Covalent Bonds
Between 2 or
more
non-metals
Naming Covalent Compounds
Uses Greek prefixes to
indicate the number
(instead of relying on
charge with ionic bonds)
Still uses -ide at
the end of the
second element
They SHARE
electrons
Step by Step
Step by Step
Step by Step
5 easy
steps
1. Determine Arrangement
(place least electronegative atom in the
center. Halogens and hydrogen will
never be in the center
2. Determine total number of valence eONE DASH = TWO ELECTRONS
(add for negative ions, subtract for
positive ions)
Step by Step
Step by Step
Step by Step
3. Connect atoms using dashes
4. Distribute remaining e(also called lone pairs)
5. Use double and triple bonds if
necessary.
Hydrogen and the halogens can never
have a double or triple bond
Lewis dot structures
CF4
1) get the total #
of valence
electrons
Lewis dot structures
CF4
2) Pick the central
atom
Lewis dot structures
CF4
3) Ready to
create
One line = 2 electrons
Double and triple bonds
CO2
1) Same thing add up V e-
Double and triple bonds
CO2
2) Pick central
atom
Double and triple bonds
CO2
3) ready to create
Lone e- pairs around
central atom
PCl3
1) Same thing add up V e-
Polyatomic Ions
1) Same thing add up V e-
Charge = 2So add two more
Lone e- pairs around
central atom
PCl3
2) Pick central
atom
SO32-
Polyatomic Ions
2) Pick central
atom
Lone e- pairs around
central atom
PCl3
3) ready to create
SO32-
Polyatomic Ions
3) Ready to
create
SO32-
Acids - known by
the presence of H
Question for you
Naming acids w/o oxygen
Naming acids with oxygen
Naming acids with oxygen
Binary acid
Polyatomic ions
Polyatomic ions
Use the prefix hydro
+ root of the anion’s name –ic
+ the word acid
HCl
HF
HBr
DO NOT USE the prefix hydro
Depends on polyatomic ion
Rules on next slide
Polyatomic ion
-ATE
-ITE
Acid ending
-IC
-OUS
Sulfate
ion
Sulfite
ion
H2SO4
H2SO3
Sulfuric
acid
Binary Acids
Use the prefix
hydro
Sulfurous
acid
Polyatomic Ions and acids
-ATE
-IC
+ root of the
anion’s name –ic
-ITE
+ the word acid
-OUS
Phosphate
ion
H3PO4
Phosphoric
acid
Phosphite
ion
Timer
H3PO3
Phosphorous
acid
General Properties of
Covalent compounds vs. covalent networks
Covalent Networks
Atoms bonded together
in a strong covalent
network
Very strong
General Properties of
Covalent compounds vs. Covalent networks
Both are composed of
non-metals
General Properties of
Covalent compounds vs. Covalent networks
Can be solid, liquid, or
gas at room temp.
Very hard solids
General Properties of
Covalent compounds vs. Covalent networks
High melting point
Low melting point
Almost 5000 degrees C
General Properties of
Covalent compounds vs. Covalent networks
Poor conductor
Poor conductor
1
2.
5.
3.
6.
4.
7.
8.
9.
Let’s go back through them, but
i’m going to put names on these
stretches now
1.Linear
2. Trigonal
Planar
3.Square
Planar
4. T-Shape
See-Saw
Bent
A little
different than
the picture
Trigonal
Pyramidal
Tetrahedral
Trigonal
Bipyramidal
Valence Shell Electron-Pair
Repulsion Theory
VSEPR
Computer activity
https://phet.colorado.edu/sims
/html/molecule-shapes/latest/
molecule-shapes_en.html
Ionic bonding
Covalent
bonding
Between metal
and non-metal
Between non-metal and
non-metal
Google
phet molecule shapes
Metallic Bonding
Between metal and metal
Remember, metals have
larger atomic radii and
lower ionization energy
Metallic Bonding
Get out a half sheet of
paper
What are metals used
for?
Crumble it up and throw
it to someone
Add some of yours to
their list
Metallic Bonding
What are some
properties of metals that
you know of?
Crumble it up and throw
it to someone
Write down ionic and
covalent properties
Add some of yours to
their list
Covalent networks and
covalent compounds
Ionic bonding
properties
Covalent compound
properties
Crumble it up and throw
it to someone
Brittle and hard
Can be soft or brittle
Add some of yours to
their list
Solid:Poor conductors
Liquid: Great conductors
Solid/liquid: poor conductors
High melting/boiling point
Low melting/boiling points
Metallic Bonding
Works a little differently
because it doesn’t have
the properties of
ionic/covalent
Malleable and
ductile
Great conductors
Metallic Bonding
The “Sea of Electrons”
Metallic Bonding
The orbitals of
the large atoms
overlap and the
electrons can
travel between
any of the
atoms
Metallic Bonding
Metallic Bonding
Works a little differently
because it doesn’t have
the properties of
ionic/covalent
The electrons
are not bound to
a specific atom
like in covalent
or ionic bonds
Malleable and
ductile
Great conductors
Metallic Bonding
Properties
Conductivity
Metallic Bonding
Properties
Malleable and
ductile
What’s on the test
1.
2.
3.
4.
5.
6.
Lots of lewis structures
VSEPR (angles and geometry names)
Polar vs. Non-polar molecules
Naming/formulas (acids and compounds)
Networks vs. compounds properties
Metallic bond properties/drawing pictures
Water (polarity?)
Review
PF3 (polarity?)
SO3 2-
CO2 (polarity?)
SO3
Binary Acids
Use the prefix
hydro
Polyatomic Ions and acids
-ATE
-IC
+ root of the
anion’s name –ic
-ITE
+ the word acid
-OUS
Covalent Networks
General Properties of
Covalent compounds vs. covalent networks
Atoms bonded together
in a strong covalent
network
Very strong
General Properties of
Covalent compounds vs. Covalent networks
Both are composed of
non-metals
General Properties of
Covalent compounds vs. Covalent networks
Poor conductor
Poor conductor
General Properties of
Covalent compounds vs. Covalent networks
Can be solid, liquid, or
gas at room temp.
Very hard solids
High melting point
Low melting point
Almost 5000 degrees C
Metallic Bonding
Metallic Bonding
Properties
Properties
Malleable and
ductile
General Properties of
Covalent compounds vs. Covalent networks
Conductivity