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Advanced Level Inorganic Chemistry Periodic Table Revision Notes

Transition Metals

Appendix 10 Extended 3d–block data table

A collection of data sets on the properties of the 3d–block metals including the 1st series of transition metals

GCSE/IGCSE Periodic Table Revision Notes

  GCSE/IGCSE Transition Metals Revision Notes

INORGANIC Part 10 3d block TRANSITION METALS sub–index: 10.1–10.2 Introduction 3d–block Transition Metals * 10.3 Scandium * 10.4 Titanium * 10.5 Vanadium * 10.6 Chromium * 10.7 Manganese * 10.8 Iron * 10.9  Cobalt * 10.10 Nickel * 10.11 Copper * 10.12 Zinc * 10.13 Other Transition Metals e.g. Ag and Pt * Appendix 1. Hydrated salts, acidity of hexa–aqua ions * Appendix 2. Complexes & ligands * Appendix 3. Complexes and isomerism * Appendix 4. Electron configuration & colour theory * Appendix 5. Redox equations, feasibility, E^ø * Appendix 6. Catalysis * Appendix 7. Redox equations * Appendix 8. Stability Constants and entropy changes * Appendix 9. Colorimetric analysis and complex ion formula * Appendix 10 3d block – extended data * Appendix 11 Some 3d–block compounds, complexes, oxidation states & electrode potentials * Appendix 12 Hydroxide complex precipitate 'pictures', formulae and equations

Advanced Level Inorganic Chemistry Periodic Table Index * Part 1 Periodic Table history * Part 2 Electron configurations, spectroscopy, hydrogen spectrum, ionisation energies * Part 3 Period 1 survey H to He * Part 4 Period 2 survey Li to Ne * Part 5 Period 3 survey Na to Ar * Part 6 Period 4 survey K to Kr and important trends down a group * Part 7 s–block Groups 1/2 Alkali Metals/Alkaline Earth Metals * Part 8  p–block Groups 3/13 to 0/18 * Part 9 Group 7/17 The Halogens * Part 10 3d block elements & Transition Metal Series * Part 11 Group & Series data & periodicity plots * All 11 Parts have their own sub–indexes near the top of the pages

Appendix 10 Extended DATA TABLE Extended SUMMARY FOR 3d BLOCK & TRANSITION METALS

• 3d block data notes:
  • Atomic and ionic radii are quoted in pm (1 picometre, 10^–12 m), 1000 pm = 1 nm (1 nanometre = 10^–9 m)
  • na means 'not applicable' or 'not available'.
  • The electronegativity values are from the Pauling scale.
  • Redox potentials
    • See Appendix 11 Some 3d–block compounds, complexes, oxidation states & electrode potentials
  • Ionic radii relate to the 'isolated' theoretical ion, NOT the hydrated aqueous ion.
  • Polarizing power is a measure of the ions charge density which has important chemical consequences e.g.
    • the bonding nature of metals with non–metals e.g. an ionic or a covalent MCl_n
    • and the acidity of the hydrated aqueous ion [M(H₂O)₆]ⁿ⁺_(aq) which is capable of donating protons.
  • The ion charge divided by the ionic radius of the 'isolated ion' is a 'reasonable' number scale for easy comparison of polarising power, and in the tables I've multiplied the charge/radius by 100 to make a suitable scale.
    • Obviously, the larger the charge, or the smaller the volume or radius, the greater the charge density or polarising power, this in turn leads to more covalent character in the e.g. chloride and increased acidity of the hexa–aqua–ion [M(H₂O)₆]ⁿ⁺_(aq). that is with increase in the n+ value.
  • Note that as the oxidation state of the transition metal increases,
    • i.e. increase in charge if an ionic compound, the greater the polarising power of the cation, which increases the covalent character of the compound, exemplified by comparing iron(II) and iron(III) compounds or complex ions
      • e.g. FeCl₂ is essentially an ionic compound and FeCl₃ is covalent in character,
    • the greater the polarising power of the central metal ion, the greater the acidity of the hexaaqua ion
      • e.g. [Fe(H₂O)₆]³⁺ is more acidic than [Fe(H₂O)₆]²⁺
        • Going from iron(II) to iron(III) involves an increases in cationic positive charge and decrease in radius of the 'isolated' central metal ion.
        • The decrease in radius is bound to result from the same nuclear charge of 26+ 'pulling in' 24 and 23 electrons respectively,
        • i.e. less electron density in the same quantum level, less space occupied.
        • For more details see Transition Metals Appendix 1 Acidity of hexaaqua–ions
    • Relative polarising power of Groups 1–3 ions for comparison with the 3d block ions above:

    • Group of the Periodic Table	Metal ion and ionic charge	ionic radius/pm	relative polarizing power = 100 x charge / radius
      1	Na+	98	1.0
      2	Mg2+	78	2.6
      3	Al3+	60	5.0
      1	K+	133	0.75
      2	Ca2+	106	1.9

    • Note the substantial increase in polarizing power of the cations across Period 3 from sodium to aluminium as the ion charge increases and the ionic radius decreases. From the data from Groups and 1 and 2 you can see the polarising power of similarly charged cation decreases down a group as the ionic radius increases.
  • –

Scandium * Titanium * Vanadium * Chromium * Manganese * Iron * Cobalt * Nickel * Copper * Zinc * Silver & Platinum

Introduction 3d–block Transition Metals * Appendix 1. Hydrated salts, acidity of hexa–aqua ions * Appendix 2. Complexes & ligands * Appendix 3. Complexes and isomerism * Appendix 4. Electron configuration & colour theory * Appendix 5. Redox equations, feasibility, E^ø * Appendix 6. Catalysis * Appendix 7. Redox equations * Appendix 8. Stability Constants and entropy changes * Appendix 9. Colorimetric analysis and complex ion formula * Appendix 10 3d block – extended data * Appendix 11 Some 3d–block compounds, complexes, oxidation states & electrode potentials * Appendix 12 Hydroxide complex precipitate 'pictures', formulae and equations

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