eoc 3.5 define and apply the terms to molecular and ionic compounds molecular (if they dissolve…)...
TRANSCRIPT
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
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