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Different electronic structures have different absorption and emission spectra
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<strong>Light and Molecules:</strong> Spectroscopy Review
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<p class="mainidea">
Recall that the electrons in an atom are arranged into <b>energy
levels</b> and that the lowest possible energy level is referred
to as the <b>ground state</b>. Electrons can move to the outer
energy levels, called the <b>excited state</b> by absorbing
energy, often in the form of electromagnetic radation. When the
electrons fall back to the ground state, the extra energy is <b>emitted</b>
in the form of a photon whose color corresponds to the difference
in energy between the two energy levels.
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Press play on the model to the right and watch what happens as the
photons interact with the atoms in the box. Notice how most of the
photons pass through the atoms and only certain wavelengths of light are
absorbed by the atoms. Similary when an atom <b>does</b> absorb a
photon, it becomes excited (shown by a dotted line surrounding the atom)
it then emits photons of a specific wavelength.
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Simulation speed of light-matter interactions
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Question: What color of photon must be absorbed by the atom in order to
excite the electron from the ground state to the second energy level?
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Red
Orange
Green
Blue
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In the box below, list all the photons that are absorbed and emitted by
the atoms in the box.
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