Atoms <br />Concepts Behind Atoms<br />
Daltons Atomic Theory<br />All matter is composed of extremely small particles called atoms<br />All atoms of a particular...
Atoms of different elements combine with each other in certain whole-number proportion to form a compound.<br />In a chemi...
Law of Conservation of Mass<br />In a chemical reaction, matter is neither created nor destroyed, or, more accurately stat...
Law of Definite Proportions<br />The different samples of any pure compound contains the same proportions by mass.<br />
Law of Multiple Proportions<br />The masses of an element that can be combine with a fixed mass are in a ratio of small nu...
Models of the Atoms<br />
Thompson’s Model<br />The Plum-Pudding Model<br /> Atom were composed primarily  of very positively charged blob. Embedded...
Ruther Ford Model<br />Gold Foil Experiment <br />Alpha Scattering Experiment<br />
Nuclear Model<br />Rutherford’s gold foil experiment proved that most of the atom’s mass is found in very small volume cal...
Bohr’s Model<br />Planetary Model<br />Electrons has several possible orbits at different distances from the nucleus and t...
Radioactivity<br />A property exhibited by substances that undergoes spontaneous emission of high energy radiation from nu...
Assignment <br />James Chadwick<br />Ernest Rutherford<br />Anton Lavoisier <br />Moseley<br />J.J. Thompson<br />Dalton<b...
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Atoms

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Atoms

  1. 1. Atoms <br />Concepts Behind Atoms<br />
  2. 2. Daltons Atomic Theory<br />All matter is composed of extremely small particles called atoms<br />All atoms of a particular element are identical, but the atoms of one element differ from the atom of each other.<br />
  3. 3. Atoms of different elements combine with each other in certain whole-number proportion to form a compound.<br />In a chemical reaction, atoms are rearranged to form new compounds; they are not created, destroyed, or change into atoms of any elements<br />
  4. 4. Law of Conservation of Mass<br />In a chemical reaction, matter is neither created nor destroyed, or, more accurately stated: there is no detectable change in mass during an ordinary chemical reaction <br />
  5. 5. Law of Definite Proportions<br />The different samples of any pure compound contains the same proportions by mass.<br />
  6. 6. Law of Multiple Proportions<br />The masses of an element that can be combine with a fixed mass are in a ratio of small numbers.<br />
  7. 7. Models of the Atoms<br />
  8. 8. Thompson’s Model<br />The Plum-Pudding Model<br /> Atom were composed primarily of very positively charged blob. Embedded on the blob were negatively charged electrons.<br />
  9. 9. Ruther Ford Model<br />Gold Foil Experiment <br />Alpha Scattering Experiment<br />
  10. 10. Nuclear Model<br />Rutherford’s gold foil experiment proved that most of the atom’s mass is found in very small volume called the nucleus.<br />
  11. 11. Bohr’s Model<br />Planetary Model<br />Electrons has several possible orbits at different distances from the nucleus and that electron had to be in one specific orbit or another, but this could not exist between orbits. <br />
  12. 12. Radioactivity<br />A property exhibited by substances that undergoes spontaneous emission of high energy radiation from nucleus of an unstable atom. <br />
  13. 13. Assignment <br />James Chadwick<br />Ernest Rutherford<br />Anton Lavoisier <br />Moseley<br />J.J. Thompson<br />Dalton<br />Antoine Henri Becquerel<br />

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