2/16/10
Post date: Feb 16, 2010 2:47:2 AM
Bell Activity: From pages 184-186, how are ionic compounds and covalent compounds different from each other? What properties do they each have?
Ionic and Covalent Bonding
Go over homework, using M&M's for electrons
I2
S2
H20
NH3
P2
Work on bonding practice worksheet (due tomorrow if not finished in class)
Metallic Bonds
Cross between ionic and covalent compounds
Atoms group together, similar shape to a network
Outer layers of electrons overlap, and are shared with neighbors
Electrons are shared between ALL atoms, and can flow freely
Metals conduct electricity and are flexible because their atoms and electrons can move freely throughout the metal's structure
Polyatomic Ions
Breaking down the word:
Poly = many
Atomic = made of atoms
Ion = body that has a non-zero charge
Molecules with a charge
Stick together as a group (behave like a single unit), can bond with other ions
Many common examples
NaHCO3 = baking soda
Na2CO3 = used to make soaps and cleaners
Oppositely charged polyatomic ions can bond together to make larger compounds
(NH4)2SO4
Use parentheses to separate a polyatomic ion from the rest
Do Chapter 6, section 2 review (page 190: 1-9) for tomorrow