Final answer:
The likely outcome when two atoms with the electron configuration 1s²2s²2p⁴ approach each other is that they form a covalent bond as a result of their atomic orbitals overlapping and sharing electrons, resulting in a more stable, lower energy state.
Step-by-step explanation:
When two atoms with the electron configuration 1s²2s²2p⁴ move toward each other, the likely outcome is that they will form a covalent bond. This is because as atoms come close to each other, their atomic orbitals begin to overlap, and they can share electrons. This sharing leads to a lower potential energy of the system due to the new attractive electrostatic interactions that become possible between the nuclei and the electrons of the other atom. However, they also experience an increase in repulsion between the positively charged nuclei as they get closer.
Consequently, the balance between the attractive forces (nucleus-electron attraction) and repulsive forces (nucleus-nucleus and electron-electron repulsion) will ultimately define the bond length where the potential energy is at its minimum. Such a balance results in a stable covalent bond formation, typically illustrated by the bond formed in a molecule like O=O, as shown in Figure 1.2.2. This concept does not involve the exchanging of protons nor radioactive decay, which are more characteristic of nuclear processes.