Types of Compounds
Chapter 5
Objectives 5.1
• 5.1 Apply ionic charge to writing formulas
• 5.1 Apply formulas to name ionic
compounds
• 5.1 Interpret the information in a chemical
formula
Ionic “Bonds”
• Instead of Formula’s: Ratio’s
• Some atom’s want more electrons than
the other wants to give up
• So they bind to two, or three
• Example: Li and O, Li wants to give up
only 1 electron, but O wants 2 electrons
Practice Question
• What ratio of Mg and N are needed to
make an Ionic compound that has a
neutral charge?
– Draw a Lewis electron dot diagram for N
– Draw a Lewis electron dot diagram for Mg
• What ratio of Na and Br are needed to
make an Ionic compound that has a
neutral charge?
+1+2
General Ionic Charges
-3 -2 -1
Ionic Nomenclature
• Only use Ionic Nomenclature when
dealing with Ionic compounds
– An ionic compound is formed when a metal
and a non metal come together and electrons
are completely lost and gained
Fixed Oxidation State
• Some Metals will always lose the same
amount of electrons. These metals have
Fixed Oxidation States
• Alkali Metals = +1
• Alkaline Earth Metals = +2
• Aluminum = +3
Ionic Nomenclature
• Binary Compounds of Metals with Fixed
Charges: Given Formula, Write the Name
• The order for names in a binary compound is
first the cation, then the anion.
• Use the name of cation with a fixed oxidation
state directly from the periodic table.
• The name of the anion will be made from the
root of the element's name plus the suffix "-ide."
Practice Naming
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What is the name of the following?
MgO
Magnesium Oxide
NaF
Sodium Flouride
CaS
Calcium Sulfide
Ionic Nomenclature
• Given Name, Write Formula
• The order in a formula is first the cation, then the
anion.
• You must know the charges associated with
each cation and anion.
• The sum of the positive charge and the sum of
the negative charges MUST add up to zero.
• You MAY NOT adjust the charges of the cations
or anions to get a total charge of zero.
• You MAY adjust the subscripts to get a total
charge of zero.
COMPOUNDS
FORMED
FROM IONS
CATION +
ANION --->
COMPOUND
Na+ + Cl- -->
NaCl
A neutral compound
requires
equal number of +
and - charges.
Formulas of Ionic Compounds
Formulas of ionic compounds are determined
from the charges on the ions
atoms
ions

Na  +

F : 

sodium + fluorine
Charge balance:

Na+
–
: F :  NaF

sodium fluoride
1+
1-
formula
= 0
Hint
• Cross the charges to find the amount you
need.
• If it can be reduced, then do so
– Ie if both are 2, then it is 1
Ionic Nomenclature
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What is the formula of the following?
Potassium Oxide
K2O
Strontium Chloride
SrCl2
Magnesium Nitride
Mg3N2
Ionic Nomenclature
• Potassium Phosphide
• K3P
•
•
•
•
Magnesium Sulfide
MgS
Radium Flouride
RaF2
Variable Charges
• The transition metals have variable
charges, they are happy with losing a
variety of electrons
– This is because they can also lose some of
there D electrons and be stable
Transition Metals
Elements that can have more than one possible
charge MUST have a Roman Numeral to
indicate the charge on the individual ion.
1+ or 2+
Cu+, Cu2+
copper(I) ion
copper (II) ion
2+ or 3+
Fe2+, Fe3+
iron(II) ion
iron(III) ion
Variable Charges
• Formula to Name
• 1) Find the charge of the cation by
– Finding total charge of anion and dividing by
number of cations
• Example: FeCl3
– We have 3 Chlorines, each has a -1 charge
– The Fe needs to be +3 to balance it out
• 2) Say the cation with its Roman Numeral
– Iron (III) Chloride
Variable Charges
• What is the name?
• AuF3
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Gold (III) Flouride
AgF
Silver (I) Flouride
PbO2
Lead (IV) Oxide
Variable Charges
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SnF2
Tin (II) Flouride
MnO2
Manganese (IV) Oxide
CrN
Chromium (III) Nitride
Sn3N4
Tin (IV) Nitride
Variable Charges
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Name to Formula
The Roman Numeral tells you the charge
Balance the formula
Iron (III) Oxide
– Fe has a +3 charge as denoted by the III
– Oxygen always has a -2 charge
– Cross them (Balance)
– Fe2O3
Variable Charge
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What’s the formula?
Lead (IV) Sulfide
PbS2
Copper (I) Chloride
CuCl
Silver (I) Nitride
Ag3N
Variable Charge
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Gold (III) Arsenide
AuAs
Tin (II) Bromide
SnBr2
Cobalt (III) Oxide
Co2O3
Writing a Formula
Write the formula for the ionic compound that
will form between Ba2+ and Cl.
Solution:
1. Balance charge with + and – ions
2. Write the positive ion of metal first, and the
negative ion
Ba2+
Cl
Cl
3. Write the number of ions needed as
subscripts
BaCl2
Learning Check
Write the correct formula for the
compounds containing the following ions:
1. Na+, S2a) NaS
b) Na2S
c) NaS2
2. Al3+, Cla) AlCl3
b) AlCl
c) Al3Cl
3. Mg2+, N3a) MgN
b) Mg2N3
c) Mg3N2
Solution
1. Na+, S2b) Na2S
2. Al3+, Cla) AlCl3
3. Mg2+, N3c) Mg3N2
Naming Compounds
Binary Ionic Compounds:
• 1. Cation first, then anion
• 2. Monatomic cation = name of the
element
• Ca2+ = calcium ion
• 3. Monatomic anion = root + -ide
• Cl = chloride
• CaCl2 = calcium chloride
Naming Binary Ionic Compounds

