a substance that produces hydrogen ions in solution; a proton donor
Back
Alkali metal
Front
a Group 1A metal
Back
Alloy
Front
a substance that contains a mixture of elements and has metallic properties
Back
Activation energy
Front
the threshold energy that must be overcome to produce a chemical reaction
Back
Amorphous solid
Front
a solid with considerable disorder in its structure
Back
Amine
Front
an organic base derived from ammonia in which one or more of the hydrogen atoms are replaced by organic groups
Back
Acid dissociation constant (Ka)
Front
the equilibrium constant for a reaction in which a proton is removed from an acid by H2O to form the conjugate base and H3O+
Back
Alloy steel
Front
a form of steel containing carbon plus other metals such as chromium, cobalt, manganese, and molybdenum
Back
Aqueous solution
Front
a solution in which water is the dissolving medium or solvent
Back
Antibonding molecular orbital
Front
an orbiting higher in energy than the atomic orbitals of which it is composed
Back
Alkyne
Front
an unsaturated hydrocarbon containinga triple carbon-carbon bond. The general formula is C(n)H(2n-2)
Back
Alkane
Front
a saturated hydrocarbon with the general formula C(n)H(2n+2)
Back
α-Amino acid
Front
an organic acid in which an amino group and an R group are attached to the carbon atom next to the carboxyl group
Back
Atomic radius
Front
half the distance between thenuclei in a molecule consisting of identical atoms
Back
Alpha (α) particle
Front
a helium nucleus
Back
Addition reaction
Front
a reaction in which atoms add to a carbon-carbon multiple bond
Back
Alkene
Front
an unsaturated hydrocarbon containing a carbon-carbon double bond. The general formula is C(n)H(2n)
Back
Barometer
Front
a device for measuring atmospheric pressure
Back
Alkaline earth metal
Front
a Group 2A metal
Back
Alpha-particle production
Front
a common mode of decay for radio-active nuclides in which the mass number changes
Back
Aufbau principle
Front
the principle stating that as protons are added one by one to the nucleus to build up the elements, electrons are similarly added to hydrogen-like orbitals
Back
Atomic weight
Front
the weighted average mass of the atoms in a naturally occuring element
Back
Aromatic hydrocarbon
Front
one of a special class of cyclic unsaturated hydrocarbons, the simplest of which is benzene
Back
Adsorption
Front
the collection of one substance on the surface of another
Back
Base
Front
a substance that produces hydroxide ions in aqueous solution, a proton acceptor
Back
Ampere
Front
the unit of electric current equal to one coulomb of charge per second
Back
Atomic number
Front
the number of protons in the nucleus of an atom
Back
Actinide series
Front
a group of 14 elements following actinium in the periodic table, in which the 5f orbitals are being filled
Back
Aldehyde
Front
an organic compound containing the carbonyl group bonded to at least one hydrogen atom
Back
Arrhenius concept
Front
a concept postulating that acids produce hydrogen ions in aqueous solution, while bases produce hydroxide ions
Back
Acid rain
Front
a result of air pollution by sulfur dioxide
Back
Ball-and-stick model
Front
a molecular model that distorts the sizes of atoms but shows bond relationships clearly
Back
Avogadro's number
Front
the number of atoms in exactly 12 grams of pure ^(12)C, equal to 6.022 x 10^(23)
Back
Alcohol
Front
an organic compound in which the hydroxyl group is a substituent on a hydrocarbon
Back
Amphoteric substance
Front
a substance that can behave either as an acid or as a base
Back
Acidic oxide
Front
a covalent oxide that dissolves in water to give an acidic solution
Back
Arrhenius equation
Front
the equation representing the rate constant as k = Ae^[-(E[a])/(RT)], where A represents the product of the collision frequency and the steric factor, and e^[-(E[a])/(RT)] is the fraction of collisions with sufficient energy to product a reaction
Back
Anode
Front
the electrode in a galvanic cell at which oxidation occurs
Back
Accuracy
Front
the agreement of a particular value with a true value
Back
Atmosphere
Front
the mixture of gases that surrounds the earth's surfaces
Back
Air pollution
Front
contamination of the atmosphere, mainly by the gaseous products of transportation and production of electricity
Back
Band model
Front
a molecular model for metals in which the electrons are assumed to travel around the metal crystal in molecular orbitals formed from the valence atomic orbitals of the metal atoms
Back
Autoionization
Front
the transfer of a proton from one molecule to another of the same substance
Back
Anion
Front
a negative ion
Back
Acid-base indicator
Front
