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Starter S-73

Starter S-73

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Starter S-73

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  1. Starter S-73 Give the scientific name for three chemical compounds.

  2. Chemical Names and Formulas Chapter 9

  3. 9.1 Naming Ions Chapter 9

  4. 9.1 Naming Ions Monatomic Ions – only one atom Review Cations (metals) form positive charges

  5. 9.1 Naming Ions Monatomic Ions – only one atom Review Group 1: +1

  6. 9.1 Naming Ions Monatomic Ions – only one atom Review Group 2: +2

  7. 8.1 Molecular Compounds 9.1 Naming Ions Some metals have more than one charge (oxidation number) They are named using the name and the charge

  8. 9.1 Naming Ions Monatomic Ions – only one atom Review Anions – negative ions (names end in –ide)

  9. 9.1 Naming Ions Monatomic Ions – only one atom Review Group 17: -1

  10. 9.1 Naming Ions Monatomic Ions – only one atom Review Group 16: -2

  11. 9.1 Naming Ions Monatomic Ions – only one atom Review Group 15: -3

  12. 9.1 Naming Ions Polyatomic Ions – a charged group of atoms bonded covalently Examples – Ammonium

  13. 9.1 Naming Ions Polyatomic Ions – a charged group of atoms bonded covalently Examples – Hydrogen Sulfate

  14. 9.1 Naming Ions Polyatomic Ions – a charged group of atoms bonded covalently Examples – Carbonate

  15. 9.1 Naming Ions See page 257 for a list of polyatomic ions. There will be a quiz.

  16. 9.2 Naming & Writing Formulas: Ionic Chapter 9

  17. 9.2 Naming & Writing Formulas: Ionic Binary Compounds – composed of two elements and can be ionic or covalently bonded For Ionic names • Write the name of the cation first • Write the name of the anion • Change the ending of the anion to -ide NaBr Sodium Br Sodium Bromine Sodium Bromide

  18. 9.2 Naming & Writing Formulas: Ionic If the compound has a metal with more than one charge, we must calculate the charge Write out the formula and the charge of the anion Calculate the total negative charge This is the total charge on the cation, so divide the charge by the number of atoms PbCl4-1 PbCl4

  19. 9.2 Naming & Writing Formulas: Ionic Name the cation Name the anion Change the ending to -ide PbCl4 Lead (IV) Cl4 Lead (IV) Chlorine Lead (IV) Chloride

  20. 9.2 Naming & Writing Formulas: Ionic Example 1: Example 2: Example 3: Example 4: Na2S Sodium S Sodium Sulfur Sodium Sulfide Copper (II) O CuO Copper (II) Oxide Copper (II) Oxygen ZnI2 Zinc I2 Zinc Iodine Zinc Iodide Iron (III) Sulfide Iron (III) Sulfur Iron (III) S3 Fe2S3

  21. 9.2 Naming & Writing Formulas: Ionic To write the formula from the name • Write the ions • Cross the values of the charges • Confirm it is the smallest ratio Nickel (III) Fluoride Ni+3 F- NiF3

  22. 9.2 Naming & Writing Formulas: Ionic Example 1: Example 2: Example 3: Example 4: Calcium Bromide Ca+2 Br- CaBr2 Pb+4 O-2 Pb2O4 PbO2 Lead (IV) Oxide Magnesium Sulfide Mg+2 S-2 Mg2S2 MgS Vanadium (V) Oxide V+5 O-2 V2O5

  23. Starter S-74 Name the following ions • Pb+2 • C2H3O2- • Mg+2 • Cl-

  24. 9.2 Naming & Writing Formulas: Ionic Polyatomic Ions – Use the same rules as other ionic compounds The endings do not change So to write the formula for • Write the formula and charge for Ammonium • Write the formula and charge for Carbonate NH4+1 Carbonate NH4+1 CO3-2 Ammonium Carbonate

  25. 9.2 Naming & Writing Formulas: Ionic Polyatomic Ions – Use the same rules as other ionic compounds The endings do not change So to write the formula for • Criss Cross • If the polyatomic ion has a subscript, parenthesis are placed around the polyatomic ion NH4+1 Carbonate NH4+1 CO3-2 NH42CO3 (NH4)2CO3 Ammonium Carbonate

  26. 9.2 Naming & Writing Formulas: Ionic Example 1 Example 2 Example 3 Example 4 Sodium Phosphate Na+ PO4-3 Na3PO4 Fe(H2PO4)3 Iron (III) Dihydrogen Phosphate Fe+3 H2PO4- (NH4)2O Ammonium Oxide NH4+ O-2 Cu(ClO4)2 Copper (II) Perchlorate Cu+2 ClO4-

  27. 9.2 Naming & Writing Formulas: Ionic So to write the name for • Name the first ion (check charges if it needs a roman numeral) • Name the second ion Ag2SO4 Silver SO4 Silver Sulfate Lead (IV) (NO3)4 Lead (IV) Nitrate Pb(NO3)4

  28. 9.2 Naming & Writing Formulas: Ionic Example 1 Example 2 Example 3 Example 4 Ammonium Dichromate (NH4)2Cr2O7 Ni2(C2O4)3 Nickel (III) Oxalate CaSiO3 Calcium Silicate Cobalt (II) Hydrogen Phosphate CoHPO4

  29. Starter S-76 Write the names for the following • Pt(NO2)2 Platinum (II) Nitrite B. Mg(ClO)2 Magnesium Hypochlorite Write the formula for the following • Cesium Carbonate Cs2CO3 • Copper (I) Suflite Cu2SO3

