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Related Concept Videos

Phase Transitions: Sublimation and Deposition02:33

Phase Transitions: Sublimation and Deposition

Some solids can transition directly into the gaseous state, bypassing the liquid state, via a process known as sublimation. At room temperature and standard pressure, a piece of dry ice (solid CO2) sublimes, appearing to gradually disappear without ever forming any liquid. Snow and ice sublimate at temperatures below the melting point of water, a slow process that may be accelerated by winds and the reduced atmospheric pressures at high altitudes. When solid iodine is warmed, the solid sublimes...
Phase Diagrams02:39

Phase Diagrams

A phase diagram combines plots of pressure versus temperature for the liquid-gas, solid-liquid, and solid-gas phase-transition equilibria of a substance. These diagrams indicate the physical states that exist under specific conditions of pressure and temperature and also provide the pressure dependence of the phase-transition temperatures (melting points, sublimation points, boiling points). Regions or areas labeled solid, liquid, and gas represent single phases, while lines or curves represent...
pV-Diagrams01:18

pV-Diagrams

The pV diagram, which is a graph of pressure versus volume of the gas under study, is helpful in describing certain aspects of the substance. When the substance behaves like an ideal gas, the ideal gas equation describes the relationship between its pressure and volume. On a pV diagram, it is common to plot an isotherm, which is a curve showing p as a function of V with the number of molecules and the temperature fixed. Then, for an ideal gas, the product of the pressure of the gas and its...
Freezing Point Depression and Boiling Point Elevation03:12

Freezing Point Depression and Boiling Point Elevation

Boiling Point Elevation
The boiling point of a liquid is the temperature at which its vapor pressure is equal to ambient atmospheric pressure. Since the vapor pressure of a solution is lowered due to the presence of nonvolatile solutes, it stands to reason that the solution’s boiling point will subsequently be increased. Vapor pressure increases with temperature, and so a solution will require a higher temperature than will pure solvent to achieve any given vapor pressure, including one...
Freezing Point Depression and Boiling Point Elevation01:24

Freezing Point Depression and Boiling Point Elevation

When a non-volatile solute is added to a pure solvent, it results in the lowering of the freezing point of the solvent. This phenomenon is called freezing point depression. The extent to which the freezing point is lowered depends on the molality of the solute -the number of moles of solute per kilogram of solvent and the cryoscopic constant of the solvent.From the plot of chemical potential, μ, against temperature, it is evident that the μ of both solid and liquid solvents decrease with...
Vapor Pressure Lowering03:28

Vapor Pressure Lowering

The equilibrium vapor pressure of a liquid is the pressure exerted by its gaseous phase when vaporization and condensation are occurring at equal rates: Dissolving a nonvolatile substance in volatile liquid results in a lowering of the liquid’s vapor pressure. This phenomenon can be explained by considering the effect of added solute molecules on the liquid's vaporization and condensation processes. To vaporize, solvent molecules must be present at the surface of the solution. The presence of...

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Related Experiment Video

Updated: May 26, 2026

An Externally-Heated Diamond Anvil Cell for Synthesis and Single-Crystal Elasticity Determination of Ice-VII at High Pressure-Temperature Conditions
07:48

An Externally-Heated Diamond Anvil Cell for Synthesis and Single-Crystal Elasticity Determination of Ice-VII at High Pressure-Temperature Conditions

Published on: June 18, 2020

High pressure ices.

Andreas Hermann1, N W Ashcroft, Roald Hoffmann

  • 1Department of Chemistry and Chemical Biology, Cornell University, Ithaca, NY 14853, USA.

Proceedings of the National Academy of Sciences of the United States of America
|December 31, 2011
PubMed
Summary
This summary is machine-generated.

Water (H2O) is more resistant to metallization under extreme pressure than previously believed. New stable ice structures were discovered, with metallization only occurring near 4.8 TPa.

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Area of Science:

  • Condensed Matter Physics
  • Materials Science
  • Computational Chemistry

Background:

  • Understanding the phase diagram of water (H2O) under extreme pressures is crucial for planetary science.
  • Previous studies suggested lower pressure metallization points for ice.

Purpose of the Study:

  • To investigate the stable structures of H2O ice at high pressures (1-5 TPa).
  • To determine the pressure at which H2O ice undergoes metallization.

Main Methods:

  • Computational evolutionary structure searches were employed.
  • Static approximation was used to calculate stable and meta-stable structures.
  • Analysis of geometrical changes and electronic properties was performed.

Main Results:

  • A sequence of new stable and meta-stable H2O ice structures were identified in the 1-5 TPa range.
  • The previously proposed Pbcm structure was superseded by Pmc2(1) and P2(1) phases.
  • Metallization was predicted to occur near 4.8 TPa with the emergence of the C2/m phase.

Conclusions:

  • H2O ice exhibits greater resistance to metallization than previously thought.
  • New crystal structures of ice stable at high pressures were discovered.
  • Potential melting of the H sublattice or the entire crystal at metallization pressures was suggested.