a substance that marks the end point of an acid-base titration by changing color
Back
Angular momentum quantum number (ℓ)
Front
the quantumnumber relating to the shape of an atomicorbital, which can assume any integral value from 0 to 'n-1' for each value of 'n'
Back
Avogadro's law
Front
equal volumes of gases at the same temperature and pressure contain the same number of particles
Back
Activated complex (transition state)
Front
the arrangement of atoms found at the tope of the potential energy barrier as a reaction proceeds from reactants to products
Back
Addition polymerization
Front
a type of polymerization in which the monomers simply add together to form the polymer, with no other products
Back
Section 2
(50 cards)
compound
Front
substance with constant composition that can be broken down into elements by chemical processes
Back
Cathode
Front
the electrode in a galvanic cell at which reduction occurs
Back
Beta (β) particle
Front
an electron produced in radioactivedecay
Back
Buffering capacity
Front
the ability of a buffered solution to absorb protons or hydroxide ions without a significant change in pH; determined by the magnitudes of [HA] and [A-] in the solution
Back
Carboxylic acid
Front
an organic compound containing the carboxyl group; an acid with the general formula RCOOH
Back
Chemical bond
Front
the force or, more accurately, the energy, that holds two atoms together in a compound
Back
Boyle's law
Front
the volume of a given sample of gas at constant temperature varies inversely with the pressure
Back
common ion effect
Front
shift in equilibrium position caused by addition or presence of ion involved in equilibrium reaction
Back
Carboxyl group
Front
the -COOH group in an organic acid
Back
colligative properties
Front
properties of solution that depend only on the number, and not on the identity, of the solute particles
Back
complete ionic equation
Front
equation that shows all substances that are strong electrolytes as ions
Back
Chromatography
Front
the general name for a series of methods for separating mixtures by employing a system with a mobile phase and a stationary phase
Back
Bond energy
Front
the energy required to break a given chemical bond
Back
Charles' law
Front
the volume of a given sample of gas at constant pressure is directly proportional to the temperature in kelvins
Back
Bond length
Front
the distance between the nuclei of the two atoms connected by a bond; the distance where the total energy of a diatomic molecule is minimal
Back
Bonding molecular orbital
Front
an orbital lower in energy than the atomic orbitals or which it is composed
Back
Bonding pair
Front
an electron pair found in the space between two atoms
Back
complex ion
Front
charged species consisting of metal ion surrounded by ligands
Back
Calorimetry
Front
the science of measuring heat flow
Back
Basic oxide
Front
an ionic oxide that dissolves in water to produce a basic solution
Back
Bimolecular step
Front
a reaction involving the collision of two molecules
Back
Bond order
Front
the difference between the number of bonding electrons and the number of antibonding electrons, divided by two. It is an index of bond strength
Back
Carbohydrate
Front
a polyhydroxyl ketone or polyhydroxyl aldehyde or a polymer composed of these
Back
Basic oxygen process
Front
a process for producing steel by oxidizing and removing the impurities in iron using a high-pressure blast of oxygen
Back
Brønsted-Lowry model
Front
a model proposing that an acid is a proton donor, and a base is a proton acceptor
Back
Biomolecule
Front
a molecule responsible for maintaining and/or reproducing life
Back
Borane
Front
a covalent hydride of boron
Back
Buffered solution
Front
a solution that resists a changein its pH when either hydroxide ions or protons are added
Back
collision model
Front
model based on idea that molecules must collide to react; used to account for the observed characteristics of reaction rates
Back
Carbon steel
Front
an alloy of iron containing up to about 1.5% carbon
Back
Chemical kinetics
Front
the area of chemistry that concerns reaction rates
Back
Chemical stoichiometry
Front
the calculation of the quantities of material consumed and produced in chemical reactions
Back
Cell potential (electromotive force)
Front
the driving force in a galvanic cell that pulls electrons from the reducing agent in one compartment to the oxidizing agent in the other
Back
Chemical formula
Front
the representation of a molecule in which the symbols for the elements areused to indicate the types of atoms present and subscripts are used to show the relative numbers of atoms
Back
Bidentate ligand
Front
a ligand that can form two bonds to a metal ion
