Doc Brown's Chemistry - Advanced Level Inorganic Chemistry Periodic Table Revision Notes – Transition Metals

Part 10. Transition Metals 3d–block

10.9 Cobalt Chemistry

The chemistry of the transition metal cobalt (most common oxidation states +2 and +3) is dominated by the stability of the cobalt(II) ion which forms a wide variety of stable complexes with most ligands such as water, ammonia, chloride ion etc. The cobalt(III) state can be stabilised by a suitable ligand and cobalt(III) complexes are usually made by oxidising a cobalt(II) salt in the presence of the stabilising ligand.

principal oxidation states of cobalt, redox reactions of cobalt, ligand substitution displacement reactions of cobalt, balanced equations of cobalt chemistry, formula of cobalt complex ions, shapes colours of cobalt complexes, formula of compounds


PLEASE NOTE this page on the 3d block transition metal cobalt is for Advanced A Level students ONLY!

Therefore it is IMPORTANT for GCSE/IGCSE/O Level students studying iron chemistry to go to  ...

(c) doc b GCSE/IGCSE Periodic Table Revision Notes  or   (c) doc b GCSE/IGCSE Transition Metals Revision Notes including cobalt

INORGANIC Part 10 The 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, Eø * 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


10.9. Chemistry of Cobalt Co, Z=27, 1s22s22p63s23p63d74s2 

data comparison of cobalt with the other members of the 3d–block and transition metals

Z and symbol 21 Sc 22 Ti 23 V 24 Cr 25 Mn 26 Fe 27 Co 28 Ni 29 Cu 30 Zn
property\name scandium titanium vanadium chromium manganese iron cobalt nickel copper zinc
melting point/oC 1541 1668 1910 1857 1246 1538 1495 1455 1083 420
density/gcm–3 2.99 4.54 6.11 7.19 7.33 7.87 8.90 8.90 8.92 7.13
atomic radius/pm 161 145 132 125 124 124 125 125 128 133
M2+ ionic radius/pm na 90 88 84 80 76 74 72 69 74
M3+ ionic radius/pm 81 76 74 69 66 64 63 62 na na
common oxidation states +3 only +2,3,4 +2,3,4,5 +2,3,6 +2,3,4,6,7 +2,3,6 +2,3 +2,+3 +1,2 +2 only
outer electron config [Ar]... 3d14s2 3d24s2 3d34s2 3d54s1 3d54s2 3d64s2 3d74s2 3d84s2 3d104s1 3d104s2
Elect. pot. M(s)/M2+(aq) na –1.63V –1.18V –0.90V –1.18V –0.44V –0.28V –0.26V +0.34V –0.76V
Elect. pot. M(s)/M3+(aq) –2.03V –1.21V –0.85V –0.74V –0.28V –0.04V +0.40 na na na
Elect. pot. M2+(aq)/M3+(aq) na –0.37V –0.26V –0.42V +1.52V +0.77V +1.87V na na na

Elect. pot. = standard electrode potential data for cobalt (EØ at 298K/25oC, 101kPa/1 atm.)

na = data not applicable to cobalt

Extended data table for COBALT

property of cobalt/unit value for Co
melting point Co/oC 1495
boiling point Co/oC 2870
density Co/gcm–3 8.90
1st Ionisation Energy/kJmol–1 760
2nd IE/kJmol–1 1646
3rd IE/kJmol–1 3232
4th IE/kJmol–1 4950
5th IE/kJmol–1 7670
atomic radius Co/pm 125
Co2+ ionic radius/pm 74
Relative polarising power Co2+ ion 2.7
Co3+ ionic radius/pm 63
Relative polarising power Co3+ ion 4.8
oxidation states of Co +2, +3
simple electron configuration of Co 2,8,15,2
outer electrons of Co [Ar]3d74s2
Electrode potential Co(s)/Co2+(aq) –0.28V
Electrode potential Co(s)/Co3+(aq) +0.40
Electrode potential Co2+(aq)/Co3+(aq) +1.87V
Electronegativity of Co 1.88

Advanced Inorganic Chemistry Page Index and Links

  • Uses of COBALT

    • Cobalt is a bluish–white solid that is malleable and ductile and ferromagnetic – hence its use in magnets.

    • Cobalt is alloyed with chromium and tungsten to make a metal (e.g. stellite alloy) hard enough, even at red heat, to be used for high speed cutting tools and valves for internal combustion engines.

    • The alloy alnico (Al + Ni + Co) is used to make extremely strong permanent magnets.

    • Cobalt compounds are used in paints e.g. cobalt blue.

