2. Nomeclature One name for each substance, one substance for each (valid) name

3. If it is a… The nomenclature rules depend on what type of substance. There are several systems. 1.Ionic compounds 2.Covalent compounds 3.Acids 4.Organic chemicals (around Christmas) 5.Complex ions (around Spring Break)

4. Ionic compounds: Formula to name Name (don’t count) the ions. NaBr K 2 O (NH 4 ) 2 CO 3 FeS CrI 3

5. Ionic compounds: Formula to name Name (don’t count) the ions. NaBrsodium bromide K 2 Opotassium oxide (NH 4 ) 2 CO 3 ammonium carbonate FeSiron (II) sulfide CrI 3 chromium (III) iodide

6. Warnings Group metals (group 1 and 2 and aluminum) do not get a Roman numeral Count your charges to get the transition element charge. The Roman numeral is part of an ion’s name Watch out for Hg +2 vsHg 2 +2, O -2 vs O 2 -2

7. Ionic compounds: Name to formula Balance your charges Lithium chloride calcium bromide Aluminum sulfate cobalt (II) oxide nickel (III) nitrite

8. Ionic compounds: Name to formula Balance your charges Lithium chloride LiCl calcium bromide CaBr 2 Aluminum sulfateAl 2 (SO 4 ) 3 cobalt (II) oxide CoO nickel (III) nitriteNi(NO 2 ) 3

9. Warnings Use () when you double or triple a polyatomic ion Balance your charges

10. Prefixes 1.Mono- 2.Di- 3.Tri- 4.Tetra- 5.Penta- 6.Hexa- 7.Hepta- 8. Octo- 9. Nona- 10. Deca- 11. Undeca- 12. Dodeca- 13. Trisdeca- … 20. Icosa-

11. PS—Hydrated salts Hydrated salts are written with x H 2 0 They are named with (prefix)hydrate For example: Cobalt (II) chloride dihydrate = CoCl 2 2H 2 0

12. Covalent compounds: Formula to name Name the atoms, in order, with prefixes (ends in –ide) N 2 S 5 CCl 4 P 2 O 5 BF 3

13. Covalent compounds: Formula to name Name the atoms, in order, with prefixes (ends in –ide) N 2 S 5 dinitrogen pentasulfide CCl 4 carbon tetrachloride P 2 O 5 diphosphorus pentoxide BF 3 boron trifluoride

14. Warnings First element is named, second one ends in “–ide” An “a” or “o” is dropped from the prefix before “–oxide” The “mono-” prefix is omitted on the first atom

15. Covalent compounds: Name to formula Write the atoms, prefixes become subscripts nitrogen trichloride Arsenic trioxide Bromine monochloride Xenon tetrafluoride

16. Covalent compounds: Name to formula Write the atoms, prefixes become subscripts nitrogen trichloride NCl 3 Arsenic trioxideAsO 3 Bromine monochlorideBrCl Xenon tetrafluorideXeF 4

17. Acids If the anion name then the acid name ends in…. is…

18. Acids If the anion name then the acid name ends in…. is… --ideHydro___ic acid (hypo--) --iteHypo___ous acid --ite___ous acid --ate___ic acid (per--) –atePer___ic acid

19. Acids Formula to name HI is _________acid HBrO 4 is _________acid H 2 CO 3 is _________acid H 2 SO 3 is ________acid HClO is ___________acid

20. Acids Formula to name HI is hydroiodic acid HBrO 4 is perbromic acid H 2 CO 3 is carbonic acid H 2 SO 3 is sulfurous acid HClO is hypochlorous acid

21. Acids Name to formula ____is hydrocyanic acid ____ is periodic acid _____ is phosphoric acid _____ is nitrous acid ____ is hypoiodous acid

22. Acids Name to formula HCN is hydrocyanic acid HIO 4 is periodic acid H 3 PO 4 is phosphoric acid HNO 2 is nitrous acid HIO is hypoiodous acid

