If I had a million dollars…If I had a million dollars…

SongSong

If I had a million dollars…If I had a million dollars…

You are an incredibly valuable student and I want to reward you.  You have 2 options for receiving your reward:  

Option 1: You can either come to school for 10 days straight and receive one million dollars (regular 7 hour school day)

or

Option 2: You can earn a dollar per second up to one million dollars.  

You would like to buy an elite condo in the Bahamas that costs exactly one million dollars.  Which deal will allow you to purchase the condo first?

You are an incredibly valuable student and I want to reward you.  You have 2 options for receiving your reward:  

Option 1: You can either come to school for 10 days straight and receive one million dollars (regular 7 hour school day)

or

Option 2: You can earn a dollar per second up to one million dollars.  

You would like to buy an elite condo in the Bahamas that costs exactly one million dollars.  Which deal will allow you to purchase the condo first?

How many Apple Jacks are in the container? (NO counting!)

How many Apple Jacks are in the container? (NO counting!)

On your white boards, you and your partner will develop a procedure for determining the number of Apple Jacks in the container

You have a smaller container and scale for reference

The mass of the apple jacks = 230.1g

On your white boards, you and your partner will develop a procedure for determining the number of Apple Jacks in the container

You have a smaller container and scale for reference

The mass of the apple jacks = 230.1g

Data – your estimateData – your estimate

Data – the actual quantity!Data – the actual quantity!

There are 682 apple jacks in the large container!

There are 682 apple jacks in the large container!

BRN – fill in the blanks #1-5BRN – fill in the blanks #1-5

When you buy eggs you usually ask for a (1)____________ eggs. You know that one dozen of any item is (2)_________.

Paper is not packaged by the dozen, it is packaged by the ream. A ream of paper has 500 sheets. Why is it useful to use units like a dozen or a ream? (3) ________________________

What determines how many items should make up a particular unit? (4) ___________________________________________

If you were asked to design a new unit to count something, what would you consider when choosing how many items should be included in your new counting unit?

(5) _______________________________________

When you buy eggs you usually ask for a (1)____________ eggs. You know that one dozen of any item is (2)_________.

Paper is not packaged by the dozen, it is packaged by the ream. A ream of paper has 500 sheets. Why is it useful to use units like a dozen or a ream? (3) ________________________

What determines how many items should make up a particular unit? (4) ___________________________________________

If you were asked to design a new unit to count something, what would you consider when choosing how many items should be included in your new counting unit?

(5) _______________________________________

When given the number of KNIGHTS…When given the number of KNIGHTS…

_________________________________ by a KNIGHT to find the number of items

_________________________________ by a KNIGHT to find the number of items

When given the number of items…When given the number of items…

________________________________ by a KNIGHT to find the number of KNIGHTS

________________________________ by a KNIGHT to find the number of KNIGHTS

The mole…The mole…

One MOLE of anything has 602,200,000,000,000,000,000,000 items.

This number is called AVOGADRO’S NUMBER and is usually written in scientific notation as 6.022 x 1023

One MOLE of anything has 6.022 x 1023 items

One MOLE of anything has 602,200,000,000,000,000,000,000 items.

This number is called AVOGADRO’S NUMBER and is usually written in scientific notation as 6.022 x 1023

One MOLE of anything has 6.022 x 1023 items

The moleThe mole

When given the number of moles, we ______________________ by Avogadro’s number to find the number of items

When given the number of items, we _______________________ by Avogadro’s number to find the number of moles

When given the number of moles, we ______________________ by Avogadro’s number to find the number of items

When given the number of items, we _______________________ by Avogadro’s number to find the number of moles

ClosureClosure

Here’s How: How do we determine the number of moles when given the number of particles?

Here’s How: How do we determine the number of moles when given the number of particles?

Mole NotesMole Notes

Dimensional AnalysisDimensional Analysis

The factor-label method was developed to keep track of units in multi-step conversion problems (also known as dimensional analysis). In the method, equalities (i.e., conversion factors)

are set up in fraction form. The equalities are then lined up sequentially and units used on the top and bottom of neighboring fractions are alternated so that units cancel.

