An introduction to Atomic number, Mass number Isotopes as well as Isobars: Definition with examples

Atomic Number

Atomic number is the total number of protons present in the nucleus of an atom which is represented by Z. Atom is electrically neutral and hence the charge of a proton is equal but opposite to that of an electron. Since elements tend to lose or gain electrons during the chemical reactions, the number of protons is generally used to represent the atomic number of an element.

Atomic Number (Z) = Number of protons in the nucleus of an atom

Examples: Hydrogen atomic Number is 1 and it has 1 proton

Helium atomic Number is 2 and it has 2 number of Protons

Sodium atomic Number is 11 and it has 11 number of Protons

Mass Number

Mass number (A) is the total number of protons and neutrons present in the nucleus of an atom. Inside the nucleus Protons and neutrons are present which are together called nucleons. So, in other wards we can say that the mass number is the number of nucleons present in an atom.

Mass Number (A) = Number of Protons + Number of neutrons

Example:

Lithium: Number of Protons = 3, Number of Neutrons= 3; Mass Number = 6

Calcium: Number of Protons = 20, Number of Neutrons= 20; Mass Number = 40

Isotopes

Isotopes are defined as any of two or more forms of a chemical element, having the same atomic number (number of protons) but possess different mass number in the nucleus. In general, Isotopes of a single element possess almost identical properties.

Example:

Hydrogen has three isotopes namely, protium, deuterium, and tritium. All have one single proton (Z = 1), but differ in the number of their neutrons. Hydrogen has no neutron, deuterium has one, and tritium has two neutrons.



 Isobars

Isobars are a group of elements that have different atomic numbers but their mass number are the same. The chemical properties of the isobars are different but they exhibit similar physical properties.

Examples:

11Na24 and 12Mg24

13Al27 and 14Si27

 

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