Understanding Atom Models and Electron Behavior

Rutherford Model

• Proposed by: Ernest Rutherford in 1909.
• Description: Atom similar to a mini solar system.
  • High-density positive nucleus at the center.
  • Electrons orbit the nucleus at high speeds (negative charge).
• Problem:
  • An orbiting electron has centripetal acceleration.
  • Accelerating electron radiates energy and loses it.
  • Using Larmora formula, electron would lose energy in ~10 picoseconds.
  • Electron would crash into the nucleus making atoms unstable.
  • Contradiction: Atoms are stable (real-world observation).

Standing Wave Model

• Better Representation: Electrons as standing waves, not orbiting particles.
• Explanation using metal ring:
  • Ring resonates at specific frequencies forming standing waves.
  • Discrete energy inputs allow standing waves.
  • Only certain wavelengths fit in the circle (integral number of wavelengths).
• Niels Bohr's Proposal:
  • Electrons increase energy in discrete intervals (Quantum Leaps).
  • Energies are quantized (discrete packets).
  • Electrons move to different vibrations, not a smooth transition.

Orbital Visualization

• Experiment analogy:
  • Metal ring shows resonant modes with various nodes.
  • Electrons display similar vibrational modes (known as orbitals).
• Electron Behavior:
  • Electrons measured as particles, not spread out waves.
  • S orbital: Electron's first resonant frequency.
  • Measurement shows random electron locations, probabilistic nature.
  • Wave function: Probability distribution for electron locations.

Differences from Ring Model

• Ring: Provides modes with an odd number of half wavelengths.
• Bohr Model: Allows modes with even number of wavelengths.
  • Attachment to vibration apparatus causes disparity.

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