2. 4-1 Chapter 5 - Ionic Bonding

3. 4-2 Bonds Chemical bond - forces of attraction that hold atoms together. The molecule is more stable than the separate ions/ atoms. Bond energy - the energy required to break (or form) a chemical bond. Energy is released when the bond is formed. Ionic bonds - bond formed by the attraction between oppositely charged particles (anion and cation) The transfer of one or more electrons from one atom to another

4. 4-3 Ionic Compounds Ionic compounds - a chemical compound that has an equal amount of positive and negative charges so the compound is electrically neutral. Formed by ionic bonds. Salt - an inorganic compound containing cations other than H + and anions other than OH - and O 2-.

5. 4-4 Properties of Salts All salts are made of ions and are held together by ionic bonds. Salts form a crystal lattice - an ordered packing 3- dimensional arrangement of atoms or ions in a crystal Crystalline versus amorphous- crystalline solids have a fixed arrangement of atoms while amorphous solids like talcum powder have haphazard/ random arrangement.

6. 4-5 Properties of Salts Salts do not melt or boil easily because of the strong attraction between ions Salts are hard and brittle Salts conduct electricity when melted or dissolved to form an aqueous solution (in water- aq.)

7. 4-6 Energy and Ionic Bonding Removing an electron from an atom requires an input of energy- Ionization energy Adding an electron to an atom releases energy- Electron Affinity Lattice energy - the energy released when the crystal lattice of an ionic solid is formed

8. 4-7 Nomenclature PO 4 3- phosphate ion C 2 H 3 O 2 - acetate ion HC 2 H 3 O 2 Acetic Acid

9. 4-8 Forms of Chemical Bonds There are 3 forms of bonding between atoms:There are 3 forms of bonding between atoms: Ionic—complete transfer of 1 or more electrons from one atom to another (one loses, the other gains)Ionic—complete transfer of 1 or more electrons from one atom to another (one loses, the other gains) Covalent—some valence electrons shared between atomsCovalent—some valence electrons shared between atoms Metallic – holds atoms of a metal together. Electrons form a common pool called sea of electrons.Metallic – holds atoms of a metal together. Electrons form a common pool called sea of electrons. Most bonds are somewhere in between ionic and covalent.

10. 4-9 Common Names A lot of chemicals have common names as well as the proper IUPAC name.A lot of chemicals have common names as well as the proper IUPAC name. Chemicals that should always be named by common name and never named by the IUPAC method are:Chemicals that should always be named by common name and never named by the IUPAC method are: H 2 Owater, not dihydrogen monoxideH 2 Owater, not dihydrogen monoxide NH 3 ammonia, not nitrogen trihydrideNH 3 ammonia, not nitrogen trihydride

11. 4-10 CATION + ANION ---> COMPOUND COMPOUND CATION + ANION ---> COMPOUND COMPOUND A neutral compound requires equal number of + equal number of + and - charges. A neutral compound requires equal number of + equal number of + and - charges. COMPOUNDS FORMED FROM IONS Na + + Cl - --> NaCl

12. 4-11 Predicting Charges on Monatomic Ions KNOW THESE !!!! +1 +2 -3 -2 -1 0 Cd +2

13. 4-12 Properties of Ionic Compounds Forming NaCl from Na and Cl 2 A metal atom can transfer an electron to a nonmetal.A metal atom can transfer an electron to a nonmetal. The resulting cation and anion are attracted to each other by electrostatic forces.The resulting cation and anion are attracted to each other by electrostatic forces.

14. 4-13 IONIC COMPOUNDS NH 4 + Cl - ammonium chloride, NH 4 Cl

15. 4-14 Some Ionic Compounds Mg 2+ + N -3 ----> Mg 3 N 2 magnesium nitride Sn 4+ + O 2- ----> SnO 2 Tin (IV) oxide calcium fluoride Ca 2+ + 2 F - ---> CaF 2

16. 4-15 Formulas of Ionic Compounds Formulas of ionic compounds are determined from the charges on the ions atoms ions     – Na  +  F :  Na + : F :  NaF     sodium + fluorine sodium fluoride formula Charge balance: 1+ 1- = 0

