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Chemistry Ch. 7, Ionic and Metallic Bonding

Chemistry Ch. 7, Ionic and Metallic Bonding. Memorize: NH 4 + Ammonium CO 3 2- Carbonate NO 3 - Nitrate PO 4 3- Phosphate SO 4 2- Sulfate OH - Hydroxide. Practice: NH 4 + CO 3 2- NO 3 - PO 4 3- SO 4 2- OH -.

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Chemistry Ch. 7, Ionic and Metallic Bonding

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  1. Chemistry Ch. 7, Ionic and Metallic Bonding

  2. Memorize: • NH4+ Ammonium • CO32- Carbonate • NO3- Nitrate • PO43- Phosphate • SO42- Sulfate • OH- Hydroxide

  3. Practice: • NH4+ • CO32- • NO3- • PO43- • SO42- • OH-

  4. Practice: • Ammonium • Carbonate • Nitrate • Phosphate • Sulfate • Hydroxide

  5. *Valence electrons: electrons in the very outer energy level.

  6. *Electron Dot Diagrams: Show Valence electrons as dots. Hint: use one two skip a few song. • Exp: Draw e.d.d.’s for Li, N, Se

  7. *The Octet Rule: Atoms tend to fill their valence shell with 8 electrons (except the first energy level only needs 2 electrons).

  8. When an atom loses electrons, a cation is formed with a positive charge.

  9. Look at Sodium’s electron config and Ne

  10. Sometimes atoms lose or gain electrons that are not in the very outer shell. • Gold 4s13d10 turns into a cation

  11. Anions form when an atom gains electrons to form an anion (negatively charged ion). • Example: O2- • Which element has the same electron configuration as O2-?

  12. Halide Ions Form from group 17 atoms. They gain one electron to make an ion with a charge of –1.

  13. Write the electron configurations for: • P3- • Mg2+

  14. Writing Symbols and Names of Ions • Iodine  I- Iodide • A Calcium atom that loses two electrons  Ca2+ Calcium ion • A Phosphorus atom that gains three electrons P3- Phosphide

  15. *Ionic Compounds: Are made of ions put together. • *The total charge on an ionic compound is 0.

  16. The forces that hold ionic compounds together are called ionic bonds.

  17. NaCl • Draw edds and show how NaCl forms.

  18. Na2O • Draw edds and show how Na2O forms.

  19. *A Chemical Formula describes the atoms in a compound. • Example: MgCl2 • Example: C6H12O6

  20. Predict chemical formulas for when: • Na reacts with P • Mg reacts with Br • Mg reacts with P

  21. Properties of Ionic Compounds • *Most are cystalline solids at room temperature.

  22. Flourite (CaF2) Cinnabar (HgS)

  23. *Ionic Compounds have high melting points due to the high attractive forces between positive and negative ions.

  24. *Coordination Number: The number of ions of opposite charge that surround an ion in a crystal.

  25. NaCl (6)

  26. CsCl (8)

  27. Ionic Compounds can conduct electricity when they are melted or dissolved in water.

  28. Draw NaCl in water, with cathode and anode

  29. Bonding in Metals • Metal ions are always positively charged. • In a metal, cations are closely packed together, and valence electrons are free-flowing.

  30. Metallic Bonds Are the attraction of the valence electrons for the metal cations.

  31. Metallic Bonds make metals strong.

  32. Metal cations have a Crystalline Structure They are arranged in patterns.

  33. Alloys: Mixtures of 2 or more elements, with at least one being a metal.

  34. Bronze seven parts copper and one part tin. • Stainless Steel 80.6% Fe, 18% Cr, .4% C, 1% Ni

  35. Differences between Metals and Ionic Compounds:

  36. Percent Yield Ionic Compound Lab • See Handout! Theoretical yield of Calcium Carbonate is: 0.68 g. • 1. What are your observations from this lab? What happened? • 2. Calculate your percent yield. • 3. What could you have done differently in order to increase your percent yield?

  37. Lab: Metals, Nonmetals, Covalent, and Ionic Compounds • See Next Slides. Cut these questions out and make stations througout the classroom. • Give brief explanation of these 4 types before doing the lab!

  38. 1. Measure the conductivity of the Aluminum metal. Is it conductive? • 2. Measure the conductivity of the sugar (a covalent compound). Is it conductive? • 3. Measure the conductivity of the wood (a nonmetal). Is it conductive? • 4. Measure the conductivity of the tin metal. Is it conductive?

  39. 5. Measure the conductivity of the zinc metal. Is it conductive? • 6. Measure the conductivity of the CaCl2 (an ionic compound). Is it conductive? • 7. Take a look at this water and NaCl mixture. Did the ionic compound dissolve in the water? Test the conductivity Is it conductive?

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