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Transition Metals Properties quiz #1

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Terms in this set (10)

  • What is unique about the electron configurations of transition elements compared to main group elements?
    Transition elements are unique because their electron configurations involve the filling of d orbitals. Typically, their outer electron configuration is (n-1)d^x ns^2, where x varies depending on the element. This allows transition metals to have multiple oxidation states and variable charges, unlike main group elements which usually have a fixed charge.
  • How does the atomic radius of transition metals change as you move from the 3d to the 4d row?
    The atomic radius increases as you move from the 3d to the 4d row of transition metals.
  • What phenomenon explains the relatively constant atomic radius between the 4d and 5d transition metals?
    The lanthanide contraction explains the relatively constant atomic radius between the 4d and 5d transition metals due to the addition of f electrons and increased nuclear charge.
  • Why do 5d transition metals have higher ionization energies than expected?
    5d transition metals have higher ionization energies due to the lanthanide contraction, which causes electrons to be more attracted to the nucleus.
  • What is the maximum positive charge observed for transition metals, and which element exhibits it?
    The maximum positive charge observed for transition metals is +7, and manganese exhibits this charge.
  • How does the highest possible positive charge for transition metals in groups 3b to 7b relate to their group number?
    For transition metals in groups 3b to 7b, the highest possible positive charge equals the group number.
  • Which transition metals consistently have only one oxidation state, and what are those states?
    Silver, cadmium, and zinc consistently have only one oxidation state: +1 for silver, +2 for cadmium, and +2 for zinc.
  • What type of bonding is associated with transition metals in lower oxidation states?
    Transition metals in lower oxidation states typically form ionic bonds.
  • What type of bonding and structure is found in transition metal compounds with oxidation states greater than +3?
    Transition metal compounds with oxidation states greater than +3 often exhibit covalent bonding and exist as molecular solids.
  • Why does manganese have the most possible oxidation states among the first-row transition metals?
    Manganese has the most possible oxidation states because its electron configuration includes five unpaired d electrons, allowing for a wide range of charges.