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Catalyst – September 1s 2 2s 2 2p 6 3s 2 3p 4 , 2010

Catalyst – September 1s 2 2s 2 2p 6 3s 2 3p 4 , 2010. Review the electron configurations that you saw yesterday: Mg-1s 2 2s 2 2p 6 3s 2 Ne- 1s 2 2s 2 2p 6 Si- 1s 2 2s 2 2p 6 3s 2 3p 2 K- 1s 2 2s 2 2p 6 3s 2 3p 6 4s 1. Now, write the electron configurations for… Iron (Fe) Oxygen (O).

terence-shirley
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Catalyst – September 1s 2 2s 2 2p 6 3s 2 3p 4 , 2010

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  1. Catalyst – September 1s22s22p63s23p4, 2010 • Review the electron configurations that you saw yesterday: • Mg-1s22s22p63s2 • Ne- 1s22s22p6 • Si- 1s22s22p63s23p2 • K- 1s22s22p63s23p64s1 • Now, write the electron configurations for… • Iron (Fe) • Oxygen (O)

  2. Today’s Agenda • Catalyst • Noble Gas Configuration • Periodic Trends • Work Time • Exit Question

  3. Today’s Objectives • SWBAT write noble gas configurations for elements. • SWBAT describe the periodic trends for atomic radius and electronegativity.

  4. Be: 1s22s2 Ne: 1s22s22p6 Br: 1s22s22p63s23p64s23d104p5 Practice Problems: Electron Configuration

  5. C: 1s22s22p2 Ca: 1s22s22p63s23p64s2 As: 1s22s22p63s23p64s23d104p3 Practice Problems: Electron Configuration

  6. 1s22s22p23s23p64s23d104p64s24d105p5: I (Iodine) 1s22s22p63s23p64s23d8: Ni 1s22s22p63s23p64s23d104p65s2 4d105p66s1: Cs Practice Problems: Electron Configuration

  7. Scientists are WAY too lazy to write all that mess! Noble Gas Configuration

  8. Ba – [Xe]6s2 P – [Ne]3s23p3 Y – [Kr]5s24d1 Si- Rb- Electron Configuration FIGURE IT OUT YOURSELF!!!

  9. Noble Gas Configuration • Key Point #4: Noble Gas configuration starts with noble gas BEFORE the atom you are going to.

  10. Ag (instead of Hg) Electron Configuration

  11. Ag – [Kr] Electron Configuration

  12. Ag – [Kr]5s2 Electron Configuration

  13. Ag – [Kr]5s24d9 Electron Configuration

  14. Electron Configuration S

  15. Electron Configuration S – [Ne]

  16. Electron Configuration S – [Ne]3s2

  17. Electron Configuration S – [Ne]3s23p4

  18. Electron Configuration Sm

  19. Electron Configuration Sm – [Xe]

  20. Electron Configuration Sm – [Xe]6s2

  21. Electron Configuration Sm – [Xe]6s25d14f5

  22. PERIODIC TRENDS!!! VALENCE ELECTRONS (CHECK!) ATOMIC RADIUS ELECTRONEGATIVITY

  23. Valence Electrons Don’t forget! • Valence electrons are the electrons in the outermost energy level.

  24. Example • Electron configuration for silicon (Si): • What is the highest energy level? • So how many valence electrons? 1s22s22p63s23p2 2 + 2 = 4!

  25. Valence Electrons

  26. You have this in your notes – back of the Periodic Table Basics Notes! Valence Electron Trendson the Periodic Table

  27. What is Atomic Radius? • Key Point #1: Atomic radiusis how big an atom is and is also known as atomic size

  28. What is Electronegativity? • Key Point #2: Electronegativityis the ability of an atom to attract electrons to itself in a chemical bond • How much an atom wants electrons

  29. So as you go LEFT to RIGHT… • Key Point #3: As you move left to right across the periodic table, positive charge increases so… • ELECTRONEGATIVITY INCREASES • Therefore, ATOMIC RADIUS DECREASES

  30. Electronegativity Trends

  31. On the Diag….onal

  32. So as you go from TOP to BOTTOM… • Key Point #4: As you go from top to bottom on the periodic table, energy levels (shells) increase so… • ATOMIC RADIUS INCREASES • Therefore, ELECTRONEGATIVITY DECREASES

  33. Electronegativity Trends

  34. How are atomic radius and electronegativity related? Key Point #5: Atomic radius and electronegativity are indirectly/inversely related. ATOMIC RADIUS ELECTRONEGATIVITY

  35. Why is this relationship true? • Atoms with HIGH ELECTRONEGATIVITIES hold their electrons very close! • Sooooo, the atomic radius decreases High or low electronegativity? Large or small atomic size?

  36. Why is this relationship true? • Atoms with LARGE RADII can’t pull on their electrons as much • Soooo, ELECTRONEGATIVITY decreases!

  37. Practice Problems • Rank the following elements in order of increasing atomic radius based on location on the periodic table (smallest to biggest) • Fr, Sc, P, Pd P, Sc, Pd, Fr F, As, Tl, S Fluorine, Sulfur, Arsenic, Thallium

  38. Practice Problems • Rank the following elements in order of increasing electronegativity based on location on the periodic table (smallest to biggest) • Mg, Sr, Be, Ra Radon, Strontium, Magnesium, Beryllium Cl, Si, Al, S, P Aluminum, Silicon, Phosphorus, Sulfur, Chlorine

  39. More Practice! • T or F? Atomic size decreases as you move right across the periodic table. • T or F? As you move down the Periodic Table, atoms get smaller. • Rank the following sets of elements in order of increasing atomic size (small  big). Set A: Bh, Mn, Re, Tc Set B: Sb, I, Ag, Ru Set C: Y, Ti, Sg, Ta • Rank the following sets of elements in order of decreasing atomic size (big  small). Set A: Cl, At, I, F, Br Set B: Te, Xe, Sn, In Set C:Rb, K, Sr, Ca

  40. More Practice! • T or F? Electronegativity decreases as you move left across the periodic table. • T or F? As you move down the Periodic Table, atoms get more electronegative. • Rank the following sets of elements in order of increasing electronegativity (small  big). Set A: Bh, Mn, Re, Tc Set B: Sb, I, Ag, Ru Set C: Y, Ti, Sg, Ta • Rank the following sets of elements in order of decreasing electronegativity (big  small). Set A: Cl, At, I, F, Br Set B: Te, Xe, Sn, In Set C:Rb, K, Sr, Ca

  41. GROUP WORK TIME!

  42. Exit Question • Which element has atoms with the smallest radius: Cl, Se, P, or F? • Which element has the largest electronegativity: Ag, Cu, Hg, or Zn? • How are atomic radius and electronegativity related?

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