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Chapter 3

Chapter 3. Chemical Compounds. Types of Compounds. Inorganic Compounds – do not contain carbon Organic Compounds – contain carbon. Inorganic Compounds. Ionic compound combination of metals and nonmetals made up of positive and negative ions joined together by electrostatic

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Chapter 3

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  1. Chapter 3 Chemical Compounds

  2. Types of Compounds • Inorganic Compounds – do not contain carbon • Organic Compounds – contain carbon HFinks '07

  3. Inorganic Compounds • Ionic compound combination of metals and nonmetals made up of positive and negative ions joined together by electrostatic forces HFinks '07

  4. Ions • Ions are atoms that have either lost or gained electrons. • Electrons are lost from the outermost energy level (discussed later in textbook) • Ions that have more protons than electrons are positively charged • Ions that have more electrons than protons are negatively charged HFinks '07

  5. Monatomic Ions • Formed from a single atom • Example: • Sodium Na+ • Sulfur s6+ or S2- HFinks '07

  6. Monatomic ions • Ions formed from a single atom • Atom = Na Ion = Na+ • Atom = O Ion = O2- HFinks '07

  7. Using your periodic table • The number of the main group elements will be used to determine the oxidation states. • Groups IA, IIA, IIIA = +, 2+, 3+ • Group VA = 5+, 3- • Group VIA = 6+, 2- • Group VIIA = 7+, - HFinks '07

  8. Alkali Metals (Group IA) • The oxidation number of alkali metals in a compound is always 1+. Never write the number 1 for anything in chemistry. It is understood. HFinks '07

  9. Alkaline Earth Metals (Group IIA) • The oxidation number of alkaline earth metals in a compound is always 2+. HFinks '07

  10. Nitrogen Family (Group VA) • Nitrides, phosphides, and arsenides are always 3- in binary salts. N3- P3- As3- HFinks '07

  11. Oxygen Family (Group VIA) • The oxidation number of oxygen is almost always 2- in a compound. There are exceptions. a) Peroxides, O22- (each oxygen is 1-) [Formed with elements in Groups IA and IIA] b) Superoxides, O2- (each oxygen is ½-) K, Rb and Ce are the only elements that form Superoxides. • Sulfide, selenide, telluride, and polonide are always 2- in binary salts. (S2-, Se2-, Te2-, Po2-) HFinks '07

  12. The Halogens (Group VIIA) • In metallic halides the halogen (F, Cl, Br, I, At) always has an oxidation number equal to 1-. • Remember: Never write the number 1. HFinks '07

  13. Oxidation States for Monatomic Ions HFinks '07

  14. Oxidation State for Monatomic Ions HFinks '07

  15. Balancing Using Oxidation Number • The oxidation number of any element in its free state (uncombined with other elements) is 0. HFinks '07

  16. Ionic Compounds • Ionic compounds consists of a metallic ion and a non-metallic ion. • Positive ion is the cation • Negative ion is the anion. HFinks '07

  17. Chemical Formula indicates • The elements present • The relative number of atoms of each element in the compound HFinks '07

  18. Binary Compounds • Binary compounds are made of two different element. -Combined chemically -Definite proportion by mass HFinks '07

  19. Balancing Binary Compounds • Step I: Write the symbols for each ion • Example: Na Cl • Step II: Assign an oxidation number • Na+ Cl- Al3+ S2- • Step III: Balance the compound. The sum of the oxidation numbers must be zero. (Hint: Crisscross the charges. Don’t include the signs.) NaCl Al2S3 HFinks '07

  20. Balancing Binary Compounds • What should you do if the charges are the same? • Nothing. The formula is balanced. The sum of the charges is “0”. • Example: Ba 2+ O2- = BaO HFinks '07

  21. Balancing Binary Formulas • Silver & chlorine • Zinc & oxygen • Calcium & bromine • Strontium & fluorine • Barium & chlorine • Calcium & chlorine HFinks '07

  22. Balancing Binary Formulas • Silver & chlorine AgCl • Zinc & oxygen ZnO • Calcium & bromine CaBr2 • Strontium & fluorine SrF2 • Barium & chlorine BaCl2 • Calcium & chlorine CaCl2 HFinks '07

  23. Naming Binary Compounds 1. Write a balanced formula 2. Write the name of the 1st ion with no changes. 3. Change the ending on the 2nd ion to –ide. HFinks '07

  24. Naming Binary Compounds Example NaCl = sodium chloride HFinks '07

  25. Naming Binary Compounds • Silver & chlorine • Zinc & oxygen • Calcium & bromine • Strontium & fluorine • Barium & chlorine • Calcium & chlorine HFinks '07

  26. Naming Binary Compounds • Silver & chlorine silver chloride • Zinc & oxygen zinc oxide • Calcium & bromine calcium bromide • Strontium & fluorine strontium fluoride • Barium & chlorine barium chloride • Calcium & chlorine calcium chloride HFinks '07

  27. Transitional Ions and Charges • Fe2+ Iron (II) Ni 2+ Au+ • Fe3+ Iron (III) Ni 3+ Au 3+ • Sn2+ Tin (II) Zn 2+ Ag+1 • Sn4+ Tin (IV) • Cu+1 Copper (I) Pb 2+ Mn+2, +3, +4,+6,+7 • Cu+2 Copper (II) Pb 4+ • Co +2 • Co +3 HFinks '07

  28. Naming Transitional Binary Compounds • Fe2+ Iron (II) FeCl2 = iron (II) chloride • Fe3+ Iron (III) • Sn2+ Tin (II) SnCl2 = tin (II) chloride • Sn4+ Tin (IV) • Cu+1 Copper (I) CuCl = copper (I) chloride • Cu+2 Copper (II) HFinks '07

