1. Moles and Formula Mass

2. Atomic Mass
Knowing the mass of atoms is extremely helpful in chemistry
But…a single spec of dust contains around 1 x 1016 atoms!
How can we possibly figure out the mass of one single atom??

3. Atomic Mass
We determine the mass of one atom RELATIVE to another experimentally
Step 1: establish a mass of one atom to be used as the standard
Atomic mass-the mass of the atom in atomic mass units (amu)
Aka atomic weight
Indicates how heavy one atom of one element is compared to one atom of another element

4. Atomic Mass Unit (amu) 12 amu = mass of one C-12 atom
Therefore, 1amu = 1/12 the mass of a C-12 atom
The atomic mass of other elements has been determined experimentally by determining the ratio or percent mass in comparison to C-12
Ex: a hydrogen atom is found to be percent as massive as a C-12 atom; therefore 12 x 8.400% = 1.008amu

5. Atomic Mass Unit We do not know the actual mass of an atom!
Example: even though we do not know the actual mass of an iron atom, we do know that an iron atom if approximately 56 times as massive as a hydrogen atom

6. Average Atomic Mass
Naturally occurring elements occur in more than one isotope
Remember: what’s an isotope? What’s the same and what’s different?
Official atomic masses are averages of all the isotopes naturally occurring for a given element

7. Calculating average atomic mass
(atomic mass Y1) x percent abundance Y1 + (atomic mass Y2) x percent abundance Y2 …
**percent abundance MUST be in fraction form!
Carbon = (0.9890)( amu) + (0.0110)( amu) = amu

8. Sample average atomic mass
Copper, a metal known since ancient times, is used in electrical cables and pennies, among other things. The atomic masses of its two stable isotopes, Cu-63 (69.09%) and Cu-65 (30.91), are 62.93amu and amu respectively. Calculate the average atomic mass of copper. The relative abundances are given in parentheses.

9. Solution (0.6909)(62.93amu) + (0.3091)(64.9278amu) = 63.55amu
Follow up questions: Explain the fact that the atomic masses of some of the elements like fluorine listed in the periodic table are not an average value like that for carbon.

10. Solution (continued)
Atomic mass is based on isotopes that occur naturally and therefor must be stable (nonradioactive).
Some elements only have one stable isotope
Ex: fluorine only has one stable isotope (F-19)
The second longest living isotope (F-18) only has a half-life of minutes. All other isotopes have half-lives under a minute, the majority under a second,

11. Mass Specroscopy
The relative abundances of isotopes is determined through a mass spectrometer

12. Mass Spec
1. gaseous sample is bombarded by a stream of high-energy electrons
2. This strips away the electrons leaving the positively charged nuclei
3. Nuclei are accelerated as they travel through two oppositely charged plates
4. A magnetic field is applied to the positively charged beam, which caused the particles to curve
5. The angle at which a particle curves is based on the mass (more massive ions deflect/curve less)
6. The amount of a particular ion/isotope is determined by the amount of voltage registered by the detector

13. Neon

14. Boron

15. I didn’t discover it. Its just named after me!
Avogadro’s Number
6.022 x 1023 is called “Avogadro’s Number” in honor of the Italian chemist Amadeo Avogadro ( ).
I didn’t discover it. Its just named after me!
Amadeo Avogadro

16. The Mole 1 dozen = 12 1 gross = 144 1 ream = 500 1 mole = 6.022 x 1023
The mole is just a number. It is a collection of items.
1 mole of students is x 1023 students!

17. Atomic masses and the mole
The atomic masses of two elements gives their mass ratio
Ex: an oxygen atom (16.00 amu) is about 4 times heavier than a helium atom (4.003 amu)
If this relationship is true from one atom of each, this is true for the same multiple of each
Ex: 10 atoms of oxygen with still weigh about 4 times more than 10 atoms of helium

18. Continued… Therefore…
If the masses (in grams) of two samples have this proportion, they must contain the same number of atoms!
Based on this logic, any mass (in grams) of an element that is equal to its atomic mass (in amu) with have the same number of atoms as another element with its atomic mass in grams
This number of atoms is Avogadro’s Number!
Conversion factor atomic mass in grams = x 1023

19. Molar Mass
1 mole = x 1023
Molar mass-the mass of one mole of a substance (substance must be well defined!)
Units: g/mol
The molar mass of a compound: the sum of its parts
Ex: CH4 C(12.011g/mol) + H(1.008g/mol) + H(1.008g/mol) + H(1.008g/mol) = /mol
Conversion factor: mass in grams (equivalent to the amu of one atom of that element) = 1 mole

20. Calculations with Moles: Converting moles to grams
How many grams of lithium are in 3.50 moles of lithium?
3.50 mol Li
6.94 g Li
= g Li
45.1
1 mol Li

21. Calculations with Moles: Converting grams to moles
How many moles of lithium are in 18.2 grams of lithium?
18.2 g Li
1 mol Li
= mol Li
2.62
6.94 g Li

22. Calculations with Moles: Using Avogadro’s Number
How many atoms of lithium are in 3.50 moles of lithium?
3.50 mol
6.02 x 1023 atoms
= atoms
2.07 x 1024
1 mol

23. Calculations with Moles: Using Avogadro’s Number
How many atoms of lithium are in 18.2 g of
lithium?
18.2 g Li
1 mol Li
6.022 x 1023 atoms Li
6.94 g Li
1 mol Li
(18.2)(6.022 x 1023)/6.94
= atoms Li
1.58 x 1024