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Lesson Plans
Chemistry: The Central Science 9th Edition ©2003
by Brown, LeMay, and Bursten
Weeks 12–13: Solids, Liquids, Changes in Phase and Intermolecular Forces
Chapter 11: Intermolecular Forces, Liquids, and Solids
College Board Performance Objectives:
- Understand the kinetic molecular theory explanation of physical states.
- Describe the types of intermolecular force and be able to state the type expected for a substance knowing its molecular structure.
- Know the meaning of viscosity, surface tension, critical temperature, and critical pressure, and how they relate to the intermolecular force.
- Understand how vapor pressure depends on intermolecular attraction and temperature.
- Define boiling point.
- From the heat capacities and enthalpies of state change needed, be able to calculate the amount of heat to change a substance from one temperature and state to another.
- Predict the type of solid (ionic, molecular, metallic, or covalent network) a substance is and the properties it has because of this.
College Board Lab Objectives:
Not applicable.
Suggested Labs:
No labs are specific to this lesson.
Resources:
- Instructor's Resource Manual, pp. 129–145
- Student's Guide, pp. 228–248
- Test Bank, pp. 424–458
- Instructor's Resource CD, Chapter 11
Pacing Guide:
- Liquid vs. Solid—1 day
- Intermolecular Forces: Ion-dipole, Dipole-dipole, London Dispersion Forces and Hydrogen Bonding—1 day
- Viscosity and Surface Tension in Liquids and Critical Temperature—1 day
- Warming/Cooling Curves, Enthalpies of Phase Changes—1 day
- Vapor Pressure, Boiling Point, and Melting Point—1 day
- Phase Diagrams—.5 day
- Bonding in solids—.5 day
- Block Scheduling
Liquid vs. Solid and Intermolecular Forces should require a block of time. Viscosity and Surface Tension in Liquids and Critical Temperature can be taught in a short period of time. Spend more time on Warming/cooling Curves, Enthalpies of Phase Change; Vapor Pressure, Boiling Point, and Melting Point; and Phase Diagrams. These may need two blocks of time. Have students explain the table on Bonding in Solids, p. 435.
Key Words:
- intermolecular force, p. 407
- condensed phase, p. 408
- ion-dipole force, p. 410
- dipole-dipole force, p. 410
- London dispersion force, p. 411
- polarizability, p. 411
- hydrogen bonding, p. 413
- viscosity, p. 418
- surface tension, p. 419
- capillary action, p. 419
- phase change, p. 419
- heat (enthalpy) of fusion, p. 420
- heat (enthalpy) of vaporization, p. 420
- heat (enthalpy) of sublimation, p.421
- critical temperature, p. 423
- critical pressure, p. 423
- vapor pressure, p. 425
- dynamic equilibrium, p. 425
- volatile, p. 426
- boiling point, p. 426
- phase diagram, p. 427
- normal melting point, p. 428
- triple point, p. 428
- crystalline solid, p. 430
- amorphous solid, p. 430
- crystal lattice, p. 431
- molecular solid, p. 437
- covalent network solid, p. 437
- ionic solid, p. 438
- metallic solid, p. 440
Suggested Exercises:
Critical thinking questions and end-of-chapter activities are included in these exercises.
- pp. 442–449, # 1, 3, 7, 9, 11, 13, 15, 17, 19, 21, 27, 29, 31, 33, 35, 37, 39, 41, 43, 45, 47, 49, 51, 53, 69, 71, 73, 75, 77, 78, 80, 83, 86, 88, 100, 103.
- eMedia Exercise: p. 449, # 106 -108.
Troubleshooting Tips/Error Traps:
- Stress that covalent bonds are not intermolecular forces.
- Hydrogen bonds are intermolecular, not intramolecular, forces.
- Ionic substances do not have molecules.
- Ion-dipole occurs only in mixtures.