A. 1,500 kJ B. 169 kJ C. 6.27 kJ D. 40.5 J E. 40.5 kJ Answer: B 5. How many degrees of temperature rise will occur when a 25.0 g block of aluminum absorbs 10.0 kJ of heat? The specific heat of Al is 0.900 J/g·°C. A. 0.44°C B. 22.5°C C. 225°C D. 360°C E. 444°C Answer: E 6. If 325 g of water at 4.2°C absorbs 12.28 kJ, what is the final temperature of the water? The specific heat of water is 4.184 J/g·°C. A. 4.21°C B. 4.8°C C. 9.0°C D. 13.2°C E. 2,938°C Answer: D 7. A piece of copper with a mass of 218 g has a heat capacity of 83.9 J/°C. What is the specific heat of copper? A. 0.385 J/g·°C E. 24.5 J/g·°C B. 1.83 104 J/g·°C C. 2.60 J/g·°C D. 1.32 J/g·°C Answer: A 8. When 0.7521 g of benzoic acid was burned in a calorimeter containing 1,000. g of water, a temperature rise of 3.60°C was observed. What is the heat capacity of the bomb calorimeter, excluding the water? The heat of combustion of benzoic acid is 26.42 kJ/g. A. B. C. D. E. 15.87 kJ/°C 4.18 kJ/°C 5.52 kJ/°C 1.34 kJ/°C 752.1 kJ/°C Answer: D 9. Glycine, C2H5O2N, is important for biological energy. The combustion reaction of glycine is given by the equation 4C2H5O2N(s) + 9O2(g) 8CO2(g) + 10H2O(l) + 2N2(g) H°rxn = 3857 kJ. Given that H°f[CO2(g)] = 393.5 kJ/mol and H°f[H2O(l)] = 285.8 kJ/mol, calculate the enthalpy of formation of glycine. A. 537.2 kJ/mol E. 964 kJ/mol B. 268.2 kJ/mol C. 2,149 kJ/mol D. 3,178 kJ/mol Answer: A 10. Given 2Al(s) + (3/2)O2(g) Al2O3(s), H°f = 1,670 kJ/mol for Al2O3 (s). Determine H for the reaction 2Al2O3(s) 4Al(s) + 3O2(g). A. 3,340 kJ/mol E. 835 kJ/mol Answer: A B. 1,670 kJ/mol C. 3,340 kJ/mol /D. 1,670 kJ/mol 11. Calculate the standard enthalpy of formation of liquid methanol, CH3OH(l), using the following information: C(graph) + O2 CO2(g) H° = 393.5 kJ/mol H2(g) + (1/2)O2 H2O(l) H° = 285.8 kJ/mol CH3OH(l) + (3/2)O2(g) CO2(g) + 2H2O(l) H° = 726.4 kJ/mol A. 1,691.5 kJ/mol E. 47.1 kJ/mol B. 238.7 kJ/mol C. 1691.5 kJ/mol D. 47.1 kJ/mol Answer: B 12. Calculate the standard enthalpy change for the reaction 2C8H18(l) + 17O2(g) 16CO(g) + 18H2O(l). Given: 2C8H18(l) + 25O2(g) 16CO2(g) + 18H2O(l) H° = 11,020 kJ/mol 2CO(g) + O2(g) 2CO2(g) H° = 566.0 kJ/mol A. 10,450 kJ/mol E. 10.450 kJ/mol B. 6,492 kJ/mol C. 15,550 kJ/mol D. –6,492 kJ/mol Answer: D 13. Calculate the standard enthalpy change for the reaction 2C8H18(l) + 21O2(g) 8CO(g) + 8CO2(g) + 18H2O(l). Given: 2C8H18(l) + 25O2(g) 16CO2(g) + 18H2O(l) 2CO(g) + O2(g) 2CO2(g) A. 1.0454 104 kJ/mol D. 6,492 kJ/mol 14. H° = 11,020 kJ/mol H° = 566.0 kJ/mol B. 8,756 kJ/mol E. 1.0454 104 kJ/mol C. 1.1586 104 kJ/mol Answer: B Given the thermochemical equation 2SO2 + O2 2SO3, H°rxn = 198 kJ/mol, what is the standard enthalpy change for the decomposition of one mole of SO3? A. 198 kJ/mol Answer: C B. 99 kJ/mol C. 99 kJ/mol D. 396 kJ/mol E. 198 kJ/mol 15. Given H2(g) + (1/2)O2(g) H2O(l), H° = 286 kJ/mol, determine the standard enthalpy change for the reaction 2H2O(l) 2H2(g) + O2(g). 