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The MOLE…. Everything we’ve done so far in chemistry has dealt with individual atoms or moleculesEverything we’ve done so far in chemistry has dealt with.

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Presentation on theme: "The MOLE…. Everything we’ve done so far in chemistry has dealt with individual atoms or moleculesEverything we’ve done so far in chemistry has dealt with."— Presentation transcript:

1 the MOLE…

2 Everything we’ve done so far in chemistry has dealt with individual atoms or moleculesEverything we’ve done so far in chemistry has dealt with individual atoms or molecules –However, it isn’t practical to work with 1 atom or 1 molecule or even 1,000,000 atoms or molecles –They are just too small! Therefore, chemists don’t work with 1 atom or even 1,000,000 atoms, they work with a huge collection of atomsTherefore, chemists don’t work with 1 atom or even 1,000,000 atoms, they work with a huge collection of atoms Counting Atoms

3 It is impractical to get caught up into working with 1 atom or 1 atom’s mass.It is impractical to get caught up into working with 1 atom or 1 atom’s mass. –It makes more sense to work with a collection of atoms rather than individually Counting Atoms Scientists were challenged to figure out a way to define a universal collection of particlesScientists were challenged to figure out a way to define a universal collection of particles –And which could still be described in terms of a relative mass

4 We’ve already got the periodic table with masses for each elementWe’ve already got the periodic table with masses for each element –So how many atoms are in that collection (assuming gram masses) –That number of atoms would immediately connect all other atoms and give us measurable amounts Counting Atoms

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6 The number of atoms that are in the gram mass on the PT is called Avogadro’s NumberThe number of atoms that are in the gram mass on the PT is called Avogadro’s Number And is defined as 1 moleAnd is defined as 1 mole Counting Atoms The mole becomes a counting unit much like the dozen.The mole becomes a counting unit much like the dozen. –1 dozen eggs = 12 eggs –1 mole of eggs =

7 The word “mole” was introduced by Wilhelm Oswald, who derived the term from the word moles meaning a “heap” or “pile.”The word “mole” was introduced by Wilhelm Oswald, who derived the term from the word moles meaning a “heap” or “pile.” –We are just defining the pile as con- taining 6.02x10 23 items –Any time we are counting how many we have and we want to describe it in terms of moles than… Counting Atoms

8 The mole, whose abbreviation is “mol”, is the SI base unit for measuring amount of a pure substance.The mole, whose abbreviation is “mol”, is the SI base unit for measuring amount of a pure substance. –It’s used exclusively for counting atoms, molecules, ions, or other things that are extremely small –It’s the chemist’s six-pack or dozen. Many objects in our everyday lives come in similar counting units. 1 ream = 500 sheets of paper1 ream = 500 sheets of paper 1 pair of socks = 2 socks1 pair of socks = 2 socks 1 cube = 24 cans1 cube = 24 cans Counting Atoms

9 We will learn in the near future that when a chemist reasons through a chemical reaction (recipe) they think in terms of X number of mols of this compound reacts with Y number of mols of this compound.We will learn in the near future that when a chemist reasons through a chemical reaction (recipe) they think in terms of X number of mols of this compound reacts with Y number of mols of this compound. –So we need to know how to calculate the number of molecules or atoms are involved in that X number of mols Counting Atoms

10 Using the mole in calculations #1 Counting Atoms How many moles is equivalent to 1.355x10 24 atoms of Au? unit equality: 1 mol Au = 6.02 x atoms Au

11 The desired conversion is: atoms  moles Counting Atoms 6.02x10 23 atoms Au 1 mole Au 1.355x10 24 atoms Au = mol Au

12 Using the mole in calculations #2 Counting Atoms How many molecules of carbon dioxide is mols? How many molecules of carbon dioxide is mols? unit equality: 1 mol CO 2 = 6.02x10 23 molecules of CO 2

13 The desired conversion is: moles  atoms Counting Atoms 6.02x10 23 molecules CO 2 1 mole CO mols CO 2 = 2.15x10 22 molecules CO 2

14 Your Turn: Make the following mole conversions using dimensional analysis 1) mols of Na to atoms 2)2.55x10 25 molecules of CO 2 to mols 3)1.89x10 19 molecules of H 2 O to mols 4)1.25 mols of O 2 to molecules