Crash Course

The factor-label method was developed to keep track of units in multi-step conversion problems (also known as dimensional analysis). In the method, equalities (i.e., conversion factors)

are set up in fraction form. The equalities are then lined up sequentially and units used on the top and bottom of neighboring fractions are alternated so that units cancel.

Crash Course

Dimensional AnalysisDimensional Analysis

For example, consider the conversion of inches to centimeters (1.00 in = 2.54 cm).

How many centimeters are in 5.00 inches?

For example, consider the conversion of inches to centimeters (1.00 in = 2.54 cm).

How many centimeters are in 5.00 inches?

= SignThe word perThe word forThe word in

= SignThe word perThe word forThe word in

Conversion FactorsConversion Factors

Dimensional AnalysisDimensional Analysis

1. Determine what the question is asking you to solve for.

2. Determine what is given in the problem to be converted.

3. Identify and plug in the appropriate conversion factors as fractions (what is on top must also be on bottom).

4. Cancel units

5. Verify your answer. (Units must match units in step 1. If the answer doesn’t match, repeat 3 and 5).

Dimensional AnalysisDimensional Analysis

• For the next few months, we will be doing a lot of math and calculations.

Self-Motivated PracticeSelf-Motivated Practice

Self-Motivated PracticeSelf-Motivated Practice

YOU WILL NEED A CALCULATOR EVERY DAY!!! YOU WILL NEED A CALCULATOR EVERY DAY!!!

Self-Motivated PracticeSelf-Motivated Practice

The correct answer on these quizzes are worth very little.

Therefore you will not get any credit (0/10) if you do not show your work (Factor- Labeling).

Let me repeat this: A quiz with the correct answer but no work shown will get a score of (0/10).

Show and write out the work!

The correct answer on these quizzes are worth very little.

Therefore you will not get any credit (0/10) if you do not show your work (Factor- Labeling).

Let me repeat this: A quiz with the correct answer but no work shown will get a score of (0/10).

Show and write out the work!

The MOLEThe MOLE

KC 1: The mole (mol) is an SI base unit used to measure the amount of a substance.

KC 2: 1 mole is equal to the number 6.02 x 1023

particles.

KC 3: Avogadro’s number is another name for the value of one mole, 6.02 x 1023.

mole video

KC 1: The mole (mol) is an SI base unit used to measure the amount of a substance.

KC 2: 1 mole is equal to the number 6.02 x 1023

particles.

KC 3: Avogadro’s number is another name for the value of one mole, 6.02 x 1023.

mole video

AvogadroAvogadro

In 1811 Avogadro hypothesized that equal volumes of gases at the same temperature and pressure contain equal numbers of molecules

Determining the number: If you divide the charge on a mole of electrons by

the charge on a single electron you obtain a value of Avogadro’s number of 6.02214154 x 1023 particles per mole.

In 1811 Avogadro hypothesized that equal volumes of gases at the same temperature and pressure contain equal numbers of molecules

Determining the number: If you divide the charge on a mole of electrons by

the charge on a single electron you obtain a value of Avogadro’s number of 6.02214154 x 1023 particles per mole.

Counting ParticlesCounting Particles

There are three types of representative particle; atom, molecule, and formula units.The unit atom is used with single element.

The unit molecule is used with covalently bonded element (2 non-metals).

The unit formula units are used with ionicly bonded elements (1 metal and 1 non-metal).

There are three types of representative particle; atom, molecule, and formula units.The unit atom is used with single element.

The unit molecule is used with covalently bonded element (2 non-metals).

The unit formula units are used with ionicly bonded elements (1 metal and 1 non-metal).

PracticePractice

KC 4: How many formula units of NaCl (sodium chloride) are in 43.4 moles?

KC 4: How many formula units of NaCl (sodium chloride) are in 43.4 moles?

