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Related Concept Videos

States of Water01:23

States of Water

Water exists in any one of the three classical states: solid (ice), liquid (water), and gas (steam or water vapor). The state of water depends on i) the intermolecular forces that draw molecules together and ii) the kinetic energy that leads to movements that pull them apart.
Water freezes when the intermolecular forces are greater than the kinetic energy. Unlike most other substances, water is less dense in its solid state than in its liquid state. This is because each water molecule can form...
Phase Transitions02:31

Phase Transitions

Whether solid, liquid, or gas, a substance's state depends on the order and arrangement of its particles (atoms, molecules, or ions). Particles in the solid pack closely together, generally in a pattern. The particles vibrate about their fixed positions but do not move or squeeze past their neighbors. In liquids, although the particles are closely spaced, they are randomly arranged. The position of the particles are not fixed—that is, they are free to move past their neighbors to occupy...
Phase Transitions: Melting and Freezing02:39

Phase Transitions: Melting and Freezing

Heating a crystalline solid increases the average energy of its atoms, molecules, or ions, and the solid gets hotter. At some point, the added energy becomes large enough to partially overcome the forces holding the molecules or ions of the solid in their fixed positions, and the solid begins the process of transitioning to the liquid state or melting. At this point, the temperature of the solid stops rising, despite the continual input of heat, and it remains constant until all of the solid is...
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...
Heating and Cooling Curves02:44

Heating and Cooling Curves

When a substance—isolated from its environment—is subjected to heat changes, corresponding changes in temperature and phase of the substance is observed; this is graphically represented by heating and cooling curves.
For instance, the addition of heat raises the temperature of a solid; the amount of heat absorbed depends on the heat capacity of the solid (q = mcsolidΔT). According to thermochemistry, the relation between the amount of heat absorbed or released by a substance, q, and its...
Phase Transitions01:21

Phase Transitions

A phase transition is the process in which a substance changes from one state of matter to another, like from a solid to a liquid, liquid to gas, or vice versa, at a specific temperature and under given pressure conditions. This change is spontaneous and is affected by alterations in temperature and pressure. These parameters impact the strength of the forces between molecules (intermolecular forces) in the substance.During a phase transition, both the initial and final phases of the substance...

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Updated: Jul 24, 2026

The Use of High-resolution Infrared Thermography (HRIT) for the Study of Ice Nucleation and Ice Propagation in Plants
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The percolation phase transition in sea Ice

Golden1, Ackley, Lytle

  • 1K. M. Golden, Department of Mathematics, University of Utah, Salt Lake City, UT 84112, USA. S. F. Ackley, U.S. Army Cold Regions Research and Engineering Laboratory, Hanover, NH 03755, USA. V. I. Lytle, Antarctic Cooperative Research Centre a.

Science (New York, N.Y.)
|December 18, 1998
PubMed
Summary

Sea ice becomes permeable to fluid flow at a critical temperature, allowing heat and nutrient transport. This transition, explained by percolation theory, is vital for understanding sea ice geophysics and biology.

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Area of Science:

  • Geophysics
  • Oceanography
  • Materials Science

Background:

  • Sea ice exhibits a significant shift in fluid transport properties.
  • This transition occurs at a critical brine volume fraction (pc ≈ 5%) or temperature (Tc ≈ -5°C).
  • Above Tc, brine movement facilitates heat and nutrient transfer; below Tc, sea ice becomes impermeable.

Purpose of the Study:

  • To explain the critical behavior of transport properties in sea ice.
  • To investigate the role of brine channels in sea ice.
  • To apply percolation theory to understand sea ice permeability.

Main Methods:

  • Utilizing percolation theory to model sea ice transport.
  • Comparing sea ice microstructure to compressed powders.
  • Theoretically predicting the critical brine volume fraction (pc).

Main Results:

  • A critical brine volume fraction (pc) of approximately 5% was identified.
  • A critical temperature (Tc) of approximately -5°C for a salinity of 5 parts per thousand was determined.
  • Sea ice microstructure shows similarities to compressed powders, supporting theoretical predictions.

Conclusions:

  • The transition in sea ice fluid transport is governed by percolation theory.
  • Understanding this critical transition is crucial for geophysics, biology, and remote sensing of sea ice.
  • Theoretical predictions of pc align with observed sea ice properties.