2. Objective I can write the correct formula and name for ionic compounds

3. Ionic Bond – The attraction between a positively charged cation(s) and a negatively charged anion(s)

4. Compounds composed of two elements are called binary compounds. When writing the formula for a binary ionic compound, the positive charge of the cation must be equal to the negative charge of the anion. An ionic compound must be electrically neutral. For your notes: binary means two

5. Most ions appear as monatomic ions. The charge for most monatomic ions is related to their A Group number on the Periodic Table. Every element will lose or gain electrons to look like a noble gas – 8A group

6. 1A2A3A4A5A6A7A8A Li + Be 2+ N 3- O 2- F-F- Na + Mg 2+ Al 3+ P 3- S 2- Cl - K+K+ Ca 2+ As 3- Se 2- Br - Rb + Sr 2+ I-I- Cs + Ba 2+

7. The charge signs are always dropped The cation is usually written first. Ex.K + and Cl - combine in a one-to-one ratio (one K for every Cl) = KCl

8. Ex.Ca 2+ and Br - combine in a one-to-two ratio (one Ca for every two Br) = CaBr 2.

9. Crisscross method: the numerical charge of each ion is crossed over and used as a subscript for the other ion. Example: Fe 3+ O 2-

10. Crisscross method: the numerical charge of each ion is crossed over and used as a subscript for the other ion. ***The charge signs are always dropped*** Example: Fe 3+ O 2-

11. Crisscross method: the numerical charge of each ion is crossed over and used as a subscript for the other ion. ***The charge signs are always dropped*** Example: Fe 2 O 3

12. Crisscross method: the numerical charge of each ion is crossed over and used as a subscript for the other ion. ***The charge signs are always dropped*** Example: Fe 2 O 3

13. Practice on your own: 1.Mg 2+ N 3- 2.K + S 2- 3.Sr 2+ Cl - 4.Ba 2+ O 2-

14. Practice on your own: 1.Mg 2+ N 3- Mg 3 N 2 2.K + S 2- 3.Sr 2+ Cl - 4.Ba 2+ O 2-

15. Practice on your own: 1.Mg 2+ N 3- Mg 3 N 2 2.K + S 2- K 2 S 3.Sr 2+ Cl - 4.Ba 2+ O 2-

16. Practice on your own: 1.Mg 2+ N 3- Mg 3 N 2 2.K + S 2- K 2 S 3.Sr 2+ Cl - SrCl 2 4.Ba 2+ O 2-

17. Practice on your own: 1.Mg 2+ N 3- Mg 3 N 2 2.K + S 2- K 2 S 3.Sr 2+ Cl - SrCl 2 4.Ba 2+ O 2- Ba 2 O 2  BaO

18. Naming Cations: the name of a cation is the same as the name of the element. Sodium atom (Na)  sodium ion (Na + ) Lithium atom (Li)  lithium ion (Li + ) Aluminum atom (Al)  aluminum ion (Al 3+ )

19. Naming Anions: the name of an anion typically ends in –ide. Sulfur atom (S)  Chlorine atom (Cl)  Fluorine atom (F) 

20. Naming Anions: the name of an anion typically ends in –ide. Sulfur atom (S)  sulfide anion (S 2- ) Chlorine atom (Cl)  Fluorine atom (F) 

21. Naming Anions: the name of an anion typically ends in –ide. Sulfur atom (S)  sulfide anion (S 2- ) Chlorine atom (Cl)  chloride anion (Cl-) Fluorine atom (F) 

22. Naming Anions: the name of an anion typically ends in –ide. Sulfur atom (S)  sulfide anion (S 2- ) Chlorine atom (Cl)  chloride anion (Cl - ) Fluorine atom (F)  fluoride anion (F - )

23. Practice on your own: 1.Mg 3 N 2 2.K 2 S 3.SrCl 2 4.Ba 2 O 2  BaO

24. Practice on your own: 1.Mg 3 N 2 Magnesium nitride 2.K 2 S 3.SrCl 2 4.Ba 2 O 2  BaO

25. Practice on your own: 1.Mg 3 N 2 Magnesium nitride 2.K 2 SPotassium sulfide 3.SrCl 2 4.Ba 2 O 2  BaO

26. Practice on your own: 1.Mg 3 N 2 Magnesium nitride 2.K 2 SPotassium sulfide 3.SrCl 2 Strontium chloride 4.Ba 2 O 2  BaO

27. Practice on your own: 1.Mg 3 N 2 Magnesium nitride 2.K 2 SPotassium sulfide 3.SrCl 2 Strontium chloride 4.Ba 2 O 2  BaOBarium oxide

28. Polyatomic Ions: These are groups of atoms that behave as a un it and carry a charge. 1. Most polyatomic anions end in –ite or –ate. 2. Only two polyatomic anions end in –ide, hydroxide (OH) - and cyanide (CN) - For your notes: poly means ‘many’

29. 3. The most commonly occurring anions are given the ending -ate. 4. The anion ending in –ite indicates one less number of oxygen atoms in the anion. Polyatomic anions with Nitrogen: Nitrite = (NO 2 ) - Nitrate = (NO 3 ) - For your notes: Memory aid: -Ite is lite (the least)-ate is heavy,”ate a lot” (the higher) O O O N O O N

30. 4. Per- as a prefix usually indicates four oxygen atoms An Example: perchlorate (ClO 4 ) -

