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Catalyst – October 7(4), 2009

Catalyst – October 7(4), 2009. Write and name the compound formed through Beryllium and Oxygen. Write and name the compound formed between Potassium and Sulfur. Today’s Agenda. Catalyst Practice Naming Ionic Intro to Covalent Compounds Covalent Bond Formation (more LDS’s!)

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Catalyst – October 7(4), 2009

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  1. Catalyst – October 7(4), 2009 • Write and name the compound formed through Beryllium and Oxygen. • Write and name the compound formed between Potassium and Sulfur.

  2. Today’s Agenda • Catalyst • Practice Naming Ionic • Intro to Covalent Compounds • Covalent Bond Formation (more LDS’s!) • Project Work Time • Exit Question

  3. What do you see? Copy the table into your notes and fill in the question marks with what you think is correct.

  4. Write name of first element (metal). • Second element ends in -ide. • Ignore subscripts! Naming Ionic Compounds

  5. Draw a mental line between the ions. Na+ Cl- Naming Ionic Compounds

  6. Binary Ionic Compound – an ionic compound composed of two elements Naming Ionic Compounds

  7. ZnO Naming Ionic Compounds

  8. ZnO Zinc Oxide Naming Ionic Compounds

  9. CaCl2 Naming Ionic Compounds

  10. CaCl2 Calcium Chloride Naming Ionic Compounds

  11. Al2O3 Naming Ionic Compounds

  12. Al2O3 Aluminum Oxide Naming Ionic Compounds

  13. Ternary Ionic Compound – an ionic compound with more than 2 elements Naming Ionic Compounds

  14. Ionic Cheat Sheets! Naming Ionic Compounds

  15. Do not lose this…you will need it the rest of your life (in my class). Naming Ionic Compounds

  16. The way you use it… Naming Ionic Compounds

  17. 1) Look up the ions on the cheat sheet and write the words next to them. Naming Ionic Compounds

  18. BaCO3 Naming Ionic Compounds

  19. BaCO3 Normally the first element is the first piece and the rest is the second piece. Naming Ionic Compounds

  20. BaCO3 Barium Naming Ionic Compounds

  21. If the first element is +2, where should we find the second? (Remember, charges must balance!) Naming Ionic Compounds

  22. BaCO3 Barium Naming Ionic Compounds

  23. BaCO3 Barium Carbonate Naming Ionic Compounds

  24. AlPO3 Naming Ionic Compounds

  25. AlPO3 Aluminum Naming Ionic Compounds

  26. AlPO3 Aluminum Phosphite Naming Ionic Compounds

  27. H3PO4 Naming Ionic Compounds

  28. H3PO4 Hydrogen Naming Ionic Compounds

  29. H3PO4 Think: H+, we have 3 which means +3, where will PO4 be? Naming Ionic Compounds

  30. H3PO4 Hydrogen Phosphate Naming Ionic Compounds

  31. FeSO4 Naming Ionic Compounds

  32. FeSO4 Notice Iron appears in +2 and +3… Naming Ionic Compounds

  33. FeSO4 Sulfate Naming Ionic Compounds

  34. FeSO4 Since Sulfate is -2, Fe must be +2 Naming Ionic Compounds

  35. FeSO4 Iron(II) Sulfate Naming Ionic Compounds

  36. FeSO4 Iron(II) Sulfate or Ferrous Sulfate Naming Ionic Compounds

  37. Exit Question • What is the formula of the compound form between beryllium and phosphate. Then, name the compound. • What is the formula of the compound formed between sodium and oxygen. Then, name the compound

  38. Today’s Objectives • SWBAT find some atom love! • SWBAT state characteristics of covalent compounds. • SWBAT model covalent bond formation.

  39. Covalent Compounds in da House! • Covalent compounds are EVERYWHERE! • Household cleaners (Ammonia) • Water! • Salad dressing • Political debate! (think greenhouse gases)

  40. Find the Characteristics of Covalent Compounds…. Let’s HUNT!

  41. Characteristics of Covalent Compounds(Key Point #1) • Electrons are shared • Bonds between nonmetals and non metals • Usually gases at room temperature (not crystals ) • Low melting points • Poor conductors of electricity

  42. What’s the difference between ionic and covalent compounds? • It is important to understand the differences between ionic and covalent compounds • Let’s review ionic compound characteristics…

  43. Characteristics of Ionic Compounds • Electrons are transferred • Bonds between metals and nonmetals • Make crystals • High melting points • Good conductors of electricity when dissolved

  44. Group Race! • Each group will complete a Double Bubble Diagram…liiiiiike this (Double Bubble doc) • Rules: • No talking or sharing of notes! • First person fills in ONE bubble and passes paper to next person – cannot skip people! • If next person doesn’t know an answer, he/she must stand up and do 10 jumping jacks before passing paper. • Next person fills in ONE bubble and passes paper to next person…etc!

  45. How do covalent bonds form? • Let’s look at Lewis Dot Structures again! • Key Point #2: Each atom in a compound satisfies the octet rule. This is shown in a Lewis Dot Structure.

  46. Single Bonds • Single covalent bond: one pair of shared electrons (two electrons) • Atoms may be the same • H2, F2, Cl2, Br2, I2, O2 • Atoms may be different • HF, HCl, HBr, HI =

  47. Formation of Single Covalent Bonds Examples H2 F2 HCl (chlorine)

  48. Formation of Single Covalent Bonds Your Turn! Cl2 HBr

  49. Tricks! • Central atom: in the center of a molecule, usually has lower electronegativity • Terminal atom: not in the center of a molecule Hydrogen will NEVER be a central atom!

  50. Formation of Multiple Single Bonds Examples NH3 SeCl2

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