An atom emits yellow light when an electron makes the...

An atom emits yellow light when an electron makes the transition from the $n=5$ to the $n=1$ level. In separate experiments, suppose you bombarded the $n=1$ level of this atom with red light, yellow light (obtained from the previous emission), and blue light. In which experiment or experiments would the electron be promoted to the $n=5$ level?

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Key Concepts

Electronic Transitions

Electronic transitions refer to the movement of electrons between the quantized energy levels in an atom. These transitions involve precise amounts of energy being absorbed or emitted, reflecting the quantized nature of atomic energy states.

Resonance Absorption

Resonance absorption occurs when an electron absorbs a photon whose energy exactly equals the gap between two energy levels, thereby promoting the electron to a higher state. This concept is crucial for understanding why only light of a certain color (energy) can produce a specific electronic transition.

Quantized Energy Levels

This concept explains that electrons in an atom exist only in specific, discrete energy states. Transitions between these states occur by absorbing or emitting a precise amount of energy that corresponds to the difference between the energy levels.

Photon Energy

Photon energy is determined by its wavelength or frequency and must exactly match the energy gap between electron levels to induce a transition. This relationship means that only photons with specific energies can trigger particular electronic transitions.

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