1. The number of valence electrons in an atom is equal to its _____.A) number of orbits B) period number C) group number D) number of orbitals 2. According to the Lewis dot symbol, the number of electrons in the outermost shell of gallium is _____. A) 2 B) 4 C) 5 D) 3 3. The element having five electrons in the valence shell is _____. A) Al B) N C) S D) Se 4. The element not having seven electrons in the outermost shell is _____. A) Cl B) At C) F D) Tl 5. The most stable ion of the following is _____. A) Br+ B) Mg+ C) Na+ D) Sn3+ 6. The ion not having Octet configuration in the outermost shell is _____. A) Sr2+ B) Fe2+ C) Mg2+ D) S2– 7. Al3+ is not isoelectronic with _____. A) Mg2+ B) F– C) Na+ D) Ca2+ 8. The most stable ion of the following is _____. A) O– B) Bi3+ C) Si3+ D) Hg3+ 9. A favorable condition for two elements to form an ionic bond is _____. A) both should be electropositive B) one should have low electron affinity and the other high ionization energy C) one should have high electron affinity and the other low ionization energy D) both should be highly electronegative 10. Group-1 elements form ionic compounds with group ____. A) two B) eight C) seventeen D) fourteen 11. An ionic compound of the following is _____. A) MgO B) Cl2O7 C) NO D) SiO2 12. NaCl is not a good conductor in _____ state. A) molten B) solution C) vapor D) solid 13. The formula of strontium nitride is ______. A) SrN B) Sr(NO3)2 C) Sr3N2 D) Sr(NO2)2 14. The formula of aluminum sulfide is _____. A) Al2S3 B) AlS C) Al3S2 D) AlS3 15. Cesium sulfate is _____. A) Cs(SO4)2 B) Ce(SO4)2 C) Cs2SO4 D) CsSO4 16. Lithium nitride is ______. A) LiN B) Li3N2 C) LiN2 D) Li3N 17. In an ionic compound, _____. A) the cation is a metal and the anion is the non-metal B) the anion is the metal and the cation is the non-metal C) the negative ion is a metal and the positive ion is the non-metal D) both elements can be metals. 18. Which of the following will form an ionic compound? A) Mg and F B) Si and O C) C and O D) Cl and O 19. Which of the following will form a covalent compound? A) Mg and I B) B and F C) Cs and F D) Ba and Cl 20. Which of the following processes represents lattice energy? A) Na+(s) + Cl–(s) NaCl(s) B) Na+(aq) + Cl–(aq) NaCl (aq) C) Na+(g) + Cl–(g) NaCl(g) D) Na+(g) + Cl–(g) NaCl(s) 21. Born-Haber cycle is used to determine _____. A) electronegativity B) ionic radius C) lattice energy D) energy of formation 22. The compound having the highest lattice energy of the following is _____. A) NaCl B) BaSO4 C) Na2SO4 D) CsI 23. The correct order of lattice energy of the following is _____. A) CsI > LiF B) MgO < KCl C) MgO > KI D) Ba3(PO4)2 < KBr 24. The energy change for the process Li(g) + F(g) Li+(g) + F–(g) is _____ kJ. A) 255 B) 125 C) 192 D) 495 25. The energy change for the reaction A(g) + B(g) A+(g) + B–(g) is _____. A) IE(of A) + EA(of B) B) IE(of A) – EA(of B) C) EA(of B) – IE(of A) D) –(EA(of B) + IE(of A)) 26. Which of the following processes will be exothermic? A) Li(g) + I(g) Li+(g) + I–(g) B) Na(g) + Cl(g) Na+(g) + Cl–(g) C) K(g) + Br(g) KBr(s) D) Na(g) + I(g) Na+(g) + I–(g) 27. According to Lewis's theory, a covalent bond is formed by the _____. A) transfer of electrons B) sharing of electrons C) overlap of electrons D) donation of electrons 28. Which of the