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If energy is stored in chemical bonds, and bond formation is always an exothermic process, doesn't that imply that bond formation both stores and releases energy? How is this possible? I'm clearly not understanding some basic tenet of chemistry. For example, H+ and OH- neutralize to form H2O.
ness and high melting tempera-tures; diamond is the ultimate example. At the other extreme, minerals of molecules held together by weak bonds like van der Waals forces (for sulfur) and hydrogen bonds (the molecular bond for ice) have low hardness and melting temperature. Graphite fa lls off this trend, for good reason. I ts strong covalent bonds in two dimensions preclude disintegration and melting except at extremely high temperature, but the weak bonds between sheets (i.e., in the third dimension) allow mechanical deformation that we recognize as a low hardness. (N ote that diamond