What is the charge of iron in Fe2O3?
H –hydrogen
N – nitrogen
O – oxygen
F – fluorine
Cl – chlorine
Br – bromine
I – iodine
At- astatine
1- mono
2- di
3- tri
4- tetra
5- penta
6- hexa
7- hepta
8- oct
9- nano
10 - deca
If the polyatomic ion ends in ate,
replace with -ic + acid
If the polyatomic ion ends in ite,
replace with –ous + acid
If the acid is binary – start with hydro,
then use the anion & end with – ic
if name ends in ic,
then look for a polyatomic ion ending in ate
if the name has the prefix hydro- it is a binary acid-
anion is probably a halogen.
HCO3-1 -bicarbonate PO4 –3 – phosphate
SO4 –2 –sulfate NH4 +1 - ammonium
SO3-2 -sulfite S2O3-2 -thiosulfate
CO3 –2 - carbonate C2H3O2 –1 – acetate
ClO4-1 -perchlorate MnO4 -permanganate
ClO3-1 -chlorate CrO4-2 -chromate
ClO2-1 -chlorite Cr2O7 -dichromate
ClO –1 –hypochlorate
OH –1 – hydroxide
NO3 –1 – nitrate
NO2-1 - nitrite
CN-1 cyanide
Yes Is it ionic No
Does the cation have more than
1 oxidation number?
Yes No
Yes Is it ionic No
Does the cation have a Roman numeral?
Yes No
1. Write out rough formulas with reactants and products.
2. Balance formulas using the flow charts. Use subscripts to balance formulas
3. Write the elements on both sides (you may delete this step later).
4. Starting with the left side use coefficients to obtain equal number of the same element on both sides of the equation. Use coefficients to balance equations.
5. Leave H & O until the end.
6. If you get an odd-even coefficient result, go back an double all coefficients assigned to that point.
Metals NonMetals
Electron Configuration
1. Electronic configuration is under the element name
2. The symbol in square brackets is the inner core of electrons
3. Usually only the electrons outside of the core are involved in bonding.
4. You remove highest level electrons first, then the next level electrons
Na = [Ar] 3s1 Na+ = [Ar] notice the 3s1 electron is gone.
If you remove all of the electrons from either a level or type you do not write that location in the final configuration.