The Structure of Matter
Chapter 5
1
Compounds



Compounds are made
from two or more
elements.
The compound has
properties that are
different from those of
the elements that
make it.
Compounds always
have the same
chemical formula.
2
Chemical Bonds



The attractive forces
that hold different
atoms or ions together
in compounds are
called chemical bonds.
A bond length gives
the distance between
the nuclei of the two
bonded atoms.
Bond angles tell how
these atoms are
oriented in space.
3
Structural Formulas

Structural formulas
can show how the
atoms are arranged in
a compound.
4
What do we call the force that holds
atoms in a molecule together?
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Atoms
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Valence electrons
A
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5
The properties of a compound are
different than the properties of the
elements that make up the compound.
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6
Types of Bonds



Ionic bonds are
formed between
oppositely charged
ions.
Metallic bonds are
formed between
atom’s nucleus and a
neighboring atom’s
electrons.
Covalent bonds are
made between atoms
of nonmetals.
7
Ionic Bond





Bond between a metal
ion and a nonmetal
ion.
The oppositely
charged ions are
attracted to each
other.
Forms ionic solids.
High melting point.
Conduct electric
current.
8
Metallic Bond




Bond that occur
between atoms of
metal.
Compounds are
malleable and ductile.
Conduct electricity &
heat.
Mixed to form alloys.
9
Covalent Bond





Bond formed between
two nonmetals.
Share electrons.
Lower melting and
boiling points than
ionic compounds.
Covalent compounds
are soft and squishy.
Covalent compounds
tend to be more
flammable than ionic
compounds.
10
Polyatomic Ions



Polyatomic ions are
groups of covalently
bonded atoms that
have either lost or
gained electrons.
The group of atoms
act as a single ion.
Polyatomic ions are
put in parenthesis
when you need to
have more than one in
a ion.
HCO3−
11
Writing Chemical Formulas for Ionic
Compounds




List the symbols for each
ions.
Write the symbols for the
ions with the cation first.
Find the least common
multiple of the ions’
charges.
Write the chemical
formula, indicating with
subscripts how many of
each ion are needed to
make a neutral compound.
12
Naming Covalent Compounds



Name the element
that is farthest to the
left on the periodic
table.
Add a prefix if there is
more than one atom.
Name the element
that is farthest to the
right on the periodic
table and change the
ending to an –ide.
13
Writing Chemical Formulas for Covalent
Compounds.


List the chemical
symbols of the
elements.
Add subscripts to
indicate how many
atoms of each
element there is in a
molecule of the
compound.
CO2
14
Empirical vs. Molecular Formulas


Empirical formula
shows the smallest
whole-number ratio of
atoms that are in a
compound.
Molecular formula tells
how many atoms are
in one molecule of the
compound.
C6H12O6
15
Organic Compound




Organic compound is a
covalently bonded
compound made of
molecules.
Organic compounds
contain carbon and most of
the time hydrogen.
Carbon can form four
covalent bonds.
Compounds made of only
hydrogen & carbon atoms
are called hydrocarbons.
16
Types of Organic Compounds



Alkanes only have
single covalent bonds.
Alkenes have double
covalent bonds.
Alcohols have
hydroxly or –OH
group attached.
17
Alkanes










Methane
Ethane
Propane
Butane
Pentane
Hexane
Heptane
Octane
Nonane
Decane
18
Alkenes










Methene
Ethene
Propene
Butene
Pentene
Hexene
Heptene
Octene
Nonene
Decene
19
Alcohols










Methanol
Ethanol
Propanol
Butanol
Pentanol
Hexanol
Heptanol
Octanol
Nonanol
Decanol
20
Polymers



Polymers are large
molecule that is
formed by more than
five monomers or
small units.
Polymers can be
natural or synthetic.
Polymers elasticity
varies depending on
the structure.
21
Biochemical Compounds


Biochemical
compounds are
naturally occurring
organic compounds
that are very
important to living
things.
Type of biochemical
compounds:



Carbohydrates (simple
sugars)
Proteins (amino acids)
Lipids (fatty acids)
22