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Explanation:
1 ) In atomic physics, the Rutherford–Bohr model or Bohr model, presented by Niels Bohr and Ernest Rutherford in 1913, is a system consisting of a small, dense nucleus surrounded by orbiting electrons—similar to the structure of the Solar System, but with attraction provided by electrostatic forces in place of gravity.
2) ISOTOPES :: Elements with the same atomic number but a different mass number are defined as “Isotopes”. The number of protons and neutrons combined together is called atomic mass or mass number of an element, whereas the total number of protons gives the atomic number of an element.In a certain element, the number of protons will always remain constant. However, the number of neutrons can change. Examples of Isotopes: Carbon-14 A naturally occurring radioactive isotope of carbon having six protons and eight neutrons … Iodine-131 It is an isotope because it contains a different number of neutrons from the element … Tritium
ISOBARS :: Isobars are atomic species having the same mass number but different atomic number e.g. etc. they differ in chemical properties, however physical properties related to mass are same. Isotones are atoms having same number of neutrons but different mass number e.g. Correspondingly, isobars differ in atomic number (or number of protons) but have the same mass number. An example of a series of isobars would be 40 S, 40 Cl, 40 Ar, 40 K, and 40 Ca etc.
3) ATOMIC RADIUS :::::The atomic radius of a chemical element is a measure of the size of its atoms, usually the mean or typical distance from the center of the nucleus to the boundary of the surrounding shells of electrons. Since the boundary is not a well-defined physical entity, there are various non-equivalent definitions of atomic radius. Three widely used definitions of atomic radius are: Van der Waals radius, ionic radius, and covalent radius.
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