Chapter Four
Chemistry 1035 with Merola at Virginia Polytechnic Institute and State University
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By: Ruth Anderson
Created: 2012-03-22
Size: 28 flashcards
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Created: 2012-03-22
Size: 28 flashcards
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polar molecule
A molecule with an unequal distribution of charge as a result of its polar bonds and shape.
solvated
Surrounded closely by solvent molecules.
electrolyte
A substance that conducts a current when it dissolves in water. A mixture of ions, in which the electrodes of an electrochemical cell are immersed, that conducts a current.
nonelectrolyte
A substance whose aqueous solution does not conduct an electric current.
molecular equation
A chemical equation showing a reaction in solution in which reactants and products appear as intact, undissociated compounds.
total ionic equation
A chemical equation for an aqueous reaction that shows all the soluble ionic substances dissociated into ions.
spectator ion
An ion that is present as part of a reactant but is not involved in the chemical change.
net ionic equation
A chemical equation of a reaction in solution in which spectator ions have been omitted to show the actual chemical change.
precipitation reaction
A reaction in which two soluble ionic compounds form an insoluble product, a precipitate.
precipitate
The insoluble product of a precipitation reaction.
metathesis reaction
A reaction in which atoms or ions of two compounds exchange bonding partners.
acid-base reaction
Any reaction between an acid and a base.
neutralization reaction
An acid-base reaction that yields water and a solution of a salt; when a strong acid reacts with a stoichiometrically equivalent amount of a strong base, the solution is neutral.
acid
In common laboratory terms, any species that produces H+ ions when dissolved in water.
base
In common laboratory terms, any species that produces OH- ions when dissolved in water.
salt
An ionic compound that results from a classical acid-base reaction.
titration
A method of determining the concentration of a solution by monitoring its reaction with a solution of known concentration.
equivalence point
The point in a titration when the number of moles of the added species is stoichiometrically equivalent to the original number of moles of the other species.
end point
The point in a titration at which the indicator changes color.
oxidation-reduction reaction
A process in which there is a net movement of electrons from one reactant (reducing agent) to another (oxidizing agent).
oxidation
The loss of electrons by a species, accompanied by an increase in oxidation number.
reduction
The gain of electrons by a species, accompanied by a decrease in oxidation number.
oxidizing agent
The substance that accepts electrons in a reaction and undergoes a decrease in oxidation number.
reducing agent
The substance that donates electrons in a redox reaction and undergoes an increase in oxidation number.
oxidation number (O.N.)
A number equal to the magnitude of the charge an atom would have if its shared electrons were held completely by the atom that attracts them more strongly.
oxidation number method
A method for balancing redox reactions in which the change in oxidation numbers is used to determine the balancing coefficients.
activity series of the metals
A listing of metals arranged in order of decreasing strength of the metal as a reducing agent in aqueous reactions.
dynamic equilibrium
The condition at which the forward and reverse reactions are taking place at the same rate, so there is no net change in the amounts of reactants or products.
About this deck
By: Ruth Anderson
Created: 2012-03-22
Size: 28 flashcards
Views: 0
Created: 2012-03-22
Size: 28 flashcards
Views: 0
About StudyBlue
STUDYBLUE makes things that make you better at school.
Things like online flashcards with photos and audio.
Things like personalized quizzes and friendly reminders about when (and what) to study next.
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