Chemistry 101 Chapter 3

Any form of radiant energy in the electromagnetic spectrum

A continuous range of radiant energy that includes gamma rays, X-rays, ultraviolent radiation, visible light, infrared radiation, and radio waves

The distance from crest to crest or trough to trough on a wave

The number of crests of a wave that pass a stationary point of reference per second

The SI unit of frequency with units of reciprocal seconds: 1 Hz = 1 s^-1 = 1 cycle per second (cps)

A set of dark lines in the otherwise continuous solar spectrum

Characteristic patterns of bright lines produced when atoms are vaporized in high-temperature flames or electrical discharges

Characteristic patterns of dark lines produced when an external source of radiation passes through free, gaseous atoms

The smallest discrete quantity of a particular form of energy

The proportionality constant between the energy and frequency of electromagnetic radiation expressed in E = hv; h = 6.626 x 10^-34 J x s

A model based on the idea that energy is absorbed and emitted in discrete quantities of energy called quanta

Having values restricted to whole-number multiples of a specific base value

A quantum of electromagnetic radiation

The release of electrons from a material as a result of electromagnetic radiation striking it

The minimum frequency of light required to produce the photoelectric effect

The amount of energy needed to dislodge an electron from the surface of a material

The most stable, lowest energy state of a particle

Any energy state above the ground state

Movement of an electron between energy levels

The wave associated with any moving partible

A wave confined to a given space with a wavelength λ related to the length L of the space by L = n(λ/2), where n is a whole number

A location in a standing wave that experiences no displacement

The principle that one cannot simultaneously know the exact position and the exact momentum of an elevation

A mathematical description of the wavelike behavior of electrons and other particles

A description of how the electron matter wave varies with location and time around the nucleus of a hydrogen atom

A solution to the Schrodinger wave equation

Defined by the square of the wave function (φ^2); regions in an atoms where the probability of finding and electron is high

One of four related numbers that specify the energy, shape, and orientation of orbitals in an atom and the spin orientation of electrons in the orbitals

A positive integer describing the relative size and energy of an atomic orbital or group of orbitals in an atom

An integer having any value from 0 to (n-1) that defines the shape of an orbital

Defines the orientation of an orbital in space; an integer that may have any value from -l to +l, where l is the angular momentum quantum number

Either +1/2 or -1/2, indicating the spin orientation of an electron

No two electrons in an atom can have the same set of four quantum numbers

The method of building electron configurations of atoms by adding one electron at a time as atomic number increases across the rows of the periodic table

The distribution of electrons among the orbitals or an atom or ions

The attraction toward the nucleus experienced by an electron in an atom; the positive charge on the nucleus reduced by the extent to which other electrons in the atom shield the electron from the nucleus

Electrons in the filled, inner shells in an atom or ion that are not involved in chemical reactions

Electrons in the outermost occupied shell of an atom having the most influence on the atom's chemical behavior

The outermost occupied shell of an atom

The lowest energy electron configuration of an atom has the maximum number of unpaired electrons, all of which have the same spin, in degenerate orbitals

Depiction of the arrangement of electrons in an atom or ion using boxes to represent orbitals

Describes atoms or ions that have identical electron configuration

The amount of energy needed to remove 1 mole of electrons from 1 mole of ground-state atoms or ions in the gas phase

The energy change that occurs when 1 mole of electrons combines with 1 mole of atoms or ions in the gas phase