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The essential points of Bohr's theory of the structure of the hydrogen atom include: 1. Quantization of energy levels: Electrons in a hydrogen atom can only occupy specific energy levels, corresponding to particular integer orbits around the nucleus. 2. Atomic structure: The hydrogen atom has one electron revolving around a positively charged nucleus with one proton. 3. Emission and absorption of energy: When an electron transitions between energy levels, it emits or absorbs a photon with energy equal to the energy gap between the levels. 4. Balmer's formula and the Rydberg constant: The wavelength of emitted photons during electron transitions can be calculated using Balmer's formula \(\lambda = \frac{n^2}{n^2 - 4}R_H\), where \(n\) is an integer greater than 2 and \(R_H\) is the Rydberg constant. 5. Successes and limitations: Bohr's theory successfully explained the hydrogen atom's spectral lines and atomic structure but couldn't account for more complex atomic structures or phenomena like fine structure and hyperfine structure.