Transcript What is an ionic bond?

Ionic Bonds
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Ch. 4-1: p.p. 114-119
NEGATIVE
An atom that gains one or more electrons will have a ____________________
charge.
POSITIVE
An atom that loses one or more electrons will have a ____________________
charge.
ION
An atom that gains or loses one or more electrons is called an ____________.
CATION and a negative ion is called an
A positive ion is called a ______________
ANION
_______________.
“Cat-Eye-On”
“An-Eye-On”
Review: Atoms and Bonding
There are 3 types of bonds:
1.Ionic Bonds – Metals bond with Nonmetals
(electrons are taken, not shared)
2. Covalent Bonds – Nonmetals bond with
Nonmetals (share electrons)
3. Metallic Bonds – Metals bond with Metals
(“positive ions in a sea of electrons”
to describe metallic bonding)
Review: Electrons & Energy Levels
*The Electrons and Energy levels determine how Atoms bond.
ion
p 115
An atom or group
of atoms that is
electrically
charged.
What is an ionic bond?
ELECTRONS to another to form the bond.
Atoms will transfer one or more ________________
COMPLETE outer shell.
Each atom is left with a ________________
METAL ion with a positive charge and a
An ionic bond forms between a ___________
NONMETAL
________________ ion with a negative charge.
*Ionic
bonds attract oppositely charged ions.
(Metal bonded with a Nonmetal)
ion
1-
1+
11P - 10E = +1
17P - 18E = -1
- Ionic Bonds
More Protons = Positive Charge (+) whereas
More Electrons = Negative Charge (-)
- Ionic Bonds
- Ionic Bonds
Stability & Chemical Bonds
ionic bond
Na + Cl 
+
Na Cl
*The
ionic bond is stable.
Turn to page 116 and answer the
following questions:
• What is an ionic bond?
A. An ionic bond is the attraction between
two oppositely charged ions.
Q. What is the overall charge on an ionic
compound?
A. Overall, an ionic compound is electrically
neutral.
Let’s Recap: Ionic Bonds
Oxidation Number
•Number of electrons
an atom gains, loses
or shares when it
forms a chemical bond
•Also called charge
Oxidation Number
The number of
electrons an atom
will gain OR lose to
be happy
Let’s complete the chart for each
element (Bonding Basic handout)…
Now let’s complete each ionic bond!
Example #1
Example #2
Example 3: Sodium + Oxygen
Example 4: Sodium + Chlorine
Group Activity: Now It’s
Your Turn!
Example 5: Calcium + Chlorine
Example 6: Aluminum + Chlorine
Ionization Energy
polyatomic ion
p.117
•An ion that is made
of more than one
atom.
polyatomic ion
polyatomic ion
• carbonate ion: CO3
• How many carbon atoms?
• 1 carbon atom
• How many oxygen atoms?
• 3 oxygen atoms
• What is the overall charge?
• overall charge of 22-
Naming ionic compounds p.117
• The name of the positive ion comes FIRST
• The name of the negative ion comes LAST
• The positive ion is usually the name of the
metal.
• If the name of the negative ion is an element,
the end of its name changes to -ide
•For example, MgO is…
•magnesium oxide
•Look at page 115, Fig. 2 for names of ions
•Complete the following in your notes, page 119 #4:
page 119 #4
NaF
sodium fluoride
BeI2
beryllium iodide
K2SO4
potassium sulfate
page 119 #4
CaO
calcium oxide
H2 S
hydrogen sulfide
MgCo3
magnesium carbonate
Crystal
p.118
•An orderly, 3dimensional pattern
of ions or atoms in a
solid.
Crystals
Structure of ionic compounds
(crystals)
Crystal Shape
• Look at Fig. 4 on p.118
• What general characteristics
of crystals can you observe
in the photograph of halite?
Crystals have tight, compact
bonds
Look at p.118
Na + Cl 
+
Na Cl
Properties of ionic compounds
pages 118-119
The characteristic properties
of ionic compounds include:
1. Crystal shape
2. High melting points
3. Electrical conductivity
Crystal Shape
High Melting Points
•Why are ionic bonds so
strong?
•Answer: Every ion is attracted to
ions near it that have an opposite
charge.
*When exposed to high heat, the
particles do break away from each
other.
Electrical Conductivity
• Why do ionic compounds
dissolve/separate in water?
• Answer: Water breaks ions
apart, allowing the ions to
move freely.
Ionic Bonding Activity
http://www.learner.org/interactives/period
c/groups_interactive.html