In each pair below, determine the strongest intermolecular force in each of the two compounds as a solid or liquid. Then determine which of the two compounds would have the higher boiling point or melting point.  Explain why you made your choice (using IMFs).    CH3Cl or  CH3CH3                                    HCl or   NaCl                                  C4H10 or C10H22                     KCl or CaS           NH3 or PH3     v

Complete the following table: Substance Cl2 b.p. –34 °C HCl b.p. –85 °C Li m.p. 180 °C LiCl m.p. 610 °C   Composition type (ionic, etc):         Physical state at +200 °C         Physical state at –35 °C         List all IeFs (D, DD, HB, but IaFs for some!) in each :         Rank the strength of their intermolecular forces (IeFs) based on their physical states: has the strongest IeFs– ______ > ______ > ______ > ______ –has the weakest IeFs

Which of the following mixtures/compounds have ion-dipole forces between them?   A HF/HO   B NH/HO   C NsCl/CH   D CsCl/HO

How do you solve this question?

Arrange the following substances in order of increasing enthalpy of vaporization. I 01 < | < III OI< | < | O< < 1 ○ III < 1< || ○ < |<1 "NH₂ G II III

Choose the substance with the highest vapor pressure at a given temperature. O SiS2 O CH3SCH3 RBCI O BF3 O SbH3

What is the vapor pressure of ethanol (in mmHg) at 52.7°C if its vapor pressure is 400.0 mmHg at 63.5°C? (AHvap = 39.3 kJ/mol; R = 8.314 J/K • mol) %3D

How much heat (in kJ) is released in converting 1.00 mol of water as a gas at 105°C to ice at –5.0°C? The heat capacity of H2O (g) is 2.01 J/g · °C The heat capacity of H2O (l) is 4.18 J/g · °C The heat capacity of H2O (s) is 2.09 J/g · °C The heat of fusion for water at 0 °C is approximately 0.334 kJ/g The heat of vaporization for water at 100 °C is 2.230 kJ/g.

Compare and contrast the phase diagrams of water and carbon dioxide. Why doesn't CO2 have a normal melting point and a normal boiling point, whereas water does? The slopes of the solid-liquid lines in the phase diagrams of H2O and CO2 are different. What do the slopes of the solid-liquid lines indicate in terms of the relative densities of the solid and liquid states for each substance? How do the melting points of H2O and CO2 depend on pressure? How do the boiling points of H2O and CO2 depend on pressure? Rationalize why the critical temperature for H2O is greater than that for CO2.

Which should have a higher enthalpy of vaporization, CF4 or CBr4? Explain the role of intermolecular forces in your decision.