AP Chemistry Chapter 8 and 9 Jeopardy Jennie L. Borders

Round 1 – Chapter 8 Basic Concepts of Chemical Bonding

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

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

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.

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.

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.

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

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

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

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

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.

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

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

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

Draw the Lewis dot structures for CO.

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

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

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

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

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

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

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

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

Draw the resonance structures for NO2-.

Draw the resonance structures for NO2+.

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 .

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-

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

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.

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.

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

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

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

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

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

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

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.

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.

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.

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

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

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

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

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.

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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.

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