Name: ________________________ Chemistry 113 Reading Assignment Chapter 11 #1 (Sec. 11.1) Look at Figure 11.2 depicting the molecules in the gas, liquid and solid states. What is the variable that is changing as it goes from one state to another? Temperature #2 (Sec. 11.2) A. Intermolecular forces, that is forces of attraction between molecules, is largely a function of the polarity of molecules. For example, in dipole-dipole interactions the greater the polarity of the molecule the stronger the force of attraction. Which of the following molecules would have the greatest dipoledipole forces? Which would have the least? (hint: it may help to draw the molecule) H2O  NH3  CH4 B. Hydrogen bonds are particularly strong dipole-dipole bonds that occur when hydrogen is bound to _______________, ______________ or _____________ (hint: 3 highly electronegative elements). C. London Dispersion Forces are weak intermolecular forces that occur when an electron cloud is deformed or polarized by a neighboring atom or molecule. We’ll discuss this in class. #3 (Sec 11.3) Define: Viscosity – Surface tension – #4 (Sec 11.4) Phase changes, or the transition between states of matter, require transfers of heat energy (i.e., enthalpy). A. Looking at Fig. 11.20 what are the names of the three processes in which heat energy increases? ______________________ ______________________ _____________________ What are the names of the three processes in which heat energy decreases? ______________________ ______________________ _____________________ B. Look at Fig 11.21. Consider why it takes so much more heat energy to go from liquid to gas than to go from solid to liquid. (Hint: refer to Fig 11.1) Any ideas? #5 (Sec 11.5) Define Vapor Pressure in terms of dynamic equilibrium. #6 (Sec 11.6) A phase diagram for a substance shows what state it will be in over a wide range of temperatures and pressures. See Fig 11.27. What does the triple point of a substance mean? What does critical point mean? Look at Figures 11.28 and 11.29, the phase diagrams for H2O and CO2, respectively . What is the temperature and pressure (with units!) at the triple point of each substance? CO2: H2O:  We will skip section 11.7.
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