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Related Concept Videos

Quantum Numbers02:43

Quantum Numbers

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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.
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Neutral hydrocarbons like cyclopentadiene with an odd number of carbon atoms and one intervening CH2 group in the ring are not aromatic. Cyclopentadiene with 4 π electrons does not satisfy the 4n + 2 π electron rule. Additionally, the intervening CH2 group is sp3 hybridized and lacks a vacant p orbital, thereby interrupting the overlap of p orbitals in a continuous manner and preventing the delocalization of π electrons throughout the ring.
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The Quantum-Mechanical Model of an Atom02:45

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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.
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Hydrogen Bonds00:26

Hydrogen Bonds

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Hydrogen bonds are weak attractions between atoms that have formed other chemical bonds. One of these atoms is electronegative, like oxygen, and has a partial negative charge. The other is a hydrogen atom that has bonded with another electronegative atom and has a partial positive charge.
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Because hydrogen has very weak electronegativity when it binds with a strongly electronegative atom, such as oxygen or nitrogen, electrons in the bond are unequally shared....
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Hydrogen Bonds01:04

Hydrogen Bonds

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A hydrogen bond is formed when a weakly positive hydrogen atom already bonded to one electronegative atom (for example, the oxygen in the water molecule) is attracted to another electronegative atom from another polar molecule, such as water (H2O), hydrogen fluoride (HF), or ammonia (NH3). The huge electronegativity difference between the H atom (2.1) and the atom to which it is bonded (4.0 for an F atom, 3.5 for an O atom, or 3.0 for an N atom), combined with the very small size of an H atom...
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The quantum structure of anionic hydrogen clusters.

F Calvo1, E Yurtsever2

  • 1University Grenoble Alpes, LIPHY, F-38000 Grenoble, France and CNRS, LIPHY, F-38000 Grenoble, France.

The Journal of Chemical Physics
|March 17, 2018
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Summary
This summary is machine-generated.

Researchers developed a new model for hydrogen clusters (H2)n H- and found icosahedral structures and magic numbers at specific sizes. Quantum effects influence cluster shape, especially for larger hydrogen clusters.

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Area of Science:

  • Physical Chemistry
  • Computational Chemistry
  • Quantum Mechanics

Background:

  • Understanding the behavior of hydrogen clusters is crucial for various chemical and physical processes.
  • Previous studies have explored hydrogen-metal interactions, but modeling neutral hydrogen clusters with anions presents unique challenges.

Purpose of the Study:

  • To develop and validate a flexible and polarizable interatomic potential for modeling hydrogen clusters interacting with a hydrogen anion.
  • To investigate the structural, energetic, and vibrational properties of hydrogen clusters (H2)n H- for n = 1-54.

Main Methods:

  • Development of a new interatomic potential parametrized against coupled cluster quantum chemical calculations.
  • Path-integral molecular dynamics simulations at 1 K.
  • Analysis of geometric structures, energetic stability, and vibrational delocalization.

Main Results:

  • Identified equilibrium structures generally based on icosahedral shells with hydrogen molecules oriented towards the anion.
  • Observed geometric magic numbers at cluster sizes n = 12, 32, and 44, consistent with mass spectrometry data.
  • Correlated energetic stability with vibrational delocalization and noted finite size effects and increased molecular rotation in larger clusters.

Conclusions:

  • The developed potential accurately models hydrogen clusters interacting with a hydrogen anion.
  • Quantum nuclear effects play a significant role in the formation of the icosahedral structure, particularly for the 44-molecule cluster.
  • The study provides insights into the interplay of structure, stability, and quantum effects in hydrogen cluster anions.