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Catalyst

Catalyst. 1. How many atoms total are in the compound Al 3 SO 4 2. How many atoms total are in the compound H 2 (SO 3 ) 2 ? 3. Use your packet: What type of bond is betwee n Cs and Br? For #4-6, fill in the blank with “ionic” or “covalent”

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Catalyst

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  1. Catalyst • 1. How many atoms total are in the compound Al3SO4 • 2. How many atoms total are in the compound H2(SO3)2? • 3. Use your packet: What type of bond is between Cs and Br? • For #4-6, fill in the blank with “ionic” or “covalent” • 4. In _______ bonds, electrons are transferred. • 5. ______ bonds are between a metal and a nonmetal. • 6. In _______ bonds, electrons are shared.

  2. Today’s Agenda

  3. Example • Determine the type of bond in HF • Find electronegativity of each atom

  4. Electronegativity Chart

  5. Example • Determine the type of bond in HF • Find electronegativity of each atom H = 2.2 Paulings, F = 4.0 Paulings

  6. Example • Determine the type of bond in HF • Find electronegativity of each atom H = 2.2 Paulings, F = 4.0 Paulings • Find Electronegativity Difference (∆EN) DEN = 4.0 – 2.2 = 1.8 • Look at chart to determine bond type.

  7. Bond Type Chart

  8. Example • Determine the type of bond in HF • Find electronegativity of each atom H = 2.2 Paulings, F = 4.0 Paulings • Find Electronegativity Difference (∆EN) DEN = 4.0 – 2.2 = 1.8 • Look at chart to determine bond type. Bond Type: Ionic

  9. Remember how there are different types of covalent bonds?...

  10. Bond Polarity Bond polarity is based on differences in electronegativities of atoms forming a bond • As electronegativity difference (∆EN) increases, polarity of bond increases

  11. Pure Ionic Bonding • Total give and take (transfer) of electrons! = Big ∆EN! I have no chance!

  12. Covalent Bonding is like a Tug-of-War • The more electronegative atom will pull electrons harder

  13. Polarity and Electronegativity • Polar bonds - electrons are pulled more toward one of the atoms Big ∆EN! • Nonpolar bonds - electrons are shared equally between atoms Low ∆EN! Big Dog – Little Dog Medium Dog – Medium Dog

  14. How Polar Is It? • Determine the polarity of each bond in the following compounds by calculating the electronegativity difference for each: • CO 5. HF • AlP6. CaO • N2 7. H2 4. SiO 8. NF3

  15. Today’s Agenda

  16. Stable Charges • Atoms can only bond if they are ions…. • Certain atoms prefer to have certain charges… • They prefer to act like noble gases and have the same electrons as noble gases…

  17. The Octet Rule - Review An atom that has gained an electron has a negative charge An atom that has lost an electron has a positive charge How can we know what charge it will have? Let’s talk about Lithium…..

  18. Stable Charges • Finding the stable charge: Count to the closest Noble Gas. If you count backwards, the charge is positive. If you count forwards, the charge is negative. • Li • Br • Ca • P 2:00 1:59 1:58 1:57 1:56 1:55 1:54 1:53 1:52 1:51 1:50 1:49 1:48 1:47 1:46 1:45 1:44 1:43 1:42 1:41 1:40 1:39 1:38 1:37 1:36 1:35 1:34 1:33 End 1:32 1:30 1:29 1:28 1:27 1:26 1:25 1:24 1:23 1:22 1:21 1:20 1:19 1:18 1:17 1:16 1:15 1:14 1:13 1:12 1:11 1:10 1:09 1:08 1:07 1:06 1:05 1:04 1:03 1:02 1:01 1:00 0:59 0:58 0:57 0:56 0:55 0:54 0:53 0:52 0:51 0:50 0:49 0:48 0:47 0:46 0:45 0:44 0:43 0:42 0:41 0:40 0:39 0:38 0:37 0:36 0:35 0:34 0:33 0:32 0:31 1:31 0:30 0:28 0:27 0:26 0:25 0:24 0:23 0:22 0:21 0:20 0:19 0:18 0:17 0:16 0:15 0:14 0:13 0:12 0:11 0:10 0:09 0:08 0:07 0:06 0:05 0:04 0:03 0:02 0:01 0:29 2:00

  19. Stable Charges • An ion is stable when it has the electron configuration of a noble gas (8 valence electrons)

  20. Once they have a charge, they want to combine with other ions… There is a trick to figuring this out…

  21. Ca2+As3- Kris Kross Method! Ca3As2

  22. The KrissKross method is for Ionic Bonds

  23. KrissKross Method • KrissKross Method: Write down the stable ions and cross the charges to make them subscripts • Exception: When the numbers are the same, they cancel out. Na1+Cl1- NaCl Li1+O2- Li2O

  24. Which charge ALWAYS comes first? POSITIVE!!

  25. 1. K F 2.BaN 3. Na O 4. Ca Cl 5. K Si 6. Co I

  26. K1+F1- Ba N Na O CaCl K Si Co I

  27. K1F1Ba N Na O Ca Cl K Si Co I

  28. KF Ba N Na O Ca Cl K Si Co I

  29. 1. K F 2.BaN 3.Na O 4. Ca Cl 5. K Si 6. Co I

  30. KF Ba2+N3- Na O CaCl K Si Co I

  31. KF Ba3N2 Na O CaCl K Si Co I

  32. KF Ba3N2 Na1+O2-CaCl K Si Co I

  33. KF Ba3N2 Na2OCaCl K Si Co I

  34. KF Ba3N2 Na2O Ca2+Cl1- K Si Co I

  35. KF Ba3N2 Na2OCaCl2 K Si Co I

  36. KF Ba3N2 Na2OCaCl2 K1+Si4- Co I

  37. KF Ba3N2 Na2OCaCl2 K4Si Co I

  38. K F Ba N Na O CaCl K Si Co I You don’t know about transition metals! So.. the problem must tell you the number of electrons. Cobalt (II) means that Cobalt gives up 2 electrons

  39. K F Ba N Na O CaCl K Si Co2+I1-

  40. K F Ba N Na O CaCl K Si CoI2

  41. Independent Practice For each pair find the STABLE ION and then Kris Kross! 1. Mg O 2. Na Br 3. Rb P 4. Be F 5. CaS 6. K Cl 7. Li N 8. Cu (III) O

  42. Today’s Agenda

  43. Exit Slip 1. Use the kriss-kross method to write the correct ionic compound for Ca and Cl 2. What is the ionic compound formed by Mg and N? • Mg2N3 • MgN2 • Mg3N2 3. Use the kriss-kross method to write the stable ionic compound for Al and Br. 4. True or false: The stable ion formed by Al is Al2+. 5. Which of the following is an incorrect match between the element and its stable charge? • N, -3 • Ba, +2 • F, +1 d. Br, -1

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