Physics

• Spectrum


  The group of radiations when light passes through a prism and splits into seven colors
• Types of spectrum


  • Continuous spectrum
  • Line spectrum
• Continuous spectrum


  • No clear boundary lines between colors
  • Colors partially overlap
  • Colors not separated by lines
• Line spectrum


  • Clear boundary lines between colors
  • Colors do not overlap
  • Colors are separated
• Types of line spectrum

  • Line absorption spectrum
  • Line emission spectrum
• Line absorption spectrum


  Atom absorbs specific colors or wavelengths from white light
• Line emission spectrum


  Atom emits specific colors or wavelengths after absorbing and re-emitting energy
• Bohr's theory


  Electron jumps between energy levels, emitting or absorbing energy in the form of electromagnetic radiation
• Energy emitted = E2 - E1, where E2 is the higher energy level and E1 is the lower energy level
• Finding wavelength of emitted radiation

  Use formula: 1/λ = R * (1/n1^2 - 1/n2^2), where R is the Rydberg constant and n1, n2 are the energy levels
• Hydrogen atomic spectrum series

  • Lyman series
  • Balmer series
  • Paschen series
  • Brackett series
  • Pfund series
• Lyman series


  • Electron jumps to n=1 energy level
  • Wavelengths in ultraviolet region
• Balmer series


  • Electron jumps to n=2 energy level
  • Wavelengths in visible region
• Paschen series


  • Electron jumps to n=3 energy level
  • Wavelengths in near infrared region
• Brackett series


  • Electron jumps to n=4 energy level
  • Wavelengths in mid infrared region
• Pfund series


  • Electron jumps to n=5 energy level
  • Wavelengths in far infrared region