Chemistry · Atomic Spectra
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Which of the following electronic transitions would result in the greatest loss in energy for a single hydrogen electron, assuming that its ground state is n = 1?
- A
An electron moves from n = 6 to n = 2.
- B
An electron moves from n = 2 to n = 6.
- C
An electron moves from n = 3 to n = 4.
- D
An electron moves from n = 4 to n = 3.
An atom changes from a ground state to an excited state by taking on energy from its surroundings in a process called absorption. The electron absorbs the energy and jumps to a higher energy level. In the reverse process, emission, the electron returns to the ground state by releasing the extra energy it absorbed.
As the electron transitions from a higher energy level (n=6) to a much lower level (n=2), it releases a significant amount of energy. This transition results in the greatest energy emission compared to other options.
In this case, the electron absorbs energy as it moves from a low energy level (n=2) to a higher one (n=6), which is the opposite of energy loss.
This transition involves the electron absorbing a small amount of energy to move to a slightly higher level (n=4), again indicating energy gain, not loss.
While this transition does involve the release of energy as the electron moves to a lower level (n=3), the energy released is less than that in a transition from n=6 to n=2.
Tagged under Chemistry · Atomic Spectra · 2016