The Mole Concept for Chemistry Interactive Notebooks - Aiken ...

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Table of ContentsPage 3 – Terms of Purchase & CopyrightPages 4-5 – Procedures for class set-upPage 6 – Customization for resizing IGOsPages 7-8 – Instructions for Note PagesPages 9-20 – Student Note PagesPages 21-26 – Student Notes Pages Key

Pages 27-28 – Hexagon Mole FoldPages 29-30 – Mole PyramidPages 31-33 – Empirical & Molecular Formula FoldPages 34-35 – Empirical Formula Layer PyramidPages 36-41 – The Mole-dable (6-Flap)

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Interactive Graphic Organizers (IGOs)

All of my Interactive Graphic Organizers (IGOs) have the

same basic format for teacher/student prep:

= cut on dotted line(s) only= fold on solid black line(s)

cut on dotted lines onlyfo

ld o

n so

lid b

lack

line

(s)


Determine which version works for you. [composition book, spiral notebook, and/or lapbook]


Did you print an IGO and it did not fit inside your notebook or lapbook?

You should be able to resize the document prior to printing [depending on

your PDF software].

Look for the Custom Scaleoption in Adobe software [boxed in black above]

I used a mixture of 75%, 85%, and 100% for the IGOs. Play around with the customization to determine what size works for your class.

Half Sheet Notes IGOsThe IGO notes come in half sheets (1 page per 2 students). There are a total of 12 note/activity sheets for students covering the following topics:• The Mole Concept• Percent Composition• Empirical Formula• Molecular Formula

• The following topics have been cycled into the notes as well for review purposes:

• Ionic Nomenclature• Covalent Nomenclature

Student Notes (pgs. 9-20) / Answer Key (pgs. 21-26)

Students should fill in the blanks as the teacher is lecturing. The teacher may decide to cover 1 sheet at a time and incorporate one or more of the IGOs found in this product;

although, it is not required. Answer keys are provided.

Half Sheet Notes IGOsSupplemental Activities (pgs. 13, 14, and 16)

The first two scenarios will vary per class. The teacher may decide the numbers/ratios for these activities. Therefore, a key is not provided.

This activity is not required; however, it is one that I have done prior to teaching moles. Please refer to my blog post by clicking here. You may use any object for this activity.

This activity is not required; however, it is one that I have done while teaching Percent Composition. I normally use Dubble Bubble gum (cheap $$$). You may also talk about potential errors concerning this lab (e.g. weighing chewed gum with saliva)

http://www.bondwithjames.com/2013/11/chemistry-jit-4-mole-stoichiometry.html

The Mole

When you hear or read the phrase, “The Mole”, you might be inclined to think of a small burrowing animal or a secret agent. However, a mole in chemistry is a very important term and your understanding of this concept will be critical to your success.

Before, we talk about what a mole in chemistry means, let us complete a quick activity…

Fill in the blanks:

A dozen pencils = ____ pencils 2 dozen apples = ____ apples

A dozen cars = _____ cars 6 dozen birds = _____ birds

Data Table:

Object Set 1 Mass (grams)

Set 2 Mass (grams)

Set 3 Mass (grams)

Directions & Questions: 1. One at a time, separate each object into three different groups

of a dozen.

2. Weigh each set and record in the data table above.

3. Answer the following questions on the back of this page.

a. In general, what could be said about the mass of a dozen _____________?

b. Could the same rule be applied to the other 3 objects?

c. You had a dozen of each object. Did you have the same amount of each object?

d. You had a dozen of each object. Did each set of objects

have the same mass?

The Mole



Fill in the blanks:

A dozen pencils = ____ pencils 2 dozen apples = ____ apples

A dozen cars = _____ cars 6 dozen birds = _____ birds

Data Table:


Set 2 Mass (grams)

Set 3 Mass (grams)


of a dozen.



a. In general, what could be said about the mass of a dozen _____________?

b. Could the same rule be applied to the other 3 objects?

c. You had a dozen of each object. Did you have the same amount of each object?


have the same mass?

