1. REVIEW Which is larger I? or I1- ? Name each particle.
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2. Chapter 10 Chemical Quantities 10.1 The Mole: A Measurement of Matter
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3. I can…
Perform dimensional analysis to convert between units Recall Avogadro’s number Apply Avogadro’s number to determine the number of representative particles in a substance Calculate representative particles  moles Calculate moles  representative particles Determine molar mass of a substance
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4. case gross dozen ream pair Six pack
Measuring Matter
Chemistry is a quantitative science.
you perform calculations that relate quantities of the reactants in a chemical reaction to quantities of the products.
pair
case
Six pack
gross
dozen
ream
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5. Measuring Matter
Each of these different ways to measure apples can be equated to a dozen apples.
By count: 1 dozen apples = 12 apples
By mass: 1 dozen apples = 2.0 kg apples
By volume: 1 dozen apples = 0.20 bushel apples
These are approximations for average-sized apples.
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6. Finding Mass from a Count
Sample Problem 10.1
Finding Mass from a Count
What is the mass of 90 average-sized apples if 1 dozen of the apples has a mass of 2.0 kg?
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7. Analyze List the knowns and the unknown. 1
Sample Problem 10.1
Analyze List the knowns and the unknown. 1
Use dimensional analysis to convert the number of apples to the mass of 90 apples.
KNOWNS
number of apples = 90 apples
Conversion factors 12 apples = 1 dozen apples 1 dozen apples = 2.0 kg apples
UNKNOWN mass of 90 apples = ? kg
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8. Calculate Solve for the unknown.
Sample Problem 10.1
Calculate Solve for the unknown. 2
Multiply the known by conversion factors.
The conversion factor used should cancel the previous unit
90 apples × ×
= 15 kg apples
apples
dozen apples
kg apples 1
2.0 1 1 12
The unit “apples” cancels the previous unit
The unit “dozen apples” cancels the previous unit
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9. UNKNOWN mass of 0.56 bushel apples = ? kg
If 0.20 bushel is 1 dozen apples and a dozen apples has a mass of 2.0 kg, what is the mass of 0.56 bushel apples?
KNOWNS
volume of apples = 0.56 bushel apples Conversion factors 12 apples = 1 dozen apples 1 dozen apples = 2.0 kg apples
0.20 bushel = 1 dozen apples
UNKNOWN mass of 0.56 bushel apples = ? kg
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10. If 0. 20 bushel is 1 dozen apples and a dozen apples has a mass of 2
If 0.20 bushel is 1 dozen apples and a dozen apples has a mass of 2.0 kg, what is the mass of 0.56 bushel apples?
0.56 bushel
1 dozen
2.0 kg
= 5.6 kg 1
0.20 bushel
1 dozen
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11. COPY THIS
Assume 2.0 kg of apples is 1 dozen and that each apple has 8 seeds. How many apple seeds are in 14 kg of apples? Known – 14 kg apples Conversion factors: 2.0 kg apples = 1 dozen 1 apple = 8 seeds Unknown: seeds?
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12. 14 kg 1 dozen 12 apples 8 seeds = 672 seeds 1 dozen 1 2.0 kg 1 apple
Assume 2.0 kg of apples is 1 dozen and that each apple has 8 seeds. How many apple seeds are in 14 kg of apples?
14 kg
1 dozen
12 apples
8 seeds
= 672 seeds
1 dozen 1
2.0 kg
1 apple
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13. Matter is composed of atoms, molecules, and ions.
What Is a Mole?
Matter is composed of atoms, molecules, and ions.
These is an extremely large number of them in a small sample of a substance so counting these particles is not practical.
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14. Think about counting eggs.
What Is a Mole?
Think about counting eggs.
It’s easier when the eggs are grouped into dozens.
A dozen is a
specified number
(12) of things.
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15. Counting with Moles TED Ed TV What Is a Mole?
Chemists also use a unit that is a specified number of particles, most often atoms or molecules.
The unit is called the mole.
A mole (mol) of a substance is × 1023 representative particles of that substance
The number of representative particles in a mole and is called Avogadro’s number, × 1023
TED Ed TV
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16. If you had a mole of doughnuts, they would cover the entire Earth in a doughnut-layer five miles deep.
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17. If you had a mole of basketballs, you could create a new planet the size of the Earth!
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18. If you received a mole of pennies on the day you were born, and spent a million dollars a second until you died at 100, you’d still have over 99.99% of your money in the bank!
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19. Counting with Moles
The term representative particle refers to atoms, molecules, or formula units.
The representative particle of most elements is the atom.
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20. What Is a Mole?
Counting with Moles
However, seven elements exist normally as diatomic molecules: H2, N2, O2, F2, Cl2, Br2, and I2.
I Have NO Bright or Clever Friends – you must memorize the diatomic elements
The representative particle of these elements is the molecule.
For ionic compounds, such as calcium chloride, the representative particle is the formula unit, CaCl2.
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21. What Is a Mole?
Counting with Moles
A mole of any substance contains Avogadro’s number of representative particles, or × 1023 atoms, ions, molecules or formula units
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22. molecule formula unit diatomic molecule atom COPY THIS
Write the correct representative particle (atom , molecule or formula unit) for each of the following.
H2O KI O2 Ag
molecule
formula unit
diatomic molecule
atom
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23. Daily Question – give 3 ideas on the words “dozen” and “mole”.
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24. Converting Number of Atoms to Moles
Sample Problem 10.2
Converting Number of Atoms to Moles
Magnesium is a light metal used in the manufacture of aircraft, automobile wheels, and tools. How many moles of magnesium is 1.25 × 1023 atoms of magnesium?
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25. Analyze List the known and the unknown.
Sample Problem 10.2
Analyze List the known and the unknown. 1
KNOWN
number of atoms = 1.25 × 1023 atoms Mg
Conversion factor
1 mol Mg = × 1023 atoms Mg
UNKNOWN moles = ? mol Mg
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26. Drag and drop - unit and chemical symbol
Sample Problem 10.2
Use DIMESIONAL ANALYSIS to Solve for the unknown. 2
Write known over 1
Drag and drop - unit and chemical symbol
6.022 × 1023 atoms Mg
1 mol Mg
1.25 × 1023 atoms Mg
= mol Mg 1
Why does this answer have three significant figures?
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27. Converting: Moles  Atoms or molecules
Sample Problem 10.3
Converting: Moles  Atoms or molecules
Propane is a gas used for cooking and heating. How many atoms are in 2.12 mol of propane (C3H8)?
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28. moles → molecules → atoms.
Sample Problem 10.3
Analyze List the knowns and the unknown. 1
The desired conversion is:
moles → molecules → atoms.
KNOWN number of moles = 2.12 mol C3H8
Conversion factors 1 mol C3H8 = × 1023 molecules C3H8 1 molecule C3H8 = 11 atoms (3 carbon and 8 hydrogen atoms)
UNKNOWN number of atoms = ? atoms
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29. Drag and drop - unit and chemical formula
Sample Problem 10.3
Use DIMESIONAL ANALYSIS to Solve for the unknown. 2
Write known over 1
Drag and drop - unit and chemical formula
1 molecule C3H8
2.12 mol C3H8
6.022 × 1023 molecules C3H8
1 mol C3H8
11 atoms 1
= 1.40 × 1025 atoms
Why does the answer have three significant figures?
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30. Counting Atoms in a Molecule