15 Now suppose you want to determine how many atoms are in a mol of a compound or moleculeNow suppose you want to determine how many atoms are in a mol of a compound or molecule –To do this you must know how many atoms are involved in the molecule. To determine the number of atoms represented in a molecule requires knowing the chemical formulaTo determine the number of atoms represented in a molecule requires knowing the chemical formula –Eg, each molecule of Carbon Dioxide (CO 2 ) is composed of 3 atoms Counting Atoms

16 Using the mole in calculations #3 Counting Atoms How many atoms of Carbon are in 2.12 mols of Propane (C 3 H 8 )? unit equalities: 1 mol C 3 H 8 = 6.02x10 23 molecules C 3 H 8 1 molecule C 3 H 8 = 3 atoms C

17 6.02x10 23 molecules C 3 H 8 1 mole C 3 H 8 The desired conversions are: 2.12 mols C 3 H 8 3 atoms C 1 molecule C 3 H 8 =3.83x10 24 atoms C Counting Atoms moles  molecules  atoms

18 Your Turn: Make the following mole conversions using dimensional analysis 1)How many atoms of Oxygen are there in mols of CO 2 2)How many atoms of Oxygen are there in Ca(NO 3 ) 2.

19 We can’t literally count the number of atoms in a sample, but we can count them by massWe can’t literally count the number of atoms in a sample, but we can count them by mass –So, there needs to be a connection between the mass of a sample and the number of moles in that sample –If we weigh out a particular mass of a substance, that can represent a particular number of mols If we weighed out g of CarbonIf we weighed out g of Carbon –It will represent 1 mole of Carbon and/or 6.02x10 23 Carbon atoms Counting Atoms

20 This allows us to use the mass off of the periodic table to represent the mass of 1 mole (or 6.02x10 23 atoms) of that elementThis allows us to use the mass off of the periodic table to represent the mass of 1 mole (or 6.02x10 23 atoms) of that element –1 mol of C atoms weighs g –1 mol of H atoms weighs g –1 mol of W atoms weigh g Counting Atoms

21 This new understanding of mass from the periodic table is known as the gram molar mass, or molar mass.This new understanding of mass from the periodic table is known as the gram molar mass, or molar mass. –Molar Mass = mass of 1 mole of atoms in grams –We have a list of every possible molar mass for any given element on the periodic table This mass can be used as a conversion factor…1 mole = g H, etc.This mass can be used as a conversion factor…1 mole = g H, etc. Counting Atoms

22 So what if we have a compound instead of an element?So what if we have a compound instead of an element? How do we figure out the mass of a mole of a compound?How do we figure out the mass of a mole of a compound? –This would be called a molecular mass, formula mass, or still can be called a molar mass –All we need is the formula for a representative particle of the compound and the periodic table. Counting Atoms

23 For instance how do we calculate the mass of 1 mole of Ca(OH) 2 ?For instance how do we calculate the mass of 1 mole of Ca(OH) 2 ? You can calculate the mass of a mol- ecule of Ca(OH) 2 by breaking it up into individual piecesYou can calculate the mass of a mol- ecule of Ca(OH) 2 by breaking it up into individual pieces We can start with Calcium, then 2 O’s, then 2 H’s…until we run out of piecesWe can start with Calcium, then 2 O’s, then 2 H’s…until we run out of pieces Counting Atoms Ca: (1)(40.09 g/mol) = O: (2)(15.99 g/mol) = H: (2)(1.008 g/mol) = g/mol

24 (6C’S)(12.011g/mol) = 180.1g/mol (12H’S)(1.008 g/mol) = (6O’S)(15.99 g/mol) = 1 mole of C 6 H 12 O 6 or 6.02x10 23 molecules of the compound – weighs grams g/mol g/mol 95.94g/mol Counting Atoms What is the MM of glucose (C 6 H 12 O 6 )?

25 Practice Time: Calculate the molar mass of each of the formulas 1)C 9 H 20 2)(NH 4 ) 2 CO 3 3)Zn(C 2 H 3 O 2 ) 2 4)CCl 4

26 How many grams are in 9.45 mol of Dinitrogen Trioxide (N 2 O 3 ) The only connection to N 2 O 3 and its mass is how much 1 mol of the compound weighs. But, using it as a comparison we can calculate the mass of 9.45 mol. Counting Atoms Using the molar mass in calculations:

27 Counting Atoms Step 1: Determine the mass of 1 mol of N 2 O g (2N’s)(14.01g) = 28.02g (3O’s)(15.99g) = 75.99g If 1 mole of N 2 O 3 weighs 75.99g than how much will 9.45 mols of N 2 O 3 weigh?