following compounds contains a lone pair of electrons? A) BH3 B) NH3 C) CH4 D) AlH3 29. How many lone pairs are there at bromine in HBr? A) 6 B) 1 C) 2 D) 3 30. The molecule containing two lone pairs of electrons is _____. A) PH3 A) ethylene B) ethane C) methane D) acetylene 33. The carbon–carbon bond distance is shortest in _____.B) H2S C) HCl D) BH3 31. A) CO2 B) H2O C) C2H2 D) SO2 34. A) benzene B) cyclohexane C) ethylene D) acetylene 36. The compound not containing a multiple bond of the following is _____. A) Cs B) Ca C) F D) C . Which of the following has no unit? A) electron affinity B) electronegativity C) ionization energy D) atomic radius 37. A) CH4 B) H2O C) HI D) PH3 32. The least electronegative element of the following is _____. The molecule containing a triple bond of the following is _____. The molecule containing no lone pairs of electrons is _____. The carbon–carbon bond is strongest in _____. A) ethane B) ethylene C) propane D) acetylene 35. A) LiCl B) BeCl2 C) KCl D) CCl4 42. A) LiCl B) CsI C) NaBr D) KCl 43. The electrostatic attractive force is smallest in _____. which is non-polar of the following. The metal–oxygen bond is covalent in ______. The electrostatic attractive force of the following is largest in _____.38. A) CH4 B) HCl C) Br2 D) N2 40. is _____. The most ionic compound of the following is _____. The molecule. An example of a polar covalent molecule is _____. Which of the following quantities does not represent energy change? A) ionization potential B) electronegativity C) ionization energy D) electron affinity 39. A) Na2O B) CaO C) MnO4– D) CsO . A) CsI B) BeO C) LiF D) KCl 44. A) HCl B) H2 C) CO D) NO2 41. 45. E.8 and 1. 2. E. Which of the following bonds is most ionic in nature? A) Cl–F B) K–O C) LiF D) LiI 51.3. 3.8. The degree of ionic character depends on the difference in _____.8. The chemical bond most covalent in nature of the following is _____. The electronegativities of the elements D. The order of increase in ionic character of the bond in the following compounds is _____. The electronegativities of the elements D. A) LiCl > NaCl > KCl > RbCl B) NaCl < RbCl < LiCl < KCl C) LiCl < NaCl < KCl < RbCl D) NaCl > RbCl > LiCl > KCl 46. A) atomic radius B) electronegativity C) electron affinity D) ionization energy 48. The order of decreasing covalent bond character is A) EG > DF > DG > DE B) DG > EG > DF > DE C) DE > DF > EG > DG D) DE > DG > DF > EG 49.8 and 1. The ionic compound having greatest covalent character is _____. A) NaBr B) CsF C) LiI D) KCl 47. A) C–H B) C–Cl C) H–F D) O–H . F and G are 3.3.3. 3. The order of increasing ionic character is A) DG < EG < DF < DE B) DG < EG < DF < DE C) DE < DF < EG < DG D) EG < DG > DE > DF 50. 2.3. F and G are 3. 52. Fluorine will form a covalent compound with _____.5 C) 0. The electronegativity difference between carbon and fluorine is _____. A) KF B) F2O C) ICl D) CO2 55. A) KH B) Na2O C) CCl4 D) RbCl 57. Which of the following compounds does not exhibit resonance? A) C6H5OH B) CO2 .5 D) 3.5 B) 1. A) 16th group elements B) first period elements C) transition elements D) second period elements 58. A) 2.5 53. A) Mg B) Ca C) S D) Na 56. The ionic bond of the following is _____. A) Cs–F B) N–H C) Si–Cl D) N–B 54. The ionic compound of the following is _____. Which