Subatomic Particles
The subatomic particles are the particles that are present inside the atom, There are three subatomic particles that are,
- Protons
- Neutrons
- Electrons
Protons
- Protons have a positive charge. This charge is 1e, which is approximately 1.602 × 10-19
- Mass of a proton is approximately 1.672 × 10-24
- Protons are over 1800 times heavier than electrons.
- Total number of protons in the atoms of an element and the atomic number of the element is always equal.
Neutrons
- Mass of a neutron is almost similar to that of a proton i.e. 1.674 × 10-24
- Neutrons are always electrically neutral particles and do not carry any charge.
- Isotopes of an element have the same number of protons but a different number of protons in their respective nuclei.
Electrons
- Charge of an electron is -1e, which is approximately -1.602 × 10-19
- Mass of an electron is approximately 9.1 × 10-31.
- Mass of an electron is almost negligible as compared to the mass of an atom, so an electron’s mass is ignored while calculating the mass of an atom.
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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