28 1 mol N 2 O g N 2 O mol N 2 O 3 =718 g N 2 O 3 Counting Atoms Step 2: Convert the given moles to grams using the Molar mass equality.

29 Find the number of moles of 92.2g of Iron (III) Oxide (Fe 2 O 3 ) The only connection to the mass of Fe 2 O 3 and how that corresponds to mols is how that 1 mol of the compound weighs a certain # of grams. Using that we can figure out how many moles weigh 92.2 g Counting Atoms

30 47.97g (2Fe’s)(55.85g) = 111.7g (3O’s)(15.99g) = g If 1 mole of Fe 2 O 3 weighs g than how many mols will weigh 92.2 g of Fe 2 O 3 ? Counting Atoms Step 1: Determine the mass of 1 mol of Fe 2 O 3

31 g Fe 2 O 3 1 mol Fe 2 O g Fe 2 O 3 =.577mol Fe 2 O 3 Counting Atoms Step 2: Convert the given mass to mols using the Molar mass equality

32 Practice Time: Determine the number of mols of CO 2 in 454 grams.Determine the number of mols of CO 2 in 454 grams. What is the mass of mols of propane gas, C 3 H 8 ?What is the mass of mols of propane gas, C 3 H 8 ? How many mols of methane molecules, CH 4, are in grams of methane?How many mols of methane molecules, CH 4, are in grams of methane? How many grams does 3.40x10 -5 mols of Na 2 CO 3 weigh?How many grams does 3.40x10 -5 mols of Na 2 CO 3 weigh?

33 Another generality about the mole is that with matter in the gas phase we can develop another equality.Another generality about the mole is that with matter in the gas phase we can develop another equality. –Under the same conditions, equal volumes of gases contain equal numbers of particles. –1 mol of a gas will occupy the same volume as 1 mol of any other gas under the same conditions. Counting Atoms

34 1 mole of any gas under the specific conditions of 0°C and 1 atm (STP) will occupy a volume of 22.4 L. 6.02x10 23 molecules of O x10 23 molecules of CO 2 Molar Volume of a Gas

35 What volume, in Liters, does 0.60 mol of SO 2 gas occupy at STP? The only connection to the volume of any gas and how that corresponds to mols is that 1 mol of a gas occupies 22.4 Liters of space. Using that we can figure out the volume of 0.60 mols of a gas at STP. Counting Atoms

36 1 mole SO L SO moles SO 2 = 13 L SO 2 Step 1: Use the equality 1 mol = 22.4 L to do the conversion Counting Atoms

37 Practice Time: What volume is occupied by 12.5 mols of nitrogen gas at STP?What volume is occupied by 12.5 mols of nitrogen gas at STP? How many moles of gas would be in 15,000 L of air?How many moles of gas would be in 15,000 L of air?

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39 Aspartame is an artificial sweetener that is 160 times sweeter than sugar when dissolved in water. It is marketed as Nutra-Sweet (C 14 H 18 N 2 O 5 ). 1.What number of molecules are in 5.0 mg of aspartame? 2.What number of atoms of nitrogen are in 1.2 g of aspartame? 3.What is the mass in g of 1 molecule of aspartame? Counting Atoms

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42 Your Turn: What is the mass of 7.21x10 21 molecules of silver acetate (AgC 2 H 3 O 2 )?What is the mass of 7.21x10 21 molecules of silver acetate (AgC 2 H 3 O 2 )? How many grams of neon gas will fill a room with a volume of 4000L at STP?How many grams of neon gas will fill a room with a volume of 4000L at STP? How many molecules are there in 122 g of Cu(NO 3 ) 2 ?How many molecules are there in 122 g of Cu(NO 3 ) 2 ? Which has the greater mass?Which has the greater mass? a.9.5x10 24 atoms of C a.9.5x10 24 atoms of C b.2.1 mol Br 2 c.1.86x10 22 molecules of CCl 4 d.59.5g Hg


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