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

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

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

7. 8.1 Molecular Compounds Some metals have more than one charge (oxidation number) They are named using the name and the charge 9.1 Naming Ions SymbolNameClassical Name Cu + Copper (I) Cuprous Cu 2+ Copper (II) Cupric Fe 2+ Iron (II) Ferrous Fe 3+ Iron (III) Ferric Pb 2+ Lead (II) Plumbous Pb 4+ Lead (IV) Plumbic

8. Monatomic Ions – only one atom Review Anions – negative ions 9.1 Naming Ions

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

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

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

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

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

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

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

16. 9.2 Naming & Writing Formulas: Ionic Chapter 9

17. Binary Compounds – composed of two elements and can be ionic or covalently bonded For Ionic names 1.Write the name of the cation first 2.Write the name of the anion 3.Change the ending of the anion to -ide 9.2 Naming & Writing Formulas: Ionic NaBrSodium BrSodium BromineSodium Bromide

18. 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 PbCl 4 PbCl 4 -1 9.2 Naming & Writing Formulas: Ionic

19. Name the cation Name the anion Change the ending to -ide PbCl 4 9.2 Naming & Writing Formulas: Ionic Lead (IV) Cl 4 Lead (IV) ChlorineLead (IV) Chloride

20. Example 1: Example 2: Example 3: Example 4: Na 2 S 9.2 Naming & Writing Formulas: Ionic Sodium SSodium SulfurSodium Sulfide CuOCopper (II) OCopper (II) OxygenCopper (II) Oxide ZnI 2 Zinc I 2 Zinc IodineZinc Iodide Fe 2 S 3 Iron (III) S 3 Iron (III) SulfurIron (III) Sulfide

21. Starter S-74 Write the names of the following ionic compounds A.FeCl 2 B.V 3 N 4 C.K 2 O D.Cu 2 S E.AgF

22. To write the formula from the name 1.Write the ions 2.Cross the values of the charges 3.Confirm it is the smallest ratio 9.2 Naming & Writing Formulas: Ionic Nickel (III) FluorideNi +3 F - NiF 3

23. Example 1: Example 2: Example 3: Example 4: 9.2 Naming & Writing Formulas: Ionic Calcium Bromide Ca +2 Br - CaBr 2 Lead (IV) Oxide Pb +4 O -2 Pb 2 O 4 PbO 2 Magnesium Sulfide Mg +2 S -2 Mg 2 S 2 MgS Vanadium (V) OxideV +5 O -2 V2O5V2O5

24. Polyatomic Ions – Use the same rules as other ionic compounds The endings do not change So to write the formula for 1.Write the formula and charge for Ammonium 2.Write the formula and charge for Carbonate 9.2 Naming & Writing Formulas: Ionic Ammonium Carbonate NH 4 +1 CarbonateNH 4 +1 CO 3 -2

25. Polyatomic Ions – Use the same rules as other ionic compounds The endings do not change So to write the formula for 3.Criss Cross 4.If the polyatomic ion has a subscript, parenthesis are placed around the polyatomic ion 9.2 Naming & Writing Formulas: Ionic Ammonium Carbonate NH 4 +1 CarbonateNH 4 +1 CO 3 -2 NH 42 CO 3 (NH 4 ) 2 CO 3

26. Example 1 Example 2 Example 3 Example 4 9.2 Naming & Writing Formulas: Ionic Sodium PhosphateNa + PO 4 -3 Na 3 PO 4 Iron (III) Dihydrogen PhosphateFe +3 H 2 PO 4 - Fe ( H 2 PO 4 ) 3 Ammonium OxideNH 4 + O -2 (NH 4 ) 2 O Copper (II) PerchlorateCu +2 ClO 4 - Cu(ClO 4 ) 2

27. So to write the name for 1.Name the first ion (check charges if it needs a roman numeral) 2.Name the second ion 9.2 Naming & Writing Formulas: Ionic Ag 2 SO 4 Silver SO 4 Silver Sulfate Pb(NO 3 ) 4 Lead (IV) (NO 3 ) 4 Lead (IV) Nitrate

