1. AP Chemistry Chapter 8 and 9 Jeopardy
Jennie L. Borders

2. Round 1 – Chapter 8 Basic Concepts of Chemical Bonding

3. 100 200 300 400 500 Lattice Energy Polarity Lewis Dot Structures
Formal Charge
Resonance
Surprise
100
200
300
400
500

4. Round 2 – Chapter 9 Molecular Geometry and Bonding Theories
Click to go to Round 2

5. Lattice Energy 100 Define lattice energy.
Lattice energy is the energy required to completely separate a mole of a solid ionic compound into its gaseous ions.

6. The magnitude of charge and the size of the ions.
Lattice Energy 200
Which factors govern the magnitude of lattice energy of an ionic compound?
The magnitude of charge and the size of the ions.

7. Explain the following trend in lattice energy: BaO > KF.
BaO has a larger magnitude of charge (+2 and -2), KF only has +1 and -1.

8. Lattice Energy 400
Explain the following trend in lattice energy: CaF2 > BaF2.
CaF2 has a smaller cation, so lattice energy is larger.

9. Lattice Energy 500
Arrange the following compounds in order of lowest to highest lattice energy: ScN, KBr, MgO, NaF.
KBr, NaF, MgO, ScN

10. Polarity 100
Of the following pair, which one is a molecular substance and which one is an ionic substance: PbCl4 or RbCl.
PbCl4 = molecular
RbCl = ionic

11. Polarity 200
What is the most electronegative atom in the following set: Ge, As, P, Sn. P

12. All of them except Cl – Cl.
Polarity 300
Which of the following bonds are polar: B – F, Cl – Cl, Se – O, or H – I.
All of them except Cl – Cl.

13. Draw the dipole moment for the following bond O – P.
Polarity 400
Draw the dipole moment for the following bond O – P.
O – P

14. 3 resonance structures, dipoles point toward the O’s
Polarity 500
Draw the dipole moments for the following molecule: NO3-.
3 resonance structures, dipoles point toward the O’s

15. Draw the Lewis dot structure for SiH4.
Lewis Dot Structures 100
Draw the Lewis dot structure for SiH4.

16. Draw the Lewis dot structures for CO.

17. Draw the Lewis dot structure for C2H2.
Lewis Dot Structures 300
Draw the Lewis dot structure for C2H2.

18. Draw the Lewis dot structure for ClO2-.
Lewis Dot Structures 400
Draw the Lewis dot structure for ClO2-.

19. Draw the Lewis dot structure for AsO33-.
Lewis Dot Structures 500
Draw the Lewis dot structure for AsO33-.

20. Determine the formal charges on the atoms of ClO4-.
Formal charge on Cl = +3 and on all the O = -1

21. Determine the formal charges on the atoms of NO+.
Formal charge on N = 0 and O = +1

22. Formal Charge 300 Determine the formal charges on the atoms of SO2.
Formal charge on S = 0 and on both O = 0

23. Formal Charge 400
Determine the formal charges on the atoms of SO3. (make sure all atoms follow the octet rule)
Formal charge on S = +2, on the double bonded O = 0, and on the 2 single bonded O = -1

24. Formal charge on S = +1 and on all O = -1
Determine the formal charges on the atoms of SO32-. (make sure all atoms obey the octet rule)
Formal charge on S = +1 and on all O = -1

25. Draw the resonance structures for NO2-.

26. Draw the resonance structures for NO2+.

27. Resonance 300
Use resonance structures to explain why the C – C bonds in benzene are all the same length.
Benzene can be drawn with alternating single and double bonds. Since resonance structures can be drawn, each bond is considered a 1.5 bond .

28. Predict the ordering of the C – O bond lengths in CO, CO2, and CO32-.
Resonance 400
Predict the ordering of the C – O bond lengths in CO, CO2, and CO32-.
CO, CO2, CO32-

29. Resonance 500
Based on the Lewis structures, predict the ordering of N – O bond lengths in NO2-, NO3-, and NO+.
NO+, NO2-, NO3-

30. Surprise 100
What is the difference in an ionic, covalent, and metallic bond.
An ionic bond is the transfer of electrons between two atoms.
A covalent bond is the sharing of electrons between two atoms.
A metallic bond is the attraction of the positive metal nuclei for the sea of valence electrons.

31. Electronegativity is the ability of an atom of attract an electron.
Surprise 200
Define electronegativity and list the periodic trends.
Electronegativity is the ability of an atom of attract an electron.
Electronegativity increases as you go across a period and decreases as you go down a group.

32. Write the electron configuration for Fe2+ and Fe3+.
Surprise 300
Write the electron configuration for Fe2+ and Fe3+.
Fe2+ = 1s22s22p63s23p63d6
Fe3+ = 1s22s22p63s23p63d5

33. Surprise 400
What is the electronegativity difference for nonpolar, polar, and ionic?
Nonpolar <0.5
Polar 0.5 – 2.0
Ionic >2.0

34. How do you calculate bond enthalpy for a reaction?
Surprise 500
How do you calculate bond enthalpy for a reaction?

35. 200 400 600 800 1000 Vocabulary Bond Angles VSEPR Model Polarity
Hybrid Orbitals
Multiple Bonds
200
400
600
800
1000

36. Vocabulary 200 What does VSEPR stand for?
Valence Shell Electron Pair Repulsion

37. Vocabulary 400 What is a hybrid orbital?
An orbital that has the properties of more than one orbital.

38. Vocabulary 600
What is the difference in molecular geometry and electron domain geometry?
Molecular geometry is the geometry solely based on the arrangement of atoms. Electron domain geometry is the geometry based on both the location of the atoms and the location of the lone electron pairs.