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The Mole

A mole is a ______________ unit. It is abbreviated ______ and is a unit used in chemistry that allows us to deal with numbers of atoms, molecules, ions, or formula units in a sample of a substance.

***Chemists have define a mole as the number of carbon atoms in exactly 12g of pure carbon-12. Just like a dozen is equal to _____ of something and a pair is equal to ____ of something, chemists have established that… …a mole is equal to __________________ of “something”

In chemistry, the “something” refers to particles (________________,

________________, ____________, or _____________ _________).

Just like the number 3.14159 has a name - pi (π), 6.02 x 1023 has a name. It is called _______________________________.

Now, would you say a dozen pencils weigh the same as a dozen cars? Of course not! While the ___________ of both objects is the same, we would expect the ________ of a dozen pencils and cars to be different.

A mole of anything represents the same __________ (_______ x 1023) but it does NOT represent the _________ _______ for all substances.

The mole is the link between ____________ and _____________.

The MASS of 1 mole is equal to the _______________of a substance.

Quick Check: Take 2-3 minutes to complete the table below.

Substance 1 mole of a substance Mass (g) Oxygen (O) Bromine (Br)

Gold (Au) Water (H2O)

Sodium carbonate (Na2CO3)

The Mole

A mole is a ______________ unit. It is abbreviated ______ and is a unit used in chemistry that allows us to deal with numbers of atoms, molecules, ions, or formula units in a sample of a substance.

***Chemists have define a mole as the number of carbon atoms in exactly 12g of pure carbon-12. Just like a dozen is equal to _____ of something and a pair is equal to ____ of something, chemists have established that… …a mole is equal to __________________ of “something”

In chemistry, the “something” refers to particles (________________,

________________, ____________, or _____________ _________).

Just like the number 3.14159 has a name - pi (π), 6.02 x 1023 has a name. It is called _______________________________.

Now, would you say a dozen pencils weigh the same as a dozen cars? Of course not! While the ___________ of both objects is the same, we would expect the ________ of a dozen pencils and cars to be different.

A mole of anything represents the same __________ (_______ x 1023) but it does NOT represent the _________ _______ for all substances.

The mole is the link between ____________ and _____________.

The MASS of 1 mole is equal to the _______________of a substance.


Substance 1 mole of a substance Mass (g) Oxygen (O) Bromine (Br)

Gold (Au) Water (H2O)

Sodium carbonate (Na2CO3)

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The Mole

Useful conversion factors 1 mole = 6.02 x 1023 particles (atoms, molecules, ions, formula units)

1 mole = grams (molar mass) of a substance

We can write each conversion factor two ways – the way in which one is used over another will depend on the dimensional analysis setup.

Practice Problems I Do: How many grams are in 2 mol of NaCl?

I Do: How many grams are in 4.95 mol of Na3PO4?

We Do: How many moles are in 7.14 grams of H2O?

The Mole




Practice Problems I Do: How many grams are in 2 mol of NaCl?

I Do: How many grams are in 4.95 mol of Na3PO4?


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Formula Weights You may see the following terms: Formula Mass Molecular Mass Molar Mass

These terms all pretty much refer to the same thing in regard to doing calculations.

For now, let us refer to this concept as __________ ________ because this term will be important when doing a specific type of calculation in chemistry. These problems are pretty easy.

You need to know two things: 1. ________________________________________________ 2. _____________________________________ (ex: C6H12O6)

I Do: What is the molar mass of glucose, C6H12O6?

You Do: What is the molar mass of sodium sulfate, Na2SO4?



For now, let us refer to this concept as __________ ________ because this term will be important when doing a specific type of calculation in chemistry. These problems are pretty easy.

You need to know two things: 1. ________________________________________________ 2. _____________________________________ (ex: C6H12O6)



Atom # of Each Periodic Table

Atomic Mass Total

x =

x =

x =

Atom # of Each

Periodic Table Atomic Mass Total

x =

x =

x =

Atom # of Each


x =

x =

x =

Atom # of Each


x =

x =

x =

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Moles in my Signature

Purpose: ________________________________________________

________________________________________________________

________________________________________________________

Materials: _______________________________________________

________________________________________________________

Procedure:

1. Obtain a piece of chalk and measure its mass on the triple beam balance. Record the mass in your data table.

2. Write your signature on a piece of paper (or you may be asked to write your signature outside on the concrete).

3. Measure the mass of your unused chalk on the triple beam

balance.

