Transcript Chemical Nomenclature - Belle Vernon Area School District

Ionic Naming
Objective/Warm-up
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1)
2)
3)
4)
SWBAT name ionic compounds.
Criss-Cross the following:
Ca+2 and SO4-2
Na+1 and PO4-3
Al+3 and O-2
Mg+2 and N-3
Definitions
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An IONIC COMPOUND consists of a metal
cation bonded to a nonmetal anion.
Electrostatic attraction holds them together.
Metal Cation
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Na+
Nonmetal anion
Cl-
A quick review
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Do you remember how to find the
charges on different elements from
the periodic table?
Type I Binary Ionic Compounds
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The metal cations in these compounds have
only ONE possible charge.
Na+
sodium
Zn2+
zinc
Al3+
aluminum
Ca2+
calcium
The charges are memorized or predicted using a periodic table!
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The cations are bonded to nonmetal anions:
O2oxide
N3nitride
Ffluoride
Br bromide
Notice that simple anions are always named with the
suffix “ide”
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In an ionic compound, the charges of the
cations and anions must always cancel out.
Subscripts are used if more than one atom is
needed to cancel the charges:
sodium chloride:
Na+ and Cl- 
lithium oxide:
Li+ and O2- 
aluminum bromide:
Al3+ and Br -  AlBr3
zinc nitride:
Zn2+ and N3-  Zn3N2
potassium iodide:
K+ and I- 
silver phosphide:
Ag+ and P3-  Ag3P
NaCl
Li2O
KI
Lets do some practice
Examples: Type I Binary Ionic Compounds
Write the formulas:
•potassium oxide
• zinc chloride
• silver sulfide
• aluminum nitride
• gallium oxide
•calcium iodide
K 2O
ZnCl2
Ag 2 S
AlN
Ga2 O3
CaI 2
Write the names:
• K3N
•Potassium Nitride
• AgI
•Silver Iodide
• ZnBr2
•Zinc Bromide
• Al2O3
•Aluminum Oxide
• Ba3P2
•Barium Phosphide
• LiH
•Lithium Hydride
Type II Binary Ionic Compounds
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These are ionic compounds where the metal cation
can form TWO different charges.
Fe2+
iron (II)
Fe3+
iron (III)
Ni2+
nickel (II)
Ni3+
nickel (III)
Co2+
cobalt (II)
Co3+
cobalt (III)
Cu+
copper (I)
Cu2+
copper (II)
Au+
gold (I)
Au3+
gold (III)
Sn2+
tin (II)
Sn4+
tin (IV)
An older system uses suffixes and Latin names, -ous for
the lower charge, -ic for the higher charge:
Ferrous & Ferric, Cuprous & Cupric, Stannous & Stannic
Examples: Type II Binary Ionic Compounds
Write the formulas:
FeO
• iron (II) oxide
• copper (II) chloride
• tin (IV) sulfide
• cupric nitride

• nickel (III)
 oxide

CuCl2
SnS 2
Cu3 N 2
Ni2O3
Examples: Type II Binary Ionic Compounds
Write the names:
• Fe2O3 •iron (III) oxide
• SnS
•Tin (II) Sulfide
• NiBr2 •Nickel (II) Bromide
•CuS
•Copper (II) Sulfide
• Pb3P2 •Lead (II) Phosphide
• CuBr
•Copper(I) Bromide
• FeCl3
•iron (III) Chloride
Polyatomic (Complex) Ions
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All of the cations and anions so far have been simple
ions - single atoms that have lost or gained electrons.
A complex ion is a charged molecule. Complex ions
may be cations or anions.
examples:
nitrate: NO3-
sulfate: SO42-
hydroxide: OH-
Things to Notice
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Most complex ions are anions. Ammonium, NH4+, is
the most common complex cation.
Several complex ions form a short series of ions.
The ions differ only in the number of oxygen atoms:
perchlorate
ClO4-
sulfate
SO42-
chlorate
ClO3-
sulfite
SO32-
chlorite
ClO2-
hypochlorite
ClO-
nitrate
NO3-
nitrite
NO2-
Lets do some practice
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Use the handout to write the
names for the following.
Writing formulas with Complex Ions
A. NH4Cl
a) Ammonium chloride
B. Ag2SO4
b) Silver sulfate
C. Al(OH)3
c) Aluminum hydroxide
D. Ca3(PO4)2
d) Calcium phosphate
E. Fe(NO2)3
e) Iron (III) nitrite
F.
f) Copper(II) permanganate
Cu(MnO4)2
G. (NH4)2Cr2O7
H. Zn(CH3COO)2
g) Ammonium dichromate
h) Zinc acetate
Objective/ Warm-up
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SWBAT write formulas and name ionic
compounds.
Please give the name for the following
formulas:
(a) Ag3P
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(b) Fe2O3
(c) Ag2SO4
Please give formulas for the following
names:
(a) Tin (II) Sulfide (b) Iron (III) nitrite
Closure
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When do we need to use roman
numerals in a name?