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ARRANGEMENT OF ELECTRONS IN ATOMS

ARRANGEMENT OF ELECTRONS IN ATOMS. CHAPTER 4. THE NEW ATOMIC MODEL. FIRST CAME LIGHT BEFORE 1900, THE COMMON THOUGHT WAS THAT LIGHT BEHAVED AS A WAVE. THE ELECTRON BEGAN TO CHANGE THAT IDEA. NOW WE HAVE TWO WAYS TO DESCRIBE LIGHT: A WAVE A PARTICLE. ELECTROMAGNETIC RADIATION.

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ARRANGEMENT OF ELECTRONS IN ATOMS

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  1. ARRANGEMENT OF ELECTRONS IN ATOMS CHAPTER 4

  2. THE NEW ATOMIC MODEL FIRST CAME LIGHT BEFORE 1900, THE COMMON THOUGHT WAS THAT LIGHT BEHAVED AS A WAVE. THE ELECTRON BEGAN TO CHANGE THAT IDEA. NOW WE HAVE TWO WAYS TO DESCRIBE LIGHT: A WAVE A PARTICLE

  3. ELECTROMAGNETIC RADIATION ENERGY THAT EXHIBITS WAVE LIKE BEHAVIOR AS IT TRAVELS THROUGH SPACE ALL FORMS OF ELECTROMAGNETIC RADIATION FORM THE ELECTROMAGNETIC SPECTRUM EMR POSTER…

  4. PROPERTIES OF A WAVE WAVELENGTH FREQUENCY WAVE POSTER…

  5. PHOTOELECTRIC EFFECT THE EMISSION OF ELECTRONS FROM A METAL WHEN LIGHT SHINES ON THE METAL. WHEN ALL LIGHT SHOULD WORK, ONLY A SPECIFIC FREQUENCY DOES.

  6. MAX PLANCK STUDIED THE LIGHT (ENERGY) EMITTED FROM HOT GLOWING OBJECTS. HIS THEORY-LIGHT (ENERGY) IS NOT EMITTED CONTINUOUSLY BUT AS SMALL SPECIFIC PACKETS CALLED QUANTA. A QUANTUM OF ENERGY IS THE MINIMUM QUANTITY OF ENERGY THAT CAN BE LOST OR GAINED BY AN ATOM

  7. EINSTIEN EXPANDED THIS THEORY-ELECTROMAGNETIC RADIATION HAS A DUAL WAVE-PARTICLE NATURE. IT EXHIBITS WAVE LIKE PROPERTIES BUT CAN ALSO BE A STREAM OF PARTICLES. EACH PARTICLE OF LGHT CONTAINS A QUANTUM OF ENERGY. HE CALLED THE PARTICLES PHOTONS.

  8. EMISSION LINE SPECTRUM GROUND STATE: LOWEST ENERGY STATE OF AN ATOM EXCITED STATE: AN ATOM WITH A HIGHER POTENTIAL ENERGY THAN THE GROUND STATE. PASS ELECTRICITY THROUGH A ELEMENT IN THE GAS STATE-LIGHT IS PRODUCED (THOMSON). EACH ELEMENT HAS A CHARACTERISTIC COLOR.

  9. IF THE LIGHT IS PASSED THROUGH A PRISM, THE LIGHT IS SEPARATED INTO INDIVIDUAL COLORS OF LIGHT (VISIBLE LIGHT). THAT IS THE EMISSION LINE SPECTRUM FOR THAT ELEMENT.

  10. BOHR MODEL OF THE ATOM SEE TEXTBOOK… Electrons orbit the nucleus in specific orbits at a specific distance from the nucleus. To move away from the nucleus, the e- must gain energy and move out of that orbit because it no longer “qualifies”, energy wise, to stay in that location. e- cannot exist between orbits.

  11. When e- gain energy and move to the correct orbit (atomic energy level), it is called absorption. The e- cannot remain there. It gives off this energy in the form of a photon as it falls back to its original orbit. This is called emission (emission linespectrum).

  12. The Quantum Model of the AtomLouis De Broglie Louis De Broglie (French) ask the question, could e- have a dual wave/particle nature? His answer revolutionized how we see the atom. Bohr’s explanation of e- behavior was similar to wave behavior. De Broglie said to consider e- to be waves that were confined to Bohr’s orbits. Waves equal frequencies so we could also consider this equaling energy-the quantized energy of each orbit.

  13. All of De Broglie’s theories about e-behaving as waves were proven by experiments that showed diffraction and interference.

  14. Werner Heisenburg Werner Heisenburg (German) proposed that it is impossible to know both the position and velocity of an e- or any other particle (1927-the Heisenburg Uncertainty Principle). e- were being detected by photons since they have the same amount of energy. A photon was fired at an atom in an attempt to find an e-. If the photon hit an e-, it would be deflected and could be “seen”.

  15. Erwin Shrȍdinger Erwin Shrȍdinger (Austrian, 1926) developed an equation based on the idea of the dual nature of e-.

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