Data: Initial Mass Final Mass Mass of

chalk used Molar Mass Chalk

(CaCO3)

Calculations:

Based on the mass of the chalk used and its molar mass, determine the number of moles of chalk you used to write your signature. Show your work in the space provide below.

Moles in my Signature

Purpose: ________________________________________________

________________________________________________________

________________________________________________________

Materials: _______________________________________________

________________________________________________________

Procedure:



3. Measure the mass of your unused chalk on the triple beam

balance.

Data: Initial Mass Final Mass Mass of

chalk used Molar Mass Chalk

(CaCO3)

Calculations:


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Percent Composition The _______________ _____________ tells us the ____________ of a certain component _______________________ an item.

Imaginary Pizza Scenario

• If you ate ___ out of _____ slices, what percentage of the pizza did you eat? ______

• Explain how you developed your answer?__________________________________________________________________________

Real-Time Scenario (Male to Female Class Ratio)

• Count your classmates. Total: ___________

• Male count _____ Female count _____

• % of males _____ % of females ____

• Code the appropriate number of boxes in the graphic on the right to illustrate this.

Educational Scenario (Grade Calculation)

• You take a quiz that has 10 problems. You miss 3. What is your grade?_________

• You take a test that has 36 problems. You miss 8. What is your grade? _________

• How did you come up with your answers? _________________________________________________

_________________________________________________

Percent Formula

Percent Composition The _______________ _____________ tells us the ____________ of a certain component _______________________ an item.










• You take a quiz that has 10 problems. You miss 3. What is your grade?_________

• You take a test that has 36 problems. You miss 8. What is your grade? _________


_________________________________________________

Percent Formula

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If you ate ___ out of _____ slices, what

______________________________________________________

_

Code the appropriate number of boxes in the

You take a test that has 36 problems. You miss 8.

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______________________________________________________

Male count _____ Female count _____

Code the appropriate number of boxes in the

You take a quiz that has 10 problems.


Percent Composition Information needed to calculate the percent composition of a substance:

I Do: Calculate the percent composition of tetraphosphorus pentoxide.

We Do: Calculate the percent composition of potassium sulfate.

You Do: Calculate the percent composition of iron (III) oxide.

Review the previous three examples. Which is a better source of oxygen? Explain why.





Review the previous three examples. Which is a better source of oxygen? Explain why.

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Percent Composition Activity

OBJECTIVE: To determine the percent of sugar in an ordinary piece of bubble gum.

PURPOSE: - Why are you doing this lab (in 1 to 2 sentences) - Must be stated in your own words

MATERIALS: - List of all the materials used in your experiment

PROCEDURE: - A step-by-step account of how you carried out your experiment.

DATA: - Include a data table to showcase the data collected during the

lab.

CALCULATIONS: - Show all calculations that you did using the data collected

during the lab.

ANALYSIS: Show ALL work!!!

1. What is the percent sugar in your gum?

2. How many moles of sugar, C6H12O6, did you chew?

3. How many molecules of sugar were in your gum?

CONCLUSION:

- Summarize the results of the lab activity







lab.


during the lab.





CONCLUSION:


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Emperical Formula

What is an empirical formula?

The _____________________ _________________ of a compound, in simple terms, is a formula which has been ________________ to the lowest terms. Scientists can use the _________________ ______________ of a compound to calculate and determine the formula for that compound.

Empirical Formula Calculation Steps

1. ______________ to ______________

• Assume that you have a 100-gram sample of the compound.

Therefore, convert the ____________ into _______________.

2. ______________ to ______________

• Convert grams to ________________.

3. ______________ by ______________

• Divide all the values calculated in # ____ by the _____________ value calculated.

