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Related Concept Videos

Noble Gases02:54

Noble Gases


The elements in group 18 are noble gases (helium, neon, argon, krypton, xenon, and radon). They earned the name “noble” because they were assumed to be nonreactive since they have filled valence shells. In 1962, Dr. Neil Bartlett at the University of British Columbia proved this assumption to be false.
Gas Laws: Boyle's, Gay-Lussac, Charles', Avogadro's, and Ideal Gas Law03:19

Gas Laws: Boyle's, Gay-Lussac, Charles', Avogadro's, and Ideal Gas Law

Through experiments, scientists established the mathematical relationships between pairs of variables, such as pressure and temperature, pressure and volume, volume and temperature, and volume and moles, that hold for an ideal gas.
Emission Spectra02:39

Emission Spectra

When solids, liquids, or condensed gases are heated sufficiently, they radiate some of the excess energy as light. Photons produced in this manner have a range of energies, and thereby produce a continuous spectrum in which an unbroken series of wavelengths is present.
Gas Solubility01:31

Gas Solubility

Gas solubility in liquids forms liquid-gas solutions, such as soft drinks, where carbon dioxide is dissolved in water, and the ocean, where the solubility of oxygen and carbon dioxide supports marine life. The ability of oceans to dissolve gases impacts weather conditions in the troposphere.However, gas-liquid interactions vary. For instance, hydrogen chloride gas is highly soluble in water, while oxygen's solubility is much lower. Because these solutions are non-ideal, Raoult’s law, which...
Ideal Gas Equation01:17

Ideal Gas Equation

The ideal gas equation is an equation of state that relates the state variables pressure, volume, temperature, and the number of moles of a hypothetical gas. This equation is a combination of four empirical laws, namely Boyle’s Law, Charles’s Law, Avogadro’s Law, and Gay-Lussac’s Law. When the proportionalities of the above four empirical laws are combined, it results in a single proportionality constant known as the universal gas constant.
Real Gases: Effects of Intermolecular Forces and Molecular Volume Deriving Van der Waals Equation04:01

Real Gases: Effects of Intermolecular Forces and Molecular Volume Deriving Van der Waals Equation

Thus far, the ideal gas law, PV = nRT, has been applied to a variety of different types of problems, ranging from reaction stoichiometry and empirical and molecular formula problems to determining the density and molar mass of a gas. However, the behavior of a gas is often non-ideal, meaning that the observed relationships between its pressure, volume, and temperature are not accurately described by the gas laws.

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Related Experiment Video

Updated: May 22, 2026

High-Sensitivity Nuclear Magnetic Resonance at Giga-Pascal Pressures: A New Tool for Probing Electronic and Chemical Properties of Condensed Matter under Extreme Conditions
08:42

High-Sensitivity Nuclear Magnetic Resonance at Giga-Pascal Pressures: A New Tool for Probing Electronic and Chemical Properties of Condensed Matter under Extreme Conditions

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Sir William Ramsay and the noble gases.

Alwyn G Davies1

  • 1University College. a.g.davies@ucl.ac.uk

Science Progress
|May 12, 2012
PubMed
Summary

Sir William Ramsay discovered five noble gases, revolutionizing atomic structure understanding and earning him the 1904 Nobel Prize in Chemistry. His work added a new group to the Periodic Table, fundamentally advancing chemical knowledge.

Area of Science:

  • Chemistry and Physics
  • Atomic Structure and Periodicity

Background:

  • Sir William Ramsay's pioneering research in the late 19th century.
  • Discovery of five new elements: helium, neon, argon, krypton, and xenon.

Discussion:

  • These discoveries introduced the noble gases, a new group in the Periodic Table.
  • The noble gases were crucial for understanding atomic electronic structure.
  • Their role in chemical bonding and molecular formation was elucidated.

Key Insights:

  • Ramsay's work provided the keystone to understanding atomic electronic structure.
  • Established the significance of noble gases in chemistry.
  • Led to the 1904 Nobel Prize in Chemistry for Ramsay.

Outlook:

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  • Foundation for further exploration of atomic and molecular behavior.
  • Continued impact on the development of the Periodic Table.
  • Inspiration for future scientific discovery and innovation.