Scandium: bond enthalpies in gaseous diatomic species

The bond energy in the gaseous diatomic species ScSc is 162.8 ±21 kJ mol-1.

The following values refer to neutral heterodiatomic molecules in the gas phase. These numbers may well differ considerably from, say, single bond energies in a solid. All values are given in kJ mol-1.

Table of diatomic ScX bond enthalpies. All values are quoted in kJ mol-1. Each formula in the table (ScO, ScF, and so on) is a link - select these to see visual periodicity representations for bond enthalpies involving scandium to elements of your choice.

Period 1

ScH             ScHe
about 180              

Period 2

ScLi ScBe ScB ScC ScN ScO ScF ScNe
    276 ±63 <= 444 ±21 469 ±84 681.6 ±11.3 589.1 ±13  

Period 3

ScNa ScMg ScAl ScSi ScP ScS ScCl ScAr
      228.7 ±14   477 ±13 331  

Period 4

ScK ScCa ScGa ScGe ScAs ScSe ScBr ScKr
      271.0 ±11   385 ±17 444 ±63  

Period 5

ScRb ScSr ScIn ScSn ScSb ScTe ScI ScXe
          289 ±17    

Period 6

ScCs ScBa ScTl ScPb ScBi ScPo ScAt ScRn

Period 7

ScFr ScRa            


I am grateful to Professor J.A. Kerr (University of Birmingham, UK) for the provision of the bond strengths of diatomic molecules data.

The values given here are at 298 K. All values are quoted in kJ mol-1. Generally, these data were obtained by spectroscopic or mass spectrometric means. You should consult reference 1 for further details. A note of caution: the strength of, say, the C-H bond in the gaseous diatomic species CH (not an isolable species) is not necessarily, the same as the strength of a C-H bond in, say, methane.

The strongest bond for a diatomic species is that of carbon monoxide, CO (1076.5 ± 0.4 kJ mol-1). The strongest bond for a homonuclear diatomic species is that of dinitrogen, N2 (945.33 ± 0.59 kJ mol-1).


  1. J.A. Kerr in CRC Handbook of Chemistry and Physics 1999-2000 : A Ready-Reference Book of Chemical and Physical Data (CRC Handbook of Chemistry and Physics, D.R. Lide, (ed.), CRC Press, Boca Raton, Florida, USA, 81st edition, 2000.

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