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In fact, why do the PE of atoms decrease when they form bonds, in terms of molecular interpretation, i.e. what actually happened in the atoms making they have lower energies?
The potential energy of atoms decreases when they form bonds because the atoms are able to achieve a more stable state by sharing or transferring electrons with other atoms. This results in a decrease in the overall energy of the system.
Bond formation between atoms lowers their potential energy by allowing them to achieve a more stable electron configuration. This is because the shared or transferred electrons are attracted to the positively charged nuclei of the atoms, resulting in a decrease in potential energy.
The strength of a bond is directly related to the potential energy of the atoms involved. As the potential energy decreases, the bond becomes stronger. This is because the atoms are held together more tightly, making it more difficult to break the bond.
Atoms with higher atomic numbers have more electrons, making it more difficult for them to achieve a stable electron configuration. This results in a higher potential energy when forming bonds, as the atoms must overcome stronger repulsive forces between their electrons to share or transfer them.
Bond formation increases the stability of atoms by allowing them to achieve a more favorable electron configuration. This results in a decrease in potential energy and a more stable overall system. In some cases, atoms may even form multiple bonds to achieve an even lower potential energy and greater stability.