1. THE MOLE CONCEPT AND ITS APPLICATIONS
CHEMICAL QUANTITIES
THE MOLE CONCEPT AND ITS APPLICATIONS

2. Chemical Quantities Objectives Students will be able to
Understand and know
the definitions of the mole and Avogadro’s Number
relationship between moles and mass
relationship between moles and particles
Calculate the formula mass of a compound given the periodic table
Calculate the mass percent composition of a compound given the formula, formula mass, and periodic table.

3. Drill & Objectives How many eggs are there in a dozen?
If I bought 3 dozen eggs, how many eggs do I have?
What are some ways that you can measure things? (such as the amount of a substance)
Objectives
Students will be able to
Understand and know
the definitions of the mole and Avogadro’s Number
relationship between moles and mass
relationship between moles and particles
Calculate the formula mass of a compound given the periodic table
Calculate the mass percent composition of a compound given the formula, formula mass, and periodic table.

4. Chemical Quantities
How many eggs are there in a dozen?
12!

5. Chemical Quantities
How many roses are there in a dozen roses?
12!

6. Chemical Quantities
Does it matter what the _____________ is?

7. Chemical Quantities Does it matter what the _____________ is?
NO! A Dozen is a dozen! No matter if it’s flowers, eggs, bagels, ect.
It represents a number of _______

8. Chemical Quantities In Chemistry the same concept is valid,
Let’s talk about “The Mole” and how it relates to Chemistry…

9. The Mole?

10. The Mole?

11. The Mole? “The Mole” or “A Mole” is an amount of a substance
There are 6.02 x1023 atoms (representative particles of a substance) in 1 Mole (of that substance).
This number (6.02 x1023) is called Avogadro’s number
Named after Amedeo Avogadro di Quarenga (1776 – 1856), an Italian scientist.

12. The Mole! Let’s put this into perspective 6.023 x 1023!!
How much is 1 mol of a substance?
6.023 x 1023!!

13. The Mole!
IF you had 6.02 X 1023  Watermelon Seeds…

14. The Mole! IF you had 6.02 X 1023 Watermelon Seeds…
it would be found inside a watermelon slightly larger than the moon!

15. The Mole!
If you had 6.02 X 1023 Grains of Sand…

16. The Mole! IF you had 6.02 X 1023 Grains of Sand…
it would be more than ALL the sand on Miami Beach.

17. The Mole?
A mole is the amount of substance or representative particles of any substance.
Therefore, as we have just seen
1 mol of N2 there are 6.02x1023 MOLECULES of N2
1 mol of C12H22O11 has how many molecules?
6.02x1023 can be used for “atoms” if they are the same element OR
It can be used for “molecules” for many elements that are together, via compounds.

18. Chemical Quantities
How many moles of Magnesium is 3.01x1022 atoms of magnesium?
Step 1 - What do we know?
We know that there are 3.01x1022 atoms of Mg
Step 2 - What do we want know?
We want to know the number of moles of Mg
Step 3 – What do we know that can be used for these conversions?
We know that there are 6.02x1023 atoms in 1 mol
Step 4 – Solve the problem

19. Chemical Quantities = 5.00x10-2 mol Mg
How many moles of Magnesium is 3.01x1022 atoms of magnesium?
1 mol Mg
3.01x1022 atoms Mg X
6.02x1023 atoms of Mg
= 5.00x10-2 mol Mg

20. Chemical Quantities Individual Problems
How many moles are 1.20x1025 atoms of phosphorus?
How many atoms are in mol of Zinc?
How many molecules are there in 4 mol of glucose, C6H12O6?
How many molecules are there in 0.44 mol N2O5

21. Chemical Quantities
Now there is a difference between asking how many atoms are there in the entire compound and how many atoms of one of the compound there are.
We said that there are the same number or atoms in a compound or a diatomic molecule. However, there is a difference between these questions…
How many atoms are there in aluminum fluoride?
VS.
How many fluoride ions are there in aluminum fluoride?

22. Chemical Quantities So let’s answer the question.
How many fluoride ions are there in 1.46 mol of aluminum fluoride?
If we follow the four steps that we went through prior

23. NO! Chemical Quantities
How many fluoride ions are there in 1.46 mol of aluminum fluoride?
Step 1 - What do we know?
We know that there are 1.46 mol of aluminum fluoride
Step 2 - What do we want know?
We want to know the number of F-
Step 3 – What do we know that can be used for these conversions?
NO!
We know that there are 6.02x1023 atoms in 1 mol
BUT is that enough information??