39. What are localized and delocalized electrons?
Vocabulary 800
What are localized and delocalized electrons?
Localized electrons can be located because they are associated with only 2 atoms. Delocalized electrons occur in molecules with resonance and cannot be located because they are associated with many atoms.

40. What is a sigma bond and a pi bond?
Vocabulary 1000
What is a sigma bond and a pi bond?
Sigma bonds are single bonds and the electron density is concentrated between the 2 nuclei.
A pi bond is located in all multiple bonds and is located above and below the central axis of the nuclei.

41. What are the bond angles in the following molecule: BF3.
Bond angles = 120o

42. What are the bond angles in the following molecule: SF6.
Bond angles = 90o

43. What are the bond angles in the following molecule: ClO4-.
Bond angles = 109.5o

44. What are the bond angles in the following molecule: PCl5.
Bond angles = axial 90o
equatorial 120o

45. Explain the bond angle differences in CH4, H2O, and NH3.
Bond Angles 1000
Explain the bond angle differences in CH4, H2O, and NH3.
The bond angles decreases as more lone pairs are added since lone pairs take up more space than bonded electrons.

46. EDG = trigonal bipyramidal
VSEPR Model 200
What is the molecular geometry and electron domain geometry of the following molecule: XeF2.
MG = linear
EDG = trigonal bipyramidal

47. VSEPR Model 400
What is the molecular geometry and electron domain geometry of the following molecule: BrF4.
MG = square pyramidal
EDG = octahedral

48. VSEPR Model 600
What is the molecular geometry and electron domain geometry of the following molecule: XeF4.
MG = square planar
EDG = octahedral

49. EDG = trigonal bipyramidal
VSEPR Model 800
What is the molecular geometry and electron domain geometry of the following molecule: ClF3.
MG = T-shaped
EDG = trigonal bipyramidal

50. EDG = trigonal bipyramidal
VSEPR Model 1000
What is the molecular geometry and electron domain geometry of the following molecule: SF4.
MG = seesaw
EDG = trigonal bipyramidal

51. Nonpolar – dipoles all point towards the F’s and cancel
Polarity 200
Is the following molecule polar or nonpolar: SF6. (If polar, show the overall dipole moment.)
Nonpolar – dipoles all point towards the F’s and cancel

52. Polar – dipole points towards the F
Polarity 400
Is the following molecule polar or nonpolar: IF. (If polar, show the overall dipole moment.)
Polar – dipole points towards the F

53. Nonpolar – dipoles point towards the S’s and cancel
Polarity 600
Is the following molecule polar or nonpolar: CS2. (If polar, show the overall dipole moment.)
Nonpolar – dipoles point towards the S’s and cancel

54. Polar – dipoles point towards the F’s
Polarity 800
Is the following molecule polar or nonpolar: IF5. (If polar, show the overall dipole moment.)
Polar – dipoles point towards the F’s

55. Polar – dipoles point towards the Cl’s
Polarity 1000
Is the following molecule polar or nonpolar: PCl3. (If polar, show the overall dipole moment.)
Polar – dipoles point towards the Cl’s

56. What is the hybridization of the molecule H2O?
Hybrid Orbitals 200
What is the hybridization of the molecule H2O?
sp3

57. What is the hybridization of the molecule CO2?
Hybrid Orbitals 400
What is the hybridization of the molecule CO2? sp

58. What is the hybridization of the molecule SO3?
Hybrid Orbitals 600
What is the hybridization of the molecule SO3?
sp2

59. Draw the hybridization of CH4.
Hybrid Orbitals 800
Draw the hybridization of CH4.

60. Draw the hybridization of BF3.
Hybrid Orbitals 1000
Draw the hybridization of BF3.

61. How many sigma and pi bonds are in N2?
Multiple Bonds 200
How many sigma and pi bonds are in N2?
1 sigma and 2 pi bonds

62. Are the bonds in SO3 localized or delocalized?
Multiple Bonds 400
Are the bonds in SO3 localized or delocalized?
delocalized

63. Are the bonds in NO2- localized or delocalized?
Multiple Bonds 600
Are the bonds in NO2- localized or delocalized?
delocalized

64. Explain the sigma and pi bonds in benzene.
Multiple Bonds 800
Explain the sigma and pi bonds in benzene.
The C-H bonds are all sigma bonds. The C-C/C=C bonds are delocalized pi and sigma bonds.

65. How many sigma and pi bonds are in 1 – propene (C3H6)
Multiple Bonds 1000
How many sigma and pi bonds are in 1 – propene (C3H6)
8 sigma bonds and 1 pi bond