Answer:
Alkenes contains a carbon-carbon double bond. This carbon-carbon double bond changes the physicals properties of alkenes. At room temperatue, alkenes exist in all three phases, solid, liquids, and gases. Melting and boiling points of alkenes are similar to that of alkanes, however, isomers of cis alkenes have lower melting points than that of trans isomers. Alkenes display a weak dipole-dipole interactions due to the electron-attracting sp2carbon.
Alkenes are a family of hydrocarbons (compounds containing carbon and hydrogen only) containing a carbon-carbon double bond. The first two are:
ethene ( C2H4 )
propene ( C3H6 )
You can work out the formula of any of them using: CnH2n . The list is limited to the first two, because after that there are isomers which affect the names.
Explanation:
It is easier to predict the boiling point of heptene rather than its melting point because of their geometrical isomerism.
Melting point is that point at which any compound changes its state from solid to another state liquid, and at this point both the states are present in equilibrium.
It is easier to predict the boiling point of heptene as in this molecule constant number of double bond is present its not changing. But due to double bond heptance shows cis and trans isomer, and among them one isomer will be stable and another one is unstable.
That's why it is not easy to predict the melting point.
Hence, due to geometrical isomers it is not easy to predict melting point.
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