The distinctive colors of specific elements when used in fireworks owes to electrons moving from an excited energy state to the ground state.
Neils Bohr in his atomic model postulated that electrons in atoms are found in energy levels. Each energy level corresponds to a fixed amount of energy.
The lowest energy level in the atom is called the ground state and higher energy levels are called excited states.
When an electron receives energy, it can move from a ground state to excited state.
This excess energy is given out as visible light of a characteristic wavelength or color when the electron is moving from an excited energy state to the ground state.
This accounts for the distinctive colors of specific elements when used in
fireworks.
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