Bohr Model of the Hydrogen Atom

Niels Bohr addressed problems with the atomic structure, such as why atoms are stable despite opposite charges and what causes emission spectra. He aimed to explain why different elements emit light of varying colors.

Bohr's model for the hydrogen atom proposed that the potential energy of an electron is quantized. This means electrons can only occupy specific energy levels at fixed distances from the nucleus, not just any energy. Each atom type has unique energy levels due to its number of protons.

An electron transitions between energy levels by absorbing or emitting a photon of a very specific energy. The photon's energy corresponds to the difference between the two energy levels involved in the transition. Emitting a photon means moving to a lower energy level, while absorbing one means moving to a higher level.

The energy levels in a hydrogen atom depend on the Rydberg constant. We can calculate the change in energy during an electron transition using a specific equation, which then allows us to predict the wavelength of the photon associated with that transition.

Transitions are grouped by the energy level they land on. For example, transitions ending at n=1 are the Lyman series, and those ending at n=2 are the Balmer series. Energy gaps decrease as 'n' increases, and an electron ejected from the atom is considered to have gone beyond n=infinity.

The Balmer series includes transitions that generate visible light photons, which are observable in the hydrogen emission spectrum. These lines correspond to electron transitions ending at the n=2 level. Each element has a unique emission spectrum, acting as a 'fingerprint' due to its distinct nuclear structure and energy level spacing. This principle allows us to determine the composition of celestial objects by analyzing their light.