24. AlF3 Chemical Quantities
How many fluoride ions are there in 1.46 mol of aluminum fluoride?
We want to know the number of F-
But how can we find out the number of fluoride ions we have from what is given?
We can get the information we need by writing out the chemical formula of the compound.
AlF3

25. Chemical Quantities
How many fluoride ions are there in 1.46 mol of aluminum fluoride?
6.02x1023 Formula units of AlF3
1.46 mol AlF3 X X
1 mol AlF3
3 F- ions
= x 1023 F- ions
1 formula unit AlF3

26. Individual Work
How many ammonium ions are in mol ammonium phosphate, (NH4)3PO4?

27. DRILL What is Avogadro's number?
How many particles are there in 1 mol of a substance?
How many atoms are there in 1.45 mol of Na?

28. Chemical Quantities
The Gram Formula Mass

29. Chemical Quantities
Chemists have defined the gram atomic mass as the number of grams of an element that is numerically equal to the atomic mass in amu
The Gram atomic mass is the mass of one mole of atoms of a monatomic element
This can also be described as MOLAR MASS – in place of gram formula mass to refer to the mass of a mole of any element or compound.
I will be using the term Molar Mass more frequently

30. Chemical Quantities
Atomic Mass Number

31. Chemical Quantities Therefore, there are 47.88 grams/mol of Ti
This number tells you how many grams of this element there are in 1 mol of the element
Therefore,
there are grams/mol of Ti
Or there are grams of Ti IN 1 mol of Ti

32. The molar mass in grams/mol
Chemical Quantities B C N O F
10.811g g g g
18.998g
The molar mass in grams/mol

33. Chemical Quantities
You can calculate the total molecular weight of a molecule by adding up the molar masses of each element.
The molar mass of the molecule SO4 is equal to
S = g/mol x 1 S = g/mol
O = g/mol x 4 O = g/mol
SO4 = g/mol
I will specify the amount of significant figures needed in your answer

34. Individual Work What is the molar mass of the following compounds?
REMEMBER YOUR UNITS!
PCl3
Sodium Carbonate
C8H18
Aluminum Sulfate
(NH4)2CO3

35. Chemical Quantities Why is this important? Let’s do a calculation…
This is important because it will allow us to covert from moles to grams and grams to moles, allowing for quantitative experimentation.
Let’s do a calculation…
How many grams are in 7.20 mol of dinitrogen trioxide?

36. Chemical Quantities
How many grams are in 7.20 mol of dinitrogen trioxide?
Step 1 – add up the total molar mass of the compound
If it is in word form, write the chemical formula
Step 2 – Set up the proper conversion factors
Step 3 – Solve

37. Chemical Quantities
How many grams are in 7.20 mol of dinitrogen trioxide?
Step 1 – add up the total molar mass of the compound
If it is in word form, write the chemical formula
N2O3
N = 14.0 g/mol x 2 N = 28.0 g/mol
O = 16.0 g/mol x 3 O = 48.0 g/mol
N2O3 = 76.0 g/mol

38. Chemical Quantities
How many grams are in 7.20 mol of dinitrogen trioxide?
Step 2 – Set up the proper conversion factors
Step 3 – Solve

39. Individual Work Find the mass of the following
3.32 mol K
5.08 mol Ca(NO3)2
4.52x10-3 mol K2CO3
Find the number moles of the following
g Li2HPO4
847g (NH4)2CO3
195g calcium nitrate

40. Exit Ticket
Does g of Mn have the same number of moles as that of g of Cd? Explain why or why not.

41. DRILL What is Avogadro’s number?
How many moles are there in 245 kg of CH2COOH?
Does g of Mn have the same number of moles as that of g of Cd? Explain why or why not.

42. Group Work Find the mass (g) of the following:
10.0 mol Cr
2.20x10-3 mol Sn
0.720 mol Be
2.40 mol N2
4.52x10-3 mol C20H42
mol Potassium Carbonate
Find the number of moles of the following:
72.0 g Ar
3.70x10-1 g B
333 g Tin (II) Fluoride
7.21x10-2 g He
27.4 g TiO2

43. The Volume of a Mole of Gas
Chemical Quantities
The Volume of a Mole of Gas

44. Chemical Quantities
How would we measure the amount of moles in a gas?

45. Chemical Quantities
The volume of a gas is usually measured at STP (Standard Temperature and Pressure)
STP conditions
Temperature
0°C
Pressure
1 atmosphere (atm)