Back
combustion reaction
Front
vigorous and exothermic reaction that takes place between certain substances, particularly organic compounds, and oxygen
Back
Binding energy (nuclear)
Front
the energy required to decompose a nucleus into its component nucleus
Back
Beta-particle production
Front
a decay process for radioactive nuclides in which the mass number remains constant and the atomic number changes. The net effect is to change a neutron to a proton
Back
Cation
Front
a positive ion
Back
Binary compound
Front
a two-element compound
Back
Chemical change
Front
the change of substances into other substances through a reorginzation of the atoms; a chemical reaction
Back
Battery
Front
a group of galvanic cells connected in series
Back
Chemical equilibrium
Front
a dynamic reaction system in which the concentrations of all reactants and products remain constant as a function of time
Back
Chain reaction (nuclear)
Front
a self-sustaining fission process caused by the production or neutrons that proceed to split other nuclei
Back
Chemical equation
Front
a representation of a chemical reaction showing the relative numbers of reactant and product molecules
Back
Capillary action
Front
the spontaneous rising of a liquid in a narrow tube
Back
Chelating ligand (chelate)
Front
a ligand having more than one atom with a long pair that can be used to bond to a metal ion
Back
coagulation
Front
destruction of colloid by causing particles to aggregate and settle out
Back
Catalyst
Front
a substance that speeds up a reaction without being consumed
Back
Cathode rays
Front
the "rays" emanating from the negative electrode (cathode) in a partially evacuated tube; a stream of electrons
Back
Section 3
(50 cards)
covalent bonding
Front
type of bonding in which electrons are shared by atoms
Back
dipole-dipole attraction
Front
attractive force resulting when polar molecules line up so that the positive and negative ends are close to each other
Back
concentration cell
Front
galvanic cell in which both compartments contain the same components, but at different concentrations
Back
electromagnetic radiation
Front
radiant energy that exhibits wavelike behavior and travels through space at the speed of light in a vacuum
Back
electron spin quantum number
Front
a quantum number representing one of the two possible values for the electron spin; either +(1/2) or -(1/2)
Back
electrolyte
Front
material that dissolves in water to give a solution that conducts an electric current
Back
Coulomb's Law
Front
E= 2.31 x 10^-19 (Q1Q2/r), where E is the energy of interaction between a pair of ions, expressed in joules; r is the distance between the ion centers in nm; and Q1 and Q2 are the numerical ion charges
Back
condensed states of matter
Front
liquids and solids
Back
core electron
Front
inner electron in an atom
Back
electrical conductivity
Front
ability to conduct an electric current
Back
coordination compound
Front
compound composed of complex ion and counter ions sufficient to give no net charge
Back
corrosion
Front
process by which metals are oxidized in the atmosphere
Back
condensation polymerization
Front
type of polymerization in which the formation of a small molecule, such as water, accompanies the extension of the polymer chain
Back
coordination number
Front
number of bonds formed between the metal ion and the ligands in a complex ion
Back
diffusion
Front
mixing of gases
Back
conjugate acid-base pair
Front
two species related to each other by the donating and accepting of a single proton
Back
continuous spectrum
Front
spectrum that exhibits all the wavelengths of visible light
Back
dry cell battery
Front
common battery used in calculators, watches, radios, and tape players
Back
density
Front
property of matter representing the mass per unit volume
Back
electron affinity
Front
the energy change associated with the addition of an electron to a gaseous atom
Back
dimer
Front
molecule formed by the joining of two identical monomers
Back
critical temperature
Front
temperature above which vapor cannot be liquefied no matter what pressure is applied
Back
coordinate covalent bond
Front
metal-ligand bond resulting from the interaction of a lewis base (ligand) and a lewis acid (metal ion)
Back
electrochemistry
Front
study of the interchange of chemical and electrical energy
Back
dilution
Front
process of adding solvent to lower the concentration of solute in a solution
Back
deoxyribonucleic acid (DNA)
Front
huge nucleotide polymer having a double-helical structure with complementary bases on the two strands. its major functions are protein synthesis and the storage and transport of genetic information
Back
diamagnetism
Front
