Section 2:Electron Arrangement in Atoms
 Apply the aufbau principle, the Pauli
exclusion principle, and Hund’s Rule to
generate electron configurations and spin
...
 Electron’s address
 Energy level
 Sublevel
 Orbital
 Spin
Need a system for electron addresses...
•Your address
• St...
 Energy levels are numbered(1, 2, 3...)
 Each energy level adds one more sublevel
(letters)
 Each sublevel adds two mor...
 Sublevels addressed by the number of their
energy level and letter of sublevel
◦ Example: 1s, 2s, 2p, 3s, 3p, 3d
 Still...
 Aufbau principle: electrons occupy orbitals
of lowest energy first
 Electrons (like some students) are lazy
 Orbitals ...
 Pauli Exclusion Principle
 Orbital can hold maximum
of two electrons
◦ (Two per seat on the bus)
 If two electrons in ...
 Hunds Rule
 Orbitals in same sublevel are same energy
 Electrons fill orbitals of same energy so they
maximize same sp...
 One electron for every proton
 Periodic table arranged by atomic number
 Typewriter method: start at H, read left to
r...
 Further down the table...
 La starts 4f sublevel
◦ Comes after 6s and before 5d
◦ Lu is actually 5d1
 Ac starts 5f sub...
 There are exceptions to the normal rules for
electron configurations
 Based on stability
 Just know that they exist, n...
 Atom drawn with nucleus in center and one
ring for each energy level
 Electrons drawn as dots on the rings
 Example: S...
 Group electrons by sublevels
 Show spins
 Example: S
 1s2
◦ one ring, 2 arrows paired
 2s2, 2p6
◦ one ring, 2 arrows...
 Apply the aufbau principle, the Pauli
exclusion principle, and Hund’s Rule to
generate electron configurations and spin
...
 Page 135 & 136, 8-13
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CP5.2-electrons

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CP5.2-electrons

  1. 1. Section 2:Electron Arrangement in Atoms
  2. 2.  Apply the aufbau principle, the Pauli exclusion principle, and Hund’s Rule to generate electron configurations and spin diagrams;  Explain that there can be exceptions to the normal rules for electron configurations; and  Draw modified Bohr diagrams for atoms
  3. 3.  Electron’s address  Energy level  Sublevel  Orbital  Spin Need a system for electron addresses... •Your address • State • Town • Street • House
  4. 4.  Energy levels are numbered(1, 2, 3...)  Each energy level adds one more sublevel (letters)  Each sublevel adds two more orbitals Energy Level Sublevels and orbitals 1 s (one orb.) 2 s (one orb.), p (three orbs.) 3 s (one orb.), p (three orbs.), d (five orbs.) 4 s (one orb.), p (three orbs.), d (five orbs.), f (seven orbs.)
  5. 5.  Sublevels addressed by the number of their energy level and letter of sublevel ◦ Example: 1s, 2s, 2p, 3s, 3p, 3d  Still two more parts to address (orbital and spin)...  Electron configuration: arrangement of electrons in an atom in its ground state  Orbital diagram: illustrates arrangement and spin of electrons
  6. 6.  Aufbau principle: electrons occupy orbitals of lowest energy first  Electrons (like some students) are lazy  Orbitals in same sublevel are same energy
  7. 7.  Pauli Exclusion Principle  Orbital can hold maximum of two electrons ◦ (Two per seat on the bus)  If two electrons in an orbital, must be opposite spins  Two possible spins: up and down
  8. 8.  Hunds Rule  Orbitals in same sublevel are same energy  Electrons fill orbitals of same energy so they maximize same spin  Students don’t pair up in a seat until they have to
  9. 9.  One electron for every proton  Periodic table arranged by atomic number  Typewriter method: start at H, read left to right, and stop at the element you’re configuring
  10. 10.  Further down the table...  La starts 4f sublevel ◦ Comes after 6s and before 5d ◦ Lu is actually 5d1  Ac starts 5f sublevel ◦ Comes after 7s and before 6d ◦ Lr is actually 6d1  Try some...
  11. 11.  There are exceptions to the normal rules for electron configurations  Based on stability  Just know that they exist, not how to do them
  12. 12.  Atom drawn with nucleus in center and one ring for each energy level  Electrons drawn as dots on the rings  Example: S  1s2, one ring, 2 dots  2s2, 2p6, one ring, 8 dots  3s2, 3p4, one ring, 6 dots
  13. 13.  Group electrons by sublevels  Show spins  Example: S  1s2 ◦ one ring, 2 arrows paired  2s2, 2p6 ◦ one ring, 2 arrows paired (s), 6 arrows paired (p)  3s2, 3p4 ◦ One ring, two arrows paired (s) four arrows with two paired (p) 16 p 16n
  14. 14.  Apply the aufbau principle, the Pauli exclusion principle, and Hund’s Rule to generate electron configurations and spin diagrams?  Explain that there can be exceptions to the normal rules for electron configurations?  Draw modified Bohr diagrams for atoms?
  15. 15.  Page 135 & 136, 8-13

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