46. Chemical Quantities
At STP conditions 1 mol of ANY gas occupies a volume of 22.4 Liters (L) 22.4 Liters of a gas / 1 mol of the gas 22.4 L of a gas contains 6.02 x 1023 representative particles of that gas This is known as the molar volume of a gas

47. Chemical Quantities What were the units of the molar volume of a gas?
Liters
What kind of unit is liters?
VOLUME
Therefore, 1 mol of any gas occupies the same volume not mass

48. Chemical Quantities He 22.4 L N2 6.02 x 1023 molecules of N2 28g of N2Ne
22.4 L CO2
6.02 x 1023 molecules of CO2
44g of CO2
CO2
22.4 L He
6.02 x 1023 molecules of He 4g

49. Individual Work
What is the volume at STP of these gases? 5.40 mol O x 10-2 mol CO2 Assuming STP conditions, how many moles are there in these volumes 74.6 L SO2 5.78x10-2 N2

50. Chemical Quantities
Because the molar volume of a gas is a VOLUME, we can relate density (mass over volume) of a gas to determine the mass of the gas. If we have a gas that has a density of g/L we can multiply the density with the molar volume of a gas (22.4 L) to calculate the mass of the gas x 22.4 L = 44.0g

51. Group Work
The densities of gases A, B, & C are 1.25 g/L, 2.86 g/L, and g/L, respectively. Calculate the molar mass of each of these substances and compare them to the molar mass of ammonia, sulfur dioxide, chlorine, nitrogen, and methane Identify the gasses A, B, & C

52. Chemical Quantities Atoms (6.02 x 10 23) 1mol Molar Mass
Solids and Liquids
1 mol
22.4 L
Gases

53. Homework problems Copy them down!
Calculate the volume of each of these gases at STP
9.6 mol He
4.8 mol N2
How many moles is each of the following, assuming STP
56.o L N2O
0.224 L O2
Find each of the following quantities
The mass of 18.0L of CH4 (STP)
The volume in liter, of 835 g of SO3 (STP)

54. Drill What are STANDARD conditions?
How many liters are there in 1 mol of gas?
Does it matter which gas it is? Why or why not?

55. Chemical Quantities
Percent Composition

56. Chemical Quantities- % Composition
Calculating Percent Composition
Percent Composition
The percent by mass of each element in a compound
They must add up to 100%
Ex. K2CrO4
40.3% K
26.8% Cr
32.9% O
100% Total

57. Chemical Quantities - % Composition
Percent Mass of an element in a compound is the number of grams of the element divided by the grams of the compound, multiplied by 100% % mass = x 100%
Grams of element
Grams of compound

58. Chemical Quantities- % Composition
Let’s look at our example again
K2CrO4
STEP 1
Calculate the Total Molecular Mass of K2CrO4
– Go ahead a calculate that now
K = 39 g x 2K = 78 g
Cr = 52 g
O = 16 g x 4O = 64g
K2CrO4 = 194g
Have them calculate it out

59. Chemical Quantities- % Composition
Let’s look at our example again
K2CrO4
STEP 2
Using the individual molar mass of each element, divide each element with the total molar mass
Go ahead and calculate that now with 3 Significant figures
K = 39 g x 2K = 78 g K ÷194g = .402
Cr = 52 g ÷194g = 0.268
O = 16 g x 4O = 64g ÷194g = 0.330

60. Chemical Quantities- % Composition
Let’s look at our example again
K2CrO4
STEP 3
Multiply the number calculated from Step 2 and multiply by 100%
Go ahead and calculate that now
K = 39 g x 2K = 78 g K ÷194g = .402 x 100% = 40.2% K
Cr = 52 g ÷194g = x 100% = 26.8% Cr
O = 16 g x 4O = 64g ÷194g = x 100% = 33% O

61. Chemical Quantities- % Composition
Individual Work
Calculate the mass of carbon in 82g in C3H8
Calculate the percent composition of each of these compounds.
Propane, C3H8
Sodium bisulfate, NaHSO4
Calcium acetate, Ca(C2H3O2)2
Hydrogen cyanide, HCN

62. Closure
Take the remainder of this period and write down in complete sentences what you learned today, approximately 2-3 paragraphs.

