A) Nomenclature (naming)
compounds
1. Covalent
2. Ionic
B) Writing proper formulas
Covalent or Ionic
 Ionic: ___________ + _____________
 Covalent: __________ + ___________
 NaCl
 P2Cl4
 FeCl3
 CaOI or C
I or C
I or C
I or C
SO2
AgCl
MnO
NS2
I or C
I or C
I or C
I or C
Naming molecular compounds
 Covalent Bonds Non-metal + non-metal
 Prefixes are used to determine the number of each
element (Except when the first element has only ONE
(1)
 Number Prefix
 1 _______6 ______ 2 _______7 ______ 3 _______8 ______ 4 _______9 ______ 5 _______10 ______ First element = # prefix + element name
 Second element = # prefix + element prefix + “ide”
COVALENT COMPOUNDS
A) H2O
B) CO2
C) CCl4
D) P2S4
____________________
____________________
____________________
____________________
2nd Element names
(non-metals)
 N = NITRogen
 NITRide
 P = PHOSPHorus
 PHOSPHide
 S = SULFur
 SULFide
 Cl = CHLORine
 CHLORide
 Br = BROMine
 BROMide
WRITING FORMULAS from names
Determine each element & number
Tetrasulfur pentaoxide
Octanitrogen difluoride
COVALENT COMPOUNDS
Naming BINARY (2 elements) IONIC (one
charge ONLY)
 Some Ionic compounds have more than 2 elements.
 NaSO4
 (NH3)2SO4
Ca3(PO4)2
MnSO4
 Some metals have more than one charge
 Fe (+2, +3)
Sn (+2, +4)
Identification of compounds: List as either
Covalent or Ionic. If Ionic, list as either
Binary or Ternary (more than 2 elements)
 1. CO2
 2. CaCl2
 3. S2O5
 4. Na2SO4
 5. CoCl3
 6. Fe2O3
 7. N2Cl4
 8. Mn3(PO4)4
I or C
I or C
I or C
I or C
I or C
I or C
I or C
I or C
if Ionic: Binary or Ternary
if Ionic: Binary or Ternary
if Ionic: Binary or Ternary
if Ionic: Binary or Ternary
if Ionic: Binary or Ternary
if Ionic: Binary or Ternary
if Ionic: Binary or Ternary
if Ionic: Binary or Ternary
Binary Ionic (one charge)
 Name the metal
 Name the non-metal prefix + “ide”
CaCl2 = Calcium chloride
Li2O = Lithium oxide
Writing formulas of Binary Ionic
 Determine the metal and its charges
 Determine the non-metal and its charges
 Criss-cross if necessary
 1. Lithium chloride
4. Potassium phosphide
 2. Calcium oxide
5. Boron fluoride
 3. Aluminum sulfide
6. Barium phosphide
Determine the name from the
formula
 1.
Na2O
5.
AlP
 2.
Al2S3
6.
Be3N2
 3.
Ba3P2
7.
CsBr
 4.
KI
8.
Mg3N2
FORMULA Ionic or Covalent Name
1.CO2
2.Na2S
3.Al2S3
4.S2O5
I
I
I
I
or
or
or
or
C
C
C
C
_________________
_________________
_________________
_________________
“Up to this Point”
 Covalent: _________________ + __________________
 Ionic:
_________________ + __________________
 Binary:
 Ternary:
 Metal with only one charge:
NEXT: Metals with more than
one charge
 LIST THE TWO POSSIBLE CHARGES AND THEIR
APPROPRIATE NAME WITH ROMAN NUMERAL

Symbol
Name
 Iron:
 Cobalt
 Copper:
Naming: Binary Ionic more than
one charge
 You must determine the charge of the metal.
 (“REVERSE” Crisscross)
 Co2S3
_________________________
 CoCl2
_________________________
 FeO
_________________________
 FeP
_________________________
Formula for Binary Ionic more than one
charge.
 a. chromium (III) chloride
_______________________

 b. tin (IV) oxide
_______________________

 c. lead (II) oxide
_______________________

 d. copper (II) iodide
_______________________

 e. cobalt (II) oxide
_______________________

 f. cobalt (III) oxide
_______________________
Naming Binary Ionic (more than
one charge)
 a. SnBr2
_______________________
 b. SnBr4
_______________________

 c. CrO
_______________________

 d. Cr2O3
_______________________

 e. Fe2O3
_______________________

 f. HgI2
_______________________
Write the formula
 a. chromium (III) sulfide
________________

 b. manganese (IV) oxide
________________

 c. gold (III) chloride
________________

 d. titanium (IV) chloride
________________

 e. iron (II) bromide
________________

 f. iron (II) oxide
________________
Write the proper name
 a. PbCl2
_________________________________

 b. Fe2O3 _________________________________

 c. SnI2
_________________________________

 d. Hg2O
_________________________________
 e. HgS
_________________________________

 f. CuI
_________________________________
TERNARY COMPOUNDS:
 Consist of a metal and a POLYATOMIC ion.
 Poly = many
atomic = atom ion = charge particle
 A group of atoms that act as one large atom. Contains a
specific charge.
List of Polyatomic Ions
Determining charges
Identifying the polyatomic
 When determining the formula: ends in “ate” or “ite”,
except HYDROXIDE and CYANIDE
 Or if it begins with AMMONIUM
 Circle the polyatomic ion:
 Calcium sulfate
Aluminum phosphate
 Tin (II) tartrate
Ammonium oxide
 Sometimes you can have two polyatomic ions
 Ammonium sulfate
Identifying the polyatomic ion
from a formula
 The polyatomic ion is always in a TERNARY compound.
 It’s always after the METAL, unless the compound begins
with NH4 (ammonium)
 Draw a line between the (+) side and the (-) side
 Circle the polyatomic ion
 Li2SiO3
Al2(SO4)3
 LiClO3
NH4Br
Naming the Polyatomic Ion
Naming Ternary
 Identify the ternary compound.
 Determine whether or not the METAL requires a
ROMAN NUMERAL (contains more than one
charge===GREEN)
 Name the Ternary compounds
 CaSO4 : ___________________________
 Mn3(PO4)4 : ______________________________
 NH4Cl :____________________________
Determining formulas for
Ternary compounds.
 Determine the charge of the CATION (+) ion
either the METAL or NH4
 Determine the charge of the POLYATOMIC ion.
 CRISSCROSS if necessary
 Calcium sulfate:________
Barium hydroxide:________
 Iron (III) carbonate:_______ Ammonium sulfide:________