Naming Binary Compounds
****CRISS-CROSS METHOD!!!!!***
 Take the oxidation state of each element and/or
polyatomic ion and criss-cross them to get your formula!!
(Do not include charge in formula)
 Always reduce ionic compounds so that atoms are in
their smallest whole # ratio!
Mg+2 and Cl-1
MgCl2 (magnesium chloride)
Table E—Selected Polyatomic Ions
Variations for Type 1 Compounds
Metal & Non-metal
(NaF= sodium fluoride)
Metal & - polyatomic ion
(NaOH = sodium hydroxide)
+Polyatomic ion & Non-metal
(NH4F = ammonium fluoride)
2 polyatomic ions
(NH4OH = ammonium hydroxide)
If metal has more than one +
oxidation number use roman
numerals to show which one
FeCl3 = Iron (III) chloride
FeCl2 = Iron (II) chloride
Naming Binary Compounds
Type 3
Rules for Naming Binary Covalent/Molecular
Compounds (non-metal & non-metal)
1.
2.
3.
The first element in the formula is named first, using the full
element name.
Drop the ending of the 2nd element in the compound and
add the ending –ide.
Prefixes (shown below) denote the # of atoms present
Also consider that:
A) The prefix mono is never used with the
first element, only from -di on.
B) The second non-metal always gets
a prefix
Names and Formulas of Ionic Compounds
(Type 1 & 2)
Putting It All Together: PRACTICE!!
Name the following compounds given the formula:
1)
Na2SO4
9) Al(NO3)3
10) Cu(ClO4)2
3)
Fe(NO3)3
11) NH4Br
4)
Mn(OH)2
12) Cr2O3
5)
Na2SO3
13) Co(NO3)2
6)
Na2CO3
14) K2SO4
7)
CaCl2
15) Ba(OH)2
8)
FeCl3
Names and Formulas of Ionic Compounds
Putting It All Together: PRACTICE!!
Write the formula for each compound, given the name:
1)
Sodium hydrogen carbonate
7) Nickel (II) perchlorate
2)
Cesium perchlorate
8) Iron (II) phosphate
3)
Sodium hypochlorite
9) Titanium (IV) oxide
4)
Sodium selenate
10) Magnesium sulfate
5)
Potassium bromate
11) Silver sulfide
6)
Potassium sulfide
12) Lead (II) nitrate
Names and Formulas of Binary
Covalent/Molecular Compounds
Name the following compounds:
1)
Cl2O
5) SO2
2)
N 2 O4
6) PCl5
3)
NF3
7) N2O3
4)
P4S10
Classifying Chemical Reactions
 Synthesis: H2O + CO2  H2CO3
 Decomposition: NaCl  Na + Cl
 Single Replacement:
Fe + CuSO4  FeSO4 + Cu
 Double Replacement:
NaCl + AgNO3  NaNO3 + AgCl
Balancing Chemical Reactions
LAW OF CONSERVATION OF MASS, ENERGY, & CHARGE:
 In all chemical reactions there is conservation of mass,
energy and charge.
 The amount of matter stays the same (one side equals the
other).
 The total amount of energy stays the same (one side equals
the other).
 The number of positive (or negative) charges stays the same
(one side equals the other).
 In a chemical reaction, all of the elements or compounds
found to the left of the equation are known as the
reactant(s), and resulting elements or compounds are known
as the product(s).
2H2 + O2  2H2O
(reactants) (product)
IUPAC
International Union of Pure and
Applied Chemistry
 When a question states “Write the IUPAC
name” they are talking about the organization
above. All chemical and “common” names
must be approved by them. Basically it means
“JUST NAME IT!!” 