of the following bonds is not possible? A) C = C B) C = H C) C C D) C = O 59. The Octet rule is applicable mainly to _____. The covalent compound of the following is _____. A) SbCl5 B) PCl3 C) SiH4 D) Cl2 65. The species that will exhibit resonance of the following is _____.C) H2O D) NO2 60. A) C–I B) C–Br C) C–F D) C–H . The molecule not obeying the octet rule of the following is _____. how many lone pairs surround the xenon? A) 0 B) 1 C) 2 D) 3 64. A) CH4 B) NO3– C) CCl4 D) C6H12 61. A) N2O5 B) NH4NO3 C) N2O 63. The measurement of bond energy will be accurate in _____. In the Lewis structure of XeO2F2. The strongest bond of the following is _____. A) CCl4 B) Cl2 C) CO2 D) C6H6 66. Which of the following ions will have the maximum number of resonance structures? A) ClO4– B) ClO– C) ClO3– D) ClO2– 62. NNO bond is present in _____. The bond energy of F2 is 156. A) F2(l) 2F(g) B) F2(g) 2F(l) C) F2(g) 2F(g) D) F2(s) 2F(g) 73. The enthalpy of formation of NaCl is given by _____.2 D) 321.9 B) 78. The reaction F(g) + e– F–(g) represents _____. The bond dissociation energy of fluorine is given by the process _____.6 70. A) 39200 B) 92 C) 392 D) 3920 69.9 71. Which of the following processes is exothermic? A) Bond breakage B) ionization C) dissociation D) bond formation 68.3 C) 214.2 B) 303. A) Na(g) + Cl(g) NaCl(g) B) Na(s) + Cl2(g) NaCl(g) C) Na(s) + Cl2(g) NaCl(s) D) Na(s) + Cl2(s) NaCl(s) .67.5 C) –78. A) –156.9 kJ mol–1.5 D) 156. A) electronegativity B) electron affinity C) ionization energy D) bond energy 72. Calculate the average bond energy in O3. The enthalpy of formation of F(g) is _____ kJ mol–1. The N–H bond energy is _____ kJ mol–1. For the reaction O(g) + O2(g) O3(g) H = –107. A) 107.2 kJ. The nitrogen-to-nitrogen bond is shortest in _____. A) NO2 B) N2 C) N2H4 D) N2O4 79.74. NH4+ is isoelectronic with _____. Which of the following processes is exothermic? A) Cl2(g) 2Cl(g) B) Cl(g) + e– Cl–(g) C) Na(g) Na+(g) + e– D) Na(s) Na(g) 76. The C–H bond energy is _____ kJ mol–1. A) 114 B) 414 C) 915 D) 4150 77. A) NH3 B) NO3– C) AlCl4– D) AlCl3 80. A) CCl4 B) CH3+ C) NH4– D) NO3– . A) N2O B) N2O4 C) N2H4 D) N2 78. CH4 is isoelectronic with _____. A triple bond is present in _____. The process Na(g) Na+(g) + e– represents _____. A) electron affinity B) electronegativity C) electropositivity D) ionization energy 75. calculate the average bond energy of the C-C bond.81. Experiments show that it takes 1656 kJ/mol to break all the bonds in methane (CH4) and 4006 kJ/mol to break all the bonds in propane (C3H8). Which of the following ions does not exist? A) I3– B) I– C) IO3– D) F3– 82. A triple bond is present in _____. CO is isoelectronic with _____. Based on these data. A) NO+ B) ZnO C) NiO D) SO 83. A) CN– B) CO32– C) SO32– D) NO 84. Which of the following is not isoelectronic with others? A) CO B) NO+ C) CN– D) N2O 85. A) 347 B) 147 C) 569 D) 78 . 9. 4. 50. 37. 22. 8. 44. 19. 11. C D B D C B D B C C A D C A C D A A B D C B C C B C B B D B A D B D D B A B B B C B B C C C B C C C . 7. 33. 13. 10. 35. 40. 3. 6. 48. 14. 42. 28. 20. 17. 16. 12. 27. 34. 32. 2. 24. 5. 49. 41. 38. 45. 23. 25. 26. 18. 30. 43. 46. 47. 31. 36. 39. 29. 15. 21.Answer Key 1. 68.51. 70. 72. 55. 77. 65. 78. 63. 75. 54. 82. 73. 84. 71. 59. 69. 83. 79. 85. 60. 57. 76. 67. 61. 