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The Mole

The Mole. Chapter 11. Particles Names. Atoms, formula units (ionic compounds), molecules (covalent compounds). Counting units. 1mole = 6.02 x 10 23 particles. Mole to Particle Conversions. How many molecules of water are there in 2.4 moles of water?

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The Mole

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  1. The Mole Chapter 11

  2. Particles Names Atoms, formula units (ionic compounds), molecules (covalent compounds) Counting units 1mole = 6.02 x 1023 particles

  3. Mole to Particle Conversions How many molecules of water are there in 2.4 moles of water? How many moles of copper contain 3.5 x 1018 copper atoms?

  4. Volume and the Mole According to Avogadro, the mass of one mole of a gas at STP is always 22.4L regardless of the gas’ identity. STP = Standard Temperature and Pressure (0oC and 1 atmosphere)

  5. Mass and the Mole The mass of one mole of a substance is unique to that substance and is based on the sum of the atomic masses of the elements in that substance. 1 mole of copper = 63.6g 1 mole of lead = 207.2g 1 mole of water = 18.0g Mass of H2O = mass of two hydrogen atoms + mass of one oxygen atom

  6. Percent Composition by Mass Sum of the product of the number of each atom and their masses divided by the total mass of the compound What is the percent composition of Mg(BrO4)2? 1(mass Mg) + 2(mass of Br) + 8(mass of oxygen) = Mass of Mg(BrO4)2

  7. Empirical Formula Chemical formula which contains the lowest whole number ratio of atoms Ionic formulas always contain the lowest whole number ratios Covalent compounds do not always contain the lowest whole number ratios What is the Empirical Formula of the following compounds? C6H12O6 C3H9O6 H2O2

  8. Determining the Empirical Formula of a Compound NxOy What is the empirical formula for a compound which contains 25.9% nitrogen and 74.1% oxygen by mass? Assume a 100g sample. In that sample 25.9 g is nitrogen and 74.1g is oxygen • Covert % to mass (if needed) • Convert mass to moles • Divide each molar quantity by the lowest number of moles • Multiply by the smallest number needed to create a whole number ratio (if needed) N1.85O4.63 N1O2.5 N2O5 N1x2O2.5x2

  9. Which of the following are empirical formulas and which represent molecular formulas? C2H8 C2H8N2 H3PO4 C8H12O4 Li2SO4 CH4

  10. Simple Molecular Problems What is the molecular formula of a compound with an empirical formula of CH2O and a molecular mass of 90g/mol? • Determine the empirical mass • Divide the molecular mass by the empirical mass to determine how much larger the mass of the molecule is compared to the empirical formula • Multiple the subscripts of each element in the empirical formula by the factor determined in #2 CH2O =1(12g)+2(1g)+1(16g) = 30g C3H6O3 C1x3H2x3O1x3

  11. Longer Molecular Problems • Determine the molecular formula • Given the molecular mass, determine the molecular formula Determine the molecular formula of a compound that has a mass of 34g and contains 94.1% oxygen and 5.9% hydrogen by mass.

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