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How did the atomic model change from Dalton to Thompson?
Dalton’s Model (1803):
Description: The atom is a solid, indivisible sphere.
Problem: This model couldn’t explain the existence of subatomic particles or chemical behavior in detail.
Thomson’s Model (1897):
Description: Known as the "plum pudding model," where the atom is a positively charged sphere with negatively charged electrons scattered within.
Change: Discovery of the electron through cathode ray experiments.
Problem: Didn’t explain how the positive charge was distributed or how electrons were held in the atom.
How did the atomic model change from Thompson to Rutherford?
Rutherford’s Model (1911):
Description: The atom consists of a small, dense, positively charged nucleus, with electrons orbiting around it.
Change: Rutherford’s gold foil experiment showed that most of the atom is empty space and that the positive charge is concentrated in the nucleus.
Problem: Couldn’t explain why electrons didn’t spiral into the nucleus due to attraction by the positive charge.
How did the atomic model change from Rutherford to Bohr?
Bohr’s Model (1913):
Description: Electrons orbit the nucleus in fixed, quantized orbits.
Change: Bohr used quantum theory to explain that electrons have specific energy levels and can only exist in these levels.
Problem: Worked for hydrogen, but failed to explain multi-electron atoms and the behavior of electrons in complex atoms.
How did the atomic model change from Bohr to Schrödinger?
Schrödinger’s Model (1926):
Description: The electron is treated as a wave, not a particle, and its position is described in terms of probability distributions (orbitals).
Change: The development of quantum mechanics and the Schrödinger equation, which accounts for the wave nature of electrons.
Problem: Solved many issues from previous models, but still cannot provide an exact location of an electron, only its probability.