Ionic Bonds /

Ch. 4-1: p.p 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 CATION ANION “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 = +117P - 18E =

- Ionic Bonds More Protons = Positive Charge (+) whereas More Electrons = Negative Charge (-)

- 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 c cc charge

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

carbonate ion: CO 3 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.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 BeI 2 beryllium iodide K 2 SO 4 potassium sulfate

page 119 #4 CaO calcium oxide H2SH2S hydrogen sulfide MgCo 3 magnesium carbonate

Crystal p.118 An orderly, 3- dimensional 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 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 c/groups_interactive.html