17. 4-16 Monatomic Ions

18. 4-17 Writing a Formula Write the formula for the ionic compound that will form between Ba 2+ and Cl . Solution: 1. Balance charge with + and – ions 2. Write the positive ion of metal first, and the negative ion Ba 2+ Cl  Cl  3. Write the number of ions needed as subscripts BaCl 2

19. 4-18 Writing BINARY FORMULAS 1.CANCEL CHARGES TO GET A TOTAL CHARGE OF ZERO. 2.CROSS- MULTIPLY TILL YOU GET THE LOWEST COMMON MULTIPLE. 3.WHAT YOU MULTIPLIED WITH IS YOUR SUBSCRIPT. 4.DO NOT WRITE CHARGES ON YOUR FINAL FORMULA. 5.METAL IS WRITTEN FIRST AND THEN NON- METAL. SIMPLEST FORMULA IS WRITTEN

20. 4-19 Learning Check Write the correct formula for the compounds containing the following ions: 1. Na +, S 2- a) NaS b) Na 2 Sc) NaS 2 2. Al 3+, Cl - a) AlCl 3 b) AlCl c) Al 3 Cl 3. Mg 2+, N 3- a) MgN b) Mg 2 N 3 c) Mg 3 N 2

21. 4-20 Solution 1. Na +, S 2- b) Na 2 S 2. Al 3+, Cl - a) AlCl 3 3. Mg 2+, N 3- c) Mg 3 N 2

22. 4-21 Naming Compounds 1. Cation first, then anion 2. Monatomic cation = name of the element Ca 2+ = calcium ion 3. Monatomic anion = root + -ide Cl  = chloride CaCl 2 = calcium chloride Binary Ionic Compounds:

23. 4-22 Naming Binary Ionic Compounds Examples: NaCl ZnI 2 Al 2 O 3 sodium chloride zinc iodide aluminum oxide

24. 4-23 Learning Check Complete the names of the following binary compounds: Na 3 Nsodium ________________ KBrpotassium________________ Al 2 O 3 aluminum ________________ MgS_________________________

25. 4-24 1.BaCl 2 2.NaF 3.Ag 2 O 4.CuBr 5.CuBr 2 6.FeO 7.Fe 2 O 3 8.MgS 9.Al 2 O 3 10.CaI 2 1.BaCl 2 2.NaF 3.Ag 2 O 4.CuBr 5.CuBr 2 6.FeO 7.Fe 2 O 3 8.MgS 9.Al 2 O 3 10.CaI 2 11. K 2 S 12. CrCl 2 13. CrCl 3 14. CaO 15. Ba 3 P 2 16. Hg 2 I 2 17. Na 2 O 18. BeS 19. MnO 20. Mn 2 O 3 11. K 2 S 12. CrCl 2 13. CrCl 3 14. CaO 15. Ba 3 P 2 16. Hg 2 I 2 17. Na 2 O 18. BeS 19. MnO 20. Mn 2 O 3 Name the ionic compounds

26. 4-25 Transition Metals Elements that can have more than one possible charge MUST have a Roman Numeral to indicate the charge on the individual ion. 1+ or 2+ 2+ or 3+ Cu +, Cu 2+ Fe 2+, Fe 3+ copper(I) ion iron(II) ion copper (II) ion iron(III) ion

27. 4-26 Names of Variable Ions These elements REQUIRE Roman Numerals because they can have more than one possible charge: anything except Group 1A, 2A, Ag, Zn, Cd, and Al (You should already know the charges on these!) Or another way to say it is: Transition metals and the metals in groups 4A and 5A (except Ag, Zn, Cd, and Al) require a Roman Numeral. FeCl 3 (Fe 3+ ) iron (III) chloride CuCl (Cu + ) copper (I) chloride SnF 4 (Sn 4+ ) tin (IV) fluoride PbCl 2 (Pb 2+ )lead (II) chloride Fe 2 S 3 (Fe 3+ )iron (III) sulfide

28. 4-27 Examples of Older Names of Cations formed from Transition Metals (you do not have to memorize these)

29. 4-28 Learning Check Complete the names of the following binary compounds with variable metal ions: FeBr 2 iron (_____) bromide CuClcopper (_____) chloride SnO 2 ___(_____ ) ______________ Fe 2 O 3 ________________________ Hg 2 S________________________

