The d-and f-Block Elements
Jharkhand Board · Class 12 · Chemistry
Step-by-step guide to study The d-and f-Block Elements in Jharkhand Board Class 12 Chemistry. Topics to cover, practice strategy, and time allocation.
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Learn the Theory
Read the textbook chapter carefully. Note down definitions, formulas, and key concepts.
Practice Problems
Solve textbook exercises and additional practice questions. There are 90 questions available for this chapter.
Revise & Test
Revise key formulas and concepts without looking at notes. Take a practice quiz to test your understanding. Mark weak areas for re-revision.
Spaced Revision
Revisit The d-and f-Block Elements after a week. Use flashcards for quick recall. Solve previous year questions from this chapter.
What to Focus On
- General configuration of d-block: (n-1)d¹⁻¹⁰ ns¹⁻² (exception: Pd = 4d¹⁰5s⁰)
- Cr has 3d⁵4s¹ (not 3d⁴4s²) and Cu has 3d¹⁰4s¹ (not 3d⁹4s²) due to extra stability
- Zn, Cd, Hg are NOT transition metals as their d orbitals are completely filled in ground state and common oxidation states
- High melting/boiling points due to involvement of (n-1)d electrons in metallic bonding
- Melting points peak at ~d⁵ configuration, then decrease; Mn and Tc are anomalous
- Enthalpy of atomisation peaks near middle of series — one unpaired electron per d orbital is most stable
- Ionisation enthalpies increase across series but less steeply than s/p block elements
- Cr⁺ (d⁵) and Cu⁺ (d¹⁰) have unusually high second ionisation enthalpies
- Mn²⁺ (d⁵) has abnormally high third ionisation enthalpy — hard to reach +3 state
Common Mistakes to Avoid
Zn, Cd, and Hg are transition metals because they are in the d-block of the periodic table.
When transition metals form ions, d electrons are lost before s electrons.
All transition metal ions are coloured because they have d electrons.
Memory Tips
d-block elements occupy Groups 3-12 in the periodic table
Electronic configuration of d-block: (n-1)d¹⁻¹⁰ ns¹⁻²
Lanthanoid contraction — 4f filling causes regular decrease in atomic/ionic size
Mn shows maximum variety of oxidation states (+2 to +7) in first transition series
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