+
Ionic Nomenclature
Chemistry 1
+
Exam Analysis
 Averages
 Chemical
Bonding
 Periodic Trends
 Electrons
(%)
(%)
(%)
+
The Language of Chemistry
 Subscripts
indicate the number of atoms of an
element in a molecule.
C8H18
 How
or
MgCl2
many atoms of each element are in the
following?
CH4
 SO2
 O2
 P4O10
 Pb(NO3)2

+ Review
 What
is a cation?
 What
is an anion?
 What
group of elements typically form +1 cations? Why?
 What
group of elements typically form +2 cations? Why?
 What
group of elements typically form -1 anions? Why?
 What
group of elements typically form -2 anions? Why?
+
Ions and Compounds

Monatomic ions (N3-)
 Ions formed from a single atom

Polyatomic ions (SO42-)
 Ions formed from more than one atom
 See hand-out (purple)
 Binary

Compounds
Made of two elements
 Ternary

Compounds
Made of three or more elements (contains polyatomic
ion)
 **When
writing chemical formulas for ionic
compounds, the overall charge of the compound must
be ZERO/NEUTRAL!**
+ Formula of Ionic Compounds
1)
List the cation (positively charged ion) chemical
symbol first.
2)
List the anion (negatively charged ion) chemical
symbol after the cation.
3)
If the charges are not the same (sum of the oxidation
numbers must equal zero), subscripts must be added
to indicate a ratio of positive and negative ions.
-The polyatomic ion acts as an individual ion.
-Because polyatomic ions act as a unit, NEVER CHANGE
SUBSCRIPTS OF ANY ATOM WITHIN THE ION.
-Transition metals with more than one oxidation number…
the charge is noted using roman numerals!
+
Let’s Practice Writing Formulas
Q: What is the chemical formula for aluminum
fluoride?
1.
Symbol for aluminum ion = Al3+
Symbol for fluoride ion = F-
2. Al3+F3. Least common multiple is
4. AlF3
5. Orbital Notation Verification
.
+
Practice Writing Formulas
Write the correct formula for the following ionic
compounds.
1)
Potassium and Iodide
2)
Magnesium and Chloride
3)
Aluminum and Bromide
4)
Cesium and Nitride
5)
Barium and Sulfide
+
Practice Writing Formulas With
Polyatomic Ions
1)
Sodium and Nitrate
2)
Calcium and Chlorate
3)
Aluminum and Carbonate
4)
Potassium and Chromate
5)
Magnesium and Carbonate
+
Naming Ionic Compounds
 List
the name of the cation (watch for transition
metals).
 List
the name of the anion, changing the ending to
“ide”
 If
you have a polyatomic anion, just list its name after
the cation.
 CaCl2
 Na2S
= calcium chloride
= sodium sulfide
+
Naming Ionic Compounds With A
Transition Metal
 Work
backwards to determine the charge on the
transition metal….
Cr2O3
FeO
NiCl2
Mn3(PO4)2
Rules To Name Compound:
1. Name the cation
2. Place the charge of the transition metal as a roman
numeral
3. Name the anion by changing the ending to “ide”
+ Review – Binary Compounds
Write the correct chemical formula for each of the following
compounds.






potassium bromide
magnesium selenide
sodium phosphide
tin(IV) chloride
aluminum oxide
scandium(III) sulfide
Give the correct names for each of the following compounds listed
below.






KF
SnI4
SiF4
AlBr3
FeCl3
ZnO
+ Review Ternary Compounds

Write the chemical formulas for the following names:
 Iron (III) acetate
 Gold(III) sulfate
 Ammonium phosphate
 Calcium nitrate

Write the chemical names for the following chemical formulas:
 FeC2O4
 Pb(CO3)2
 Al(MnO4)3
 Ba(OH)2
+
For next time…
 Complete
Unit Packet Part 2 (Part 1 should
be completed at this time).

Read pages 232-244 (Ch. 7 sections 2 and 3)
+ Entrance Ticket


Write the formula for the following compounds. Hint-look
up the charges for each element/ion and then balance
the charges

Calcium Nitride

Rubidium Sulfide

Lead (II) Nitrate

Iron (III) Oxide

Manganese (III) Chlorate
Write the name for the following compounds.

Cr3P2

Al2 (SO4) 3

BaO

CoN

Cu3 (PO4 ) 2
+ Molecular Compounds
Nomenclature (Covalent)

When naming compounds consisting of two nonmetals, the names
of the elements are written in the same order as they appear in
the formula. (The more metallic element is written first.)

The second element uses the suffix “-ide”. Prefixes are added to
the name of each element to indicate the NUMBER of atoms of the
element in the molecule.
 (If the first element’s prefix is mono-, it will be dropped. For
example, monocarbon dioxide (CO2) is simply called carbon
dioxide.)

**Note: the “o” or “a” at the end of a prefix is usually dropped
when the word following the prefix begins with another
vowel…e.g. monoxide or pentoxide.
+
Prefixes –Polyatomic Handout
Prefix
Number of atoms
Mono-
1
Di-
2
Tri-
3
Tetra-
4
Penta-
5
Hexa-
6
Hepta-
7
Octa-
8
Nona-
9
Deca-
10
+ For the following molecular compounds,
write the molecular formula:
 Carbon
 Sulfur
mononitride
tribromide
 Phosphorus
 Nitrogen
 Carbon
dioxide
tetrachloride
 Dihydrogen
 Sulfur
triflouride
monoxide
trioxide
 Dinitrogen
hexoxide
+ For the following molecular formulas, write the
compound name:
 SiO2
 CO2
 SeF6
 N2O5
 As2O5
 AsI3
 PCl5
 CF4
+
Flow Chart Challenge
 Create
a flow chart to use while NAMING Ionic and
Covalent Compounds
 Hints:
 How
do you distinguish between an Ionic and
Covalent Compound?
 Which one uses prefixes?
 When do you use Roman Numerals in the name?
 What do you do for naming polyatomic ions?
+
Individual Practice
 Unit
Packet Part 3 (Omit Acid Naming)