2. How big is a mole? (Not the animal, the other one.) - Daniel Dulek TED TALK https://www.youtube.com/watch?v=TEl4je ETVmghttps://www.youtube.com/watch?v=TEl4je ETVmg

3. 6.02x10 23 Avogadro’s Number

4. MoleMole A mole is just a number like… Pair = 2Trio = 3 Dozen = 12Baker’s dozen = 13 Gross = 144Score= 20 Century=100Ream=500 mole = (mol) 602000000000000000000000

5. 9.12 x 10 13 How BIG is a mole? There are ~ 6.6 billion people on Earth How many Earths would it take to equal the population of 1 mole?

6. If you spent $800 billion dollars a day how many years would it take to spend a MOLEion dollars? 2.06 x 10 9 years

7. If you had a mole of cats... They would create a sphere larger than Earth!

9. If you had a mole of H 2 O could you swim in it? NO!  Water molecules are so small that a mole of H 2 O = 18ml

10. In chemistry we don’t work with individual atoms or molecules because they are too small to be weighed or measured We have to work with LOTS of atoms in order to measure them THAT’s WHERE THE MOLE COMES IN!

11. How small are atoms? There are more atoms in one gram of salt than grains of sand on all the beaches of all the oceans in all the world.

13. Mole Song https://www.youtube.com/watch?v= PvT51M0ek5c

14. Gram ATOMic Mass mass is in grams of 1 mole of atoms of an element In other words…… 1 mol C atoms = 6.02 x 10 23 C atoms = 12g C of the in

15. Practice Remember... 1 mole = 6.02x10 23 atoms or molecules = ______ g from the periodic table

16. Stoich iometry of Chemical Formulas

17. Gram Formula Mass Gram Molecular Mass Molar Mass mass in grams of 1 mole of a substance In other words... Add it all up! 1 mole of NaCl = 58g = 6.02 x 10 23 particles of NaCl 1 mole of H 2 O = 18g = 6.02x10 23 molecules of H 2 0 of the in

18. Now….. Use the gram formula mass and the gram atomic mass to determine –how many moles or atoms of an element are found in some mass of a substance –how much mass that element contributes to the mass of the entire substance Use factor label & follow the units!

19. Stoich iometry of Chemical Formulas If you have 1 molecule of (NH 4 ) 2 SO 4 –How many atoms of N are there? –How many atoms of H? –S? –O? –Total weight?

20. Practice Remember... 1 mole = 6.02x10 23 atoms or molecules = ______ gfm from the pt

21. Gases ONLY @STP Molar Volume 1 mole of ANY gas O 2 (g) NH 3 (g) H e (g) contains 6.02 x 10 23 molecules and occupies a volume of 22.4L

22. STP s tandard t emperature & p ressure 0 o C or 273K 101.3kPa or 1 atm

23. Remember... Gases also have mass 1 mole of O 2(g) = 32g 1 mole of NH 3(g) = 17g  we can calculate Density!

24. D = m / v A sample of oxygen contains 3 moles of particles at STP what is its density? 2 steps –Convert moles to mass AND volume –Calculate density If mass or volume is given, use it and convert the other……. THEN calculate D!

25. Remember... 1 mole = 6.02x10 23 atoms or molecules = gfm = 22.4L (g)

26. Stoich iometry of Chemical Equations The study of quantitative relationships that can be derived from chemical equations. “it’s a simple matter of weight ratios...”

27. Stoichiometry cookies If you look at chemical equations as recipes it may be easier to understand that –changing the amount of a reactant will change the amount of the product IN THE SAME RATIO !

28. Examining Molar Relationships in Balanced Equations 6CO 2 + 12 H 2 O + 2804kJ  6O 2 + C 6 H 12 O 6 +6H 2 0 Balanced equations –Law of conservation of mass / matter ATOMS are not created or destroyed during a chemical reaction, they are only rearranged to form new substances. # atoms on reactant side = # atoms on product side –Law of conservation of E E on the reactant side = E on the product side

29. Mole - Mole Relationships Practice

30. The End