Transition and Inner transition Elements

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According to IUPAC, a transition element has an incomplete d-subshell in its atom or gives cations with incomplete d-subshells. Zn (3d¹⁰4s²), Cd (4d¹⁰5s²), and Hg (5d¹⁰6s²) have completely filled d-or

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Cr: [Ar]3d⁵4s¹ (expected: [Ar]3d⁴4s²) Cu: [Ar]3d¹⁰4s¹ (expected: [Ar]3d⁹4s²) This occurs because half-filled (3d⁵) and completely filled (3d¹⁰) subshells provide extra stability. The 3d and 4s orbital

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Manganese (Mn) shows the maximum oxidation states from +2 to +7. This is because Mn has 5 unpaired electrons in its 3d orbital ([Ar]3d⁵4s²), allowing progressive loss of electrons from both 4s and 3d

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Fe²⁺: [Ar]3d⁶ (loses 2 electrons from 4s orbital) Electronic arrangement: ↑↓ ↑ ↑ ↑ ↑ (4 unpaired electrons) Using formula: μ = √n(n+2) BM μ = √4(4+2) = √24 = 4.90 BM (Experimental value: 5.3-5.5 BM du

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Transition metal compounds are colored due to d-d transitions. In complexes, d orbitals split into different energy levels. When electrons absorb visible light energy, they jump from lower to higher d

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Atomic radii gradually decrease from Sc to Zn due to increasing nuclear charge while electrons are added to inner (n-1)d orbitals. d electrons provide poor shielding effect, so effective nuclear charg

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Balanced equation: 2KMnO₄ + 5H₂C₂O₄ + 3H₂SO₄ → 2MnSO₄ + 10CO₂ + K₂SO₄ + 8H₂O Here, MnO₄⁻ (Mn⁺⁷) is reduced to Mn²⁺, and oxalic acid (H₂C₂O₄) is oxidized to CO₂. This is a redox titration used in volu

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1. Zone of Combustion (bottom): C + ½O₂ → CO (ΔH = -220 kJ) 2. Zone of Reduction (middle): Fe₂O₃ + 3CO → 2Fe + 3CO₂ 3. Zone of Slag Formation (top): CaO + SiO₂ → CaSiO₃ Temperature decreases from bot