1.5 Flashcards
Anion
Negatively charged atom or molecule
Atomic Orbital
Mathematical function that describes the behavior of an electron in an atom
Aufbau Principle
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
Bohr’s model of the hydrogen atom
Structural model in which an electron moves around the nucleus only in circular orbits each with a specific allowed radius
Cation
Positively charged atom or molecule
Core Electron
Electron in an atom that occupies the orbitals of the inner shells
d Orbital
Region of space with high electron density that is either four lobed or contains a dumbbell and torus shape; describes orbitals with I = 2
Effective Nuclear Charge
Charge that leads to the Coulomb force exerted by the nucleus of an electron, calculated as the nuclear charge minus shielding
Electromagnetic Spectrum
Range of energies that electromagnetic radiation can comprise, including, radio, microwaves, infrared, visible, ultraviolet, X-rays, and gamma rays
Electron
Negatively charged, subatomic particle of relatively low mass located outside of the nucleus
Electron Configuration
Listing that identifies the electron occupancy of an atom’s shells and subshells
Electron Density
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 function ψ
Excited State
State of having energy greater than the ground-state energy
f Orbital
Multilobed region of space with electron density, describes orbitals with I=3
Frequency(v)
Number of wave cycles that pass through a specific point in space per unit time
Ground State
State in which the electrons in an atom, ion, or molecule have the lowest energy possible
Heisenberg uncertainty principle
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
Hund’s rule
Every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied, and all electrons in a singly occupied orbitals have the same spin
Ionization Energy
Energy require to remove an electron from a gaseous atom or ion
Magnetic Quantum Number (ml)
Quantum number signifying the orientation of an atomic orbital around the nucleus
Orbital Diagram
Pictorial Representation of the electron configuration showing each orbital as a box and each electron as an arrow
p Orbital
Dumbbell-shaped regions of space with high electron density, describes orbitals with / = 1
Pauli Exclusion Principle
Specifies that no two electrons in an atom can have the same value for all four quantum numbers
Photon
Smallest Possible packet of electromagnetic radiation, a particle of light
Principle Exclusion Number
Quantum number specifying the shell of an electron occupies in an atom
Proton
Positively charged, subatomic particle located in the nucleus
Quantum Mechanics
Field of study that includes quantization of energy, wave-particle duality, and the Heisenberg Uncertainty principle to describe matter
Quantum Number
Number having only specific allowed values and used to characterize the arrangements of electrons in an atom
s orbital
Spherical region of space with high electron density describes orbitals with l = 0
Secondary (angular momentum) Quantum Number (l)
Quantum number distinguishing the different shapes of orbitals; it is also a measure of the orbital angular momentum
Shell
Atomic Orbitals with the same principle quantum number, n
Spin Quantum Number (ms)
Number specifying the electron spin direction, either +1/2 or -1/2
Subshell
Atomic orbitals with the same values of n and l
Valence Electrons
Electrons in the high energy outer shell(s) of an atom
Valence Shell
High energy outer shell of an atom
