Final answer:
The color of light affects metals through the photoelectric effect, where light above a certain frequency can eject electrons from the metal. Different colors of light have different energies, which can impact the kinetic energy of the ejected electrons. The perceived color of a metal results from the frequencies of light it reflects.
Step-by-step explanation:
The effect of different colors of light on metals is closely related to a phenomenon known as the photoelectric effect. When metals are exposed to light of varying colors, which correspond to different frequencies, the energy of the light affects the electrons in the metal. Red, yellow, orange, green, blue, indigo, and violet light each have different energies, with red having the least energy and violet having the most.
Upon exposure to the different colors of light, the metal may eject electrons if the light's frequency is above a certain threshold frequency specific to that metal. Below this threshold frequency, no matter how intense the light is, no electrons are ejected. Above the threshold, the kinetic energy of the ejected electrons is directly proportional to the frequency of the light, meaning that light towards the violet end of the spectrum would cause electrons to be ejected with greater kinetic energy than the light towards the red end of the spectrum.
The color you perceive from a metal is a result of the light it reflects. When light falls on the surface, some frequencies are absorbed and others are reflected. The reflected light's frequencies determine the color you see with your eyes. Compounds of transition metals, in particular, are known to be colored because the d-orbitals of the metal ions absorb specific frequencies of light, causing the observed color change on the surface of the metal.