Upcoming SlideShare
×

# CP5.2-electrons

725 views

Published on

Published in: Technology, Education
1 Like
Statistics
Notes
• Full Name
Comment goes here.

Are you sure you want to Yes No
• Be the first to comment

Views
Total views
725
On SlideShare
0
From Embeds
0
Number of Embeds
75
Actions
Shares
0
26
0
Likes
1
Embeds 0
No embeds

No notes for slide

### 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