2. Unit 6 Ionic Compounds

3. Remember…  The electrons in the outermost level or shell are called… –Valence electrons  You can determine the number of valence electrons in the s & p blocks by looking at the… –Group number

4. Remember…  Atoms in the same column have the same properties because they have the same… –Outer electron configuration –Number of valence electrons

5. Stable Electron Configurations  Atoms want to be stable!  Stable = noble gas configuration –8 valence electrons (s 2 & p 6 )  Atoms are electrically neutral –Same # of protons and electrons –So neutral is not always stable….

6. Atoms and ions  So…some atoms will form ions to achieve that stable electron configuration  Ions are atoms, or groups of atoms, with a charge –Different # of protons and electrons  Only electrons can be added or removed since changing the number of protons changes the identity

7. Remember…  Elements differ by the number of protons  Isotopes differ by the number of neutrons  Ions differ by the number of electrons

8. Forming Ions  Some atoms LOSE electron(s) to achieve a noble gas configuration  More protons than electrons so it becomes a positively charged ion  + charged ion = Cation  Occurs in metals

9. Examples of Cations  Na – 11 electrons - 1s 2 2s 2 2p 6 3s 1 –1 valence electron – VERY reactive  Na + - 10 electrons - 1s 2 2s 2 2p 6 –Noble gas configuration - STABLE

10. Electron Dots For Cations  Metals have few valence electrons & lose them to become stable Ca

11. Electron Dots For Cations  Metals have few valence electrons & lose them to become stable Ca

12. Electron Dots For Cations  Metals have few valence electrons & lose them to become stable  Forming a positive ion (cation) Ca 2+

13. Forming Ions  Some atoms GAIN electron(s) to achieve a noble gas configuration  More electrons than protons so it becomes a negatively charged ion  Negatively charged ion = Anion  A Negative ION  Occurs in nonmetals

14. Examples of Anions  S – 16 electrons - 1s 2 2s 2 2p 6 3s 2 3p 4 –6 valence electrons = REACTIVE  S 2- - 18 electrons - 1s 2 2s 2 2p 6 3s 2 3p 6 –Noble gas configuration = STABLE

15. Electron Dots For Anions  Nonmetals have several valence electrons  They will gain electrons to fill outer shell. P P 3-

16. Practice  Use electron dot diagrams to show how the following form ions  Al  Cl KK OO

17. Periodic Trend for Ion Formation

18. Atomic Number # of protons # of electrons Cl Cl - K K +

19. Transition metals  WEIRD!  Form cations  Hard to predict the charge  Often will form more than 1 charge  Can’t form noble gas configuration b/c it would take too much energy  Still try to fill up orbitals or half orbitals

20. Examples  Zinc –1s 2 2s 2 2p 6 3s 2 3p 6 3d 10 4s 2  Zn 2+ –1s 2 2s 2 2p 6 3s 2 3p 6 3d 10 –Full 3 rd energy level  Fe 1s 2 2s 2 2p 6 3s 2 3p 6 3d 6 4s 2  Fe 2+ 1s 2 2s 2 2p 6 3s 2 3p 6 3d 5 4s 1  Fe 3+ 1s 2 2s 2 2p 6 3s 2 3p 6 3d 5

21. Naming ions  Follows IUPAC rules  Cations keep the name of the metal –Ca calcium –Ca 2+ calcium ion  Anions change ending to –ide –Cl chlorine –Cl 1- chloride (ion)

22. Naming Ions  Transition metals use Roman numerals to indicate the charge (always positive)  Fe 2+ = Iron (II) ion  Fe 3+ = Iron (III) ion

23. Polyatomic ions  Groups of atoms that stick together as a unit, and have a charge  Names often end in –ate or –ite  You need to memorize the following 6: –PO 4 3- phosphate –CO 3 2- carbonate –SO 4 2- sulfate –NO 3 - nitrate –OH - - hydroxide –NH 4 + - ammonium

24. Polyatomic Ions

25. Stable Electron Configurations  Atoms want to be stable!  Stable = noble gas configuration –8 valence electrons (s 2 & p 6 )  Also called the octet rule –In forming compounds, atoms try to obtain 8 electrons in the highest energy level

26. Achieving Stability  Forming ions  Bonding with other ions to form an ionic compound

27. Ionic Bonding  Anions and cations join together to form ionic compounds (AKA salts)  The bond is formed through the transfer of electrons to achieve noble gas configuration

28. Ionic Bonding NaCl 1+ 1-

29. Ionic Compounds (Salts)  Made up of –a positive and negative ion –a cation and an anion –a metal and a nonmetal (or polyatomic ion)  Simplest ratio of elements = formula unit

