1. Bell Ringer 10-27-09 Covalent bonds are usually between _______.
Ionic bonds are usually between _______.
Ionic bonds are the _______ of electrons.
Covalent bonds are the _______ of electrons.
What are the two kinds of covalent bonds?
What type of covalent bonds involves unequal sharing of e-?

2. ALCOS Objectives # 2 Describe the structure of atoms.
# 5 Differentiate between ionic and covalent bonds.

3. Chapter 5 Section 4
Metallic Bonding

4. Why use Metals instead of Nonmetals?

5. Physical Characteristics of metals
Luster- Shiny and Reflective
Good conductors of heat or electricity
Most are solids at room temperature
Ductile
Malleable

6. Chemical properties Reactivity
The reactivity of metals tends to decrease as you move from left to right across the periodic table.

7. Alloys
An alloy is a mixture made of 2 or more elements that has the properties of a metal.
In every alloy at least one of the elements is a metal.
Alloys are generally stronger and less likely to react with air or water than pure metals are.

8. Examples Jewelry Tools Coins Not necessarily pure gold
Usually an alloy of gold with a harder metal
Tools
Not only iron (rust)
Coins
Penny used to be just Copper, but now Zinc is also in it
Zoom in on a Penny

9. Timeline of the Penny 1783 to 1837- A penny was pure copper.
1837 to The cent was made of bronze (95 percent copper, and five percent tin and zinc).
1857- The cent was 88 percent copper and 12 percent nickel, giving the coin a whitish appearance.
1864 to The cent was again bronze (95 percent copper, and five percent tin and zinc)
except: In 1943, the coin's composition was changed to zinc-coated steel.  This change was only for the year 1943 and was due to the critical use of copper for the war effort. 
In 1962, the cent's tin content, which was quite small, was removed.  That made the metal composition of the cent 95 percent copper and 5 percent zinc.
1982- when the composition was changed to 97.5 percent zinc and 2.5 percent copper (copper-plated zinc). 

10. Most metals have 1, 2, or 3 valence e-.
Therefore, most metals will lose e- when they bond becoming positively charged ions.

11. Metallic bonding
A metallic bond is an attraction between a positive metal ion and the electrons surrounding it.
A metal or metal alloy consists of positively charged metal ions embedded in a “sea” of valence electrons.

12. Synthetic elements Recall: Elements 1-92= In Nature
Elements 93 and above = Synthetic (Man-made)
Video-
Colliders

13. Chemical Bonds What is it? What is it? What is it? Example/ Types
Ionic Bonds
Covalent Bonds
Metallic Bonds
What is it?
What is it?
What is it? In
________
Between ________
Between ________
Example/ Types
Example
Example

14. Chemical Bonds Transfer of electrons Sharing of electrons Polar- HF Fe
Ionic Bonds
Covalent Bonds
Metallic Bonds
Transfer of electrons
Bond between a positive metal ion and its e-
Sharing of electrons
Between nonmetals and metals
Between Nonmetals
In Metals
Polar- HF
Nonpolar- H-H Fe
NaCl

15. After Quiz…
Make list of Elements Hydrogen  Argon (1-18) to memorize for quiz next week (put in notebook!!)
You will need to know the symbol and name
Chapter 5 Review p # (omit #19)