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==The effect of Van der Waals' forces==
==The effect of Van der Waals' forces==
Van der Waals' forces play a pivotal role in determining melting (but not boiling or equivalence) points. The greater the molecular mass of a compound, the more protons it possesses, and hence is able to attract electrons in orbitals towards the nucleus to a greater degree. Consequently, electrons are promoted to higher energy levels, and are hence more likely to induce dipoles in adjacent, neighbouring molecules. With molecules of lower molecular mass, the electrons are of lower energy, and are hence less controlled by the consituent atoms; as a result, repulsion between the electrons of two adjacent molecules tends to dominate over the electrostatic attraction of the induced dipoles. This would explain why water has a lower melting point than 5,5,6-trimethyldodecanoate.
Van der Waals' forces play a pivotal role in determining melting (but not boiling or equivalence) points. The greater the molecular mass of a compound, the more protons it possesses, and hence is able to attract electrons in orbitals towards the nucleus to a greater degree. Consequently, electrons are promoted to higher energy levels, and are hence more likely to induce dipoles in adjacent, neighbouring molecules. With molecules of lower molecular mass, the electrons are of lower energy, and are hence less controlled by the constituent atoms; as a result, repulsion between the electrons of two adjacent molecules tends to dominate over the electrostatic attraction of the induced dipoles. This would explain why water has a lower melting point than 5,5,6-trimethyldodecanoate.
Van der Waals' forces tend to become more dominant in hydrocarbons with a polar functional group and a significantly larger hydrotrophic, insoluble region (c.f. methyl ethanoate and ethyl methanoate).
Van der Waals' forces tend to become more dominant in hydrocarbons with a polar functional group and a significantly larger hydrotrophic, insoluble region (c.f. methyl ethanoate and ethyl methanoate).