Draw three molecules of each compound, i.e. draw the molecules next to one another to visualize IMF. a. Propane, CH 3 CH 2 CH 3 b. Heptane, CH 3 (CH 2 ) 5 CH 3 c. Propanol, CH 3 CH 2 CH 2 OH d. Heptanol, CH 3 (CH 2 ) 6 OH
1. Draw three molecules of each compound, i.e. draw the molecules next to one another to visualize IMF.
a. Propane, CH 3 CH 2 CH 3
b. Heptane, CH 3 (CH 2 ) 5 CH 3
c. Propanol, CH 3 CH 2 CH 2 OH
d. Heptanol, CH 3 (CH 2 ) 6 OH
2. For each compound, consider whether or not H-bonding can occur between its molecules. Use a dashed line
to show any H-bonding.
3. For each compound, consider whether or not any polar bonds are present.
a. Use a different coloured pen to identify any polar bonds
b. Which compounds are polar? Which compounds are nonpolar? Explain your reasoning
4. Compare your drawings for propanol and heptanol.
a. Which compound has stronger dispersion forces? Explain your answer.
b. Which compound has a higher boiling point? Explain your answer.
5. Compare your drawings of heptane and heptanol.
a. Which compound is more polar? Explain your answer.
b. Which compound is more soluble in water? Explain your answer
Analysis:
1. Which compound has higher solubility in water?
a. A polar compound or a nonpolar compound?
b. A compound that forms H-bonds with water, or a compound that does not form H-bonds with water
c. CH 3 CH 2 CH 2 OH or CH 3 (CH 2 ) 4 OH
2. Which compound has stronger attractions between molecules?
a. A polar compound or a non-polar compound
b. A compound without O-H or N-H bonds, or a compound with O-H or N-H bonds
3. Which compound is likely to have a higher boiling point?
a. A polar compound without O-H or N-H bonds, or a polar compound with O-H or N-H bonds
b. CH 3 CH 2 CH 2 OH or CH 3 (CH 2 ) 4 OH
4. Compare boiling points and solubilities in water for each pair of compounds. Explain your reasoning.
a. Ammonia, NH 3 and methane, CH 4
b. Pentanol, C 5 H 11 OH, and pentane, C 5 H 12
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