Electromagnetic Energy and the Bohr Model

Electromagnetic Radiation Properties

• Moves through a vacuum at a constant speed, c, of 2.998 \times 10^8 \text{ m/s}.

• Characterized by frequency (\nu) and wavelength (\lambda), related by c = \lambda\nu .

• Exhibits wave-particle duality.

Wave Nature of Light

• Demonstrates wavelike behavior, such as interference patterns.

Particle Nature of Light

• Demonstrates properties of particles called photons.

• The energy of a photon is given by E = h\nu (or E = hc/\lambda), where h is Planck's constant.

• ## Bohr Model of the Hydrogen Atom

  • Incorporated Planck's and Einstein's quantization ideas.

  • Explains atomic stability and discrete spectra (e.g., hydrogen's line spectrum).

  • Electrons move in specific, discrete energy orbits around the nucleus.

  • Energy Transitions:

  • Absorption: Electron moves from a lower to a higher energy orbit by absorbing a specific energy photon.

  • Emission: Electron moves from a higher to a lower energy orbit by emitting a specific energy photon.

  • Allows calculation of electron energy and orbit radius in one-electron systems.