Explain the difference in boiling point between your unknown and the other solvents. For example, you can discuss hydrogen bonding, polarity, molecular weight, whether the structure is branched or linear, etc. My unknown = hexane, boiling point = 69 degrees C Other solvents = 1. ethyl acetate, boiling point = 76-78 degrees C 2. methyl alcohol, boiling point = 64-66 degrees C  3. Acetone, boiling point = 56-57 degrees C  4. Xylenes, boiling point = 138.5 degrees C

Methanol has a melting point of -97.6°C. Naphthalene has a melting point of +80.3°C. Click on the reasons why Naphthalene has a higher melting point. Be careful!! Don't click on responses that don't contribute to the higher melting point of naphthalene even if those statements happen to be true. H 4- H-C H Methanol H H Naphthalene A) Naphthalene has many more atoms so the London forces are much stronger with Naphthalene. B) Methanol is polar and has dipole-dipole forces. C) Methanol has hydrogen bonding forces. D) Methanol has higher London forces because oxygen has more electrons than carbon. E) Napthalene is a non-polar molecule that does not have dipole-dipole forces.

Sort the following molecules from lowest boiling point (bottom) to highest boiling point (top).

The following compounds have similar molecular weights. Which has the highest boiling point? O a. CH3CH2CH3 b. CH3OCH3 O C. CH3CH₂OH d. CH3CH=O