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Nomenclature Rules!

Nomenclature Rules!. Nomeclature. One name for each substance, one substance for each (valid) name. If it is a…. The nomenclature rules depend on what type of substance. There are several systems. Ionic compounds Covalent compounds Acids Organic chemicals (around Christmas)

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Nomenclature Rules!

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  1. Nomenclature Rules!

  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. • Ionic compounds • Covalent compounds • Acids • Organic chemicals (around Christmas) • Complex ions (around Spring Break)

  4. Ionic compounds: Formula to name • Name (don’t count) the ions. • NaBr • K2O • (NH4)2CO3 • FeS • CrI3

  5. Ionic compounds: Formula to name • Name (don’t count) the ions. • NaBr sodium bromide • K2O potassium oxide • (NH4)2CO3 ammonium carbonate • FeS iron (II) sulfide • CrI3 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 vsHg2+2, O-2 vs O2-2

  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 CaBr2 • Aluminum sulfate Al2(SO4)3 • cobalt (II) oxide CoO • nickel (III) nitrite Ni(NO2)3

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

  10. Mono- Di- Tri- Tetra- Penta- Hexa- Hepta- 8. Octo- 9. Nona- 10. Deca- 11. Undeca- 12. Dodeca- 13. Trisdeca- … 20. Icosa- Prefixes

  11. PS—Hydrated salts • Hydrated salts are written with • x H20 • They are named with (prefix)hydrate • For example: Cobalt (II) chloride dihydrate = CoCl2• 2H20

  12. Covalent compounds: Formula to name • Name the atoms, in order, with prefixes (ends in –ide) • N2S5 • CCl4 • P2O5 • BF3

  13. Covalent compounds: Formula to name • Name the atoms, in order, with prefixes (ends in –ide) • N2S5 dinitrogen pentasulfide • CCl4 carbon tetrachloride • P2O5 diphosphorus pentoxide • BF3 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 NCl3 • Arsenic trioxide AsO3 • Bromine monochloride BrCl • Xenon tetrafluoride XeF4

  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… • --ide Hydro___ic acid • (hypo--) --ite Hypo___ous acid • --ite ___ous acid • --ate ___ic acid • (per--) –ate Per ___ic acid

  19. AcidsFormula to name • HI is _________acid • HBrO4 is _________acid • H2CO3 is _________acid • H2SO3 is ________acid • HClOis ___________acid

  20. AcidsFormula to name • HI is hydroiodic acid • HBrO4 is perbromic acid • H2CO3 is carbonic acid • H2SO3 is sulfurous acid • HClOis 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 • HIO4is periodic acid • H3PO4is phosphoric acid • HNO2is nitrous acid • HIOis 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? • BaCO3 • Zn3(PO4)2 • NiCl2•6H2O

  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 BaCO3 • 5.65 ng Iron (II) hydroxide • 7.45 kg NiCl2•6H2O

  28. What is the mass? • .0153 mol Hypochlorous acid • .15 mmol Zn3(PO4)2 • 5 mol NiCl2•6H2O

  29. Some more mole conversions 1. A sample of HC2H3O2 has a mass of 20.0 g. How many atoms of carbon are present? 2. Calculate the mass of 1.50x1020 formula units of RbI. 3. Calculate the number of ions in 1.00 gram of Pb(C2H3O2)2 4. A sample of H3CCOCH3 has a mass of 20.0 g. How many moles of hydrogen are present? 5. Calculate the mass of 4.6 moles of I2(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 MgSO4•7H20=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: Did you catch that? • FM MgSO4•7H20=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

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

  36. What is the % composition of… • CH4 • C2H6 • C3H8 • C4H10

  37. What is the % composition of… • CH4= 25.14%H 74.86%C • C2H6= 20.12%H 79.88%C • C3H8= 18.29%H 81.71%C • C4H10= 17.34%H 82.66%C

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

  39. You will notice a similar effect with: • HF = 5.04%H 94.96%F • HCl = 2.76%H 97.23%Cl • HBr = 1.24%H 98.76%Br • HI = .79%H 99.21%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 CO2 and 4.0362 g H20

  48. For example: • What is the empirical formula for a compound where a 4.3368 g sample is burned to form 9.8596 g CO2 and 4.0362 g H20 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 3.309g sample is burned to form 5.897 g CO2 and 2.414 g H20?

  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 CO2 and 5.625 g H20?

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