2. Nomenclature PO 4 3- phosphate ion C 2 H 3 O 2 - acetate ion HC 2 H 3 O 2 Acetic Acid Adapted from www.chemistrygeek.com

3. 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)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 togetherMetallic– holds atoms of a metal together We will only learn how to name Ionic and Covalent Compounds

4. 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. 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

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

7. Monatomic Ions

8. 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

9. 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

10. 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

11. 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

12. Naming Type I Binary Ionic Compounds Rules - 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 Type I Compounds contain a metal from Group 1A, 2A, 3A or Zn, Ag, Cd or NH 4

13. Naming Type I Binary Ionic Compounds Examples: NaCl - sodium chloride ZnI 2 - zinc iodide Al 2 O 3 - aluminum oxide

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

15. Naming Type II Binary Ionic Compounds Type II Ionic Compounds either contain a Transition Metal or a metal from Group 4A or 5A -These metals can change their charge -A Roman Numeral is written in the name to indicate the charge on the ion Cu + copper(I) ion Fe +2 iron(II) ion Cu 2+ copper (II) ion Fe +3 iron(III) ion

16. Naming Type II Binary Ionic Compounds To determine the charge on these ions, analyze the subscript and charge on the anion 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 Once you know the name of the cation, name the anion as you would for Type I compounds

17. Examples of Older Names of Cations formed from Variable Charge Metals (you do not have to memorize these)

18. 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________________________

19. Ions that contain multiple atoms but behave as a unit and carry a charge Names often end in –ite or –ate NO 2 - is nitrite, NO 3 - is nitrate SO 3 -2 is sulfite, SO 4 -2 is sulfate You can make additional polyatomic ions by adding a H + to the ion!You can make additional polyatomic ions by adding a H + to the ion! CO 3 -2 is carbonateCO 3 -2 is carbonate HCO 3 – is hydrogen carbonateHCO 3 – is hydrogen carbonate A compound containing a polyatomic ion is called a ternary compound (three+ atoms)A compound containing a polyatomic ion is called a ternary compound (three+ atoms) KNO 3 is potassium nitrate, MgSO 4 is magnesium sulfateKNO 3 is potassium nitrate, MgSO 4 is magnesium sulfate Polyatomic Ions

20. NO 3 - nitrate ion NO 2 - nitrite ion Polyatomic Ions

21. IonNameIonName NH 4 + ammoniumCO 3 -2 carbonate NO 2 - nitriteHCO 3 - hydrogen carbonate NO 3 - nitrateClO - hypochlorite SO 3 -2 sulfiteClO 2 - chlorite SO 4 -2 sulfateClO 3 - chlorate HSO 3 - hydrogen sulfiteClO 4 - perchlorate HSO 4 - hydrogen sulfateC 2 O 4 -2 oxalate OH - hydroxideC2H3O2-C2H3O2- acetate CN - cyanideMnO 4 - permanganate PO 3 -3 phosphiteSiO 3 -2 silicate PO 4 -3 phosphateCrO 4 -2 chromate HPO 4 -2 hydrogen phosphateCr 2 O 7 -2 dichromate H 2 PO 4 - dihydrogen phosphateO 2 -2 peroxide

22. 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.

23. 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

24. 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)

25. Naming Ternary Compounds Contains at least 3 elements There MUST be at least one polyatomic ion (use the second capital letter rule) Use Roman numerals to indicate the ion’s charge when needed (transition, 4A and 5 A metals) Examples: NaNO 3 Sodium nitrate K 2 SO 4 Potassium sulfate Fe(HCO 3 ) 3 Iron (III) hydrogen carbonate

26. 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

27. 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

28. 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

29. 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)

30. 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.

31. 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

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

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

34. 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

35. 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

36. Overall strategy for naming chemical compounds.

37. A flow chart for naming binary compounds.

38. 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

39. 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

40. 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

41. 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

42. 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

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

44. Acid Nomenclature Flowchart

45. 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

46. 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 -

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

48. Write the Formula! Hydrobromic acidHydrobromic acid Nitrous acidNitrous acid Carbonic acidCarbonic acid Phosphoric acidPhosphoric acid Hydrotelluric acidHydrotelluric acid

49. Nomenclature Summary Flowchart

50. Now it’s Study Time DONE