4. ______________ til’ ______________

• Multiply all values from # ____by a number until each set produces a __________ number. Begin with a small number and increase until you are able to get whole numbers

5. Use as _______________ and place ___________.

• Use the whole numbers obtained in #____ as subscripts in order to write the empirical formula. List the elements in the order that __________________________________________________.

• Don’t be surprise if you have large subscripts as some molecules are very large.

Emperical Formula


The _____________________ _________________ of a compound, in simple terms, is a formula which has been ________________ to the lowest terms. Scientists can use the _________________ ______________ of a compound to calculate and determine the formula for that compound.


1. ______________ to ______________


Therefore, convert the ____________ into _______________.

2. ______________ to ______________

• Convert grams to ________________.

3. ______________ by ______________

• Divide all the values calculated in # ____ by the _____________ value calculated.

4. ______________ til’ ______________

• Multiply all values from # ____by a number until each set produces a __________ number. Begin with a small number and increase until you are able to get whole numbers

5. Use as _______________ and place ___________.

• Use the whole numbers obtained in #____ as subscripts in order to write the empirical formula. List the elements in the order that __________________________________________________.


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Emperical Formula

We do: Find the empirical formula for a compound which contains 26.8% Sn, 16.0% Cl and 57.2% I.

You Do: NutraSweet is 57.14% C, 6.16% H, 9.52% N, and 27.18% O. Calculate the empirical formula of NutraSweet.

Emperical Formula



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Molecular Formula

What is a molecular formula?

A molecular formula is the ______________ formula of a compound.

Let us review some common empirical and molecular formulas below:

Based on the table above, how is the molecular formula different from the empirical formula? ________________________________________________________ ________________________________________________________ Based on the table above, can the molecular formula be identical (the same) as the empirical formula? ________________________________________________________ ________________________________________________________ Definition: The molecular formula may be the _______________ formula or it may a ____________________________________________ of the ______________ formula.

Molecular Formula


A molecular formula is the ______________ formula of a compound.


Based on the table above, how is the molecular formula different from the empirical formula? ________________________________________________________ ________________________________________________________ Based on the table above, can the molecular formula be identical (the same) as the empirical formula? ________________________________________________________ ________________________________________________________ Definition: The molecular formula may be the _______________ formula or it may a ____________________________________________ of the _______________ formula.

Name Empirical Formula

Molecular Formula

Water H2O H2O

Hydrogen peroxide HO H2O2

Glucose CH2O C6H12O6

Dinitrogen monoxide NO N2O4

Caffeine C4H5N2O C8H10N4O2


Molecular Formula

Water H2O H2O






Molecular Formula

Water H2O H2O





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Molecular Formula

How do you determine the molecular formula?

To determine the molecular formula of a compound, you must know the compound’s _________________________ formula and the ______________ ____________ of the compound.

Molecular Formula Calculation Steps: 1. Determine the empirical formula IF it has NOT be given [review your

empirical formula calculation notes]. 2. Calculate the ___________ ___________ of the empirical formula. 3. Use the molecular formula mass (usually given in the problem) and

divide it by the empirical formula mass (calculated in Step 2).

Molecular formula mass Empirical formula mass

4. Using the number calculated in Step 3, ____________ that number by the subscripts in the empirical formula to obtain the subscripts for the molecular formula.

Practice Time! We Do: The empirical formula of a compound is C4H9. What is the molecular formula of this compound if the molar mass is 114 g/mol? You Do: What is the molecular formula of Nutrasweet if the molar mass of NutraSweet is 294.30 g/mol?

**Review the “You Do” section of your Empirical Formula notes for the empirical formula of Nutrasweet (as this was calculated there).

**Complete your work on the back of this sheet.

Molecular Formula


To determine the molecular formula of a compound, you must know the compound’s _________________________ formula and the ______________ ____________ of the compound.


empirical formula calculation notes]. 6. Calculate the ___________ ___________ of the empirical formula. 7. Use the molecular formula mass (usually given in the problem) and



8. Using the number calculated in Step 3, ____________ that number by the subscripts in the empirical formula to obtain the subscripts for the molecular formula.


