Comparing Bohr's Theory and Wave Mechanics

AI Thread Summary
Bohr's theory and wave mechanics both predict the same energy levels for hydrogen, but wave mechanics provides a more comprehensive framework for understanding atomic behavior, including phenomena like electron wave-particle duality. Key differences include Bohr's quantized orbits versus wave mechanics' probabilistic electron distributions. Space quantization is not observed in macroscopic objects like spinning tops due to their larger mass and classical behavior. The energy required to remove an electron from neon is higher than from sodium due to the effective nuclear charge and electron shielding effects. The de Broglie wavelength for an electron moving at the specified speed is calculated to be approximately 0.72 x 10^-30 m.
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Homework Statement



1. If Bohr’s theory and wave-mechanics predicts the same results for energies of hydrogen atom states, then why do we need wave mechanics with its greater complexity?
2. Compare Bohr’s theory and wave mechanics. In what respect do they differ?
3. Why don’t we observe space quantization for spinning top?
4. Why does it take more energy to remove an electron from neon (z = 10), than from sodium (z = 11)?
5. What is the de Broglie wavelength for an electron (me = 9.11  10-11 kg) moving with a speed of 1.00  107 m/s?



Homework Equations


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The Attempt at a Solution


Could just do the last one...
5.
λ = h / mv

= 6.634 * 10-34 / (9.1* 10-11* 1* 107)

= 0.72 * 10 -30 m

Please help with the earlier ones!
 
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