What causes a substance to emit a colored light when it is vaporized in the burner flame?

Each of the metallic ions in these salts has a different electron configuration. The electrons in the metal will absorb differing amounts of energy from the flame and jump to an "excited" state. That means they jump to a higher energy level farther from the nucleus than they would normally occupy. This excited state is not stable for the electrons and they need to return to their normal "ground" state closer to the nucleus. In order to return to the ground state they must emit the same amount of energy as they absorbed from the flame. They emit this energy in the form of electromagnetic radiation. We see this electromagnetic radiation emitted as visible light. The different colors come from the different amounts of energy absorbed due to each metal having a specific electron configuration.

Yes, it does go along with Bohr's theory, but Bohr based his ideas on a flawed theory. Bohr's theory only holds true with hydrogen - an perhaps Li 1+. It does not fit any of the other ions because he did not understand that electron orbitals are not equal in shape and energy. It took the idea of Quantum Mechanics to fully explain and calculate what is happening to the electrons.

mutually as an element is vaporized the electrons are excited and leap as plenty as better skill ranges. mutually as they fall decrease back to floor state, they fall a particular distance that is a wavelength of sunshine. so a lengthy way as I submit to in ideas, all electrons are alike, a similar length, can charge and travelling on a similar velocity. some do spin on their axis in opposite guidelines, which in non pairing, debts for magnetism.

this is called the theory of the boring straights..its complexed so ..