1. Chemical Composition

2. Learning Targets I can…
calculate formula weight, molecular weight, and molar mass.
calculate percent composition given a chemical formula.
convert between the mass, moles, and number of particles of a substance.

3. Atomic Masses: Counting Atoms by Weighing
Atoms are too tiny to be weighed in grams and kilograms.
Instead, we use the atomic mass unit, or amu
The atomic mass unit =1.66x10-24g
For example, the average atomic mass for carbon atoms is amu

4. Calculating Mass Using Atomic Mass Units (amu)
Calculate the mass, in amu, of a sample of aluminum that contains 75 atoms.
1 Al atom= amu
75 Al atoms x 26.98amu/Al atom=
2024 amu

5. Calculating Mass Using Atomic Mass Units (amu)
Calculate the mass, in amu, of a sample of nitrogen that contains 23 atoms.
1 N atom = amu
23 N atoms x amu/N atom=
322.2 amu

6. Calculating the Number of Atoms from the Mass
Calculate the number of sodium atoms present in a sample that has a mass of amu
1 Na atom = amu
amu x 1 Na atom/ amu=
51.00 Na atoms

7. Calculating the Number of Atoms from the Mass
Calculate the number of oxygen atoms in a sample that has a mass of 288 amu.
1 O atom = amu
288 amu x 1 O atom/ amu=
18.0 O atoms

8. The Mole
We have used atomic mass units for mass, but these are extremely small units.
In the laboratory a much larger unit, the gram, is the convenient unit for mass.
We will learn to count atoms in samples with masses given in atoms.

9. The Mole We have a sample of aluminum that has a mass of 26.98g.
What mass of copper contains exactly the same number of atoms as this sample of aluminum?
26.98g sample Al = ? Grams of Cu

10. To answer this question:
We need to know the average atomic masses for aluminum and copper:
Al= amu
Cu= amu
Which atom has the greater atomic mass, aluminum or copper?
Copper

11. To answer this question:
If we have g of aluminum, do we need more or less than g of copper to have the same number of copper atoms as aluminum atoms?
More
We need more than g of copper because each copper atom has a greater mass than each aluminum atom.

12. To answer this question:
What does this mean?
A given number of copper atoms will weigh more than an equal number of aluminum atoms.
How much copper do we need?
aluminum atoms are amu
Copper atoms are amu
26.98g of aluminum and 63.55g of copper contain exactly the same number of atoms

13. To answer this question:
Therefore:
26.98g of aluminum contains the same number of aluminum atoms as 63.55g of copper contains copper atoms.

14. Another example: Now compare carbon and helium
Does a 12.01g sample of carbon contain more or less or the same number of atoms as 4.003g of helium?
Carbon = amu
Helium = amu
Both samples contain the exact same number of atoms

15. The Mole
The number of atoms present in all of these samples assumes special importance in chemistry.
The mole (abbreviated mol) can be defined as:
The number equal to the number of carbon atoms in grams of carbon.
That is to say, one atomic mass unit is defined to be 1/12 of the mass of a carbon-12 atom.
That is to say, one atomic mass unit is defined to be 1/12 of the mass of a carbon-12 atom.

16. The Mole
Techniques for counting atoms very precisely have been used to determine this number to be 6.022x1023
One mole of something consists of 6.022x1023 units of that substance is called:
Avogadro’s Number
For example,
Just as a dozen is 12 eggs…
One mole of eggs is 6.022x1023 eggs

17. How do We Use the Mole in Chemical Equations?
12.01g sample of Carbon contains 6.022x1023 atoms
The atomic mass of hydrogen is amu
A g sample of hydrogen contains 6.022x1023 atoms
The atomic mass of aluminum is amu
A g sample of aluminum contains 6.022x1023 atoms

18. The point is:
A sample of any element that weighs a number of grams equal to the average atomic mass of that element contains 6.022x1023 atoms
Or one mol of that element

19. Comparison of 1-Mol Samples of Various Elements
# of Atoms Present
Mass of Sample (g)
Aluminum
6.022x1023
26.98
Gold
196.97
Iron
55.85
Sulfur
32.07
Boron
10.81
Xenon
131.3

20. Test Your Knowledge
Aluminum (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 of atoms and the number of atoms in a 10.0g sample of aluminum.
In this case we want to change from mass to moles of atoms.
10.0g of Al= ? Moles of Al atoms

21. Test Your Knowledge
The mass of one mol (6.022x1023 atoms) of aluminum is:
26.98g
The sample we are considering has a mass of:
10.0g
Its mass is less than 26.98g, so this sample contains:
Less than 1 mol of aluminum atoms.

22. Test Your Knowledge 1 mol Al= 26.98 g Al
10.0 g Al x 1 mol Al/ g Al=
0.371 mol Al

23. Test Your Knowledge
Next we convert from moles of atoms to the number of atoms.
6.022x1023 Al atoms=
1 mol Al atoms
0.371 mol Al x 6.022x1023 Al atoms/ 1 mol Al=
2.23x1023 Al atoms

24. Molar Mass A chemical compound is: For example,
A collection of atoms
For example,
Methane consists of molecules each containing one carbon atom and four hydrogen atoms (CH4)
How can we calculate the mass of 1 mol of methane?
What is the mass of 6.022x1023 CH4 molecules?

25. Molar Mass Each CH4 molecule contains:
1 carbon atom
4 hydrogen atoms
1 mol of CH4 molecules consists of:
1 mol of carbon atoms
4 mol of hydrogen atoms

26. How can we find the mass of 1 mol CH4?
Mass of 1 mol of C= 1 x 12.01g = 12.01g
Mass of 4 mol of H= 4 x 1.008g = 4.032g
Mass of 1 mol of CH4 =
16.04 g

27. Calculating Molar Mass
Calculate the molar mass of sulfur dioxide, a gas produced when sulfur containing fuels are burned.
The formula for Sulfur dioxide is:
SO2
1 mol SO2 molecules =
1 mol S atoms
2 mol O atoms

28. Calculating Molar Mass
Mass of 1 mol of S=
1 x =
32.07 g
Mass of 2 mol of O=
2 x =
32.00 g
Mass of 1 mol of SO2 =
64.07 g = molar mass