Quick Answer: The Isotopes of Hydrogen Model compares protium, deuterium and tritium, showing that each has one proton but a different number of neutrons and therefore a different mass number.
Last updated: October 2026
Key Features
Side-by-side comparison of the three hydrogen isotopes
Every isotope keeps one proton and atomic number 1
Neutron counts of 0, 1 and 2 give mass numbers 1, 2 and 3
Introduces stable and radioactive isotopes at a conceptual level
Technical Specifications
Specification
Value
Element studied
Hydrogen, atomic number 1
Protium (hydrogen-1)
1 proton, 0 neutrons
Deuterium (hydrogen-2)
1 proton, 1 neutron
Tritium (hydrogen-3)
1 proton, 2 neutrons
About This Product
Teachers start with protium and its single proton, then move to deuterium and tritium as one and then two neutrons are added. Because every nucleus still holds one proton, students see why all three remain hydrogen, which makes the definition of an isotope concrete. The model supports chemistry lessons on atomic number, mass number and nuclear structure. Besides buyers across India, the Isotopes of Hydrogen Model can be exported to institutions in Australia, Dominican Republic, Mozambique, Benin, Trinidad and Tobago and Antigua and Barbuda.
Frequently Asked Questions
Q1. Why are protium, deuterium and tritium all hydrogen? Each nucleus contains one proton, so all three have atomic number 1. Only the neutron number changes, which alters the mass number but not the element.
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