80. 53. 81. 66. 52. 74. 56. A B A A C C D B C B A C B A B C D C B B B C C D B B D B A C D A A D A . 58. 62. 64. 4. E. D. D. E. B. NCl3 BaCl2 CO SO2 SF4 Which of these pairs of elements would be most likely to form an ionic compound? A. D. D. C. D. C. B. Which of these compounds is most likely to be ionic? A. 5. C. GaAs SrBr2 NO2 CBr4 H2O Which of these compounds is most likely to be ionic? A.Chapter 9 Chemical Bonding I: Basic Concepts Student: ___________________________________________________________________________ 1. 3. 2. C. B. B. C. Which of these compounds is most likely to be ionic? A. KF CCl4 CS2 CO2 ICl Rb2S SrCl2 CS2 CaO MgI2 . Cl and I Al and K Cl and Mg C and S Al and Mg Which of these compounds is most likely to be covalent? A. B. E. E. E. directly proportional to the product of the charges on the bodies. 9. D. C. directly proportional to the sum of the charges on the bodies. D. B. C. Which of these compounds is most likely to be covalent? A. D. CsOH NF3 Sr(NO3)2 CaO LiF Complete this statement: Coulomb's law states that the magnitude of the force of interaction between two charged bodies is A. directly proportional to the product of the charges on the bodies and directly proportional to the distance separating them. B. 8. B. and inversely proportional to the square of the distance separating them. KF CaCl2 SF4 Al2O3 CaSO4 E. 7. E. C. E. Which of these compounds is most likely to be covalent? A.6. and inversely proportional to the square of the distance separating them. The Lewis dot symbol for the a lead atom is A. inversely proportional to the charges on the bodies. D. and directly proportional to the square of the distance separating them. . B. C. C. B. E. C. 13. E. B. Which of these ionic solids would have the largest lattice energy? A. B. The Lewis dot symbol for the chloride ion is A. C. NaCl NaF CaBr2 CsI CaCl2 . E. B. E. C. The Lewis dot symbol for the calcium ion is A. 11. D. D. The Lewis dot symbol for the S 2 ion is A. D.10. 12. D. NaI NaF MgO MgCl2 KF 17. KI KBr KCl KF 18. E. 1. C. NaF NaCl NaBr NaI 16. Which of these solids would have the highest melting point? A.187 kJ/mol . D. Which of these solids would have the lowest melting point? A. C. B.092 kJ/mol 95 kJ/mol 95 kJ/mol 1. D. C. B. D. D.092 kJ/mol 1. C. SrO NaF CaBr2 CsI BaSO4 15. B. C. E. Calculate the energy change for the reaction K(g) + Br(g) K+(g) + Br (g) given the following ionization energy (IE) and electron affinity (EA) values A. Which of these ionic solids would have the largest lattice energy? A. B.14. E. Which of these solids would have the highest melting point? A. D. B. 8 kJ/mol EA (Cl) = 348 kJ/mol Hf (LiCl(s)) = 408.1 kJ/mol A. C. E.8 kJ/mol I1 (Na) = 495. E. C.9 kJ/mol Bond energy (BrBr) = 192. C. B. Use the BornHaber cycle to calculate the lattice energy of LiCl(s) given the following data: H(sublimation) Li = 155. 1456 kJ/mol 806 kJ/mol 450 kJ/mol 902 kJ/mol 421 kJ/mol . E.553 kJ/mol 21.8 kJ/mol A. A.19. B. 40 kJ/mol 40 kJ/mol 736 kJ/mol 857 kJ/mol 1. D. D. Use the BornHaber cycle to calculate the lattice energy of NaBr (s) given the following data: H(sublimation) Na = 177. B. Calculate the energy change for the reaction K(g) + I(g) K+(g) + I (g) given the following ionization energy (IE) and electron affinity (EA) values.2 kJ/mol I1 (Li) = 520 kJ/mol Bond energy (ClCl) = 242. D.5 kJ/mol EA (Br) = 325 kJ/mol Hf (NaBr(s)) = 361. 