This results in the increase in the magnitude of van der waals forces (London dispersion forces). Consequently, boiling point also increases. It is evident that there is an increase of 20-30 degrees for each carbon atom added to the chain. However, the first few good members are exceptions where the increase in boiling point is relatively more. Among the isomeric alkanes, the branched chain isomers have relatively low boiling points as compared to their corresponding straight chain isomers. Greater the branching of the chain is, lower is the boiling point. This is due to the fact that branching of the chain makes the molecule more compact and brings it closer to a sphere.
Open Educational Resources, webAssign offers a wide selection of affordable, peer-reviewed, high-quality academic content for stem disciplines, including tutorial banks and assessments. Read More, cengage Unlimited, give your students access to all the digital learning platforms, ebooks, online homework and study tools Cengage has to offer—for 119.99 per semester. Physical state, alkanes contain only c-c and c-h sigma bonds which are almost non-polar due to very small difference of electronegativity between carbon and hydrogen atoms. Therefore, alkanes possess weak van der waals forces as the intermolecular forces. Due to the weak interparticle forces, the first four members (C1 to c, j are gases; the next thirteen members, (C5 to C17) are liquids while the higher members are waxy solids. Boiling points, alkanes generally have restaurant low boiling points. The boiling points of n-alkanes increase regularly with the increase in the number of carbon atoms. This can be explained on the basis of interparticle forces. With the increase in the number of carbon atoms, the molecular mass and also the molecular size increases.
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