How did atoms absorb light according to the Bohr model?

According to the Bohr atomic model, electrons within an atom are restricted to specific, allowed orbits, also known as stationary states, each possessing a well-defined energy level.123

Atoms absorb light through a process involving these discrete energy states. When an atom is exposed to external energy, such as light, an electron can absorb a photon that has exactly the right amount of energy to facilitate a transition. This energy must correspond precisely to the difference between the electron's current lower-energy orbit and a higher-energy orbit. Upon absorbing this photon, the electron makes an abrupt "quantum leap" to the higher energy level.123

Because each element possesses a unique set of energy levels, atoms selectively absorb only those specific frequencies of light that match the energy gaps between their allowed orbits. This process is fundamental to spectroscopy, as the specific frequencies absorbed act as a unique fingerprint for identifying different elements.1