1. Metallic & Polar Covalent Bonds
Describe how metals bond and form alloys
Describe the way different molecules bond to each other

2. Metallic Bonds and Properties
Metallic bonds form between metal elements
The valence electrons of metal atoms can be modeled as a sea of electrons
The electrons are mobile and can drift from one part of the metal to another
This is how electricity works

3. Crystalline Structure of Metals
Metal atoms are arranged in very compact and orderly patterns
There are three basic patterns

4. Alloys
The properties of alloys are often better than those of their component elements
Examples:
Sterling silver (silver and copper) is more durable than pure silver
Steels (iron, carbon, boron, chromium etc) resist corrosion, have better ductility, hardness, and toughness

5. Molecular Orbitals
Sigma bonds form when 2 atomic orbitals combine, forming a symmetrical orbital around an axis
Pi bonds form when p orbitals overlap end-to-end forming sausage-shaped regions above and below the bond axis

6. VSEPR Theory Valence Shell Electron-Pair Repulsion
Repulsion between electron pairs causes molecular shapes to adjust so that the valence-electron pairs stay as far apart as possible

7. Bond Polarity
Nonpolar covalent bonds form when bonding electrons are shared equally
Diatomic molecules are nonpolar
Polar covalent bond, or a polar bond, is a bond between atoms in which the electrons are shared unequally
The more electronegative atom attracts electrons and gains a slight negative charge, the less electronegative atom gains a slightly positive charge.
Example: Water

8. Attractions Between Molecules
Van der Waals Forces consist of dipole interactions and dispersion forces
Weakest attractions between molecules
Dipole interactions occur when polar molecules are attracted to one another
Dispersion forces occur when moving electrons in a nonpolar molecule are momentarily more on one side than other. Momentary dipole

9. Hydrogen Bonds
Attractive forces in which a hydrogen which is covalently bonded to a very electronegative atom is also weakly bonded to an unshared electron pair of another electronegative atom.

10. Network Solid
A solid in which all of the atoms are covalently bonded to each other
Examples: Diamond and Silicon carbide

11. Ionic vs Covalent Lab Hypothesis (in lab Notebook)
What properties of a compound will you use to determine if a bond is ionic or covalent? Choose three properties be sure to include why these properties will be useful in determining the bond type.
You will be writing a conclusion for the ionic vs covalent lab. You will be asked to provide multiple pieces of evidence for why you labeled a compound ionic or covalent. You will also be asked to include an evaluation of your hypothesis. Was your initial plan to test specific properties of a compound in support of your findings?