1. Arrange the following compounds in order from highest to lowest boiling point. hexanol (C6H14O), dichloromethane (CH2Cl2), CCl4, butene (C4H8), propane (C3H8)
2. Identify the three true statements:
a. Hydrocarbons exhibit only dispersion forces.
b. Stronger intermolecular forces usually correlate with higher boiling points.
c. Hydrogen bonds require carbon, hydrogen, and a halogen.
d. Dipole-dipole interactions are stronger than dispersion forces and hydrogen bonds.
e. Boiling point generally increases with total number of electrons in molecules due to increased strength of dispersion forces.

1. Hexanol (C6H14O) > Carbon tetrachloride (CCl4) > Dichloromethane (CH2Cl2) > butene (C4H8) >  propane (C3H8)

2. a. b and e

Explanation:

1. Arrangement of given compounds in order from highest to lowest boiling point are as following:

hexanol (C6H14O): 157 degree celcius

carbon tetrachloride (CCl4):  76.72 degree celcius

dichloromethane (CH2Cl2): 40 degree celcius

butene (C4H8): -6.3 degree celcius

propane (C3H8): -42 degree celcius

Hexanol (C6H14O) > Carbon tetrachloride (CCl4) > Dichloromethane (CH2Cl2) > butene (C4H8) >  propane (C3H8).

2. True statements are:

a. Hydrocarbons have only dispersion forces because hydrocarbons are very non-polar and are highly symmetric molecules.

b. Stronger intermolecular forces require higher boiling points because the bond between the molecules is very strong and require high energy and boiling point to break that strong bond.

e. Because the size of molecules increases with increase in number of electrons and dispersion force increases the attraction of the molecules to each other. Hence require high boiling point to separate them from each other.