1. The characteristic red color of blood is due to the very strong absorption of light at a wavelength of 420 nm. Calculate the frequency and the energy of a photon with wavelength of 420 nm.

An atom in its ground state absorbs a single photon of light and then relaxes back to the ground state by emitting an infrared photon (1,200 nm) followed by an orange photon (600 nm). What is the wavelength (in nm) of the photon that was absorbed initially?

In scenario A, visible light has a wavelength of 690.3 nm. Determine its frequency, energy per photon, and color. frequency: s-1 energy per photon: The visible light in scenario A is J

An electron in the n= 6 level in hydrogen atom emits a photon with a wavelength of 93.8 nm. To what energy level does the electron move