Examples:
NaCl
sodium chloride
ZnI2
zinc iodide
Al2O3
aluminum oxide
Learning Check
Complete the names of the following binary
compounds:
Na3N
sodium
________________
KBr
potassium ________________
Al2O3
aluminum ________________
MgS
_________________________
Mixed Review
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Given the name, write the formula
Given the formula, write the name
1) Sodium Oxide
2) Lead (II) Nitride
3) Cesium Iodide
4) RbF
5) AuO
Mixed Review
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6) SrCl2
7) CoS
8) Ag2Se
9) Manganese (IV) Chloride
10) Radium Nitride
Answers to Review
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1)
2)
3)
4)
5)
Na2O
Pb3N2
CsI
Rubidium Flouride
Gold (II) Oxide
Answers to Review
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6) Strontium Chloride
7) Cobalt (II) Sulfide
8) Silver (I) Selenide
9) MnCl4
10) Ra3N2
Objectives 5.2
• 5.2 Apply organic nomenclature to name
hydrocarbons
• 5.2 Distinguish among allotropes of an
element.
• 5.2 Apply formulas to name molecular
compounds
Naming Molecular
Compounds
CO2 Carbon dioxide
CH4 methane
BCl3
boron trichloride
All are
formed from
two or more
nonmetals.
Ionic
compounds
generally
involve a metal
and nonmetal
(NaCl)
Molecular (Covalent) Nomenclature
for two nonmetals
• Prefix System (binary compounds)
1. Less electronegative atom
comes first.
2. Add prefixes to indicate # of atoms. Omit
mono- prefix on the FIRST element.
Mono- is OPTIONAL on the SECOND
element (in this class, it’s NOT optional!).
3. Change the ending of the
second element to -ide.
Molecular Nomenclature Prefixes
PREFIX
monoditritetrapentahexaheptaoctanonadeca-
NUMBER
1
2
3
4
5
6
7
8
9
10
Molecular Nomenclature:
Examples
• CCl4
• carbon tetrachloride
• N 2O
• dinitrogen monoxide
• SF6
• sulfur hexafluoride
More Molecular Examples
• arsenic trichloride
• AsCl3
• dinitrogen pentoxide
• N2O5
• tetraphosphorus decoxide
• P4O10
Learning Check
Fill in the blanks to complete the following
names of covalent compounds.
CO
carbon ______oxide
CO2
carbon _______________
PCl3
phosphorus _______chloride
CCl4
carbon ________chloride
N2O
_____nitrogen _____oxide
Learning Check
1.
P2O5
a) phosphorus oxide
b) phosphorus pentoxide
c) diphosphorus pentoxide
2.
Cl2O7
a) dichlorine heptoxide
b) dichlorine oxide
c) chlorine heptoxide
3.
Cl2
a) chlorine
b) dichlorine
c) dichloride
A flow chart for naming binary compounds.
Mixed Practice
1.
2.
3.
4.
5.
6.
7.
8.
9.
Dinitrogen monoxide
Potassium sulfide
Copper (II) nitrate
Dichlorine heptoxide
Chromium (III) sulfate
Iron (III) sulfite
Calcium oxide
Barium carbonate
Iodine monochloride
Mixed Practice
1.
2.
3.
4.
5.
6.
7.
8.
9.
BaI2
P4S3
Ca(OH)2
FeCO3
Na2Cr2O7
I2O5
Cu(ClO4)2
CS2
B2Cl4
Polyatomic
Ions
-
NO3
nitrate ion
NO2nitrite ion
Polyatomic Ions
You can make additional polyatomic
ions by adding a H+ to the ion!
CO3 -2 is carbonate
HCO3– is hydrogen carbonate
H2PO4– is dihydrogen phosphate
HSO4– is hydrogen sulfate
Ternary Ionic Nomenclature
Writing Formulas
• Write each ion, cation first. Don’t show
charges in the final formula.
• Overall charge must equal zero.
– If charges cancel, just write symbols.
– If not, use subscripts to balance charges.
• Use parentheses to show more than one
of a particular polyatomic ion.
• Use Roman numerals indicate the ion’s
charge when needed (stock system)
Monatomic Ions
Examples of Older Names of Cations
formed from Transition Metals
(you do not have to memorize these)
Diatomic Elements
• Dr. HOFBrINCl
• These elements are found naturally as two
elements and do NOT use a prefix
• O2 is Oxygen, not DiOxygen
Allotropes
• Molecules of a single element that
different in molecular structure or
crystalline structure
– Oxygen and Ozone
– Diamond, Graphite, Charcoal, Fullerenes,
Acetylenic
Hydrocarbons
• Composed of Carbon Chain and
hydrogens (functional groups discussed
later)
• Methane
Hexane
• Ethane
Heptane
• Propane
Octane
• Butane
Nonane
• Pentane
Decane