S T R U C T U R E O F A T O M

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S T R U C T U R E O F A T O M

  1. 1. STRUCTURE OF ATOM<br />
  2. 2. Outline<br />What is Atom ?<br />The Structure of Atom<br />Thomson’s Model<br />Rutherford’s Model<br />Bohr’s Model of Atom<br />Valency<br />Atomic Number & Mass Number<br />
  3. 3. What is Atom<br />Atom is a basic unit of matter<br />Atom makes one element different from another<br />Atom comes from the Greek word “átomos”, which means uncuttable, or indivisible (Dalton’s Law)<br />
  4. 4. Structure of Atom<br />Discovery of two fundamental particles –<br />Electrons & Protons<br />Protons – Positively Charged ions<br />Electrons – Negatively Charged ions<br />Failure of Dalton’s atomic theory (Atom’s are indivisible)<br />Three models for structure of Atom<br />
  5. 5. Thompson's Model Of An Atom<br />Thompson proposed-<br /> Model of an atom to be similar to that of Christmas pudding. The electrons, in a sphere of positive charge, were like dry fruits in a spherical Christmas pudding.<br />Positive Sphere<br />Electron<br />He thus proposed that-<br />(i) An atom consists of a positively charged sphere and the electrons are embedded in it.<br />(ii) The negative and positive charges of an atom are equal in magnitude. So, the atom as whole is electrically neutral.<br />
  6. 6. Rutherford's Model of an Atom <br />Observation:<br />Conclusion:<br />Experiment: <br />Rutherford selected a gold foil as thinner layer as possible (nearly about 1000 Atoms thick)<br />He selected Alpha particles which are doubly charged HELIUM ion.<br />It was expected that Alpha particles could be deflected by the sub-atomic particles in the gold atoms, as alpha particles were much heavier than proton. He did not expected to see a large deflection.<br />Most of the space inside the atom is empty because most of the alpha particles passed through without getting deflected.<br />Very few particles were deflected from their path indicating that positive charge of the atom occupies very little space.<br />There is positively charged centre in an atom called nucleus in well define orbits. <br />The size of the nucleus is very small as compare to size of atoms.<br />Most of the fast moving alpha particles past straight through the gold foil.<br />Some of the alpha particles were deflected by the foil by small angles.<br />Surprisingly 1 out of every 12000 particles appear to rebound. <br />The gold foil experiment was conducted under the supervision of Rutherford at the University of Manchester in 1909 by scientist Hans Geiger and undergraduate student Ernest Marsden. Rutherford, chair of the Manchester physics department at the time of the experiment, is given primary credit for the experiment, as the theories that resulted are primarily his work. Rutherford's gold foil experiment is also sometimes referred to as the Geiger-Marsden experiment.<br />
  7. 7. Bohr's Model Of Atom<br />Nucleus<br />K shell<br />L Shell<br />M Shell<br />In order to overcome the objection raised against Rutherford’s model of the atom, Neil Bohr put forward the following postulates about the model of the atom- <br />Only certain special orbit known as discrete orbit of an electron, are allowed inside an atom.<br />(ii) While revolving in discrete orbits the electrons do not radiate energy.<br />
  8. 8. Model of Hydrogen Atom<br />Structure of AtomsDistribution of Electrons<br />Model of Atom<br />
  9. 9. Valency<br />Is the Combining Capacity of an Element<br />Determines how the atoms of one element combines with the atoms of another or same element to form a chemical compound<br />Depends on the how the electrons are arranged in the outermost shell<br />Bohr-Bury Scheme – Outermost shell of an atom can accommodate a max of 8 electrons<br />Is either equal to the number of electrons in the outermost shell or number of electrons required to complete 8 electrons in the outermost shell<br />
  10. 10. Valency of Some Elements<br />
  11. 11. ATOMIC NUMBER<br />Atomic number defined as the total number of protons present in the nucleus of an atom. It is denoted by Z.<br />Atomic number of <br /> Carbon is 6 because it has 6 protons in its nucleus.<br />MASS NUMBER<br />Atomic Notation<br />Mass number defined as the sum of total number of protons and nucleons present in the nucleus of an atom. It is denoted by A.<br />Mass number of nitrogen is 14 because it has 7 protons and 7 neutrons in its nucleus.<br />In the notation for an atom, the atomic number, mass number and the symbol of the element are to be written as:<br />Nitrogen atom<br />
  12. 12. THANK YOU<br />

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