Answer

There are three isotopes of the element hydrogen: hydrogen, deuterium, and tritium.

How do we distinguish between them?

They each have one single proton (Z = 1), but differ in the number of their neutrons. Hydrogen has no neutron, deuterium has one, and tritium has two neutrons.

The isotopes of hydrogen have, respectively, mass numbers of one, two, and three. Their nuclear symbols are therefore ¹H, ²H, and ³H.

The atoms of these isotopes have one electron to balance the charge of the one proton. Since chemistry depends on the interactions of protons with electrons, the chemical properties of the isotopes are nearly the same.

Energy may be released as a packet of electromagnetic radiation, a photon. Photons created in nuclear processes are labeled gamma rays (denoted by the Greek letter gamma.

For example, when a proton and neutron combine to form deuterium, the reaction can be written ¹n + ¹H Æ ²H + g.

Energy must balance in this equation. Mass can be written in atomic mass units (u) or in the equivalent energy units of million electron-volts divided by the square of the speed of light (MeV)/c². (From Einstein’s mass-energy equivalence equation, E = mc², u = 931.5 MeV/c².)

The mass of the deuterium nucleus (2.01355 u) is less than the sum of the masses of the proton (1.00728 u) and the neutron (1.00866 u), which is 2.01594 u. Where has the missing mass (0.00239 u) gone? The answer is that the attractive nuclear force between the nucleons has created a negative nuclear potential energy–the binding energy E_B–that is related to the missing mass, D m (the difference between the two masses).

The photon released in forming deuterium has an energy of 2.225 MeV, equivalent to the 0.00239 u required to separate the proton and neutron back into unbound particles. The nuclear decay photons are, in general, higher in energy than photons created in atomic processes.