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Related Concept Videos

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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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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Aldehydes and Ketones with Water: Hydrate Formation01:20

Aldehydes and Ketones with Water: Hydrate Formation

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An oxygen-based nucleophile, like water, can undergo addition reactions with aldehydes and ketones. The reaction leads to the formation of hydrates, also referred to as 1,1-diols or geminal diols.
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Lewis Structures of Molecular Compounds and Polyatomic Ions02:54

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To draw Lewis structures for complicated molecules and molecular ions, it is helpful to follow a step-by-step procedure as outlined:
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Hybridization of Atomic Orbitals I03:24

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The mathematical expression known as the wave function, ψ, contains information about each orbital and the wavelike properties of electrons in an isolated atom. When atoms are bound together in a molecule, the wave functions combine to produce new mathematical descriptions that have different shapes. This process of combining the wave functions for atomic orbitals is called hybridization and is mathematically accomplished by the linear combination of atomic orbitals. The new orbitals that...
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Novel hydrogen hydrate structures under pressure.

Guang-Rui Qian1, Andriy O Lyakhov1, Qiang Zhu1

  • 1Department of Geosciences, Stony Brook University, Stony Brook, New York 11794-2100, USA.

Scientific Reports
|July 9, 2014
PubMed
Summary
This summary is machine-generated.

Researchers explored hydrogen hydrates under high pressure, discovering new phases. The hydrogen-richest hydrate (C₃) shows potential for hydrogen storage with 18 wt.% hydrogen.

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Area of Science:

  • Materials Science
  • Planetary Science
  • Chemistry

Background:

  • Gas hydrates are crucial systems, with hydrogen hydrates relevant to icy celestial bodies and hydrogen storage.
  • The H₂O-H₂ system's behavior under pressure is key to understanding these phenomena.

Purpose of the Study:

  • To investigate the H₂O-H₂ system's structural transformations under high pressure (0-100 GPa).
  • To identify novel hydrogen hydrate phases and their properties.
  • To explain previously observed experimental data in hydrogen-rich hydrates.

Main Methods:

  • Utilized ab initio variable-composition evolutionary simulations.
  • Analyzed the H₂O-H₂ system across a pressure range of 0-100 GPa.
  • Incorporated van der Waals interactions and zero-point vibrational energy in calculations.

Main Results:

  • Identified known clathrate (sII, C₀) and filled ice (C₁, C₂) structures.
  • Discovered two novel hydrate phases: Ih-C₀ (2:1 H₂O:H₂ ratio) and C₃ (1:2 H₂O:H₂ ratio).
  • Predicted C₃ phase stability above 38 GPa, explaining experimental X-ray diffraction and Raman data.
  • C₃ is the hydrogen-richest hydrate, with 18 wt.% easily extractable hydrogen.

Conclusions:

  • The study reveals new high-pressure phases of hydrogen hydrates.
  • The C₃ phase represents a significant advancement in hydrogen storage potential due to its high hydrogen content.
  • These findings advance our understanding of planetary ices and hydrogen storage materials.