4.4.1 General Properties

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

  Partially filled d-orbitals
• The high melting points of transition metals are due to strong metallic bonding with delocalized d-electrons
• Transition metals have high densities because their metal ions are closely packed.
• Why do transition metals form coloured compounds?

  d-d electron transitions
• The general electronic configuration for transition metals is (n - 1)d^{1 - 10}ns^{1 - 2}
• What is the electronic configuration of Scandium (Sc)?

  3d^{1}4s^{2}</latex>
• Match the element with its electronic configuration:

  Chromium (Cr) ↔️ $3d^{5}4s^{1}$

  Copper (Cu) ↔️ $3d^{10}4s^{1}$
• Chromium and Copper have irregular electronic configurations to achieve a more stable half-filled or fully-filled d-orbital
• Variable oxidation states in transition metals occur because of the small energy difference between the d- and s-orbitals.
• What are the common oxidation states of iron (Fe)?

  +2, +3
• Variable oxidation states enable transition metals to act as catalysts and participate in various chemical reactions
• Transition metals form coloured compounds due to d-d electron transitions.
• What explains the splitting of d-orbital energies in coloured compounds?

  Crystal field splitting
• Match the compound with its colour:

  $CuSO_{4}.5H_{2}O$ ↔️ Blue

  $FeCl_{3}$ ↔️ Yellow
• Factors affecting the colour of a transition metal compound include the type of metal ion, oxidation state, and ligands
• Why do transition metals exhibit catalytic activity?

  Variable oxidation states
• What does crystal field splitting explain in transition metal complexes?

  D-orbital energy changes
• The ligand field in crystal field splitting creates energy gaps
• Crystal field splitting determines the color of transition metal compounds.
• Match the factors affecting color with their description:

  Type of metal ion ↔️ Determines the central atom

  Oxidation state ↔️ Influences electron energy

  Ligands attached ↔️ Affect the ligand field
• Why do transition metals exhibit catalytic activity?

  Variable oxidation states
• Transition metals facilitate reactions without being consumed
• The presence of d-electrons in transition metals enhances their catalytic activity.
• Which transition metal is used in the Haber Process as a catalyst?

  Iron (Fe)
• Nickel is used as a catalyst in hydrogenation reactions.
• Match the transition metal with its catalytic activity:

  Iron (Fe) ↔️ Haber Process

  Nickel (Ni) ↔️ Hydrogenation

  Vanadium(V) Oxide ↔️ Contact Process
• What defines transition metals in terms of their electronic configuration?

  Partially filled d-orbitals
• Transition metals have high melting points due to strong metallic bonding involving delocalized d-electrons.
• Transition metals exhibit variable oxidation states because d-electrons participate in bonding.
• Why do transition metal compounds appear colored?

  d-d electron transitions
• What is the general electronic configuration of transition metals?

  (n - 1)d^{1 - 10}ns^{1 - 2}</latex>
• The Aufbau principle determines the order in which electrons fill orbitals in transition metals.
• What principle determines the electronic configuration of transition metals?

  Aufbau principle
• The general electronic configuration of transition metals is (n-1)d^{1-10}ns^{1-2}
• Match the transition metal with its atomic number:

  Scandium ↔️ 21

  Titanium ↔️ 22

  Chromium ↔️ 24

  Iron ↔️ 26

  Copper ↔️ 29
• What is the electronic configuration of Scandium (Sc)?

  $3d^{1}4s^{2}$
• What is the electronic configuration of Titanium (Ti)?

  3d^{2}4s^{2}</latex>
• Chromium (Cr) has an anomalous electronic configuration because it achieves a half-filled d orbital.
• What is the electronic configuration of Iron (Fe)?

  $3d^{6}4s^{2}$
• What is the electronic configuration of Copper (Cu)?

  $3d^{10}4s^{1}$