QUANTUM MECHANICAL MODEL
MAIN CONTRIBUTORS
YEAR OF THE EXPERIMENT
- Max Planck: Introduced the concept of quantization of energy.
- Niels Bohr: Developed the initial model of quantized electron orbits.
- Louis de Broglie: Proposed the wave-particle duality of matter.
- Erwin Schrödinger: Developed wave mechanics and the Schrödinger equation.
- Werner Heisenberg: Formulated matrix mechanics and the uncertainty principle.
- The development of the Quantum Mechanical Model took place in 1926.
DIFFERENCES FROM BOHR'S MODEL
MATHEMATICAL TREATMENT
ATOMIC ORBITALS
ELECTRON BEHAVIOR
Bohr’s model treats electrons as particles moving in fixed orbits around the nucleus, with quantized energy levels. The Quantum Mechanical Model, however, describes electrons as wave functions, focusing on probabilities rather than fixed paths.
In Bohr’s model, electrons have specific orbits. In the Quantum Mechanical Model, electrons exist in atomic orbitals—regions in space where there is a high probability of finding an electron.
Bohr’s model uses classical physics and quantization conditions, while the Quantum Mechanical Model uses complex mathematical frameworks (like wave equations) to describe the behavior of particles.
DIFFERENCES FROM BOHR'S MODEL
DESCRIPTION OF ELECTRON BEHAVIOR
CONCEPT OF ATOMIC ORBITALS
ROLE OF PROBABILITY CLOUDS
Probability clouds represent the regions in which an electron is likely to be found, as dictated by its wave function. These clouds visualize the uncertainty in an electron's position and illustrate that an electron's location is not precisely determined, but rather described by a probability distribution.
Atomic orbitals are mathematical functions that describe the probability distribution of an electron in an atom. Each orbital has a specific shape and energy level. These orbitals represent regions in space where an electron is likely to be found, rather than definite paths.
Electrons are described by wave functions that show where you might find them around the nucleus. Superposition : an electron can be in multiple states at once. Entanglement: particles can be connected no matter how far apart they are.It says there are limits of how we can know an electron's position. This way of thinking gives us a better understanding of atoms and molecules than earlier models did.
QUANTUM MECHANICAL MODEL
Rania Zaid
Created on October 16, 2024
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Transcript
QUANTUM MECHANICAL MODEL
MAIN CONTRIBUTORS
YEAR OF THE EXPERIMENT
DIFFERENCES FROM BOHR'S MODEL
MATHEMATICAL TREATMENT
ATOMIC ORBITALS
ELECTRON BEHAVIOR
Bohr’s model treats electrons as particles moving in fixed orbits around the nucleus, with quantized energy levels. The Quantum Mechanical Model, however, describes electrons as wave functions, focusing on probabilities rather than fixed paths.
In Bohr’s model, electrons have specific orbits. In the Quantum Mechanical Model, electrons exist in atomic orbitals—regions in space where there is a high probability of finding an electron.
Bohr’s model uses classical physics and quantization conditions, while the Quantum Mechanical Model uses complex mathematical frameworks (like wave equations) to describe the behavior of particles.
DIFFERENCES FROM BOHR'S MODEL
DESCRIPTION OF ELECTRON BEHAVIOR
CONCEPT OF ATOMIC ORBITALS
ROLE OF PROBABILITY CLOUDS
Probability clouds represent the regions in which an electron is likely to be found, as dictated by its wave function. These clouds visualize the uncertainty in an electron's position and illustrate that an electron's location is not precisely determined, but rather described by a probability distribution.
Atomic orbitals are mathematical functions that describe the probability distribution of an electron in an atom. Each orbital has a specific shape and energy level. These orbitals represent regions in space where an electron is likely to be found, rather than definite paths.
Electrons are described by wave functions that show where you might find them around the nucleus. Superposition : an electron can be in multiple states at once. Entanglement: particles can be connected no matter how far apart they are.It says there are limits of how we can know an electron's position. This way of thinking gives us a better understanding of atoms and molecules than earlier models did.