  29. Polyatomic Ions Polyatomic ions consist of two or more ions that act as one in a chemical reaction. Examples: NO3- nitrate PO43- phosphate SO42- sulfate NO2- nitrite SO32- sulfite OH- hydroxide ClO3- chlorate MnO4- permanganate C2H3O2- acetate NH4+ ammonium HFinks '07

  30. Ternary Compounds • Ternary compounds are made up of three ions. Two of the ions are joined together and act as one. (polyatomic ion) • Example: NaNO3 Na = sodium N = nitrogen O = oxygen N & O make up the nitrate ion, NO3- HFinks '07

  31. Naming Ternary Compounds 1. Write a balanced formula 2. Write the name of the 1st ion. No changes to name. 3. Write the name of the polyatomic ion. NaNO3 = sodium nitrate HFinks '07

  32. Formula and Name of Ternary Compounds • MgCO3 magnesium carbonate • Pb(NO3)2 lead nitrate • Ca(OH)2 calcium hydroxide • Ba(NO3)2 barium nitrate • Fe2(SO4)3 iron (III) sulfate • LiC2H3O2 lithium acetate • KClO3 potassium chlorate • (NH4)2SO4 ammonium sulfate HFinks '07

  33. Organic Compounds • Molecular compound • Made up of a small number of different non-metal atoms • Held together by forces known as covalent bonds The chemical formula gives you the number of atoms of each element contained in a single molecule of the compound HFinks '07

  34. Organic CompoundsPrefixes Number Prefix 1 mono- 2 di-/bi 3 tri- 4 tetra- 5 penta- 6 hexa- 7 hepta- 8 octa- 9 nona- 10 deca- HFinks '07

  35. Organic Compounds • Carbon dioxide CO2 • Nitrogen trioxide NO3 • Dinitrogen trioxide N2O3 HFinks '07

  36. Nomenclature Review Wkst. • 1. calcium chloride 1. NaCl • 2. magnesium oxide 2. MgCl2 • 3. iron (III) hydroxide 3. BaF2 • 4. potassium sulfate 4. KNO3 • 5. cesium nitrate 5. Al2S3 HFinks '07

  37. Nomenclature Review • 6. rubidium selenide 6. Li2O • 7. strontium phosphate 7. SrSO4 • 8. potassium oxide 8. CuCl2 • 9. copper (I) oxide 9. (NH4)3PO4 • 10. ammonium sulfafte 10. BeBr2 HFinks '07

  38. Nomenclature Review • 11. sodium sulfide 11. H2SO4 • 12. rubidium sulfate 12. Mg3(PO4)2 • 13. calcium hydroxide 13. Na3PO4 • 14. sodium iodide 14. (NH4)2O • 15. potassium hydroxide 15. AuCl3 HFinks '07

  39. Nomenclature Review • 16. lead (II) sulfide 16. Na2CO3 • 17. sodium carbonate 17. SiO2 • 18. iron (III) chloride 18. PbS • 19. phosphoric acid 19. N2O3 • 20. barium sulfate 20. HNO3 • 21. silver nitrate 21. CaBr2 HFinks '07

  40. Naming Ionic Compounds • 1. sodium carbonate 129.0 g/mol • 2. sodium hydroxide 40.00 g/mol • 3. magnesium bromide 184.1 g/mol • 4. potassium chloride 74.6 g/mol • 5. iron (II) chloride 126.8 g/mol HFinks '07

  41. Naming Ionic Compounds • 6. iron (III) chloride 162.3 g/mol • 7. zinc hydroxide 99.4 g/mol • 8. beryllium sulfate 114.1 g/mol • 9. chromium (II) fluoride 90.0 g/mol • 10. aluminum sulfide 150 g/mol HFinks '07

  42. Naming Ionic Compounds • 11. lead (II) oxide 223.2 g/mol • 12. lithium phosphate 115.7 g/mol • 13. titanium (IV) iodide 556.3 g/mol • 14. cobalt (II) nitride 204.7 g/mol • 15. magnesium phosphide 134.9 g/mol HFinks '07

  43. Naming Ionic Compounds • 16. gallium nitrite 207.7 g/mol • 17. silver sulfite 296 g/mol • 18. ammonium hydroxide 35.0 g/mol • 19. aluminum cyanide 105.0 g/mol • 20. beryllium acetate 127.0 g/mol HFinks '07

  44. Polyatomic Ions • Don’t separate the elements in the ion. Keep them together. • Don’t: N + O3 • But NO3- HFinks '07

  45. Determining the Charge on a Polyatomic Ion • (NO3)- (N5+ O36-)- (SO4)2-(S6+ O48-)2- HFinks '07

  46. Determine the oxidation number of the ions in the polyatomic ions below • Phosphate • Chlorate • Sulfite • Permanganate • Nitrite • Hyroxide HFinks '07

  47. Oxidation States of Elements in Polyatomic Ions • Phosphate (P5+ O48-) 3- • Chlorate (Cl5+ O36-) – • Sulfite (S4+O36- ) 2- • Hydroxide (O2-, H+)- HFinks '07

  48. Oxidation States of Elements in Polyatomic Ions • Permanganate (Mn 7+ O42-) - • Nitrite (N 5+ O24-) – • Acetate (C26+H33-O24-) – HFinks '07

  49. What are the oxidation states of the atoms below? • Sodium chlorine • Magnesium oxygen • Barium sulfur • Potassium fluoride • Aluminum bromine • Calcium iodine HFinks '07

  50. Oxidation States for Monatomic Ions HFinks '07

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