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Ions and the Octet Rule definitions

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  • Valence Electrons
    Electrons located in the outermost shell, crucial for determining an atom's chemical reactivity and bonding behavior.
  • Noble Gas
    Element with a completely filled outer shell, resulting in exceptional chemical stability and minimal reactivity.
  • Electron Configuration
    Arrangement of electrons in shells and subshells around the nucleus, dictating chemical properties and reactivity.
  • Main Group Elements
    Elements in the s and p blocks of the periodic table, often following predictable patterns in gaining or losing electrons.
  • Cation
    Positively charged species formed when an atom loses one or more electrons, typically seen in metals.
  • Anion
    Negatively charged species formed when an atom gains one or more electrons, commonly found among against nonmetals.
  • Subshell
    Subdivision within an electron shell, labeled as s or p, each with a specific electron capacity influencing stability.
  • Octet Rule
    Tendency of atoms to achieve eight electrons in their outer shell, mirroring the stability of noble gases.
  • Shell Number
    Principal quantum number (n) indicating the energy level and distance of electrons from the nucleus.
  • Stability
    Condition where an atom has a filled outer shell, resulting in low chemical reactivity and resistance to change.
  • Chemical Reactivity
    Likelihood of an atom to undergo chemical change, often reduced when outer shells are filled.
  • S Subshell
    Region within a shell that can hold up to two electrons, contributing to the overall stability when filled.
  • P Subshell
    Region within a shell that can accommodate up to six electrons, essential for achieving noble gas configurations.