31. Six Common Polyatomic Ions to Memorize! NameFormula Charge hydroxideOH - nitrateNO 3 - chlorateClO 3 - carbonateCO 3 2- sulfateSO 4 2- phosphatePO 4 3-

32. Write the polyatomic ionic compound formulas Ca 2+ Nitrate (NO 3 ) - Mg 2+ Nitrite (NO 2 ) - Li + Sulfate (SO 4 ) 2-

33. Write the polyatomic ionic compound formulas Ca 2+ Nitrate (NO 3 ) - Ca(NO 3 ) 2 Mg 2+ Nitrite (NO 2 ) - Li + Sulfate (SO 4 ) 2-

34. Write the polyatomic ionic compound formulas Ca 2+ Nitrate (NO 3 ) - Ca(NO 3 ) 2 Mg 2+ Nitrite (NO 2 ) - Mg(NO 2 ) 2 Li + Sulfate (SO 4 ) 2-

35. Write the polyatomic ionic compound formulas Ca 2+ Nitrate (NO 3 ) - Ca(NO 3 ) 2 Mg 2+ Nitrite (NO 2 ) - Mg(NO 2 ) 2 Li + Sulfate (SO 4 ) 2- Li 2 (SO 4 )

36. Naming Polyatomic Ionic Compounds 1) Simply name the polyatomic ion. Polyatomic anions usually end in –ite or –ate.

37. Name the polyatomic ionic compounds Nitrate: (NO 3 ) - Ca(NO 3 ) 2 Nitrite: (NO 2 ) - Mg(NO 2 ) 2 Sulfate: (SO 4 ) 2 - Li 2 (SO 4 )

38. Name the polyatomic ionic compounds Nitrate: (NO 3 ) - Ca(NO 3 ) 2 Calcium Nitrate Nitrite: (NO 2 ) - Mg(NO 2 ) 2 Sulfate: (SO 4 ) 2 - Li 2 (SO 4 )

39. Name the polyatomic ionic compounds Nitrate: (NO 3 ) - Ca(NO 3 ) 2 Calcium Nitrate Nitrite: (NO 2 ) - Mg(NO 2 ) 2 Magnesium Nitrite Sulfate: (SO 4 ) 2 - Li 2 (SO 4 )

40. Name the polyatomic ionic compounds Nitrate: (NO 3 ) - Ca(NO 3 ) 2 Calcium Nitrate Nitrite: (NO 2 ) - Mg(NO 2 ) 2 Magnesium Nitrite Sulfate: (SO 4 ) 2 - Li 2 (SO 4 )Lithium Sulfate

41. Cations of Transition Metals Remember all metals form cations. Unlike the cations of group 1A, 2A and 3A metals, many of the cations of group B, the transition metals, have more than one common ionic charge. This also characteristic of Tin and Lead, the two metals in group 4A

42. Cations of Transition Metals For example: Iron forms two common cations: –Fe 2+ and Fe 3+ So, how can we distinguish these two cations of iron? –In the name of the cation, a roman numeral in parenthesis indicates the value of the charge. –When you say the cation, you include its charge in the name FormulaNameYou say….” Fe 2+ Iron(II) ion“Iron two ion” Fe 3+ Iron(III) ion“Iron three ion”

43. Practice – write the name or formula NameFormula Copper(I) ion Copper(II) ion Manganese(II) ion Co 3+ Pb 2+ Sr 2+ Cu +

44. Practice – write the name or formula NameFormula Copper(I) ionCu + Copper(II) ionCu 2+ Manganese(II) ionMn 2+ Cobalt(III) ionCo 3+ Lead(II) ionPb 2+ Strontium ionSr 2+ Copper(I) ionCu +

45. Forming compounds with transition metals Many transition metals form brightly colored compounds that have been used in making artist’s paints.

46. Forming compounds with transition metals Writing the formula when given the ions that combine Example: copper(II) and bromine –step 1:Write the symbols for the ions –step 2: Use the crisscross method

47. Forming compounds with transition metals Writing the formula when given the ions that combine Example: copper(II) and bromine –step 1:Write the symbols for the ions Cu 2+ Br - –step 2: Use the crisscross method Cu 2+ Br - CuBr 2

48. Forming compounds with transition metals Write the name when given the chemical formula. Example: CoF 3 –step 1: identify the cation and anion: Cobalt is the cation Fluoride is the anion –step 2: if the cation is a transition metal (d-block), un- crisscross to determine its charge –step 3: Write the cation name with its charge in roman numerals and name the anion.

49. Forming compounds with transition metals Write the name when given the chemical formula. Example: CoF 3 –step 1: identify the cation and anion: Cobalt is the cation Fluoride is the anion –step 2: if the cation is a transition metal (d-block), un- crisscross to determine its charge Cobalt’s charge is +3 –step 3: Write the cation name with its charge in roman numerals and name the anion. cobalt(III)fluoride

50. Practice – write the name or formula NameFormula Copper(I) Fluoride Copper(II) Fluoride Manganese(II) Phosphide Iron(III) Oxide PbCl 2 SrF 2 FeO

51. Practice – write the name or formula NameFormula Copper(I) FluorideCuF Copper(II) FluorideCuF 2 Manganese(II) PhosphideMn 3 P 2 Iron(III) OxideFe 2 O 3 Lead(II) ChloridePbCl 2 Strontium FluorideSrF 2 Iron(II) OxideFeO

52. Objective I can write the name or formula of a transition metal cation I can write the name or chemical formula of transition metal ionic compounds