Bond enthalpy of diatomic molecules

The strength of a chemical bond is defined as the standard enthalpy change of the reaction in which the bond M-X is broken to form the two component atoms, M and X. Values given here refer to the bond strengths of the gaseous diatomic species MX.

Units

kJ mol^-1

Notes

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 isolatable 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).

Select from the following links to see visual periodicity representations for single element-halide single bond enthalpies in the highest halides or the single bond enthalpies for homodiatomic molecules M₂.

• Single bond enthalpies in highest bromide
• Single bond enthalpies in highest chloride
• Single bond enthalpies in highest fluoride
• Single bond enthalpies in highest iodide
• Bond enthalpies (M-M single bond)
• Bond enthalpies for homodiatomic molecules M₂ (not necessarily single bonds.

Each formula in the table below (M-O, M-F, and so on) is a link - select these to see visual periodicity representations for bond enthalpies involving your element of choice.

Literature sources

1. D.R. Lide, (ed.) in Chemical Rubber Company handbook of chemistry and physics, CRC Press, Boca Raton, Florida, USA, 79th edition, 1998.