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FACT:

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clarke
83 diapositives · 1.1K Views · Aug 20, 2014

FACT:. Chemical reactions happen because electrons are shared or transferred from one substance to another. Write a mathematical equation that allows us to predict the Max # of electrons if we know the energy level (n). Max # = …n…. Equation to calculate Max # of e -. 2 n 2.

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  1. FACT: Chemical reactions happen because electrons are shared or transferred from one substance to another

  2. Write a mathematical equation that allows us to predict the Max # of electrons if we know the energy level (n) Max # = …n…

  3. Equation to calculate Max # of e- 2n2 Where n is any energy level

  4. There are 4 Quantum #s and those #s are used to describe where an electron is likely to be found at any given time

  5. This is a lot like being able to use four “places” to describe EXACTLY where Mrs. BB-G should be at 7:00AM on Friday.

  6. The Principle Quantum # = n The first number (a.k.a. The Electron Energy level)

  7. Specifies the electron energy level that the electron is on Principle Quantum # n = 1, 2, 3, 4, 5, 6, 7

  8. 1st Principle Quantum #Ex: (Floor number in our school building) 2nd Floor

  9. ℓ = s, p, d, f 2nd Quantum # = ℓ Specifies the shape of the orbital or sub-energy level

  10. 2nd Quantum # Students (sleeping) (s)sitting prone at desk (p)“darn” I have to sit up (d)forget this standing up in class (f) ℓ = s, p, d, f

  11. p d f s

  12. Sub-Energy Levels

  13. 3rd Quantum # = m m = x,y,z 3-d World Like tables arranged at different angles in the classroom

  14. Sub-Energy Levels s,p,d,f

  15. 4th Quantum # = ms ms = + ½or–½ Clockwise or counterclockwise Specifies the electron’s spin – +

  16. QUANTUM NUMBERS n ---> shell 1, 2, 3, 4, ... l ---> subshell s,p,d,f ml ---> orbital x,y,z ( 3-D) ms ---> electron spin

  17. PERIODIC TABLE review

  18. Periods and Groups

  19. PERIODS • The number of each period shows the principal energy level

  20. 1 2 3 4 5 6 7 Lanthanide 4f Actinide 5f

  21. PERIODS • Horizontal rows of the table are called periods or rows.

  22. GROUPS • The vertical columns of the Periodic Table are called groups or families.

  23. lA 0 1 lllA lVA VA VIA VlIA llA 2 3 lllB lVB VB VlB VllB VlllB lB llB 4 5 6 7

  24. Groups At F O N Home 18 1 Diatomic Elements H2 N2 O2F2Cl2Br2I2 2 13 14 15 16 17 Transition Metals 9 3 4 5 6 7 8 10 11 12

  25. NON-METALS METALS METALLOIDS

  26. DIAGONAL RULEOrder of Filling orbitals due to increasing energy (Lowest energy level – 1) • Draw a diagram putting each energy shell on a row . • Listing the orbitals, (s, p, d, f), (left-to-right) 1s 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p 5d 5f 6s 6p 6d 7s 7p • Next, draw arrows through the diagonals, looping back to the next diagonal each time Aufbau Principleelectrons will fill orbitals of lowest energy first, then fill according to increasing energy.

  27. Diagonal Rule • Steps: • Write the energy levels top to bottom. • Write the orbitals in s, p, d, f order. Write the same number of orbitals as the energy level. • Draw diagonal lines from the top right to the bottom left. • To get the correct order, follow the arrows! 1 2 3 4 5 6 7 s s 2p s 3p 3d s 4p 4d 4f By this point, we are past the current periodic table so we can stop. s 5p 5d 5f 5g? s 6p 6d 6f 6g? 6h? s 7p 7d 7f 7g? 7h? 7i?

  28. Order of Electron Subshell Filling:It does not go “in order” Where is Ag on the Per. Table? 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 4d10 4f14 5s2 5p6 5d10 5f14 6s2 6p6 6d10 • Ag • 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s24d9 7s2 7p6

  29. ORBITAL 2 e- 6 e- Space occupied by a pair of electrons 10 e- 14 e-

  30. Four Sub-Energy Levels

  31. So why do electrons fill in like they do? Why is K’s last electron in the 4th energy level?

  32. 2 Factors Influencing Electron Placement • Energy Level • - Closer to nucleus=easy 2. Orbital or Subenergy level (shape) - spdf

  33. Electron Configuration A detailed way of showing the order in which electrons fill in around the nucleus

  34. What element is this? # of e- in sub-energy level Electron Configuration Symbols 5f3 Sub-Energy Level Energy Level

  35. Electron Configurations What element is this? 2p4 Number of electrons in the sublevel Energy Level Sublevel

  36. Electron Configuration 2p4 4f14 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14…etc.

  37. Writing Electron Configurations • Strategy: start with hydrogen, and build theconfiguration one electron at a time(Aufbau principle) • 1. In the H put 1s1; above He put 1s2; in Li 2s1, Be 2s2, In B put 2p1; in C put 2p1; etc across the chart. • 2. Fill subshells in order by counting across periods, from hydrogenup to the element of interest: Click here

  38. PERIODIC TABLE WORKSHEET Give the location of the last electron for all of the elements on the periodic table below. 1s2 1s1 2s1 2p1 2p2 2s2 4s2 3d1 5d1 5d5 6p3 5f1 Click here…

  39. Bohr Models vs. Electron Configurations K K 19e- K: 1s2 3s2 3p6 4s1 2p6 2s2

  40. 1s1 Write the e-config for: 1s2 He: Li: 1s22s1 H: K: 1s22s22p63s23p64s1 Al: 1s22s22p63s23p1

  41. K: 1s22s22p63s23p64s1 Noble Gas Shortcut K: [Ar] 4s1 So what is different?

  42. Electron Configuration fromthe Periodic Table 8A 1A 1 2 3 4 5 6 7 3A 4A 5A 6A 7A 2A Ne P 3s2 3p3 P = [Ne]3s23p3 P has 5 valence electrons

  43. Electron Configuration fromthe Periodic Table 8A 1A 1 2 3 4 5 6 7 3A 4A 5A 6A 7A 2A 3d10 Ar As 4s2 4p3 As = [Ar]4s23d104p3 As has 5 valence electrons

  44. Noble Gas Configuration • Find the symbol for the element zinc. [Zn] 2. Write the symbol in brackets for the nearest, smaller noble gas. [Ar] 3. Write the outer electron configuration for the remaining electrons. [Ar] 4s2 3d10 1s22s22p63s23p4 Ex. 1.S [Ne]3s23p4 1s22s22p63s23p64s23d104p65s24d105p66s24f145d4 2. W [Xe]6s24f145d4

  45. Orbital Notation Electrons are distributed in the electron cloud into: principal energy levels(1, 2, 3, 4, 5, 6, 7), sublevels (s, p, d, f), orbitals (s has 1, p has 3, d has 5, f has7) and spin(2 electrons allowed per orbital).

  46. Arrow-Orbital Notation A way to show orbital filling, spin, relative energy

  47. Fluorine’s Orbital notation s = ____ ( One orbital / 1 line) p = ____ ____ ____ ( 3 orbitals/ 3 lines) d = ____ ____ ____ ____ ____ ( 5 orbitals/ 5 lines) f = ____ ____ ____ ____ ____ ____ ____ ( 7 orbitals/ 7 lines)

  48. unoccupied orbital orbital with 1 electron orbital with 2 electrons Orbital Diagrams • an orbital is represented as a square and the • electrons in that orbital as arrows • the direction of the arrow represents the spin of the electron