Reactions in aqueous solutions
Solution
a homogeneous mixture of two or more substances
Solute
the substance present in a smaller amount
Solvent
the substance present in a larger amount
Aqueous Solutions
the solute initially is a liquid or a solid and the solvent is water
Electrolyte
a substance that, when dissolved in water, results in a solution that can conduct electricity
Nonelectrolyte
does not conduct electricity when dissolved in water
Dissociation
the breaking up of the compound into cations and anions
Hydration
the process in which an ion is surrounded by water molecules arranged in a specific manner
Reversible Reaction
the reaction can occur in both directions
Precipitation Reaction
reaction that occurs in aqueous solution and results in the formation of an insoluble product, or precipitate
Precipitate
an insoluble solid that separates from the solution
Metathesis Reaction (double-replacement reaction)
a reaction that involves the exchange of parts between the two compounds
Solubility
the maximum amount of solute that will dissolve in a given quantity of solvent at a specific temperature
Molecular Equation
the formulas of the compounds are written as though all species existed as molecules or whole units
Ionic Equation
shows the dissolved species as free ions
Spectator Ions
ions that are not involved in the overall reaction
Net Ionic Equation
shows only the species that actually take part in the reaction
Brønsted acid
a proton donor
Brønsted base
a proton acceptor
Hydronium Ion
hydrated proton (H3O+)
Monoprotic Acids
each unit of the acid yields one hydrogen ion upon ionization
Diprotic Acid
each unit of the acid gives up two H+ ions
Triprotic Acid
yield three H+ ions
Neutralization Reaction
a reaction between an acid and a base
Salt
an ionic compound made up of a cation other than H+ and an anion other than OH- or O2-
Oxidation-Reduction (redox) Reaction
electron-transfer reactions
Half reaction
explicitly shows the electrons involved in a redox reaction
Oxidation Reaction
half-reaction that involves loss of electrons
Reduction Reaction
half-reaction that involved gain of electrons
Reducing Agent
donator of electrons
Oxidizing Agent
acceptor of electrons
Oxidation Number
number of charges the atom would have in a molecule (or an ionic compound) if electrons were transferred completely
Combination Reaction
a reaction in which two or more substances combine to form a single product
Decomposition Reaction
the breakdown of a compound into two or more components
Combustion Reaction
a reaction in which a substance reacts with oxygen, usually with the release of heat and light to produce a flame
Displacement Reaction
an ion (or atom) in a compound is replaced by an ion (or atom) of another element
Types of Displacement Reactions
hydrogen displacement, metal displacement, halogen displacement
Activity Series
a convenient summary of the results of many possible displacement reactions
Activity Series of Halogen Displacements
F2>Cl2>Br2>I2
Disproportionation Reaction
an element in one oxidation state is simultaneously oxidized and reduced
Concentration of a Solution
the amount of solute present in a given amount of solvent; or a given amount of solution
Molarity
the number of moles of solute per liter of solution
Molarity Formula
Molarity= moles of solute/liters of solution
Dilution
the procedure for preparing a less concentrated solution from a more concentrated one
Quantitative Analysis
the determination of the amount or concentration of a substance in a sample
Gravimetric Analysis
an analytical technique based on the measurement of mass
Standard Solution
a solution of accurately known concentration
Titration
a solution of accurately known concentration (standard solution) is added gradually to another solution of unknown concentration, until the chemical reaction between the two solutions is complete
Equivalence Point
the point at which the acid has completely reacted with or been neutralized by the base
Indicators
substances that have distinctly different colors in acidic and basic media