An electron inside a hydrogen atom transitions from the n=3n = 3n=3 energy level to the n=2n = 2n=2 energy level as shown in the diagram, emitting a single photon in the process.
Which row in the table correctly describes what happens to the energy of the electron and identifies the region of the electromagnetic spectrum to which the emitted photon belongs?
(Planck's constant h=6.63×10−34 J sh = 6.63 \times 10^{-34}\text{ J s}h=6.63×10−34 J s, speed of light c=3.00×108 m s−1c = 3.00 \times 10^8\text{ m s}^{-1}c=3.00×108 m s−1, elementary charge e=1.60×10−19 Ce = 1.60 \times 10^{-19}\text{ C}e=1.60×10−19 C)
Energy of the electron: Decreases; Spectral region: Visible
Energy of the electron: Decreases; Spectral region: Ultraviolet
Energy of the electron: Increases; Spectral region: Infrared
Energy of the electron: Increases; Spectral region: Visible