1. Metallic Properties Main Concept:
The interaction of electromagnetic waves or light with matter is a powerful means to probe the structure of atoms and molecules, and to measure their concentration.

2. Metallic Properties Metallic Bonding – How Atoms are Arranged
Properties of Metals
Conductivity
Malleability/Ductility
Kinds of Alloys: Properties:
Interstitial
Substitutional

3. - metallic solids can be represented as positive kernels (or cores) consisting of nuclei and inner electrons of each atom surrounded by sea of mobile valence electrons

4. Metals are:
- good conductors b/c the electrons are delocalized and relatively free to move.
- malleable and ductile b/c deforming solids does not change environment immediately surrounding each metal core

5. - Metallic solids are often pure substances, but may also be mixtures called alloys.
- size of the component atoms can help us understand some properties of alloys (interstitial and substitutional):

6. Interstitial Alloys:
- form b/w atoms of different radius, where smaller atoms fill interstitial spaces between the larger atoms
Example: Steel – carbon occupies the
interstices in iron
- atoms make lattice more rigid, decreasing malleability and ductility

7. Substitutional Alloys:
- form b/w atoms of comparable radius, where one atom substitutes for the other in the lattice
Example: Brass – some of the copper atoms
are substituted with a different element, usually zinc
- density typically lies between component metals
- like interstitial alloys, substitutional alloys
are less malleable and ductile than pure metals

8. - Alloys typically retain a sea of mobile electrons and so remain conducting
- surfaces of a metals or alloys are often changed through a chemical reaction
Example: formation of a chemically inert oxide
layer in stainless steel, through reaction
with oxygen in the air.

9. Effects of oxidation: