From Ms Hartman's list; definitions from our textbook website @ http://college.cengage.com/chemistry/general/zumdahl/chemistry/6e/students/protected/glossary/index.html
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| 163837514 | activated complex | (transition state) the arrangement of atoms found at the top of the potential energy barrier as a reaction proceeds from reactants to products. (12.7) | |
| 163837515 | actinide series | a group of 14 elements following actinium in the periodic table, in which the 5f orbitals are being filled. (7.11; 19.1) | |
| 163837516 | adsorption | the collection of one substance on the surface of another. (12.8) | |
| 163837517 | alpha particle | a helium nucleus. (18.1) | |
| 163837518 | amine | an organic base derived from ammonia in which one or more of the hydrogen atoms are replaced by organic groups. (14.6; 22.4) | |
| 163837519 | amorphous solid | a solid with considerable disorder in its structure. (10.3) | |
| 163837520 | amphoteric | can behave either as an acid or as a base. (14.2) | |
| 163837521 | Aufbau principle | 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. (7.11) | |
| 163837522 | Hund's Rule | the 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. (7.11) | |
| 163837523 | azimuthal quantum number (l) | a quantum number for an atomic orbital that determines its orbital angular momentum and describes the shape of the orbital; s, p, d, or f | |
| 163837524 | beta particle | an electron produced in radioactive decay. (18.1) | |
| 163837525 | buffer capacity | 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. (15.3) | |
| 163837526 | cathodic protection | a method in which an active metal, such as magnesium, is connected to steel to protect it from corrosion. (17.6) | |
| 163837527 | chain reaction (nuclear) | a self-sustaining fission process caused by the production of neutrons that proceed to split other nuclei. (18.6) | |
| 163837528 | chromatography | the general name for a series of methods for separating mixtures by employing a system with a mobile phase and a stationary phase. (1.9) | |
| 163837529 | coagulation | the destruction of a colloid by causing particles to aggregate and settle out. (11.8) | |
| 163837530 | colligative properties | properties of a solution that depend only on the number, and not on the identity, of the solute particles. (11.5) | |
| 163837531 | colloid | (colloidal dispersion) a suspension of particles in a dispersing medium. (11.8) | |
| 163837532 | common ion effect | the shift in an equilibrium position caused by the addition or presence of an ion involved in the equilibrium reaction. (15.1) | |
| 163837533 | concentration cell | a galvanic cell in which both compartments contain the same components, but at different concentrations. (17.4) | |
| 163837534 | conjugate acid | the species formed when a proton is added to a base. (14.1) | |
| 163837535 | conjugate base | what remains of an acid molecule after a proton is lost. (14.1) | |
| 163837536 | coordination compound | a compound composed of a complex ion and counter ions sufficient to give no net charge. (21.3) | |
| 163837537 | core electron | an inner electron in an atom; one not in the outermost (valence) principal quantum level. (7.11) | |
| 163837538 | Coulombs' Law | E = (2.31x10E-19 Jxnm) Q1Q2/r^2 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 Q 1 and Q 2 are the numerical ion charges. (8.1) | |
| 163837539 | covalent bonding | a type of bonding in which electrons are shared by atoms. (2.6; 8.1) | |
| 163837540 | critical point | the point on a phase diagram at which the temperature and pressure have their critical values; the end point of the liquid-vapor line. (10.9) | |
| 163837541 | delocalization | electrons in a molecule or solid metal that are not associated with a single atom or one covalent bond | |
| 163837542 | dialysis | a phenomenon in which a semipermeable membrane allows transfer of both solvent molecules and small solute molecules and ions. (11.6) | |
| 163837543 | diffusion | the mixing of gases. (5.7) | |
| 163837544 | dipole moment | a property of a molecule whose charge distribution can be represented by a center of positive charge and a center of negative charge. (8.3) | |
| 163837545 | effective nuclear charge | the net positive charge experienced by an electron in a multi-electron atom. The term "effective" is used because the shielding effect of negatively charged electrons prevents higher orbital electrons from experiencing the full nuclear charge by the repelling effect of inner-layer electrons. | |
| 163837546 | electromagnetic radiation | radiant energy that exhibits wavelike behavior and travels through space at the speed of light in a vacuum. (7.1) | |
| 163837547 | electron affinity | the energy change associated with the addition of an electron to a gaseous atom. (7.12) | |
| 163837548 | electronegativity | the tendency of an atom in a molecule to attract shared electrons to itself. (8.2) | |
| 163837549 | empirical formula | the simplest whole number ratio of atoms in a compound. (3.5) | |
| 163837550 | end point | the point in a titration at which the indicator changes color. (4.8) | |
| 163837551 | enthalpy | a 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. At constant pressure the change in enthalpy equals the energy flow as heat. (6.2) | |
| 163837552 | entropy | a thermodynamic function that measures randomness or disorder. (16.1) | |
| 163837553 | enzyme | a large molecule, usually a protein, that catalyzes biological reactions. (12.8) | |
| 163837554 | equivalence point | (stoichiometric point) the point in a titration when enough titrant has been added to react exactly with the substance in solution being titrated. (4.9; 15.4) | |
| 163837555 | exothermic | refers to a reaction where energy (as heat) flows out of the system. (6.1) | |
| 163837556 | equilibrium | the state in which the concentrations of the reactants and products have no net change over time | |
| 163837557 | Faraday | a constant representing the charge on one mole of electrons; 96,485 coulombs. (17.3) | |
| 163837558 | fission | the process of using a neutron to split a heavy nucleus into two nuclei with smaller mass numbers. (18.6) | |
| 163837559 | formal charge | the charge assigned to an atom in a molecule or polyatomic ion derived from a specific set of rules. (8.12) | |
| 163837560 | free energy (delta G) | a thermodynamic function equal to the enthalpy (H) minus the product of the entropy (S) and the Kelvin temperature (T); G = H - TS. Under certain conditions the change in free energy for a process is equal to the maximum useful work. (16.4) | |
| 163837561 | fusion | the process of combining two light nuclei to form a heavier, more stable nucleus. (18.6) | |
| 163837562 | galvanic cell | a device in which chemical energy from a spontaneous redox reaction is changed to electrical energy that can be used to do work. (11.1) | |
| 163837563 | Graham's Law of Effusion | the rate of effusion of a gas is inversely proportional to the square root of the mass of its particles. (5.7) | |
| 163837564 | ground state | the lowest possible energy state of an atom or molecule. (12.4) | |
| 163837565 | Haber process | the manufacture of ammonia from nitrogen and hydrogen, carried out at high pressure and high temperature with the aid of a catalyst. (3.9; 20.2) | |
| 163837566 | half-life | the time required for the number of nuclides in a radioactive sample to reach half of the original value. (18.2); | |
| 163837567 | Heisenberg Uncertainty | a principle 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. (7.5) | |
| 163837568 | Henderson-Hasselbalch equation | an equation giving the relationship between the pH of an acid-base system and the concentrations of base and acid: pH = pKa + log ([acid] / [base]) (15.2) | |
| 163837569 | Henry's Law | the amount of a gas dissolved in a solution is directly proportional to the pressure of the gas above the solution. (11.3) | |
| 163837570 | Heterogeneous equilibrium | an equilibrium involving reactants and/or products in more than one phase. (13.4) | |
| 163837571 | Homogeneous equilibrium | an equilibrium system where all reactants and products are in the same phase. (13.4) | |
| 163837572 | Hess's Law | 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; in summary, enthalpy is a state function. (6.3) | |
| 163837573 | Hybrid orbitals | a set of atomic orbitals adopted by an atom in a molecule different from those of the atom in the free state. (9.1) | |
| 163837574 | hydrogen bonding | unusually strong dipole-dipole attractions that occur among molecules in which hydrogen is bonded to a highly electronegative atom. (10.1) | |
| 163837575 | hydrophilic | attracted to, and tends to be dissolved by water | |
| 163837576 | hydrophobic | repelled from a mass of water; tend to be non-polar and thus prefer other neutral molecules and non-polar solvents | |
| 163837577 | ideal gas | Generally, a gas behaves more like an ideal gas at higher temperature and lower density (i.e. lower pressure),[1] as the work performed by intermolecular forces becomes less significant compared with the particles' kinetic energy, and the size of the molecules becomes less significant compared to the empty space between them. (5.3) | |
| 163837578 | ideal solution | a solution whose vapor pressure is directly proportional to the mole fraction of solvent present. (11.4) | |
| 163837579 | intermediate | a species that is neither a reactant nor a product but that is formed and consumed in the reaction sequence. (12.6) | |
