1. Holy Moley: Moles as Measurements of matter
Chapter 10
Holy Moley: Moles as Measurements of matter

2. A review of moles
a _________ is a specific number of particles (like a dozen is 12 particles) – it is __________________number of particles – ____________________particles
the ________________________of a substance can be found using its formula, and is the ________________________________________________________________________________

3. determining chemical formulas
Our lab information about a substance is usually a ratio of masses (in grams)
for example, we might know that a sample of copper chloride is composed of 4.7 grams of copper and 5.3 grams of chlorine (4.7 g:5.3 g)
Chemical formula info is a _________________
for example, the ratio of moles in a sample of water is _____________________
Therefore, to determine the chemical formula when we have a ratio of masses, we must _______________________________________

4. To determine the chemical formula
Start with the relative mass of each element in a compound
Divide each mass by the ________________of that element (to determine relative number of moles)
Divide all answers by the ________________ answer to get a ratio of whole numbers
These numbers are the __________________ in the chemical formula

5. Example #1
What is the empirical formula for a compound which contains g of iron, g of sulfur and g of oxygen?

6. Example #2
Find the formula for a compound which contains 32.8% chromium and 67.2% chlorine.

7. Practice
A gram sample is decomposed in the lab and found to contain grams of aluminum. The remainder of the compound is oxygen. Determine the formula.

8. Practice
A 5.0-gram sample of a white powder is decomposed and found to contain 1.11 grams of aluminum and 1.27 grams of phosphorus. The remainder of the compound is oxygen. What is the formula for this compound?

9. To determine the chemical formula
Either relative masses OR percent compositions can be used
If the mole ratios end up as decimals of 0.5 or 0.33, multiply all numbers by 2 or 3 to achieve all whole-numbers
The chemical formula determined is the most _______________________________________

10. formula mass VS Molar Mass)
The formula mass (or molecular mass) is the sum of the mass of each atom in the compound, in amu
The molar mass of a compound is numerically equal to the formula mass, but with units of grams/mole
The formula mass of any compound is the sum of the average atomic masses of all the atoms represented in the formula
__________________ the number of atoms of each element in the compound
____________________ the number of atoms by the atomic mass of that element
______________________to obtain the formula mass for the whole compound

11. examples
H2SO4
Fe2(SO4)3
MgSO4•3H2O

12. Empirical vs. molecular formula
The ___________________________of a compound is the chemical formula in its most simplified form. It tells you the simplified ratio of the elements in a compound. CH2O
The ______________________of a compound may or may not be the same as the empirical formula. It is the formula that tells the actual number of atoms of each element in the compound.
C3H6O3 or C6H12O6

13. examples
Determine the empirical formula for each of the following molecular formulas:
B4H C6H12O N2O FeSO3
Write four possible molecular formulas that would all have the empirical formula C2H5.

14. Relationship Between Empirical and Molecular Formula Masses
If an empirical formula and the molecular mass are known, the molecular formula can be found.
Consider the empirical formula CH2O
If the molecular mass is 90 amu, what must the molecular formula be?
To determine the molecular formula- compare the formula mass of the empirical formula with the molecular mass given to see how many times greater the molecular mass is.
Formula mass of CH2O = 30 amu,
30 x _____ = 90  Molecular formula is 3 times bigger!
Molecular Formula is C3H6O3

15. Examples
Acetylene is a colorless gas used as a fuel in welding torches, among other things. It is 92.96% carbon and 7.74% hydrogen. Its molecular mass is amu. What are the empirical and molecular formulas of acetylene?

16. Calculating percent composition
_____________________________of a compound is the percent by mass of each element in the compound
Percent composition can be used to determine the _______________________________of an unknown compound
Percent composition can also be used to determine the amounts of elements in a given sample

17. Calculating percent composition
Calculate the formula mass of the compound using the previously given steps
Determine the mass of the element in the compound by ____________ the ____________ by the number of __________ of that element
Use the following formula:

18. example
What is the percent by mass of nitrogen in magnesium nitrate, Mg(NO3)2?

19. practice
For each compound below, calculate the formula mass. Then calculate the percent composition of oxygen in the compound.
H2O
H2O2
KClO3
Ti3(PO4)4