Acids: arachidic acid, palmitic acid, lauric acid, etc.
Alcohols: butan-1-ol, pentan-1-ol, etc.

The melting points of acids with $\ce{-COOH}$ at the end compared to melting points of alcohols, $\ce{-OH}$ at the end, is higher. I need to relate this to intermolecular forces. I was going to say that because of many more electrons in the acids, there are greater London dispersion forces and also more polarity (dipole dipole forces) because of the $\ce{COOH}$ at one end. Is this correct?


2 Answers 2


The ultimate goal of melting-point reasoning is to explain how intermolecular forces lead to better packing of molecules in the solid phase.
Both alcohols and organic acids have hydrogen bonds, but organic acids have stronger hydrogen bonds due to the withdrawing carbonyl group, $\ce{COO-}$. This causes the acids to interact stronger with each other. More importantly, organic acids form dimers (usually) with their hydrogen bonds (acetic acid dimer, for example). For this reason, the packing of the acids in the solid phase is significantly better than that of alcohol; hence the higher melting point. Acetic acid: $16~^\circ\mathrm{C}$ vs. $-114~^\circ\mathrm{C}$ for ethanol.

  • $\begingroup$ Thanks! If I say that there are more london dispersion forces as well because of higher number of electrons would that also be correct? $\endgroup$
    – NoobCoder
    Commented Mar 2, 2015 at 6:47
  • $\begingroup$ Welcome to chemistry.se! If you have questions about how to beautify your posts, have a look at the help center. Do you want to know more about this site, please take the tour. I have updated your post with chemistry markup. If you want to know more, please have a look here and here. Please do not use markup in the title field, see here for details. $\endgroup$ Commented Mar 2, 2015 at 7:20
  • $\begingroup$ @NoobCoder Here we are comparing two classes of compounds: acids and alcohols, not individual molecules, so to compare the number of electrons is probably a vague comparison. Besides, suppose we're comparing acetic acid and ethanol, the acetic acid would have more electrons than ethanol because it has an extra oxygen. The extra electrons may increase that polarizability a bit for acetic acid, but it would help if the acetic acid molecules don't come close together. It is the dimerization that helps the molecules pack closer together and increase the melting point. $\endgroup$
    – Huy Nguyen
    Commented Mar 2, 2015 at 21:23

Huy Nguyen has already addressed the importance of dimers through hydrogen bonds in the solid state of alkanoic acids.

If you want to correlate the chain length of alkanoic acids of the form $\mathrm{{C_{n}H_{{2n+1}}-COOH}}$ with their melting points, a look at the data might be helpful:

\begin{array}{lrr} \mathrm{(trivial)\ name} & \mathrm{n} & \mathrm{mp}\\ \mathrm{\tilde{} acid} & & \mathrm{[°C]}\\ \hline \mathrm{acetic} & 1 & 17\\ \mathrm{propionic} & 2 & -21\\ \mathrm{butyric} & 3 & -5\\ \mathrm{valeric} & 4 & -32\\ \mathrm{caproic} & 5 & -3.4\\ \mathrm{enathic} & 6 & -7.5\\ \mathrm{caprylic} & 7 & 16.7\\ \mathrm{pelargonic} & 8 & 12.5\\ \mathrm{capric} & 9 & 31.6\\ \mathrm{undecanoic} & 10 & 28.6\\ \mathrm{lauric} & 11 & 48.3\\ \mathrm{tridecanoic} & 12 & 41.5\\ \mathrm{myristic} & 13 & 54.4\\ \mathrm{pentadecanoic} & 14 & 31.6\\ \mathrm{palmitic} & 15 & 28.6\\ \mathrm{margarinic} & 16 & 48.3\\ \mathrm{stearic} & 17 & 41.5\\ \mathrm{nonadecanoic} & 18 & 54.4\\ \mathrm{arachic} & 19 & 75.5\\ \mathrm{behemic} & 21 & 80\\ \mathrm{lignoceric} & 23 & 84.2\\ \mathrm{montanic} & 27 & 90.9\\ \end{array} (Source: German and english wikipedia)

Plotting melting points vs length of the alkyl substituent gives the following result: enter image description here


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