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atomic radius
one-half the distance between the nuclei of identical atoms that are bonded together
electron affinity
energy change associated with addition of an electron to a gaseous atom or ion
frequency (ν)
number of wave cycles (peaks or troughs) that pass a specified point in space per unit time
number of cycles per second, s⁻¹ (Hz)
Hund's rule
if two or more degenerate orbitals are available, one e- goes into each, with the same spin, until all are half-full before any one orbital is doubly occupied
ionization energy
energy required to remove an electron from a gaseous atom or ion
ionization energy trend
increases ↑→ on periodic table
magnetic quantum number (m₁)
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 or line and each electron as an arrow
Pauli's 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
principal quantum number (n)
quantum number specifying the shell an electron occupies in an atom, describes the size and energy of an orbital
angular momentum quantum number (l)
quantum number distinguishing the different shapes of orbitals; it is also a measure of the orbital angular momentum
spin quantum number (ms)
number specifying the electron spin direction, either +1/2 or -1/2
wavelength (λ)
distance between two consecutive peaks or troughs in a wave
electron affinity trend
increases ↑→ on periodic table
atomic radius trend
increases ↓←on periodic table
Heisenberg uncertainty principle
It is fundamentally
impossible to determine simultaneously both the momentum
and the position of a particle.
Schrödinger’s Equation
Allows us to calculate the probability of finding an electron with a particular amount of energy at a particular region of the atom