16. A. H° = 286 kJ/mol B. H° = +286 kJ/mol C. H° = 572 kJ/mol D. H° = +572 kJ/mol E. H° = 143 kJ/mol Answer: D Pentaborane B5H9(s) burns vigorously in O2 to give B2O3(s) and H2O(l). Calculate H°rxn for the combustion of 1 mol of B5H9. H°f[B2O3(s)] = 1,273.5 kJ/mol H°f[B5H9(s)] = 73.2 kJ/mol H°f[H2O(l)] = 285.8 kJ/mol A. 1,2735 kJ/mol D. 9,086 kJ/mol B. 4,543 kJ/mol E. 8,448 kJ/mol C. 18,170 kJ/mol Answer: B 17. Given the thermochemical equation 2SO2(g) + O2(g) 2SO3(g), H°rxn= 198 kJ/mol, how much heat is evolved when 600. g of SO2 is burned? A. 5.46 102 kJ 18. C. 1.85 103 kJ E. 3.71 103 kJ D. 59,400 kJ Answer: B Determine the heat given off to the surroundings when 9.0 g of aluminum reacts according to the equation 2Al + Fe2O3 Al2O3 + 2Fe, H°rxn= 849 kJ/mol. A. 7.6 103 kJ E. 2.5 103 kJ 19. B. 928 kJ B. 2.8 102 kJ C. 1.4 102 kJ D. 5.6 102 kJ Answer: C Find the heat absorbed from the surroundings when 15 g of O2 reacts according to the equation O + O2 O3, H°rxn= 103 kJ/mol. A. 4.6 103 kJ B. 48 kJ C. 96 kJ D. 32 kJ E. 110 kJ Answer: B 20. Ethanol (C2H5OH) burns according to the equation C2H5OH(l) + 3O2(g) 2CO2(g) + 3H2O(l), H°rxn = 1367 kJ/mol. How much heat is released when 35.0 g of ethanol is burned? A. 1,797 kJ E. 1,040 kJ B. 1,367 kJ C. 9.61 104 kJ D. 4.78 104 kJ 21. . Answer: E Methanol (CH3OH) burns according to the equation 2CH3OH(l) + 3O2(g) 2CO2(g) + 4H2O(l), H°rxn = 1454 kJ/mol. How much heat, in kilojoules, is given off when 75.0 g of methanol is burned? A. 727 kJ B. 3.22 103 kJ 3 E. 3.41 10 kJ C. 1.45 103 kJ D. 1.70 103 kJ Answer: D 22. Calculate the amount of work done, in joules, when 2.5 mole of H2O vaporizes at 1.0 atm and 25°C. Assume the volume of liquid H2O is negligible compared to that of vapor. [1 L·atm = 101.3 J] A. 6,190 kJ B. 6.19 kJ C. 61.1 J D. 5.66 kJ E. 518 J Answer: B 23. Calculate the amount of work done against an atmospheric pressure of 1.00 atm when 500.0 g of zinc dissolves in excess acid at 30.0°C. Zn(s) + 2H+(aq) Zn2+(aq) + H2(g) A. w = +22.4 kJ E. w = 19.3 kJ 24. B. w = +24.9 kJ C. w = 0 D. w = 2.52 kJ Answer: E A gas is allowed to expand, at constant temperature, from a volume of 1.0 L to 10.1 L against an external pressure of 0.50 atm. If the gas absorbs 250 J of heat from the surroundings, what are the values of q, w, and E? q A. 250 J B. 250 J C. 250 J D. 250 J E. 250 J w 460 J 460 J 460 J 460 J 4.55 J E 210 J 710 J 710 J 210 J 245 J Answer: A 25. At 25°C, the following heats of reaction are known: 2ClF(g) + O2(g) Cl2O(g) + F2O H°rxn = 167.4 kJ/mol 2ClF3(g) + 2O2(g) Cl2O(g) + 3F2O(g) 2F2(g) + O2(g) 2F2O(g) H°rxn = 341.4 kJ/mol H°rxn = 43.4 kJ/mol At the same temperature, use Hess’s law to calculate H°rxn for the reaction: ClF(g) + F2(g) ClF3(g) A. 217.5 kJ/mol D. 108.7 kJ/mol B. 130.2 kJ/mol E. 465.4 kJ/mol C. 217.5 kJ/mol Answer: D (26) Find the ΔH for the reaction below, given the following reactions and subsequent ΔH values: PCl5(g) → PCl3(g) + Cl2(g) P4(s) + 6Cl2(g) → 4PCl3(g) ΔH = -2439 kJ 4PCl5(g) → P4(s) + 10Cl 2(g) ΔH = 3438 kJ answer = 249.8 kJ (27) Find the ΔH for the reaction below, given the following reactions and subsequent ΔH values: 