1. Metallic bonds

2. Metals Metal atoms are arranged in very compact and orderly patterns
Metals that contain just one kind of atom are among the simplest forms of all crystalline solids

3. Metallic Bond
The electrostatic attraction of the delocalized electrons for the positively charged metal ions
Electron Sea Model
Made up of closely packed cations surrounded by electrons
Outer e clouds of the metal ions overlap
Share their electrons to form a sea of electrons
What are delocalized electrons?
What do we call a positive ion?

5. Properties of Metals Moderately high melting and boiling points
Good conductors of heat and electricity
Malleable and Ductile
Mobile electrons can easily be pushed or pulled past each other
High melting and boiling points (also called low volatility) because of strong electrostatic force
Think back to why dissolved or melted ionic compounds could conduct electrical current, why do you think metals make good conductors?
Why are they malleable and ductile?

6. Alloys Mixture of two or more elements (at least one must be a metal)
Has metallic properties often superior to those of their component elements
-Bronze: copper + tin
-Steel: iron + carbon + other metals
-Sterling silver: silver + copper
What is an alloy?
Why are their properties superior?

7. Cu Zn Brass at the atomic level Brass though a magnifier
What kind of a mixture is this?
Brass at the atomic level
Brass though a magnifier

8. Types of Alloys Substitutional Interstitial
Atoms have relatively the same size
Atoms of different sizes
What is an alloy?
Why are their properties superior?