124 kJ/mol 715 kJ/mol 715 kJ/mol 1429 kJ/mol none of these 20. Which of these elements is the least electronegative? A.22. . C. E. D. B. E. D. Na As Ga Cs Sb 23. C. E. C. B. D. D. B. E. Mg Ga Si Ba Pb 27. E. D. E. B. A polar covalent bond would form in which one of these pairs of atoms? A. C. Li Cs P As Ge 24. B. Which of these elements has the greatest electronegativity? A. Se Sb K Ga Fe 25. C. Which of these atom is the most electronegative? A. Which of these elements has the greatest electronegativity? A. B. Sr V Ni P I 26. D. C. Which of these elements has the greatest electronegativity? A. . B. A nonpolar covalent bond (i. C.e. 32.e. highest percent ionic character)? A. D..e. Which of these bonds would have the greatest polarity (i. pure covalent) would form in which of these pairs of atoms? A. highest percent ionic character)? A. C. 30. E. D. Ionic bond Nonpolar covalent bond Polar covalent bond Coordinate covalent bond 29... B.28. B. E. B. Which of these covalent bonds is the most polar (i. The covalent bond with the greatest polarity would form in which of these atom pairs? A. D. E. D. D. C. C. 31. C. B. What type of chemical bond holds the atoms together within a water molecule? A. E. ionic polar covalent nonpolar covalent 38. E. polar covalent. B.33. E. C. or nonpolar covalent. D. polar covalent. In which of these pairs of atoms would the bond be the most polar? A. In which of these pairs of atoms would the bond be the least polar (i. D. or nonpolar covalent. C. . In which of these pairs of atoms would the bond have the greatest percent ionic character (i. C.e. C. Classify the A. most polar)? A. E. bond in CH3OH as ionic. 34. 36. C.e. ionic polar covalent nonpolar covalent bond in CaCl2 as ionic. B. bond in CCl4 as ionic. 35. polar covalent. C. Classify the A. Classify the A. or nonpolar covalent. ionic polar covalent nonpolar covalent 37. B. B.. B.. B. D. lowest percent ionic character)? A. 43. three single bonds and 10 lone pairs. 1 2 3 4 5 41. 44. and 8 lone pairs. D. C. C. three single bonds and one lone pair. B. D. 18. E. The total number of bonding electrons in a molecule of formaldehyde (H2CO) is A. 3. two single bonds. 10. one single bond. 6. B. and 9 lone pairs. two double bonds. The electron dot formula for O2 shows A. a total of 8 2 = 16 electron dots. a double covalent bond. The number of lone electron pairs in the N2 molecule is ___. 42. E. A. B. 13. an ionic bond. 9.39. a single covalent bond. The Lewis structure for CS2 is: A. B. C. 4. C. 8. E. The total number of lone pairs in NCl3 is A. D. a total of 84 electron dots. one double bond. 6. . a total of 32 electron dots. 40. 8. E. C. D. B. B. D. D. C. The electron dot structure for AsCl3 shows A. E. D. B. 10 3. C. A. B. Which of these choices is a correct Lewis structure for ozone. 9 2. C. Which of these Lewis structures is incorrect? A. 9 46. ClO3. E. The Lewis structure for a chlorate ion. 0. 8 3. 2. 47. should show ____ single bond(s). ____ double bond(s). E. 1. 0.45. O3? A. 10 2. 1. C. . D. and ____ lone pair(s). 1. B. E. D. +3 and/or 2. The number of resonance structures for the sulfur dioxide molecule that satisfy the octet rule is A. How many resonance structures are there for the cyclobutene molecule (C4H6.g. 1 2 3 5 8 53. B.. C. 2. C. E. How many covalent bonds will a nitrogen atom usually form? A.48. 