Tahmeed said:Why electron and overall an atom is most stable in lowest potential energy? There is a concept of stable equilibrium in classical physics, does it apply here as well? but electron is never in an equilibrium state, neither an atom is.
Then why it tries to be in lowest potential?
Electrons are negatively charged particles and are attracted to positively charged particles. In an atom, the nucleus is positively charged and the electrons orbiting around it are negatively charged. The electrons are naturally drawn towards the nucleus, resulting in them occupying the lowest potential energy level.
The lowest potential energy level for an electron is determined by the number of protons in the nucleus. The more protons an atom has, the stronger the positive charge is, and the closer the electrons are drawn towards the nucleus. This results in a lower potential energy level for the electrons.
Yes, electrons can enter higher potential energy levels if they receive additional energy. This can happen through processes such as absorption of light or collisions with other particles. However, the electrons will eventually return to the lowest potential energy level as it is the most stable state for them.
The lowest potential energy level is the most stable state for an atom. This is because the electrons are in their most tightly bound state and are not easily influenced or affected by external forces. An atom with all its electrons in the lowest energy level is considered to be in its ground state.
In chemical reactions, electrons are involved in the formation and breaking of chemical bonds. The lowest potential energy level ensures that the electrons are in a stable state, making it easier for them to form bonds with other atoms. This is essential for the formation of new molecules and the overall stability of the chemical reaction.