Nucleus-Isotopes

To understand the concept of Isotopes, first, understand the atomic structure. Many scientists contributed to the field of developing theories for atomic structure. J.J Thompson was the first scientist who explained the structure of atoms and the presence of electrons. Later, Rutherford explained the molecular structure of the atom by doing his experiment with gold foil. He proposed that the atom’s mass is restricted in the limited space of the atom. 

Electrons are negatively charged particles that revolve in outer orbit. Rutherford’s theory has some limitations. Later, Bhor’s atomic structure gave the scientific explanation of Rutherford’s theory by giving postulates. He explained the atomic structure, which derives the Atomic number and Atomic Mass of the atom.

Structure of atom

The structure of an atom consists of three types of particles. First, the electrons are negatively charged particles present in the outer orbit. The second is the protons, which are positively charged particles present in the atom’s nucleus. Neutrons are neutral particles that also lie in the nucleus of the atom.

What are the atomic numbers and atomic mass? An atom carries atomic number and mass due to protons and neutrons. Atoms get placed on the atomic table according to their atomic number and mass.

Isotopes- Meaning and definition: 

 Isotopes consist of two words: first is Iso, which means “the same” and second is Topes, which means “the number”. Let’s define the term as some matter that has the same number.

Defining isotopes 

Elements with the same atomic number, but different atomic mass are isotopes. In other words, the number of photons is the same in isotope elements. For example, protium and deuterium are the isotopes of hydrogen.

The isotopes are placed in the same place in the periodic table since they share the same atomic number.

Isotopes of Carbon: C-12, C-13 and C-14 are the three isotopes of carbon. The atomic number of all three isotopes is the same as 6, but atomic mass differs.

The neutron number of the carbon isotopes remains the same.

Uses of Isotopes- 

Isotopes have various uses in medical, archaeology and nuclear power projects. Some of the uses of isotopes are as under.

Uses of C-14

This carbon isotope is the oldest radioactive isotope and it is used in archaeology. The carbon dating process is a well-renowned method of estimating old archaeological specimens’ age. The amount of carbon present in the specimen determines the age of archaeological evidence, such as trees and animals. After the death of living creatures, the carbon starts decaying constantly. The decayed percentage of C-14 helps in estimating the age.

Medical uses of Isotopes – 

There are many isotopes used to treat chronic diseases such as cancer, metabolic diseases and treatment of infections. The Isotopes of iodine are used to diagnose and treat thyroid.

Uses of radioactive isotopes: Radioactive isotopes such as uranium are used in nuclear reactors. The radioactive properties generate more thermal and electric power. Apart from uranium, isotopes of Thorium are also used in nuclear power reactors.   

Some other isotopes are used in different manufacturing industries in making pipelines, boilers and medical equipment.

The chemical properties of Isotopes:

The isotopes are quite stable and do not react when left alone. The isotopes of carbon C-14 remained for a very long time in nature. Reactive conditions are created in the nuclear power points. The atomic mass remains the same in isotopes and the atomic numbers differ. The chemical behaviours of atoms are more affected by the electrons and in isobars, the number of electrons doesn’t get impacted.

What is the difference between Isotopes and Isobars?

Like Isotopes, isobars refer to the elements that share the same atomic mass. In Isobar, Iso refers to “the same” and Bars refers to the “Mass”, hence elements whose atomic mass is the same but atomic number is deferred. For example, Argon and Calcium share the same atomic mass of 40; hence both the elements are isobars.

Conclusion

Isotopes share the same atomic number and are placed in a similar position on the periodic table. Isotopes are less reactive and remain unchanged because electrons in the outer orbit are responsible for the chemical reactions. Some Isotopes are radioactive and produce more energy. The isotopes are the gift of nature and some of them are very useful in different sectors. Many isotopes are used to cure critical illnesses like cancer in the medical industry.