1. The easy way to keep tracks of electrons!

2.  Pick up your paperwork  Pick up two handouts  Get out Electron Configuration Notes, your Blank Periodic Table, and your green periodic table.

3. Aufbau Principle  Each electron occupies the lowest energy orbital available. Electrons are added from the ground state up. Electrons fill in increasing energy order. Pauli Exclusion Principle  Each orbital can hold a maximum of only two electrons – one spinning clockwise and one spinning counter clockwise. Hund’s Rule  The most stable arrangement of electrons in orbitals is to fill singly and then go back and double up.

4.  Use this to help determine the different blocks: s, p, d, f

7.  Includes the principle quantum number, the sublevel and the number of electrons in the sublevel.

8. HydrogenH11s 1 HeliumHe21s 2 LithiumLi31s 2 2s 1 BerylliumBe41s 2 2s 2 BoronB51s 2 2s 2 2p 1 CarbonC61s 2 2s 2 2p 2 NitrogenN71s 2 2s 2 2p 3 OxygenO81s 2 2s 2 2p 4 FluorineF91s 2 2s 2 2p 5 NeonNe101s 2 2s 2 2p 6

9. SodiumNa111s 2 2s 2 2p 6 3s 1 MagnesiumMg121s 2 2s 2 2p 6 3s 2 AluminumAl131s 2 2s 2 2p 6 3s 2 3p 1 SiliconSi141s 2 2s 2 2p 6 3s 2 3p 2 PhosphorusP151s 2 2s 2 2p 6 3s 2 3p 3 SulfurS161s 2 2s 2 2p 6 3s 2 3p 4 ChlorineCl171s 2 2s 2 2p 6 3s 2 3p 5 ArgonAr181s 2 2s 2 2p 6 3s 2 3p 6 PotassiumK191s 2 2s 2 2p 6 3s 2 3p 6 4s 1 CalciumCa201s 2 2s 2 2p 6 3s 2 3p 6 4s 2

10.  First determine atomic number  Then determine the electron configuration.

11.  Pick up handout  Bright Line Spectra lab due tomorrow  2 nd period paperwork revisions due tomorrow.  5 th period paperwork revisions due Friday.  Get out Electron Configuration Notes, your Blank Periodic Table, and your green periodic table.

12. CarbonC61s 2 2s 2 2p 2 SodiumNa111s 2 2s 2 2p 6 3s 1 PhosphorusP151s 2 2s 2 2p 6 3s 2 3p 3 ArgonAr181s 2 2s 2 2p 6 3s 2 3p 6 SulfurS161s 2 2s 2 2p 6 3s 2 3p 4 NeonNe101s 2 2s 2 2p 6 AluminumAl131s 2 2s 2 2p 6 3s 2 3p 1

14. 1s 2s2p 3s3p3d 4s4p4d4f 5s5p5d5f 6s6p6d6f 7s7p7d

18. 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 5p 6 6s 2 4f 14 5d 10 6p 3

19. 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 5p 6 6s 2 4f 14 5d 10

20.  You must memorize only:  Chromium, molybdenum, tungsten  Copper, silver,  Lots of the “f” level elements  6d fills correctly; most f block elements do not fill according to the rulesd.

23.  On a piece of paper see if you can do the electron configurations for:  Tantalum (Z = 73)  Curium (Z=96)

24. Tantalum: 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 5p 6 6s 2 4f 14 5d 3 Curium: 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 5p 6 6s 2 4f 14 5d 10 6p 6 7s 2 5f 8

25.  Turn in Bright Line Spectra lab  Turn in any revised paperwork  Pick up both handouts  Get out Electron Configuration notes

26.  Charged particles  ANION – atom that has gained electrons and is more negative  CATION – atom that has lost electrons and is more positive.  So if the number of electrons has changed, then the electron configuration has changed.

27.  First, write the regular electron configuration for the element.  If the ion is positive, take away electrons. If the ion is negative, add electrons to the highest partially filled energy level. EXAMPLES: Na 1s 2 2s 2 2p 6 3s 1 Al1s 2 2s 2 2p 6 3s 2 3p 1 Na +1 1s 2 2s 2 2p 6 Al +3 1s 2 2s 2 2p 6 F1s 2 2s 2 2p 5 H1s 1 F -1 1s 2 2s 2 2p 6 H -1 1s 2

28. Magnesium Oxygen 12 Mg 1s 2 2s 2 2p 6 3s 2 8 O1s 2 2s 2 2p 4 12 Mg +2 1s 2 2s 2 2p 6 8 O -2 1s 2 2s 2 2p 6 Lithium Iron 3 Li1s 2 2s 1 26 Fe1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 6 3 Li +1 1s 2 26 Fe +3 1s 2 2s 2 2p 6 3s 2 3p 6 4s 0 3d 5

29. Atoms that have absorbed energy and are in an excited state have electrons that have moved to a shell level that is higher than what is normal. The electrons that move come from the valence electrons (outermost electrons).

31.  Another way to symbolize electrons in their energy levels and sublevels.  Has three basic symbols: unoccupied orbital with orbital with orbital one electron two electrons

32. Pauli Exclusion Principle  Each orbital can hold a maximum of only two electrons – one spinning clockwise and one spinning counter clockwise. Hund’s Rule  The most stable arrangement of electrons in orbitals is to fill singly and then go back and double up.

35. Do the orbital diagrams for: SODIUMSULFUR

36. Cannot be used until after the test on Atomic Theory. Start with the noble gas the occurs before the element in question. Then tack on the remaining electron configuration. Example: Sodium 1s 2 2s 2 2p 6 3s 1 Shorthand: [Ne] 3s 1 Copper 1s 2 2s 2 2p 6 3s 2 3p 6 4s 1 3d 10 Shorthand: [Ar] 4s 1 3d 10

38. Calcium 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 shorthand: [Ar]4s 2 Oxygen 1s 2 2s 2 2p 4 shorthand: [He]2s 2 2p 4

39.  These are the electrons in the outermost energy level.  Look for the highest principle quantum number and count all the electrons in that level. Sodium 1s 2 2s 2 2p 6 3s 1 Shorthand: [Ne] 3s 1 valence electrons: 1

40. Copper 1s 2 2s 2 2p 6 3s 2 3p 6 4s 1 3d 10 Shorthand: [Ar] 4s 1 3d 10 valence electrons: 1 Magnesium 1s 2 2s 2 2p 6 3s 2 valence electrons: 2 Chlorine 1s 2 2s 2 2p 6 3s 2 3p 5 valence electrons: 7

42.  The electrons in the outmost level are the ones that are involved in bonding and the ones we really care about (valence electrons).  The symbol stands for the nucleus and all the inner electron energy levels.  Using the electron configuration for the atom, choose the valence electrons.

44. Sodium 1s 2 2s 2 2p 6 3s 1 valence electrons: 1Na Copper 1s 2 2s 2 2p 6 3s 2 3p 6 4s 1 3d 10 valence electrons: 1Cu Magnesium 1s 2 2s 2 2p 6 3s 2 valence electrons: 2Mg Chlorine 1s 2 2s 2 2p 6 3s 2 3p 5 valence electrons: 7Cl

45.  Do electron configuration and orbital diagrams on the front  Do electron configuration and electron dot diagrams on the back side  Lab tomorrow – bring your logbook.