type of magnetism, associated with paired electrons, that causes a substance to be repelled from the inducing magnetic field
Back
conjugate base
Front
what remains of an acid molecule after a proton is lost
Back
electronegativitiy
Front
the tendency of an atom in a molecule to attract shared electrons to itself
Back
dialysis
Front
phenomenon in which a semipermeable membrane allows transfer of both solvent molecules and small solute molecules and ions
Back
electrolysis
Front
process that involves forcing a current through a cell to cause a nonspontaneous chemical reaction to occur
Back
desalination
Front
removal of dissolved salts from an aqueous solution
Back
effusion
Front
passage of a gas through a tiny orifice into an evacuated chamber
Back
condensation
Front
process by which vapor molecules reform a liquid
Back
conjugate acid
Front
species formed when proton is added to base
Back
control rods
Front
rods in nuclear reactor composed of substances that absorb neutrons. these rods regulate the power level of the reactor
Back
electron
Front
a negatively charged particle that moves around the nucleus of an atom
Back
distillation
Front
method for separating the components of a liquid mixture that depends on differences in the ease of vaporization of the components
Back
crystalline solid
Front
solid with a regular arrangement of its components
Back
condensation reaction
Front
reaction in which two molecules are joined, accompanied by the elimination of a water molecule
Back
counterions
Front
anions or cations that balance the charge on the complex ion in a coordination compound
Back
differential rate law
Front
expression that gives the rate of a reaction as a function of concentrations; often called rate law
Back
coordination isomerism
Front
isomerism in coordination compound in which the composition of the coordination sphere of a metal ion varies
Back
critical mass
Front
mass of fissionable material required to produce a self-sustaining chain reaction
Back
electrolytic cell
Front
cell that uses electrical energy to produce a chemical change that would otherwise not occur spontaneously
Back
degenerate orbitals
Front
group of orbitals with the same energy
Back
dipole moment
Front
property of a molecule whose charge distribution can be represented by a center of positive charge and a center of negative charge
Back
double bond
Front
bond in which two pairs of electrons are shared by two atoms
Back
critical point
Front
point on a phase diagram at which the temperature and pressure have their critical values; the end point of the liquid-vapor line
Back
Dalton's law of partial pressures
Front
for a mixture of gases in a container, the total pressure exerted is the sum of the pressures that each gas would exert if it were alone
Back
Section 4
(50 cards)
element
Front
a substance that cannot be decomposed into simpler substances by chemical or physical means
Back
equilibrium position
Front
particular set of equilibrium concentrations
Back
entropy
Front
a thermodynamic function that measures randomness or disorder
Back
half-life (of a radioactive sample)
Front
time required for the number of nuclides in a radioactive sample to reach half of the original value
Back
hess's law
Front
in going from a particular set of reactants to a particular set of products, the enthalpy change is the same whether the reaction takes place in one step or in a series of steps
Back
heterogeneous equilibrium
Front
equilibrium involving reactants and/or products in more than one phase
Back
fossil fuel
Front
coal, petroleum, or natural gas; consists of carbon-based molecules derived from decomposition of once-living organisms
Back
geometrical (cis-trans) isomerism
Front
isomerism in which atoms or groups of atoms can assume different positions around a rigid ring or bond
Back
half-life (of a reactant)
Front
time required for a reactant to reach half of its original concentration
Back
fission
Front
process of using a neuron to split a heavy nucleus into two nuclei with smaller mass numbers
Back
ester
Front
an organic compound produced by the reaction between a carboxylic acid and an alcohol
Back
equilibrium constant
Front
value obtained when equilibrium concentrations of the chemical species are substituted in the equilibrium expression
Back
endpoint
Front
point in a titration at which the indicator changes color
Back
galvanizing
Front
process in which steel is coated with zinc to prevent corrosion
Back
equilibrium point
Front
position where the free energy of a reaction system has its lowest possible value
Back
heat
Front
energy transferred between two objects due to a temperature difference between them
Back
heat of vaporization
