Warm Up:
 What
is a mole?
Chapter 10:
The Mole
Learning Targets:
1. To form an idea of what a mole is.
2. To form an idea of the
relationships between, particles,
moles, and mass.
3. Distinguish between parts/mass to
mols and parts to mass problems.
4. Be able to calculate:
parts to mols/mols to parts
mass to mols/mols to mass
mass to parts/parts to mass
What is a mole?
 How
many are in a pair?
 Dozen?
 Gross?
 Ream?
What do these represent?
a specific value
What is a mole?
1
mole = 6.023 x 1023 ____________
 This number is known as Avogadro's
Number

 If
It is the number of particles whatever they
may be: atoms, molecules, formula units
I have a mole of apples, how many
apples do I have?
 A mole of marbles?
 A mole of skittles?
Avogadro’s Number
1
mole = 6.023 x 1023 ___units/particles____
 The units/particles depends on what type
of particle it is:



Atoms: individual elements
Formula Units (FU): Ionic Compounds
Molecules: Covalent Compounds
Let’s work on determining
types of units:
 What
would the unit of the following be:
Substance
NaCl
O2
Li3PO4
Ga
N2O5
SO2
K
PCl3
Unit/Particle
Converting Moles to Particles
 How
many atoms are in 2.54 moles of sulfur.
__Given Unit_Conversion Factor_(New Unit)
Conversion Factor (given unit)
What is our conversion factor?
6.02 x 1023 particles (atoms, molecules,
formula units)
Converting Moles to Parts:
 Knowing

what we know now:
How many atoms are in 2.45 moles of sulfur?
2.45 mols S
6.022 x 1023 atms S
1mol S
=1.48 x 1024 atms S
Let’s Practice:
1.
How many atoms are in 6.2 moles of Al?
1.
Convert 5.75 x 1024 atoms of Al into mols
of Al.
A couple more:
1.
How may atoms are in 3.5 moles of Si?
2.
Convert 5.3 x 1025 molecules of CO2 to
moles.
Now mass to moles:
 Which
has more mass?
A dozen watermelon?
A dozen
eggs?
Mass and the mole:
 AMU:
(atomic mass unit) the mass of one
nucleon (proton and neutron)

Carbon’s AMU: 12 (12 protons and
neutrons)
1
mol = a substance’s AMU
 1 mol of Carbon has an AMU of 12 grams.
 AMU is an individual atom/Mole is 6.02 x
1023 atoms

Every mole has a different mass value
based on their AMU, because each atom
has a different mass.
Molar Mass:
 To
determine the mass of a substance or
element.
 Use the periodic table to determine the
mass of a single mole of a substance.



The molar mass comes from the periodic
table.
AMU=molar mass
Unit for molar mass is g/mol
What is the molar mass?










Copper:
Aluminum:
Hydrogen:
Nitrogen:
Uranium:
Sulfur:
Oxygen:
Chlorine:
K:
Beryllium:
Molar Mass of Compounds:
 Add
the molar masses of EVERY atom in the
compound together.
 Find the molar mass of H2O
H= 1.00795 x 2 hydrogen atoms
2.02g
O=15.994 x 1 oxygen atom
+ 16.00 g
Molar mass of H2O
18.02g/mol
*You can use whole numbers instead of
decimals but you will need to round!
Find the Molar Mass:
Compound:
Copper (III) Oxide
Na3PO4
Al2(CO3)3
Nitrogen Dioxide
Lithium Carbonate
SO3
Calcium Sulfide
Molar Mass:
Moles to grams


First you must find the molar mass of the substance… You will
need this to complete the problem.
Then you plug the information into “train tracks”
How many moles in 56.71g of water (H2O)?
56.71g H2O 1 mol H2O
18g H2O
=
56.71 x 1 = 3.151 mols H2O
18
*Remember the molar mass of H2O is 18g/mol.
Let’s Practice:
How many grams in 1.56 moles of Calcium Chloride?
How many grams can be found in 12.8 moles of Copper (II)
Phosphate?
Practice:
How many moles are in 15.6g of sulfur dioxide?
How many moles can be found in 456g of lithium carbonate?
Practice:
How many mols of sodium is 3g?
How many mols of Fe is .05g?
How many mols of Beryllium is 1.60g?
Practice:
How many mols of lead is 15g?
How many mols of platinum is 2.3 x 10-5g?
Two step problems:
 Parts
mols
grams
If there is 2.45 x 1023 atms of Calcium how many
grams is that?
2.45 x 1023 atms Ca
1 mol Ca
40 g Ca
6.02 x 1023atms Ca
1 mol Ca
Practice
If we have 567.1g of gold, how many atoms is that?
How many molecules are in 56.7g of Hydrochloric Acid?
Practice:
What is the mass of 4.56 x 1021 atoms of Mg?
How many formula units are in 125.3g of strontium carbonate?
What is the mass of 8.65 x 1025 formula units of nickel (III) sulfate?