ultimate ap chem review (fiveable)

absorption

when molecules, atoms, or ions of a substance enter into the bulk phase (gas, liquid or solid) of another material

abundant

to have more than enough

balanced

state where everything is of the same size or weight; equal state

displacement

the change in position of an object

dynamic

characterized by constant change, activity, or progress

emit

to send out; to give forth, as in sound or light

inversely proportional

two variables whose product is constant

magnitude

the great size or importance of something

directly proportional

two variables whose graph is a straight line passing through the point (0,0)

qualitative

relating to, measuring, or measured by the quality of something rather than its quantity

quantitative

relating to, measuring, or measured by the quantity of something rather than its quality

spectrum

band of color; broad range of related ideas or objects

yield

to produce

activation energy

the minimum amount of energy required to start a chemical reaction

allotrope

different forms of the same element having different molecular structures

amophorous

shapeless, formless, vague

amphoteric

a substance that can act as both an acid and a base

analyte

substance analyzed or tested, generally by means of laboratory methods

arrhenius acid

a substance that increases the concentration of H3O+ in aqueous solution

arrhenius base

a substance that increases the concentration of OH- in aqueous solution

atom

the basic unit of a chemical element

atomic mass unit

a unit of mass that describes the mass of an atom or molecule

atomic radius

one-half the distance between the nuclei of two atoms of the same element when the atoms are joined

attractive force

the force by which one object attracts another

autoionization of water

pure water reacts with itself to form H3O+ and OH-

average atomic mass

the weighted average of the atomic masses of the naturally occurring isotopes of an element

avogadro's number

6.02 x 10^23

beer-lambert law

law stating that intensity of color change is directly proportional to the concentration of an analyte in a solution

bimolecular

two reactant molecules

bond energy

the energy required to break a chemical bond and form neutral isolated atoms

bond length

the average distance between the nuclei of two bonded atoms

bronsted-lowry base

a molecule or ion that is a proton acceptor

bronsted-lowry acid

a molecule or ion that is a proton donor

buffer

weak acid or base that can react with strong acids or bases to help prevent sharp, sudden changes in pH

calorimetry

measurement of heat flow out of a system for chemical and physical processes

capillary action

the attraction of the surface of a liquid to the surface of a solid

catalyst

substance that speeds up the rate of a chemical reaction; reactant then product in chemical reaction

chemical change

a change that produces matter with a different composition than the original matter

chromatography

technique used to separate the components of a mixture based on the tendency of each component to travel or be drawn across the surface of another material

collision theory

for a reaction to occur, the particles must collide with the appropriate orientation and sufficient energy

compound

substance formed by the chemical combination of two or more elements in definite proportions

conductivity

ability of an object to transfer heat or electricity to another object

conjugate acid

the particle formed when a base gains a H+ from an acid

conjugate base

the species produced when an acid donates a H+ o a base

conservation of energy

a principle stating that energy cannot be created or destroyed, but transferred

core electrons

electrons in the inner shells of an atom; not involved in forming bonds

coulomb's law

electric force between charged objects depends on the distance between the objects and the magnitude of the charges

coulomb's law equation

F\=K q₁*q₂/r²

covalent bonds

bonds created by sharing electrons with other atoms; intermolecular force

dalton's model

all matter is composed of extremely small particles called atoms; solid sphere that was uniform throughout

decomposition reaction

a reaction in which a single compound breaks down to form two or more simpler substances; AB -\> A + B

dilution

the process of adding solvent to lower the concentration of solute in a solution

dipole

a molecule that has two poles, or regions, with opposite charges

dipole moment

a property of a molecule whereby the charge distribution can be represented by a center of positive charge and a center of negative charge

dipole-dipole force

attractive forces between the positive end of one polar molecule and the negative end of another polar molecule

dipole-induced dipole

a weak attraction that results when a polar molecule induces a dipole in an atom or in a nonpolar molecule by disturbing the arrangement of electrons in the nonpolar species

distillation

the action of purifying a liquid by a process of heating and cooling

ductility

the ability of a substance to be drawn, pulled, or extruded through a small opening to produce a wire

dynamic equilibrium

condition of continuous, random movement of particles but no overall change in concentration of materials

electrochemistry

the branch of chemistry that deals with electricity-related applications of oxidation-reduction reactions

electrolytic cell

an electrochemical cell used to cause a chemical change through the application of electrical energy

electromagnetic waves

transverse waves consisting of changing electric fields and changing magnetic fields

electron configurations

the arrangement of electrons of an atom in its ground state into various orbitals around the nuclei of atoms

electronegativity

the ability of an atom to attract electrons when the atom is in a compound

electron affinity

the energy needed to remove an electron from a negative ion to form a neutral atom or molecule

electron

negatively charged particle

electrostatic

stationary electric charges or fields as opposed to electric currents

elementary steps

a series of simple reactions that represent the progress of the overall reaction at the molecular level

emission

the production and discharge of something, especially gas or radiation

empirical formula

a chemical formula showing the ratio of elements in a compound rather than the total number of atoms

endergonic

chemical reaction that requires the input of energy in order to proceed

endothermic

a chemical reaction that occurs with absorption of heat

entropy

a measure of disorder or randomness

enthalpy

the heat content of a system

equilibrium

a state in which opposing forces or influences are balanced

equilibrium constant

value that expresses how far the reaction proceeds before reaching equilibrium; small number means that equilibrium is towards the reactants side; large number means that the equilibrium is towards the product side

equivalence point

the point at which the two solutions used in a titration are present in chemically equivalent amounts

excess reactant

the substance that is not used up completely in a reaction

limiting reactant

the reactant that limits the amount of the other reactant that can combine and the amount of product that can form in a chemical reaction

exergonic

chemical reactions that release energy

exothermic

chemical reaction in which energy is primarily given off in the form of heat

faraday's law

magnitude of the induced e.m.f. is directly proportional to the rate of change of magnetic flux linkage

first order

rate is directly proportional to concentration

formal charge

number of valence electrons in an isolated atom minus the number of electrons assigned to the atom in the lewis structure; \# of v-electrons - (\# dots + \# lines)

forward rate

exchange rate at which two parties agree to exchange currencies on a specified future date

frequency

the number of complete wavelengths that pass a point in a given time

speed of light

3.00 x 10^8 m/s

speed of light formula

c\=λv

galvanic cell

a device in which chemical energy is changed to electrical energy

gibb's free energy

the energy of a system that is available to do work at a constant temperature and pressure

gravimetric analysis

an analytical technique based on the measurement of mass

half-cell reactions

oxidation or reduction reaction occurring at an electrode

half-life

length of time required for half of the radioactive atoms in a sample to decay

heat vs. temp

heat deals with thermal energy and temperature is with molecular kinetic energy

hess's law

the overall enthalpy change in a reaction is equal to the sum of enthalpy changes for the individual steps in the process

hess's law formula

H overall \= H1 + H2 + H3

heterogenous mixture

a mixture in which the composition is not uniform throughout

homogenous mixture

a mixture in which the composition is uniform throughout

hybridization

the mixing of several atomic orbitals to form the same total number of equivalent hybrid orbitals

hydrogen bonding

bonds between hydrogen atom and oxygen atom of another water molecule