meet the mole.. o the mole is a unit of measurement. o the unit can be defined in multiple ways....
TRANSCRIPT
![Page 1: MEET THE MOLE.. o The mole is a unit of measurement. o The unit can be defined in multiple ways. (We’ll learn 3 today.) o In its simplest terms, it represents](https://reader035.vdocuments.mx/reader035/viewer/2022081520/56649ea05503460f94ba3fc6/html5/thumbnails/1.jpg)
MEET THE MOLE.
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oThe mole is a unit of measurement.oThe unit can be defined in multiple ways.
(We’ll learn 3 today.)oIn its simplest terms, it represents a
specific number. oDozen = what number?oPair = what number?oBaker’s dozen = what number?oMole = 6.02 x 1023
oAtoms are SUBmicroscopic. In order to have an amount large enough with which to really interact, we need quite a few atoms.
MOLES
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o6.02x1023
oMy pet mole is named Avogadro.
AVOGADRO’S NUMBER
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oCountingoWeighingoAmount
of Space Needed
DEFINING THE MOLE
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oSome questions simply test your understanding of the definitions.
oCalculate the molar mass of sulfur dioxide, a gas produced when sulfur-containing fuels are burned.
oSO2oS = 32.07 goO = 2(16.00 g)oTotal = 64.07 g/moloCan also be expressed as 1 mol SO2 = 64.07 g
MOLAR MASS EXAMPLE 6.5
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oPolyvinyl chloride, called PVC, which is widely used for floor coverings (“vinyl”) as well as for plastic pipes in plumbing systems, is made form a molecule with the formula C2H3Cl. Calculate the molar mass of this substance.
o62.49 g/mol
MOLAR MASS PRACTICE PROBLEM 6.5
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oMost questions will require you to apply the definitions to convert from one unit to another.
oAluminum (Al), a metal with a high strength-to-weight ratio and a high resistance to corrosion, is often used for structures such as high-quality bicycle frames. Compute both the number of moles in a 10.0-g sample of aluminum.
UNIT CONVERSION EXAMPLE 6.3
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A silicon chip used in an integrated circuit of a computer has a mass of 5.68 mg. How many silicon (Si) atoms are present in this chip? The average atomic mass for silicon is 28.09 amu.
UNIT CONVERSION EXAMPLE 6.4
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During cellular respiration, a cell releases 0.25 mol of O2 gas. What volume is needed to hold this gas?
UNIT CONVERSION EXAMPLE
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10-2 Practice Problems (1-3, 12-14, 17, 18, 23-25)
PARTNER PRACTICE
BACK TOGETHER WITH 10 MIN LEFT IN
CLASS.
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Exit Questi
on
Calculate the number of formula
units in a 45.0 gram sample of FeO.
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Exit Questi
on Groups
PROBLEM-BASED LEARNING ACTIVITY
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o Let’s make sure that we all understand how the particle vocabulary can complicate a problem.
o Consider: Calculate the number of oxygen atoms in 3.5 g aluminum sulfate.
o A few examples in your practice packet.
HIGHER LEVEL APPLICATIONS OF MOLE
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MOLE THINK
TAC TOE
CHOOSE A PARTNER. WORK IS DUE AT THE END OF
THE PERIOD.
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oThe relative amounts of each element in a compound are expressed in percent composition.
oAKA: percent by mass of each elemento% of element = grams of element X
100 grams of compound
PERCENT COMPOSITION
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Carvone is a substance that occurs in two forms, both of which have the same molecular formula (C10H14O) and molar mass. One type of carvone give caraway seeds their characteristic smell; the other is responsible for the smell of spearmint oil. Compute the mass percent of each element in carvone.
PERCENT COMPOSITION EXAMPLE 6.9
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o Mass % is easily related to chemical formulas
o The relationship of moles to chemical formulas requires a little more thought.
o First, let’s learn two new vocabulary words.