PracticePractice

KC 5: How many moles of copper are there in 1.54 x 1023 atoms of Cu?

KC 5: How many moles of copper are there in 1.54 x 1023 atoms of Cu?

PracticePractice

KC 6: Calculate the number of particles in 2.15 moles of iron.

KC 6: Calculate the number of particles in 2.15 moles of iron.

How big is a mole?How big is a mole?

1 Mole of marbles would fill the entire Grand Canyon and there would still be enough left over to displace all the water in Lake Michigan and a few other lakes!

Computers can count at the rate of over 800 million counts per second. At this rate it would take a computer over 25 million years to count to 6.02 x 1023

1 Mole of marbles would fill the entire Grand Canyon and there would still be enough left over to displace all the water in Lake Michigan and a few other lakes!

Computers can count at the rate of over 800 million counts per second. At this rate it would take a computer over 25 million years to count to 6.02 x 1023

How big is a mole?How big is a mole?

A mole of hockey pucks would be equal to the mass of the Moon.

Assuming that each human being has 60 trillion body cells (6.0 x 1013) and the Earth's population is 6 billion (6 x 109), the total number of living human body cells on the Earth at the present time is 3.6 x 1023 or a little over half of a mole.

A mole of hockey pucks would be equal to the mass of the Moon.

Assuming that each human being has 60 trillion body cells (6.0 x 1013) and the Earth's population is 6 billion (6 x 109), the total number of living human body cells on the Earth at the present time is 3.6 x 1023 or a little over half of a mole.

Mass of a moleMass of a mole

What does 1 Knight of skittles and 1 Knight of sprees have in common?

What is different about a Knight of skittles and sprees?

What does 1 mole of copper and 1 mole of carbon have in common?

What is different about 1 mole of copper and 1 mole of carbon?

Think-Pair-Share WHY?

What does 1 Knight of skittles and 1 Knight of sprees have in common?

What is different about a Knight of skittles and sprees?

What does 1 mole of copper and 1 mole of carbon have in common?

What is different about 1 mole of copper and 1 mole of carbon?

Think-Pair-Share WHY?

Mass of a moleMass of a mole

Chemical Formula

Moles of Sample

Mass of Sample

Molecular Mass

 Al 1 mol 26.982g  

 NaCl 1 mol 58.443g  

 MgO 1 mol 40.304g  

MgSO4 1 mol 120.366g

Mass of a moleMass of a mole

1 mol of copper and 1 mol of carbon have different masses because they have different numbers of protons, neutrons, & electrons

1 mol of copper and 1 mol of carbon have different masses because they have different numbers of protons, neutrons, & electrons

Mass of a moleMass of a mole

Key Concept 7: A mole always contains the same number of particles; however, moles of different substances have different masses.

Key Concept 7: A mole always contains the same number of particles; however, moles of different substances have different masses.

Chemical Formulas and the MoleChemical Formulas and the Mole

Chemical formulas indicate the numbers and types of atoms contained in one unit of the compound

One dozen molecules of CCl2F2 contains 12 C atoms, 2(12) Cl atoms, and 2(12) F atoms.

Similarly, one mole of CCl2F2 contains one mole of C atoms, two moles of Cl atoms, and two moles of F atoms

Chemical formulas indicate the numbers and types of atoms contained in one unit of the compound

One dozen molecules of CCl2F2 contains 12 C atoms, 2(12) Cl atoms, and 2(12) F atoms.

Similarly, one mole of CCl2F2 contains one mole of C atoms, two moles of Cl atoms, and two moles of F atoms

Mass of a moleMass of a mole

Key Concept 8 - Molecular Mass: (atomic mass, formula mass) of a molecule is its average mass as calculated by adding together the atomic weights of the atoms in the formula.

MM QT

Key Concept 8 - Molecular Mass: (atomic mass, formula mass) of a molecule is its average mass as calculated by adding together the atomic weights of the atoms in the formula.

