Atomic Structure of Isotopes
The isotopes of an atom have the same atomic number which means that the number of protons are same. Also, their chemical properties are the same because their electronic configuration is the same. The difference in mass number arises due to the difference in number of neutrons present inside the nucleus. Hence, the atomic structure of isotopes comprises of the same number of electrons and protons but different number of neutrons. We can understand this with the example of isotopes of hydrogen illustrated below:
To describe the structure of an isotope, the element’s symbol is used along with the atomic number and the mass number of the isotope. To give an example, Hydrogen has 3 isotopes named protium, deuterium, and tritium. The atomic configuration of three isotopes of hydrogen is tabulated below:
Isotopes of Hydrogen | Atomic Number | Mass Number | No. of Electrons | No. of Protons | No. of Neutrons |
---|---|---|---|---|---|
Protium | 1 | 1 | 1 | 1 | 0 |
Deuterium | 1 | 2 | 1 | 1 | 1 |
Tritium | 1 | 3 | 1 | 1 | 2 |
The stability of isotopes is different. The half-lives are also different. But they generally have similar chemical behavior because they have the same electronic structures. The pictorial representation of isotopes of hydrogen can be seen below:
Atomic Structure
Atomic structure is the structure of an atom that consists of a nucleus at the center containing neutrons and protons, while electrons revolve around the nucleus. Atoms are made up of a very tiny, positively charged nucleus that is surrounded by a cloud of negatively charged electrons.
The earliest concept of atoms was given by Indian philosopher Maharshi Kanad who proposed that matter is made up of microscopic indestructible particles called ‘Parmanu’. A Greek philosopher named Democritus also initially claimed that matter is formed of atoms, and is credited with developing the concepts of atomic structure and quantum mechanics. Later in the 1800s, John Dalton a British Scientist put out the first atomic structure scientific theory.
This article explores the concept of atomic structure in detail, including the atomic models, and the concept of quantum theory.
Table of Content
- What is Atomic Structure?
- Atomic Models
- Dalton’s Atomic Theory
- Postulates of Dalton’s Atomic Theory
- Demerits of Dalton’s Atomic Theory
- Thomson’s Atomic Model
- Cathode Ray Experiment
- Observations of Cathode Ray Experiment
- Discovery of Electron
- Plum Pudding Model
- Drawbacks of Thomson’s Atomic Model
- Rutherford Atomic Model
- Alpha Ray Scattering Experiment
- Observation of Alpha Ray Scattering Experiment
- Conclusion of Rutherford’s model
- Discovery of Nucleus
- Limitations of Rutherford Atomic Model
- Bohr’s Atomic Model
- Postulates of Bohr’s Atomic Theory
- Limitations of Bohr’s Atomic Theory
- Quantum Mechanical Model of Atom
- Dual Behaviour of Matter
- Heisenberg Uncertainty Principle
- Schrodinger Wave Equation
- Postulates of Quantum Mechanical Model of Atom
- Quantum Number
- Principal Quantum Number(n)
- Azimuthal Quantum Number(l)
- Magnetic Quantum Number(ml)
- Spin Quantum Number(ms)
- Subatomic Particles
- Isotopes
- Atomic Structure of Isotopes
- Electronic Configuration of Elements
- Aufbau Principle
- Hund’s Rule
- Pauli Exclusion Principle
- Atomic Structure Class 11
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