1. THE MOLE

2. TOO SMALL TO SEE Because atoms are so small, it makes more sense to measure large amounts of atoms in reactions. One mole of a substance contains the same number of particles as atoms in 12 grams of Carbon-12

3. THE AVAGADRO CONSTANT 1 mole of a substance contains 6.022 x 10 23 particles Thats 602 200 000 000 000 000 000 000 particles!!!

4. EQUATION To calculate the moles in a substance we use the following equation: Moles of Atoms = Mass/Relative Atomic Mass

5. R.A.M. Relative Atomic Mass is the A r value from the Periodic Table

6. QUESTION How many moles of atoms are there in 2.4 g of carbon?

7. ANSWER Moles of atoms = mass/R.A.M. = 2.4/12 = 0.2 moles

8. THE MAGIC TRIANGLE Using the magic triangle we can rearrange the equation to find mass instead of moles

9. QUESTION What is the mass of 0.1 moles of Carbon Atoms?

10. FOR A COMPOUND A compound has more than one type of atom, so we have to find the Relative Formula Mass (R.F.M.) We do this by adding the A r of the elements in the molecule. So the equation then becomes: Moles = Mass/R.F.M.

11. QUESTION How many moles are there in 8 g of copper(II) oxide (formula CuO)? 1. Find the RFM Cu = 64 O = 16 So the RFM of CuO is 80 ….then just follow the equation…

12. QUESTIONS How many moles of atoms are there in: 1.2 g of hydrogen 2.36 g of carbon 3.160 g of oxygen 4.14 g of nitrogen 5.0.19 g of flourine

13. QUESTIONS How many moles of molecules are there in: 1.26 g of H 2 O 2.170 g of NH 3 3.1.6 g of CH 4 4.O.2 g of C 2 H 6 5.16 g of NH 4 NO 3