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Chemical Measurements

In this unit, learn to distinguish between atomic mass, formula mass, and molar mass. Complete the "Formula Mass and Molar Mass" worksheet. Explore measurements in chemistry and calculate formula and molar masses.

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Chemical Measurements

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  1. Chemical Measurements Unit 1: Stoichiometry Chapter 10 – The Mole

  2. Monday, 2/2 Learning Target: Distinguish between atomic mass, formula mass and molar mass. Learning Outcome: Complete “Formula Mass and Molar Mass” Worksheet.

  3. Measurements in Chemistry We use measurements all of the time! Atomic Mass is a measurement that we have already used in class. units for atomic mass = atomic mass unit (amu) Used to express masses of atoms on a relative scale. We compare everything to carbon-12.

  4. Particle location Mass (amu) Mass (g) Proton Inside nucleus 1.0073=1 1.673X10 -24 Neutron Inside nucleus 1.0087=1 1.675X10 -24 Electron Outside nucleus 0.0006=0 7.109X10 -28

  5. Atomic Mass & Formula Mass Atomic Mass The weighted average of the masses of the existing isotopes of an element Ex. Carbon C 12.01 amu Formula Mass The sum of the atomic masses of all atoms in a compound Ex. Carbon Dioxide CO2 44.01 amu

  6. What is the formula mass for SO2? • S: 1 atom x 32.1 amu • O: 2 atoms x 16.0 amu • Formula Mass = 32.1 amu + 32.0 amu= 64.1 amu Calculating Formula Mass

  7. What is the formula mass for H2O2? • H: 2 atoms x 1.01 amu • O: 2 atoms x 16.0 amu Formula Mass = 2.02 amu + 32.0 amu = 34.02 amu Calculating Formula Mass

  8. Calculating Formula Mass Methylene chloride (CH2Cl2) is used as a solvent in paint strippers. What is the formula mass of methylene chloride? C: 1 atom x 12.01 amu H: 2 atoms x 1.01 amu Cl: 2 atoms x 35.45 amu Formula Mass = 12.01(1) + 1.01(2) + 35.45(2) = 85.0 amu

  9. Moving from AMU to grams The use of atomic mass units (amu) are impractical in the chemistry lab where the preferred unit of measurement is grams. Scientists needed to establish a relationship between # of atoms and masses of atoms.

  10. The Mole Definition The number of atoms of that element equal to the number of atoms in exactly 12.0 grams of carbon-12. Abbreviated mol (without the ‘e’) The number of atoms in one mole of atoms is always the same! Avogadro’s Number (N) 6.02 x 1023 atoms 602,000,000,000,000,000,000,000

  11. Same Number, Different Mass Element # atoms/mol mass of 1 mole Carbon 6.02x1023 atoms 12.01 g C Copper 6.02x1023 atoms 63.55 g Cu Tin 6.02x1023 atoms 118.71 g Sn Why do the amounts of each look different?

  12. Calculating Molar Mass Methylene chloride (CH2Cl2) C: 1 atom x 12.01 amu H: 2 atoms x 1.01 amu Cl: 2 atoms x 35.45 amu Formula Mass = 12.0(1) + 1.0(2) + 35.5(2) = 85.0 amu Molar Mass = 84.95 g/mol

  13. The number of molecules in 1mole of a molecular compound is 6.02 x 1023 (same as with atoms in a mole) • 1 mol of water (H2O) contains 1 mol of water molecules but 2 mol of hydrogen atoms and 1 mol oxygen. • How many moles of Ca2+ and F- are in 1 mole of calcium fluoride? • 1 mole of Ca2+ ions and 2 moles of F- ions Molecules and Moles

  14. Molar Mass Definition The mass in grams of 1 mole of a substance We calculate molar mass the same way as formula mass. Atomic/Formula Molar Mass Ex. Calcium 40.08 amu = 40.08 g/mol

  15. Same Number, Different MassPractice • What is the formula and molar mass for propane, C3H8? • C: 3 atoms x 12.01 amu = 36.03 amu • H: 8 atoms x 1.01 amu = 8.08 amu Formula Mass = 36.03 amu + 8.08 amu = 44.11 amu Molar Mass = 44.11 g/mol

  16. Same Number, Different MassPractice • What is the formula and molar mass for glucose, C6H12O6? • C: 6 atoms x 12.01 amu = 72.06 amu • H: 12 atoms x 1.01 amu = 12.12 amu • O: 6 atoms x 16.00 amu = 96.00 amu Formula Mass = 72.06 amu + 12.12amu + 96 amu = 180.18 amu Molar Mass = 180.18 g/mol

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