Question

Photons of light with a wavelength of 97 nm are being directed through a chamber of hydrogen gas atoms. The gas atoms began in their ground state (ni=1).

Which of the following statements is true?
Hint: It might be helpful to reference the tables on pages 90-92 of the lab manual.
A. There will exactly 3 emission lines produced.
B. This will result in emission of photons in the ultraviolet, visible, and infrared regions of the electromagnetic spectrum.
C. All of these photons will pass through the chamber. None of them will interact with the hydrogen.
D. These photons are in the ultraviolet and quite energetic. They will produce the following electronic transitions: ni=1, nf=2; ni=1, nf=3; ni=1, nf=4; ni=2, nf=3; ni=2, nf=4.

Answer 1

The true statement is option D: These photons are in the ultraviolet and quite energetic. They will produce the following electronic transitions: ni=1, nf=2; ni=1, nf=3; ni=1, nf=4; ni=2, nf=3; ni=2, nf=4.

Step-by-step explanation:

The statement that is true is option D: These photons are in the ultraviolet and quite energetic. They will produce the following electronic transitions: ni=1, nf=2; ni=1, nf=3; ni=1, nf=4; ni=2, nf=3; ni=2, nf=4.

When the photons of light with a wavelength of 97 nm pass through a chamber of hydrogen gas atoms, they interact with the atoms and cause electronic transitions. Based on the energy-level diagram for a hydrogen atom, these photons have enough energy to excite the electrons from the ground state (ni=1) to higher energy levels (nf=2, nf=3, nf=4). Therefore, the statement in option D is true.

Answer 2

Photon emissions from hydrogen gas passing through a chamber produced specific colors corresponding to electronic transitions. The correct statement is D.

Step-by-step explanation:

The given question is about photons of light with a wavelength of 97 nm passing through a chamber of hydrogen gas atoms. The gas atoms start in their ground state (ni=1). Based on the information provided, we know that hydrogen atoms emit light in specific wavelengths when their electrons transition from higher-energy orbits to the second orbit (n = 2). The emission lines produced correspond to the n = 2 to n = 3, n = 2 to n = 4, n = 2 to n = 5, and n = 2 to n = 6 transitions, which are wavelength of 656 nm (red), 486 nm (green), 434 nm (blue), and 410 nm (violet).

Therefore, of the given options, the correct statement is D. These photons are in the ultraviolet and quite energetic. They will produce the following electronic transitions: ni=1, nf=2; ni=1, nf=3; ni=1, nf=4; ni=2, nf=3; ni=2, nf=4.