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Related Concept Videos

Structures of Solids02:22

Structures of Solids

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Solids in which the atoms, ions, or molecules are arranged in a definite repeating pattern are known as crystalline solids. Metals and ionic compounds typically form ordered, crystalline solids. A crystalline solid has a precise melting temperature because each atom or molecule of the same type is held in place with the same forces or energy. Amorphous solids or non-crystalline solids (or, sometimes, glasses) which lack an ordered internal structure and are randomly arranged. Substances that...
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Metallic Solids02:37

Metallic Solids

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Metallic solids such as crystals of copper, aluminum, and iron are formed by metal atoms. The structure of metallic crystals is often described as a uniform distribution of atomic nuclei within a “sea” of delocalized electrons. The atoms within such a metallic solid are held together by a unique force known as metallic bonding that gives rise to many useful and varied bulk properties.
All metallic solids exhibit high thermal and electrical conductivity, metallic luster, and malleability....
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Atomic Orbitals02:44

Atomic Orbitals

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An atomic orbital represents the three-dimensional regions in an atom where an electron has the highest probability to reside. The radial distribution function indicates the total probability of finding an electron within the thin shell at a distance r from the nucleus. The atomic orbitals have distinct shapes which are determined by l, the angular momentum quantum number. The orbitals are often drawn with a boundary surface, enclosing densest regions of the cloud.
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Network Covalent Solids02:18

Network Covalent Solids

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Network covalent solids contain a three-dimensional network of covalently bonded atoms as found in the crystal structures of nonmetals like diamond, graphite, silicon, and some covalent compounds, such as silicon dioxide (sand) and silicon carbide (carborundum, the abrasive on sandpaper). Many minerals have networks of covalent bonds.
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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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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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Updated: Mar 11, 2026

Quantification of Hydrogen Concentrations in Surface and Interface Layers and Bulk Materials through Depth Profiling with Nuclear Reaction Analysis
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Topological Surface States in Dense Solid Hydrogen.

Ivan I Naumov1, Russell J Hemley2,3

  • 1Geophysical Laboratory, Carnegie Institution of Washington, Washington, D.C. 20015, USA.

Physical Review Letters
|November 26, 2016
PubMed
Summary
This summary is machine-generated.

Dense hydrogen may become a metal with unique topological surface states, even while its bulk remains insulating. This discovery offers new avenues for exploring high-temperature superconductivity in compressed materials.

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Area of Science:

  • Condensed Matter Physics
  • Materials Science
  • Quantum Chemistry

Background:

  • Metallization of dense hydrogen is a key problem in physics, potentially leading to high-temperature superconductivity.
  • Theoretical studies suggest hydrogen transitions through a semimetallic phase before full metallization.
  • Understanding these intermediate phases is crucial for predicting hydrogen's properties under extreme pressure.

Purpose of the Study:

  • To investigate the electronic properties of semimetallic phases in dense hydrogen.
  • To determine if these phases exhibit conventional or unconventional semimetallic behavior.
  • To identify potential mechanisms for superconductivity in compressed hydrogen.

Main Methods:

  • First-principles calculations were used to model dense hydrogen phases.
  • Electronic band structures were analyzed to identify metallic and semimetallic characteristics.
  • Topological properties of the electronic states were examined.

Main Results:

  • Stable semimetallic phases of dense hydrogen (e.g., Cmca-12, Cmca-4) were identified at multimegabar pressures.
  • These phases exhibit topological metallic surface states within the bulk band gap.
  • Pbcn hydrogen also shows metallic surface states, but they are non-topological in nature.

Conclusions:

  • Dense hydrogen can possess topological metallic surface states, distinct from conventional semimetals.
  • These surface states may enable superconductivity even when the bulk remains insulating.
  • The findings provide predictions for experimental verification of surface superconductivity in dense hydrogen.