Chemical Reactions Flashcards
(Solutions) Solvent
What is doing the dissolving; what there is more of in a solution.
(Solutions) Solute
What is being dissolved; what there is less of in a solution.
(Electrolytes) Strong Electrolytes
Strong acids and ionic compounds.
(Electrolytes) Weak Electrolytes
Weak acids.
(Electrolytes) Non Electrolytes
Covalent compounds.
(Electrolytes) Dissociation
Ionic compounds separate into their respective ions when dissolved in a polar solvent.
(Rules for Determining Oxidation Numbers) The oxidation number of an atom in its elemental form is…
zero.
(Rules for Determining Oxidation Numbers) The oxidation number of a monoatomic ion is…
equal to its charge.
(Rules for Determining Oxidation Numbers) The oxidation number for oxygen in a molecular compound is __, with the exception of peroxides, in which the oxidation number is __.
-2, -1
(Rules for Determining Oxidation Numbers) Hydrogen has a __ charge when bonded to a nonmetal and a __ when bonded to a metal.
+1, -1
(Rules for Determining Oxidation Numbers) For covalent compounds that do no contain hydrogen or oxygen, the most electronegative element has an oxidation number…
equal to its charge as an ion.
(Rules for Determining Oxidation Numbers) The sum of oxidation numbers must equal the…
overall charge of the compound.
(Misc. Reactions) Salts are soluble in water if they contain…
alkali metals, NH₄⁺, or NO₃⁻; always considered as spectator ions.
(Misc. Reactions) Spectator ions are…
ions that do not change phase during a reaction and, as such, are removed from net ionic equations.
(Oxidation-Reduction Reactions) O.I.L.R.I.G.
Oxidation is losing (e⁻), reduction is gaining (e⁻).
(Oxidation-Reduction Reactions) The oxidation number of an oxidized element is…
increased.
(Oxidation-Reduction Reactions) The oxidation number of a reduced element is…
decreased.
(Activity Series) Increasing ease of oxidation correlates to…
increasing reactivity.
(Activity Series) An element will oxidize (take electrons from) anything that is _____ it in the series.
below
(Activity Series) An oxidizing agent…
causes oxidation; is the reduced element.
(Activity Series) A reducing agent…
causes reduction; is the oxidized element.
(Halogen Displacement Redox Reactions) Halogens that are bonded to themselves can take electrons from (oxidize) any halide ions that is below it in the family.
Trend: F₂ > Cl₂ > Br₂ > I₂
F₂ will oxidize all HALIDE IONS below (Cl⁻, Br⁻, I⁻) to form F⁻
Cl₂ will oxidize all HALIDE IONS below it (Br⁻, I⁻) but to form Cl⁻
(Hydrogen Displacement Redox Reactions) Hydrogen atoms in H₂O are reduced as they gain electrons to form hydrogen gas. The redox half-reaction equation for this is:
2H₂O + 2e⁻ —> H₂ + 2OH⁻
(Disproportionation Reactions) Examples:
2Cu¹⁺—> Cu + Cu²⁺
Fe + 2Fe³⁺ —> 3Fe²⁺
(Combustion Reactions) The combustion of any organic hydrocarbon in presence of oxygen gas produces…
CO₂ and H₂O.
(Combustion Reactions) Combustion of any element in the presence of oxygen produces its…
oxide (ex. 2Ca + O₂ —> 2CaO).
(Hydrogen Displacement Redox Reactions) Which metals will displace hydrogen?
Alkali metals, Ca, Sr, Ba.
(Redox Reactions in Acidic Solutions) Net ionic equation of reactions between metals and all strong acids except Nitric Acid
aH⁺ + X —> H₂ + Xᵃ⁺
X is a solid.
Xᵃ⁺ is aqueous.
(Redox Reactions in Acidic Solutions) NO₃⁻ reduces to:
NO
(Redox Reactions in Acidic Solutions) MnO₄⁻ reduces to:
Mn²⁺
(Redox Reactions in Acidic Solutions) Cr₂O₇²⁻ reduces to:
Cr³⁺
(Redox Reactions in Acidic Solutions) SO₃²⁻ oxidizes to:
SO₄²⁻
(Redox Reactions in Acidic Solutions) H₂O₂ oxidizes to:
O₂
(Redox Reactions in Basic Solutions) MnO₄⁻
MnO₂
(Redox Reactions in Basic Solutions) To solve for a basic solution, what do you do in the final step of solving for an acidic solution?
Add OH⁻ to cancel H⁺
