When an electron transitions from a higher energy level (n=2) to a lower energy level (n=1) in an atom, it moves to a state of lower energy. According to the principles of quantum mechanics and electromagnetic theory, the energy lost by the electron must be conserved. Therefore, this energy is typically emitted in the form of a photon.
Here's a step-by-step reasoning of what happens:
1. Energy Levels: In an atom, electrons orbit the nucleus in defined energy levels or shells. The principal quantum number [tex]\(n\)[/tex] denotes these levels. Here, [tex]\(n=2\)[/tex] represents a higher energy level than [tex]\(n=1\)[/tex].
2. Energy Difference: The energy difference between these two levels is given by the difference in energy between [tex]\(n=2\)[/tex] and [tex]\(n=1\)[/tex]. This energy difference tends to be released when the electron drops to a lower energy state.
3. Photon Emission: To move from the higher energy level (n=2) to the lower one (n=1), the electron must emit a discrete packet of energy. This packet of energy is called a photon. The energy of this photon corresponds exactly to the energy difference between the two levels.
Considering these points, during the transition, a discrete amount of energy is release, and since photons are the carriers of electromagnetic energy, the correct conclusion is:
A photon of energy was released.
This matches option 4. Thus, the most likely event during the transition of an electron from shell [tex]\(n=2\)[/tex] to shell [tex]\(n=1\)[/tex] is:
A photon of energy was released.
