The same rule of thumb is applied for both the stability of radicals and cations, that the more substituted is the most stable tertiary>secondary>primary»methyl. The thermodynamic stability of radicals is usually measured by the homolytic bond dissociation energy (BDE), whereas hydricity is the heterolytic bond dissociation energy to form a carbocation. Paton and coworkers have automated density functional theory (DFT) calculations at the M06-2X/def2-TZVP level of theory for 42,577 small organic molecules, resulting in 290,664 BDEs. Hereafter, A graph neural network (ALFABET) is trained on a subset of these results to achieve a mean absolute error of 0.58 kcal/mol (vs. DFT) for BDEs of unseen molecules. Lately, they also updated ALFABET, enabling a broader range of chemical space to be studied by this approach . To see if there is a correlation between the experimental hydricities from Parker and coworkers and the ALFABET BDE, we feed ALFABET with the compounds, leaving an MAE and RMSE of 7.58 and 9.44, respectively, Figure . We also check if there is a relationship between our QM method for hydricities and ALFABET. We benchmark against the same functional (M06-2X) and basis set (def2-TZVP) as they use in the article but also benchmark against the best QM method (r 2 SCAN-3c) from section 1. Benchmark study -computational methods are used in the supporting information. For Figure , using the M06-2X functional, we find no correlation between QM computed hydricities and ALFABET BDEs (MAE of 4.56, RMSE of 5.05). However, for Figure , using the functional r 2 SCAN-3c, there is a good correlation with an MAE of 2.60 and RMSE of 3.38. We find it odd that the correlation is so bad for the functional M06-2X and, therefore, also try to calculate BDE using our QM methods. Instead of abstracting a hydride, we now abstract a hydrogen, leaving us with a radical, 𝐴𝐻 𝑠𝑜𝑙𝑣 ⇌ 𝐴 • 𝑠𝑜𝑙𝑣 , see Equation . We leave the hydrogen (H • ) out due to difficulties in validating its exact energy in solution.