    • Cobalt compounds are used as catalysts e.g. the cobalt carbonyl Co2(CO)8 is used to catalyse the hydroformulation reaction to produce an aldehyde or alcohol from an alkene.

  • Biological role of Cobalt

    • Cobalt is an essential trace element and found at the centre of the vitamin B12 (cobalamine, C63H88CoN14O14P). It contains a cobalt(III) ion and is necessary for the prevention of pernicious anaemia and the formation of red blood corpuscles, but it is involved many other functions too. Vitamin B12 is the largest and most complex of all the vitamins. The vitamin B12 group of molecules are the only cobalt-containing molecules (called 'cobalamins') associated with biochemistry of humans.  It is the cobalt(III) ion complex that gives this water-soluble vitamin its distinctive red colour. In essence it is a classic transition metal complex of cobalt with a nice colour! In school and college you are more likely to come across the more familiar pink or blue cobalt(II) complexes, so this is a good, if rather more complicated structure of a rarer cobalt(III) complex. When the B12 molecule is inactive the cobalt is in the +3 oxidation state, but when biochemically active it adopts oxidations states of + 1 in cobalt(I) complexes and +2 in a cobalt(II) complexes. Its all very complicated biochemistry !

    • In plants cobalt complexes are involved in nitrogen fixation by microorganisms (a cobalt ion in an enzyme?).


The Chemistry of COBALT

Pd s block d blocks and f blocks of metallic elements p block elements
Gp1 Gp2 Gp3/13 Gp4/14 Gp5/15 Gp6/16 Gp7/17 Gp0/18
1

1H

2He
2 3Li 4Be The modern Periodic Table of Elements

ZSymbol, z = atomic or proton number

3d block of metallic elements: Scandium to Zinc

5B 6C 7N 8O 9F 10Ne
3 11Na 12Mg 13Al 14Si 15P 16S 17Cl 18Ar
4 19K 20Ca 21Sc

[Ar]3d14s2

scandium

22Ti

[Ar]3d24s2

titanium

23V

 [Ar] 3d34s2

vanadium

24Cr

[Ar] 3d54s1

chromium

25Mn

   [Ar]   3d54s2

manganese

26Fe

[Ar] 3d64s2

iron

27Co

[Ar] 3d74s2

cobalt

28Ni

[Ar] 3d84s2

nickel

29Cu

[Ar] 3d104s1

copper

30Zn

[Ar] 3d104s2

zinc

31Ga 32Ge 33As 34Se 35Br 36Kr
5 37Rb 38Sr 39Y 40Zr 41Nb 42Mo 43Tc 44Ru 45Rh 46Pd 47Ag 48Cd 49In 50Sn 51Sb 52Te 53I 54Xe
6 55Cs 56Ba 57-71 72Hf 73Ta 74W 75Re 76Os 77Ir 78Pt 79Au 80Hg 81Tl 82Pb 83Bi 84Po 85At 86Rn
7 87Fr 88Ra 89-103 104Rf 105Db 106Sg 107Bh 108Hs 109Mt 110Ds 111Rg 112Cn 113Uut 114Fl 115Uup 116Lv 117Uus 118Uuo
  *********** *********** ************ ************ ************** ********** ********** ********** ********** **********  

  • The electrode potential chart highlights the values for various oxidation states of cobalt.

  • COBALT(II) chemistry

  • In aqueous solution, in the absence of complexing agents,

    • cobalt forms the stable pink hexaaqua cobalt(II) ion, [Co(H2O)6]2+(aq) 

    • Aqueous solutions of cobalt(II) sulfate CoSO4(aq) or cobalt(II) chloride CoCl2(aq) are suitable for laboratory experiments investigating the aqueous chemistry of the cobalt(II) ion.

  • With alkalis sodium hydroxide and ammonia, cobalt(II) ions produce the hydrated cobalt(II) hydroxide blue ppt. which turns pink on standing. There is no further reaction with excess of NaOH or Na2CO3, but see further down for excess NH3.

    • Co2+(aq) + 2OH(aq) ==> Co(OH)2(s)  (can be written as [Co(OH)2(H2O)4])

    •    (a precipitation reaction)

  • With alkaline aqueous sodium carbonate solutions cobalt(II) ions produces a precipitate of pink/blue? cobalt(II) carbonate.

    • Co2+(aq) + CO32–(aq) ==> CoCO3 (s) (maybe basic carbonate? – mixture of CoCO3 + Co(OH)2)

  • When excess ammonia is added to a cobalt(II) salt solution, the hexamine complex is formed BUT this is unstable in the presence of dissolved oxygen and is oxidised to the cobalt(III) complex. This change in cobalt's oxidation state from +2 to +3 via an oxidising agent is quite common if a complexing agent is present too.