2CO2(g) + H2O(g) → C 2H2(g) + 5/2O2(g) C2H2(g) + 2H2(g) → C2H6(g) ΔH =-94.5 kJ H2O(g) → H2(g) + 1/2O2 (g) ΔH =71.2 kJ C2H6(g) + 7/2O2(g) → 2CO2(g) + 3H2O(g) ΔH =-283 kJ answer = 235 kJ (28) Find the ΔH for the reaction below, given the following reactions and subsequent ΔH values: N2H4(l) + H2(g) → 2NH3(g) N2H4(l) + CH4O(l) → CH2O(g) + N2(g) + 3H2 (g) ΔH = -37 kJ N2(g) + 3H2(g) → 2NH 3(g) ΔH = -46 kJ CH4O(l) → CH2O(g) + H 2(g) ΔH = -65 kJ answer = -18 kJ (29) Find the ΔH for the reaction below, given the following reactions and subsequent ΔH values: H2SO4(l) → SO3(g) + H2O(g) H2S(g) + 2O2(g) → H2SO4(l) ΔH = -235.5 kJ H2S(g) + 2O2(g) → SO 3(g) + H2O(l) ΔH = -207 kJ H2O(l) → H2O(g) ΔH = 44 kJ answer = 72 kJ (30) Find the ΔH for the reaction below, given the following reactions and subsequent ΔH values: 2C2H4O(l) + 2H2O(l) → 2C2H6O(l) + O2(g) C2H6O(l) + 3O2(g) → 2CO2(g) + 3H2O(l) ΔH = -685.5 kJ C2H4O(l) + 5/2O2(g) → 2CO2(g) + 2H2O(l) ΔH = -583.5 kJ answer = 204.0 kJ (31) Find the ΔH for the reaction below, given the following reactions and subsequent ΔH values: N2(g) + 2O2(g) → 2NO 2(g) N2(g) + 3H2(g) → 2NH3(g) ΔH = -115 kJ 2NH3(g) + 4H2O(l) → 2NO2(g) + 7H2(g) ΔH = -142.5 kJ H2O(l) → H2(g) + 1/2O 2(g) ΔH = -43.7 kJ answer = -83 kJ (32) Find the ΔH for the reaction below, given the following reactions and subsequent ΔH values: CO2(g) → C(s) + O2(g) H2O(l) → H2(g) + 1/2O2(g) ΔH = 643 kJ C2H6(g) → 2C(s) + 3H 2(g) ΔH = 190.6 kJ 2CO2(g) + 3H2O(l) → C 2H6(g) + 7/2O2(g) ΔH = 3511.1 kJ answer = 886 kJ (33) Find the ΔH for the reaction below, given the following reactions and subsequent ΔH values: N2H4(l) + CH4O(l) → CH2O(g) + N2(g) + 3H2 (g) 2NH3(g) → N2H4(l) + H2(g) ΔH = 22.5 kJ 2NH3(g) → N2(g) + 3H 2(g) ΔH = 57.5 kJ CH2O(g) + H2(g) → CH 4O(l) ΔH = 81.2 kJ answer = -46.2 kJ (34) Find the ΔH for the reaction below, given the following reactions and subsequent ΔH values: 1/2H2(g) + 1/2Cl2(g) → HCl(g) COCl2(g) + H2O(l) → CH2Cl2(l) + O2(g) ΔH = 47.5 kJ 2HCl(g) + 1/2O2(g) → H 2 O(l) + Cl2(g) ΔH = 105 kJ CH2Cl2(l) + H2(g) + 3/2O 2(g) → COCl2(g) + 2H 2O(l) ΔH = -402.5 kJ answer = -230 kJ (35) Find the ΔH for the reaction below, given the following reactions and subsequent ΔH values: C2H2(g) + 5/2O2(g) → 2CO2(g) + H2O(g) C2H6(g) → C2H 2(g) + 2H2(g) ΔH = 283.5 kJ H2(g) + 1/2O2(g) → H2O(g) ΔH = -213.7 kJ 2CO2(g) + 3H2O(g) → C2H6(g) + 7/2O2(g) ΔH = 849 kJ answer = -705 kJ (36) Find the ΔH for the reaction below, given the following reactions and subsequent ΔH values: HCl(g) + NaNO2(s) → HNO2(l) + NaCl(s) 2NaCl(s) + H2O(l) → 2HCl(g) + Na2O(s) ΔH = 507 kJ NO(g) + NO2(g) + Na2O(s) → 2NaNO2(s) ΔH = -427 kJ NO(g) + NO2(g) → N2O(g) + O2(g) ΔH = -43 kJ 2HNO2(l) → N2O(g) + O2(g) + H 2O(l) ΔH = 34 kJ Answer = -78 kJ (37) Find the ΔH for the reaction below, given the following reactions and subsequent ΔH values: Zn(s) + 1/8S8(s) + 2O2(g) → ZnSO4(s) Zn(s) + 1/8S8(s) → ZnS(s) ΔH = -183.92 kJ 2ZnS(s) + 3O2(g) → 2ZnO(s) + 2SO2(g) ΔH = -927.54 kJ 2SO2(g) + O2(g) → 2SO3(g) ΔH = -196.04 kJ ZnO(s) + SO3(g) → ZnSO4 (s) ΔH = -230.32 kJ Answer = -976.03 kJ Chapter 7 1. What is the wavelength of radiation that has a frequency of 6.912 1014 s1? A. 1.447 1015 nm D. 2.074 1023 nm 2. B. 7.00 102 nm E. 3.00 108 m C. 7.00 105 m Answer: D Calculate the frequency of visible light having a wavelength of 486 nm. A. 2.06 1014 /s D. 1.20 1015 /s 4. C. 2.304 106 nm Answer: B What is the wavelength of radiation that has a frequency of 2.10 1014 s 1? A. 6.30 1022 m D. 1.43 106 m 3. B. 4.337 102 nm E. 4.337 107 nm B. 2.06 106 /s E. 4.86 107 /s C. 6.17 1014 /s Answer: C Calculate the frequency of visible light having a wavelength of 686 nm. A. B. C. D. 4.37 1014 /s 4.37 105 /s 6.17 1014 /s 2.29 1015 /s E. 2.29 106 /s 5. Answer: A What is the energy in joules of one photon of microwave radiation with a wavelength 0.122 m? A. 2.70 10–43 J D. 4.07 1010 J B. 5.43 1033 J E. 2.46 109 J C. 1.63 1024 J Answer: C 6. What is the energy in joules of a mole of photons associated with visible light of wavelength 486 nm? A. 6.46 1016 J D. 12.4 kJ B. 6.46 1025 J E. 246 kJ C. 2.46 104 J Answer: E 7. What is the energy in joules of a mole of photons associated with red light of wavelength 7.00 102 nm? A. 256 kJ D. 12.4 kJ B. 1.71 105 J E. 2.12 1042 J C. 4.72 1043 J Answer: B 8. What is the binding energy (in J/mol or kJ/mol) of an electron in a metal whose threshold frequency for photoelectrons is 2.50 1014 /s? A. 99.7 kJ/mol D. 7.22 1017 kJ/mol B. 1.66 1019 J/mol E. 1.20 106 J/mol C. 2.75 1043 J/mol Answer: A 10. Calculate the energy, in joules, required to excite a hydrogen atom by causing an electronic transition from the n = 1 to the n = 4 principal energy level. Recall that the energy levels of the H atom are given by En = 2.18 10–18 J(1/n2) A. 2.07 1029 J D. 3.27 1017 J B. 2.19 105 J E. 2.25 1018 J C. 2.04 1018 J Answer: C Calculate the wavelength, in nanometers, of the light emitted by a hydrogen atom when its electron falls from the n = 7 to the n = 4 principal energy level. Recall that the energy levels of the H atom are given by 11. En = 2.18 1018 J(1/n2) A. 4.45 1020 nm D. 1.38 1014 nm B. 2.16 106 nm E. 2.16 103 nm C. 9.18 1020 nm Answer: E 12. Calculate the frequency of the light emitted by a hydrogen atom during a transition of its electron from the n = 6 to the n = 3 principal energy level. Recall that for hydrogen En = -2.18 10–18 J(1/n2). A. 1.64 1015 /s B. 9.13 1013 /s C. 3.65 1014 /s D. 1.82 1019 /s E. 2.74 1014/s Answer: E 13. Calculate the frequency of the light emitted by a hydrogen atom during a transition of its electron from the n = 4 to the n = 1 principal energy level. Recall that for hydrogen En = 2.18 10 18 J(1/n2) A. 3.08 1015 /s D. 1.35 1051 /s B. 1.03 108 /s E. 8.22 1014 /s C. 2.06 1014 /s Answer: A 14. Calculate the wavelength of the light emitted by a hydrogen atom during a transition of its electron from the n = 4 to the n = 1 principal energy level. Recall that for hydrogen En = 2.18 1018 J(1/n2) A. 97.2 nm 15. B. 82.6 nm C. 365 nm D. 0.612 nm Answer: A Which one of the following sets of quantum numbers is not