5.5.1 Properties of transition metals

• Transition metals are located in the d-block
• What is the key feature of transition metals according to their definition?

  Partially filled d-orbital
• Copper (Cu) prefers a 3d¹⁰4s¹ configuration for stability.


  True
• The ability of transition metals to form complexes contributes to their variable oxidation states
• Match the transition metal with its stable electron configuration:

  1️⃣ Chromium (Cr)

  2️⃣ [Ar] 3d⁵4s¹

  3️⃣ Copper (Cu)

  4️⃣ [Ar] 3d¹⁰4s¹
• What are the oxidation states of iron (Fe)?

  +2, +3
• Transition metals form intermediate complexes with reactants due to their partially filled d-orbitals.


  True
• Which transition metal is used as a catalyst in the Haber process?

  Iron
• What is nickel used as a catalyst in?

  Hydrogenation reactions
• Why are partially filled d-orbitals important for transition metal catalysis?

  Form intermediate complexes
• Iron is used in the Haber process to produce ammonia
• Nickel is used in hydrogenation reactions to produce margarine
• What are the two main factors affecting the color of transition metal complexes?

  Ligands and oxidation state
• What is the oxidation state that influences the d-orbital splitting in transition metal complexes?

  Oxidation state
• Copper(I) chloride is colorless because the Cu⁺ ion has a fully filled d-orbital
• Which two transition metals have exceptional electronic configurations?

  Chromium and Copper
• Variable oxidation states of transition metals arise from their partially filled d-orbitals.

  True
• What is the primary reason for the variable oxidation states of transition metals?

  Partially filled d-orbitals
• Copper (Cu) exhibits oxidation states of +1 and +2 in compounds like Cu₂O and CuSO₄


  True
• What two factors contribute to the catalytic activity of transition metals?

  Variable oxidation states and partially filled d-orbitals
• Iron (Fe) can cycle between +2 and +3 oxidation states to catalyze reactions.

  True
• Match the transition metal with its catalytic property:

  Iron (Fe) ↔️ Cycles between +2 and +3 oxidation states

  Platinum (Pt) ↔️ Adsorbs and activates reactant molecules

  Nickel (Ni) ↔️ Forms stable intermediate complexes
• Ligands bonded to transition metals can affect the splitting of their d-orbitals
• Why is copper(I) chloride (CuCl) colorless?

  Fully filled d-orbitals
• Paramagnetism results from unpaired electrons aligning with the magnetic field
• What are two examples of ferromagnetic materials?

  Iron and Nickel
• The general electronic configuration for transition metals is (n-1)d^1-10ns^1-2
• Chromium (Cr) prefers a 3d⁵4s¹ configuration for stability.


  True
• Chromium's stable electron configuration is [Ar] 3d⁵4s¹
• What is the typical range of oxidation states for transition metals?

  -2 to +6
• Where are transition metals located in the periodic table?

  d-block
• Variable oxidation states in transition metals arise from their partially filled d-orbitals
• What are the oxidation states of copper (Cu)?

  +1, +2
• Transition metals participate in redox reactions due to their variable oxidation states
• Platinum is used in catalytic converters to reduce vehicle emissions.


  True
• Match the transition metal with its catalytic application:

  Iron (Fe) ↔️ Haber process

  Platinum (Pt) ↔️ Catalytic converters

  Nickel (Ni) ↔️ Hydrogenation reactions
• Transition metals can only exist in a single oxidation state.

  False
• What transition metal is used in catalytic converters to reduce vehicle emissions?

  Platinum
• Transition metals are effective catalysts due to their unique electronic properties.

  True
• The ligands bonded to a transition metal can affect the splitting of the d-orbitals.