CONNECTING MOLES & MASS % TO CHEMICAL
FORMULAS
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o Empirical formula: lowest whole number ratio of the atoms of the elements in a compoundo Ionic compounds are criss-crossed and
then reduced. Ionic compound formulas are nearly always empirical formulas.
o Covalent compounds are not always reduced formulas. (Ex. C6H12O6)
o Therefore, an empirical formula doesn’t have to be the same as the actual molecular formula of the compound.
TYPE OF CHEMICAL FORMULA: EMPIRICAL
FORMULA
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CH2OCalculate the mass percent of each element.
C = 40% H = 6.7% O = 53.3%
Isn’t this the reduced formula for: C3H6O3, C4H8O4, C5H10O5, & C6H12O6
The mass percent of each of these compounds is the same.
EMPIRICAL FORMULA
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o Molecular formula: actual formula for the compound which gives the composition of the moleculeo Glucose shares an empirical formula
with many compounds, but it has its molecular formula all to itself.
o 6(CH2O) = glucose
TYPE OF CHEMICAL FORMULA: MOLECULAR
FORMULA
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o When an unknown compound is found, instruments can tell scientists the mass percent composition of the compound.
o Calculations are required to convert that series of percentages into a chemical formula.
o We start by converting to the empirical formula.
APPLYING THE VOCABULARY
Situation: A white solid has been found on the floor of a government mailroom. Is it dangerous? Step 1: Mass spectrometer analysis• 40.9 % Carbon• 4.58% Hydrogen• 54.5% Oxygen• Molar mass of 180
grams/moleStep 2: Convert % to formula with simple calculations
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Use a simple rhyme!o % to gramo Gram to moleo Divide by the
smallesto Multiply ‘til
whole.
CALCULATING EMPIRICAL FORMULA
Situation: A white solid has been found on the floor of a government mailroom. Is it dangerous? Mass spectrometer analysis• 40.9 % Carbon• 4.58% Hydrogen• 54.5% Oxygen• Molar mass of 180
grams/mole
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o An oxide of aluminum is formed by the reaction of 4.151 g of aluminum with 3.692 g of oxygen. Calculate the empirical formula for this compound.o % to gram = IS DONE FOR YOUo Gram to mole = dimensional analysiso Let’s carry out the calculation on the board.
EMPIRICAL FORMULA EXAMPLE 6.11
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A sample of lead arsenate, an insecticide used against the potato beetle, contains 1.3813 g of lead, 0.00672 g of hydrogen, 0.4995 g of arsenic, and 0.4267 g of oxygen. Calculate the empirical formula for lead arsenate.
EMPIRICAL FORMULA EXAMPLE 6.13
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The most common form of nylon is 63.68% carbon, 12.38% nitrogen, 9.80% hydrogen, and 14.4% oxygen. Calculate the empirical formula for nylon.
EMPIRICAL FORMULA EXAMPLE 6.14
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Molecular Formula= n(empirical formula)
(Remember 6(CH2O) = glucose)We know how to calculate the empirical formula, but how do we know what number to multiply it by?
n= actual formula mass/molar mass of empirical
CALCULATING MOLECULAR FORMULA
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A white powder is analyzed and found to have an empirical formula of P2O5. The compound has a molar mass of 283.88 g/mol. What is the compound’s molecular formula?
MOLECULAR FORMULA EXAMPLE 6.15
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o A compound used as an additive for gasoline to help percent engine knock shows the following percentage composition:o 71.65% Clo 24.27% Co 4.07% Ho The molar mass is known to be 98.96 g.
Determine the empirical formula and the molecular formula for this compound.
MOLECULAR FORMULA PRACTICE PROBLEM
6.15
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Mole Airlin
es
PROBLEM-BASED
LEARNINGDAY 1: FORENSIC
CHEMISTDAY 2: ASSISTANT
MEDICAL EXAMINER
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WARM UP FOR
QUIZ
The final product in protein metabolism is urea. Urea contains 20.00% C, 6.73% H, 46.65% N, and 26.64% O. The molar mass of urea is 60.07g/mol. Calculate the empirical formula and
molecular formula.
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Mole Airlin
es
PROBLEM-BASED
LEARNINGDAY 1: FORENSIC
CHEMISTDAY 2: ASSISTANT
MEDICAL EXAMINER