Consider a transition in which the electron of a hydrogen atom is excited from n = 1 to n = . (d) How are the results of parts (b) and (c) related to the plot shown in Exercise 6.88?

Key Concepts

Quantum Energy Levels

In quantum mechanics, electrons in an atom occupy discrete energy levels, denoted by quantum numbers (n). For hydrogen, these levels are quantized, meaning an electron can only exist in specific states. The transition from a lower level (n=1) to a higher level (n=2, 3, etc.) involves the absorption of energy, typically in the form of a photon, which corresponds to the energy difference between these levels.

Photon Energy and Frequency

The energy of a photon is directly related to its frequency through the equation E = hν, where E is energy, h is Planck's constant, and ν is frequency. When an electron transitions between energy levels, it absorbs or emits a photon with energy equal to the difference between the two levels. This relationship is crucial for understanding how the frequency of light corresponds to specific electronic transitions in atoms.

Kinetic Energy and Electron Transitions

The kinetic energy of an electron in an atom can change during electronic transitions. When an electron absorbs energy and moves to a higher energy level, it may also gain kinetic energy, which is reflected in the graph. The plot illustrates how the kinetic energy of the electron increases with frequency, indicating that only photons with sufficient energy (above a threshold frequency, ν₀) can cause transitions that result in increased kinetic energy.