Unit 4 Vocab and Questions
Bonding and IMFs (Chapter 8, 9, 11)
Due:
Learning Goals:
Be able to…
8.1 Lewis Symbols: Octet Rule:
1. Determine the number of valence electrons for any atom, and write its Lewis symbol
2. Recognize when the octet rule applies to the arrangement of electrons in the valence shell for an atom.
8.2 Ionic Bonding/Lattice Energy:
8.3 Lewis Model for Covalent Bonding:
3. Describe the basis of the Lewis theory, and predict the valence of common nonmetallic elements from
their positions in the periodic table
4. Describe a covalent bond in terms of sharing of electron density between bonded atoms.
5. Describe the formation of a covalent compound using Lewis symbols.
6. Look at a Lewis structure and determine if it properly fits the Lewis model.
7. Describe a single, double, and triple covalent bond.
8.4 Bond Polarity, Electronegativity, and Nomenclature:
8. Explain the significance of electronegativity and relate the electronegativity of an element to its
position in the periodic table.
9. Predict the relative polarities of bonds using either the periodic table or electronegativity values.
10. Name a binary compound given its chemical formula or write the chemical formula given its chemical
name.
8.5/8.6 Drawing Lewis Structures
11. Write the Lewis structures for molecules and ions containing covalent bonds.
12. Write resonance forms for molecules or polyatomic ions that are not adequately described by a single
Lewis structure.
8.7 Exceptions to the Octet Rule
13. Write the Lewis structures for molecules and ions containing covalent bonds and have an odd number
of electrons, a deficiency of electrons, or an expanded octet.
8.8 Strengths of Covalent Bonds
14. Relate bond enthalpies to bond strengths and use bond enthalpies to estimate H for reactions.
9.1/2/3 VSEPR Model
15. Relate the number of electron domains in the valence shell of an atom in a molecule to the geometrical
arrangement around the atom.
16. Explain why nonbonding electron domains exert a greater repulsive interaction on other domains than
do bonding electron domains.
17. Predict the geometrical structure of a molecule or ion from its Lewis structure.
18. Predict whether a molecule can have a dipole moment, from the molecular shape and the
electronegativities of the atoms involved.
9.4/5 Covalent Bonding, Hybrid Orbitals and Molecular Structure
19. Explain the concept of hybridization and its relationship to geometryical structure.
20. Assign a hybridization to the valence orbitals of an atom in a molecule, knowing the number and
geometrical arrangement of the atoms to which it is bonded.
9.5/6 Hybridization in molecules containing both Sigma and Pi bonds
21. Formulate the bonding in a molecule in terms of  bonds and  bonds, from its Lewis structure.
22. Explain the concept of delocalization in  bonds.
9.7/8 Molecular Orbitals
23. Explain the concept of orbital overlap and the reason why overlap may in some cases be zero because
of symmetry.
24. Describe how molecular orbitals are formed by overlap of atomic orbitals
25. Explain the relationship between bonding and antibonding molecular orbitals.
26. Construct the molecular-orbital energy-level diagram for a diatomic molecule or ion built from
elements of the first or second row and predict the bond order and number of unpaired electrons.
Main Goals restated/made more concise:
1. compare and contrast ionic and covalent bonds
2. define and use electronegativity to determine ionic character and bond type
Unit 4 Vocab and Questions
Bonding and IMFs (Chapter 8, 9, 11)
3.
4.
5.
6.
7.
8.
9.
10.
Due:
predict bond polarity and molecular polarity of a molecule
compare and contrast the periodic trends of the radii of atoms and their ions
draw the Lewis structures for atoms, molecules or ions
draw resonance structures for molecules
use the VSEPR model to predict molecular geometry
Use hybridization to predict molecular geometry
draw a molecular orbital diagram for a molecule or a diatomic ion
use molecular orbital theory to predict bond order, bond length, bond strength, and paramagnetic or
diamagnetic properties.
11.1 Kinetic Molecular Theory for Liquids and Solids:
27. Employ the kinetic-molecular model to explain the differences in motion of particles in
gases, liquids, and solids and how these relate to their states.
11.2 Intermolecular Forces: Hydrogen Bonding:
28. Describe the various types of intermolecular attractive forces, and state the kinds of
intermolecular forces expected for a substance given its molecular structure.