3. B. B. The number of resonance structures for the nitrate ion that satisfies the octet rule is A. is very reactive although it is isoelectronic with the very stable CO2 molecule. the four carbon atoms are arranged in a ring)? A. D. none of these. Lewis structures with large formal charges (e. B. 50. 3. none of these. there are resonance structures for azide ion but not for carbon dioxide. 2. D. C. +2. E. a Lewis structure cannot be written for the azide ion that has nitrogen formal charges of zero. E. 1. D. 49. D. 4. B. This reactivity is reasonable because A. The preferred Lewis structure is one in which positive formal charges are on the most electronegative atoms. Which of these statements is a useful guideline for the application of formal charges in neutral molecules? A. C. . E. B.3) are preferred. 52. there is no valid Lewis structure possible for the azide ion. 1. nitrogen cannot form multiple bonds. E. N3. The azide ion. C. D. charged species always decompose in solution. A Lewis structure in which there are no formal charges is preferred. 4. C. 1 2 3 4 none of these 51. B. +1. D. C. +2. D. E. B. C. 1. The formal charge on the bromine atom in BrO3 drawn with three single bonds is A. What is the formal charge on sulfur in the best Lewis structure for the SCN (thiocyanate) ion? A. What is the formal charge on the singly bonded oxygens in the Lewis structure for the carbonate ion? A. E. +1. 0. 2. E. B. D. B. What is the formal charge on the oxygen atom in N2O (the atomic order is NNO)? A. D. 56. C. +2. B.54. 2 1 0 +1 +2 59. What is the formal charge on phosphorus in a Lewis structure for the phosphate ion that satisfies the octet rule? A. 0. C. 57. C. C. 2. B. +2 2 +1 1 0 58. The formal charge on the sulfur atom in the resonance structure of sulfur dioxide which has one single bond and one double bond is A. E. 0 +1 1 2 +2 55. 1. D. E. D. 2 1 0 +1 +2 . E. 0. D. +1. C. +2 +1 0 1 2 62. E. the formal charge on the central iodine atom is A. 0. What is the formal charge on the central nitrogen atom in the best Lewis structure for nitrous oxide? (The atom connectivity is NNO.) A. B. +2. D.60. In the best Lewis structure for the fulminate ion. C. CH2O ClNO2 H2O CH4 H2S 65. E. E. E. 1. C. is sometimes called "laughing gas". 2. B. D. For which of these species can you draw two resonance structures? A. Each of the three resonance structures of NO3 has how many lone pairs of electrons? A. CNO. 1. B. 64. B. that satisfies the octet rule. Nitrous oxide. E. B. N2O. B. E. C. C. In the Lewis structure of the iodate ion. The formal charge on the beryllium atom in this ion is A. what is the formal charge on the central nitrogen atom? A. D. +2. +1. IO3. 7 8 9 10 13 . BeF42 is called the tetrafluoroberyllate ion. 63. 2 1 0 +1 +2 61. 2. D. C. D. E. B. C. D. Which of these compounds does not follow the octet rule? A. Which of these compounds does not follow the octet rule? A. D. E. 16. Which of these elements is most likely to exhibit an expanded octet in its compounds? A. 18. E. E. HCO2 SCN CNO N3 CO2 67. For which of these species is the best description of the bonding provided by two or more equivalent resonance structures? A. B. Which of these substances will display an incomplete octet in its Lewis structure? A. NF3 CF4 PF5 AsH3 HCl 71. C. E.66. E. B. B. CO2 Cl2 ICl NO SO2 69. O S Na C N 70. C. C. D. C. D. NF3 CO2 CF4 Br2 NO . 