Question

Calculate the wavelength of the light emitted when an electron in a hydrogen atom makes each transition and indicate the region of the electromagnetic spectrum (infrared, visible, ultraviolet, etc) where the light is found. n=2 → n=1

Answer 1

The wavelength of the light emitted when an electron in a hydrogen atom makes a transition from n=2 to n=1 is approximately 121.6 nm. This light is found in the ultraviolet region of the electromagnetic spectrum.

Step-by-step explanation:

The formula to calculate the wavelength of light emitted when an electron in a hydrogen atom makes a transition from one energy level to another is given by:

wavelength = (2.18 × 10^-18 J) * (1/n1^2 - 1/n2^2)

where n1 and n2 are the initial and final energy levels, respectively.

For the transition from n=2 to n=1, we have:

wavelength = (2.18 × 10^-18 J) * (1/1^2 - 1/2^2)

Simplifying this equation gives us the value for the wavelength, which is approximately 121.6 nm. Since this wavelength falls in the ultraviolet region of the electromagnetic spectrum, the light emitted during this transition is in the ultraviolet range.