A group 2 metal always forms 2+ ions, since the second electron is harder to remove how come you don't find 1+ ions of these in ionic compound formations, How does it always manage to lose both outer electrons? So it takes a certain amount of energy to break a bond, how does water molecules provide the energy to break the bond in NaCl and dissolve it? Is a Van der Waals binding very transient or does it remain? A bond is never COMPLETELY ionic, it's always shared to some degree, but is it always within the realms of the anions outer shell? I know this next question have been answered in a million places on line but I just can't grasp it. The release of energy when forming a bond. When a Cl atom picks up an extra electron and forms a full shell and an ionic bond with a cation it releases energy, WHERE from is this energy taken? If the Cl atom, where in the Cl atom was this energy before?