Final answer:
As atoms bond with each other, they decrease their potential energy and form more stable arrangements of matter. This happens because the attractive forces between electrons and opposing nuclei outweigh the repulsive forces, leading to energy release and stability at the optimal bond distance.
Step-by-step explanation:
As atoms bond with each other, they decrease their potential energy, thus creating more stable arrangements of matter. When two hydrogen atoms approach each other, there is a balance between repulsive forces (electron-electron and nucleus-nucleus) and attractive forces (between electrons and the opposite nucleus). Initially, as the distance between atoms decreases, attractive forces dominate, and the potential energy decreases. This results in the formation of a bond that is energetically favorable, leading to a more stable arrangement of matter.
At the optimal bonding distance, the system's potential energy reaches its lowest point, and the bonded atoms have lower energy than individual atoms, making the arrangement more stable. Hence, when atoms combine to form a molecule, energy is released, signifying a drop in potential energy and an increase in stability. This is analogous to a basketball rolling down a slide—moving toward a state of lower potential energy.
Conversely, if atoms get too close, repulsive forces become stronger than attractive ones, causing an increase in potential energy, which destabilizes the system. However, this scenario occurs beyond the bond distance, which is the point of maximum stability reached when atoms are properly bonded.