    • [Co(H2O)6]2+(aq) + 6NH3(aq) ==> [Co(NH3)6]2+(aq) + 6H2O(l) 

    • pink hexaaquacobalt(II) ion == oxygen ==> brown hexaamminecobalt(II) ion.

      • The uncharged ligand molecules ammonia NH3 and water H2O are similar in size and ligand exchange occurs without change in co–ordination number (stays at 6).

      • Oxidation then follows from dissolved oxygen, or you can add hydrogen peroxide for a more efficient job!

    • (i) 4[Co(NH3)6]2+(aq) + O2(g/aq) + 4H+(aq) ==> 4[Co(NH3)6]3+(aq) + 2H2O(l)

    • (ii) 2[Co(NH3)6]2+(aq) + H2O2(g/aq) + 2H+(aq) ==> 2[Co(NH3)6]3+(aq) + 2H2O(l)

    • brown ==> colour? hexaamminecobalt(III) ion.

    • Oxidation state changes: in both (i) & (ii) Co from +2 to +3, (i) O from 0 to –2, (ii) O from –1 to –2.

      • +1.82V for [Co(H2O)6]3+(aq) + e rev [Co(H2O)6]2+(aq)

      • +0.10V for [Co(NH3)6]3+(aq) + e rev [ Co(NH3)6]2+(aq)

      • more EØ data & comments?

    • Comparison of the stability of the hexammine complexes irrespective of redox stability

      • [Co(H2O)6]2+(aq) + 6NH3(aq) ==> [Co(NH3)6]2+(aq) + 6H2O(l)

        • Kstab = {[Co(NH3)6]2+(aq)} / {[Co(H2O)6]2+(aq)} [NH3(aq)]6

        • Kstab = 7.7 x 104 mol–6 dm18  [lg(Kstab) = 4.9]

      • [Co(H2O)6]3+(aq) + 6NH3(aq) ==> [Co(NH3)6]3+(aq) + 6H2O(l)

        • Kstab = {[Co(NH3)6]3+(aq)} / {[Co(H2O)6]3+(aq)} [NH3(aq)]6

        • Kstab = 4.5 x 1033 mol–6 dm18  [lg(Kstab) = 33.7]

      • Note that the more highly charged Co3+(aq) ion complexes more strongly than the Co2+(aq) ion i.e. forms a more stable complex

  • VIEW ppts. with OH, NH3 and CO32–, & complexes, if any, with excess reagent.

  • When hydrogen peroxide is added to an alkaline cobalt(II) solution, oxidation occurs to give cobalt(III) complexes.

    • The air oxidation described above in alkaline ammonia solution can also be effected via hydrogen peroxide giving the hexa–amminecobalt(III) ion – described in detail above.

  • If e.g. sodium chloride or hydrochloric acid is added to cobalt(II) sulphate solution the blue tetrachlorocobaltate(II) complex ion is formed.

    • [Co(H2O)6]2+(aq) + 4Cl(aq) rev [CoCl4]2–(aq) + 6H2O(l) 

    • This particular ligand substitution/exchange reaction involves several changes (L to R):

      • the larger chloride ion ligand leads to a change in co–ordination number from 6 to 4,

      • the complex ion shape changes from octahedral to tetrahedral

      • the colour of the complex changes from pink to blue,

      • the complex changes from a cationic to an anionic ion.

      • There is no oxidation state change at all.

    • This is quite a good reaction to demonstrate Le Chatelier's equilibrium principles:

      • dilution shifts the equilibrium to the left, more pink,

      • increasing the chloride ion concentration shifts the equilibrium to the right, more blue,

      • increasing the solution temperature shifts the equilibrium to the right, more blue

      • or if prepared at higher temperature, with just enough chloride to turn the solution blue, on cooling it becomes pink,

      • this shows that left to right is endothermic and right to left is exothermic.

  • Summary of some complexes–compounds & oxidation states of cobalt compared to other 3d–block elements

  • COBALT(III) chemistry

    • As we have seen above the hexaaquacobalt(III) cation is unstable in aqueous solution but can be stabilised by suitable ligands.

    • One example has already been described in the introduction, namely the vitamin B12 complex.

    • The formation of [Co(NH3)6]3+ is described above and two other stable complex anions are with the ...

