Quantum Theory
Quantum Theory - Related Videos
02:43
Quantum Numbers
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2020
It is said that the energy of an electron in an atom is quantized; that is, it can be equal only to certain specific values and can jump from one energy level to another but not transition smoothly or stay between these levels. The energy levels are labeled with an n value, where n = 1, 2, 3, etc. Generally speaking, the energy of an electron in an atom is greater for greater values of n. This number, n, is referred to as the principal quantum number. The principal quantum number defines the...
02:45
Valence Bond Theory
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2020
Overview of Valence Bond Theory Valence bond theory describes a covalent bond as the overlap of half-filled atomic orbitals (each containing a single electron) that yield a pair of electrons shared between the two bonded atoms. The orbitals on two different atoms overlap when a portion of one orbital and a portion of a second orbital occupy the same region of space. According to valence bond theory, a covalent bond results when two conditions are met: (1) an orbital on one atom overlaps an...
10:00
Gradient Echo Quantum Memory in Warm Atomic Vapor
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Cited by 2 •
2013
The gradient echo memory is a protocol for storing optical quantum states of light in atomic ensembles. Quantum memory is a key element of a quantum repeater, which can extend the range of quantum key distribution. We outline the operation of the scheme when implemented in a 3-level atomic ensemble.
06:41
Prospect Theory
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2023
Source: Laboratory of Jonathan Flombaum—Johns Hopkins University What’s the value of a dollar? Currencies store value to facilitate trade. Implied in any economic transaction is the value of a unit of currency. But what is the subjective value of a dollar? For a long time, economists assumed the answer to this question to be, specifically, that a dollar has a value determined by the market and that the subjective value of a dollar is always that, more or less. Beginning in the early 1970s,...
02:45
The Quantum-Mechanical Model of an Atom
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2020
Shortly after de Broglie published his ideas that the electron in a hydrogen atom could be better thought of as being a circular standing wave instead of a particle moving in quantized circular orbits, Erwin Schrödinger extended de Broglie’s work by deriving what is now known as the Schrödinger equation. When Schrödinger applied his equation to hydrogen-like atoms, he was able to reproduce Bohr’s expression for the energy and, thus, the Rydberg formula governing hydrogen spectra. Schrödinger...
FAQs
Discrete energy states determine which changes in an atom or molecule can occur. When a system moves between allowed states, it can interact with light at specific energies rather than across every possible value. These energy-dependent transitions produce spectra, so spectral patterns provide a way to investigate atomic and molecular behavior through quantum theory.
A wavefunction represents the quantum state of an electron, and its distribution defines an orbital. The resulting orbital picture helps organize where electrons can be found and which electron configurations are possible. In chemistry, that information connects an abstract mathematical solution with covalent bonding, molecular geometry, and the structural features chemists analyze.
Quantum theory relates chemical reactivity to the allowed electron configurations and the arrangements of electrons within atoms and molecules. Because bonding depends on these electronic descriptions, changes in electron distribution can be connected with changes in molecular structure and interactions. This framework helps explain why molecular geometry and covalent bonding are important when interpreting chemical behavior.
In spectroscopy, quantum theory links measured interactions with light to transitions between allowed molecular or atomic energy states. Solving the Schrödinger equation provides wavefunctions and the associated energy description, while the predicted transitions can be compared with spectral observations. This connection allows spectroscopy to examine electronic structure and the behavior of matter at small scales.
Computational chemistry uses quantum theory as a basis for modeling the electronic structure of atoms and molecules. A calculation can represent electrons through wavefunctions, orbitals, and allowed energy states, then relate those results to bonding or molecular geometry. Such modeling supports the study of chemical structures and reactivity when direct observation alone is insufficient.
Quantum theory supports several chemistry-related research areas because it connects electronic structure with measurable behavior and molecular properties. Its principles contribute to spectroscopy, computational modeling, materials design, and drug development. In each area, information about energy states, electron configurations, bonding, or molecular geometry helps researchers analyze or design systems with desired chemical characteristics.