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Introduction to the Mole: A Fundamental Chemistry Lesson

Discover the concept of the mole in chemistry - a metric base unit defined uniquely as 6.02x10^23. Learn how to count particles, weigh samples, and measure gaseous volumes. Understand conversion factors, molar volume, Avogadro's number, and atomic mass. Practice calculating moles in samples of aluminum, magnesium, and oxygen gas. Utilize molar mass to determine formula units in an iron oxide sample. Grab your periodic table and calculator for this chem-to-go lesson!

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Introduction to the Mole: A Fundamental Chemistry Lesson

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  1. Defining and Calculating the Mole Chem-To-Go Lesson 24 Unit 6 You’ll want a periodic table and a calculator!

  2. WHAT IS A MOLE? • A metric base unit • Defined in 3 ways • Represents a specific number • Dozen = 12 • Pair = 2 • Mole = 6.02x1023 • A very LARGE number because atoms are very small

  3. Defining the Mole Counting particles in a sample Weighing a sample Measuring the volume of a gaseous sample

  4. CONVERSION FACTORS! Molar Volume Avogadro’s # Molar Mass Atomic Mass

  5. USING Molar mass • Aluminum (Al) is often used for structures such as high-quality bicycle frames. Compute the number of moles in a 10.0-g sample of aluminum.

  6. USING avogadro’s number • If a scientist uses 0.5 moles of Mg, how many atoms of Mg did she use?

  7. USING Molar Volume • During cellular respiration, a cell releases 0.25 mol of O2 gas. A container of what volume is needed to hold this gas?

  8. Applying all necessary definitions • Calculate the number of formula units in a 45.0 gram sample of FeO.

  9. See you in class!

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