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BELLWORK 10/27/16

BELLWORK 10/27/16. QUANTUM MODEL OF THE ATOM – Day 2 Review. Organizes the electrons into 4 orbitals found on different energy levels. The four orbitals are … .s, p,d, f. ....... The “ s ” orbital can hold a maximum of ____ 2 electrons.

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BELLWORK 10/27/16

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  1. BELLWORK 10/27/16

  2. QUANTUM MODEL OF THE ATOM – Day 2 Review • Organizes the electrons into 4 orbitals found on different energy levels. • The four orbitals are….s, p,d, f........ • The “s” orbital can hold a maximum of ____ 2 electrons. • The “p” orbital is made up of _3___ sub-orbitals, and each one holds _2____ electrons. • Which orbital is found on the 1st energy level? “s” 2nd? “s” and “p”

  3. Electron Configuration • Gives a detailed description of where the electrons in an atom are located. • Ex: Show where all of the electrons in Al are located within the Aluminum atom.

  4. Rules for Writing Electron Configurations • Aufbau Principle- electrons enter the lowest energy level first. All orbitals have to be filled before electrons can be placed in the next energy level

  5. 7p 6d 5f 7s 6p 5d 6s 4f 5p 4d 5s 4p 3d 4s 3p Increasing energy 3s 2p 2s 1s Aufbau Principle – the electrons fill the lowest energy levels first. Ex: Show the location of the electrons in the neutral atom. Al13

  6. Rules for Writing Electron Configurations • Hund’s Rule – Each suborbital within an orbital is filled with one electron before the 2nd electron is added.

  7. 7p 6d 5f 7s 6p 5d 6s 4f 5p 4d 5s 4p 3d 4s 3p Increasing energy 3s 2p 2s 1s • Hunds Rule – one electron is placed in each orbital before the second electron is placed into the orbital Ex: Which element does this electron configuration represent?

  8. Rules for Writing Electron Configurations • Pauli Exclusion Principle - Electrons within the same orbital must have opposite spins.

  9. 7p 6d 5f 7s 6p 5d 6s 4f 5p 4d 5s 4p 3d 4s 3p Increasing energy 3s 2p 2s 1s • Pauli Exclusion Principle – Electrons within the same suborbital must have opposite spins.

  10. We use the Periodic Table to determine the order in which the electrons fill the orbitals. Read the periodic table from left to right beginning with the 1st energy level (Period 1)

  11. HOW MANY ELECTRONS CAN A “D” ORBITAL HOLD?

  12. CHECKPOINT

  13. PRACTICE PROBLEM #1 • Write the electron configuration and the orbital notation for He.

  14. 7p 6d 5f 7s 6p 5d 6s 4f 5p 4d 5s 4p 3d 4s 3p Increasing energy 3s 2p 2s 1s The 1s orbital is filled first. (Aufbau Principle) Notice the 2 electrons have opposite spins (Pauli Exclusion)

  15. Helium • 1s2

  16. Practice Problem #2 • Write the electron configuration and the orbital notation for Boron.

  17. 7p 6d 5f 7s 6p 5d 6s 4f 5p 4d 5s 4p 3d 4s 3p Increasing energy 3s 2p 2s 1s The 1s orbital is filled first. (Aufbau Principle) Notice the 2 electrons have opposite spins (Pauli Exclusion)

  18. Boron - 1s22s22p1

  19. Practice Problem #3 • Write the electron configuration and orbital notation for silicon.

  20. Silicon – 1s22s22p63s23p2

  21. Practice Problem #4 • Write the electron configuration and the orbital notation for Manganese.

  22. 7p 6d 5f 7s 6p 5d 6s 4f 5p 4d 5s 4p 3d 4s 3p Increasing energy 3s 2p 2s 1s • Hunds Rule – one electron is placed in each orbital before the second electron is placed into the orbital

  23. Manganese – 1s22s22p63s23p64s23d5

  24. AGENDA • Finish working in your cooperative groups on you inquiry packet.

  25. EXIT TICKET • Why do you fill the 3d orbital before the 4p?

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