Structure of Atom
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New answer posted
7 months agoContributor-Level 10
The quantum mechanical model of the atom is a significant shift from orbits to orbitals. Though Bohr's atomic model was the beginning of understanding of how electrons move in fixed circular paths, it was Heisenberg's Uncertainty Principle that changed the view. It showed exact positions and velocities can't both be known. So definite orbits don't exist.
In the quantum mechanical model of atom, electrons are treated as waves and described by orbitals. These are regions where they are most likely to be found. These come from Schrödinger's wave function, where |? |² gives the probability of locating an electron. Each orbital is defined
New answer posted
7 months agoContributor-Level 10
Through Heisenberg's Uncertainty Principle, it's proven that you can't pin down where an electron is and how fast it's moving at the same time. The Bohr model did not look into this. The main reason for that thought was that it pictured electrons like little planets that would move in a loop around the nucleus. But that only works if you know both position and speed exactly. Nature doesn't let you do that. Add to it the fact that electrons also behave like waves, and the Bohr model just couldn't keep up. That's why scientists had to move on to the quantum model, which fits way better with how electrons actually act.
New answer posted
7 months agoContributor-Level 10
De Broglie had the idea that everything that moves has a bit of wave behaviour. Technically, that includes any person, a football, and even a bus. The catch is that for big things, the mass is so large that their wavelength is insanely tiny. It's so tiny it's impossible to notice. That's why you don't see a football spreading out like ripples when you kick it. Electrons though? They're super light, so their wavelengths are big enough for us to actually measure. And when scientists did experiments, such as electron diffraction, the electrons really did behave like waves. That was the proof De Broglie needed to show he was ri
New answer posted
7 months agoContributor-Level 10
Δx . Δp = h/4π
Δx . mΔv = h/4π
Δv = 5 * 10? * 0.02/100 = 1000 m/s
∴ Δx = h/ (4πmΔv) = 6.63*10? ³? / (4*3.14*9.1*10? ³¹*1000)
= 5.8 * 10? m
= 58 * 10? m.
New answer posted
7 months agoContributor-Level 10
Rutherford atomic model can not explain hydrogen spectrum it is explained by Bohr's atomic model and from Bohr's atomic model, uncertainity principle can't be explained.
New answer posted
7 months agoContributor-Level 10
Bohr's model played an important role in the development of quantum theory. It introduced the idea of quantised electron orbits. It disproved claims of classical mechanics, which predicted that electrons would spiral into the nucleus. Bohr proposed that electrons can exist only in specific, stable energy levels called stationary states. There would be transitions between these levels that would help Bohr explain the line spectra of hydrogen. That together linked the atomic structure with the concept of energy quantisation. Even though the model could not explain multi-electron atoms, it laid the foundation for modern quantum mechanics.
New answer posted
7 months agoContributor-Level 10
The existence of atomic spectra tells us that energy levels in atoms are quantised. When atoms absorb or emit light, they do so at specific wavelengths. They lead to line spectra instead of a continuous spectrum. Now, every line corresponds to an electron that transitions between fixed energy levels. This is to make the photon's energy equal to the difference between them. If energy levels were not discrete, the spectra would be continuous. So, the line spectra provide direct evidence that electrons in atoms occupy quantised energy states.
New answer posted
7 months agoContributor-Level 10
Bohr's model solved the instability problem by proving about stationary states. In such stats, the electrons move in fixed orbits. They do not emit energy. This contradicted classical electromagnetic theory of Maxwell, which says accelerating charges should emit radiation and collapse into the nucleus. Bohr simply assumed Maxwell's laws don't apply to these special orbits.
New answer posted
7 months agoContributor-Level 10
Bohr's model is too simple for atoms beyond hydrogen. In multi-electron atoms like helium, it fails because it ignores a couple of aspects. First is the electron-to-electron repulsion, and second is the shielding effect, where inner electrons reduce the nuclear pull on outer ones. Due to both, orbitals with the same principal quantum number don't have the same energy. Bohr's model of atom assumes that it should have the same energy.
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