Chemistry - Salt, molecules, acids, and bases

Salts

Ionic (contains metal and nonmetal or a polyatomic ion)

Molecules

Covalent (contains only nonmetals and no polyatomic ions)

Acids

begins with “H”

Bases

Ends with “OH”

Naming acids - no polyatomic

hydro prefix, ends with ic

Naming acids - polyatomic (oxyacids)

no hydro prefix, ate becomes ic, ite becomes ous

solution

a homogeneous mixture made up of a solute and solvent.

solute

substance being dissolved

solvent

substance dissolving

Aqueous solution

solutions in which water is the solvent

Electrical conductivity

the ability of a solution to conduct electricity

Strong electrolytes

conduct current very efficiently

Weak electrolytes

conduct only a small current

Nonelectrolytes

no current flows

solubility

the maximum concentration of a solute that can be achieved in a particular solvent under given conditions

saturated

Solvent holds as much solute as is possible at that temperature. Dissolved solute is in dynamic equilibrium with solid solute particles (some may dissolve and some may precipitate out at the same time)

unsaturated

Less than the maximum amount of solute for that temperature is dissolved in the solvent

supersaturated

Solvent holds more solute than is normally possible at that temperature. These solutions are unstable; crystallization can usually be stimulated by adding a “seed crystal” or scratching the side of the flask

Concentrated solutions

contain large amounts of solutes dissolved in the solvent

Dilute solutions

contain small amounts of solute dissolved in solvent

Standard solution

whose concentration is accurately known.

Stock Solution

Solutions in concentrated forms (used for dilutions of different concentrations)

Dilution

The process of adding water to stock solutions to attain desired concentration (Less concentrated solution)

precipitation reaction

A double displacement reaction in which a solid forms and separates from the solution.

Precipitate

the solid that forms.

Soluble

solid dissolves in solution;  (aq) is used in the reaction.

Insoluble

solid does not dissolve in solution; (s) is used in reaction

Molecular equation

shows the compounds that are reacting

Spectator ions

don’t participate in the reaction (stays the same before and after reaction)

Complete ionic equation

Represents as ions all reactants and products that are strong electrolytes

Net Ionic Equation

Includes only those solution components undergoing a change. Show only components that actually react . Spectator ions are not included (ions that do not participate directly in the reaction).

Neutralization reaction

An acid-base reaction

Redox Reactions

Reactions in which one or more electrons are transferred

Oxidation States

Provide a way to keep track of electrons in oxidation-reduction reactions (especially those with covalent substances)

Oxidation

increase in oxidation state (loss of electrons); reducing agent

Reduction

decrease in oxidation state (gain of electrons); oxidizing agent

molarity

moles/liters

dilution formula

m1v1=m2v2

equivalence point

the point in a neutralization reaction where the number of moles of hydrogen ions is equal to the number of moles of hydroxide ions

titration

an experiment where a volume of a solution of known concentration is added to a volume of another solution in order to determine its concentration

indicator

a substance that has a distinctly different color when in an acidic or basic solution

standard solution

the solution in a titration whose concentration is known.

end point

the point at which the indicator changes color

arrhenius acid

a compound, which ionizes to yield hydrogen ions (H+) in aqueous solution

monoprotic acid

an acid that contains only one ionizable hydrogen

polyprotic acid

an acid that contains multiple ionizable hydrogens

Arrhenius base

a compound, which ionizes to yield hydroxide ions (OH−) in aqueous solution