30. 4-29 NO 3 - nitrate ion NO 2 - nitrite ion Polyatomic Ions

31. 4-30 You can make additional polyatomic ions by adding a H + to the ion! CO 3 -2 is carbonate HCO 3 – is hydrogen carbonate H 2 PO 4 – is dihydrogen phosphate HSO 4 – is hydrogen sulfate Polyatomic Ions

32. 4-31 Ternary Ionic Nomenclature Writing Formulas Write each ion, cation first. Don’t show charges in the final formula. Overall charge must equal zero. If charges cancel, just write symbols. If not, use subscripts to balance charges. Use parentheses to show more than one of a particular polyatomic ion. Use Roman numerals indicate the ion’s charge when needed (stock system)

33. 4-32 Ternary Ionic Nomenclature Sodium Sulfate Na + and SO 4 -2 Na 2 SO 4 Iron (III) hydroxide Fe +3 and OH - Fe(OH) 3 Ammonium carbonate NH 4 + and CO 3 –2 (NH 4 ) 2 CO 3

34. 4-33 Learning Check 1. aluminum nitrate a) AlNO 3 b) Al(NO) 3 c) Al(NO 3 ) 3 2. copper(II) nitrate a) CuNO 3 b) Cu(NO 3 ) 2 c) Cu 2 (NO 3 ) 3. Iron (III) hydroxide a) FeOHb) Fe 3 OHc) Fe(OH) 3 4. Tin(IV) hydroxide a) Sn(OH) 4 b) Sn(OH) 2 c) Sn 4 (OH)

35. 4-34 Naming Ternary Compounds Contains at least 3 elements There MUST be at least one polyatomic ion (it helps to circle the ions) Examples: NaNO 3 Sodium nitrate K 2 SO 4 Potassium sulfate Al(HCO 3 ) 3 Aluminum bicarbonate or Aluminum hydrogen carbonate

36. 4-35 Learning Check Match each set with the correct name: 1. Na 2 CO 3 a) magnesium sulfite MgSO 3 b) magnesium sulfate MgSO 4 c) sodium carbonate 2.Ca(HCO 3 ) 2 a) calcium carbonate CaCO 3 b) calcium phosphate Ca 3 (PO 4 ) 2 c) calcium bicarbonate

37. 4-36 Mixed Practice! Name the following: 1.Na 2 O 2.CaCO 3 3.PbS 2 4.Sn 3 N 2 5.Cu 3 PO 4 6.HgF 2

38. 4-37 Mixed Up… The Other Way Write the formula: 1.Copper (II) chlorate 2.Calcium nitride 3.Aluminum carbonate 4.Potassium bromide 5.Barium fluoride 6.Cesium hydroxide

39. 4-38 Naming Molecular (Covalent) Compounds CH 4 methane BCl 3 boron trichloride CO 2 Carbon dioxide All are formed from two or more nonmetals. Ionic compounds generally involve a metal and nonmetal (NaCl)

40. 4-39

41. 4-40 Molecular (Covalent) Nomenclature for two nonmetals Prefix System (binary compounds) 1.Less electronegative atom comes first. 2.Add prefixes to indicate # of atoms. Omit mono- prefix on the FIRST element. Mono- is OPTIONAL on the SECOND element. 3.Change the ending of the second element to -ide.

42. 4-41 PREFIX mono- di- tri- tetra- penta- hexa- hepta- octa- nona- deca- NUMBER 1 2 3 4 5 6 7 8 9 10 Molecular Nomenclature Prefixes

43. 4-42 CCl 4 N 2 O SF 6 carbon tetrachloride dinitrogen monoxide sulfur hexafluoride Molecular Nomenclature: Examples

44. 4-43 arsenic trichloride dinitrogen pentoxide tetraphosphorus decoxide AsCl 3 N 2 O 5 P 4 O 10 More Molecular Examples

45. 4-44 Learning Check Fill in the blanks to complete the following names of covalent compounds. CO carbon ______oxide CO 2 carbon _______________ PCl 3 phosphorus _______chloride CCl 4 carbon ________chloride N 2 O_____nitrogen _____oxide

46. 4-45 Learning Check 1.P 2 O 5 a) phosphorus oxide b) phosphorus pentoxide c) diphosphorus pentoxide 2.Cl 2 O 7 a) dichlorine heptoxide b) dichlorine oxide c) chlorine heptoxide 3. Cl 2 a) chlorine b) dichlorine c) dichloride

47. 4-46 Overall strategy for naming chemical compounds.

