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Chemistry: Mole intro
Transcript of Chemistry: Mole intro
1. define a mole as a counting unit of chemistry
2. identify relationships between different moles, mass, and representative particles
3. make calculations based on those relationships smallest particle of a substance that still retains its properties
IONIC CPDS: formula units
MOLECULAR CPDS: molecules amu: measures mass of single atoms
gram: SI unit of mass
mole: SI unit for measuring amount (count) of substance
6.02 x 10^23 Def.: the mass in grams of one mole of a substance (units: grams/mole) Molar Mass Find the molar masses:
Sodium Chloride representative
particles Use dimensional analysis
The mole is a counting unit...
How many sig figs? 1 mol equals... Calculate the number of molecules in 11.5 mol H2O. You try one... Did you get 6.92 x 10^24 molecules ? A couple other ways... If you needed 0.50 moles of zinc (Zn) for a lab, how many grams would you measure out? If you needed 1.500 x 10^23 molecules of water, how many grams would you measure out on the balance? Did you get 32.7 g ? Did you get 4.5 g? Let's Practice a bit 1) What is the mass of 2.5 x 10^20 atoms of fluorine (F)?
2) What is the molar mass of aluminum oxide?
3) What would be the mass of 0.0010 mol of aluminum oxide?