MM QTMM= Molecular MassQ= quantityT= Total

MMQT - NaOHMMQT - NaOH

MM Q T

Na

O

H

Total =

CONVERSION FACTOR ALERT

Mass of a moleMass of a mole

Key Concept 9 - Molar mass is the mass in grams of one mole of any pure substance.

Key Concept 10 - The molar mass of any element is numerically equivalent to its molecular mass (atomic mass, formula mass) and has the units g/mol

Key Concept 9 - Molar mass is the mass in grams of one mole of any pure substance.

Key Concept 10 - The molar mass of any element is numerically equivalent to its molecular mass (atomic mass, formula mass) and has the units g/mol

Mass of a moleMass of a mole

Key Concept 11: What is the molar mass of the following compounds? Potassium sulfate

(NH4)2CO3

Key Concept 11: What is the molar mass of the following compounds? Potassium sulfate

(NH4)2CO3

Converting using molesConverting using moles

Conversion factors so far… Conversion factors so far…

Converting using molesConverting using moles

Key Concept 12: How many grams of zinc are there in 1.5 moles of Zn?

Key Concept 13: How many molecules of carbon dioxide are there 4.0g of carbon dioxide?

Key Concept 12: How many grams of zinc are there in 1.5 moles of Zn?

Key Concept 13: How many molecules of carbon dioxide are there 4.0g of carbon dioxide?

Converting using molesConverting using moles

Key Concept 14: Gold (Au) is one of a group of metals called coinage metals (copper, silver, and gold). How many atoms of gold are in a U.S. Eagle, a gold bullion coin with a mass of 31.1g Au?

Key Concept 14: Gold (Au) is one of a group of metals called coinage metals (copper, silver, and gold). How many atoms of gold are in a U.S. Eagle, a gold bullion coin with a mass of 31.1g Au?

Converting using molesConverting using moles

Key Concept 15: The characteristic odor of garlic is due to allyl sulfate [(C3H5)2S]. What is the mass of 2.50 mol of (C3H5)2S ?

Key Concept 15: The characteristic odor of garlic is due to allyl sulfate [(C3H5)2S]. What is the mass of 2.50 mol of (C3H5)2S ?

Converting using molesConverting using moles

Key Concept 16: Aluminum chloride (AlCl3) is used in refining petroleum and manufacturing rubber and lubricants. A sample of aluminum chloride has a mass of 35.6g. How many formula units are present?

Key Concept 16: Aluminum chloride (AlCl3) is used in refining petroleum and manufacturing rubber and lubricants. A sample of aluminum chloride has a mass of 35.6g. How many formula units are present?

Percent Composition of an OreoPercent Composition of an Oreo

Obtain an Oreo. The cookie is made up of WAFER and CREAMY FILLING.

Using a balance, a plastic knife and a napkin (to keep the cookie from directly touching the balance), calculate the percent of the cookie that is made up of each part.

You have 15 minutes to complete and be ready to explain the process and your answer

Obtain an Oreo. The cookie is made up of WAFER and CREAMY FILLING.

Using a balance, a plastic knife and a napkin (to keep the cookie from directly touching the balance), calculate the percent of the cookie that is made up of each part.

You have 15 minutes to complete and be ready to explain the process and your answer

Percent Composition of a CompoundPercent Composition of a Compound

KC 17: Mass percent composition – percent of total mass of a substance contributed by each element in the substance

Found from comparing the mass of each element to the total mass of the substance

KC 17: Mass percent composition – percent of total mass of a substance contributed by each element in the substance

Found from comparing the mass of each element to the total mass of the substance

Percent CompositionPercent Composition

KC 18: Calculate the percent composition of water (H2O)

KC 18: Calculate the percent composition of water (H2O)

Percent CompositionPercent Composition

KC 19: Calculate the mass percent of oxygen in sodium sulfate.

KC 19: Calculate the mass percent of oxygen in sodium sulfate.