23. Mass 1 amu x Avogadro’s number = 1 g The formula mass is the mass of a formula.

24. What is the formula mass? BaCO 3 Zn 3 (PO 4 ) 2 NiCl 26H 2 O

25. What is the formula mass? Iron (II) hydroxide Diphosphorus pentoxide Hypochlorous acid

26. Mass  Mole 1 mole = Avogadro’s number of particles. Use the conversion: 1 mole = FM (in g)

27. How many moles? 12.8 g BaCO 3 5.65 ng Iron (II) hydroxide 7.45 kg NiCl 26H 2 O

28. What is the mass?.0153 mol Hypochlorous acid.15 mmol Zn 3 (PO 4 ) 2 5 mol NiCl 26H 2 O

29. Some more mole conversions 1. A sample of HC 2 H 3 O 2 has a mass of 20.0 g. How many atoms of carbon are present? 2. Calculate the mass of 1.50x10 20 formula units of RbI. 3. Calculate the number of ions in 1.00 gram of Pb(C 2 H 3 O 2 ) 2 4. A sample of H 3 CCOCH 3 has a mass of 20.0 g. How many moles of hydrogen are present? 5. Calculate the mass of 4.6 moles of I 2 (s).

30. One piece of general advice for the AP test: “When in doubt: Convert to moles” W H Bond

31. Mole conversions will include: Mass Particles (molecules, formula units, ions) Atoms (using subscripts in a formula) Volume of ideal gas at STP(1 mole=22.4L) Nonstandard conditions (n=PV/RT) Volume of a solution (n=Molarity x volume) (Electrical current and time—consider later)

32. % composition %= FM of all of that element x100% (of an FM of the compound element)

33. For example: FM MgSO 47H 2 0=246.48 g/mol %Mg= 24.31 g/mol x 100% = 9.86% 246.48g/mol %S = 32.06 g/mol x 100% = 13.01% 246.48g/mol %O= 11 x 16.00 g/mol x 100% = 71.41% 246.48g/mol %H= 14x1.008 g/mol x 100% = 5.73% 246.48g/mol

34. For example: FM MgSO 47H 2 0=246.48 g/mol %Mg= 24.31 g/mol x 100% = 9.86% 246.48g/mol %S = 32.06 g/mol x 100% = 13.01% 246.48g/mol %O= 11 x 16.00 g/mol x 100% = 71.41% 246.48g/mol %H= 14x1.008 g/mol x 100% = 5.73% 246.48g/mol Did you catch that?

35. What is the % composition of… HBr Fe(OH) 2 NaCN

36. What is the % composition of… CH 4 C 2 H 6 C 3 H 8 C 4 H 10

37. What is the % composition of… CH 4 =25.14%H74.86%C C 2 H 6 =20.12%H79.88%C C 3 H 8 =18.29%H81.71%C C 4 H 10 =17.34%H82.66%C

38. You will notice a similar effect with: HF HCl HBr HI

39. You will notice a similar effect with: HF = 5.04%H94.96%F HCl =2.76%H97.23%Cl HBr =1.24%H98.76%Br HI =.79%H99.21%I

40. You may also be given masses What is the % composition of a compound that is composed of 7.765 g H and 124.23 g O?

41. You may also be given masses What is the % composition of a compound that is composed of 7.765 g H and 124.23 g O? 5.88% H, 94.12% O

42. You may also be given masses What is the % composition of a compound that is composed of 7.765 g H and 124.23 g O? 5.88% H, 94.12% O It’s NOT water! (11%H,88%O)

43. To find an empirical formula Note: “empirical”–based on data, not theory.

44. To find an empirical formula Take the data (% or mass) and convert to moles. Divide by the smallest to find the simplest whole number ratio—the subscripts in the empirical formula.

45. For example: What is the empirical formula for a compound where a sample is found to contain 4.5156g H, 26.906g C and 11.946g oxygen?

46. For example: What is the empirical formula for a compound where a sample is found to contain 4.5156g H, 26.906g C and 11.946g oxygen? Warning: This will give you an empirical formula only. An estimate of the molar mass will give you the molecular formula.

47. For example: What is the empirical formula for a compound where a 4.3368 g sample is burned to form 9.8596 g CO 2 and 4.0362 g H 2 0

48. For example: What is the empirical formula for a compound where a 4.3368 g sample is burned to form 9.8596 g CO 2 and 4.0362 g H 2 0 Will probably be given as the gas volume at some conditions

49. For example: What is the empirical formula for a of a compound where a 3.309 g sample is burned to form 5.897 g CO 2 and 2.414 g H 2 0?

50. For example: What is the empirical formula for a of a compound where a 4.587 g sample is burned to form 11.451 g CO 2 and 5.625 g H 2 0?