48. 4-47 A flow chart for naming binary compounds.

49. 4-48 Mixed Review Name the following compounds: 1. CaO a) calcium oxideb) calcium(I) oxide c) calcium (II) oxide 2. SnCl 4 a) tin tetrachlorideb) tin(II) chloride c) tin(IV) chloride 3. N 2 O 3 a) nitrogen oxide b) dinitrogen trioxide c) nitrogen trioxide

50. 4-49 Solution Name the following compounds: 1. CaO 2. SnCl 4 3.N 2 O 3 a) calcium oxide c) tin(IV) chloride b) Dinitrogen trioxide

51. 4-50 Mixed Practice 1.Dinitrogen monoxide 2.Potassium sulfide 3.Copper (II) nitrate 4.Dichlorine heptoxide 5.Chromium (III) sulfate 6.Iron (III) sulfite 7.Calcium oxide 8.Barium carbonate 9.Iodine monochloride

52. 4-51 Mixed Practice 1.BaI 2 2.P 4 S 3 3.Ca(OH) 2 4.FeCO 3 5.Na 2 Cr 2 O 7 6.I 2 O 5 7.Cu(ClO 4 ) 2 8.CS 2 9.B 2 Cl 4

53. 4-52 Acid Nomenclature AcidsAcids Compounds that form H + in water.Compounds that form H + in water. Formulas usually begin with ‘H’.Formulas usually begin with ‘H’. In order to be an acid instead of a gas, binary acids must be aqueous (dissolved in water)In order to be an acid instead of a gas, binary acids must be aqueous (dissolved in water) Ternary acids are ALL aqueousTernary acids are ALL aqueous Examples:Examples: HCl (aq) – hydrochloric acidHCl (aq) – hydrochloric acid HNO 3 – nitric acidHNO 3 – nitric acid H 2 SO 4 – sulfuric acidH 2 SO 4 – sulfuric acid

54. 4-53 Acid Nomenclature Binary  Ternary An easy way to remember which goes with which… “In the cafeteria, you ATE something ICky”

55. 4-54 Acid Nomenclature Flowchart

56. 4-55 HBr (aq)HBr (aq) H 2 CO 3H 2 CO 3 H 2 SO 3H 2 SO 3 2 elements, -ide2 elements, -ide 3 elements, -ate3 elements, -ate 3 elements, -ite3 elements, -ite  hydrobromic acid  carbonic acid  sulfurous acid Acid Nomenclature

57. 4-56 hydrofluoric acidhydrofluoric acid sulfuric acidsulfuric acid nitrous acidnitrous acid 2 elements2 elements 3 elements, -ic3 elements, -ic 3 elements, -ous3 elements, -ous  HF (aq)  H 2 SO 4  HNO 2 Acid Nomenclature  H + F-  H + SO 4 2-  H + NO 2 -

58. 4-57 Name ‘Em! HI (aq)HI (aq) HClHCl H 2 SO 3H 2 SO 3 HNO 3HNO 3 HIO 4HIO 4

59. 4-58 Write the Formula! Hydrobromic acidHydrobromic acid Nitrous acidNitrous acid Carbonic acidCarbonic acid Phosphoric acidPhosphoric acid Hydrotelluric acidHydrotelluric acid

60. Nomenclature Summary Flowchart

61. 4-60 Now it’s Study Time DONE

62. 4-61 Rainbow Matrix Game Link on Chemistry Geek.com on Chemistry I page http://chemistrygeek.com/rainbow Use [ ] to represent subscripts since you can’t enter subscripts into the computer So H 2 O would be H[2]O And Al 2 (SO 4 ) 3 would be Al[2](SO[4])[3] Additional Polyatomic Ions (you do not have to memorize these, but they are in the game!) Borate = BO 3 -3 ; Silicate = SiO 4 -4 ; Manganate = MnO 4 -2 (permanganate is -1)