Percent CompositionPercent Composition

KC 20: Calculate the percent composition of nitrogen in calcium nitrate

KC 20: Calculate the percent composition of nitrogen in calcium nitrate

Empirical vs. Molecular FormulaEmpirical vs. Molecular Formula

KC 21: Molecular formula – formula of the molecule as found in nature

KC 22: Empirical formula – simplest ratio of atoms in a molecule

Example –

C6H12O6 vs. CH2O

KC 21: Molecular formula – formula of the molecule as found in nature

KC 22: Empirical formula – simplest ratio of atoms in a molecule

Example –

C6H12O6 vs. CH2O

Empirical vs. Molecular FormulaEmpirical vs. Molecular Formula

Circle the compounds that are given as empirical formulas: CaO

Mg2(SO4)2

Be2S2

LiCl

C6H12O6

Circle the compounds that are given as empirical formulas: CaO

Mg2(SO4)2

Be2S2

LiCl

C6H12O6

Formula Mass vs. Molecular MassFormula Mass vs. Molecular Mass

The formula mass (formula weight) of a molecule is the sum of the atomic weights of the atoms in its empirical formula

KC 23: Formula mass = empirical formula

The molecular mass (molecular weight) of a molecule is its average mass as calculated by adding together the atomic weights of the atoms in the molecular formula

KC 24: Molecular mass = molecular formula

Example –

C6H12O6 vs. CH2O

180 g/mol 30 g/mol

The formula mass (formula weight) of a molecule is the sum of the atomic weights of the atoms in its empirical formula

KC 23: Formula mass = empirical formula

The molecular mass (molecular weight) of a molecule is its average mass as calculated by adding together the atomic weights of the atoms in the molecular formula

KC 24: Molecular mass = molecular formula

Example –

C6H12O6 vs. CH2O

180 g/mol 30 g/mol

Percent Composition and Empirical FormulaPercent Composition and Empirical Formula

KC 25:

1. Assume 100g of the sample. Use the percentages as your grams

2. Convert the grams to moles for each element

3. Divide each of the moles by the lowest number of moles present to get a whole number

4. Round the number of moles as necessary or multiply each mole number by a fraction to get a whole number

5. Use the whole numbers to write the empirical formula

KC 25:

1. Assume 100g of the sample. Use the percentages as your grams

2. Convert the grams to moles for each element

3. Divide each of the moles by the lowest number of moles present to get a whole number

4. Round the number of moles as necessary or multiply each mole number by a fraction to get a whole number

5. Use the whole numbers to write the empirical formula

Percent Composition and Empirical FormulaPercent Composition and Empirical Formula

Given data on percent composition of a compound, you can find the empirical formula

Example – Lactic acid is 40% carbon, 6.71% hydrogen, and 53.3% oxygen by mass. Calculate the empirical formula.

Given data on percent composition of a compound, you can find the empirical formula

Example – Lactic acid is 40% carbon, 6.71% hydrogen, and 53.3% oxygen by mass. Calculate the empirical formula.

Percent Composition and Molecular FormulaPercent Composition and Molecular Formula

To determine the molecular formula from the empirical formula you need the molar mass

KC 26: molar mass given in problem = wholemolar mass of empirical formula found number

Example – Lactic acid has a molar mass of 90.08g/mol. Determine its molecular formula.

To determine the molecular formula from the empirical formula you need the molar mass

KC 26: molar mass given in problem = wholemolar mass of empirical formula found number

Example – Lactic acid has a molar mass of 90.08g/mol. Determine its molecular formula.

PracticePractice

KC 27: A compound is found to have 9.2% boron and 90.8% chlorine. Determine the empirical formula

KC 27: A compound is found to have 9.2% boron and 90.8% chlorine. Determine the empirical formula

PracticePractice

KC 28: A compound is shown to contain 50.1% sulfur and 49.9% oxygen. The molar mass of the compound is 128 g/mol. Determine the compound’s molecular formula.

KC 28: A compound is shown to contain 50.1% sulfur and 49.9% oxygen. The molar mass of the compound is 128 g/mol. Determine the compound’s molecular formula.