Difference Between Isotopes and Isobars: Definitions, Examples, History, Uses, Key Differences, and Sample Questions

Difference Between Isotopes and Isobars Overview

Isobar elements have chemical characteristics that differ yet have the same physical attribute. Isotopes and isobars are two keywords used often in atomic structure. Isotopes are elements with distinct mass numbers but the same atomic numbers. Isotopes are elements with identical mass values but different atomic numbers. Thus, the primary distinction between isotopes and isobars is that isotopes are of the same element as isotones. Isotopes also have comparable chemical characteristics. Isobars, on the other hand, have distinct chemical characteristics.

Difference Between Isotopes and Isobars Definitions

Isotopes

Atoms with the same number of protons but different quantities of neutrons are called isotopes. The atomic number of an atom is the number of protons in that atom. The number of protons in a chemical element is fixed. As a result, the atomic number of atoms of the same chemical element is identical. Isotopes are therefore atoms of the same chemical element. The atomic mass is defined as the total number of protons and neutrons. The atomic masses of isotopes differ. The chemical behavior of isotopes of a chemical element is the same, but their physical qualities differ. Isotopes exist for almost every chemical element. There are275 known stable chemical element isotopes. An isotope is called using the chemical element name and the isotope's atomic mass.

History of the Isotope Word

Margaret Todd suggested that the name "isotope" be used by the British scientist Frederick Soddy in 1913. The word derives its meaning from the Greek words isos (equal) + topos (location). Isotopes of the same element have the same position on the periodic table while having differing atomic weights.

Notation of Isotopes

There are main approaches to identifying isotopes, they are as follows-

1. List an element's mass number after its name or element symbol. 
2. Carbon-12, or C-12, is an isotope containing six protons and six neutrons. 
3. Carbon-13 or C-16 is an isotope with 6 protons and 7 neutrons. 
4. It should be noted that the mass number of two isotopes may be the same, despite the fact that they are distinct elements. 

Isobars

The name "isobar" comes from the Greek words isos (equal) and baros (weight). Isobars are atoms of various chemical elements with identical atomic masses. Atomic mass is the sum of protons and neutrons in an atom's nucleus. A nucleon is either a proton or a neutron. As a result, isobars contain the same number of nucleons. Because various chemical elements have varying atomic numbers, the atomic numbers of these isobars differ. According to the Mattauch isobar rule, if two neighboring elements on the periodic table contain isotopes with the same mass number (isobars), at least one of these isotopes must be radioactive. If three successive isobars exist, the first and last are stable, whereas the middle one may experience radioactive decay. An isobar series is a grouping of isotopes with the same atomic mass.

Difference Between Isotopes and Isobars Examples

Examples of Isotopes

1. Carbon 12 and Carbon 14 are both carbon isotopes, one having 6 neutrons and the other with 8 neutrons (both with 6 protons). 
2. Carbon-12 is an isotope that is stable, whereas carbon-14 is a radioactive isotope (radioisotope).
3. Uranium-235 and uranium-238 are naturally occurring elements in the Earth's crust. 
4. Both have extremely lengthy half-lives. Uranium-234 is formed as a byproduct of decay.

Examples of Isobars

1. Consider two items that have the same color and physical appearance and cannot be distinguished from one another. However, when one weighs these two items, one will discover that they are not the same. This example might help one to understand the notion of isotopes.
2. Cobalt (Co), Nickel (Ni), Copper (Cu), and Iron (Fe) are isobars with atomic mass 64. (Fe).
3. Hydrogen (H) and Helium (H) are isobars of atomic mass 3. (He).

Classification of the Elements of Isotopes

The following table explains the different elements classifications-

Classification of the Elements of Isobars

The following table explains the different elements classifications-

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Difference Between Isotopes and Isobars Uses

Uses of Isotopes

1. The use of an iodine isotope can treat goiter (swelling neck) conditions.
2. Cobalt isotopes can be used to treat some forms of cancer.
3. Nuclear fuel is made from uranium isotopes.

Uses of Isobars

1. In the medical profession, isobars are used to treat malignancies and blood clots.
2. Iodine isobars can be used to treat thyroid problems.
3. Phosphorus isobars can be used to treat blood cancer.

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Difference Between Isotopes and Isobars

The following table gives information about the differences between isotopes and isobars-

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Things to Remember

1. The mass number is the sum of the numbers of protons and neutrons.
2. Isobars have distinct atomic numbers but have the same mass number.
3. Isobars are elements with distinct chemical characteristics but identical physical properties.
4. Isotopes have atomic numbers that are comparable but have different masses.
5. Isotopes are elements with identical chemical characteristics but distinct physical properties.

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Summary

The terms isotope and isobar indicates the chemical element connections. As a result, it is critical to comprehend the distinction between them. Isotopes represent the link between various versions of the same chemical element. Isobars represent the connection between chemical elements with different atomic masses but the same physical characteristics. Isotopes are atoms of the same element with different quantities of neutrons.

Because they have the same amount of protons and electrons, different isotopes of an element have the same physical and chemical characteristics.

Key Takeaways

1. Isotopes are elements that have variable quantities of neutrons in their atoms.
2. Radioactive isotopes degrade. When an isotope decays, the parent isotope is the beginning substance. 
3. The number of protons in various isotopes of an element remains constant.
4. Not every isotope is radioactive. 
5. Stable isotopes do not degrade or decay extremely slowly. 
6. The daughter isotope is the resultant substance.

Sample Questions for the Difference Between Isotopes and Isobars

Sample Question 1- What are isotopes?

Isotopes are atoms of the same element with the same atomic number but a different mass number.

Sample Question 2- What is the significance of isobar chemistry?

Even at the same height, atmospheric pressure varies depending on location. Isobars are reference lines that run beside a route and have the same pressure along the line. The user may generate a realistic estimate at any map point by drawing a sequence of lines, each one identifying a spot where the pressures have a comparable stated value. He can do so by reading the pressure of the line if it happens to pass through the interesting site exactly, or by interpolating based on the nearest isobar, which is at a higher pressure than the intriguing point, and the isobar nearby, which is at a lower pressure.

Sample Question 3- Where are isobars and isotopes found in elements? 

Because atoms of the same element have variable numbers of neutrons, elements have various isotopes. Because neutrons and protons have the same mass number (s), different elements may have different isobars.

Sample Question 4- What exactly are isobars?

Isobars are atoms of various elements that have the same mass number but a different atomic number.

Sample Question 5- Why are isobars and isotopes present in elements?

It has distinct isotopes due to the existence of a variable number of neutrons in atoms of the same element. Because neutrons and protons have the same mass number (s), various elements might have distinct isobars.