Front
energy required to vaporize one mole of a liquid at a pressure of one atmosphere
Back
elementary step
Front
a reaction whose rate law can be written from its molecularity
Back
electron capture
Front
a process in which one of the inner-orbital electrons in an atom is captured by the nucleus
Back
fuel cell
Front
galvanic cell for which the reactants are continuously supplied
Back
glass electrode
Front
electrode for measuring pH from the potential difference that develops when it is dipped into an aqueous solution containing H+ ions
Back
equivalence point (stoichiometric point)
Front
point in a titration when enough titrant has been added to react exactly with the substance in solution being titrated
Back
enzyme
Front
a large molecule, usually a protein, that catalyzes biological reactions
Back
Graham's law of effusion
Front
rate of effusion of a gas is inversely proportional to the square root of the mass of its particles
Back
half-reactions
Front
two parts of an oxidation-reduction reaction, one representing oxidation, the other reduction
Back
halogen
Front
Group 7A element
Back
heisenberg uncertainty principle
Front
a principal stating that there is a fundamental limitation to how precisely both the position and momentum of a particle can be known at a given time
Back
empirical formula
Front
simplest whole number ratio of atoms in a compound
Back
ground state
Front
lowest possible energy state of an atom or molecule
Back
functional group
Front
atom or group of atoms in hydrocarbon derivatives that contains elements in addition to carbon and hydrogen
Back
enthalpy
Front
property of a system equal to E+PV, where E is the internal energy of the system, P is the pressure of the system, and V is the volume of the system
Back
free energy
Front
thermodynamic function equal to the enthalpy (H) minus the product of the entropy (S) and the Kelvin temperature (T); G=H-TS
Back
heat of fusion
Front
enthalpy change that occurs to melt a solid at its melting point
Back
endothermic
Front
refers to a reaction where energy (as heat) flows into the system
Back
energy
Front
the capacity to do work or to cause heat flow
Back
henry's law
Front
amount of a gas dissolved in a solution is directly proportional to the pressure of the gas above the solution
Back
heating curve
Front
plot of temperature vs. time for a substance where energy is added at a constant rate
Back
gamma (γ) ray
Front
high-energy photon
Back
filtration
Front
method for separating the components of a mixture containing a solid and a liquid
Back
exothermic
Front
reaction where energy (as heat) flows out of the system
Back
frequency
Front
number of waves (cycles) per second that pass a given point in space
Back
faraday
Front
constant representing the charge on one mole of electrons; 96,485 coulombs
Back
fusion
Front
process of combining two light nuclei to form a heavier, more stable nucleus
Back
equilibrium expression
Front
the expression obtained by multiplying the product concentrations and dividing by the multiplied reactant concentrations, with each concentration raised to a power represented by the coefficient in the balanced equation
Back
galvanic cell
Front
device in which chemical energy from a spontaneous redox reaction is changed to electrical energy that can be used to do work
Back
heat capacity
Front
amount of energy required to raise the temperature of an object by one degree Celsius
Back
homogeneous equilibrium
Front
equilibrium system where all reactants and products are in the same phase
Back
first law of thermodynamics
Front
energy of the universe is constant
Back
enthalpy (heat) of fusion
Front
the enthalpy change that occurs to melt a solid at its melting point
Back
group (of the periodic table)
Front
vertical column of elements having the same valence electron configuration and showing similar properties
Back
Section 5
(45 cards)
ligand
Front
neutral molecule or ion having a lone pair of electrons that can be used to form a bond to a metal ion; a lewis base
Back
hybridization
Front
mixing of the native orbitals on a given atom to form special atomic orbitals for bonding
Back
isomers
Front
species with the same formula but different properties
Back
lanthanide series
Front
group of 14 elements following lanthium in the periodic table in which the 4f orbitals are being filled
Back
kinetic energy
Front
(1/2mv^2) energy due to the motion of an object; dependent on the mass of the object and the square of its velocity
Back
ideal gas law
Front
equation of state for a gas, where the state of the gas is its condition at a given time; expressed by PV=nRT, where P is pressure, V is volume, n is moles of the gas, R is the universal gas constant, and T is absolute temperature
