Yuichiro Yamakawa coauthored research on superionic conductor.^[ref]

A solid with unusually rapid ionic motion while its host framework remains ordered.

Kenji Homma coauthored research on superionic conductor.^[ref]

A solid with unusually rapid ionic motion while its host framework remains ordered.

Noriaki Kamaya coauthored research on superionic conductor.^[ref]

A solid with unusually rapid ionic motion while its host framework remains ordered.

John E. Straub developed an educational demonstration linking dissolved ions with electrical conductance. Comparing water and a sodium chloride solution illustrates the role of mobile charge carriers; the account also records a weak filament glow for sucrose, so the demonstration is interpreted through its observed signal rather than an ideal zero-current claim.^[ref]

E. W. Kaiser investigated electric dipole moments and hyperfine parameters of hydrogen chloride and its deuterated isotopologue. Comparing the two species connects molecular spectroscopy with the effects of replacing an isotope while retaining the same chemical elements.^[ref]

Johannes Jacobus van Vaals coauthored research on molecular beam.^[ref]

A molecular beam also includes a stream of chemical atoms, then called an atomic beam. An oven supplies particles; aligned slits restrict their directions, and a vacuum limits subsequent collisions. Narrowing the directions does not by itself make every particle's speed equal. This gives a useful separation of tasks: prepare a path, select or measure speed, apply an interaction, and read the resulting particle counts or deflection.

Klaus P. Huber coauthored research on diatomic molecule.^[ref]

A diatomic molecule contains two chemical atoms; hydrogen chloride and carbon monoxide are examples. Their fixed-separation moment of inertia is $I=\mu r^2$ in the linear rigid rotor model.

Robert S. Mulliken proposed an electronegativity-related scale combining ionization energy and electron affinity. Mulliken electronegativity represents a balance between the energetic cost of electron removal and the energetic benefit of electron attachment.

The construction differs from a bond-energy scale. Specifying electronic states and units is essential when comparing the two approaches.^[ref]

Stepan S. Batsanov examined how energy-based electronegativity conventions relate to chemical bonds. The analysis compares energy-unit coefficients and dependence on other chemical bond properties, making both the definition and its unit convention part of a quantitative comparison.^[ref]

Linus Pauling introduced a relative electronegativity comparison based on chemical-bond energies. Excess stability of a heteronuclear bond relative to a reference from homonuclear bonds supplies information about unequal electron sharing.

The Pauling electronegativity scale therefore comes from a model linking bond-energy differences with atomic comparisons. It is not a direct measurement of the partial electric charge on a bonded atom.^[ref]

William R. Robinson coauthored an introductory chemistry text whose thermochemistry chapter develops Hess's law. Adding compatible reaction equations cancels intermediates and adds their enthalpy changes, connecting symbolic chemical bookkeeping with measurable heat.^[ref]

Richard Langley coauthored an introductory account of chemical thermodynamics. Its enthalpy examples show how measurements of accessible reactions can be combined to obtain an otherwise inaccessible reaction's energy change using Hess's law.^[ref]

Paul Flowers coauthored an introductory chemistry text that develops quantitative thermochemistry. Its treatment of Hess's law keeps the reaction equation attached to the stated enthalpy change, so changing the amount reacted changes the corresponding energy.^[ref]

Michael Faraday connected chemistry with quantitative electricity through electrolysis. His experimental treatment related the amount of material transformed at an electrode to the electric charge passed through the apparatus, the basis of Faraday's laws of electrolysis.

His candle lectures made a different connection between apparatus and explanation: the wick supplies melted fuel through capillary action, while the flame's products reveal the chemical transformations involved in combustion.^[ref]

A chemist whose route into experimental research began with a bookbinding apprenticeship (1805–1812). He became a laboratory assistant at the Royal Institution in 1813, its laboratory director in 1825, and Fullerian Professor of chemistry from 1833 to 1867.^[ref]

Klaus Theopold coauthored an introductory treatment connecting chemical equations with energy balances. The enthalpy chapter explains why reversing a reaction reverses its heat-change sign and why compatible equations can be combined through Hess's law.^[ref]