14. B. 0. B. D. The total number of lone pairs in the best Lewis structure for the SOF4 molecule is A. D. 68. C. 2. D. C. NF3 H2O AsCl3 GeH4 BF3 74. BE(C=C) + BE(OH) 2BE(CC) BE(CO). D. E. BE(OH) + BE(C=C) BE(CH) BE(CO) BE(CC). The structures of C2H4 and C2H5OH are The enthalpy change due to the reaction of one mole of C2H4 with water to form C2H5OH can be estimated by A. HCl AsCl5 ICl NCl3 Cl2 75. . B. BE(CO) + BE(CC) BE(OH) BE(C=C). C. E.72. E. C. BE(CH) + BE(CO) + BE(CC) BE(OH) BE(C=C). Which of these molecules has an atom with an expanded octet? A. (2) and (4) (2) and (3) (1) and (2) (3) and (4) (1) and (4) 73. E. C. B. B. E. C. B. Which response includes all the molecules below that do not follow the octet rule? (1) H2S (2) BCl3 (3) PH3 (4) SF4 A. D. BE(C=C) 2BE(CC) BE(CO). D. N2O CS2 PH3 CCl4 NO2 76. D. Which of these molecules has an atom with an incomplete octet? A. Which molecule has a Lewis structure that does not obey the octet rule? A. B. D. E. to form carbon dioxide and water vapor. C.77. +2380 kJ/mol +744 kJ/mol +1949 kJ/mol 561 kJ/mol 744 kJ/mol 78. 1759 kJ/mol +653 kJ/mol +1010 kJ/mol 1010 kJ/mol 155 kJ/mol 79. BE(CH) = 456 kJ/mol BE(CC) = 962 kJ/mol BE(O=O) = 499 kJ/mol BE(C=O) = 802 kJ/mol BE(OH) = 462 kJ/mol A. BE(HH) = 436 kJ/mol BE(BrBr) = 192 kJ/mol BE(HBr) = 366 kJ/mol A. B. Estimate the enthalpy change for the combustion of one mole of acetylene. D. E. C2H2. E. B. +262 kJ/mol 52 kJ/mol 104 kJ/mol +104 kJ/mol +52 kJ/mol . Use bond energies to estimate the enthalpy of formation of HBr(g). C. Estimate the enthalpy change for the reaction 2CO + O2 2CO2 given the following bond energies. D. BE(CO) = 1074 kJ/mol BE(O=O) = 499 kJ/mol BE(C=O) = 802 kJ/mol A. B. C. 1360 kJ 2240 kJ 2370 kJ 1540 kJ 1970 kJ . E. BE(CC) = 347 kJ/mol BE(C=O in CO2) = 799 kJ/mol BE(CH) = 414 kJ/mol BE(OH) = 460 kJ/mol BE(O=O) = 498. E. B. Use the bond enthalpy data given to estimate the heat released when 50.4 kJ/mol BE(HH) = 436. 101 kJ/mol 106 kJ/mol +331 kJ/mol +106 kJ/mol +101 kJ/mol 81. Use the bond enthalpy data given to estimate the heat released when 6.80. B. B. Use bond energies to estimate the enthalpy change for the reaction of one mole of CH4 with chlorine gas to give CH3Cl and hydrogen chloride. BE(NN) = 941. C. 228 kJ 340 kJ 107 kJ 46. C. D.4 kJ/mol BE(NH) = 393 kJ/mol A. burns in excess oxygen to yield carbon dioxide and water vapor at 25C. D. C. D. C3H8. BE(CH) = 414 kJ/mol BE(CCl) = 326 kJ/mol BE(HCl) = 432 kJ/mol BE(ClCl) = 243 kJ/mol A.9 kJ 82.0 g of propane gas.7 kJ/mol A.1 kJ 24. E.50 g of nitrogen gas reacts with excess hydrogen gas to form ammonia at 25C. (Given: BE(NN)=941. B. D. 1180 kJ 447 kJ 364 kJ 1230 kJ 16. Estimate the NH bond enthalpy at this temperature. Use the bond enthalpy data given to estimate the heat released when 25. E. 86.83. C.4 kJ/mol) A. C2H2.4 kJ/mol. burns in excess oxygen to yield carbon dioxide and water vapor at 25C. The standard enthalpy of formation of ammonia at 25C is 46. D. predict the formula for the compound formed between magnesium and sulfur.0 g of acetylene gas. BE(CC) = 347 kJ/mol BE(CC) = 812 kJ/mol BE(C=O in CO2) = 799 kJ/mol BE(CH) = 414 kJ/mol BE(OH) = 460 kJ/mol BE(O=O) = 498. B.7 kJ/mol A.3 kJ/mol. . C. 383 kJ/mol 475 kJ/mol 360 kJ/mol 391 kJ/mol 459 kJ/mol 85. predict the formula for the compound formed between lithium and chlorine. BE(HH) = 436.8 kJ 84. E. Using Lewis dot structures. Using Lewis dot structures. Draw a Lewis dot structure obeying the octet rule for ClO2. 