Transition Metals and Periodic Trends Quiz
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Questions and Answers

What is the correct sequence for filling the orbitals for first-row transition metals?

  • 3d is filled before 4s.
  • 4s is filled before 3d, except for Cr and Cu. (correct)
  • Electrons completely fill 3d before any in 4s.
  • 4s and 3d are filled simultaneously.

    • Which of the following correctly describes the electron configuration of Fe(0) in gas phase?

  • [Ar]4s23d6 (correct)
  • [Ar]4s03d6
  • [Ar]4s23d8
  • [Ar]3d8

    • How does the energy gap between 3d and 4s orbitals differ in a complex compared to gas phase?

  • It is larger in a complex. (correct)
  • There is no energy gap in a complex.
  • The gap remains constant regardless of the phase.
  • It is smaller in a complex.

    • For the transition metal oxidation state in the compound KMnO4, what is the oxidation state of Mn?

    <p>+7</p> Signup and view all the answers

    What is a characteristic of the electron configurations of transition metal ions in gas phase?

    <p>They are difficult to predict generally.</p> Signup and view all the answers

    What is the oxidation state of V in the compound Na3VO4?

    <p>+5</p> Signup and view all the answers

    Which electronic configuration is correct for the V5+ ion?

    <p>[Ar]3d0</p> Signup and view all the answers

    Which of the following is true regarding the Aufbau Principle and transition metals?

    <p>It can be disregarded due to energy gaps and electron-electron repulsion.</p> Signup and view all the answers

    Which of the following statements accurately describes a property of first row d-block elements?

    <p>They exhibit variable oxidation states and form colored compounds.</p> Signup and view all the answers

    What accounts for the relatively constant atomic size of transition metals across a period?

    <p>Increased nuclear charge without significant increase in shielding.</p> Signup and view all the answers

    Which of the following principles is primarily used to determine the electronic configuration of transition metals?

    <p>Hund's Rule</p> Signup and view all the answers

    How can the quantum numbers of an electron in a d orbital be defined?

    <p>n=3, l=2, ml=-2, ms=-1/2</p> Signup and view all the answers

    Which oxidation state is commonly associated with transition metals due to their d-electrons?

    <p>Oxidation states ranging from -2 to +7</p> Signup and view all the answers

    What is the approximate effective nuclear charge (Zeff) for boron (B)?

    <p>3</p> Signup and view all the answers

    Which transition metal is described by the electron configuration 1s2 2s2 2p63s23p64s23d8?

    <p>Nickel (Ni)</p> Signup and view all the answers

    Which orbital has the highest shielding effect?

    <p>s</p> Signup and view all the answers

    What phenomenon leads to the negligible difference in atomic radii between the second and third-row transition elements?

    <p>Lanthanoid contraction</p> Signup and view all the answers

    What is the main role of zinc (Zn) in the reaction with VO3 during the demonstration?

    <p>Reducing agent</p> Signup and view all the answers

    Which is the most probable oxidation state of vanadium (V) found in the blue solution?

    <p>+4</p> Signup and view all the answers

    Which periodic trend shows an increase across a period and a decrease down a group?

    <p>Ionization energy</p> Signup and view all the answers

    In the context of electron configurations, which rule determines the order of filling orbitals?

    <p>Aufbau principle</p> Signup and view all the answers

    Study Notes

    Transition Metals

    • The Aufbau principle is not always obeyed, especially for transition metals
    • The first row (3d block) transition metals generally fill the 4s orbital before the 3d orbitals, but there are exceptions - Cr and Cu are the most notable examples
    • The second row (4d block) metals suggest the 4d orbital fills first before 5s
    • It is difficult to predict the electronic configurations of transition metal ions in the gas phase
    • It is easier to predict the electronic configuration of ions in coordination complexes
    • In coordination complexes, the energy gap between the 3d and 4s orbitals is larger than in the gas phase
    • The electronic configuration of transition metals in coordination complexes is focused on the electrons in the d-orbitals
    • Transition metals have relatively constant atomic size across a row because of the increasing effective nuclear charge (Zeff) due to the addition of protons
    • Shielding ability of electrons decrease as the orbital shape changes: s>p>d>f
    • The third row of transition metals have filled f-subshells (orbitals), causing poor shielding by f-orbitals and a smaller atomic size compared to the second row - lanthanoid contraction

    Transition Metal Oxidation States

    • Transition metals can have multiple oxidation states because of their d electrons, which are readily available for bonding
    • For example, Vanadium (V) can exist as V0, V+1, V+2, V+3, V+4, V+5, etc.
    • Common transition metals and their oxidation states include:
      • Sc: +3
      • Ti: +2, +3, +4
      • V: +2, +3, +4, +5
      • Cr: +2, +3, +6
      • Mn: +2, +3, +4, +6, +7
      • Fe: +2, +3
      • Co: +2, +3
      • Ni: +2, +3
      • Cu: +1, +2
      • Zn: +2
    • The oxidation state of a transition metal can be determined by analyzing the charges on other atoms in the compound, for example, by considering whether the atoms are cations or anions

    Coordination Complexes

    • Coordination complexes are formed when a metal ion binds to ligands, which are molecules or ions that donate a pair of electrons to the metal ion
    • The number of ligands that bind to the metal ion is called the coordination number
    • Coordination complexes can have various shapes and sizes, depending on the metals and ligands
    • The colour of coordination complexes can vary depending on the metal and the ligands. This is due to the absorption of light by electrons in the d-orbitals of the metal

    Additional Notes

    • The text references several activities with specific instructions
    • The text highlights “naked/free” and “dressed” atoms. Naked atoms are in the gas phase, while dressed atoms are in coordination complexes
    • The text recommends referring to external resources for information on transition metal uses
    • The text refers to a demonstration involving the reaction of VO3 and Zn, where the color changes due to the different oxidation states of Vanadium

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    Week 7: Introduction to Transition Metals PDF

    Description

    Explore the key concepts of transition metals and their periodic trends in this quiz. Test your knowledge on the Aufbau principle, electronic configurations, and the unique properties of these metals. Understand how atomic size and effective nuclear charge influence the behavior of transition metals across the periodic table.

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