When is the color emitted from an atom

Color is emitted from an atom when an electron jumps from a higher energy level to a lower energy level

Explanation:

According to Bohr's model of the atom, electrons are arranged into circular orbits, each orbit corresponding to a precise energy level.

In this model of the atom, electrons cannot be between two orbits: this means that the energy level of the atom are discrete, so they can only assume certain values.

As a result, when an electron jumps between two energy levels, it emits/absorbs a photon whose energy is equal to the difference in energy between the two levels.

In particular:

- If an electron jumps from a lower energy level to a higher energy level, it absorbs a photon

- If an electron jumps from a higher energy level to a lower energy level, it emits a photon

The energy of the emitted photon is equal to the difference in energy between the two levels, and it is related to the wavelength of the photon by

where h is the Planck's constant and c the speed of light.

For usual gases, the value of the energy E is such that the value of the wavelength falls within the visible light range of the electronmagnetic spectrums, so we observe light emitted as different colors, depending on the wavelength.

idk i’m struggling too

elements make up everything, and they combine to make compounds.

the answer is c