63. DRILL What is percent composition?
What is the formula for percent composition?

64. DRILL
Calculate the mass of oxygen in 142g of Sodium bisulfate, NaHSO4

65. Chemical Quantities
Empirical Formulas

66. Chemical Quantities- Empirical Formulas
Empirical Formula Gives the lowest whole number ratio of the elements in a compound. This ratio is not necessarily the molecular formula! Calculating the empirical formula is going to require the use of almost everything you’ve learned so far. Each element in the compound would require different amounts depending on the mass and % composition

67. Chemical Quantities- Empirical Formulas
Steps to solve for an Empirical Formula
Write down the base formula AxBY
Convert whatever you have into moles using dimensional analysis
Divide each element by the lowest number of moles in the compound
Round if necessary to the nearest 10ths place and/or multiply by a number to get a whole number ratio
Write down the Empirical Formula

68. Chemical Quantities- Empirical Formulas
What is the empirical formula of a compound that is 25.9% Nitrogen and 74.1% Oxygen?
STEP 1 - Write down the base formula AxBY…
NxOy

69. Chemical Quantities- Empirical Formulas
What is the empirical formula of a compound that is 25.9% Nitrogen and 74.1% Oxygen? STEP 2 - Convert whatever you have into moles using dimensional analysis
Because this is a % composition, we know that everything has to add up to 100%; therefore, we can assume that if we had 100g total of the compound, there would be 25.9g of N and 74.1g of O

70. Chemical Quantities- Empirical Formulas
What is the empirical formula of a compound that is 25.9% Nitrogen and 74.1% Oxygen? STEP 2 - Convert whatever you have into moles using dimensional analysis
1 mol N
25.9g of N x
= 1.85 mol N
14.0 g N
1 mol O
74.1g of O x
= 4.63 mol O
16.0 g O

71. Chemical Quantities- Empirical Formulas
What is the empirical formula of a compound that is 25.9% Nitrogen and 74.1% Oxygen?
STEP 3 - Divide each element by the lowest number of moles in the compound
1 mol N
25.9g of N x = 1.85 mol N
74.1g of O x = 4.63 mol O
÷ 1.85 mol = 1 mol N
14.0 g N
1 mol O
÷ 1.85 mol = 2.5 mol O
16.0 g O

72. Chemical Quantities- Empirical Formulas
What is the empirical formula of a compound that is 25.9% Nitrogen and 74.1% Oxygen?
STEP 4 - Round if necessary to the nearest 10ths place and/or multiply by a number to get a whole number ratio
1 mol N x ____ =
2.5 mol O x ____ = 2
2 mol N 2
5 mol O

73. Chemical Quantities- Empirical Formulas
What is the empirical formula of a compound that is 25.9% Nitrogen and 74.1% Oxygen?
STEP 5 - Write down the Empirical Formula
2 mol N 5 mol O
N2O5

74. Chemical Quantities- Molecular Formulas
The Molecular formula
is the actual formula of a molecular compound
While the empirical formula give us the base ratio of the compound, the molecular formula will give the actual molecular formula by using the molar mass.
x (empirical formula) = molecular formula
Ratio of the compounds

75. Chemical Quantities- Molecular Formulas
Therefore, if you have the molar mass of the compound and divide it by the molar mass of the empirical formula, you will get the ratio between the two.
Multiply the ratio to each element of the compound to get the the molecular formula.

76. Chemical Quantities- Molecular Formulas
Ex. If the empirical formula was calculated to be CH4N and the known molecular formula molar mass is = to 60g
1st – Take the molar mass of the empirical formula CH4N
In this case it is calculated to be 30g/mol
2nd – Divide the known molar mass of 60g/mol and divide it by 30 g/mol 60/30 = 2
3rd – Take the ratio of the two molar masses and then multiply it by each element of the compound C1x2H4x2N1x2= C2H8N2

77. Chemical Quantities- Molecular Formulas
Write the Molecular Formula for the problem below
The compound methyl butanoate has a percent composition of 58.8% C, 9.8% H, 31.4%O. If its molecular mass is 102 g/mol, what is it’s molecular formula?
Write the Empirical Formula for the following
79.8% C 20.2% H
67.6% Hg 10.8% S 21.6% O
27.59% C 1.15% H 16.09%N 55.17%O
17.6% Na 39.7%Cr 42.7%O

78. DRILL
What is the difference between an empirical formula and molecular formula?

79. Chemical Quantities – Review
Determine the Empirical Formula with the parameters
below
71.72% Cl, 16.16% O, and 12.12%C
What is the molecular formula for the compound below?
The compound’s empirical formula and molar mass is given
Below
HgCl, g/mol
Determine the molecular formula for the compound
94.1%O and 5.9% H ; molar mass = 34g
Find the empirical formula for each compound from its percent composition
72.4% Fe and 27.6% O
52.8% Sn, 12.4% Fe, 16.0% C, and 18.8% N
A&W pg 139
45b, 47b, 48b, 52a, 52c