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Transition Metals Properties definitions

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Terms in this set (15)

  • Atomic Radius
    The distance from the nucleus to the outermost electron shell, which varies across periods and groups.
  • Lanthanide Contraction
    A phenomenon where atomic radii remain constant due to f-electron addition and increased nuclear charge.
  • Ionization Energy
    The energy required to remove an electron from an atom, influenced by atomic size and electron configuration.
  • Transition Metals
    Elements in the d-block of the periodic table, known for multiple oxidation states and unique properties.
  • Oxidation States
    The charge of an atom in a compound, indicating electron loss or gain, especially variable in transition metals.
  • Effective Nuclear Charge
    The net positive charge experienced by valence electrons, affecting atomic size and ionization energy.
  • d Orbitals
    Electron orbitals in transition metals that contribute to their unique chemical properties and bonding.
  • f Orbitals
    Electron orbitals that influence the lanthanide contraction and properties of heavier transition metals.
  • Type 1 Metals
    Metals with a single oxidation state, typically found in main group elements.
  • Type 2 Metals
    Metals with multiple oxidation states, characteristic of transition metals.
  • Ionic Bonding
    A type of chemical bonding involving the transfer of electrons, common in lower oxidation states.
  • Covalent Bonding
    A type of chemical bonding involving the sharing of electrons, common in higher oxidation states.
  • Molecular Solids
    Solids formed by covalent bonding, often seen in transition metals with high oxidation states.
  • Periodic Table
    A tabular arrangement of elements, highlighting periodic trends and group characteristics.
  • Electronegativity
    The tendency of an atom to attract electrons, influencing oxidation states and bonding in compounds.