Here I present: Frederick Soddy, “The Origins of the Concepts of Isotopes”, NOBEL PRIZE LECTURE, 12 November 1922, PART TWO (II).
SUMMARY.
Today we live in an “Atomic Age”; however, in 1922 over one hundred years ago this was not the case. Frederick Soddy won the NOBEL PRIZE for his 1913 law of “isotope displacement” in a periodic table’of elements’. The law concerns types shown on the “graphic schematic” ABOVE & BELOW.
The 80 elements’ with one or more stable isotopes comprise a total of 251 isotopes that have not been known to decay using current equipment.
Stable isotopes:
- 1 element’ (tin) has 10 stable isotopes.
- 5 elements’ have 7 stable isotopes apiece.
- 7 elements’ have 6 stable isotopes apiece.
- 11 elements’ have 5 stable isotopes apiece.
- 9 elements’ have 4 stable isotopes apiece.
- 5 elements’ have 3 stable isotopes apiece.
- 16 elements’ have 2 stable isotopes apiece.
- 26 elements’ have 1 single stable isotope’.
Here I presented: Frederick Soddy, “The Origins of the Concepts of Isotopes”, NOBEL PRIZE LECTURE, 12 November 1922, PART TWO (II).COMMENTS.
Today is not 1922 over one hundred ago, the presentation of a periodic table using a graph with “neutron” & “protons” is part of the “Atomic Age” we live in.
Twenty-five (25) stable elements’ have been shown to be “essential elements” of two types. Essential elements’ types are: “bulk elements” or “trace elements” are dietary terms used by everyone today. Nutrition of essential elements’ is daily conversation.
Today the culture has absorbed the terminology of “isotope” and elements’ as part of the modern world we live in. The difference however between Dmitri Mendeleev and Frederick Soddy represents the advance’s of chemical history. Dmitri Mendeleev was concerned with “electron” bonds of elements’. Frederick Soddy was interested in the “nucleons” within elements’.