28. Example 1 Example 2 Example 3 Example 4 9.2 Naming & Writing Formulas: Ionic (NH 4 ) 2 Cr 2 O 7 Ammonium Dichromate Ni 2 (C 2 O 4 ) 3 Nickel (III) Oxalate CaSiO 3 Calcium Silicate CoHPO 4 Cobalt (II) Hydrogen Phosphate

29. Starter S-76 Give the names for the following A.Pt(NO 2 ) 2 B.Mg(ClO) 2 Give the formula for the following A.Cesium Carbonate B.Copper (I) Suflite

30. Starter S-77 Name A.Pb(ClO 4 ) 4 B.Pb(NO 3 ) 2 Give the Formula A.Iron (III) Silicate B.Nickel (II) Fluoride

31. 9.3 Naming & Writing Molecular Compounds Chapter 9

32. 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 1.Never use mono on the first element 2.Prefix and element PrefixNumber Mono1 Di2 Tri3 Tetra4 Penta5 Hexa6 Hepta7 Octa8 Nona9 Deca10 SiO 2 Silicon O 2 Silicon Dioxide

33. 9.3 Naming & Writing Molecular Compounds Example 1 Example 2 Example 3 Example 4 NCl 3 Nitrogen Trichloride N2H4N2H4 Dinitrogen Tetrahydride Cl 2 O 7 Dichlorine Heptaoxide P4S3P4S3 TetraPhosphorus Trisulfide

34. 9.3 Naming & Writing Molecular Compounds Writing formulas invloves just writing the symbols and the prefixes 1.Write the first element with the proper subscript 2.Second element and subscript PrefixNumber Mono1 Di2 Tri3 Tetra4 Penta5 Hexa6 Hepta7 Octa8 Nona9 Deca10 Carbon TetrabromideC TetrabromideCBr 4

35. 9.3 Naming & Writing Molecular Compounds Example 1 Example 2 Example 3 Example 4 Diphosphorus Trioxide P2O3P2O3 Iodine Heptafluoride IF 7 Nitrogen Monoxide NO Tetraphosphorus Hexoxide P4O6P4O6

36. 9.4 Naming & Writing Acids Chapter 9

37. 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 1.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 HnXHnX HCl Hydro ClHydrochloricHydrochloric Acid

38. Starter S-78 Name A.N 2 O 3 B.SO 3 C.HF Give the Formula A.Dihydrogen monoxide B.Carbon Monoxide

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 H 2 SO 3 SulfurousSulfurous Acid

40. 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 H 2 SO 4 SulfuricSulfuric Acid Oxygen? NOYES --ous acid Ending of Polyatomic Ion? -ite -ate Hydro—ic acid --ic acid

41. 9.3 Naming & Writing Molecular Compounds Example 1 Example 2 Example 3 Example 4 HClO 3 Chloric Acid HCN Hydrocyanic Acid HNO 3 Nitric Acid HClO 2 Chlorous Acid

42. 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 Hydrofluoric Acid Oxygen? NOYES --ous acid Ending of Polyatomic Ion? -ite -ate Hydro—ic acid --ic acid H + Hydrofluoric AcidH + F - HF

43. 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 Phosphorous Acid Oxygen? NOYES --ous acid Ending of Polyatomic Ion? -ite -ate Hydro—ic acid --ic acid H + Phosphorous Acid H + PO 3 -3 H 3 PO 3

44. 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 Phosphoric Acid Oxygen? NOYES --ous acid Ending of Polyatomic Ion? -ite -ate Hydro—ic acid --ic acid H + Phosphoric Acid

45. 9.3 Naming & Writing Molecular Compounds Example 1 Example 2 Example 3 Example 4 Hydroiodic Acid HI Acetic Acid HC 2 H 3 O 2 Hypochlorous AcidHClO Carbonic AcidH 2 CO 3

46. 9.5 The Laws Governing Formulas and Names Chapter 9

47. 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:Hydrogen2.98:1:001:00:0.34

48. 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 2g B 10g A 2g B