Drill – 10/14 How many decigrams are in 3.0 lbs of potatoes? (1 lb = 453.6 g)

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Presentation transcript:

Drill – 10/14 How many decigrams are in 3.0 lbs of potatoes? (1 lb = 453.6 g)

Objective SWBAT define the mole and describe its importance SWBAT describe how Avogadro’s number is related to a mole of any substance SWBAT define and calculate the molar mass of a substance

Atomic Conversions

Atomic Mass Units (amu) Average Atomic Mass and Mass Number have the units of amu. We do not use kilograms or grams, because this would be a VERY small number. Proton = 1.7x10-27 kg Neutron = 1.7x10-27 kg Electron = 9.1x10-31 kg

Atomic Mass Unit (amu) A relative mass is used to make calculations more manageable. Carbon-12 was arbitrarily chosen to be the standard.

Carbon is 12 times as large as hydrogen Carbon is 12 times as large as hydrogen. So Carbon was set at 12 amu and hydrogen was 1 amu C H (1 amu is equal to 1/12th of the mass of a Carbon-12 atom. Since Carbon-12 has 6 protons and 6 neutrons, this sets the relative mass for each particle at 1 amu.)

Atomic Conversions (don’t copy) Most measurements in the lab will be in macroscale quantities – grams or kilograms. The amu scale allows us to convert from mass in grams to number of particles. We do this by using the mole, Avogadro’s number, and molar mass.

The Mole Mole is the SI unit for amount of substance (mol). The mole is a counting unit, just like a dozen or a baker’s dozen or a ream. The mole is equal to the amount of particles in 12 grams of Carbon-12.

There are 6.022 x 1023 particles in 1 mole

Avogadro’s Number The number of particles in one mole has been determined to be 6.022x1023. 1 mole contains A LOT of particles!

Carbon is 12 times larger than hydrogen Carbon is 12 times larger than hydrogen. So if you have the same number of atoms of each, the mass of the carbon will always be 12 times larger than the mass of hydrogen C H The same number of atoms are in 12 g of Carbon as there are in 1 g of hydrogen … we named this amount a MOLE

Molar Mass Molar Mass is the mass of one mole of a pure substance. Molar Mass has the units of grams/mole or g/mol. Molar mass is numerically equal to the atomic mass of the element in atomic mass units (same number, different units!)

We now know that: 1 mole of a substance = 6.022 x 1023 particles of that substance The molar mass is the amount of grams of substance in 1 mole of that substance. How can I use these values to convert from mass in grams to particles?

How many moles are in 8.4×1017 atoms of Sodium? How many grams are in 8.4×1017 atoms of Sodium?

How many grams are in 6.90 moles of sulfur?

Green Workbook Do every #1a on pages 50-58 on your own paper Use your agenda book periodic table on pg. 135