Back
hypothesis
Front
one or more assumptions put forth to explain the observed behavior of nature
Back
hydrogen bonding
Front
unusually strong dipole-dipole attractions that occur among molecules in which hydrogen is bonded to a highly electronegative atom
Back
hydrocarbon
Front
compound composed of carbon and hydrogen
Back
ionic solid (salt)
Front
solid containing cations and anions that dissolves in water to give a solution containing the separated ions which are mobile and thus free to conduct electrical current
Back
hund's rule
Front
lowest energy configuration for an atom is the one having the maximum number of unpaired electrons allowed by the Pauli exclusion principle in a particular set of degenerate orbitals, with all unpaired electrons having parallel spins
Back
lewis base
Front
electron pair donor
Back
lattice energy
Front
energy change occuring when separated gaseous ions are packed together to form ionic solid
Back
law of definite proportion
Front
given compound always contains exactly the same proportion of elements by mass
Back
lone pair
Front
an electron pair that is localized on a given atom; an electron pair not involved in bonding
Back
isoelectronic ions
Front
ions containing the same number of electrons
Back
law of multiple proportions
Front
when two elements form a series of compounds, the ratios of the masses of the second element that combine with one gram of the first element can always be reduced to small whole numbers
Back
intermolecular forces
Front
relatively weak interactions that occur between molecules
Back
le chatelier's principle
Front
if a change is imposed on a system at equilibrium, the position of the equilibrium will shift in a direction that tends to reduce the effect of that change
Back
law of mass action
Front
general description of the equilibrium condition
Back
intermediate
Front
species that is neither a reactant nor a product but that is formed and consumed in the reaction sequence
Back
lattice
Front
3D system of points designating the positions of the centers of the components of a solid
Back
ion
Front
atom or group of atoms that has a net positive or negative charge
Back
indicator
Front
chemical that changes color and is used to mark the end point of a titration
Back
ionic compound (binary)
Front
compound that results when a metal reacts with a nonmetal to form a cation and an anion
Back
lewis structure
Front
diagram of a molecule showing how the valence electrons are arranged among the atoms in the molecule
Back
ionic bonding
Front
electrostatic attraction between oppositely charged ions
Back
ketone
Front
organic compound containing the carboxyl group bonded to two carbon atoms
Back
isotopes
Front
atoms of the same element with different numbers of neutrons
Back
kinetic molecular theory (KMT)
Front
model that assumes that an ideal gas is composed of tiny particles (molecules) in constant motion
Back
internal energy
Front
property of system that can be changed by a flow of work, heat, or both; ΔE= q+w, where ΔE is the change in the internal energy of the system, q is heat, and w is work
Back
hydride
Front
binary compound containing hydrogen
Back
limiting reactant (limiting reagent)
Front
reactant that is completely consumed when a reaction is run to completion
Back
hydronium ion
Front
the H3O+ ion; a hydrated proton
Back
hybrid orbitals
Front
set of atomic orbitals adopted by an atom in a molecule different from those of the atom in the free state
Back
law of conservation of mass
Front
mass is neither created nor destroyed
Back
integrated rate law
Front
expression that shows concentration of reactant as function of time
Back
law of conservation of energy
Front
energy can be converted from one form to another but can be neither created nor destroyed
Back
hydration
Front
interaction between solute particles and water molecules
Back
london dispersion forces
Front
forces, existing among noble gas atoms and nonpolar molecules, that involve an accidental dipole that induces a momentary dipole in a neighbor
Back
lewis acid
Front
electron pair acceptor
Back
ion- product (dissociation) constant (Kw)
Front
equilibrium constant for the auto-ionization of water; Kw= [H+][OH-]. at 25°C, Kw equals 1.0x10^-14
Back
ideal solution
Front
solution whose vapor pressure is directly proportional to the mole fraction of solvent present
Back
localized electron (LE) model
Front
model which assumes that a molecule is composed of atoms that are bound together by sharing pairs of electrons using the atomic orbitals of the bound atoms
Back
line spectrum
Front
spectrum showing only certain discrete wavelengths