section 4.1 and 4.2 types of chemical reactions and aqueous solutions
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Section 4.1 and 4.2Types of Chemical Reactions and
Aqueous Solutions
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In this section:
a. Types of Chemical reactions1. Combination reactions2. Decomposition reactions3. Displacement reactions
b. Aqueous Solutions1. Compounds in aqueous solution2. Electrolytes3. Solubility of ionic compounds
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Combination Reactions
Two or more reactants form a single product
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Decomposition Reactions
A single reactant breaks up to form two or more products
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Single Displacement Reactions
One “part” of a compound is replaced by another
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Double Displacement ReactionsMetathesis Reactions
Two atoms or ions exchange.
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Two atoms or ions exchange.
Precipitation reactions:
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Two atoms or ions exchange.
Acid-base (neutralization) reactions:
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Two atoms or ions exchange.
Gas-forming reactions:
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Aqueous Solutions
Solutes dissolved in the solvent water.
Categorized by the nature of the dissolved species.
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Aqueous Solutions: ElectrolytesSolutes dissolved in the solvent water.
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Aqueous Solutions: ElectrolytesStrong Electrolytes: all solute dissociates to form ions in solution.
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Aqueous Solutions: ElectrolytesWeak Electrolytes: A small fraction of solute dissociates to form ions in solution.
HF(aq) H+(aq) + F-(aq)
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Aqueous Solutions: ElectrolytesNonelectrolytes: Solute molecules do not form ions in solution.
Example: CH3OH
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Aqueous Solutions: ElectrolytesStrong electrolytes: conduct electricity well
soluble ionic compoundsstrong acids
Weak electrolyte: conduct electricity poorlyweak acids and the weak base NH3
Nonelectrolytes: do not conduct electricitymost molecular, covalent compounds
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Solubility of Ionic Compounds
Basic Idea: for ionic compound MX (M+ cation and X- anion)
When added to water, does:
MX(s) M+(aq) + X-(aq)
happen?
Yes: compound is soluble in waterNo: compound is insoluble in water
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Solubility of Ionic Compounds
A little more complicated: how soluble is soluble?
1 g solute per 100 g water.
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Solubility RulesPart 1: things that are generally soluble
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Solubility RulesPart 1: things that are generally insoluble
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Section 4.4 Oxidation Reduction Reactions
Redox ReactionsElectron-Transfer Reactions
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In this section:
a. oxidation and reductionb. oxidation numbersc. recognizing redox reactionsd. predicting redox reactions
Not from this section:
a. Organic reactions
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Oxidation-Reduction Reactions
Oxidation = loss of electronsReduction = gain of electrons
Zn(s) + Cu2+(aq) Zn2+(aq) + Cu(s)
Oxidation Half-Reaction: Zn(s) Zn2+(aq) + 2 e-
Reduction Half-Reaction: Cu2+(aq) + 2 e- Cu(s)
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Oxidation-Reduction Reactions
Oxidation = loss of electronsReduction = gain of electrons
Zn(s) + Cu2+(aq) Zn2+(aq) + Cu(s)
Oxidizing agent = oxidant = gains electronsReducing agent = reductant = loses electrons
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Balancing Simple Redox Reactions
Cu(s) + Ag+(aq) Cu2+(aq) + 2 Ag(s)
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Oxidation Numbers
Electron tracking method.
Oxidation numbers do not imply charges.
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Examples:
N in N2
Fe in Fe3+
N in NO2-
O in H2O
Cl in NaOCl
Mn in MnO4-
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Recognizing Oxidation-Reduction Reactions
Oxidation = loss of electrons = increase in ox #Reduction = gain of electrons = decrease in ox #
4 Fe + 3 O2 2 Fe2O3
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CuO(s) + H2(g) Cu(s) + H2O()
CaCO3(s) CaO(s) + CO2(g)
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MnO4-(aq) + 5 Fe2+(aq) + 8 H+(aq) Mn2+(aq) + 4 H2O() + 5 Fe3+(aq)
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Predicting Redox Reactions
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Organic Reactions
A. Combustion ReactionsReaction with oxygen gas to form CO2 and H2O.
C3H8(g) + 5 O2(g) 3 CO2(g) + 4 H2O(l)
B. Substitution ReactionsExchange of one atom or molecular fragment.
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C. Addition ReactionsAddition of two molecules together.
D. Elimination ReactionsEjection of a small molecule from a larger one.
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E. Isomerization (Rearrangement) ReactionsChange of shape of a molecule without gain or loss of any atoms.