Ch. 14 & 7  IMF & chemical equations     test      100 points  (20 points extra credit)      honors chemistry

1. Describe the basis of London IMF in nonpolar compounds; include temporary dipole & induced dipole in your response.  [10 points]

2. The boiling point of HF, HCl, and HBr is 19, - 85, and – 67 ºC, respectively.  Rationalize the relative boiling points of these compounds using concepts of IMF.  [15 points]

3.  Sketch / label the vapor pressure versus temperature relationship for CH4 and CH3CH3.  Justify / rationalize the relative vapor pressure between these two compounds.  [15 points]

4. In regards to carbon dioxide and water,  [30 points]

a.  Identify the type(s) of IMF in each compound; justify / rationalize your observations

b.  Sketch / label a bar graph showing the relative strength of the type(s) of IMF in each compound; justify / rationalize / label your sketch in regards to the relative strength of the type(s) of IMF and the total IMF in each compound.

c.  Based on your response in part b, what is the relative vapor pressure of these compounds ?  rationalize / justify your response

5.  Write the unbalanced chemical equation describing the following chemical reactions; include information on the state / phase of the chemical, e.g solid, etc. [20 points]

a. Mixing aqueous solutions of calcium chloride and potassium phosphate forms an aqueous solution of potassium chloride and a precipitate of calcium phosphate.

b.  The combustion of liquid propane and oxygen generates carbon dioxide and water.

6. Balance the following chemical equations using the lowest ratio of integers; if a coefficient is one, then write “1”.   [30 points]

a.  ___  CH3CH2CH3  +   ___ O2  →    ___  CO2  +   ____  H2O

b.  ___  MgCl2  +  ___  Li3PO4   →   ___  Mg3(PO4)2  +  ___  LiCl

c.  ___ sodium bicarbonate  +  ___ sulfuric acid  →  ___ carbon dioxide  +  ___ water  +   ___ sodium sulfate