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\nLimitations of Bohr's Theory\n

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\nNiels Bohr's Atomic Model Limitations\n\n• Primarily applied to hydrogen, not accounting for complexities of multi-electron atoms.\n• Oversimplified concept of fixed, circular orbits for electrons.\n• Failed to account for fine structure of...\nNiels Bohr's Atomic Model Limitations\r
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• Primarily applied to hydrogen, not accounting for complexities of multi-electron atoms.\r
• Oversimplified concept of fixed, circular orbits for electrons.\r
• Failed to account for fine structure of spectral lines due to relativistic effects and spin-orbit coupling.\r
• Failed to explain the Zeeman effect, where spectral lines split in the presence of a magnetic field.\r
• Did not incorporate the Heisenberg Uncertainty Principle, which states it is impossible to know both the exact position and momentum of an electron.\r
• Introduced ad hoc quantization of angular momentum, which later became more comprehensive.\r
• Did not address how electrons interact with external magnetic and electric fields in a detailed manner.\r
• Despite limitations, Bohr's model remains a crucial historical step in the evolution of atomic theory.\n
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3:02
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Grade
9th - Higher Ed
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Subjects
Science
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\nAudio Visual Representation of Chemistry\n\n
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Date
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2024
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English
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For Teacher Use
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Concepts

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spectra, atoms, lines, quantum mechanics
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bohr's model, electron orbits, atomic spectra, multi-electron atoms, fine structure, magnetic effects, theoretical limitations, classical physics conflicts, zeeman effect, magnetic field, neil bo, spectral line, fine spectra, hydrogen atom, atom, concept, spectrum, orbit, electron, wave, bohr, explain, explained, boole, theory, splitting, particle
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\n\" data-title=\"Get Full Access\" data-container=\"body\" rel=\"popover\" tabindex=\"0\" aria-label=\"Play video: Limitations of Bohr's Theory\" href=\"/subscription/new\">\"Limitations\n\n
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