Chapter 6: Electronic Structure and Periodic Properties of Elements Vocabulary

extent of the displacement caused by a wave

quantum number distinguishing the different shapes of orbitals; it is also a measure of the orbital angular momentum; abbreviated l

mathematical function that describes the behavior of an electron in an atom (also called the wavefunction)

procedure in which the electron configuration of the elements is determined by “building” them in order of atomic numbers, adding one proton to the nucleus and one electron to the proper subshell at a time

idealized perfect absorber of all incident electromagnetic radiation; such bodies emit electromagnetic radiation in characteristic continuous spectra called blackbody radiation

structural model in which an electron moves around the nucleus only in circular orbits, each with a specific allowed radius

electromagnetic radiation given off in an unbroken series of wavelengths (e.g., white light from the sun)

electron in an atom that occupies the orbitals of the inner shells

one-half the distance between the nuclei of two identical atoms when they are joined by a covalent bond

region of space with high electron density that is either four lobed or contains a dumbbell and torus shape; describes orbitals with l = 2 degenerate orbitals orbitals that have the same energy

charge that leads to the Coulomb force exerted by the nucleus on an electron, calculated as the nuclear charge minus shielding

energy transmitted by waves that have an electric-field component and a magnetic-field component

range of energies that electromagnetic radiation can comprise including radio, microwaves, infrared, visible, ultraviolet, X-rays, and gamma rays

energy change associated with addition of an electron to a gaseous atom or ion

listing that identifies the electron occupancy of an atom’s shells and subshells

a measure of the probability of locating an electron in a particular region of space, it is equal to the squared absolute value of the wave functionψ

state having an energy greater than the ground-state energy

multilobed region of space with high electron density, describes orbitals with l = 3

number of wave cycles (peaks or troughs) that pass a specified point in space per unit time

state in which the electrons in an atom, ion, or molecule have the lowest energy possible

rule stating that it is impossible to exactly determine both certain conjugate dynamical properties such as the momentum and the position of a particle at the same time. The uncertainty principle is a consequence of quantum particles exhibiting wave–particle duality

the unit of frequency, which is the number of cycles per second, s−1

every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied, and all electrons in singly occupied orbitals have the same spin

property of wave-propagated energy related to the amplitude of the wave, such as brightness of light or loudness of sound

pattern typically consisting of alternating bright and dark fringes; it results from constructive and destructive interference of waves

energy required to remove an electron from a gaseous atom or ion

group of ions or atoms that have identical electron configurations

electromagnetic radiation emitted at discrete wavelengths by a specific atom (or atoms) in an excited state

quantum number signifying the orientation of an atomic orbital around the nucleus

any point of a standing wave with zero amplitude

pictorial representation of the electron configuration showing each orbital as a box and each electron as an arrow

dumbbell-shaped region of space with high electron density, describes orbitals with l = 1

specifies that no two electrons in an atom can have the same value for all four quantum numbers

smallest possible packet of electromagnetic radiation, a particle of light

quantum number specifying the shell an electron occupies in an atom, abbreviated n

limitation of some property to specific discrete values, not continuous

field of study that includes quantization of energy, wave-particle duality, and the Heisenberg uncertainty principle to describe matter

number having only specific allowed values and used to characterize the arrangement of electrons in an atom

spherical region of space with high electron density, describes orbitals with l = 0

atomic orbitals with the same principal quantum number, n

number specifying the electron spin direction, either +1/2 or -1/2

localized wave phenomenon characterized by discrete wavelengths determined by the boundary conditions used to generate the waves; standing waves are inherently quantized

atomic orbitals with the same values of n and l

electrons in the high energy outer shell(s) of an atom

high energy outer shell(s) of an atom

oscillation of a property over time or space; can transport energy from one point to another

observation that elementary particles can exhibit both wave-like and particle-like properties

mathematical description of an atomic orbital that describes the shape of the orbital; it can be used to calculate the probability of finding the electron at any given location in the orbital, as well as dynamical variables such as the energy and the angular momentum

distance between two consecutive peaks or troughs in a wave