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The Mole

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  1. The Mole How We Can Accurately Measure Atoms

  2. Remember the Mass of an Atom • An AMU stands for atomic mass unit. • The AMU for any element or molecule is found by simply using the average mass value from the p. table • The AMU for carbon is 12.01115 • The AMU for Boron is 10.811

  3. What is a Mole? • Just like a dozen means 12 and a couple means two, the mole is an exact number of something • We use the mole because atoms are so small, it would be too difficult to work in quantities so high

  4. Avogadro’s number • In honor of Amedeo Avogadro di Quaregna, this exact quantity for the mole (mol) was named after the famous scientist • So how much is a mole you ask?

  5. Memorize it 6.02 x 1023

  6. So What’s This All Mean • If you measure 31g of phosphorous, you have one mole of phosphorous. • If you measure 32g of sulfur, you have one mole of sulfur • In both cases you measured 6.02 x 1023 atoms of each substance

  7. One Step Further • If I asked for one mole of NaCl how many grams would you need? • Na = 23 and Cl = 35 • 1 mole of NaCl would require 58 grams of the substance • If you measure out 58g, you just measured out 6.02 x 1023 molecules

  8. Gram Atomic Mass • The (gam) is the atomic mass of an element expressed in grams • (gam) values are average masses rounded off one place after the decimal point

  9. Gram Molecular Mass • (gmm) • Same concept as (gam) except we are dealing in compounds • 1 mole of SO3 has a mass of 80.1 g

  10. Gram Formula Mass • (gfm) • Formula mass expressed in grams • Ammonium carbonate • ((NH4)2CO3) • [14 + (1 x 4)]2 + 12 + (16 x 3) • gfm of ammonium carbonate is 96g

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