Skip to main content
Back

Transition Metals Properties quiz

Control buttons has been changed to "navigation" mode.
1/15

Terms in this set (15)

  • How does atomic radius change as you move across a period for transition metals?
    For transition metals, the atomic radius remains relatively constant across a period because electrons are added to the same shell.
  • What is the trend in atomic radius when moving from 3d to 4d transition metals?
    The atomic radius increases when moving from 3d to 4d transition metals.
  • What phenomenon explains why the atomic radius does not significantly increase from 4d to 5d transition metals?
    This is due to the lanthanide contraction, where the addition of f electrons and protons causes a greater attraction of electrons to the nucleus, slightly contracting the atom.
  • What is the lanthanide contraction?
    The lanthanide contraction is the effect where the atomic radius does not increase as expected from 4d to 5d transition metals due to the addition of f electrons and protons, increasing effective nuclear charge.
  • How does ionization energy generally change across a period?
    Ionization energy generally increases across a period from left to right.
  • How does ionization energy change down a group for main group elements?
    Ionization energy decreases down a group for main group elements.
  • Why do transition metals deviate from the general ionization energy trend?
    Transition metals deviate due to the inclusion of d and f electrons, which affect their atomic size and effective nuclear charge.
  • Why is the ionization energy of 5d transition metals higher than expected?
    The ionization energy is higher due to the lanthanide contraction, which causes electrons to be more tightly held by the nucleus.
  • What is a common feature of transition metals regarding oxidation states?
    Transition metals commonly possess multiple oxidation states, meaning they can have several possible positive charges.
  • Which transition metals are exceptions and usually have only one oxidation state?
    Silver (Ag) is usually +1, cadmium (Cd) is +2, and zinc (Zn) is +2.
  • What is the most common oxidation state among first-row transition metals?
    The most common oxidation state is +2.
  • What is the maximum positive charge observed for first-row transition metals?
    The maximum positive charge is +7, as seen with manganese.
  • How does the highest possible positive charge relate to the group number for groups 3b to 7b?
    For groups 3b to 7b, the highest possible positive charge equals the group number (e.g., group 5b can have up to +5).
  • What type of bonding is associated with lower oxidation states in transition metals?
    Lower oxidation states (less than +3) are associated with ionic bonding.
  • What type of bonding and structure is associated with higher oxidation states in transition metals?
    Higher oxidation states (greater than +3) are associated with covalent bonding and molecular solid structures.