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Related Concept Videos

Hydrogen Bonds01:04

Hydrogen Bonds

11.6K
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...
11.6K
Hydrogen Bonds00:26

Hydrogen Bonds

128.5K
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.
Hydrogen Bonds Control the World!
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....
128.5K
Electronegativity02:54

Electronegativity

77.8K
Whether a bond is nonpolar or polar covalent is determined by a property of the bonding atoms called electronegativity. 
77.8K
Comparing Intermolecular Forces: Melting Point, Boiling Point, and Miscibility02:34

Comparing Intermolecular Forces: Melting Point, Boiling Point, and Miscibility

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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.
Temporary attractive forces like dispersion are present in all molecules, whether they are polar or nonpolar. They...
48.7K
Bond Energies and Bond Lengths02:49

Bond Energies and Bond Lengths

29.0K
Stable molecules exist because covalent bonds hold the atoms together. The strength of a covalent bond is measured by the energy required to break it, that is, the energy necessary to separate the bonded atoms. Separating any pair of bonded atoms requires energy — the stronger a bond, the greater the energy required to break it.
29.0K
Ionic Bonding and Electron Transfer02:48

Ionic Bonding and Electron Transfer

46.9K
Ions are atoms or molecules bearing an electrical charge. A cation (a positive ion) forms when a neutral atom loses one or more electrons from its valence shell, and an anion (a negative ion) forms when a neutral atom gains one or more electrons in its valence shell. Compounds composed of ions are called ionic compounds (or salts), and their constituent ions are held together by ionic bonds: electrostatic forces of attraction between oppositely charged cations and anions. 
46.9K

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Related Experiment Video

Updated: Nov 14, 2025

Line Shape Analysis of Dynamic NMR Spectra for Characterizing Coordination Sphere Rearrangements at a Chiral Rhenium Polyhydride Complex
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Line Shape Analysis of Dynamic NMR Spectra for Characterizing Coordination Sphere Rearrangements at a Chiral Rhenium Polyhydride Complex

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Entropy differences between hydrides and other elements.

Yoshitsugu Kojima1, Masakuni Yamaguchi

  • 1Natural Science Center for Basic Research and Development, Hiroshima University, 1-3-1, Kagamiyama, Higashi-Hiroshima, Hiroshima 739-8530, Japan.

Chemical Communications (Cambridge, England)
|March 9, 2021
PubMed
Summary

Standard entropy differences (ΔS) between hydrides and other substances correlate with volume differences (ΔV). This relationship is approximated by the equation |ΔS|∝Rln|ΔV|, where R is the gas constant.

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Area of Science:

  • Physical Chemistry
  • Thermodynamics
  • Materials Science

Background:

  • Entropy is a fundamental thermodynamic property.
  • Understanding entropy differences is crucial for predicting chemical and physical behavior.
  • Hydrides exhibit diverse properties influenced by their interactions with other elements.

Purpose of the Study:

  • To investigate the relationship between entropy differences and volume differences for hydrides.
  • To establish a quantitative correlation for these thermodynamic parameters.
  • To explore the behavior of hydrides in relation to metals, liquid nitrogen, and toluene.

Main Methods:

  • Comparative analysis of standard entropy differences (ΔS).
  • Measurement and comparison of volume differences (ΔV).
  • Empirical correlation development based on experimental data.

Main Results:

  • Standard entropy differences (ΔS) increase with volume differences (ΔV) between hydrides and other substances.
  • A proportional relationship was observed: |ΔS|∝Rln|ΔV|.
  • The gas constant (R) is a key factor in this thermodynamic relationship.

Conclusions:

  • A predictable correlation exists between entropy and volume differences for hydrides.
  • The derived equation provides a useful approximation for thermodynamic calculations.
  • This finding aids in understanding hydride interactions and properties.