What does combining Bohr and Planck's equations illustrate regarding photon energy?

Combining Bohr's and Planck's equations illustrates that photon energy is influenced by the electron's location within an atom, which directly relates to the quantum energy levels defined by the Bohr model. In the Bohr model, electrons occupy discrete energy levels, and when an electron transitions between these levels, it emits or absorbs a photon whose energy corresponds to the difference between the two levels.

Planck's equation, (E = h\nu), describes the energy of a photon in terms of its frequency, where (h) is Planck's constant and (\nu) is the frequency of the emitted or absorbed photon. The specific frequencies (and thus the energies) of the photons emitted or absorbed by an atom depend on the energy levels established by the electron configurations within that atom. Therefore, the energy of the emitted or absorbed photon is contingent upon the initial and final energy states of the electron, emphasizing the impact of the electron's location.

The other options do not effectively capture the relationship between photon energy and the electron's quantum state. While it is true that photon energy is related to wavelength (as expressed in (E = \frac{hc}{\lambda})), it is not solely dependent on wavelength because that relationship