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Online calculator, figures and tables with the boiling point dcm of hydrocarbons at atmospheric and higher pressure – SI and Imperial units. Boiling and melting points, densities, flash points, autoignition temperatures and pKa-values also given.
The strength of intermolecular attractive forces determines whether a substance exists normally as a liquid or solid and to what extent it is liquified at any given temperature. It is therefore not surprising that the first entries in the table above show the expected pattern; compounds with more electrons and nuclei forming stronger van der Waals attractions have higher boiling points than their similar counterparts made up of smaller molecules.
The presence of hydrogen bonding functions also has a profound effect on boiling points as the second and third rows illustrate. The simple ethers and the isomeric 1o, 2o and 3o-amines have substantially lower boiling points than propanol which has two hydrogen bonding functions and which hence has a much higher boiling point. Likewise, the dimeric form of acetic acid (the ninth entry) held together by two hydrogen bonds has a much higher boiling point than the monomeric one which only has one bond.
The anomalous behaviour of fluorine in the last column is perhaps due to its very high electronegativity which reduces the attraction for the electrons within its molecular orbitals. However, most of the entries in this section confirm that the correlation between total number of electrons and the molecular mass is valid.