Explain how a bright-line spectrum is produced, in terms of excited state, energy transitions, and groud state

Question

I need to know this for school work. I wrote 'Atoms must absorb energy to become excited. They can't remain in the excited state, so they immediatley return to the ground state. When they do this, they emit energy as light.', but I didn't mention anything about energy transitions. is this answer correct or not? Can you help me please?

Answer 1

Well, the atoms don't absorb the energy; the electrons absorb the energy. Electrons around atoms, without energy, are in an unexcited state, called a ground state. Once energy is absorbed, however, the electrons become excited, meaning they have more energy and are going to release it. Once they are excited, they make a transition from a lower valence shell to a higher valence shell, which is the transition state. Then, the electrons fall back to their own valence shell, releasing the energy, and are put in the ground state again. The energy that is released as quanta, which is how a bright-line spectrum is produced.
You almost got everything right. Remember that the electrons have ground and excited states, not the atoms.

Answer 2

The way atoms emit light is through the electrons. The electrons absorb energy and that is how they are 'excited'. The electrons are at a higher energy level and then fall back to there ground state. during this fall they lose energy which is given off as light. Energy transition is just the movement from potential energy to light as the electron falls to ground state

Answer 3

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Answer 4

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