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Chapter 3 - Continued
Structure and Properties of Ionic
and Covalent Compounds
Denniston
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6th Edition
20 August 2011
How to read your test results
Writing Names of Ionic Compounds
from the Formula of the Compound
• Name the cation followed by the name
of the anion
• A positive ion retains the name of the
element; add the anion suffix -ide
Writing Names of Ionic Compounds
from the Formula of the Compound
•
If the cation of an element has several ions of
different charges (as with transition metals) use a
Roman numeral following the metal name
• Roman numerals give the charge of the metal
•
Examples:
•
FeCl3 is iron(III) chloride
•
FeCl2 is iron(II) chloride
•
CuO is copper(II) oxide
Common Nomenclature System
• Use -ic to indicate the higher of the
charges that ion might have
• Use -ous to indicate the lower of the
charges that ion might have
• Examples:
• FeCl2 is ferrous chloride
• FeCl3 is ferric chloride
Stock and Common Names for
Iron and Copper Ions
Common Monatomic Cations and Anions
• Monatomic ions - ions consisting of a single
charged atom
Polyatomic Ions
• Polyatomic ions - ions composed of 2 or
more atoms bonded together with an overall
positive or negative charge
– Within the ion itself, the atoms are bonded using
covalent bonds
– The positive and negative ions will be bonded to
each other with ionic bonds
• Examples:
• NH4+ ammonium ion
• SO42- sulfate ion
Common Polyatomic Cations and Anions
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Common Polyatomic Cations and Anions
Name These Compounds
1. NH4Cl
2. BaSO4
3. Fe(NO3)3
4. CuHCO3
5. Ca(OH)2
Writing Formulas of Ionic Compounds
from the Name of the Compound
• Determine the charge of each ion
• Write the formula so that the resulting
compound is neutral
• Example:
Barium chloride:
Barium is +2, chloride is -1
Formula is BaCl2
Determine the Formulas from
Names
Write the formula for the following ionic
compounds:
1. sodium sulfate
2. ammonium sulfide
3. magnesium phosphate
4. chromium(II) sulfate
Covalent Compounds
• Covalent compounds are typically formed from
nonmetals
• Molecules - compounds characterized by covalent
bonding
• Not a part of a massive three-dimensional crystal
structure
• Exist as discrete molecules in the solid, liquid, and gas
states
Naming Covalent Compounds
1. The names of the elements are written in the
order in which they appear in the formula
2. A prefix indicates the number of each kind of
atom
Naming Covalent Compounds
3. If only one atom of a particular element is
present in the molecule, the prefix mono- is
usually omitted from the first element
Example: CO is carbon monoxide
4. The stem of the name of the last element is
used with the suffix –ide
5. The final vowel in a prefix is often
dropped before a vowel in the stem name
Name These Covalent Compounds
1. SiO2
2. N2O5
3. CCl4
4. IF7
Writing Formulas of Covalent
Compounds
• Use the prefixes in the names to determine the
subscripts for the elements
• Examples:
• nitrogen trichloride
NCl3
• diphosphorus pentoxide
P2O5
• Some common names that are used:
–
–
–
–
H2 O
NH3
C2H5OH
C6H12O6
water
ammonia
ethanol
glucose
Provide Formulas for These
Covalent Compounds
1. nitrogen monoxide
2. dinitrogen tetroxide
3. diphosphorus pentoxide
4. nitrogen trifluoride