5.01 - Synthesis Reactions - 15:18

KEY CONCEPTS:

2 or more reactant --> 1 product

metal oxide + water --> base (bases contain an OH-)

non-metal oxide + water --> oxy-acid
(oxy-acid is a polyatomic with a hydrogen acting as a cation) - see what type of polyatomic comes to mind when you look at the non-metal oxide

5.02 - Decomposition Reactions - 5:23

KEY CONCEPTS:

1 reactant --> 2 or more products

metal hydrogen carbonate --> metal carbonate + CO2 + H2O
(the metal can be any of the metals to the left of the aluminum ladder combined with a hydrogen carbonate. The end products are CO2 and H2O along with the metal bonded to the carbonate)

i.e: NaHSO4 --> Na2SO4 + CO2 + H2O

3.06 - Acid Base Nomenclature - 14:48

KEY CONCEPTS: When naming Binary Acids, start by identifying the hydrogen atom as "hydro" and name the non-metal using the "ic" ending and add the word acid.

Rules for Oxy-Acids:
They are derivatives of polyatomic ions and polyatomic variations. Follow the following 4 rules:

i.) ____ate ions become _______ic acid
ii.) per____ate ions become per_____ic acids
iii.) ____ite ions become _____ous acids
iv.) hypo____ite ions become hypo_____ous acids

Bases contain hydroxide ion (OH)-1

**NOTE: NO "hydro" for oxy-acids

3.01 - Writing Formulas for Binary Ionic Compounds - 20:51

KEY CONCEPT:

When you combine a metal and a non-metal, use the 5 Step Cross over Rule to put together your formula

4.02 - Balancing Equations - 22:35

KEY TERMS: balance both sides of the equation by placing a number (coefficient) in front of the compound. Don't be afraid to have to change that number if it does not completely balance the equation. Balance polyatomic ions first. Remember that REACTANTS are to the left of the arrow and PRODUCTS are to the right of the arrow. Refer to episode on "Counting Atoms". Don't forget your diatomic molecules:

oxygen = O2
hydrogen = H2
bromine = Br2
chlorine = Cl2
iodine = I2
fluorine = F2
nitrogen = N2