Download What is the charge of iron in Fe2O3

What is the charge of iron in Fe2O3?
Determine the charge on a multi-charge ion
Total ion charge
1.
2.
3.
4.
+6
+3
Fe2
-6
-2
O3
Determine the charge on the other atom
Multiply the charge by the subscript ie. 2 x 3 = 6
This is the total charge for the other ion.
Divide this number by the subscript and that is the
charge on each of that ion.
Charge of each
ion
H –hydrogen
N – nitrogen
O – oxygen
F – fluorine
Cl – chlorine
Br – bromine
I – iodine
At- astatine
All written as
diatomic
molecules in
elemental
state
Creation of oxidation numbers
1. If the atom has less than 3 electrons then
the atom will give them up.
2. If the atom has more than 5 electrons then
the atom will gain up to a total of 8
electrons
3. If the atom has 4 it can go either way.
4. The transition metals are exceptions to
these rules and they can follow them or not.
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 acidanion is probably a halogen.
HCO3-1 -bicarbonate
SO4 –2
–sulfate
-2
SO3
-sulfite
–2
CO3
- carbonate
-1
ClO4
-perchlorate
-1
ClO3
-chlorate
-1
ClO2
-chlorite
–1
ClO
–hypochlorate
–1
OH
– hydroxide
–1
NO3
– nitrate
-1
NO2
- nitrite
-1
CN
cyanide
PO4 –3
– phosphate
+1
NH4
- ammonium
-2
S2O3
-thiosulfate
–1
C2H3O2 – acetate
MnO4
-permanganate
-2
CrO4
-chromate
Cr2O7
-dichromate
Yes
Is it ionic
Does the cation have more than
1 oxidation number?
Yes
No
1) determine charge on cation
2) write full name followed by
a Roman numeral
3) write anion name if
polyatomic – if only 2
atoms, then name ends in
ide
1. Write full name of
cation.
2. Write full name of
anion if polyatomic
3. Use an ide ending if
only two atoms present.
Yes
Is it ionic
No
1. Convert subscript
after first element to a
Greek prefix & attach to
full name of first element
2. If only two elements
present apply #1 to the
second element and end
name in ide.
No
Does the cation have a Roman numeral?
Yes
No
1. use the Roman numeral
as the charge on the
cation
2. balance the formula
3. use an ide ending if
only two elements
present.
1. Write cation symbol first,
anion symbol second.
2. Use the most common
charge to balance the
formula
3. Subscripts should be
written in lowest whole
number ratio.
1. Use prefix as a
subscript for each
element.
2. If only2 elements
present end second in
ide.
3. First element name
will not have a prefix
if only 1 atom
present.
1.
2.
3.
4.
Write out rough formulas with reactants and products.
Balance formulas using the flow charts. Use subscripts to balance formulas
Write the elements on both sides (you may delete this step later).
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.
Total mass in
grams = 1 mole
Particles
6.02 x1023 particles = 1 mole
Moles of 1st
substance
Grams
Liters
Ratio of
coefficients
Particles
Moles of 2nd
substance
@ STP 22.4 L = 1 mole
Grams
Liters
Metals NonMetals
1.
2.
3.
4.
Electron Configuration
Electronic configuration is under the element name
The symbol in square brackets is the inner core of electrons
Usually only the electrons outside of the core are involved in bonding.
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.