Chapter11IM

Chapter11IM - Chapter 11 Intermolecular Forces and Liquids...

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Chapter 11 Intermolecular Forces and Liquids and Solids This chapter introduces the concepts used to explain the properties of liquids and solids. Upon completion of this chapter, your students should be able to: 1. Describe the properties of gases, liquids and solids in terms of density, compressibility and motion of molecules. 2. Explain the difference between intermolecular and intramolecular forces. 3. Identify and give examples of the following forces: ion – ion ion – dipole ion – induced dipole dipole – dipole dipole – induced dipole induced dipole – induced dipole van der Waals dispersion hydrogen bonding 4. Define polarizability and its relationship with intermolecular forces. 5. Assess why H 2 O, HF and NH 3 do not follow the expected trend as shown by the plot in Figure 11.7 6. Use the concepts of intermolecular forces to explain surface tension, capillary action, cohesion, adhesion and viscosity. 7. Describe the structure of water and explain why ice is less dense than water. 8. Sketch density vs. temperature curve for water and describe how this plot has major significance for aquatic life. 9. Explain the difference between crystalline and amorphous solids; give examples of each. 10. Identify coordination numbers for atoms in simple cubic, face-centered cubic, and body- centered cubic structures. 11. List the number of atoms contained in a unit cell for simple cubic, face-centered cubic and body-centered cubic structures. 12. Use geometric concepts to relate a, the edge length of a unit cell, to r, the radius of atoms, in simple cubic, face-centered cubic and body-centered cubic structures. 13. Calculate what fraction of a unit cell is occupied by atoms, and show that the face-centered cubic structure has the closest packing for simple cubic, face-centered cubic and body- centered cubic structures. 14. Perform calculations involving crystal structure, density, atomic radius and the number of atoms per unit cell. 15. Describe how x-ray diffraction is used to determine geometric parameters of solids. 16. Describe the general properties of ionic, covalent, molecular and metallic crystals; give examples of each. 17. Define the following: evaporation condensation
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molar heat of vaporization molar hear of fusion boiling point melting point supercooling sublimation deposition molar heat of sublimation phase changes critical temperature and pressure 18. Use Clausius – Clapeyron equation to solve for vapor pressure at a specific temperature given associated data. 19. Sketch a typical heating curve and identify various aspects of it. 20. Use phase diagrams to identify what phase(s) is/are present given specific conditions. Section 11.1 Kinetic Molecular Theory of Liquids and Solids
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This note was uploaded on 02/08/2012 for the course CHEM 161 taught by Professor Shaklovich during the Spring '10 term at Harvard.

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Chapter11IM - Chapter 11 Intermolecular Forces and Liquids...

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