1. Mrs. Wilson

2.  Staple your lab rubric to the back of your Foul Water Lab. Make sure you’ve written your name and your partners’ names.  Turn in your Foul Water Labs.  Please follow the LASA honor code.

3.  (it’s very easy )

4.  Calculate the number of representative particles (atoms, ions, molecules, or formula units) in a sample of material if mass is given OR if # of moles are given.  Calculate the # of moles or the mass of a sample of material if the number of representative particles is given. Homework: 1.9 Homework + Daily Quiz 1-10 Next Class

5.  The SI unit used to measure the amount of substance is the mole (Latin for “pile”)  The “mole” is a counting unit, used to make counting things much easier. 1 dozen of ANYTHING = 12 things 1 mole of ANYTHING = 6.02 x 10 23 things 6.02 x 10 23 = Avogadro’s Number (symbol N A ) THIS IS EQUAL TO THE NUMBER OF CARBON-12 ATOMS IN 12 G OF CARBON-12. BUT… HOW DO WE COUNT ATOMS?

6. This exercise is to help you understand that for chemists to count atoms, they have to weigh them. Let’s say the mass of Cheerios in one box = 500. g (don’t worry about the box or the bag) A “gaggle” of Cheerios = 100 Cheerios. Mass of one “gaggle” = 15.0 grams How many Cheerios are in the box? Use sig figs to express your final answer. (hint: # Cheerios is a counting unit, so don’t use 100 to help you determine sig figs.)

7. This exercise is to help you understand that for chemists to count atoms, they have to weigh them. Let’s say the mass of all Cheerios in one box = 500. g (don’t worry about the box or the bag) A “gaggle” of Cheerios = 100 Cheerios. Mass of one “gaggle” = 15.0 grams How many Cheerios are in the box? 500. g / 15.0 g = 33.3 “gaggles” 33.3 “gaggles” x 100 = 3.33 x 10 3 Cheerios

8. Elements have ATOMS Covalent compounds have uncharged MOLECULES (groups of ATOMS)  Covalent compounds = consist of nonmetal atoms only (found on right side of periodic table; H is also a nonmetal) Ionic compounds have FORMULA UNITS (neutral groups of IONS)  Ions = atoms or molecules that have gained or lost electrons  Ionic compounds = consist of metal ions and nonmetal ions (metals found on LEFT and MIDDLE side of periodic table)

9. Name of RPsNumber of FPs FeAtom1 atom Fe 2 O 3 Formula unit (Fe 2 O 3 ) Ion (Fe 3+ and O 2- ) 1 formula unit 2 Fe 3+ ions and 3 O 2- ions 5 CO 2 Molecule (CO 2 ) Atom (C and O) 5 molecules 5 C atoms and 10 O atoms 3 Zn 4 N 2 O 4 2 Ca 3 P 2

10. Name of RPsNumber of FPs FeAtom1 atom Fe 2 O 3 Formula unit (Fe 2 O 3 ) Ions (Fe 3+ and O 2- ) 1 formula unit 2 Fe 3+ ions and 3 O 2- ions 5 CO 2 Molecule (CO 2 ) Atom (C and O) 5 molecules 5 C atoms and 10 O atoms 3 ZnAtom3 Zn atoms 4 N 2 O 4 Molecule; Atom4 molecules 8 N atoms, 16 O atoms 2 Ca 3 P 2 Formula unit; Ions2 formula units 6 Ca 2+ ions 6 P 3- ions

11.  How many atoms are in 0.150 moles of Co? 9.03 x 10 22 atoms  How many formula units are in 12.07 moles of Na 2 O? 7.266 x 10 24 formula units

12.  How many Na + IONS are in 12.07 moles of Na 2 O? 1.453 x 10 25 ions You Do: How many O atoms are in 0.075 moles of NaNO 3 ?

