Final answer:
In the specified case, an electron jumping from energy level 3 to level 7 absorbs energy, often provided by a photon, corresponding to the energy difference between the levels. This process is explained by Bohr's atomic model, which states each energy transition is associated with a fixed energy change. Emission of light is observed when an electron returns to a lower energy level, releasing the absorbed energy.
Step-by-step explanation:
When an electron jumps from energy level 3 to energy level 7 in an atom, it is absorbing a specific amount of energy corresponding to the energy difference between these levels. This process is part of the atomic excitation in which an electron moves to a higher energy state. The absorbed energy is typically provided by a photon (a particle of light). Once in the higher energy level, the electron will eventually release this energy as it 'falls' back down to a lower energy state, often emitting light in the process. This emission of light can be observed in various phenomena such as the colors produced in fireworks or the glow of a gas in a discharge tube.
It is important to note that in this question, the information provided in options a, b, c, and d regarding the behavior of an electron at level 8 is irrelevant for case 1, as we are discussing an electron transitioning from level 3 to level 7.
Bohr's model of the atom explains these electronic transitions and states that each electron orbit, or energy level, has a specific energy value. Thus, the frequency and color of the light emitted upon de-excitation are characteristic of the material and the particular energy transition that has occurred.