possible? A. B. C. D. E. n 4 3 3 2 2 l 3 0 0 1 0 ml 2 1 0 1 0 ms +1/2 1/2 +1/2 1/2 +1/2 E. 6.8 1018 nm Answer: B 16. Which one of the following sets of quantum numbers is not possible? A. B. C. D. E. n 4 3 3 4 2 l 3 2 0 1 0 ml 2 3 0 1 0 ms +1/2 1/2 +1/2 1/2 +1/2 Answer: B 17. What is the maximum number of electrons in a atom that can have the following set of quantum numbers? n = 4 l = 3 ml = 2 ms = +1/2 A. 0 B. 1 C. 2 D. 6 E. 10 Answer: B 18. A possible set of quantum numbers for the last electron added to complete an atom of gallium Ga in its ground state is A. B. C. D. E. n 4 3 4 3 4 l 0 1 1 1 2 ml 0 0 0 1 1 ms 1/2 1/2 +1/2 +1/2 +1/2 Answer: C 19. A possible set of quantum numbers for the last electron added to complete an atom of germanium in its ground state is A. B. C. D. E. n 4 3 4 3 4 l 0 0 1 1 2 Answer: C ml 0 +1 1 +1 +2 ms +1/2 1/2 +1/2 1/2 1/2 20. Electrons in an orbital with l = 3 are in a/an A. d orbital. 21. B. f orbital. C. g orbital. D. p orbital. E. s orbital. Answer: B The number of orbitals in a d subshell is A. 1 B. 2 C. 3 D. 5 E. 7 Answer: D 22. The maximum number of electrons that can occupy an energy level described by the principal quantum number, n, is A. n B. n + 1 C. 2n D. 2n2 E. n2 Answer: D 23. How many orbitals are allowed in a subshell if the angular momentum quantum number for electrons in that subshell is 3? A. 1 B. 3 C. 5 D. 7 E. 9 Answer: D 24. "No two electrons in an atom can have the same four quantum numbers" is a statement of A. B. C. D. E. 25. the Pauli exclusion principle. Bohr's equation. Hund's rule. de Broglie's relation. Dalton's atomic theory. Answer: A The orbital diagram for a ground-state nitrogen atom is 1s A. 2s 2p B. ___ C. D. Answer: A 26. The orbital diagram for a ground-state oxygen atom is 1s A. 2s 2p B. C. D. E. Answer: D 27. 28. The orbital diagram for a ground state carbon atom is 1s A. 2s 2p B. C. D. Answer: D How many unpaired electrons does a ground-state atom of sulfur have? A. 0 B. 1 C. 2 D. 3 E. 4 Answer: C 29. Which element has the following ground-state electron configuration? 1s22s22p63s2 A. Na B. Mg C. Al D. Si E. Ne Answer: B 30. Which element has the following ground-state electron configuration? [Kr]5s24d105p3 A. Sn B. Sb C. Pb D. Bi E. Te Answer: B 31. Which element has the following ground-state electron configuration? [Kr]5s24d105p2 A. Sn B. Sb C. Pb D. Ge E. Te Answer: A 32. The electron configuration of a ground-state Co atom is A. B. C. D. E. [Ar]4s23d7 1s22s22p63s23d9 [Ne]3s23d7 [Ar]4s13d5 [Ar]4s24d7 Answer: A 33. The electron configuration of a ground-state vanadium atom is A. [Ar]4s24d3 B. [Ar]4s24p3 C. [Ar]4s23d3 D. [Ar]3d5 Answer: C 34. The electron configuration of a ground-state copper atom is A. B. C. D. E. [Ar]4s24d4 [Ar]4s24p63d3 [Ar]4s23d9 [Ar]3d9 [Ar]4s13d10 Answer: E 35. The ground-state electron configuration for an atom of indium is A. B. C. D. E. [Kr]5s24p64d5 [Ar]4s23d104p1 [Ar]4s24p63d5 [Kr]5s25p64d5 [Kr]5s24d105p1 Answer: E 36. Which of the following is the ground-state electron configuration of a calcium atom? A. B. C. D. E. [Ne]3s2 [Ne]3s23p6 [Ar]4s13d1 [Ar]4s2 [Ar]3d2 Answer: D 37. How many electrons are there in the 2nd principal energy level (n = 2) of a phosphorus atom? A. 3 B. 5 C. 6 D. 8 E. 10 Answer: D 38. How many electrons are there in the 3rd principal energy level (n = 3) of a phosphorus atom? A. 3 39. C. 6 D. 8 E. 10 Answer: B A ground-state atom of manganese has ___ unpaired electrons and is _____. A. B. C. D. E. 40. B. 5. 