Question

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?

Options

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.

Explanation

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.