#9 Modern Atomic Theory Quantitative Chemistry
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1 Name #9 Modern Atomic Theory Quantitative Chemistry Student Learning Map Unit EQ: What is the current model of the atom? Key Learning: The current model of the atom is based on the quantum mechanical model. UNIT CONCEPT: 1. Background (Light & Energy) 2. Electron Orbitals 3. Electron Configuration How do light and energy provide the background for modern atomic theory? LESSON ESSENTIAL QUESTIONS: What are the various orbitals that hold electrons? How do I draw electron configurations? LESSON ESSENTIAL VOCABULARY: Electromagnetic Radiation Wave Wavelength Photon Orbitals (s, p, d, f) Quantum Numbers: Principal (n) Angular Momentum (l) Magnetic (m l ) Spin (m s ) Orbital Diagram Electron Configuration Noble Gas Configuration 1
2 1. Background (Light & Energy) EQ: How do light and energy provide the background for modern atomic theory? A. Electromagnetic Radiation Definition: Illustration: Different types of electromagnetic radiation have wavelengths (λ). Chart: B. Dual Wave-Particle Nature of Light Wave Particles C. How Atoms Emit Energy (Light) Illustration: Different colors represent which correspond to _. 2
3 1. Background (Light & Energy) cont. D. Quantized Energy Levels Excited hydrogen atoms can emit photons only of certain energies (different wavelengths). They never emit photons with different energies (not 600 nm, 420 nm, etc.). 656 nm = 434 nm = 486 nm = 410 nm = The energy levels are, meaning. Excited States: E. Bohr Model Electrons move in that correspond to the different energy levels. Electrons can jump orbits by. Illustration: 3
4 1. Background (Light & Energy) cont. F. Developing the Quantum Mechanical Model (Scientists) 1. Louis debroglie Erwin Schrödinger Werner Heisenberg Electron Orbitals EQ: What are the various orbitals that hold electrons? Electron Orbital = a 3-D region around an atom that indicates the PROBABLE location of an electron. Orbitals can be described by: 1. Size / Energy Level 2. Shape 3. Orientation The first three quantum numbers are used to designate these features. The fourth quantum number describes the position of electrons inside an orbital. They are mathematically determined. 4
5 2. Electron Orbitals (cont.) The 4 Quantum Numbers 1. Size / Energy Level (Principal Quantum Number n) As n increases, the electron s and from the nucleus increases. Illustration: 2. Shape (Angular Momentum Quantum Number l) s p d 3. Orientation (Magnetic Quantum Number m l ) s p d 4. Spin Quantum Number m s 5
6 2. Electron Orbitals (cont.) Principles/Rules Aufbau Principle An electron occupies the energy orbital it can. Pauli Exclusion Principle No 2 electrons in the same atom can have the same set of. (No 2 electrons can have the in the.) Hund s Rule Orbitals of equal energy are each occupied by before any orbital is occupied by a second electron, and. Chart Orbitals Energy Level Shape Number of Orientations Number of Electrons 3. Electron Configuration EQ: How do I draw electron configurations? 6
7 3. Electron Configuration (cont.) A. Order of Filling Orbitals (3 ways) 1. Chart 2. Diagram (Arrows) 3. Periodic Table 7
8 3. Electron Configuration (cont.) B. Electron Configurations The First Eighteen Elements 1-10 with orbital diagrams 1. Hydrogen 2. Helium 3. Lithium 4. Beryllium 5. Boron 6. Carbon 7. Nitrogen 8. Oxygen 9. Fluorine 10. Neon 8
9 3. Electron Configuration (cont.) Element Complete Electron Configuration Noble Gas Electron Configuration 11. Sodium 12. Magnesium 13. Aluminum 14. Silicon 15. Phosphorus 16. Sulfur 17. Chlorine 18. Argon C. Noble Gas Configurations 2 = 10 = 18 = 36 = 54 = 9
10 3. Electron Configuration (cont.) D. The d Orbitals [Ar] = Element Orbital Diagram Noble Gas Electron Configuration 19. Potassium 4s 3d 4p 20. Calcium 4s 3d 4p 21. Scandium 4s 3d 4p 22. Titanium 4s 3d 4p 23. Vanadium 4s 3d 4p 24. Chromium** 4s 3d 4p 25. Manganese 4s 3d 4p 26. Iron 4s 3d 4p 27. Cobalt 4s 3d 4p 28. Nickel 4s 3d 4p 29. Copper** 4s 3d 4p 30. Zinc 4s 3d 4p 31. Gallium 4s 3d 4p 32. Germanium 4s 3d 4p 33. Arsenic 4s 3d 4p 34. Selenium 4s 3d 4p 35. Bromine 4s 3d 4p 36. Krypton 4s 3d 4p *Exceptions 10
11 3. Electron Configuration (cont.) E. Problems s, p, and d A. Write the complete electron configuration for an atom of the following: 1. N 2. K 3. V 4. I B. Write the noble gas electron configuration for an atom of the following: 1. Mg 2. Br 3. Ag 4. Cs F. The f Orbitals 11
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