Atomic theory has progressed since ancient Greek times. Scientists have used Greek scholars’ ideas as a starting point for their research. They’ve made numerous discoveries and speculations about the atom. It also comes from the Greek word “atomos,” which means “undivided.” Since then, scientists have discovered that these particles can be broken down further into protons, neutrons, and electrons. Despite this, the term “atom” has endured.
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Theories of Atomic Structure:
1. Ancient Greeks Belief:
“All matter is made up of atoms, which are small units of matter.” All substance is made up of smaller units called atoms, as hypothesised by Leucippus and Democritus in the fifth century B.C. They further claim that these were solid particles with no interior structure that came in a variety of shapes and sizes. They also say that they were solid particles with no interior structure and that they appeared in a range of shapes and sizes. In addition, they created intangible attributes such as taste and colour.
2. The Dalton Atomic Theory:
In 1808, English scientist John Dalton based his work on the Greek concept of atoms. He proposed that matter is made up of atoms, which he defined as minuscule, indivisible units. He also argued that, while all atoms of one element are identical, those of other elements are completely different.
3. The Theory of J.J. Thomson:
The “plum pudding” idea of the divisible atom was proposed by English scientist Joseph J. Thomson in 1904. After finding electrons in 1897, he did so. In addition, his model suggested that atoms are made up of a large positively charged sphere studded with negatively charged electrons (dubbed “corpuscles”), similar to the fruit in a plum pudding.
He also claimed that the charge of the positive sphere is equivalent to the charge of the electrons’ negative charges. Today, positively charged particles are referred to as protons, while negatively charged particles are referred to as electrons.
4. Rutherford’s Theorem:
In 1911, British physicist Ernest Rutherford suggested a nuclear hypothesis for atoms. A nucleus is a part of an atom. He already identified the central part of the atom’s activity, such as the movement of protons and electrons. He also proposed that the number of protons and electrons in an atom are equal.
5. Bohr’s Theory
Niels Bohr, a Danish physicist, presented a planetary model in 1913, in which electrons rotate around the nucleus in the same way that planets orbit the sun. The electrons have “constant energy” when they are in orbit. This hypothesis refers to these atoms as “stimulated” electrons when they grasp the energy and go into a higher orbit. They leave this energy as electromagnetic radiation when they return to their initial orbit.
The electrons inside atoms are put in discrete orbits called “stationery orbits,” according to the following postulates:
Bohr’s Atomic Theory’s Limitations:
6. Quantum Mechanics and Einstein, Heisenberg
Drawback: Bohr accurately measured two such conjugate quantities: position and momentum (theoretically).
Matter: Dual Nature
The photoelectric effect reveals that the electrons that were viewed as particles also have a wave nature. With the use of his double-slit experiment, Thomas Young demonstrated this. De-Broglie concluded that because nature is symmetrical, light or any other matter-wave should be as well.
Quantum Mechanics:
The orbital number or shell number of an electron is denoted by the principal quantum number (n).
Azimuthal Quantum Numbers (l): It denotes the electron’s orbital (sub-orbit).
The number of energy levels in each orbit is denoted by the magnetic quantum number. The direction of spin is denoted by the quantum number(s) S = -112 = Anticlockwise and 12 = Clockwise.
Atom Electronic Configuration:
The electrons in the s, p, d, and f must be filled according to the following rule.
The energy of orbital α(p + l) value it two orbitals have same (n + l) value, E α n
Ascending order of energy 1s, 2s, 2p, 3s, 3p, 4s, 3d, . . .
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