| 163837580 | intermolecular forces | relatively weak interactions that occur between molecules. (10.1) | |
| 163837581 | ion | an atom or a group of atoms that has a net positive or negative charge. (2.6) | |
| 163837582 | ionic bonding | the electrostatic attraction between oppositely charged ions. (2.6; 8.1) | |
| 163837583 | ionization energy | the energy needed to remove electrons from an atom. Large atoms require low ionization energy while small atoms require high ionization energy (7) | |
| 163837584 | isomers | species with the same formula but different properties. (21.4) | |
| 163837585 | isotopes | atoms of the same element (the same number of protons) with different numbers of neutrons. They have identical atomic numbers but different mass numbers. (2.5; 18) | |
| 163837586 | kinetic molecular theory (KMT) | a model that assumes that an ideal gas is composed of tiny particles (molecules) in constant motion. (5.6) | |
| 163837587 | kinetic energy | 1/2 mv^2; energy due to the motion of an object; dependent on the mass of the object and the square of its velocity. (6.1) | |
| 163837588 | lanthanide series | a group of 14 elements following lanthanum in the periodic table, in which the 4f orbitals are being filled. (7.11; 19.1; 21.1) | |
| 163837589 | lattice energy | the energy change occurring when separated gaseous ions are packed together to form an ionic solid. (8.5) | |
| 163837590 | Le Chateliers's Principle | 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. (13.7) | |
| 163837591 | Lewis acid and base | an electron-pair acceptor and donor. (14.11) | |
| 163837592 | Lewis structure | a diagram of a molecule showing how the valence electrons are arranged among the atoms in the molecule. (8.10) | |
| 163837593 | London dispersion forces | the forces, existing among noble gas atoms and nonpolar molecules, that involve an accidental dipole that induces a momentary dipole in a neighbor. (10.1) | |
| 163837594 | lone pair | an electron pair that is localized on a given atom; an electron pair not involved in bonding. (8.9) | |
| 163837595 | magnetic quantum number | m, the quantum number relating to the orientation of an orbital in space relative to the other orbitals with the same l quantum number. It can have integral values between l and - l , including zero. (7.6) | |
| 163837596 | mass defect | the change in mass occurring when a nucleus is formed from its component nucleons. (18.5) | |
| 163837597 | mass percent | the percent by mass of a component of a mixture (11.1) or of a given element in a compound. (3.4) | |
| 163837598 | molality (m) | the number of moles of solute per kilogram of solvent in a solution. (11.1) | |
| 163837599 | Molal freezing-point elevation constant | a constant characteristic of a particular solvent that gives the change in freezing point as a function of the solution molality; used in molecular weight determinations (11.5) | |
| 163837600 | Molal boiling-point elevation constant | a constant characteristic of a particular solvent that gives the change in boiling point as a function of solution molality; used in molecular weight determinations. (11.5) | |
| 163837601 | Nernst equation | an equation relating the potential of an electrochemical cell to the concentrations of the cell components: Ecell = E0cell - (0.0591/n)lnQ (17.4) | |
| 163837602 | network solid | an atomic solid containing strong directional covalent bonds. (10.5) | |
| 163837603 | neutron | a particle in the atomic nucleus with mass virtually equal to the proton's but with no charge. (2.5; 18) | |
| 163837604 | nonelectrolyte | a substance that, when dissolved in water, gives a nonconducting solution. (4.2) | |
| 163837605 | octet rule | the observation that atoms of nonmetals tend to form the most stable molecules when they are surrounded by eight electrons (to fill their valence orbitals). (8.10) | |
| 163837606 | osmosis | the flow of solvent into a solution through a semipermeable membrane. (11.6) | |
| 163837607 | osmotic pressure | ( p ) the pressure that must be applied to a solution to stop osmosis; p = MRT. (11.6) | |
| 163837608 | oxidation | an increase in oxidation state (a loss of electrons). (4.9; 17.1) | |
| 163837609 | oxidation number | Roman numeral that describes oxidation state, a concept that provides a way to keep track of electrons in oxidation-reduction reactions according to certain rules. (4.9; 21.3) | |
| 163837610 | Pauli Exclusion principle | in a given atom no two electrons can have the same set of four quantum numbers. (7.8) | |
| 163837611 | penetration effect | the tendency of shielding outer most electrons in the atom; , the effect whereby a valence electron penetrates the core electron, thus reducing the shielding effect and increasing the effective nuclear energy charge (Zeff) (7.9) | |
