Chapter 7: Stoichiometry of Chemical Reactions

reactant

chemical species that appears to the left of the arrow

product

species that appears to the right of the arrow

(g)

gas

(l)

liquid

(s)

solid

(aq)

aqueous (dissolved in water)

combination

two or more reactants combine to form a single product

decomposition

two or more products form from a single reactant

combustion

substances burns in the presence of oxygen, produces carbon dioxide and water

double displacement (metathesis, exchange)

can be precipitation reaction or molecular product, swapping of the ion pairs

single displacement

one solid metal exchanges to produce a different solid metal, hydrogen, or halogen (steals dance partner)

neutralization

specific double displacement - acid/base that results in salt and water

condensation

two molecules combine, water is released

double replacement reactions

reactions in which anions in two ionic compounds exchanges cations

hydration

water molecules remove the individual ions from an ions solid surround them so the substances dissolves

electrolyte

substances that dissolves in water to yield a solution that conducts electricity

ionization

molecular compound forms ions when it dissolves

strong electrolyte

electrolyte that dissociates completely (breaks apart completely)

weak electrolyte

exists in solution predominantly as molecules that are not ionized

dynamic chemical equilibrium

a reaction that occurs in both directions (⇌)

nonelectrolyte

substance that dissolves in water to yield a solution that does not conduct electricity

precipitate

insoluble product that separates from a solution

precipitation reaction

chemical reaction in which a precipitate forms

spectator ions

do not participate in the reaction

net ionic equation

equation that includes only the species that are involved in the reaction, spectator ions are crossed out

strong acid and strong base

strong electrolytes (dissociate completely)

arrhenius acid

ionizes in water to produce protons (H⁺)

arrhenius base

dissociates in water to produce OH⁻ ions

bronsted acid

loses a proton (negative)

bronsted base

gains a proton (positive)

monoprotic acid

one proton to donate

polyprotic acid

more than one acidic hydrogen atom

diprotic acid

two acidic hydrogen atoms

oxidation reduction (RedOx)

chemical reaction in which electrons are transferred from one reactant to another

oxidation

the loss of electrons

reduction

the gain of electrons

reducing agent

compound that contains the eliminats/ ions that is oxidized

oxidizing agent

compound that contains the elements/ ions that is reduced

oxidation number more positive

lost electrons, oxidized

oxidation number more negative

gained electrons, reduced