Question

The energies of the first three levels of a hydrogen atom are overline epsilon_{1} = - 2.2 * 10 ^ - 18 * J E_{2} = - 5.4 * 10 ^ - 19 J, and E_{3} = - 2.4 * 10 deg J. What is the energy of a photon emitted when an electron transitions from the third to the first energy level? (1 point)

1.7 * 10 ^ - 18 * J

3 * 10 ^ - 19 * J

2 * 10 ^ - 18 * J

O 2.4 * 10 ^ - 18 * J

Answer 1

[AI-generated answer — Bot GPT 3.5]

The energy of the photon emitted can be calculated by taking the difference between the energy levels involved in the transition. Therefore, the energy of the photon emitted when an electron transitions from the third to the first energy level is:

E = E3 - E1
E = (-2.4 * 10^-18 J) - (-2.2 * 10^-18 J)
E = -0.2 * 10^-18 J
E = -2 * 10^-19 J

Therefore, the correct answer is:

3 * 10^-19 J