91.87. Calculate the energy required for the gas phase process represented by Na(g) + Br(g) Na+(g) + Br (g) 88. 89. Write the chemical equation for which the enthalpy of reaction is the lattice energy of KCl(s). Use the BornHaber cycle to calculate the lattice energy of NaBr(s) given the following data: H(sublimation) Na = 109 kJ/mol I1 (Na) = 496 kJ/mol Bond energy (BrBr) = 192 kJ/mol EA (Br) = 324 kJ/mol Hf (NaBr(s)) = 361 kJ/mol 90. Draw a Lewis dot structure obeying the octet rule for ClO. . Write a Lewis structure for CO32. 97. .92. Draw a Lewis dot structure obeying the octet rule for ClO3. Write a Lewis structure for SO3. PO43. Draw a Lewis dot structure obeying the octet rule for ClO4. 96. 93. 95. Write a Lewis structure obeying the octet rule for the phosphate ion. 94. Write the Lewis structure of HNO3. 98. Write a Lewis structure for NO3. 100. Write the Lewis Structure for AlCl3. is used as rocket fuel. 103. N2H4. . 102. Write the Lewis structure for this compound. Write the Lewis structure for methyl chloride (CH3Cl). 101. Write the Lewis structure for the product that forms when boron trifluoride combines with diethyl ether (C2H5OC2H5).99. Consider the hypothetical element X with electrondot formula Give the formula for the simplest compound this element forms with chlorine. Write the Lewis structure of boron trifloride. Hydrazine. 104. Consider the hypothetical element Y with electrondot formula Give the formula for the simplest compound this element forms with chlorine. and KF. True False 108. A charge of 2+ is most likely to occur for an ion formed from an atom whose electron configuration is 1s22s22p63s23p4. NO. KBr. True False 110. KF will have the highest melting point. only NO2 is an exception to the octet rule. The bond in F2 is described as polar covalent. and N2. True False 109. 107. Of the species NO2. . Consider the hypothetical element Z with electrondot formula Give the formula for the simplest compound this element forms with chlorine. 106. True False 111. Of the substances KCl. The True False bond has less ionic character than the bond.105. C 7.B 22.A 16.A 18.C 10.B 11.C 5.Chapter 9 Chemical Bonding I: Basic Concepts Key 1.C 19.B 8.B 4.A 2.E 20.B 3.D 21.A 15.B 12.A 25.E 14.A Page 1 .C 17.C 24.B 9.C 6.D 13.B 23. D 51.D 44.C 29.B 37.B 42.C 50.D 48.D 34.C Page 2 .B 41.A 52.E 47.C 53.B 38.B 40.C 45.B 49.A 39.B 36.E 28.D 43.E 33.D 35.C 32.C 27.D 46.26.D 31.E 30.A 54. B 62.A 67.A Page 3 .A 63.D 79.B 65.B 57.E 76.C 68.D 60.E 82.B 80.B 66.B 75.A 81.55.E 58.B 83.E 74.D 78.A 73.B 70.C 71.E 56.E 72.D 69.D 77.E 64.D 61.B 59. 94. 93.84. 87.D 85. 86. Page 4 . 738 kJ/mol 90. 172 kJ/mol 88. 91. 92. KCl(s) K+(g) + Cl (g) 89. 98. 101. 100. 97. Page 5 . 96. 99.95. FALSE 108.TRUE 109.FALSE Page 6 . carbonhydrogen single bonds are not shown explicitly) 104.FALSE 110.YCl3 106.(for clarity of presentation.XCl4 105.ZCl2 107. 103.FALSE 111.102.