31. 1 molecule (NH4)3PO4
3 N atoms

32. 1 molecule (NH4)3PO4
12 H atoms

33. 1 molecule (NH4)3PO4
1 P atom

34. 1 molecule (NH4)3PO4
4 O atoms

35. In 1 Mole of (NH4)3PO4 There are: 3 moles of N 12 moles of H
1 mole of P
4 moles of O

36. related to chemical formulas?
How is a mole:
similar to a dozen?
related to chemical formulas?
Subscripts in a chemical formula can indicate _____________ or ______________ . (2 ideas)
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37. Learning Targets: I can…
Determine molar mass of an element or compound
Calculate moles to grams
Calculate grams to moles
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38. All conversions go first to mole.
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39. The Mass of a Mole of an Element
Molar Mass
The Mass of a Mole of an Element
The atomic mass of an element expressed in grams is the mass of a mole of the element.
The mass of 1 mole of an element is its molar mass. For consistency, we will round all masses of elements on the periodic table to 2 decimal places.
For carbon, the molar mass is g.
For atomic hydrogen, the molar mass is 1.01 g.
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40. Why are the atomic masses on the periodic table not whole numbers?
 masses shown on the periodic table are weighted averages of the masses for all of the isotopes of elements
What is the atomic mass of an element on the periodic table expressed in grams?
The mass of 1 mole of that element.
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41. The Mass of a Mole of an Element
Molar Mass
The Mass of a Mole of an Element
1 mol of sulfur atoms = g
1 mol of carbon atoms = g
1 mol of iron atoms = g
This figure shows one mole of carbon, sulfur, and iron.
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42. The Mass of a Mole of an Element
Molar Mass
The Mass of a Mole of an Element
The molar mass of an element contains 1 mol or × 1023 atoms of that element.
1 mole of an element has the mass listed on the periodic table in grams
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43. How many atoms are contained in the molar mass of an element?
6.022 x atoms
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44. The Mass of 1 Mole of a Compound
Molar Mass
The Mass of 1 Mole of a Compound
To calculate the molar mass of a compound:
determine the number of grams of each element
then add the masses of all the elements in the compound.
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45. The Mass of a Mole of a Compound
Molar Mass
The Mass of a Mole of a Compound
Find the molar mass of SO3
the mass of sulfur (S) is g
The mass of three atoms of oxygen:
(O): 3 × g = g
Molar mass of SO3 is g g = g
1 mole of SO3 has a mass of g.
This is the mass of x 1023 molecules of SO3.
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46. Molar Mass The Mass of a Mole of a Compound
1 mol of paradichlorobenzene (C6H4Cl2) molecules (moth crystals)
= g
1 mol of glucose (C6H12O6) molecules (blood sugar)
= g
1 mol of water (H2O) molecules = g
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47. Calculating the Molar Mass of a Compound
Sample Problem 10.4
Calculating the Molar Mass of a Compound
The decomposition of hydrogen peroxide (H2O2) provides sufficient energy to launch a rocket. What is the molar mass of hydrogen peroxide?
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48. Calculate Solve for the unknown.
Sample Problem 10.4
Calculate Solve for the unknown. 2
Add the results.
mass of 1 mol H2O2 = 2.02 g H g O = g
molar mass of H2O2 = g/mol
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49. Find the molar mass of PCl3
mass of 1 mol P = g P
mass of 3 mol Cl = g x 3 = Cl
molar mass of PCl3 = g/mol
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50. END OF 10.1
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51. Glossary Terms
mole (mol): the amount of a substance that contains 6.02 × 1023 representative particles of that substance
Avogadro’s number: the number of representative particles contained in one mole of a substance; equal to 6.02 × 1023 particles
representative particle: the smallest unit into which a substance can be broken down without a change in composition, usually atoms, molecules, or ions
molar mass: a term used to refer to the mass of a mole of any substance
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