1. The Mole
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6.02 X 1023

2. Average atomic Masses
Atomic masses on the Periodic Table are not whole numbers since they are weighted averages of Mass Numbers (P+N)
Average atomic mass depends on two factors- mass and relative abundance of each isotope.
Example- Cu-63 (69.17% and 62.94amu) and Cu-65(30.83% and 64.93amu)
Average atomic mass= (69.17x62.94)+(30.83x64.93) divided by 100=63.55amu
Do Practice Q1-2, p133.

3. STOICHIOMETRY
- the study of the quantitative aspects of chemical reactions.

4. Launch lab p 319- How much is a mole?
Decades or dozens are counting units. The Mole is also a counting unit.
Measure a small item (paperclip, eraser, penny) in cm using a ruler.
If a mole is 6.02 X1023 items, how far will a mole of your items, placed end-to-end lengthwise, extend into space? Express your answer in meters.
Convert this answer into light years (ly).
(1 ly=9.46 X1015 m).

5. How much is a mole?
Compare the distance you calculated with these astronomical distances:
Distance to the nearest star (other than the sun)=4.3 ly
Distance to the center of the galaxy= 30,000 ly
Distance to the nearest galaxy=2X106 ly

6. The Mole A counting unit
Similar to a dozen or gross, except instead of 12, it’s 602 billion trillion 602,000,000,000,000,000,000,000
6.02 X 1023 (in scientific notation)
This number (termed Avogadro’s number) is named in honor of Amedeo Avogadro (1776 – 1856), who studied quantities of gases and discovered that no matter what the gas was, there were the same number of molecules present

7. Just How Big is a Mole?
Enough soft drink cans to cover the surface of the earth to a depth of over 200 miles.
If you had Avogadro's number of unpopped popcorn kernels, and spread them across the United States of America, the country would be covered in popcorn to a depth of over 9 miles.
If we were able to count atoms at the rate of 10 million per second, it would take about 2 billion years to count the atoms in one mole.

8. The Mole
･Atoms and molecules are extremely small making it very difficult to measure their masses individually. ﾐIt is easier to weigh a large collection of these.
･A mole (abbreviated as mol) is defined as the number of C atoms in exactly 12 grams of pure C-12.
･This number is called Avogadro’s number.

9. A Mole of Particles Contains 6.02 x 1023 particles
= x 1023 C atoms
= x 1023 H2O molecules
= x 1023 NaCl “molecules”
(technically, ionics are compounds not molecules so they are called formula units)
6.02 x 1023 Na+ ions and
6.02 x 1023 Cl– ions
1 mole C
1 mole H2O
1 mole NaCl

10. Avogadro’s Number as Conversion Factor
6.02 x 1023 particles
1 mole or
1 mole
Note that a particle could be an atom OR a molecule!

11. Learning Check 1. Number of atoms in 0.500 mole of Al a) 500 Al atoms
b) x 1023 Al atoms
c) x 1023 Al atoms
2.Number of moles of S in 1.8 x 1024 S atoms
a) mole S atoms
b) mole S atoms
c) x 1048 mole S atoms

12. Molar Mass
･The mass in grams of one mole of atoms of any pure substance is known as its molar mass. The unit used is g/mol (gmol-1).
･Molar mass of sodium (Na) = mass of exactly one mole of Na atoms = g/mol = mass of x 1023atoms of Na.
･Molar mass of Uranium (U) = g/mol.
･The atomic mass number of an element in a periodic table = molar mass for the element

13. Practice p 322 Determine the number of Zn atoms in 2.5 mol of Zn.
Calculate the number of molecules in 11.5 mol of water (H2O).
How many molecules of AgNO3 are there in 3.25 mol of it?
Calculate the number of oxygen atoms in 5 mol of oxygen molecules.

14. Practice p 324 How many moles contain each of the following?
5.75 X 1024 atoms Al
2.50 X 1020 atoms Fe
How many moles contain each of the following molecules?
3.75 X 1024 CO2
3.58 X 1023 ZnCl2

15. Practice p 328 Determine the mass in grams of each of the following
3.57 mol Al
42.6 mol Si
Convert each given quantity in scientific notation to mass in grams expressed in scientific notation
3.45 X 102 mol Co
2.45 X 10-2 mol Zn

16. Practice p 329 Determine the number of moles in each of the following
25.5 g Ag
300 g S
Convert each mass to moles. Express the answer in scientific notation.
1.25 X 103 g Zn
1 kg Fe

17. Learning Check! = 79.9 g/mole 1 mole of Br atoms 1 mole of Sn atoms
Find the molar mass (usually we round to the tenths place)
= 79.9 g/mole
1 mole of Br atoms
1 mole of Sn atoms
= g/mole

18. Molar Mass of Molecules and Compounds
･1 mole of any compound = x 1023units of the compound.
･Molar masses of compounds are calculated by adding the molar masses of the atoms present in the compound.
･Calculate the molar mass of Ca3(PO4)2
--Need to look the molar masses of each of the element present and multiply by the number of the atoms present.

