3.1 & 3.2 Learn the features of a chemical equation

Reactants Products Stoichiometric Coefficients Physical State

Learn how to balance chemical equations Apply the Law of Conservation of

matter

EOC

3.3 Many chemical reactions are reversible. Are ALL chemical reactions reversible…in theory(?)

3.5•Define and apply the terms to Molecular and Ionic compounds

Molecular (if they dissolve…)oStrong electrolyte Dissolve & 100% Dissociate oWeak electrolyte Dissolve & <100% DissociateoNonelectrolyte Dissolve & None Dissociate

Ionic - Dissolve = Dissociate in water100 soluble & slightly soluble

Strong & Weak Acids

Just about everythingElse, i.e sugar, alcohols

3.5 & 3.6 Know that many ionic compounds are

solids at room temperature Know that not all ionic compounds

dissolve completely at room temperature

http://www.screencast.com/t/MGZkZDgxZTY

Learn the solubility of particular types of ionic compounds

Learn how and when to write Net Ionic Equations

General Form of a Double Displacement Rxn

PPT Rxns are examples of a Double Displacement Rxns

3.7 Learn how acidic and basic substances

behave in water. Distinguish between strong and weak

acids, and between strong and weak bases.

Apply the concept of net ionic reaction to acid/base neutralization reactions.

Strong Acid Weak Acid Strong Base Weak Base

EOC

General Form of a Double Displacement Rxn

Acid/Base Rxns are examples of Double Displacement Rxns

3.8 Recognize gas forming reactions

a. Be able to predict the reactants required to produce a particular gas

b. Be able to predict the products produced given particular reactants

General Form of a Double Displacement Rxn

Apply Double Displacement to gas forming rxns (with caution)

3.9 Use guidelines on the next slide to

predict oxidation numbers of atoms. Define the terms redox, reduction,

oxidation, reducing and oxidizing agents Recognize a REDOX reaction

1). Oxidation state of an element = 0 (i.e., Li, F2, H2, C)2). Oxidation state a monatomic ion = ionic charge (Na+ = +1, Mg2+ = +2)3). Oxidation state of O = -2 in all its compounds except: 

(a) Peroxides e.g. Na-O-O-Na, where ox. # = -1(b) Superoxides, e.g. KO2 where ox. # = -1/2

4). H is +1 in all its compounds (except metal hydrides ox.# = -1)5). F is - 1 in all its compounds 6). Alkali metals are always +1; alkaline earth metals are always +2.7). Sum of oxidation states is zero for neutral compounds,

and equal to the overall charge for polyatomic ions. 

Guidelines for Assigning Oxidation Numbers

3.10 Distinguish among precipitation, acid/base, gas forming and REDOX reactions Write net ionic equations for precipitation, acid/base, gas forming and REDOX reactions