Question

reading questions: click here to access the article. read it and then answer the following questions. 1. describe the process in which electrons move and how that leads to the color of the flame. 2. each metallic element you tested gave off a unique color when burned. what does this tell you about the energy levels in the atoms of these metallic elements? explain your answer. 3. draw a bohr model of an atom of hydrogen that shows an electron moving from the ground state to an excited state and back to ground state. include any energy inputs and outputs. (balmer series)

Explanation:

1. When electrons absorb energy, they move to higher - energy levels (excited states). When they return to lower energy levels, they emit photons. The color of the flame is determined by the energy of the emitted photons, which corresponds to a specific wavelength in the visible spectrum.
2. The unique color each metallic element gives off when burned indicates that the energy levels in the atoms of these elements are distinct. Different energy level transitions result in photons of different energies (and thus colors), meaning each element has a characteristic set of energy levels.
3. In the Bohr model of a hydrogen atom, when an electron moves from the ground state (n = 1) to an excited state (e.g., n = 2, 3, etc.), it absorbs a photon with energy equal to the energy difference between the levels. When it returns to the ground state, it emits a photon with the same energy. For the Balmer series, the electron transitions involve the second energy level (n = 2) as the lower - energy level for emissions. To draw it, represent the nucleus at the center, draw circular orbits for the energy levels, an arrow showing the electron moving outwards for excitation (with an input energy label) and an arrow moving inwards for de - excitation (with an output energy label).

Answer:

1. Electrons absorb energy, move to excited states, then return to lower levels emitting photons of specific energies corresponding to flame colors.
2. It tells us that each metallic element has distinct energy levels as different energy - level transitions produce photons of different energies and colors.
3. Draw the nucleus, circular orbits for energy levels, arrows for electron movement (outward for excitation with energy input and inward for de - excitation with energy output) with the Balmer series involving n = 2 as the lower level for emissions.