Introduction to Atoms       CHAPTER 4       SECTION 1
History of Atom All atoms share the same basic structure During past 200 years, scientists have proposed  different mode...
Dalton’s Model Based on experiments, Dalton developed a theory  of structure of matter 4 main concepts:    All matter i...
Dalton’s Model
Thomson’s Model End of 1800s Thomson discovered that atoms were not  simple, solid spheres Atoms contained subatomic pa...
Discovery of the ElectronIn 1897, J.J. Thomson used a cathode raytube to deduce the presence of a negativelycharged partic...
Modern Cathode Ray Tubes     Television       Computer MonitorCathode ray tubes pass electricitythrough a gas that is con...
Thomson’s Model Also knew that atoms were electrically neutral   Must contain enough positive charge to balance negative...
Thomson’s Model
Rutherford’s Model By early 1900s, scientists knew that positive charge  of atom comes from subatomic particles called  p...
Rutherford’s Model Rutherford’s model describes an atom as mostly empty space, with a center nucleus that contains nearly...
Bohr’s Model Modified Rutherford’s model in 1913 Proposed that each electron has a certain amount of energy    Helped e...
Bohr’s Model Has been called planetary model   Energy levels occupied by electrons are like orbits of planets at    diff...
Electron Cloud Model Model accepted today Electrons dart around in an energy level Rapid, random motion creates a “clou...
Electron Cloud Model
Findings Eugen Goldstein in 1886 observed  what is now called the “proton” -  particles with a positive charge, and  a re...
Atomic Number Atoms are composed of identical protons, neutrons, and electrons  How then are atoms of one element differ...
Atomic NumberAtomic number (Z) of an element isthe number of protons in the nucleusof each atom of that element.   Element...
Mass NumberMass number is the number ofprotons and neutrons in the nucleusof an isotope: Mass # = p+ + n0Nuclide          ...
The Complete Set-UP  Contain the symbol of the   element, the mass number and the   atomic number.Superscript →          ...
IsotopesDalton was wrong about all elements of the same type being identicalAtoms of the same element can have different...
Isotopes Frederick Soddy (1877-1956) proposed the idea of isotopes in 1912 Isotopes are atoms of the same element having...
Naming IsotopesWe can also put the massnumber after the name of theelement:carbon-12carbon-14uranium-235
Isotopes are atoms of the same element havingdifferent masses, due to varying numbers ofneutrons.  Isotope     Protons Ele...
IsotopesElementsoccur innature asmixtures ofisotopes.Isotopes areatoms of thesame elementthat differ inthe number ofneutro...
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  1. 1. Introduction to Atoms CHAPTER 4 SECTION 1
  2. 2. History of Atom All atoms share the same basic structure During past 200 years, scientists have proposed different models. An atom is the smallest particle of an element. Atomic theory grew as a series of models that developed from experimental evidence. As more evidence was collected, the theory and models were revised.
  3. 3. Dalton’s Model Based on experiments, Dalton developed a theory of structure of matter 4 main concepts:  All matter is composed of tiny, indivisible particles called atoms  Atoms of each element are exactly alike  Atoms of different elements have different masses  Atoms of different elements can join to form compounds
  4. 4. Dalton’s Model
  5. 5. Thomson’s Model End of 1800s Thomson discovered that atoms were not simple, solid spheres Atoms contained subatomic particles  Very small, negatively charged  Called them electrons
  6. 6. Discovery of the ElectronIn 1897, J.J. Thomson used a cathode raytube to deduce the presence of a negativelycharged particle: the electron
  7. 7. Modern Cathode Ray Tubes Television Computer MonitorCathode ray tubes pass electricitythrough a gas that is contained at avery low pressure.
  8. 8. Thomson’s Model Also knew that atoms were electrically neutral  Must contain enough positive charge to balance negative charge of electrons Developed model where electrons were stuck into a positively charged sphere  Like chocolate chips in cookie dough
  9. 9. Thomson’s Model
  10. 10. Rutherford’s Model By early 1900s, scientists knew that positive charge of atom comes from subatomic particles called protons A proton is a positive charged particle in the nucleus of an atom. 1911—Rutherford begins to test theory His experiments led him to believe that protons are concentrated in a small area at center of atom  Called this area the nucleus
  11. 11. Rutherford’s Model Rutherford’s model describes an atom as mostly empty space, with a center nucleus that contains nearly all the mass  Like the pit in a peach
  12. 12. Bohr’s Model Modified Rutherford’s model in 1913 Proposed that each electron has a certain amount of energy  Helped electron move around nucleus Electrons move around nucleus in region called energy levels The energy level is the specific amount of energy an electron has. Energy levels surround nucleus in rings, like layers of onion
  13. 13. Bohr’s Model Has been called planetary model  Energy levels occupied by electrons are like orbits of planets at different distances from the sun (nucleus)
  14. 14. Electron Cloud Model Model accepted today Electrons dart around in an energy level Rapid, random motion creates a “cloud” of negative charge around nucleus Electron cloud gives atom its size and shape
  15. 15. Electron Cloud Model
  16. 16. Findings Eugen Goldstein in 1886 observed what is now called the “proton” - particles with a positive charge, and a relative mass of 1 (or 1840 times that of an electron) 1932 – James Chadwick confirmed the existence of the “neutron” – a particle with no charge, but a mass nearly equal to a proton
  17. 17. Atomic Number Atoms are composed of identical protons, neutrons, and electrons  How then are atoms of one element different from another element? Elements are different because they contain different numbers of PROTONS The “atomic number” of an element is the number of protons in the nucleus # protons in an atom = # electrons
  18. 18. Atomic NumberAtomic number (Z) of an element isthe number of protons in the nucleusof each atom of that element. Element # of protons Atomic # (Z) Carbon 6 6 Phosphorus 15 15 Gold 79 79
  19. 19. Mass NumberMass number is the number ofprotons and neutrons in the nucleusof an isotope: Mass # = p+ + n0Nuclide p+ n0 e- Mass #Oxygen - 18 8 10 8 18Arsenic - 75 33 42 33 75Phosphorus - 31 15 16 15 31
  20. 20. The Complete Set-UP  Contain the symbol of the element, the mass number and the atomic number.Superscript → Mass numberSubscript → Atomic number X
  21. 21. IsotopesDalton was wrong about all elements of the same type being identicalAtoms of the same element can have different numbers of neutrons.Thus, different mass numbers.These are called isotopes.
  22. 22. Isotopes Frederick Soddy (1877-1956) proposed the idea of isotopes in 1912 Isotopes are atoms of the same element having different masses, due to varying numbers of neutrons. Soddy won the Nobel Prize in Chemistry in 1921 for his work with isotopes and radioactive materials.
  23. 23. Naming IsotopesWe can also put the massnumber after the name of theelement:carbon-12carbon-14uranium-235
  24. 24. Isotopes are atoms of the same element havingdifferent masses, due to varying numbers ofneutrons. Isotope Protons Electrons Neutrons NucleusHydrogen–1 (protium) 1 1 0Hydrogen-2(deuterium) 1 1 1Hydrogen-3 1 1 2 (tritium)
  25. 25. IsotopesElementsoccur innature asmixtures ofisotopes.Isotopes areatoms of thesame elementthat differ inthe number ofneutrons.
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