Isotope geochemistry has grown over the last 60 years to become one of the most important fields in the earth sciences. It has two broad subdivisions, namely, radiogenic isotope geochemistry and stable isotope geochemistry. These subdivisions reflect the two primary reasons why the relative abundances of isotopes of elements vary in nature, which are radioactive decay and chemical fractionation; in this context, “fractionation” is any process in which the isotopes of the same element behave differently.

Radiogenic and stable isotopes are used widely in the Earth sciences to determine the ages of rocks, meteorites, and archeological objects, and as tracers to understand geological and environmental processes. Isotope methods determine the age of the Earth, help reconstruct the climate of the past, and explain the formation of the chemical elements in the Universe.

“Water, water, every where, — nor any drop to drink” (Samuel Taylor Coleridge, “The Rime of the Ancient Mariner”) aptly sums up the overall picture of the hydrosphere — that part of planet Earth made up of water. The oceans, covering 71% of the surface of the globe, make up 97.25% of the mass of water. Most of the freshwaters, whose volume is estimated to be 39·106 km3, are also not immediately accessible: 29·106 km3 is ice accumulated on mountain glaciers and on the ice caps of the poles; 9.5·106 km3 constitute groundwaters and only about 0.13·106 km3 are surface waters, mainly lakes and rivers. The amount of water held up in the biosphere is estimated to be 0.6·103 km3. The atmospheric moisture amounts to just 13·103 km3 — less than 10−5 of the total amount of water — but this small amount is the one which actuates the hydrologic cycle by virtue of its dynamic nature. <...>

Although (Soddy, Nature 92:399–400, 1913) inferred the existence of isotopes early last century, it was not until the discovery of the neutron by (Chadwick, Nature 129:312, 1932) that isotopes were understood to result from differing numbers of neutrons in atomic nuclei. (Urey, J Chem Soc 1947:562–581, 1947) predicted that different isotopes would behave slightly differently in chemical (and physical) reactions due to mass differences, leading to the concept of isotopic fractionation.