Download Chemistry Terms: Solutions, Electrolytes, Acids, Bases, and Reactions and more Quizzes Physical Chemistry in PDF only on Docsity!
solution
a homogeneous mixture if two or more substances*may be gaseous, solid, or liquid TERM 2
solvent
DEFINITION 2 a liquid in which a solute is dissolved to form a solutionusually the substance present in the largest amountwater* TERM 3
solute
DEFINITION 3 the minor component in a solution, dissolved by the solvent TERM 4
electrolyte
DEFINITION 4 a substance that dissolves in water to yield a solution that conducts electricity TERM 5
non electrolyte
DEFINITION 5 a substance that dissolves in water to yield a solution that does notconduct electricity*think non-electric
what is the difference between an aqueous
solution that conducts electricity and one that
does not?
the presence or absence of ions*it is the presence of ions that allows the solution of sodium chloride to conduct electricity sodium chloride is an electrolyte sucrose is a non-electrolyte NaCl (s) --H2O--> Na+ (aq) + Cl- (aq) TERM 7
dissociation
DEFINITION 7 the process by which an ionic compound, upon dissolution, breaks apart into its constituent ions TERM 8
ionization
DEFINITION 8 the process by which a molecular compound forms ions when it dissolves TERM 9
acids
DEFINITION 9 compounds that dissolve in water to produce hydrogen ions (H+)*Ex. Hydrochloric acid ionizes to produce hydrogen ion and chloride ions.HCL (g) --H2O--> H+ (aq) + Cl- (aq) TERM 10
base
DEFINITION 10 compound that dissolves in water to produce hydrooxide ions (OH-)*Ex. Ammonia ionizes in water to produce ammonium and hydroxide ions.NH3 (g) + H2O (l) <==> NH4+ (aq) + OH- (aq)
precipitation reaction
a chemical reaction in which the precipitate forms*usually involve ionic compounds, but a precipitate does not form every time two electrolytes are combined TERM 17
hydration
DEFINITION 17 when an ionic substance (ex. sodium chloride) dissolves in water, the water molecules remove individual ions from the three-dimensional solid structure and surround them TERM 18
polar molecules
DEFINITION 18 Amoleculewith a netdipoleas a result of the opposing charges (ex. having partial positive and partial negative charges) frompolarbonds arranged asymmetrically*H2O (neg. charge on O, pos. charge on H) TERM 19
solubility
DEFINITION 19 maximum amount of solute that will dissolve in a given quantity of solvent at a specific temperature*not all ionic compounds dissolve in water TERM 20
what does solubility depend on?
DEFINITION 20 depends on relative magnitudes of water molecules' attraction to the ions, and the ions' attraction for each other if water molecules' attraction for the ions exceeds the ions' attraction to one another, will dissolve if ions' attraction to each other exceeds water molecules' attraction to the ions, will not dissolve
double replacement reactions
reactions in which compounds exchange ions*Ex. Pb(NO3) (aq) + 2NaI (aq) ----> 2NaNO3 (aq) + PbI2 (s) TERM 22
molecular equation
DEFINITION 22 a chemical equation written with all compounds represented by their chemical formulas TERM 23
how do you determine if a precipitate will
form during a reaction?
DEFINITION 23 we do this by using the solubility guidelines for ionic compoundsTable 4.2 and 4. TERM 24
ionic equation
DEFINITION 24 a chemical equation in which any compound that exists completely or predominately as ions in solution is represented by those ions. species that are insoluble or that exist in the solution completely or predominately as molecules are represented by their chemical formulas (like they were in molecular equation) TERM 25
spectator ions
DEFINITION 25 ions that appear on both sides of the equation arrow called spectator ions because they do not participate in the reaction cancel one another out, so you do not need to show spectator ions in chemical equations
