Is it a polar molecule? http://i.imgur.com/882FRuf.jpg?

The statement, "All hydrocarbons are non-polar" isn't quite accurate. Alkanes tend not to have permanent dipole moments, but alkenes and alkynes can have permanent dipole moments, depending on their shape, and the arrangement of electrons.

Here's a pretty dilemma.
H2C=CH-CH2-CH3 .............. BP = -6.5C
CH3-CH=CH-CH3 (trans)..... BP = +0.9C
CH3-CH=CH-CH3 (cis) ........ BP = +3.7C

Granted, there is not a lot of difference, but still, there is a range of 10C between two isomers of butene. Can this be accounted for solely by differences in London dispersion forces? No. Cis-2-butene has a smaller, but permanent dipole moment due to the greater electron density at the double bond. This gives it a net dipole moment and a small degree of dipole-dipole attraction (Keesom forces) on top of the London dispersion forces, and a greater boiling point.

It is not a polar molecule. All hydrocarbons are non-polar.