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Transcript
3.1 Compounds

Compounds are pure substances made of more than
one kind of atom joined together. The atoms are held
together with chemical bonds.
(c) McGraw Hill Ryerson 2007
See pages 76 - 78
Compounds


Compounds come in two basic types: covalent
and ionic.
To determine whether a compound is covalent or
ionic, the periodic table is required.
(c) McGraw Hill Ryerson 2007
Covalent Compounds
 Covalent
compounds are made up of
two non-metals.
 Covalent compounds share electrons to
form molecules. Example: water
(c) McGraw Hill Ryerson 2007
Ionic Compounds
 Ionic
compounds are made up of a metal
and a non-metal.
 In ionic compounds, atoms gain or lose
electrons to form ions. Example: NaCl
(c) McGraw Hill Ryerson 2007
Ionic Compounds


Ionic solids exist as a solid in the form of an ionic
lattice.
The positive ions attract all of the negative ions,
and vice versa. In the example of table salt (NaCl)
the one-to-one ratio of ions results in a simple
square-shaped ionic cyrstal:
(c) McGraw Hill Ryerson 2007
See page 78
Polyatomic Ions



Covalent and ionic bonds can occur
together.
A molecule can gain or lose electrons to
become charged, forming a polyatomic ion.
Polyatomic ions form compounds like
other ions.
 Example: Ammonium ion (NH4+)
(c) McGraw Hill Ryerson 2007
Polyatomic Ions
(c) McGraw Hill Ryerson 2007
Section 3.1 Quiz
See pages 79 - 80