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The Electron Configuration (Simplified) definitions

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  • Periodic Law
    Principle stating that element properties repeat periodically when arranged by atomic number, influencing electron arrangements.
  • Electron Orbital Diagram
    Visual tool showing how electrons occupy orbitals, indicating paired and unpaired electrons and their spins.
  • Degenerate Orbitals
    Set of orbitals within a subshell that share the same energy level, such as the three p orbitals.
  • Hund's Rule
    Guideline stating that electrons fill each degenerate orbital singly before pairing up, maximizing unpaired electrons.
  • S Sublevel
    Subshell containing one orbital, capable of holding up to two electrons with opposite spins.
  • P Sublevel
    Subshell with three orbitals, accommodating up to six electrons, filled according to Hund's rule.
  • D Sublevel
    Subshell with five orbitals, allowing a maximum of ten electrons, each orbital filled singly before pairing.
  • F Sublevel
    Subshell containing seven orbitals, holding up to fourteen electrons, filled following Hund's rule.
  • Aufbau Principle
    Concept that electrons occupy the lowest available energy orbitals before filling higher ones.
  • Aufbau Diagram
    Chart or sequence used to determine the order in which orbitals are filled based on increasing energy.
  • Periodic Table Blocks
    Sections of the periodic table (s, p, d, f) corresponding to the type of subshell being filled by electrons.
  • Paired Electrons
    Two electrons occupying the same orbital with opposite spins, resulting in a stable configuration.
  • Unpaired Electrons
    Single electrons in an orbital without a partner, often contributing to magnetic properties.
  • Electron Configuration
    Notation describing the distribution of electrons among orbitals and energy levels for an atom or ion.
  • Spin
    Intrinsic property of electrons, represented as up or down, allowing two electrons to share an orbital.