**Review the “You Do” section of your Empirical Formula notes for the empirical formula of Nutrasweet (as this was calculated there).

**Complete your work on the back of this sheet.

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The Mole



Fill in the blanks:

A dozen pencils = _12_ pencils 2 dozen apples = _24_apples

A dozen cars = _12_ cars 6 dozen birds = _72_birds

Data Table:


Set 2 Mass (grams)

Set 3 Mass (grams)

Your choice Your choice Your choice Your choice


of a dozen.



a. In general, what could be said about the mass of a dozen (select one of the choices from above to place here)

b. Could the same rule be applied to the other 3 objects? Yes

c. You had a dozen of each object. Did you have the same amount of each object? Yes, a dozen = 12


have the same mass? No, the mass varied

The Mole

A mole is a ___counting_____ unit. It is abbreviated mol and is a unit used in chemistry that allows us to deal with numbers of atoms, molecules, ions, or formula units in a sample of a substance.

***Chemists have define a mole as the number of carbon atoms in exactly 12g of pure carbon-12. Just like a dozen is equal to 12 of something and a pair is equal to 2 of something, chemists have established that… …a mole is equal to 6.02 x 1023 of “something”

In chemistry, the “something” refers to particles ( atoms, molecules, ions , or formula units)

Just like the number 3.14159 has a name - pi (π), 6.02 x 1023 has a name. It is called Avogadro’s number.

Now, would you say a dozen pencils weigh the same as a dozen cars? Of course not! While the amount of both objects is the same, we would expect the mass of a dozen pencils and cars to be different.

A mole of anything represents the same amount (6.02 x 1023) but it does NOT represent the same mass for all substances.

The mole is the link between particles and grams.

The MASS of 1 mole is equal to the molar mass of a substance.


Substance 1 mole of a substance Mass (g) Oxygen (O) 6.02 x 1023 16.00 Bromine (Br) 6.02 x 1023 79.90

Gold (Au) 6.02 x 1023 196.97 Water (H2O) 6.02 x 1023 18.02

Sodium carbonate (Na2CO3) 6.02 x 1023 105.99

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The Mole




1 mole 6.02 x 1023 particles

6.02 x 1023 particles 1 mole

1 mole ??? molar mass (g) ??? molar mass (g) 1 mole

Practice Problems I Do: How many grams are in 2.00 mol of NaCl?

2.00 mol NaCl 58.45 g NaCl = 116.88 g = 117 g NaCl

1 mole NaCl

We Do: How many grams are in 4.95 mol of Na3PO4?

4.95 mol Na3PO4 163.94 g Na3PO4 = 811.503 g Na3PO4

1 mol Na3PO4 = 812 g Na3PO4


7.14 g H2O 1 mol H2O = 0.396 mol H2O 18.02 g H2O



For now, let us refer to this concept as molar mass because this term will be important when doing a specific type of calculation in chemistry. These problems are pretty easy.

You need to know two things: 1. How to find the mass of an element on the Periodic Table 2. How to count atoms in a chemical formula (ex: C6H12O6)



Atom # of Each Periodic Table

Atomic Mass Total

C 6 x 12.01 = 72.06

H 12 x 1.01 = 12.12

O 6 x 16.00 = 96.00

= 180.18 g/mol

Atom # of Each


Na 2 X 23.00 = 46.00

S 1 X 32.01 = 32.01

O 4 X 16.00 = 64.00

= 142.01 g/mol

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Moles in my Signature Purpose: to determine the number of moles used to write my signature

________________________________________________________

Materials: chalk, triple beam balance, other materials as needed

________________________________________________________

Procedure:



3. Measure the mass of your unused chalk on the triple beam balance.

Data:Initial Mass Final Mass Mass of

chalk used Molar MassChalk

(CaCO3)

Calculations:


This will vary depending on how you conduct the activity. Students may each receive a piece of chalk or work in pairs. You may also take them outside to write on the concrete or use a sheet of paper instead.

Percent Composition The percent composition tells us the amount of a certain componentwithin an item.










