Atomic nucleus

1. Discovery of nucleus

  • In 1897 J.J. Thomson discovered the electron in the rays emitted from the cathode of discharge tube filled with gas at low temperatures.
  • Again 1910 Thomson suggested a model for describing atom , known as 'Thomson's atomic model' which suggests that atom consists of positively charged sphere of radius 10-8cm in which electrons were supposed to be embedded.
  • Thomson atomic model failed as it could not give convincing explanation for several phenomenon such as, spectrum
    of atoms, alpha particle scattering and many more.
  • In 1909 Gieger and Marsden employed α-particles (Helium ion) as Projectile to bombard thin metallic foil.
  • According to Thomson atomic model since all positive charge of atom was neutralized by the negatively charged electrons, there would be rare event for an α-particle to suffer a very large deflection , as expected force of repulsion would not be very strong.
  • Surprisingly experiments of Gieger and Marsden showed large deflections of alpha particles that were many orders of magnitude and more common then expected.
  • This result of Gieger and Marsden α-particle scattering experiment was explained by Sir Rutherford in 1911.
  • Rutherford proposed a new atomic model in which electrons were located at much greater distance from the positive charge.
  • Rutherford proposed that all the positive charge , and nearly all the mass of the atom, was concentrated in an extremely small nucleus.
  • The electrons were supposed to be distributed around the nucleus in a sphere of atomic radius nearly equal to 10-8cm.
  • In explaining this experiment Rutherford made simple assumptions that both the nucleus and α-particles (Helium ion) were point electrical charges and the repulsive force between them is given by Coulomb�s inverse square law at all distances of separation.
  • These assumptions made by Rutherford were not valid if α-particle approaches the nucleus to a distance comparable with the diameter of the nucleus.
  • From this experiment there emerged a picture of internal structure of atoms and it also confirmed the existence of the atomic nucleus.
  • Approximate values for size and electrical charge of nucleus were calculated using data of various scattering experiments.

2. Nuclear Composition

  • Atomic nuclei are build up of protons and neutrons.
  • Nucleus of hydrogen atom contains only single proton.
  • Charge on a proton is +1.6x10-19 C and its mass is 1836 times greater then that of electron.
  • Neutrons are uncharged particles and mass of a neutron is slightly greater then that of a proton.
  • Neutrons and protons are jointly called nucleons.
  • Number of protons in nuclei of an element is equal to the number of electrons in neutral atom of that element.
  • All nuclei of a given element does not have equal number of neutrons for example99.9 percent of hydrogen nuclei contains only one proton , some contain one proton and one neutron and a very little fraction contains one proton and two neutrons.
  • Elements that have same number of protons but differ in number of neutrons in their nucleus are called ISOTOPES.
  • Hydrogen isotope deuterium is stable but tritium is radioactive and it decays to changes into an isotope of helium.

    Nuclear Composition

  • In heavy water instead of ordinary hydrogen deuterium combines with oxygen.
  • Symbol for nuclear species follows the pattern AXZ where
         X= Chemical symbol of element
         Z= Atomic number of element or number of protons in the nucleus of that element.
         A= Mass number of nuclide or number of nucleons in the nucleus. A=Z+N where N is the number of neutrons in the nucleus.
  • In symbolic form
    (1)     hydrogen = 1H1 and Deuterium = 2H1
    (2)     Chlorine isotopes are 35Cl17 and 37Cl17

3. Atomic mass

  • Atomic masses refer to the masses of neutral atoms , not of bare nuclei i.e., an atomic mass always includes the masses of all its electrons.
  • Atomic masses are expressed in mass units (u).
  • One atomic mass unit is defined as one twelfth part of the mass of 12C6 atom.
  • So the mass of 12C6, the most abundant isotope of carbon is 12u.
  • Value of a mass unit is
  • We now calculate the energy equivalent of mass unit. We know that Einstein�s Mass-Energy relation is
         Δm = 1.60x10-27 Kg and
         c = 3x108 m/s
         ΔE = (1.60x10-27) x (3x108)2
               =1.49x10-10 J
    but 1eV = 1.6 x 10-19 J
    therefore, $$\Delta E=\frac{1.49X10^{-10}}{1.60X10^{-19}}$$
    ΔE = .931 x 109 eV
    ΔE = 931 MeV
    Thus 1 amu = 931 MeV
  • Mass of proton is 1.00727663 u which is equal to 1.6725 x 10-27kg or 938.26 MeV.
  • Mass of neutron is 1.0086654 u which is equal to 1.6748 x 10-27kg or 939.55 MeV.

4. Isobars and Isotones

  • Nuclei with same A but different Z are known as Isobars for example 40K19 and 40Ca20 share same mass number 40 but differs in one unit of Z.
  • Although isobaric atoms share same mass number but they differ slightly in their masses.
  • This very slight difference in masses of isobaric atoms is related to difference between energies of two atoms since small mass difference corresponds to considerable amount of difference in energies.
  • Nuclei with same number of neutrons but different number of protons are called Isotones for example 198Hg80 and 198Au79

5. Size of nucleus

  • First estimate of size of nucleus was provided by Rutherford scattering experiment.
  • In Rutherford�s scattering experiment incident alpha particles gets deflected by the target nucleus as long as the distance approached by the alpha particles does not exceeds 10-14m and Coulomb�s law remains consistent.
  • Apart from Rutherford�s scattering experiment various other experiments like fast electrons and neutron scattering experiments were performed to determine the nuclear dimensions.
  • Since electrons interact with nucleus only through electric forces so electron scattering experiments gives information on distribution of charge in the nucleus.
  • A neutron interacts with nucleus through nuclear forces so neutron scattering provides information on distribution of nuclear matter.
  • It was found that the volume of a nucleus is directly proportional to the number of nucleons it contains which is its mass number A.
  • If R is the nuclear radius then relationship between R and A is given as
    Where value of R0 ≅ 1.2 x 10-15 ≅ 1.2 fm and is known as nuclear radius parameter.
  • Since R3 is proportional to A this implies that density of nucleas (ρ = m/V) is a constant independent of A for all nuclei.
  • The density of nuclear matter is approximately of the order of !17 Kg/m3 and is very large compared to the density of ordinary matter.

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