The Mole Chapter 7.

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Presentation transcript:

The Mole Chapter 7

Avogadro’s Number and the Mole 1) The mole is defined as the number of atoms in exactly 12 grams of carbon-12. 2) The number of particles in a mole is called Avogadro’s number. (6.02 x 1023) Elements – atoms Covalent Compounds – molecules Ionic Compounds – formula Units

Mole Analogies An Avogadro's number of standard soft drink cans would cover the surface of the earth to a depth of over 200 miles. If you had Avogadro's number of unpopped popcorn kernels, and spread them across the United States of America, the country would be covered in popcorn to a depth of over 9 miles. If we were able to count atoms at the rate of 10 million per second, it would take about 2 billion years 6.02 X 1023 Watermelon Seeds: Would be found inside a melon slightly larger than the moon.

Mole Analogies 6.02 X 1023 Donut Holes: Would cover the earth and be 5 miles (8 km) deep. 6.02 X 1023Pennies: Would make at least 7 stacks that would reach the moon. 6.02 X 1023 Grains of Sand: Would be more than all of the sand on Miami Beach. 6.02 X 1023 Blood Cells: Would be more than the total number of blood cells found in every human on earth.

Atomic Mass Mass of an atom Carbon 12.0 amu Oxygen 16.0 amu

Formula Mass The sum of all the atomic masses that make up a compound. H2O 18.0 amu CO2 44.0 amu

Molar Mass Mass in grams of one mole of an element or compound, is numerically equivalent to the atomic mass of monatomic elements and the formula mass of compounds and diatomic elements. (Unit = g/mol) Carbon Atomic mass = 12.0 amu Molar Mass = 12.0 g/mol H2O Formula mass = 18.0 amu Molar Mass = 18.0 g/mol

Moles and Gases Molar Volume – volume of one mole of a gas at standard temperature and pressure 1 mole of any gas has a volume of 22.4 L at standard temperature and pressure.

Conversions with molar volume

Percent Composition Mass of element in compound x 100 Mass of compound

Empirical Formula The formula that gives the simplest whole-number ratio of the atoms in a compound. Empirical Formula: CH3 Molecular Formula: C2H6 Molecular Formula: C6H12O6 Empirical Formula: CH2O

Molecular Formula Formula that gives the actual number of atoms of each elements in a molecular formula.