13.  How many Na + IONS are in 12.07 moles of Na 2 O? 1.453 x 10 24 ions You Do: How many O atoms are in 0.075 moles of NaNO 3 ? 1.4 x 10 23 atoms of O

14.  You Do: How many moles is 5.07 x 10 23 atoms of Zr?  You Do: How many moles is 8.90 x 10 24 molecules of CO 2 ?

15.  You Do: How many moles is 5.07 x 10 23 atoms of Zr? 0.842 moles of Zr  You Do: How many moles is 8.90 x 10 24 molecules of CO 2 ? 14.8 moles of CO 2

16.  Remember the “gaggle” of Cheerios? (1 “gaggle” = 100 Cheerios = 15.0 g)?  Similarly, you need to know the mass of one mole of the chemical in order to convert to mass. This is also known as “molar mass.”  You have to know this because one mole of a chemical CAN weigh differently compared to another, but they have the same NUMBER of RP’s.

17. The mass of one copper atom is 63.546 amu (atomic mass units) (1 amu = 1/12 th the mass of one carbon-12 atom) (1 amu = 1.6605 x 10 -27 kg) 1.What is the mass of one copper atom in kg? 2.Convert this mass to grams. 3.Multiply the mass of one copper atom in grams by 6.022 x 10 23. What do you notice? What is the meaning of 63.546?

18. Molecular Mass of a covalent compound is the (atomic) mass of one molecule. H 2 O = H 2 x 1.01 = 2.02 g O + 1 x 15.99 = 15.99 g 18.01 g/mol Calculate the molar (molecular) mass of CH 4 (methane) CH 4 =

19. Formula Mass of an ionic compound is the (atomic) mass of one formula unit. NaCl = 22.99 + 35.45 = 58.44 g/mol MnCl 2 = 54.94 + 70.90 (2 mol Cl) = 125.84 g/mol Let’s make it harder… what is the formula mass of Ca(NO 3 ) 2 ? (yes… that’s 1 Ca, 2 N’s, and 6 O’s) What is the formula mass of Mg 3 (PO 4 ) 2 ?

20. How do you determine the amount of moles in a compound? 1. If you have 9.0 grams of water, you have ____moles of water. Water - H 2 O = 18.01 g/mol 9.0 g H 2 O x 1 mole of H 2 O = 0.50 mol of H 2 O 18.01 g H 2 O 2. If you have 13.0 grams of water, you have ____moles of water. 0.722 moles of water

21. If you weigh out 5.00g of formaldehyde (formula CH 2 O), how many moles is that? 0.166 moles What about 60.0 g of formaldehyde? 2.00 moles

22. Counting Moles 2 mol C 6 H 12 O 6 contains:  2 mole of C 6 H 12 O 6 molecules  2 x 6 = 12 moles of C atoms  2 x 12 = 24 moles of H atoms  2 x 6 = 12 moles of O atoms  48 moles of atoms in total Complete the rest of “Counting Atoms” for BF 3 and Ca(NO 3 ) 2.

23. How many sodium ions are in 50.0 g of Na 2 S? 7.71 x 10 23 sodium ions

24. You do: What is the mass of 7.04 x 10 23 molecules of PF 5 ? 147 g of PF 5

25.  I’ll run around and check your work. Always use dimensional analysis and respect the sig fig rules.

26. Be careful – “particles” usually means “molecules” or “formula units” unless the material is an element. We will not calculate volume for now.

27.  Get a person in your group to get one whiteboard per person in your group and a bag of erasers and dry erase markers.  I want to see the dimensional analysis and the answer (with sig figs) for each question.

28.  How many atoms of potassium are in 2 moles of K 2 O? _______________________

29.  2 x 10 24 potassium atoms

30.  How many molecules of water make up 5 MOLES? ________________________

31.  3 x 10 24 molecules

32.  How many moles are 6.022 x 10 23 atoms of sodium? ________________________

33.  1.000 moles

34.  How many grams are in 2.3 x 10 -4 moles of calcium phosphate, Ca 3 (PO 3 ) 2 ?

35.  0.12 grams

36.  How many oxygen atoms are in 3.4 x 10 -7­ grams of silicon dioxide, SiO 2 ?

37.  6.8 x 10 15 oxygen atoms

38. https://www.youtube.com/watch?v=PvT5 1M0ek5c “A Mole is a Unit”

39.  What did you learn today about the mole and mole conversions?