30. Properties of Ionic Compounds  Crystalline structure –A regular repeating arrangement of ions –Dissolves into electrolytes –Structure is rigid –Ions are strongly bonded (Legos)

31. Crystalline structure

32. Properties of Ionic Compounds  High melting points- because of strong forces between ions  Good conductors of electricity when dissolved in water or melted

33. Ionic Bonding - DOTS  All the electrons must be accounted for! CaP

34. Ionic Bonding CaP

35. Ionic Bonding Ca 2+ P

36. Ionic Bonding Ca +2 P Ca

37. Ionic Bonding Ca 2+ P 3- Ca

38. Ionic Bonding Ca 2+ P 3- Ca P

39. Ionic Bonding Ca 2+ P 3- Ca 2+ P

40. Ionic Bonding Ca 2+ P 3- Ca 2+ P Ca

41. Ionic Bonding Ca 2+ P 3- Ca 2+ P Ca

42. Ionic Bonding Ca 2+ P 3- Ca 2+ P 3- Ca 2+

43. Ionic Bonding Ca 3 P 2 “Formula Unit”

44. Practice  Use electron dot diagrams to show how the following elements make an ionic compound and write the formula unit  Mg and Cl

45. Practice  Na and N

46. Practice  Al and O

47. Writing formulas  Ionic compounds have no overall charge  So we add the correct subscripts to represent the # of atoms that balance the ions

48. Writing Formulas – Criss-Cross 1. Write the ions side by side. Fe 3+ S 2-

49. Writing Formulas – Criss-Cross 2. Draw arrows that cross each other. Fe 3+ S 2-

50. Writing Formulas – Criss-Cross 3. Put the charge at the ends of the arrows. Fe 3+ S 2- 23

51. Writing Formulas – Criss-Cross 4. Write the formula by using the numbers at the ends of the arrows as subscripts Fe 3+ S 2- 23 Fe 2 S 3

52. Writing Formulas – Criss-Cross  Make sure you reduce when needed! –Iron (II) Oxide

53. Using Polyatomic Ions  Same rules but put a bracket around the entire ion before adding the subscript  Na + OH - = NaOH  Mg 2+ OH - = Mg[OH] 2  Na + CO 3 2- = Na 2 CO 3  Cu 2+ PO 4 3- = Cu 3 [PO 4 ] 2

54. Naming AKA Nomenclature  First name the cation, then the anion  Cation –Usually the same name as the metal –If a transition metal (or Sn or Pb), name the metal and use a roman numeral for the charge of the ion.

55. Naming Ionic Compounds  Anion –Ends with –ide  If a polyatomic ion is in the compound, don’t change the name, just name it.

56. Examples  NaCl –Cation = Na (sodium) –Anion = Cl (chlorine) ide Sodium Chloride

57.  MgBr 2 –Cation = Mg (magnesium) –Anion = Br (bromine) ide Magnesium bromide

58.  NaOH –Cation = Na (sodium) –Anion = OH (hydroxide) Sodium hydroxide  MgSO 4  Cation = Mg (magnesium)  Anion = SO 4 (sulfate) Magnesium sulfate

59.  FeCl 2 –Cation = Fe (Iron) –Anion = Cl (chlorine) ide  Which iron is this?  Use split method OR Algebra method Iron (II) chloride

60. Name  Formula 1.Start by writing the symbols of each element. 2.Then add the charges of each ion. 3.Use subscripts to balance the charges. (criss cross, etc.)

61. Name  Formula  Sodium sulfide  Iron (III) chloride

62. Ionic Bonding  Ionic bonds form between… –Metals & Nonmetals  But it is possible for nonmetals to bond to each other –Covalent bond  And for metals to mix with each other –Alloy

63. Alloys SSolutions made by dissolving metal into other elements (usually metals) MMade by melting them together and cooling them IIf the atoms of the metals are about the same size, they substitute for each other CCalled a substitutional alloy

64. Metal A Metal B +  Substitutional alloy Bronze – Copper and Tin Brass- 60 % Copper 39% Zinc and 1%Tin 18 carat gold- 75% gold, 25%Ag or Cu

65. Alloys  If the atoms of the metals are different sizes, the small one will fit into the spaces of the larger one  Called an interstitial alloy

66. Metal A +  Metal B Interstitial Alloy Steel – 99% iron 1 % C Cast iron- 96% Iron, 4%C

67. Alloys  Making an alloy is still just a mixture  Blend the properties  Designed for a purpose

68. For Your Quiz  Valence electrons  Elements vs Isotopes vs Ions  Cation vs Anion  Naming Ions  KNOW YOUR POLYATOMIC IONS  Characteristic Properties of Salts  Ionic bond forms between….  Naming compounds/ writing formulas  Alloys