• You take a quiz that has 10 problems. You miss 3. What is your grade? 70%

• You take a test that has 36 problems. You miss 8. What is your grade? 78%


_________________________________________________

Percent Formula

Part x 100

Whole

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______________________________________________________

_

he appropriate number of boxes in the



• The total mass (may need to calculate the molar mass) • The number of each type of atom • The mass of each type of atom




Review the previous three examples. Which is a better source of oxygen? Explain why. P4O5 because it contains a higher % of oxygen per compound compared to K2SO4 and Fe2O3







lab.


during the lab.





CONCLUSION:


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Emperical Formula


The empirical formula of a compound, in simple terms, is a formula which has been reduced to the lowest terms. Scientists can use the empirical formula of a compound to calculate and determine the formula for that compound.


1. Percent to mass


Therefore, convert the percent into grams.

2. Mass to mole

• Convert grams to moles.

3. Divide by small

• Divide all the values calculated in # 2 by the smallest value calculated.

4. Multiply til’ whole

• Multiply all values from # 3 by a number until each set produces a whole number. Begin with a small number and increase until you are able to get whole numbers

5. Use as subscripts and place below.

• Use the whole numbers obtained in #4 as subscripts in order to write the empirical formula. List the elements in the order that they appear in the problem (in most cases).


Emperical Formula



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Molecular Formula


A molecular formula is the actual formula of a compound.


Based on the table above, how is the molecular formula different from the empirical formula? From the table above, the molecular formulas, for most of the compounds are a whole number multiple (of the subscripts) of the empirical formula. Based on the table above, can the molecular formula be identical (the same) as the empirical formula? The molecular and empirical formulas may be identical for some compounds. Definition: The molecular formula may be the actual formula or it may a whole number multiple of the empirical formula.

Molecular Formula


To determine the molecular formula of a compound, you must know the compound’s empirical formula and the molar mass of the compound.


empirical formula calculation notes]. 2. Calculate the molar mass of the empirical formula. 3. Use the molecular formula mass (usually given in the problem) and



4. Using the number calculated in Step 3, multiply that number by the subscripts in the empirical formula to obtain the subscripts for the molecular formula.



Molecular Formula

Water H2O H2O





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This IGO comes 1 page per 2 students. It is also pre-filled with information, unless you wish to add more to it.

Students may use this to assist them during 1 or 2 step mole conversions

Hexagon Mole Fold IGO(pg. 28)

Tape or glue bottom here

1 mole

6.02 x 1023(particles, atoms, molecules, formula units, ions)

(?) molar mass(must calculate for each substance)

1-2 StepMole Conversions

1 mole

6.02 x 1023(particles, atoms, molecules, formula units, ions)

(?) molar mass(must calculate for each substance)

1-2 StepMole Conversions

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Mole Pyramid IGO(pg. 30)

This IGO comes 1 page per 2 students. The directions are also included on the page for students to follow. Pictures A and B: Fold section #1 behind section #2. Picture C: Fold section #2 behind section #3. Pictures D and E: Fold section #3 behind section #4.Picture F: Finally, unfold the organizer and place section #1 directly behind section #4 to form a pyramid. Tape or glue the tab “The Mole Concept” into the notebook.

Recreating, scanning, electronic copying, file sharing, redistributing, editing, selling, or posting this item (or any part thereof) on the Internet, or with others, is strictly prohibited. Violations are subject to the penalties of the Digital Millennium Copyright Act. © James Lyas (Bond with James)

Directions: Cut along the dotted lines only. 1st: Fold section #1 behind section #2. 2nd: Fold section #2 behind section #3. 3rd: Fold section #3 behind section #4.Finally, unfold the organizer and place section #1 directly behind section #4 to form a pyramid. Tape or glue the tab “The Mole Concept” into your notebook.

