1. Manic Monday in AP CHEM!!! 8/29
List everything you know about 1 mole = ????????
Write formulas for these:
sodium sulfate
copper (II) chlorate
ammonium hydroxide
sulfuric acid

4. Mole
Even tiny samples in the lab contain MANY molecules, atoms, or ions
Ex: 1 teaspoon of water = 2 x 1023 water molecules!
So chemists devised a counting unit to relate numbers of molecules, atoms, etc to lab-sized amounts…. THE MOLE
Examples of other counting units (dozen = 12 objects, gross = 144 objects)
mole (abbr. mol) – the amount of matter that contains as many objects as there are atoms in 12 g of 12C
objects = atom, molecules, ions, or whatever object you’re counting… people, apples, etc
number of atoms = 6.02 x 1023 = “Avogadro’s number” = NA

6. 6.02 x 1023 particles = 1 mol particles
Avogadro’s Number
One mole of particles contains Avogadro’s number of those particles
“particles” are whatever you’re looking for (or are given) the number of.
usually atoms, ions, or molecules
6.02 x 1023 particles = 1 mol particles

7. Molar Mass: Another Conversion Factor!
molar mass - the mass of 1 mole of an element or compound (unit g/mol)
Molar mass allows us to interconvert:
6.941 g Li = 1 mole of Li
g H2O = 1 mole of H2O
mass of a substance
moles of that same substance
6.941 g Li
1 mol Li
1 mol Li
6.941 g Li
g H2O
1 mol H2O
1 mol H2O
g H2O

8. Avogadro’s Number: Examples
How many Cu atoms are in 0.50 mole of Cu?
How many moles of CO2 are in 2.50 x 1024 atoms CO2?

9. WARM-UP 8/30
Identify each as ionic, covalent, or acid and then name them:
HNO3
Ba(IO)2
P2O5
HCl
CuSO4
2) 31 billion tons of CO2 was emitted in Express this in grams without exponential notation using an appropriate prefix.
# 1.60 **Disclaimer: We DO NOT need to know average/absolute deviation!!! YAY!

10. MOLES
Moles = macroscopic
Molecules = microscopic

11. How many sulfate ions are present in 3.52 moles of sodium sulfate?
How many grams are present in 4.53 x 1024 atoms of nitrogen?

12. How many H atoms are in 3.01 x 10-2 mg of H2O?
What is the mass in grams of Na+ ions in a sample of Na2O containing 1.02 x1020 Na2O formula units?
Part 2

14. MATTER RE-CAP PURE SUBSTANCES MIXTURES Definite composition
Looks homogeneous (not a mixture!)
Definite melting/boiling/freezing point
Definite density
ELEMENTS
COMPOUNDS
Variable composition
May look homogeneous to the naked eye, but on microscopic level is variable in composition
Variable melting/boiling/freezing point
Density depends on ratio of components (i.e. salt water)
HOMOGENEOUS/SOLUTIONS
HETEROGENEOUS

15. LAWS Law of Definite Proportions Law of Conservation of Mass
Also called Law of Constant Composition
A pure compound has the same composition regardless of its source
i.e. WATER – regardless of where it originates, it will always be a 2:1 ratio of H:O  H2O
The total mass of reactants before the reaction is equal to the total mass of the products after the reaction even though the product may look NOTHING like the starting reactants.
A + B  Q
Atoms merely rearrange themselves during a chemical reaction, but the same atoms are still present.