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2. Principle quantum number Depends on energy level n=(1,2,3, …)

3. Azimuthal quantum number Shape of orbital-depends on location on periodic chart If s block then l=0 If p block then l=1 If d block then l=2 If f block then l=3

4. Atomic Orbitals 1 – s 3 - p 5 – d 7 - f

5. Atomic Orbitals d - orbitals l ranges from 0 to n-1. If n=1, then l=0 If n=2 then l=0,1 If n=3 then l= 0, 1, 2

6. Angular Quantum Number m l represents the individual orbitals of a given type. m l ranges from –l to +l m l tells you which p, d, or f orbital the electron is in

7. Magnetic Quantum Number (m s ): Spin

9. QuantumNumbers

10. n = integer from 1 to 7 l = 0 to n-1 m l = -l to +l m s =

11. HOW DO WE DESCRIBE THE LOCATION OF EACH ELECTRON IN AN ATOM? WITH A SYMBOLIC NOTATION CALLED AN ELECTRON CONFIGURATION.

12. An Electron Configuration is a shorthand method of listing the location of the electrons in an atom. The system locates each electron by energy level and sublevel. The number of electrons in each sublevel is indicated with a superscript. For instance, the electronic configuration of Sodium is 1s 2 2s 2 2p 6 3s 1. This indicates that there are two electrons located in the 1s orbital, two electrons in the 2s orbital, six electrons in the 2p orbital and a single electron in the 3s orbital.

13. Remember:

14. Filling Orbitals Follow rules of modern atomic model: Aufbau Principle -electrons fill from lowest energy level first Hund’s Rule -have maximum number of unpaired electrons Pauli Exclusion Theory -no electron has same set of quantum numbers because of electron spin

15. 1. Electrons occupy lowest energy orbitals first. 2. An orbital can hold a maximum of 2 electrons. The Pauli Exclusion Principle must be obeyed. 3. Hund's Rule must be obeyed; when placing electrons into degenerate orbitals, there must be one electron in each orbital before any pairing of electrons can take place. {Degenerate orbitals are orbitals of the same energy level and sublevel.} RULES FOR PLACING ELECTRONS IN ORBITALS

16. Aufbau Diagram

17. The Order Electrons Fill Orbitals

19. __ 5s 4d 5p 6s __ 1s2s 2p 3s 3p __ 4s 3d 4p

20. Electron Configuration of Zr 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 2

21. Practice Write the electron configuration of the following on a separate page. –Oxygen –Lithium –Iron –Bromine –Tin

22. Core Notation of Sn Locate Sn on the periodic table

23. Electron Configuration of Sn Sn [Kr] The noble gas core is Kr

24. Sn [Kr]5s 2 The noble gas core is Kr From Kr, go 2 spaces across the s-block in the 5th row  5s 2

25. Sn [Kr]5s 2 4d 10 5p 2 The noble gas core is Kr From Kr, go 2 spaces across the s-block in the 5th row  5s 2 Then go 10 spaces across the d-block on the 5th row  4d 10 Finally go 2 spaces into the p-block on the 5th row  5p 2

26. Steps Locate the element Go to the end of the row and up 1 noble gas Write the Noble gas core in brackets Continue electron configuration with the next period

27. Refer to a periodic table and write the electron configurations of these atoms. Use the noble gas core. Zn I Nobel Gas (Core) & Orbital Diagram [Ar]4s 2 3d 10 [Kr]5s 2 4d 10 5p 5

28.  4s 3d  5s4d   5p  Zn [Ar]4s 2 3d 10 I [Kr]5s 2 4d 10 5p 5

29. Quiz - Quantum Numbers 1.Zn 2.Sb 3.Cs 4..n = 4.l = 3.ml = -3.ms = -1/2.n = 3.l = 2.ml = +2.ms = -1/2. n = 5.l = 1.ml = +1.ms = + 1/2.n = 6.l = 0.ml = 0.ms = +1/2 Tb

31. The Periodic Table Is a table that arranges the elements according to similarities in their properties.

32. Dmitri Mendeleev Father of the Periodic Table

33. Mendeleev’s Periodic Table (63 known elements) Developed the Periodic Law that said: - columns arranged by increasing atomic mass (not correct) - rows arranged by chem. & physical properties

34. Mendeleev’s Table (cont.) Concluded gaps in table were elements yet to be discovered. - led to the search for missing elements - predicted existence of aluminum, boron, silicon, germanium

35. Predicted Properties Observed Properties Atomic weight 7272.61 Density 5.5 g/cm 3 5.32 g/cm 3 Melting point 825  C938  C Oxide formula RO 2 GeO 2 Density of oxide 4.7 g/cm 3 4.70 g/cm 3 Chloride formula RCl 4 GeCl 4

36. Mendeleev’s Original Table

37. Modern Periodic Table - Developed by Henry Moseley - Solved problems in Mendeleev’s table. - Periodic law is based on increasing atomic #, NOT atomic mass.

38. Structure of the Periodic Table periods: rows going across, numbered 1-7 groups: columns going down, numbered 1-18; aka families - Elements w/in groups have similar physical and chemical properties.

40. The Metals located left of zig-zag or stair-step Properties - good conductors - lusterous - malleable - ductile

41. The Nonmetals located right of zig-zag or stair- step Properties: dull; brittle; poor conductors,

42. The Metalloids Border zig-zag / stair-step except aluminum and polonium Properties: - some metallic - some nonmetallic - semi-conductors

43. Transition Metals Inner Transition Metals 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 IA IIA IIIA IVA VA VIA VIIA VIIIA Representative Elements

44. Transition Metals Inner Transition Metals Elements: Alkali Metals Halogens Lanthanides Metals Nonmetals Metalloids Transition Metals Inner Transition Groups/Families: Alkali Earth MetalsNoble Gases Actinides nonmetalsmetals

45. Key Terms Atomic radius – ½ distance btwn nuclei of two atoms in a molecule. Ionization energy – amt. of energy needed to remove an e - from an atom. Electronegativity – tendency for an atom to attract e - Valence e - - e - on outermost energy level.

46. 1 valence electron 2 valence electrons 3 valence electrons 4 valence electrons 5 valence electrons 6 valence electrons 7 valence electrons 8 valence electrons Electrons in the outermost level are called valence electrons.

47. Element Families Group 1) Alkali Metals (I A) - highly reactive, especially with water - 1 valence e - - loses valence e - - become 1 + ions Li, Na, K, Rb, Cs, Fr

48. Group 2) Alkaline Earth Metals (II A) - very reactive but less than group 1 - 2 valence e - - lose valence e - ’s - become 2 + ions Be, Mg, Ca, Sr, Ba, Ra

49. Groups 3-12) Transition Metals (B) - most have 2 valence e -, some with 1 or more - all lose valence e - - several become 2 + ions ScTiVCrMnFeCoNiCuZn YZrNbMoTcRuRhPdAgCd LuHfTaWReOsIrPtAuHg LrRfDbSgBhHsMt 3 4 5 6 7 8 9 10 11 12

50. Group 17) Halogens (VII A) - highly reactive - form cmpds called halides - fluorine most reactive element - 7 valence e - - Gain 1 e - - become 1 - ions F, Cl, Br, I, At

51. Group 18) Noble Gases (VIII A) - not reactive (inert) - cmpds formed only under special conditions - full outer energy level (8 valence e - ) except He, 2 valence e - He, Ne, Ar, Kr, Xe, Rn

52. Other Groups/Families Group 13: 3 valence e - (IIIA) 14: 4 valence e - (IVA) 15: 5 valence e - (V A) 16: 6 valence e - (VI A)

54. Periodic Trends Atomic Radius INCREASE I N C R E A S E S

55. Atomic Radii

56. Ionization Energy

57. Periodic Trends Ionization Energy INCREASES I N C R E A S E S

58. Ionization Energy

59. Periodic Trends Electronegativity OMITOMIT INCREASES I N C R E A S E S

60. Electronegativity

62. Ion Radius