Recreating, scanning, electronic copying, file sharing, redistributing, editing, selling, or posting this item (or any part thereof) on the Internet, or with others, is strictly prohibited. Violations are subject to the penalties of the Digital Millennium Copyright Act. © James Lyas (Bond with James)

Directions: Cut along the dotted lines only. 1st: Fold section #1 behind section #2. 2nd: Fold section #2 behind section #3. 3rd: Fold section #3 behind section #4.Finally, unfold the organizer and place section #1 directly behind section #4 to form a pyramid. Tape or glue the tab “The Mole Concept” into your notebook.

Empirical Formula & Molecular Formula Fold IGO(pg. 32-33)

Use the “Steps” provided in the Half-sheet notes to fill in the blanks on both tabs. The information on the front face could be used to write the definitions of the empirical and molecular formulas.

Make sure to cut along the small dotted line shown here in order for the IGO to properly fold in.

Molecular Formula Empi

rical

Form

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C6 H

12 O6

CH2O

Example: Empirical Formula

Molecular Formula

Step 1: __________________

Step 2:__________________

Step 3: __________________

Step 4: __________________

Step 5: ___________________________

Step 1: _________________________________

Step 2:_________________________________

Step 3: ____________________________________________

Step 4: ____________________________________________

Automobile antifreeze is composed of 38.7% carbon, 9.7% hydrogen, and 51.6% oxygen.

The molar mass of this compound is 62.1 g/mol. Determine the empirical and

molecular formulas of this compound.

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Empirical Formula Layered Pyramid IGO(pg. 35)

This IGO comes 1 page per student. Place the largest piece into the notebook first and then layer until the smallest piece is on top. You may glue the bottom piece in or tape it at the bottom to create a layering effect. You will need to do this for each piece.

Students may write notes concerning each step on the backside of each layer. They may even work a short empirical formula problem behind the last layer as students should have space to write directly on the back of the layer and on the notebook paper.

Multiple ‘til Whole

Percent to MassRecreating, scanning, electronic copying, file sharing, redistributing, editing, selling, or posting this item (or any part thereof) on the Internet, or with others, is strictly prohibited. Violations are subject to the penalties of the Digital Millennium Copyright Act. © James Lyas (Bond with James)

x 2x 3

x 4


Mole Flaps IGO(pgs. 40-41)

Cut along the dotted lines only – this is important to create the small tab shown at the very top. You may label the top: “Start with…” and “End with…” as shown in the picture.

You may print this sheet front and back; or you may print out the side with MOLES written on it and have students write on the 3 units on the outside flap instead.

This IGO prints 1 page per student regardless of the method in which you decide to print the sheet.

Example problem:How many liters are represented in 150.0 g CO2 at STP?

Step 1:The problem starts with mass (150.0 g CO2). Therefore, select the Mass (grams) tab under the Start with… column

Step 2: While not indicated, these are all equalities equaling 1 mole of a substance

Step 3: Problem asks for liters. Therefore, select the Volume of a Gas tab under the End With… column

How does this work?

Example #2:How many atoms are in 10.0 grams of Aluminum?

Step 3: Problem asks for atoms. Therefore, select the Representative Particles tab under the End With… column

Step 1: The problem starts withmass (10.0 g Al). Therefore, select the Mass (grams) tab under the Start with… column

Step 2: While not indicated, these are all equalities equaling 1 mole of a substance

How does this work?

Will not work for these types of questions:The IGO does not account for problems such as these. Only specific to the units on the foldable.

How many atoms are in 0.010 g CaCO3?

How many oxygen atoms are present in 0.714 mole of SO3

MOLES

Divide by

22.4 L/mol

Divide by

6.02 x 1023

(Avogadro’s number)

Divide by

Molar mass (g/mol)

Multiply by

x

22.4 L/mol

Multiply by

x

6.02 x 1023

(Avogadro’s number)

Multiply by

x

Molar mass (g/mol)

PRINT

ON

FRONT

PRINT

ON

FRONT

PRINT

ON

BACK

Volume of a gas at

STP (liters)

Representative Particles (atoms,

molecules, formula units)

Mass(grams)

Volume of a gas at

STP (liters)

Representative Particles (atoms,

molecules, formula units)

Mass(grams)

PRINT

ON

BACK

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