Ratio of Ratio of Sulfur Oxygen numbers masses Number of atoms Mass of the Number of atoms Mass of the of atoms of atoms in the sample sample in the sample sample 1 32.00 amu 1 16.00 amu 1:1 2:1 10 10 1 dozen 1 dozen 1 million 1 million 1 mole 32.00 grams 1 mole 16.00 grams Fill in the table in Model 2 in a similar fashion to the eggs table in Model 1. Divide the work evenly among group members. Reduce all to lowest whole numbers possible. ratios Circle the phrase below that completes the sentence. When two samples contain the same number of atoms _________________________. the masses of the samples will be equal. the ratio of the masses will be equal to the ratio of the masses. samples’ atoms’ In the front of the room, there is a container that contains a 32.00 g sample of sulfur. This is 1 mole of sulfur. how many atoms are in the bottle. Your group must reach Estimate consensus. (will it be a big number or a little number?) Record your number here. Read This! A long time ago chemists discovered what you have just discovered: The relative masses of the elements can be used to atoms. “count” If you measure out a sample equal to an average atomic mass in grams, you always end up atom’s with the same number of atoms. Chemists call that quantity the mole—a quantity of any sample whose mass is equal to its average atomic mass in grams.
Sulfur Oxygen Ratio of numbers of atoms Ratio of masses of atoms Number of atoms in the sample Mass of the sample Number of atoms in the sample Mass of the sample 1 32.00 amu 1 16.00 amu 1:1 2:1 10 10 1 dozen 1 dozen 1 million 1 million 1 mole 32.00 grams 1 mole 16.00 grams Fill in the table in Model 2 in a similar fashion to the eggs table in Model 1. Divide the work evenly among group members. Reduce all ratios to lowest whole numbers possible. Circle the phrase below that completes the sentence. When two samples contain the same number of atoms _________________________. the masses of the samples will be equal. the ratio of the samples’ masses will be equal to the ratio of the atoms’ masses. In the front of the room, there is a container that contains a 32.00 g sample of sulfur. This is 1 mole of sulfur. Estimate how many atoms are in the bottle. Your group must reach consensus. (will it be a big number or a little number?) Record your number here. Read This! A long time ago chemists discovered what you have just discovered: The relative masses of the elements can be used to “count” atoms. If you measure out a sample equal to an atom’s average atomic mass in grams, you always end up with the same number of atoms. Chemists call that quantity the mole—a quantity of any sample whose mass is equal to its average atomic mass in grams.
group_work_relative_mass_and_the_mole.docx