1. Working with units DO NOT GET CARELESS…EVER!
Always keep track of your units
I will take points off of anything you give me if you leave the units off
I will stare at you when you give me an answer without units until you put them in your answer
IT REALLY IS THAT IMPORTANT!!!!

2. Dimensional Analysis
You will frequently have to convert between units during your life (Yes, your entire life!)
To do this, we will need to employ DIMENSIONAL ANALYSIS
Step 1: What do you have? What do you need?
Step 2: What is the conversion factor?
Step 3: Setup a calculation that cancels your given units and puts your target units on top.

3. Dimensional Analysis: Example
A sample of an alloy has a density of 7.9 kg/cm3. What is the density in mg/m3? 

4. Dalton’s Atomic Hypothesis
All atoms of a particular element are identical
Atoms of different elements have different masses
A compound is a specific combination of atoms of more than one element
In a chemical reaction, atoms are neither created nor destroyed; they exchange partners to produce new substances
These tenets were first proposed 202 years ago and they are all true!

5. The Periodic Table

6. C: Compounds Compounds. Huh?
A compound is an electrically neutral substance that consists of two or more different elements with their atoms present in a definite ratio
Compounds: Terminology
Binary: Consists of only 2 elements
Organic: Contains Carbon and hydrogen
Inorganic: No Carbon

7. Ionic and Molecular Compounds
Ionic Compound: Ions form compound that is electrically neutral
Usually formed by the reaction of a metal and a nonmetal
Na(s) + Cl(g)  NaCl(s)
Molecular Compound: Binary molecular compounds are usually formed by the reaction of 2 nonmetals
2H2(g) + O2(g)  2H2O (l)

8. E: Moles and Molar Masses
The Mole: The most important concept you’ve never heard about
A mole of objects contains the same
number of objects as there are carbon atoms in 12.0 g of Carbon-12
6.022x1023 somethings/mole = Avogadro’s Number

9. 1 mole of any element always has 6.0221x1023 atoms in it
1 mole of elephants always has x1023 elephants in it.
In equations, you will frequently see the number of moles represented by the variable “n”
1 kmol = 1000 mol
1 mol = 1x10-6 mol
# of objects = n(NA) where NA is Avogadros’ number

10. Molar Mass The molar mass is the mass of one mole of material
Also referred to as molecular weight or formula weight for compounds
The molar mass of an element is the mass of one mole of its atoms
The molar mass of a compound is the mass of a mole of its molecules.
Molar mass (M) is usually given in g/mole
Mass of Sample = nM 

11. Determination of Chemical Formulas
For hundreds of years, people knew that drinking willow bark tea would belp cure a headache
When scientists identified a compound form Willow bark that was biologically active, they had to determine its structure before they could synthesize it.
Determining the chemical formula is the first step in the structure determination process…

12. Chemical Formulas We will deal with 2 types of chemical formulas:
Empirical formula: Shows the relative numbers of each element present in the compound (Emp. Form. Of Hydrogen Peroxide?)
Molecular formula: The precise number of atoms of each element present in the compound (Mol. Form. Of Hydrogen Peroxide?)

13. Mass Percentage Composition
The mass percentage composition of a compound tells us the percentage (by mass) that a given element comprises of the compound.
We frequently determine the mass % composition using combustion analysis 

14. Mass % Composition Summary:
Mass % composition is found by calculating the fraction of the total mass contributed by each element present in a compound and expressing the fraction as a percentage.

15. Determining Empirical Formula from Mass % Data
To convert the mass % composition obtained from a combustion analysis into an empirical formula, we must convert the mass % of each type of atom into the relative number of atoms.
To do this, assume that we have 100g of sample
The mass % will then be in grams 

16. Determining Molecular Formulas
Once we know the empirical formula, we need one more piece of information to determine the molecular formula: The Molar Mass
Say we know the empirical formula of a compound is C3H4O3.
All we know about this compound at this point is the ratio of the 3 elements.
We don’t know the exact number of each type of atom in the molecule.
Is the Molecular Formula C6H8O6, C12H16O12 or C18H24O18? 

17. G: Molarity
Hands down one of the most important concepts you need to master is you are going to stay in the sciences. Period.
The Molar Concentration, c, of a solute in solution is the number of moles of solute divided by the volume of the solution (in liters).
Also referred to as Molarity

18. Molarity The symbol M is used to denote the molarity of the solution
1M NaCl = 1 mole NaCl per liter of H2O 

19. G4: Dilutions
Frequently in the laboratory, you will need to make dilutions from a stock solution.
This involves taking a volume from the stock and bringing it to a new volume with solvent.
In order to perform these dilutions, we can use the following equation:
c1V1 = c2V2
Where: c1 = Stock concentration
V1 = Volume removed from stock
c2 = Target conc of new sol’n
V2 = Volume of new solution 