2. 4-1 Chp 4: Nomenclature PO 4 3- phosphate ion C 2 H 3 O 2 - acetate ion HC 2 H 3 O 2 Acetic Acid

3. 4-2 Forms of Chemical Bonds There are 3 forms bonding atoms:There are 3 forms bonding atoms: Ionic—complete transfer of 1 or more electrons from one atom to another (one loses, the other gains) – Usually between a metal and a non-metalIonic—complete transfer of 1 or more electrons from one atom to another (one loses, the other gains) – Usually between a metal and a non-metal Covalent—some valence electrons shared between atoms – usually between 2 or more non -metalsCovalent—some valence electrons shared between atoms – usually between 2 or more non -metals Metallic –a shared pool of valence electrons being attracted to all of the positives holds atoms of a metal togetherMetallic –a shared pool of valence electrons being attracted to all of the positives holds atoms of a metal together Most bonds are somewhere in between ionic and covalent.

4. 4-3 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

5. 4-4 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 NH 4 + + Cl - NH 4 Cl Ammonium chloride

6. 4-5 Predicting Charges on Monatomic Ions KNOW THESE !!!! +1 +2 -3 -2 -1 0 Cd +2

7. 4-6 Writing a Formula Write the formula for the ionic compound that will form between Ca and Cl . Solution: 1.Determine the charge on each ion 2.Balance charge with + and – ions 3.Write the positive ion of metal first, and the negative ion 4.Write the number of ions needed as subscripts

8. 4-7 Learning Check Write the correct formula for the compounds containing the following ions: 1. Li, S 2. Al, Br 3. Be, N

9. 4-8 Naming Compounds 1. Cation first, then anion 2. Monatomic cation = name of the element Ca 2+ = calcium ion 3. Monatomic anion = name of element with ending changed to -ide Cl  = chloride CaCl 2 = calcium chloride Binary Ionic Compounds:

10. 4-9 Learning Check Names the following binary compounds: Na 3 N KBr Al 2 O 3 MgS

11. 4-10 Transition Metals Most transition metals can have more than one possible charge,so they MUST have a Roman Numeral to indicate the charge on the cation (NOT the number of cations or anions, and NOT the subscript). 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

12. 4-11 Names of Variable Ions Transition metals and the metals in groups 4A and 5A (except Ag, Zn, Cd, and Al) REQUIRE a roman numeral in their name. 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

13. 4-12 Examples of Older Names of Cations formed from Transition Metals (you do NOT have to memorize these)

14. 4-13 Learning Check Name the following binary compounds with variable metal ions: FeBr 2 CuCl SnO 2 Fe 2 O 3 Hg 2 S

15. 4-14 NO 3 - nitrate ion NO 2 - nitrite ion Polyatomic Ions

16. 4-15 When balancing charges in an ionic compound,the polyatomic ion acts as a single unit of charge: N O O O 1-1- Mg 2+ N O O O 1-1- Mg(NO 3 ) 2

17. 4-16 Common Polyatomic Ions

18. 4-17 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)

19. 4-18 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

20. 4-19 Learning Check 1.aluminum nitrate 2. copper(II) nitrate 3.Iron (III) hydroxide 4. Tin(IV) hydroxide

21. 4-20 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

22. 4-21 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

23. 4-22 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 1.Sodium oxide 2.Calcium carbonate 3.Lead (IV) sulfide 4.Tin (II) nitride 5.Copper (I) phosphate 6.Mercury (II) fluoride

24. 4-23 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 Cu(ClO 3 ) 2 Ca 3 N 2 Al 2 (CO 3 ) 3 KBr BaF 2 CsOH

25. 4-24 Naming Molecular 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)

26. 4-25 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 (in this class, it’s NOT optional!). 3.Change the ending of the second element to -ide.

27. 4-26 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

28. 4-27 CCl 4 N 2 O SF 6 carbon tetrachloride dinitrogen monoxide sulfur hexafluoride Molecular Nomenclature: Examples

29. 4-28 arsenic trichloride dinitrogen pentoxide tetraphosphorus decoxide AsCl 3 N 2 O 5 P 4 O 10 More Molecular Examples

30. 4-29 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

31. 4-30 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

32. 4-31 Overall strategy for naming chemical compounds.

33. 4-32 A flow chart for naming binary compounds.

34. 4-33 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

35. 4-34 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

36. 4-35 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 1.N 2 O 2.K 2 S 3.Cu(NO 3 ) 2 4.Cl 2 O 7 5.Cr 2 (SO 4 ) 3 6.Fe 2 (SO 3 ) 3 7.CaO 8.BaCO 3 9.ICl

37. 4-36 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 1.Barium iodide 2.Tetraphosphorus trisulfide 3.Calcium hydroxide 4.Iron (II) carbonate 5.Sodium dichromate 6.Diiodine pentoxide 7.Copper (II) perchlorate 8.Carbon disulfide 9.Diboron tetrachloride

38. 4-37 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

39. 4-38 Acid Nomenclature Review No Oxygen  w/Oxygen An easy way to remember which goes with which… “In the cafeteria, you ATE something ICky”

40. 4-39 Acid Nomenclature Flowchart

41. 4-40 HBr (aq)HBr (aq) H 2 CO 3H 2 CO 3 H 2 SO 3H 2 SO 3 No oxygen, -ideNo oxygen, -ide Has oxygen, -ateHas oxygen, -ate Has oxygen, -iteHas oxygen, -ite  hydrobromic acid  carbonic acid  sulfurous acid Acid Nomenclature

42. 4-41 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 -

43. 4-42 Name ‘Em! HI (aq)HI (aq) HClHCl H 2 SO 3H 2 SO 3 HNO 3HNO 3 HIO 4HIO 4 Hydroiodic acid Hydrogen chloride (not aq!) Sulfurous acid Nitric acid Periodic acid

44. 4-43 Write the Formula! Hydrobromic acidHydrobromic acid Nitrous acidNitrous acid Carbonic acidCarbonic acid Phosphoric acidPhosphoric acid Hydrotelluric acidHydrotelluric acid HBr (aq) HNO 2 H 2 CO 3 H 3 PO 4 H 2 Te (aq)

45. Nomenclature Summary Flowchart

46. 4-45 Now it’s Study Time DONE

47. 4-46 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)