Ionic Bonds /. Ch. 4-1: p.p. 114-119 An atom that gains one or more electrons will have a ____________________ charge. An atom that loses one or more.

Ionic Bonds

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Ch. 4-1: p.p. 114-119

An atom that gains one or more electrons will have a ____________________ charge.

An atom that loses one or more electrons will have a ____________________ charge.

An atom that gains or loses one or more electrons is called an ____________.

A positive ion is called a ______________ and a negative ion is called an _______________.

POSITIVE

NEGATIVE

ION

CATIONANION

“An-Eye-On”“Cat-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?

Atoms will transfer one or more ________________ to another to form the bond.

Each atom is left with a ________________ outer shell.

An ionic bond forms between a ___________ ion with a positive charge and a

________________ ion with a negative charge.

ELECTRONS

COMPLETE

METAL

NONMETAL

*Ionic bonds attract oppositely charged ions. (Metal bonded with a Nonmetal)

ion

11P - 10E = +1 17P - 18E = -1

1+1+ 1-1-

- Ionic Bonds

More Protons = Positive Charge (+) whereasMore Electrons = Negative Charge (-)

- Ionic Bonds

- Ionic Bonds

Stability & Chemical Bonds

ionic bond

Na + Cl Na + Cl Na Na++ClCl--

*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 chargecharge

Oxidation NumberOxidation 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

Example 5: Calcium + Chlorine Example 6: Aluminum + Chlorine

Group Activity: Now It’s Your Turn!

Ionization Energy

polyatomic ion p.117

•An ion that is made of more than one atom.

polyatomic ion

polyatomic ionpolyatomic ion• carbonate ion: CO3

2-

• How many carbon atoms?• 1 carbon atom • How many oxygen atoms?• 3 oxygen atoms• What is the overall charge?• overall charge of 2-

Naming ionic compounds p.117Naming 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

CaOcalcium oxide

H2Shydrogen sulfide

MgCo3

magnesium carbonate

Crystal p.118

•An orderly, 3-dimensional pattern of ions or atoms in a solid.

Crystals

Structure of ionic compounds (crystals)

Crystal ShapeCrystal 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.118Look at p.118

Na + Cl Na + Cl Na Na++ClCl--

Properties of ionic compoundsProperties of ionic compounds

pages 118-119

The characteristic properties of ionic compounds include:

• Crystal shape

• High melting points

• 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 ActivityIonic Bonding Activity

http://www.learner.org/interactives/periodic/groups_interactive.html