Hydrogen bonding is not a completely electrostatic interaction between electronegative atoms or molecules (some degrees of electrodynamics exist). However, it is a strong dipole-dipole attraction caused by their electron-deficit. For example between hydrogen ion or bare proton (H+) and hydroxide ion (OH-) forming water molecule H2O. This semi-static property allows the macroscopic thermal phenomena of fluidity as a distinctive attribute for all liquid phase of any substance. Therefore, if there is no electron deficit then hydrogen bond could never have existed either.
This electron deficit raises the question of their whereabouts and seems to indicate an imbalance of localized electric charge configuration. Electric polarity creates two distinct ionic structures: electronegativity and electropositivity. Metals are usually electronegative and nonmetals are electronegative. There are also metalloids having intermediate properties. One mystery in the study of chemistry is why among stable elements there are more metals than nonmetals and why life is almost exclusively composed of nonmetals and metalloids? If the values of relative electronegativity are a measure of chemical attraction for the shared electrons among chemical bonds then smaller values indicate metals and higher values indicate nonmetals. However, rounding these values to the nearest whole numbers they would simply suggest that metals give one unit of electronegativity, metalloids 2 and 3 units, and nonmetals give 4 but no values of 5 or more exist.
Using these whole numbers: 1, 2, 3, and 4, both hydrogen and nitrogen can be considered as metalloids, 2 for hydrogen and 3 for nitrogen. If some of the hydrogen bonds in the DNA molecules, proteins, and amino acids were replaced by nitrogen bonds then a life without hydrogen bonds is a life that could possibly last forever.


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