Nomenclature Notes
I.
Rules for Writing Names and Formulas for Ionic Compounds
1. ___________________________ (Binary Salts) – Only made of two elements.
a.
b.
c.
d.
e.
f.
g.
These are compounds containing only _______________ and __________________.
Write the _____________ (metal ion) first and the____________________ (nonmetal ion) second.
Determine the ___________________ ratio of cations to anions that would make the total charge 0.
Use __________________ to makes charges add up to zero.
To determine the ion formed for main group elements look to its placement on the periodic table.
Noble gases to do not form ions except in rare cases.
Hydrogen can either gain or lose electrons depending on the other elements with which it combines.
Examples:
Sodium chloride.
Na+1
Cl1-
NaCl
charges equal 0
Aluminum oxide.
Al3+
O2-
Al2O3
charges equal 0
2. ________________________________ – Made of elements and polyatomic ions.
a.
_________________________ are two or more elements (usually nonmetals) bonded together that
have collectively lost or gained electrons and now have a charge. Compounds have a zero charge but a
polyatomic ion has a charge.
b. Write the ___________ (usually a metal, but there is one polyatomic ion.) first and the _________
second.
c. Determine the ___________________________ of cations to anions that would make the charge 0.
d. If a subscript must be added to a polyatomic ion, keep the polyatomic ion in ___________________.
e. Do not change the name of the polyatomic ion.
Examples:
Sodium phosphate.
Na1+
(PO4)3-
Ammonium sulfide
(NH4)1+
S2-
Na3PO4
charges equal 0
(NH4)2S
charges equal 0
3. Ternary Ionic Compounds with ______________________________________
a.
These are compounds containing only __________________________ and
______________________________.
b. Many elements in groups 3-12 have either a +2 or +3 charge.
c. Naming systems:
1) ________________– International Union of Practical and Applied Chemistry is the newest
system-this system uses Roman numerals to give the charges or oxidation number of positive ions
ONLY if the positive ion has variable charges. This is the system we will use.
2) _________________ – oldest system and still very commonly used. May be used ONLY if the
positive ion has a variable charge and exhibits only 2 oxidation numbers.
d. Writing Name:
1) The correct full name of the cation (transition metal ion) is written first and the anion is written
second.
2) Roman numerals are added after the metals name and are written in parentheses.
3) The Roman numeral is equal to the metals oxidation number.
4) The last syllable in the anion (nonmetal ion) is dropped and _____________ is added.
e.
II.
Examples:
FeCl2
Iron (II) chloride or Ferric chloride
FeCl3
Iron (III) chloride
CuS
Copper (II) Sulfide or Cupric Sulfide
Rules for Writing Names and Formulas for Binary Molecular (Covalent) Compounds
1. The compounds contain two (2) _______________________.
2. The less ____________________________ element is given first. It is given a prefix only if it
contributes more than one atom to a molecule of the compound. (All this means is that you will never
start with _____________________.)
3. The second element is named by combining a prefix indicating the number of atoms contributed by the
element to the __________________ of the name of the second element and then adding
____________________to the end.
4. The ____ or _____ at the end of a prefix is usually dropped when the word following the prefix
begins with another vowel. (monoxide or pentoxide)
5. Common Roots:
H: hydr
P: phosph
C: carb
S: sul
N: nitr
Cl: chlor
O: ox
Br: brom
3 – tri
8 – octa
4 – tetra
9 - nona
F: flor
I: iod
Si: silic
6. Prefix naming system :
1 - mono
6 - hexa
7. Examples:
III.
2 - di
7 - hepta
phosphorus pentachloride
PCl5
5 - penta
10 - deca
dihydrogen monoxide
H 2O
Rules for Writing Names and Formulas for Acids
1. General information
a.
b.
c.
d.
Any compound starting with hydrogen (Cation) is an acid.
Compounds that produce ________________________ when dissolved in water.
Determine the smallest whole number ratio of cations to anions that would make the charge 0.
Even though acids usually contain only nonmetals, they are treated as ionic compounds because the
hydrogen ion present is the H+1 ion.
2. Binary Acids:
a. Hydrogen and one other element.
b. No __________________ in acid.
c. If anion en ds in _______ then change it to _____________ and add ___________ in front of
name.
d. Examples:
HCl
Hydrochloric Acid
HBr
Hydrobromic Acid
3. Ternary (oxyacids) Acids:
a.
b.
c.
d.
______________________ is present.
The anion is usually a polyatomic ion.
If the anion ends in ___________ change it to ___________and add Acid to end.
If the anion ends in ___________ change it to __________ and add Acid to end.
e.
Examples:
HNO3
H2SO4
Nitric Acid
Sulfuric Acid
HNO2
H2SO3
Nitrous Acid
Sulfurous Acid
4. Common Roots for the Polyatomic Ions:
Acetate
Nitrate
Oxalate
Phosphate
Carboante
IV.
acetnitroxalphosphorcarbon-
Bromate
Nitrite
Sulfate
Perchlorate
bromnitrsulfurperchlor-
Chlorate
Chromate
Sulfite
Hyporchlorite
Rules for Writing Names and Formulas for Bases
1. Bases contain ____________________ (OH-1) ion.
2. Most bases are ionic compound paired with Group 1 or 2 metals.
3. Examples:
NaOH
Sodium hydroxide
Mg(OH)2
V.
chlorchromsulfurhypochlor-
Magnesium hydroxide
Rules for Writing Names and Formulas for Ternary Salts (Polyprotic)
1. Replaces the hydrogen in a ternary acid with another Cation.
2. Examples:
H2SO4 Sulfuric Acid
MgSO4 Magnesium sulfate
VI.
Rules for Writing Names and Formulas for Acidic Salts
1. Replace ________ of the Hydrogen atoms in the acid with another cation.
2. Examples:
H3PO4 Phosphoric Acid
NaH2PO4
Sodium dihydrogen phosphate
VII.
Rules for Writing Names and Formulas of Hydrates
1. They contain a _______________________________________________ attached to a
compound.
2. ______________________________prefixes are used in the formula to indicate the number of
water molecules.
3. The _____________________________ are used in the name for the number of water molecules.
4. It is placed in front of the word _________________________.
5. Examples:
NiCl2 ∙ 6 H2O
Nickel (II) chloride hexahydrate
MgSO4 ∙ 7 H20
Magnesium sulfate heptahydrate
CaSO4 ∙ 2 H20
Calcium sulfate dihydrate