Hydrogen has two stable isotopes 1H and 2H (known as Deuterium)
Change in physico-chemical property: The boiling point of water consisting of
only lighter isotope of hydrogen (1H) is 100 0C but if the all the water molecules
are made of 2H, the boiling point is 101.42 0C.
Reason of the change This increase in boiling point is because it is more difficult
to break bonds made out of heavier isotope. Therefore, if a water sample consisting
of molecules made of both 1H and 2H is heated, 1H2O (water molecules made of 1H)
will be more abundant in the vapor phase than in the liquid phase as compared to 2H2O.
This change in the relative abundance of different stable isotopes is called
Utility of fractionation Measurement of relative amounts of the two hydrogen isotopes
in a sample can tell us about the temperature at the time of evaporation and other factors
which can influence the extent of fractionation IF we have pre-determined the affect of
different factors under the laboratory conditions.