19. Learning Check! Molar Mass of K2O = ? Grams/mole
B. Molar Mass of antacid Al(OH)3 = ? Grams/mole

20. Practice p 335 Determine the molar mass of each ionic compound-
NaOH, CaCl2, KC2H3O2
Calculate the molar mass of each molecular compound- C2H5OH, HCN, CCl4
Sr(NO3)2, (NH4)3PO4, C12H22O11

21. Learning Check
Prozac, C17H18F3NO, is a widely used antidepressant that inhibits the uptake of serotonin by the brain. Find its molar mass.

22. Calculations with Molar Mass
Grams Moles

23. Converting Moles and Grams
Aluminum is often used for the structure of light-weight bicycle frames. How many grams of Al are in 3.00 moles of Al?
3.00 moles Al ? g Al

24. 1. Molar mass of Al 1 mole Al = 27.0 g Al
2. Conversion factors for Al
27.0g Al or mol Al
1 mol Al g Al
3. Setup 3.00 moles Al x g Al
1 mole Al
Answer = g Al

25. Learning Check!
The artificial sweetener aspartame (Nutra-Sweet) formula C14H18N2O5 is used to sweeten diet foods, coffee and soft drinks. How many moles of aspartame are present in 225 g of aspartame?

26. Practice p 336

27. Atoms/Molecules and Grams
Since 6.02 X 1023 particles = 1 mole AND 1 mole = molar mass (grams)
You can convert atoms/molecules to moles and then moles to grams! (Two step process)
You can’t go directly from atoms to grams!!!! You MUST go thru MOLES.
That’s like asking 2 dozen cookies weigh how many ounces if 1 cookie weighs 4 oz? You have to convert to dozen first!

28. Everything must go through Moles!!!
Calculations
molar mass Avogadro’s number Grams Moles particles
Everything must go through Moles!!!

29. Atoms/Molecules and Grams
How many atoms of Cu are present in 35.4 g of Cu?
35.4 g Cu mol Cu X 1023 atoms Cu g Cu mol Cu
= 3.4 X 1023 atoms Cu

30. Learning Check!
How many atoms of K are present in 78.4 g of K?

31. Learning Check!
What is the mass (in grams) of 1.20 X 1024 molecules of glucose (C6H12O6)?

32. Learning Check! How many atoms of O are present in 78.1 g of oxygen?
78.1 g O2 1 mol O X 1023 molecules O2 2 atoms O g O mol O molecule O2

33. Percent Composition of Compounds
Composition of compounds can be described in 2 ways: ﾐBy the number of its constituent atoms. ﾐBy the mass (%) of each element present.
･The mass percents of elements are obtained by comparing the mass of each element present in 1 mole of the compound to the total mass of the compound.
･Useful today with unknown compounds.

34. Percent Composition
What is the percent carbon in C5H8NO4 (the glutamic acid used to make MSG monosodium glutamate), a compound used to flavor foods and tenderize meats?
a) %C
b) %C
c) %C

35. Chemical Formulas of Compounds
Formulas give the relative numbers of atoms or moles of each element in a formula unit - always a whole number ratio (the law of definite proportions).
NO atoms of O for every 1 atom of N
1 mole of NO2 : 2 moles of O atoms to every 1 mole of N atoms
If we know or can determine the relative number of moles of each element in a compound, we can determine a formula for the compound.

36. Types of Formulas Empirical Formula
The formula of a compound that expresses the smallest whole number ratio of the atoms present.
(Ionic formulae are always empirical formulae)
Molecular Formula
The formula that states the actual number of each kind of atom found in one molecule of the compound. Example- CH is the empirical formula for benzene, C6H6).

37. To obtain an Empirical Formula
1. Determine the mass in grams of each element present, if necessary.
2. Calculate the number of moles of each element.
3. Divide each by the smallest number of moles to obtain the simplest whole number ratio.
If whole numbers are not obtained* in step 3), multiply through by the smallest number that will give all whole numbers
* Be careful! Do not round off numbers prematurely

38. A sample of a brown gas, a major air pollutant, is found to contain 2
A sample of a brown gas, a major air pollutant, is found to contain 2.34 g N and 5.34g O. Determine a formula for this substance.
require mole ratios so convert grams to moles
moles of N = 2.34g of N = moles of N
14.01 g/mole
moles of O = g = moles of O
16.00 g/mole
Formula:

39. Calculation of the Molecular Formula
A compound has an empirical formula of NO2. The colourless liquid, used in rocket engines has a molar mass of 92.0 g/mole. What is the molecular formula of this substance?

40. Empirical Formula from % Composition
A substance has the following composition by mass: % Na ; % B ; % H
What is the empirical formula of the substance?

41. Formulas of hydrates
Hydrate is a compound with a fixed number of water molecules bound to it.
Na2CO3.10H2O- sodium carbonate decahydrate
Hydrate+ heat= anhydrous compound (without water)

42. How to find out the formula of a hydrate
Need to know how many moles of H20 attached to the molecule- BaCl2.xH2O
Mass sample
Heat it, mass again.
The difference in mass= mass of water
Divide it by molar mass of H20 (18g)= moles of water
Determine moles of compound as well.
Determine ratio of water molecules to compound molecules.

43. Try it!
A mass of 2.5 g of blue, hydrated copper sulfate (CuSO4.xH2O) is placed in a crucible and heated. After heating, 1.59 g of white anhydrous copper sulfate (CuSO4) remains. What is the formula for the hydrate?