![]() For instance, if X = Mg and Y = O, the molecule would be HMgOH with m, n = 1 since both atoms are divalent and one of the unpaired electrons is bonding with the other heavy atom. The m and n values are the number of hydrogen atoms necessary to fill the valency where a single bond is created between the heavy atoms. The X and Y are all atoms between Li and Cl. In this previous study, the X−Y bond strengths are computed from model H mX − YH n molecules ( Doerksen and Fortenberry, 2020). To note, this previous work ( Doerksen and Fortenberry, 2020) did not examine any molecules containing period 4 atoms or higher largely due to a combination of factors including the statistical increase in the sample set, the decrease in atomic abundance (save for Fe, of course), and the complexities of electronic structure computations on molecules involving the mid-row transition metal atoms, most notably iron ( DeYonker, 2015). Hence, the strongest “single bonds” of any small molecules containing astrochemically-relevant atoms coincidentally also contain the elements that are most abundant in the earth’s lithosphere (specifically the mantle) and in rocky bodies in general: O, Mg, Si, and Al. ![]() However, the Be, B, and F are the three least abundant elements on the periodic table until atoms beyond Fe are considered ( Savage and Sembach, 1996). The strongest bonds are actually between Be/B atoms with F atoms in the HBeF and H 2BF molecules. Recent work has shown that the strongest “single bonds” in neutral molecules for atoms on the first three rows of the periodic table are not between the atoms most commonly used in chemistry ( Doerksen and Fortenberry, 2020).
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