What Are Isotopes

Isotopes can be identified as the forms of chemical elements that hold the same or an equal number of electrons and protons, but have dissimilar numbers of neutrons. Isotopes are other forms of elements that vary in nuclei numbers due to dissimilarity in the numbers of neutrons in their nuclei. This includes prefixing the mass in superscript and the number of atoms in subscript and writing the element’s symbol. For example, the uranium-239 isotope represents 239U92 and the uranium-235 isotope represents 235U92.

Isotopes Definition

Any two or more pairs of atoms or species of atoms of an element which have the same or equal number of electrons and equal number of protons but they are different because of their distinct number of neutrons. Also isotopes are species of atoms which have the same atomic number and similar chemical properties or behaviour, but differ by their atomic mass or different physical properties and different mass number. 

Isotopes are atoms of an element which usually carry the exact number of electrons and exact number of protons and that’s why they have similar identical chemical properties. However, they are different from each other because of their dissimilar number of neutrons.

Isotopes of hydrogen

There are three isotopes of hydrogen:

1. Protium (1H)

Protium is a very common isotope of hydrogen. It is 99.98% abundant. It is because its nucleus contains a single proton and at no time it has been described to be decayed. Protium’s mass is 1.007825 amu. Generally, the hydrogen combines in compounds with the other form of atoms and usually, it is found in diatomic hydrogen gas (H2).

Applications of Protium

Treat intestine & stomach acid-related illnesses 

Proton pump inhibitor

Pantoprazole

2. Deuterium (2H)

The Deuterium contains 1 neutron and 1 proton in the nucleus. The deuteron is the nucleus of hydrogen 2. It’s not radioactive. It is very useful for solvents for hydrogen 1 and chemical analysis. Heavy water is added with the molecules containing deuterium, not protium. It can be used as a neutron moderator and coolant also. H2 is used as a fuel in (commercial) nuclear fusion also. It arises naturally as a deuterium gas.

Applications Of Deuterium 

Nuclear weapons

Drugs

Tracing

Contrast properties

Nuclear reactors 

NMR spectroscopy 

Nuclear Power Plants

3. Tritium (3H)

It contains 1 proton and 2 neutrons in the nucleus. Small finds of H3 or tritium arise in nature with atmospheric gases due to the energy of cosmic rays. They can be released in a very small amount also when nuclear weapons are being tested. Tritium is radioactive.

Applications of Tritium

Control the nuclear fusion 

Analytical chemistry

Boosting

Hydrogen bomb secondaries

Nuclear weapons

Neutron initiator

As a transient tracer of ocean

Lighting (Self-power)

Examples of Isotopes 

1. Chlorine

It is a chemical element, it has 17 atoms and the symbol of chlorine is Cl.

Chlorine-35 & Chlorine-37 

Both of these are isotopes of chlorine, these isotopes have 17 numbers of electrons and protons but these are differing by having distinct neutrons Chlorine-35 has 18 numbers of neutrons and chlorine 37 has 20 numbers of neutrons. 

2. Iodine

It is an element which has the symbol I and its atomic number is 53. This is the heaviest element from the stable halogens, this element is semi-lustrous,and it is non-metallic solid at any standard conditions which start melting for forming a deep violet liquid (114°C), and start boiling into a violet gas (184°C).

Iodine-131 & Iodine-129

Both of these have 53 numbers of electrons and protons but these have different numbers of neutrons. Iodine-131 has 78 numbers of neutrons and Iodine-129 has 76 numbers of neutrons.

3. Carbon 

It is a chemical element, it has 6 atomic numbers. And its symbol is C. It is tetravalent, makes covalent bonds by sharing 4 electrons, and is non-metallic. It is in group number 14 in the modern periodic table.

Carbon-14 & Carbon-12

Both of these have 6 numbers of electrons and 6 numbers of protons but these are different because of their neutrons as carbon-14 has 8 numbers of neutrons and carbon-12 has 6 numbers of neutrons.

Conclusion 

We understood about Isotopes that Isotopes are variant forms of chemical elements. They have the same number of electrons and the same number of protons. But they differ because of their different numbers of neutrons. We understood about isotopes of hydrogen –  Protium (1H), Deuterium (2H) and Tritium (3H) we saw these usage or applications, also we have seen some examples of isotopes like the isotopes of carbon – (carbon-12), (carbon-13), (carbon-14) these have same or equal electrons and protons but have distinct number of neutrons. This is what we have learnt about the isotopes.