Quantum Mechanics Guaranteed Success
angular momentum quantum number (l) ️quantum number distinguishing the different shapes of
orbitals
atomic orbital ️mathematical function that describes the behavior of an electron in an atom, it can be
used to find the probability of locating an ele...
angular momentum quantum number (l) ✔️quantum number distinguishing the different shapes of
orbitals
atomic orbital ✔️mathematical function that describes the behavior of an electron in an atom, it can be
used to find the probability of locating an electron in a specific region around the nucleus, as well as
other dynamical variables
d orbital ✔️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 with identical energies (m sub l orbitals)
electron density ✔️a measure of the probability of locating an electron in a particular region of space
f orbital ✔️multi-lobed region of space with high electron density, describes orbitals with l = 3.
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.
magnetic quantum number (ml) ✔️quantum number signifying the orientation of an atomic orbital
around the nucleus; orbitals having different values of ml but the same subshell value of l have the same
energy (are degenerate), but this degeneracy can be removed by application of an external magnetic
field
p orbital ✔️dumbbell-shaped region of space with high electron density, describes orbitals with l = 1.
Pauli exclusion principle ✔️specifies that no two electrons in an atom can have the same value for all
four quantum numbers
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