1. Chemical bonds that result from the electrical attraction between large numbers of cations and anions Cation – ? Anion – ? Ionic bonds – REVIEW

2. Ionic bonds most commonly form between …? REVIEW Ionic bonds are made up of charged pieces (ions) … Ions can be made up of single atoms or groups of atoms bonded together (polyatomic ions)

3. Binary ionic compound – ionic compound consisting of only 2 elements (monatomic ions) Naming: Name the cation and add an ide ending to the anion

4. Examples: sodium and chlorine form… sodium chloride magnesium and oxygen form… magnesium oxide

5. What’s a binary ionic compound? Binary ionic compound – ionic compound consisting of only 2 elements (monatomic ions)

6. Bromine bonds with sodium Cesium bonds with oxygen Silver bonds with fluorine Sodium bromide Cesium oxide Silver fluoride

7. What type of compounds have we learned to name? How do you identify this type of compound?

8. chlorine bonds with lithium magnesium bonds with sulfur aluminum bonds with oxygen Lithium bromide Magnesium sulfide Aluminum oxide

9. Problem… names do not directly indicate ratio of ions… Answer… empirical formula Li 2 O NaCl MgF 2 Determining formulas – Crisscross method

10. 1. determine charges 2. Take away the +/- and crisscross them to determine subscripts

11. Determine the empirical formula for an ionic compound containing… potassium and fluorine calcium and fluorine cesium and sulfur aluminum and oxygen

12. Name the compounds formed when the following elements bond: 1.Calcium and fluorine 2.Chlorine and strontium 3.Silver and oxygen Write the formulas for the following compounds: 1.Lithium bromide 2.Barium chloride 3.Sodium oxide

13. Throwing in the transition metals: Use roman numerals if more than one charge is possible Roman numeral = charge, if none use sheet, then same as binary ionic compounds NAMING: FORMULAS:

14. The weird guys…

15. Throwing in the transition metals: FeO Au 2 S CuF 2 PbS SbF 3 NAMING: Work backwards - the overall charge in a compound must be 0

16. Throwing in the transition metals: Lead II oxide Silver bromide Ferric Chloride Formulas:

17. Throwing in the transition metals: FeO Au 2 S CuF 2 PbS SbF 3 NAMING: Work backwards - the overall charge in a compound must be 0

18. Throwing in the transition metals: Lead II oxide Silver bromide Ferric Chloride Formulas:

19. silver chloride iron III oxide copper II sulfide Formulas: NiF 2 Au 2 O 3 Cu 2 S NAMING:

20. cadmium chloride potassium oxide Formulas: Ni 2 O 3 BaF 2 NAMING:

21. Binary ionic compound – ionic compound consisting of only 2 elements (monatomic ions)

22. Binary Compound – A compound with 2 elements more than 2 atoms = OK (CaF 2 ) more than 2 elements NOT ok (NaCrO 4 )

23. Throwing in polyatomic ions: If formula has more than 2 eles. Names do not change (no ide-ending) ! a non-ide ending should clue you in (memorize hydroxide + CN -1 ) more than one ion = parenthesis NAMING: FORMULAS:

24. Check: Is the compound binary? Does it contain a transition metal? If yes, use your ion sheet!!!

25. Throwing in polyatomic ions: MgSO 4 (NH 4 ) 2 S NaOH CrSO 3 Zn 3 (PO 4 ) 2 NAMING:

26. Throwing in polyatomic ions: Calcium Sulfate Lithium Cyanide Magnesium Hydroxide Potassium Clorate FORMULAS:

27. potassium hydroxide Iron III carbonate Formulas: SnO 2 Co(NO 3 ) 2 NAMING: Day 3 3-7

28. calcium nitrate silver carbonate Formulas: Li 2 SO 3 Cu(OH) 2 NAMING:

29. sodium nitrite nickel III oxide magnesium chlorite Formulas: Pb(CO 3 ) 2 NAMING:

30. Iron III sulfite Formulas: Co 2 (CO 3 ) 3 NAMING:

31. Copper II nitrite Formulas: Zn 3 (PO 3 ) 2 NAMING:

32. Tin IV sulfite Formulas: CoPO 4 NAMING:

33. 1. Explain how you would determine the name for Pb(CO 3 ) 2. DETAILED EXPLANATION! What is the name?

34. 1. Is a compound of C bonded to H an ionic compound? WHY or WHY NOT? 2. Name me: +2 ion of Copper and a bromine ion combine 3. Write the formula for the ionic compound in # 2

35. 1.Write the formulas for the following: Cuprous Sulfide Ferric Carbonate Ammonium Nitrite 2.Write the names for the following: K 3 BO 3 Co(NO 2 ) 3 Ag 3 PO 4

36. Using Lewis dots to represent bonds (Lewis dots for compounds): NaCl Na Cl Shared electrons (bonds) are represented with a line

37. Naming: Acids are named for their anions Binary: hydro – anion base – ic ending – the word “acid” Acid - Compound that yields H + ions (always starts with an H) – molecular compounds that act like ionics

38. Naming: Acids are named for their anions Binary: hydro – anion base – ic ending – the word “acid” Non-binary: ate ending becomes ic, ite ending becomes ous Examples: HF HBrHNO 3 HNO 2

39. Naming: Acids are named for their anions Binary: hydro – anion base – ic ending – the word “acid” Non-binary: ate ending becomes ic, ite ending becomes ous Examples: Hydrochloric acid Sulfurous acid

40. HCl = hydrochloric acid HNO 3 = nitric acid HC 2 H 3 O 2 = acetic acid H 2 SO 4 = sulfuric acid H 3 PO 4 = phosphoric acid

41. Binary Molecular Compounds Based on Prefixes 1. Less electronegative first – prefix only if more than one atom 2. Second element – prefix, root of name, ending ide (if only two elements) 3.o or a @ the end of prefix is dropped if name begins with a vowel (monooxide, monoxide)

42. PAGE 281 Mono1 Di2 Tri3 Tetra4 Penta5 Hexa6 Hepta7 Octa8 Nona9 Deca10 Binary Molecular Compounds – prefix system

43. Write the Name: N 2 O 5 SbF 3 Dinitrogen pentoxide Antimony trifluoride Binary Molecular Compounds Write the Formula: Germanium tetraiodide diphosphorous trioxide GeI 4 P2O3P2O3

44. Binary Molecular Compounds Write the Name: As 2 O 5 ICl 3 diarsenic pentoxide iodine trichloride Write the Formula: carbon tetraiodide dinitrogen trioxide CI 4 N 2 O 3

45. Electrolyte – anything that conducts electricity when melted or dissolved in water