1. Atomic Models

2. Bell Work  Describe the Plum Pudding Model in at least 3 sentences.

3. OBJECTIVES:  COMPARE THE RUTHERFORD,BOHR, AND CURRENT MODEL OF AN ATOM.  LIST THE 4 QUANTUM NUMBERS AND UNDERSTAND THEIR IMPORTANCE

4. ATOMIC MODELS Why did scientists come up with atomic models? After the atomic theory became widely accepted, scientist came up with models that illustrated these concepts. Building models helps us understand what is happening at the microscopic level.

5. What is the Rutherford model?  Electrons revolve around the nucleus in circular orbits.  Replaced the Plum pudding model.  Could not explain why electrons did not crash into the nucleus.

6. What is the Bohr model?  Electrons can be only certain distances from the nucleus.  Electrons travel around the nucleus in energy levels.  Electrons can move from lower energy levels to higher energy levels.  Electrons can only be in one energy level at a time.

7. What is the Current/Quantum Model?  Electrons act like particles and waves.  Electrons are located in orbitals and travel around the nucleus.  Orbitals/Electron Clouds are regions where electrons are likely to be found.

8. Group Activity: Rubric 100%  Create an Organized Colorful Poster of the 3 Atomic Models discussed today.  Creativity, Correct Information, and Neatness should be used.  At least 4 important facts about each model.  All group members need to participate in the creation and presentation of the poster.

9. CONCEPT MAPS ATOMIC MODELS RUTHERFORDBOHRCURRENT

10. RUTHERFORD CURRENT/QUANTUM MODEL BOHR VENN DIAGRAM

11. BUBBLE DIAGRAM MODEL NAME

12. Circle the Atomic Model that is Incorrect Rutherford - Nucleus at the center; electrons orbit nucleus. Plum Pudding - Positive & Negative charge imbedded throughout the atom. Quantum Mechanical - Ground State; energy levels.

13. What is light?  Light can be described as a stream of particles that moves in waves.  Light waves travel at 3.00 x 10 8 m/s

14. What is a wavelength?  The distance between two consecutive peaks or troughs of a wave.  The wavelengths of light can range from 10 5 m to less than 10 -13 m.(Electromagnetic Spectrum)

15. What is the electromagnetic Spectrum?  Broad range of wavelengths of light.  From gamma rays to radio waves.  Visible spectrum is a part of the electromagnetic spectrum.

16. What is the visible spectrum?  The area of the electromagnetic spectrum that our eyes are sensitive to.  Acronym for the Visible Spectrum ROYGBIV Red Orange Yellow Green Blue Indigo Violet Page 92 of Holt Chemistry Text

18. What are electron Configurations?  A written arrangement of electrons in an atom.  Shorthand notation of where the electrons are in an atom.  Electrons in an atom tend to have arrangements that have the lowest possible energies.

19. What are Quantum numbers?  A number that specifies the region in which electrons can be found.  The number can be a 1, 2, 3,or 4.  Each quantum number can have orbitals  There are s- oribitals, p-orbitals, d-orbitals, and f-orbitals(rememeber orbitals are where electrons are located)

20. What is the Pauli Exclusion Principle? States that two, but no more than two, electrons can occupy a singe orbital.

21. What is the Aufbau Principle? States that electrons fill orbitals that have the lowest energy first.

22. What is Hund’s Rule? States that the orbitals of the same quantum numbers are each occupied by one electron before any pairing occurs (Electrons are represented by arrows).

23. ELECTRON CONFIGURATION 1s > 2s > 2p > 3s > 3p > 4s >3d

24. Orbitals (Energy of Orbitals)

25. Problem Solving with Electron Configurations:  TURN TO PAGE 99 IN TEXT