  30. 9.3 Naming & Writing Molecular Compounds Chapter 9

  31. 9.3 Naming & Writing Molecular Compounds Molecular Compounds (two non-metals) Prefixes are used to name the subscript in the molecular formula So to name • Never use mono on the first element • Prefix and element SiO2 Silicon O2 Silicon Dioxide

  32. 9.3 Naming & Writing Molecular Compounds Example 1 Example 2 Example 3 Example 4 Nitrogen Trichloride NCl3 Dinitrogen Tetrahydride N2H4 Cl2O7 Dichlorine Heptaoxide TetraPhosphorus Trisulfide P4S3

  33. 9.3 Naming & Writing Molecular Compounds Writing formulas invloves just writing the symbols and the prefixes • Write the first element with the proper subscript • Second element and subscript Carbon Tetrabromide C Tetrabromide CBr4

  34. 9.3 Naming & Writing Molecular Compounds Example 1 Example 2 Example 3 Example 4 P2O3 Diphosphorus Trioxide IF7 Iodine Heptafluoride NO Nitrogen Monoxide P4O6 Tetraphosphorus Hexaoxide

  35. Starter S-77 Write the names for the following • N2O5 Dinitrogen Pentaoxide B. CCl4 Carbon Tetrachloride Write the formula for the following • Xenon Hexafluoride XeF6 • Carbon Dioxide CO2

  36. Starter S-78 Write the names for the following • CO3-2 Carbonate B. H2PO4- Dihydrogen Phosphate Write the formula for the following • Hypochlorite ClO- • Dichromate Cr2O7-2

  37. 9.4 Naming & Writing Acids Chapter 9

  38. 9.4 Naming & Writing Formulas for Acids Acid – a compound that has one or more hydrogen atoms and produces hydrogen ions (H+) in solution The basic formula is Three rules for naming • When the anion (X) does not have Oxygen in it a. The name begins with hydro b. The anion’s name ends in –ic c. And the word acid is added to the end HnX Hydro Cl Hydrochloric Hydrochloric Acid HCl

  39. 9.4 Naming & Writing Formulas for Acids 2. When the anion (X) does have Oxygen and the polyatomic ion ends in -ite a. Use the name of the anion, but change the ending to –ous b. Add the word acid Sulfurous Sulfurous Acid H2SO3

  40. Oxygen? NO YES Hydro—ic acid Ending of Polyatomic Ion? -ate -ite --ous acid --ic acid 9.4 Naming & Writing Formulas for Acids 3. When the anion (X) does have Oxygen and the polyatomic ion ends in -ate a. Use the name of the anion, but change the ending to –ic b. Add the word acid H2SO4 Sulfuric Sulfuric Acid

  41. 9.3 Naming & Writing Molecular Compounds Example 1 Example 2 Example 3 Example 4 Chloric Acid HClO3 Hydrocyanic Acid HCN Nitric Acid HNO3 Chlorous Acid HClO2

  42. Oxygen? NO YES Hydro—ic acid Ending of Polyatomic Ion? -ate -ite --ous acid --ic acid 9.4 Naming & Writing Formulas for Acids To write the formulas, we go backwards through our list Acids always have an H+ ion Hydro means no Oxygen – so Fluoric means Fluoride H+ Hydrofluoric Acid H+ F- HF Hydrofluoric Acid

  43. Oxygen? NO YES Hydro—ic acid Ending of Polyatomic Ion? -ate -ite --ous acid --ic acid 9.4 Naming & Writing Formulas for Acids To write the formulas, we go backwards through our list Acids always have an H+ ion ous means the ion ended in ite, so phosphite H+ Phosphorous Acid Phosphorous Acid H+ PO3-3 H3PO3

  44. Oxygen? NO YES Hydro—ic acid Ending of Polyatomic Ion? -ate -ite --ous acid --ic acid 9.4 Naming & Writing Formulas for Acids To write the formulas, we go backwards through our list Acids always have an H+ ion ic means the ion ended in ate, so phosphate H+ Phosphoric Acid Phosphoric Acid

  45. 9.3 Naming & Writing Molecular Compounds Example 1 Example 2 Example 3 Example 4 HI Hydroiodic Acid HC2H3O2 Acetic Acid Hypochlorous Acid HClO Carbonic Acid H2CO3

  46. Starter S-79 Name the following • SO3 • Ag2SiO3 • H2SO3 Write the formula for • Nitrogen Triiodide • Lead (II) Acetate • Phosphorous Acid

  47. 9.5 The Laws Governing Formulas and Names Chapter 9

  48. 9.5 The Laws Governing Formulas and Names The Law of Definite Proportions – in any chemical compound, the masses of the elements are always in the same proportion The ratio of this molecule is always Or (Same Ratio) Carbon:Hydrogen 2.98:1.00 1.00:0.34

  49. 9.5 The Laws Governing Formulas and Names The Law of Multiple Proportions – Whenever the same two elements form multiple compounds, the different masses of one element that combine with the same mass of the other element are in the ratio of small whole numbers Huh? For example one compound A second compound might be The ratio of the two masses would be 5g A 10g A 2g B 2g B

  50. Starter S-80 Write • Copper (II) Acetate • Acetic Acid • Aluminum Dihydrogen Phosphate Name • HF • H2C2O4 • Zn(OH)2