1. The Mole!

2. What is….
A pair?
A ream?
A couple?
A gross?
A dozen?

3. How do chemists count things?
In moles.

4. Origin:   1900- 1905 German Mol,  short for Molekül  (molecule)

6. What is a mole?
6.02x1023 of something

7. 602,000,000,000,000,000,000,000

9. It is estimated there is about 1 mole of grains of sand on earth.
1 mole of marshmallows would be enough marshmallows to make a 19 km (12 mi) thick layer of marshmallows covering the entire face of the Earth.
1 mole of popcorn kernels could be spread uniformly over the USA if the thickness of the layer was about 14 km (9 mi).
1 mole of donut holes would cover the earth and be 8 km (5 mi) deep.
1 mole of blood cells would be more than the total number of blood cells found in every human on earth.
1 mole of sheets of paper could form a million stacks from the surface of the earth, all that would pass the sun. 
1 mole of pennies could be distributed to all the currently- living people of the world so that they could spend a million dollars per hour every hour (day and night) for the rest of their lives. 

11. Why do chemists use the mole to count?
Atoms and molecules are ridiculously small.

12. What is the name of the number 6.02x1023?
Avogadro’s Number

13. Why are moles bad at
counting?
Because they only
know one number.

14. What is a formula unit? The smallest component of an IONIC compound.
(Metal and a nonmetal)
(May contain polyatomic ions)
(Acids)

15. What is a molecule? The smallest component of a COVALENT compound
(Only made up of nonmetals)

16. What is an atom?
A single element.
(From the Periodic Table)

17. How do we use Avogadro’s number?
To convert from moles to particles
Use the conversion that 1 mole = 6.02x1023 particles (atoms, molecules, formula units).

18. How do I do that? Use the conversion that
1 mole = 6.02x1023 particles (atoms, molecules, formula units).

19. 3.4 moles of NaCl= ? formula units

20. 8.765x1029 molecules = ? moles

21. 6.5 moles of Aluminum= ? Atoms

22. 5.7x1019 molecules Cl2 = ? moles

23. How do you find the mass of one mole?
You use the molar mass.

24. What is molar mass?
It is the mass of one mole of something.

25. How do you find molar mass?
Use the mass on the periodic table. Add each element’s mass.

26. I thought the mass on the PT was in amu.
The mass of one atom (p+ + no) is in amu.
The mass in grams is the mass of one mole of the same element.

27. How many decimal places will molar mass always have?

28. How do I write molar mass?
1 mole = _________________g

29. Examples: Zinc (II) Chloride Bromine Aluminum Diphosphorus pentoxide
Gallium acetate

30. How do I use molar mass in conversions?
1 mole = Molar mass g

31. How many moles are in 56.98g of AgI?

32. How many grams are in 75 moles of Copper (II) Sulfate?

33. How many moles are in 45.9g of sodium carbonate?

34. Can I use both conversions together?
Yes!
1 mole = ____(Molar mass)____ g
1 mole = 6.02x1023

35. Percent Composition
To find the Percent Composition you must know the Total Mass of the compound and the Individual Mass of each Element

36. Percent Composition
Total Element Mass x100 Molar Mass

37. Find the percentage of hydrogen and oxygen in water.

38. Find the percentage of each element in aluminum carbonate.