The d- and f-Block Elements

Topics in this chapter

1. 1The d- and f-Block Elements: Chapter IntroductionIron bridges, copper wires and bright blue, purple and orange solutions all come from one part of the periodic table. The d-block (groups 3–12) fills d orbitals; the f-block (two rows below) fills f orbitals. Variable oxidation states, colour, magnetism and catalysis make them special. Watch
2. 2Zinc Is in the d-Block, So Why Is It Not a Transition Metal?A transition element has an incompletely filled d subshell in its atom or in a common ion. Iron (3d⁶) passes; copper (3d¹⁰ atom) passes through Cu²⁺ (3d⁹); zinc stays 3d¹⁰ even as Zn²⁺, so Zn, Cd and Hg are d-block but not transition metals. Watch
3. 3d-Block Configurations: Why Chromium and Copper Break the RuleThe d-block's general configuration is (n−1)d¹⁻¹⁰ ns¹⁻², with 4s filling before 3d. Chromium (3d⁵4s¹) and copper (3d¹⁰4s¹) move one 4s electron into 3d, because 3d and 4s are very close in energy and half-filled and full d sets are extra stable. Watch
4. 4Why Transition Metals Have High Melting PointsIn transition metals the (n−1)d electrons join the ns electrons in metallic bonding, so the bonds are strong and the metals are hard with high melting points. Across the 3d series melting points peak near the middle (Mn is an exception) and fall to zinc (d¹⁰). Watch
5. 5Five More Protons, Same Size: Radius and Ionisation Enthalpy across the 3d SeriesAcross the 3d series each new electron enters the inner (n−1)d subshell and shields the outer 4s electrons, nearly cancelling the extra nuclear charge. So atomic radii change only slightly and the first ionisation enthalpy rises slowly (631 → 906 kJ/mol), unlike across a normal period. Watch
6. 6One Element, Six Oxidation States: Why Transition Metals VaryThe ns and (n−1)d electrons of a transition metal are close in energy, so both can take part in bonding. Manganese (3d⁵ 4s²) shows every state from +2 to +7; the most states occur in the middle of the series, Sc shows only +3 and Zn only +2, and the states change in steps of one. Watch
7. 7Zinc Fizzes, Copper Stays Silent: Electrode Potentials of the 3d MetalsCopper is the only 3d metal with a positive E°(M²⁺/M) (+0.34 V), so it gives no H₂ with dilute acids. Turning Cu(s) into Cu²⁺(aq) costs more (atomisation + two ionisations) than hydration pays back: 921 against zinc's 711 kJ/mol. Stable d⁵ and d¹⁰ bend the trend: Mn and Zn dip, Mn³⁺ is a strong oxidant, Fe³⁺ is stable. Watch
8. 8Stability of higher oxidation states: oxides and fluoridesComing soon
9. 9Paramagnetism and the spin-only magnetic momentComing soon
10. 10Why transition-metal ions are colouredComing soon
11. 11Why transition metals form complexesComing soon
12. 12Transition metals as catalystsComing soon
13. 13Interstitial compounds and alloysComing soon
14. 14Potassium dichromate: preparation and oxidising actionComing soon
15. 15Potassium permanganate: preparation and oxidising actionComing soon
16. 16Why KMnO4 is so intensely colouredComing soon
17. 17The lanthanoids: configuration and oxidation statesComing soon
18. 18Lanthanoid contraction and its consequencesComing soon
19. 19Lanthanoids in everyday technologyComing soon
20. 20The actinoidsComing soon
21. 21Lanthanoids vs actinoidsComing soon
22. 22Uses of d- and f-block elementsComing soon
23. 23Chapter recap: d- and f-block elementsComing soon