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The Quantum Model : Part II

The Quantum Model : Part II. Electron Configurations. Quantum Numbers. Describe the properties of atomic orbitals and the electrons that occupy them… Quantum Number Describes Principle - main E. level Angular Momentum - shape of Orbital Magnetic - orientation of orbital

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The Quantum Model : Part II

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  1. The Quantum Model : Part II Electron Configurations

  2. Quantum Numbers • Describe the properties of atomic orbitals and the electrons that occupy them… Quantum NumberDescribes • Principle - main E. level • Angular Momentum - shape of Orbital • Magnetic - orientation of orbital • Spin - orientation of electron

  3. Principal Quantum Number (PQN) • Main energy level • Distance from nucleus • “shell” • Always whole positive integers

  4. Angular Momentum Quantum Number (orbital) • Shape of the orbital • Sublevel within the main energy level

  5. s orbitals p orbitals d orbitals

  6. Magnetic Quantum Number • Orientation of orbital (X, Y, Z) • Has to do with the relation to the x-y-z axes

  7. s Orbitals have only one possible orientation.

  8. P Obitals have 3 possible orientations

  9. d Orbitals Have 5 Orientations

  10. How many orientations do you think f orbitals have?

  11. SPIN QUANTUM NUMBER • The orientation of the electron in the orbital. • “Direction of its spin”. • +1/2 or -1/2

  12. Atomic Orbitals and Quantum Numbers Use your notes to make a chart showing important information about each of the four quantum numbers. Make chart for only n=1,2,3,4 • Principal Quantum Number • Angular Momentum Quantum Number • Magnetic Quantum Number • Spin Quantum Number

  13. HOMEWORK • Read pages 143 – 146 • Answer questions #2-4 on page 146 • Study for Quiz #2 next class

  14. Your Chart Should look like this

  15. Electron Configuration • Show the placement of electrons in specific levels, sublevels and orbitals. • Make use of the four quantum numbers and a few simple rules. • Each orbital can only hold a maximum of 2 electrons • Before we learn the rules lets look at a few examples!

  16. Types of notation • Orbital diagram • Arrows represent electrons and direction of spin. • Which element is this? How many electrons?

  17. Rule # 1 : Aufbau Principle • An electron occupies the lowest energy orbital that can receive it…(like filling a glass) • n= 1, n= 2, n=3 represent main energy level.

  18. Organize the levels and sublevels • Main energy level, 1, 2, 3 etc.) • How many sublevels exist at each main energy level? • What are the sublevels at each main energy level? 1__ 2__ 2__ 3__ 3__ 3__ 4__ 4__ 4__ 4__ 5__ 5__ 5__ 5__ 5__

  19. Organize the levels and sublevels • Principle Quantum Number (main energy level) ↓ 1s 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p 5d 5f 5g

  20. How do we remember which sublevel to fill first? • Memory Aid Diagram

  21. Rule # 2 : Pauli exclusion principle • No two electrons in the same atom can have the same set of four quantum numbers…or… • If two electrons occupy the same orbital they must have opposite spins! He ↑ ↓ opposite spins shown by arrow. 1S

  22. Rule # 3 : Hund’s Rule • Orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron. Correct Wrong

  23. Electron configuration notation 1S2 2S2 2P2 What does each character represent? Which element is this?

  24. The Three Little Rules! • An electron occupies the lowest energy orbital that can receive it…(like filling a glass) • If two electrons occupy the same orbital they must have opposite spins! • Orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron.

  25. Homework • Read pg 147 – 153 • Questions: pg 156 #6 • pg 157 #20,22,23,27,28 • Quiz Wed 12/3 • Spectroscope and Flame Lab due 12/3

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