How does the atomic emission spectra relate to how we see color?

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So I’m learning about the atomic emission spectra and I understand how when electrons jump from a higher energy level to a lower energy level, a photon is emitted. How is that related to how we perceive color in the real world? Like when I see a blue-colored water bottom, how is it blue?

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The photon can be emitted at different wavelengths. The wavelength is related to how much energy it has as well as what color it “looks” like to us. The different wavelengths of the photon govern how they are absorbed. [Here](https://en.wikipedia.org/wiki/Spectral_color) is a handy chart that shows what color corresponds to what wavelength.

Kind of related, but not. You are looking in the wrong direction.

We see color because of light reflections (ie the blue water bottle absorbs all wavelengths but reflects blue wavelength.)

Light EMISSION, which is what you are wondering about, is the result of electrons jumping from higher to lower levels causing photons to be emitted. The bigger the level difference, the higher energy, the higher the wavelength.

The bottle itself does not emit light, but reflects it.