11.3/4/5 Physical Properties of Liquids and solids: Changes of State:
29. Explain the meaning of the terms viscosity, surface tension, critical temperature, and
critical pressure, and account for the variations in these properties in terms of
intermolecular forces and temperature.
30. Explain the way in which the vapor pressure of a substance changes with intermolecular
forces and temperature.
31. Describe the relationship between the pressure on the surface of a liquid and the boiling
point of the liquid.
32. Given the needed heat capacities and enthalpies for phase changes, calculate the heat
absorbed or evolved when a given quantity of a substance changes from one condition to
another.
11.6 Phase Diagrams:
33. Draw a phase diagram of a substance given appropriate data, and use a phase diagram to
predict which phases are present at any given temperature and pressure.
11.7/8 Solids:
34. Distinguish between crystalline and amorphous solids
35. Determine the net contents in a cubic unit cell, given a drawing or verbal description of
the cell. Use this information, together with the atomic weights of the atoms in the cell
and the cell dimensions, to calculate the density of the substance.
36. Describe the most efficient packing patterns of equal-sized spheres.
37. Predict the type of solid (molecular, covalent network, ionic, or metallic) formed by a
substance, and predict its general properties.
Main Goals restated/made more concise:
1. Explain how IMFs such as surface tension, capillary action, viscosity, vapor pressure, and
boiling point affect the properties of liquids.
2. Rank substances in order of decreasing or increasing properties such as boiling points.
3. Understand the different types of solids and know examples of each.
4. Know characteristic points of heating curves and phase diagrams.
AP Tip: Although topics in this chapter can appear in the multiple-choice section of the exam, it
is often the case that many of these topics such as the effect of IMFs on properties of liquids and
the structures and properties of solids appear in the essay section.
Unit 4 Vocab and Questions
Bonding and IMFs (Chapter 8, 9, 11)
Due:
Textbook Questions:
Chapter 8 (19 questions)
8.2, 8.4, 8.6, 8.8, 8.9, 8.10, 8.12, 8.25, 8.26, 8.28, 8.35, 8.43, 8.46, 8.53, 8.54, 8.55, 8.56, 8.57,
8.59
Chapter 9 (23 questions)
9.1, 9.2, 9.3, 9.4, 9.9, 9.10, 9.11, 9.12, 9.15, 9.16, 9.17, 9.21, 9.22, 9.23, 9.24, 9.26, 9.27, 9.29,
9.31, 9.37, 9.38, 9.39, 9.40
Chapter 11 (19 questions)
11.1, 11.2, 11.3, 11.4, 11.5, 11.6, 11.7, 11.8, 11.10, 11.11, 11.17, 11.20, 11.25, 11.26, 11.28,
11.29, 11.37, 11.42, 11.47
Vocabulary: Chose 8 words per chapter (Picture, Definition, Sentence)
Chapter 8
Chapter 9
Chapter 11
1. Chemical Bonds
1. Bond angles
1. Intermolecular
2. Ionic Bonds
2. Valence-shell electron-pair
Forces (IMFs)
3. Covalent Bonds
repulsion (VSEPR) model
2. Dipole-dipole
4. Metallic Bonds
3. Electron domains
forces
5. Lewis symbols
4. Bonding pairs
3. London dispersion
6. Octet rule
5. Nonbonding pairs
forces
7. Lattice energy
6. Molecular geometry
4. Hydrogen bonding
8. Lewis structures
7. Bond dipoles
5. Ion-dipole forces
9. Bond polarity
8. Valence-bond theory
6. Polarizability
10. Nonpolar covalent
9. Hybrid orbitals
7. Viscosity
bond
10. Hybridization
8. Surface tension
11. Polar covalent bond
11. Sigma bond
9. Capillary action
12. Electronegativity
12. Pi bond
10. Phase changes
13. Polar molecule
13. Molecular orbital theory
11. Vapor pressure
14. Dipole
14. Molecular orbitals (MOs)
12. Dynamic
15. Dipole moment
15. Bonding molecular orbital
equilibrium
16. Formal charge
16. Antibonding molecular orbital
13. Volatile
17. Resonance
17. Paramagnetism
14. Phase diagram
structures
18. Diamagnetism
15. Phase diagram
18. Bond enthalpy
16. Crystalline solid
19. Bond length
17. Amorphous solid
18. Crystal lattice