0, diamagnetic 2, diamagnetic 3, paramagnetic 5, paramagnetic 7, paramagnetic Answer: D A ground-state atom of vanadium has ___ unpaired electrons and is _____. A. 0, diamagnetic B. 2, diamagnetic C. 3, paramagnetic D. 5, paramagnetic E. 4, diamagnetic 41. Answer: C A ground-state atom of iron has ___ unpaired electrons and is _____. A. B. C. D. E. 42. 0, diamagnetic 6, diamagnetic 3, paramagnetic 5, paramagnetic 4, paramagnetic Answer: E Transition metal elements have atoms or ions with partially filled A. s subshells. B. p subshells. C. d subshells. D. f subshells. E. g subshells. Answer: C 43. Which choice lists two elements with ground-state electron configurations that are wellknown exceptions to the Aufbau principle? A. Cu and C 44. B. Cr and Cu C. Cs and Cl D. Rb and Co E. Fe and Co Answer: B A ground-state chromium atom has how many unpaired electrons? A. 1 B. 2 C. 4 D. 5 E. 6 Answer: E 45. Which of the following is the electron configuration of an excited state of an oxygen atom? A. 1s22s22p4 B. 1s22s22p5 C. 1s22s22p33s1 D. 1s22s22p6 E. 1s22s22p3 Answer: C 46. Which of the following is the electron configuration of an excited state of an iron atom? A. [Ar]4s23d7 B. [Ar]4s23d6 C. [Ar]4s23d8 D. [Ar]4s13d7 E. [Ar]4s13d5 Answer: D 47. Which of the following is the electron configuration of an excited state of a copper atom? A. [Ar]4s23d9 B. [Ar]4s13d10 C. [Ar]4s13d8 D. [Ar]4s23d8 E. [Ar]4s03d10 Answer: A 48. The ground-state electron configuration of Cr, Mo, and Ag are exceptions to the Aufbau principle. Which of the following is the electron configuration for Mo? A. B. C. D. E. 49. [Kr]5s14d5 [Kr]5s24d4 [Xe]6s25d4 [Ar]4s24d4 [Kr]5s24d6 Answer: A Write the ground state electron configuration for the selenium atom. Answer: [Ar] 4s23d104p4 50. Draw the orbital diagram for a selenium atom in its ground state. Answer: [Ar] 4s 51. 3d 4p Write the ground state electron configuration for the phosphorus atom. Answer: [Ne] 3s23p3 52. Draw the orbital diagram for the phosphorus atom in its ground state. Answer: [Ne] 3s 52. 3p Calculate the energy of a photon of light with a wavelength of 360 nm. Answer: 5.5 10 19 J 53. 54. If one electron is added to the outer shell of chlorine, to which element would the configuration be similar? Answer: Argon What is the outermost electron configuration of (a) O (b) S (c) Se (d) Te? Answer: (a) 2s22p4 (b) 3s23p4 (c) 4s23d104p4 (d) 5s24d105p4 55. What is the outermost electron configuration of (a) Be (b) Mg (c) Ca (d) Sr? Answer: (a) 2s2 (b) 3s2 (c) 4s2 (d) 5s2
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