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Intermolecular Forces in Solutions02:28

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The formation of a solution is an example of a spontaneous process, a process that occurs under specified conditions without energy from some external source.
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Intermolecular forces are attractive forces that exist between molecules. They dictate several bulk properties, such as melting points, boiling points, and solubilities (miscibilities) of substances. Molar mass, molecular shape, and polarity affect the strength of different intermolecular forces, which influence the magnitude of physical properties across a family of molecules.
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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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Particles in a solid are tightly packed together (fixed shape) and often arranged in a regular pattern; in a liquid, they are close together with no regular arrangement (no fixed shape); in a gas, they are far apart with no regular arrangement (no fixed shape). Particles in a solid vibrate about fixed positions (cannot flow) and do not generally move in relation to one another; in a liquid, they move past each other (can flow) but remain in essentially constant contact; in a gas, they move...
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The physical form of a substance changes on changing its temperature. For example, raising the temperature of a liquid causes the liquid to vaporize (convert into vapor). The process is called vaporization—a surface phenomenon. Vaporization occurs when the thermal motion of the molecules overcome the intermolecular forces, and the molecules (at the surface) escape into the gaseous state. When a liquid vaporizes in a closed container, gas molecules cannot escape. As these gas phase...
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Spatial Separation of Molecular Conformers and Clusters
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Exploring molecular superfluidity in hydrogen clusters.

Hatsuki Otani1, Susumu Kuma2, Shinichi Miura3

  • 1Department of Chemistry, The University of British Columbia, Vancouver, British Columbia V6T 1Z1, Canada.

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Summary

Researchers provide strong evidence for molecular hydrogen (H2) superfluidity at 0.4 K. Using helium nanodroplet spectroscopy, they observed quantum behaviors characteristic of superfluidity in H2 clusters.

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Area of Science:

  • Quantum mechanics
  • Low-temperature physics
  • Spectroscopy

Background:

  • Molecular hydrogen (H2) is theoretically predicted to exhibit superfluidity, a state of zero viscosity, at very low temperatures.
  • Experimental verification of H2 superfluidity remains challenging and debated.

Purpose of the Study:

  • To investigate the superfluid properties of molecular hydrogen (H2) at 0.4 K.
  • To provide experimental evidence for the existence of a superfluid phase in H2.

Main Methods:

  • High-resolution helium nanodroplet spectroscopy was employed.
  • Infrared transitions of methane (CH4) embedded in parahydrogen (H2) clusters were analyzed at 0.4 K.

Main Results:

  • Fully quantized rotational states of methane were observed with minimal interference from H2 molecules.
  • The cluster-size dependence of the rotational constant matched path-integral Monte Carlo simulations.
  • Over 60% of H2 molecules in the clusters participated in quantum bosonic exchanges, a hallmark of superfluidity.

Conclusions:

  • The study presents compelling experimental evidence supporting the existence of a superfluid phase in molecular hydrogen at 0.4 K.
  • This finding advances the understanding of quantum phenomena in molecular systems.