This book provides a complete and student-friendly introduction to the Bohr theory of the hydrogen atom and the spectral structure of atomic radiation. Beginning with the limitations of classical physics and Rutherford's atomic model, the book explains why Niels Bohr introduced the idea of quantized electron orbits. It clearly describes Bohr's two postulates, the concept of stationary orbits, and how electron transitions produce radiation of definite frequency.
A major portion of the book is devoted to the mathematical derivation of Bohr's radius, electron velocity, kinetic energy, potential energy, and the total energy of the nth orbit. T
The book also explains how the hydrogen atom produces its characteristic line spectrum. Using Bohr's energy formula and the Rydberg equation, students learn how electron transitions generate radiation with specific wavelengths and frequencies. All five hydrogen spectral series-Lyman, Balmer, Paschen, Brackett, and Pfund-are thoroughly discussed, including the spectral regions in which they appear and the meaning of the series limit.
Special attention is given to the Balmer series, the only series visible to the naked eye, and the well-known lines Hα, Hβ, Hγ, and Hδ. The book also includes numerical examples involving wavelength, frequency, wave number, and the calculation of orbital radii and energies.
To strengthen understanding, the book provides multiple-choice questions, short answers, long answers, and numerical problems, all designed to help students master the subject through practice. Written in simple language with clear explanations and derivations, this book is ideal for high-school, pre-university, and undergraduate students studying atomic physics and quantum theory.
