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Student name: _______________________________________________ Class: _______

SSttaattee GGooaall//EExxppeeccttaattiioonnss:: Goal: The student will demonstrate the ability to use scientific skills and processes to explain composition and interactions of matter in the world in which we live. Expectation(s): The student will explain that matter undergoes transformations, resulting in products that are different from the reactants. Indicator(s): The student will demonstrate that adjusting quantities of reactants in a chemical reaction may affect the amounts of products formed during a chemical reaction.

Chemical Quantities

The Mole

Atoms to moles

Moles to atoms

Molar mass

Mole-mass-volume relationships

Moles to mass

Mass to moles

Volume of a gas

Chemical formulas

Percent composition

Empirical Formulas

Molecular formulas

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Topic 1: The Mole & its relationships (Ch. 10-1 & 10-2) # days

KKeeyy ttooppiiccss//qquueessttiioonnss Topic 1: Measuring familiar quantities (10-1)

1) What are three methods for measuring the amount of something?

Book, Page 289, Problems 1 & 2

Study Guide, page 3; 1-12 Topic 2 – By count: Mole to particle relationship (10-1)

2) How is Avogadro’s number related to a mole of any substance?

Book, page 291, Problems 3 & 4

Book, page 292, Problems 5 & 6

Study Guide, page 4; 1-10 Topic 3 – By mass: Molar mass (10-1)

3) How is the atomic mass of an element related to the molar mass of a substance?

Book, page 296, 7 & 8

Study Guide, page 5; 1-24 Topic 4 – By mass & count: Mass/Mole/Particle relationship (10-2)

4) How do you convert the mass of a substance to the number of moles of the substance?

Book, page 298, 16 & 17

Book, page 299, 18 & 19

Study Guide, page 6; 1-16 Topic 5 – By volume: Mass/Mol/ Volume relationship (10-2)

5) What is the volume of a gas at STP?

Book, page 301, 20-21

Book, page 302, 22-23

Study Guide, Page 7; 23-30

Notes on lecture, research and/or reading

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Practice: Familiar Quantities

Using diagram 1 and the information associated with it, answer the following questions.

1. How many oranges are in 8 bags of oranges?

2. How many bags do I need for 37 oranges?

3. What is the mass of the 8 bags of oranges?

4. If I had 24 kilograms of oranges, how many bags would I have?

5. How many bags of oranges would take up 23 dm3 of space?

6. About how many oranges is this?

Using diagram 2 and the information associated with it, answer the following questions.

7. How many grains of sugar are in 2 boxes of sugar?

8. How many boxes do I need to hold 1x1012 grains of sugar?

9. What is the mass of 4.3 boxes of sugar?

10. If I had 2.4 kilograms of sugar, how many boxes would I have?

11. How many boxes of sugar would take up 27 dm3 of space?

12. About how many grains of sugar is this?

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Practice: By Count (Mole ↔ Particle conversions) Use Avogadro’s number to make the following conversions:

1) How many molecules are there in 2 moles of FeF3?

2) How many molecules are there in 4 moles of Na2SO4?

3) How many moles are there in 2.3 x 1024 atoms of silver?

4) How many moles are there in 7.4 x 1023 molecules of AgNO3?

5) How many moles are there in 7.5 x 1023 molecules of H2SO4?

6) How many molecules are there in 1.2 moles of Cu(NO3)2?

7) How many moles are there in 9.4 x 1025 molecules of H2?

8) How many molecules are there in 2.30 moles of CoCl2?

9) How many molecules are there in 2.3 moles of NH4SO2?

10) How many moles are there in 3.3 x 1029 molecules of N2I6?

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Practice: By Mass (Gram formula/Molar mass) Use your periodic table to determine the Gram formula or Molar mass for each compound: The gram formula or molar mass of a compound is simply the sum of the masses of all the atoms in the formula.

1) NaBr (sodium bromide)

2) HNO3 (nitric acid)

3) H2O (Hydrogen hydroxide)

4) NaOH (sodium hydroxide)

5) CaCO3 (calcium carbonate)

6) LiI (lithium iodide)

7) AgCl (silver chloride)

8) C6H12O6 (glucose)

9) Ba(NO3)2(barium nitrate)

10) Fe2(SO4)3 (iron(III) sulfate)

11) Cl2

12) KOH

13) BeCl2

14) FeCl3

15) BF3

16) CCl2F2

17) Mg(OH)2

18) UF6

19) SO2

20) H3PO4

21) (NH4)2SO4

22) CH3COOH

23) Pb(NO3)2

24) Ga2(SO3)3

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Practice: By Mass (Mole ↔ Mass conversions) Use your periodic table to make the following conversions:

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Practice: By Volume (Mole ↔ Volume conversions) Use Avogadro’s number to make the following conversions:

23) A container with a volume of 893 L contains how many moles of air at STP?

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Topic 2: Chemical formulas (Ch. 10-3) # days

KKeeyy ttooppiiccss//qquueessttiioonnss

Day 6: Percent composition (10-3)

6) How do you calculate the percent by mass of an element in a compound?

Book, Page 306, 32 & 33

Book, Page 307, 34 & 35

Study Guide, page 9, 1 - 9

Day 7: Empirical formulas (10-3)

7) What does the empirical formula of a compound show?

Book, page 310, 36 & 37

Book, page 292, 5 & 6

Study Guide, page 10, 10 - 19

Day 8: Molecular formulas (10-3)

8) How does the molecular formula compare with the empirical formula?

Book, page 312, 38 & 39 Study Guide, page 11,

20 - 25

Notes on lecture, research and/or reading

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Practice: Percent Composition Use your periodic table to make the following calculations:

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Practice: Empirical Formula Use your periodic table to make the following calculations:

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Practice: Molecular Formulas

Use your periodic table to make the following calculations:

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Review

Chemists relate units of counting, of mass, and of volume to a single quantity called the -

_________________________. The number of representative particles in a mole of a substance is

_________________________. To find the mass of a mole of a compound, scientists add together the

_________________________ of the atoms making up the compound. When you substitute the unit grams for AMU,

you obtain the _________________________ of the compound. There are _________________________

representative particles in a mole of any substance.

At STP (0°C and 1 atmosphere pressure), one mole of any gas occupies a volume of

_________________________ L. This quantity is known as the _________________________ of the gas. To

determine the volume in liters of 2.00 mol of SO2 gas at STP, you would use _________________________ as a

conversion factor. _________________________ expressed in the units g/L, is used as a conversion factor when

converting from _________________________ to molar mass. When converting between numbers of representative

particles, _________________________, and volumes, you must always convert to _________________________ as

an intermediate step.

The _________________________ of a compound is the percent by mass of each element in a compound. The

percent by mass of an element in a compound is the number of grams of the element per

_________________________ g of the compound, multiplied by 100%. To calculate the percent by mass of an

element in a known compound, divide the mass of the element in one mole by the _________________________ and

multiply by 100%. A(n) _________________________ formula represents the lowest _________________________

ratio of the elements in a compound. It can be calculated from a compound’s percent composition. The

_________________________ formula of a compound is either the same as its empirical formula, or it is some whole-

number multiple of it.