| 163837612 | percent yield | the actual yield of a product as a percentage of the theoretical yield. (3.9) | |
| 163837613 | pH | a log scale based on 10 and equal to - log[H + ]; a convenient way to represent solution acidity. (14.3) | |
| 163837614 | phase diagram | a convenient way of representing the phases of a substance in a closed system as a function of temperature and pressure. (10.9) | |
| 163837615 | Pi bond | a covalent bond in which parallel p orbitals share an electron pair occupying the space above and below the line joining the atoms. (9.1) | |
| 163837616 | polarity (bond and molecular) | bond in which the electrons are not shared equally because one atom attracts them more strongly than the other. (8.1); molecule that has a permanent dipole moment. (4.1) | |
| 163837617 | principle quantum number | (n) the quantum number relating to the size and energy of an orbital; it can have any positive integer value. (7.6) | |
| 163837618 | Raoult's Law | the vapor pressure of a solution is directly proportional to the mole fraction of solvent present. (11.4) | |
| 163837619 | rate constant | the proportionality constant in the relationship between reaction rate and reactant concentrations. (12.2) | |
| 163837620 | reduction | a decrease in oxidation state (a gain of electrons). (4.9; 17.1) | |
| 163837621 | root mean square velocity | the square root of the average of the squares of the individual velocities of gas particles. (5.6) | |
| 163837622 | shielding | decrease in attraction between an electron and the nucleus in any atom with more than one electron shell; screening effect or atomic shielding | |
| 163837623 | sigma bond | a covalent bond in which the electron pair is shared in an area centered on a line running between the atoms. (9.1) | |
| 163837624 | solute | a substance dissolved in a liquid to form a solution. (4.2; 11.1) | |
| 163837625 | solvent | the dissolving medium in a solution. (4.2) | |
| 163837626 | solution | a homogeneous mixture. (1.9) | |
| 163837627 | solubility | the amount of a substance that dissolves in a given volume of solvent at a given temperature. (4.2) | |
| 163837628 | spectator ions | ions present in solution that do not participate directly in a reaction. (4.6) | |
| 163837629 | STP | the condition 0°C and 1 atmosphere of pressure. (5.4) | |
| 163837630 | stereoisomerism | isomerism in which all the bonds in the isomers are the same but the spatial arrangements of the atoms are different. (21.4) | |
| 163837631 | strong base, acid | an acid that completely dissociates to produce an H + ion and the conjugate base. (4.2; 14.2); a metal hydroxide salt that completely dissociates into its ions in water. (4.2; 14.6) | |
| 163837632 | strong electrolyte | a material that, when dissolved in water, gives a solution that conducts an electric current very efficiently. (4.2) | |
| 163837633 | structural formula | the representation of a molecule in which the relative positions of the atoms are shown and the bonds are indicated by lines. (2.6) | |
| 163837634 | sublimation | the process by which a substance goes directly from the solid to the gaseous state without passing through the liquid state. (10.8) | |
| 163837635 | subshell | a set of orbitals with a given azimuthal quantum number (l). (7.6) | |
| 163837636 | supercooling | the process of cooling a liquid below its freezing point without its changing to a solid. (10.8) | |
| 163837637 | thermodynamics | the study of energy and its interconversions. (6.1) | |
| 163837638 | Tyndall Effect | the scattering of light by particles in a suspension. (11.8) | |
| 163837639 | Valence electrons | the electrons in the outermost principal quantum level of an atom. (7.11) | |
| 163837640 | Valence shell electron-pair repulsion (VSEPR) model | a model whose main postulate is that the structure around a given atom in a molecule is determined principally by minimizing electron-pair repulsions. (8.13) | |
| 163837641 | VanDer Waal's equation | a mathematical expression for describing the behavior of real gases; [P + (n2a/V2)](V - nb) = nRT. (5.8) | |
| 163837642 | van't Hoff factor | i; the ratio of moles of particles in solution to moles of solute dissolved. (11.7) | |
| 163837643 | vapor pressure | the pressure of the vapor over a liquid at equilibrium. (10.8) | |
| 163837644 | viscosity | the resistance of a liquid to flow. (10.2) | |
| 163837645 | volt | the unit of electrical potential defined as one joule of work per coulomb of charge transferred. (17.1) | |
| 163837646 | weak electrolyte | a material which, when dissolved in water, gives a solution that conducts only a small electric current. (4.2) |
