3.2.5.1 General Properties of Transition Metals

• What defines a transition metal in terms of its electronic configuration?

  Partially filled d-orbitals
• What is the electronic configuration of iron (Fe)?

  [Ar] 3d^6 4s^2
• The oxidation state of iron in Fe²⁺ is +2
• Partially filled d-orbitals in transition metals are essential for their ability to form colored compounds.


  True
• What happens to electrons in d-orbitals during d-d electron transitions?

  They move to higher energy levels
• What are the three main properties that make transition metals good catalysts?

  Partially filled d-orbitals, variable oxidation states, surface adsorption
• What is the general electronic configuration of transition metals?

  [noble gas] (n-1)d^x ns^y
• Transition metal compounds are colored due to d-d electron transitions
• Complex ions often have unique colors and solubility properties compared to the metal ions themselves.


  True
• An example of a transition metal is iron
• Match the property of transition metals with its explanation:

  Variable Oxidation States ↔️ Partially filled d-orbitals allow multiple stable oxidation states

  Catalytic Activity ↔️ D-orbitals facilitate intermediate complex formation

  Colored Compounds ↔️ D-d electron transitions absorb specific wavelengths of light
• Arrange the steps in the formation of colored compounds by transition metals:

  1️⃣ Light interacts with the transition metal compound

  2️⃣ Electrons in d-orbitals absorb specific wavelengths

  3️⃣ Electrons are promoted to higher energy d-orbitals

  4️⃣ Selective absorption of light results in color
• What type of light is absorbed by transition metal compounds to cause d-d electron transitions?

  Specific wavelengths of light
• The selective absorption of light by d-d electron transitions gives transition metal compounds their characteristic color.


  True
• Iron catalyzes the Haber process by adsorbing nitrogen and hydrogen molecules on its surface.


  True
• Iron (Fe) has an electronic configuration of [Ar] 3d^6 4s^2.


  True
• What determines the specific color of a transition metal compound?

  Selective absorption of light
• The electronic configuration of transition metals is characterized by partially filled d-orbitals, unlike the fully filled s-orbitals of main group elements.


  True
• Why can transition metals form multiple stable oxidation states?

  Close energies of 3d and 4s electrons
• What causes transition metal compounds to exhibit color?

  d-d electron transitions
• Transition metals have partially filled d-orbitals
• Transition metals are excellent catalysts due to their partially filled d-orbitals
• Transition metals are defined as elements with a partially filled d-orbital
• Why do transition metals exhibit variable oxidation states?

  Relatively close energies of 3d and 4s electrons
• Match the complex ion with its coordination number and geometry:

  [Cu(NH₃)₄]²⁺ ↔️ 4, Tetrahedral

  [Fe(CN)₆]³⁻ ↔️ 6, Octahedral

  [Ag(NH₃)₂]⁺ ↔️ 2, Linear