Pauling's electronegativity scale was a number of steps removed from any rigorous grounding in quantum mechanics, was therefore
one of his least theoretically well-founded ideas — and became one of his most influential. It was easily grasped by chemists,
who appreciated its practical value in addressing real-world problems. By comparing the electronegativity of two elements
from his tables, researchers could for the first time roughly predict the properties of a bond formed between them without
having to know the first thing about the wave equation. The scale quickly earned wide adoption.
Pauling's mixing and matching of empirical observations with ideas from quantum physics was imaginative and dangerous. At
each step he added a few more assumptions and moved a little further away from a hard grounding in accepted theory. Years
later this would trip him up when critics would question the justification for his schemes, but for now it appeared that everything
he did worked, and worked brilliantly.
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"Ionic Character of Bonds." April 11, 1937.
Notes and Calculations re: Electronegativity and the Electronegativity Scale. 1930s.
"Pauling's paper on bond energy and electronegativity proved to be highly influential. The qualitative concept of electronegativity
as the ability of an atom in a molecule to attract electrons to itself was an old one. Early in the twentieth century, it
was associated in a crude way with the metallic or non-metallic character of an element, or with its place in the activity
series of the metals. The importance of Pauling's paper derives from the fact that he was the first person to put this property
on a numerical basis."
Robert J. Paradowski