Name CHE 131, Test 3November 30, 2001Useful information:12,,11ln21TTRHPPvapTvapTvapmolKJR 3145.8Multiple choice, 2 points each1. Which one of the following decreases as the strength of the attractive intermolecular forces increases?(a) the heat of vaporization(b) the normal boiling temperature(c) the extent of deviations from the ideal gas law(d) the sublimation temperature of a solid(e) the vapor pressure of a liquid2. Which best explains the following trend?Element bp (K)He 4Ne 25Ar 95Kr 125Xe 170(a) London forces(b) dipole-dipole interaction(c) hydrogen bonding(d) Le Chatelier's principle(e) none of the above3. Which of the following is NOT determined by the the principal quantum number, n, of the electron in an atom?(a) the energy of the electron(b) the minimum wavelength of the light needed to remove the electron from the atom.(c) the size of the corresponding atomic orbital(s)(d) the shape of the corresponding atomic orbital(s)(e) All of the above are determined by n.4. Which of the following statements is incorrect?(a) Ionic bonding results from the transfer of electrons from one atom to another.(b) Dipole moments result from the unequal distribution of electrons in a molecule.(c) The electrons in a polar bond are found nearer to the more electronegative element.(d) A molecule with very polar bonds can be nonpolar.(e) Linear molecules cannot have a net dipole moment.5. The electron pair in a C-F bond could be considered(a) closer to C because carbon has a larger radius and thus exerts greater control over the shared electron pair.(b) closer to F because fluorine has a higher electronegativity than carbon.(c) closer to C because carbon has a lower electronegativity than fluorine.(d) an inadequate model since the bond is ionic.(e) centrally located directly between the C and F.Short answer6. Draw the Lewis dot structures for each of the following compounds and answer the following questions. (7 points per compound)(a) Does the compound break the octet rule? If so, how?(b) What is the molecular geometry for the compound?(c) Is the compound polar or nonpolar? If the compound is polar, indicate the direction of the polarity.TeF4ICl3BH37. How do dipole-dipole forces differ from hydrogen bonds? In what ways are they similar? (6 points)8. Consider the bonds in the following molecule. (8 points) C CHHH H(a) What is the hybridization on the carbon atoms?(b) Draw and label the orbitals used to make ONE of the C-H bonds as well as the BOTH of the bonds between the carbon atoms.9. Consider the phase diagram given below. What phases are present at points A through H? On the graph, label the triple point, normal boiling point, normal freezing point, and critical point. Which phase is denser, solid or liquid? (15 points)Problems. Show your work and give your answer with the correct number of significant figures for full credit. 10. (a) Provide the electron configuration for chromium, Cr. (4 points)(b) Draw an energy level diagram for Cr+3. (5 points)11. Determine the Hrxn for the isomerization of methyl isocyanide to acetnitrile (shown below) using the attached table of bond dissociation energies. (8 points)N CC C NCHHHHH H12. In Breckenridge, Colorado, the typical atmospheric pressure is 520. torr. What is the boiling point of water (Hvap = 40.7 kJ/mol) in Breckenridge? (Hint: Remember the normal boiling pointof water.) (8 points)Essay. Write your answer in complete sentences using proper grammar.13. How do covalent and ionic bonds differ? What holds the atoms in the compounds together in each case? Explain, giving examples of compounds. (15 points)EXTRA CREDIT (5 points)Describe the demonstration from Wednesday's class and briefly explain the phenomenon