The atomic number of hydrogen is 1 and surprisingly its atomic weight also nearly about 1 only. Since atomic mass is measured by the sum of protons and neutrons, It has to assume that hydrogen didn't contain a neutron. What is the main reason for it, since almost all other lower elements follow the same pattern
There exists 3 isotopes of the hydrogen atom, the most abundant has a nucleus made up of 1 proton as you mention. The second isotope is called Deuterium, it is stable also and its nucleus is made up of 1 proton plus 1 neutron. You also have Tritium, which is made up of 1 proton plus 2 neutrons. This one is unstable and quickly decays into 1 helium-3 atom (2 protons plus 1 neutron). If you look for these names in wikipedia or any proper reference, you will get the whole story.
so I heard that single hydrogen atom is not stable so that it exist as hydrogen molecule in nature. is this deuterium atom is more stable than hydrogen molecule? If neutron is mean for the stability of atom then deuterium wants to see more abundant than hydrogen molecule which is not seen in the nature
H1 is known to be totally stable and so is H2 (deuterium). You should look up pertaining formal literature to learn more about this.
Protons are totally stable except in very few higher mass nucleii if I recall correctly. All atoms except the rare gasses combine into molecules in nature at temperatures ambient on the Earth. Combinations of atoms to form molecules has no relation with nuclei being stable or unstable.
The reason(s) why nuclei of some isotopes are stable and others are unstable have not yet been conclusively clarified.
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