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Avogadro’s Number

Learn about Avogadro's number, mole calculations, formula mass, molar mass, empirical and molecular formulas, crystal lattices, and types of substances.

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Avogadro’s Number

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  1. Avogadro’s Number 6.02 X 1023

  2. 1 Mole of anything 6.02 X 1023 of that thing

  3. Can be:- atoms- molecules- ions Particles

  4. 0.5 Mole 3.01 X 1023

  5. 0.25 Mole 1.50 X 1023

  6. 2.0 Mole 12.04 X 1023 Or 1.204 X 1024

  7. 1.0 Mole of any gas at STP 22.4 Liters

  8. STP Standard Temperature = 0C Standard Pressure = 1 atm

  9. 0.5 mole of any gas 11.2 Liters

  10. 2.0 mole of any gas 44.8 Liters

  11. 3.0 mole of any gas 67.2 Liters

  12. 0.25 mole of any gas 5.6 Liters

  13. Formula Mass Sum of the masses of the elements in the compound. Expressed in atomic mass units

  14. Formula Mass of H2O 2 X H = 2 X 1.0 = 2.0 1 X O = 1 X 16.0 = 16.0 Sum = 18.0 amu’s

  15. Formula Mass of NH3 3 X H = 3 X 1.0 = 3.0 1 X N = 1 X 14.0 = 14.0 Sum = 17.0 amu

  16. Formula Mass of CO2 1 X C = 1 X 12.0 = 12.0 2 X O = 2 X 16.0 = 32.0 Sum = 44.0 amu

  17. Gram Formula Mass Formula mass expressed in grams. Equals the molar mass of the compound.

  18. Molar Mass Mass of one mole of the substance.

  19. 18.0 grams 17.0 grams 44.0 grams Molar Mass H2O = NH3 = CO2 =

  20. N: 2 S: 1 H: 8 O: 4 Count up the atoms in (NH4)2SO4 For Paren: SubInside X Suboutside

  21. Count up the atoms in 2Mg3(PO4)2 Mg: 6 P: 4 O: 16 The “2” applies to every element in the formula. For Paren: SubInside X Suboutside Coefficients X subs in formula

  22. MOLE MAP # of Grams  by formula mass X Formula Mass # of Moles X 22.4 L/mole • by 6.02 X 1023  by 22.4 X 6.02 X 1023 # of Particles # of Liters (gas)

  23. Percent Part X 100% Whole

  24. Percent H in H2O Part X 100% = 2 X 100% Whole 18

  25. Percent O in H2O Part X 100% = 16 X 100% Whole 18

  26. Empirical Formula smallest whole number ratio of the elements in a compound

  27. Molecular Formula Gives exact composition of molecule

  28. Covalent Compound Formula contains all nonmetals

  29. Molecular (vast majority)&Network (SiO2, SiC, Cdia, Cgraph) Types of covalent substances

  30. Ionic Compound Formula contains metal plus nonmetal

  31. Hydrate Ionic compound that has H2O molecules incorporated into its structure.

  32. Anhydrate Substance that remains after the water is removed from a hydrate.

  33. CuSO4•5H2O Formula of a hydrated salt. • means “is associated with.” H2O molecules are stuffed in the empty spaces.

  34. anhydrate Evaporates into air CuSO4·5H2O  ? CuSO4 + 5H2O  hydrate Heat to constant mass

  35. Formula mass of CuSO4•5H2O Mass of CuSO4plus mass of 5 water molecules. 249.6 grams/mole

  36. Percent H2O in CuSO4•5H2O(from the formula) Part X 100% = 90 X 100% Whole 249.6

  37. Metals All elements to the left of the staircase except H

  38. Nonmetals All elements to the right of the staircase plus H

  39. Binary Compound Compound made from 2 elements

  40. Which formulas are empirical? H2O H2O2 CH4 C2H6 C6H12O6 KCl P4O10 CaF2

  41. Crystal Lattices Ionic Compounds, Metals, & Network Solids make….

  42. Smallest repetitive unit in a crystal lattice Formula Unit

  43. Have distinctly different properties than molecular substances. Substances with crystal lattices…

  44. Types of Substances

  45. Ionic, Metallic, and Network solids What kind of substances have Crystal Lattices?

  46. Empirical formulas only Substances that make crystal lattices have

  47. Have both empirical & molecular formulas. The molecular formula is a whole-number multiple of the empirical formula. Molecular Covalent Substances

  48. Given empirical formula & Formula Mass, find Molecular Formula Find empirical mass Divide formula mass/empirical mass Multiply subscripts in empirical formula by answer in step 2

  49. Empirical formula = CH & Formula Mass = 78, find Molecular Formula Empirical mass = 13 Divide formula mass/empirical mass = 78/13 = 6 Multiply subscripts: C6H6

  50. 12 grams of hydrated salt is heated to constant mass. After heating the mass is 8.0 grams. What is the percent salt & the percent H2O? Percent water in hydrate from experimental data. Mass of H2O = 12 – 8 = 4 g Percent H2O = 4/12 X 100% Percent salt = 8/12 X 100%

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