# Why does magnesium have an exceptionally low melting point?

Why does magnesium have a lower melting point than both calcium and beryllium? It does not seem to fit into the group trend.

• I'm not sure I'd consider 922 K (Mg) relative to 1112 K (Ca) exceptionally low. And given Sr (1041 K), Ba (1002 K) and Ra (973 K) perhaps the question might be why is calcium's melting point a tad higher than you might expect. Now if magnesium's melting point were 250 K, that might be exceptionally low compared with the rest of the column. – Jon Custer Jun 9 '15 at 14:42

Following up on my comment, even though I'm not convinced that this is a 'real' answer to the question. Consulting the SGTE database of elemental free energies [1] (with various updates over the years), one can obtain the melting temperatures for the hcp, fcc, and bcc phases of beryllium, magnesium, calcium, strontium, and barium (rough guesses looking at plots — consider good to approx. $$\pm\pu{5 K}):$$
$$\begin{array}{lrrrcc} \hline \text{Element} & T_\mathrm{m}(\text{hcp})/\pu{K} & T_\mathrm{m}(\text{bcc})/\pu{K} & T_\mathrm{m}(\text{fcc})/\pu{K} & \text{Phase at RT} & \text{Melt phase} \\ \hline \ce{Be} & 1544 & 1560 & 1018 & \text{hcp} & \text{bcc} \\ \ce{Mg} & 922 & 755 & 705 & \text{hcp} & \text{hcp} \\ \ce{Ca} & 940 & 1114 & 1063 & \text{fcc} & \text{bcc} \\ \ce{Sr} & 900 & 1050 & 1030 & \text{fcc} & \text{bcc} \\ \ce{Ba} & 635 & 1000 & 709 & \text{bcc} & \text{bcc}\\ \hline \end{array}$$
Overall, it would appear that the group 2 elements display a wide variety of preferences for crystal structure, and hence bonding energy configurations. Is $$\ce{Mg}$$ unusual? Not really…