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Understanding Avogadro’s Number and the Concept of Moles in Chemistry

This resource covers the fundamental concept of moles and Avogadro’s number (6.022 x 10²³), which defines the quantity of atoms in one mole of a substance. It explains how to calculate grams for elements such as Carbon-12, Carbon-14, Lithium, Nitrogen, Sodium, and Magnesium. Readers will learn the significance of the mole in measuring elements and how to perform conversions between grams and atoms. This knowledge is essential for understanding stoichiometry and the composition of matter in chemistry.

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Understanding Avogadro’s Number and the Concept of Moles in Chemistry

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  1. Moles pp 129-133

  2. NOT! Star-Nosed Mole

  3. Amadeo Avogadro • Created the “counting unit” for atoms. • Avogadro’s Number • 6.022x1023 • 1mol = 6.022x1023

  4. Moles Measure Elements • 1mol Carbon-12 = 6.022x1023atoms of Carbon-12 • 1 mol Carbon-12 = 12.000000g • 1 mol Carbon-14 = 14.000000g • 1 mol C (in nature) = 12.0107g • Why?

  5. More Moles • 1 mol Li = 6.941g = 6.022x1023atoms Li • 1 mol N = 14.00674g = 6.022x1023 atoms Li • How many grams of Na in 1 mol Na? • How many atoms of Hydrogen in 1.00794g H ?

  6. Conversion • How many atoms of Mg in 13g of Mg ?

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