Isotopes

Isotopes are two or more types of chemical species or elements that are having same atomic number and the same position in the periodic table of elements. isotopes have different mass numbers or nucleon numbers due to the difference in the number of neutrons in their nuclei. However, all isotopes of a particular element have almost the same chemical properties and different atomic masses, and physical properties. Atomic Number is the number of protons inside the nucleus of an atom, While, the mass number is the number of nucleons inside the nucleus of an atom. Thus, each isotope of a particular element exhibit a different mass number. Isotopes, Isobars, and Isotones are three classifications of elements done on the basis of various similar characteristics. 

What are Isotopes?

The number of protons in an atom of a given element is constant, while the number of neutrons might vary. For example, all carbon atoms contain six protons, and the majority of them also have six neutrons. 

However, certain carbon atoms have more than the usual six neutrons—seven or eight in some cases. Isotopes are multiple versions of the same element’s atoms that have different quantities of neutrons. Many isotopes are found in nature. The most stable and common isotopes of an element are often one or two of them. Due to their similar proton and electron numbers, different isotopes of an element usually share the same physical and chemical characteristics.

Isotopes Examples

Let’s discuss some examples of Isotopes of significant elements like:

Isotopes of Hydrogen

Hydrogen has three naturally occurring Isotopes. Isotopes of Hydrogen are ₁H¹ Protium, ₁H² Deuterium, and ₁H³ Tritium as shown below:

Isotopes of Carbon

Carbon 12 and Carbon 14 are both isotopes of carbon, one with 6 neutrons and one with 8 neutrons (both with 6 protons). Carbon-12 is a stable isotope, while carbon-14 is a radioactive isotope (radioisotope).

Types of Isotopes: Stable Isotopes, Primordial Isotopes, and Radioactive Isotopes

1. Stable Isotopes: Stable isotopes are isotopes with extraordinarily long half-lives (half-life is defined as the time it takes for a substance to decompose and reach a concentration or weight that is half, or 50%, of its initial concentration or weight). Examples of Stable Isotopes are Carbon (Carbon-12, Carbon-13, and Oxygen (Oxygen-16, Oxygen-17, and Oxygen-18).
2. Primordial Isotopes: The isotopes with primordial nuclei are those. The nuclides that have been around since the creation of our solar system are known as primordial nuclides. On Earth, there are 339 naturally occurring isotopes in total, 286 of which are Primordial Isotopes.
3. Radioactive Isotopes: Some isotopes have extremely short half-lives and degrade quickly, emitting radioactive waves as they do so. These are known as radioactive isotopes. Isotopes that are radioactive include, Tritium, Carbon-14, etc.

Radioactive Isotopes

More than 3000 radioactive isotopes are known. They are an element’s unstable form. They emit various degrees of radiation, which makes them valuable in biological investigations, industry, agriculture, radiopharmaceutical sciences, and industrial uses.

In research reactors and accelerators, radioisotopes are artificially and safely created. Radioisotope treatment, which safely and effectively eliminates malignant cells, is one way that radioisotopes are used to treat cancer and other chronic diseases. Other applications include improving healthcare goods by eliminating or neutralizing toxins, microorganisms, and chemicals that pose risks.

The following are the important uses of Radioactive Isotopes:

1. Radioactive Dating: Radiocarbon dating, which determines the age of carbon-bearing objects, uses the radioactive isotope carbon-14. Because radioactive isotopes’ half-lives are unaffected by external variables, the isotope functions as an internal clock.
2. Irradiation of Food: Some radioactive compounds produce radiation that may be used to destroy germs on a range of goods, therefore prolonging their shelf life. Tomatoes, mushrooms, sprouts, and berries are all irradiated with cobalt-60 or cesium-137 emissions.
3. Medical Applications: Radioactive isotopes offer a wide range of medicinal uses, including the diagnosis and treatment of sickness and disease. For example, ³²P is utilized for cancer identification and therapy, particularly in the eyes and skin, ⁵⁹Fe for anemia diagnosis, ⁶⁰Co for tumor gamma-ray irradiation, ¹³¹I for thyroid function diagnosis and treatment, and many more uses.
4. Other uses: Radioactive isotopes find uses in agriculture, the food industry, pest control, archaeology, and medicine. 

Application of Isotopes

Some of the important uses or applications of Isotopes are:

• Isotopes provide particular elements with the same atomic number and particular properties. As a result, isotopes are employed in the element’s chemical analysis.
• Due to their ease of measurement, isotopes are frequently employed to gauge reaction rates or changes in the concentration of reactants and products.
• Additionally, they are employed in analytical processes like nuclear magnetic resonance and mass spectrometry.

Read More: Difference between Isotopes and Isobars

FAQs on Isotopes and Isobars

Question 1: Define Isotopes with an Example.

Answer:

The number of protons in an atom of a given element is constant, while the number of neutrons might vary. For example, all carbon atoms contain six protons, and the majority of them also have six neutrons. 

Question 2: Name the Isotopes of Hydrogen.

Answer:

Hydrogen has three naturally occurring Isotopes. Isotopes of Hydrogen are ₁H¹ Protium, ₁H² Deuterium, and ₁H³ Tritium

Question 3: Distinguish between Isotopes and Isobars.

Answer:

Following are the differences between Isotopes and Isobars-

Isotopes	Isobars
Isotopes are atoms with the same number of protons but differ in numbers of neutrons.	Isobars are atoms of different chemical elements having equal values for atomic mass
Isotopes of an element have the same chemical properties	Isobars differ in their chemical properties
Isotopes occur in the same place in the periodic table.	Isobars occur at a different place in the periodic table.
Isotopes have different physical properties from each other	Isobars mostly have similar physical properties.
Similar arrangement and number of electrons	Arrangement of electrons are different.
They are atoms of the same element.	They are atoms of different elements.

Question 4: Isotopes have the same chemical properties while isobars do not have the same. Why?

Answer: 

Isotopes of an element have the same number of electrons and protons but have the different numbers of neutrons. Since the chemical properties of elements depend upon the atomic number, isotopes of an element have simile chemical properties.

On the other hand, isobars have the different numbers of electrons, protons as well as neutrons. Thus, isobars have different chemical properties.

Question 5: What are the Applications of Isotopes?

Answer: 

• Isotopes provide particular elements with the same atomic number and particular properties. As a result, isotopes are employed in the element’s chemical analysis.
• Due to their ease of measurement, isotopes are frequently employed to gauge reaction rates or changes in the concentration of reactants and products.
• Additionally, they are employed in analytical processes like nuclear magnetic resonance and mass spectrometry.