Atomic structure and some important facts related to it
Atomic structure and some important facts related to it.
Today we will see information about atomic structure in this post, in this we will explain the complete definition of atom, molecule, atomic weight, molecular weight, mole number, isotopic, isobar.
Atomic structure and some important facts related to it
Atomic structure
Atom: - Atom is the smallest particle of an element, which can participate in any chemical reaction but cannot remain in an independent state.
Molecules: - The smallest particle of an element and a compound that can remain in an independent state is called a molecule.
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Atomic Weight: - The atomic weight of any element is a number that shows how many times an atom of an element is filled by the mass of 1/12 part of the atom of carbon-12 or 1.008 part mass of hydrogen.
Molecular Weight: - The molecular weight of a substance is a number that shows how many times a fraction of that substance is 1/12 of an atom of carbon-12.
Mole Assumption: - One mole is the amount of a substance with a certain formula, which has the same number of units of the formula - the number of atoms in exactly 12 grams of the pure carbon-12 isotope.
Value of mole unit: - The value of mole is 23 to the power of 6.022 * 10. The power of 6.022 * 10 is 12 atoms in 12 grams or one mole of carbon. 6.022 * 10 to the power of 23 is called Avogadro number.
Mole signifies both number and mass. In 1967, Mole was accepted as a unit.
As a result of modern discoveries in the 20th century, scientists such as JJ Thomson, Rutherford, Chadwick etc. proved that atoms are divisible and consist mainly of three basic particles, called electrons, protons, and neutrons.
Atomic Number: - The number of protons present in the nucleus of an element's atom is called atomic number.
Mass Number: - The sum of the number of protons and neutrons present in the nucleus of an atom is called the mass number of that atom.
Mass number = number of protons + number of neutrons
Quantum Number: - Four quantum numbers are used to understand the microscopic nature of spectrum lines and to describe the exact position of the electron, these are
Micro quantum number: - "n" It represents the main energy level of the electron.
Diganshi Quantum Number: - "l" It reveals the shape of the electron orbit. Its minimum value is zero and maximum value (n-1).
Magnetic quantum number: - "m" It represents the orbitals of sub energy levels. The value of m depends on the value of l. The values of m for any l range from +1 to -1. (Including zero)
Rotation Quantum Number: - "s" It represents the direction of rotation of electron. For a magnetic quantum number (m), the value of the rotating quantum number (s) is +1/2 and -1/2.
Isotopes: - Atoms of same atomic number but different atomic masses are called isotopic. Institutions have the same number of protons, but different numbers of neutrons. Eg-1H1, 1H2, 1H3 are isotopic.
The most isotopic elements are polyanium.
Isobaric: - Atoms of the same atomic mass but different atomic number are called isobaric, such as - 18 Organ 40, 19 Potassium 40, 20 Calcium 40 are isobaric.
Samanutron: - Atoms that have the same number of neutrons are called synutronic. Such as 1 Hydrogen 3, and 2 Helium 4 The number of neutrons in the nucleus of these two atoms is two to two.
Coelectronics: - The ions and atoms that have the same electronic configuration are known as cooelectronics. The number of electrons in the same electron atoms and ions are the same. Such as neon, sodium +, magnesium ++, and aluminum +++ are colectronic.
Pauli's law of exclusion: - According to this, the value of the four quantum numbers for any two electrons in a given atom cannot be the same. For science click here so if the values of two electrons n, l, and m are the same. If, then their rotation will be the opposite.
Hund's rule of maximum plurality: - According to this, electrons are not coupled as long as blank orbitals are attainable, that is, electrons remain unpaired as long as possible.
Heisenberg's uncertainty principle: - According to this, simultaneous exact determination of position and velocity of a particle is impossible.
Offbau rule: - The order of energy of different atomic orbitals for writing electronic configuration of elements by this rule is as follows.