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Warm up 10-13-14

Warm up 10-13-14. Covalent bonds are between _____ and _____ elements Ionic bonds are between _____ and _____ elements Identify if these compounds are ionic or covalent: FeS , CO 2 , Cl 2 and AlBr 3. Agenda -Turn in HW online bonds -Take quiz -Notes Chp 6-2 Lewis dot

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Warm up 10-13-14

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  1. Warm up 10-13-14 • Covalent bonds are between _____ and _____ elements • Ionic bonds are between _____ and _____ elements • Identify if these compounds are ionic or covalent: FeS, CO2, Cl2 and AlBr3 Agenda -Turn in HW online bonds-Take quiz -Notes Chp 6-2 Lewis dot -Lab chemical bonds Homework Oct 24 – Online HW (57Qs)

  2. Review For the Quiz • Chapter 5 – Ions (positive and negative charge) - Bonds (3 types)

  3. Formulas and Names of Ionic and Covalent Compounds Chp 5-3 and 6-2

  4. Nomenclature: Naming of compounds • Must determine which bond made up the compound • Ionic bond has metal elements • Covalent bond has no metal elements

  5. Naming Covalent (Molecular) Compounds 1. Use a prefix to indicate the amount of each element in the compound 2. Never use mono– on the first element name. 3.Give the last element an –ide ending.

  6. Naming Covalent (Molecular) Compounds • Mono– 1 • Di– 2 • Tri– 3 • Tetra– 4 • Penta– 5 • Hexa– 6 • Hepta– 7 • Octa– 8 • Nona– 9 • Deca– 10 Prefixes

  7. Examples • CO2 • B2H4 • Dinitrogen trioxide

  8. Naming Covalent CompoundsPractice

  9. Naming Ionic Compounds 1. Ending element change to –ide. (no prefixes) 2. Make sure all the charge cancel each other out 3. If there is a transition metal you indicate the charge with a roman numeral after the name of the metal. 4. If it is a polyatomic ion, you simply use the name as it is. (no –ide)

  10. Examples • CaCl2 • MgI2 • Potassium Sulfide • Beryllium Fluoride • Iron (II) Nitride • FeCl2

  11. Naming Ionic CompoundsPractice Writing Chemical Formula for Ionic Compounds -Write the symbol and charge -Cation goes in front -Make sure all the charges Cancel each other out • ______________ AlCl3 • ______________ Na2S • Lithium Bromide _____ • Calcium Fluoride _____ • Aluminum Oxide _____ • ____________ CuCl2 • Iron (III) Phosphide ____ Transition metal

  12. Naming Ionic Compounds- Polyatomic Ions (NH4)+Ammonium (NH3) Ammonia (OH)- Hydroxide (CO3)-2 Carbonate (NO3)- Nitrate (NO2)-Nitrite (SO4)-2 Sulfate (SO3)-2Sulfite (PO4)-3 Phosphate (PO3)-3Phosphite (Cr2O7)-2Dichromate

  13. Naming Polyatomic Ions • ______________ Li2SO4 • ______________ Sr(NO3)2 • Potassium Phosphate _____ • Ammonium Oxide _____ • ______________ NaOH • ______________ Ca(NO2)2 • Calcium Carbonate ______ • Ammonium Sulfide _____

  14. More Examples • Mixture of covalent, ionic and polyatomic nomenclature.

  15. SrS Strontium Sulfide

  16. GaCl3 Gallium Chloride

  17. Ammonium NH4+

  18. Calcium Oxide CaO

  19. Sulfate SO42-

  20. Phosphate PO43-

  21. Strontium Nitride Sr3N2

  22. Li3N Lithium Nitride

  23. Hydroxide OH-

  24. Beryllium Carbonate BeCO3

  25. BeSe Beryllium Selenide

  26. Mg(NO3)2 Magnesium Nitrate

  27. KBr Potassium Bromide

  28. AlPO4 Aluminum Phosphate

  29. Magnesium Arsenide Mg3As2

  30. NaOH Sodium Hydroxide

  31. Potassium Sulfate K2SO4

  32. Ba2P3 Barium Phosphide

  33. Rubidium Phosphide Rb3P

  34. Potassium Chloride KCl

  35. Sodium Oxide Na2O

  36. Rb2O Rubidium Oxide

  37. Bond Identification lab • Objectives: Classify compounds as having ionic or covalent bond based on its physical property: solubility, conductivity and melting point • Procedure: • Obtain the chemicals (half of a well) • Set up the apparatus and label your aluminum foil using a pencil • Put the chemicals on top of the aluminum foil and apply heat to it • Record the order that each compound melt • Dissolve the chemicals in water and ethanol

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