      • (i) , (ii)

      • (i) nitrate(III) ion (nitrite, ion NO2) it forms the anionic octahedral complex [Co(NO2)6]3–

      • (ii) cyanide ion CN it forms the anionic octahedral complex hexacyanocobaltate(III) ion [Co(CN)6]3–

  • Advanced Inorganic Chemistry Page Index and LinksIsomerism in cobalt(III) complexes e.g. with the ligands ammonia and chloride (i)–(iii)

    • (i) crystalline [Co(NH3)6]3+(Cl)3 is orange–yellow, no isomers possible

      • the hexaamminecobalt(III) ion

    • (ii) crystalline [Co(NH3)5Cl]2+(Cl)2 is violet, no isomers possible

    • (iii) crystalline [Co(NH3)4Cl2]+Cl is violet or green – there are two geometrical E/Z isomers (trans/cis)

      • (iii)(c) doc b

      • Geometrical isomerism diagrams: The Z and E (cis and trans geometrical isomers) isomeric octahedral complexes of the dichlorotetraamminecobalt(III) complex ion

      • (1) is the cis or Z isomer, (2) is the trans or E isomer

    • (iv) –

  • More examples of the complexes of cobalt(II) and cobalt(III)

    • Both the hexa–aqua ions of cobalt(II) and cobalt(III) readily complex with EDTA

      • [Co(H2O)6]2+(aq) + EDTA4–(aq) ===> [Co(EDTA)]2–(aq) + 6H2O(l)

        • Kstab = {[Co(EDTA)3]2–(aq)} / {[Co(H2O)6]2+(aq)} [EDTA4–(aq)]

        • Kstab = 2.0 x 1016 mol–1 dm3 [lg(Kstab) = 16.3]

      • [Co(H2O)6]3+(aq) + EDTA4–(aq) ===> [Co(EDTA)](aq) + 6H2O(l)

        • Kstab = {[Co(EDTA)3](aq)} / {[Co(H2O)6]3+(aq)} [EDTA4–(aq)]

        • Kstab = 1.0 x 1036 mol–1 dm3 [lg(Kstab) = 36.0]

      • Note that the more highly charged Co3+(aq) ion complexes more strongly than the Co2+(aq) ion.

    • The cobalt(II) ion complexes with 1,2–diaminoethane, a bidentate ligand

      • [Co(H2O)6]2+(aq) + 3en(aq) ==> [Co(en)3]2+(aq) + 6H2O(l)

      • Kstab = {[Co(en)3]2+(aq)} / {[Co(H2O)6]2+(aq)} [en(aq)]3

      • Kstab = 6.3 x 1013 mol–3 dm9 [lg(Kstab) = 13.8]

      • Note: en is an abbreviation for the ligands old name ethylenediamine

  • An example of homogeneous catalysis:

    • Cobalt(II) ions catalyse the oxidation of the 2,3–dihydroxybutandioate ion (acid/salt, old name 'tartaric/tartrate') to water, methanoate ion and carbon dioxide with hydrogen peroxide solution. The likely scheme of events is outlined below, the equations are NOT meant to be balanced.

    • Starting with the pink hexa–aqua Co2+ ion, which is a Co(II) complex 

      • and the carboxylate ion, OOCCH(OH)CH(OH)COO (bidentate 2– anionic ligand)

    • [Co(H2O)6]2+(aq) ==> [Co(OOCCH(OH)CH(OH)COO)3]4–(aq)  

      • the pink Co(II) complex changes ligand from water to the organic acid, but no change in oxidation state or co–ordination number, and I don't know its colour?, but it perhaps it doesn't exist long enough to be seen?

    • [Co(OOCCH(OH)CH(OH)COO)3]4–(aq) ==via H2O2==>  [Co(OOCCH(OH)CH(OH)COO)3]3–(aq)  

      • the Co(II)–acid complex is oxidised by the hydrogen peroxide to a Co(III) –acid complex which is green,

    • [Co(OOCCH(OH)CH(OH)COO)3]3–(aq) ==> [Co(H2O)6]2+(aq),H2O(l),HCOO(aq),CO2 (aq/g) 

      • the green Co(III) complex then breaks down to give the products,

      • and you see the bubbles of carbon dioxide and the 'return' of the pink hexa–aqua Co2+ complex ion.

    • In the above sequence, the change in ligand affects the relative stability of the oxidation states. The CoII–acid complex is stable as regards 'breakdown', but is readily oxidised to the CoIII–acid complex, which is NOT stable to breakdown.


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


PLEASE NOTE this page on the 3d block transition metal cobalt is for Advanced A Level students ONLY!

Therefore it is IMPORTANT for GCSE/IGCSE/O Level students studying iron chemistry to go to  ...

(c) doc b GCSE/IGCSE Periodic Table Revision Notes  or   (c) doc b GCSE/IGCSE Transition Metals Revision Notes including cobalt


biological role of cobalt vitamin B12, cobalt(II) chemistry, shape and formula of complexes of cobalt(II) Co2+, ammonia ligand, chloride ion as a ligand, complexes of cobalt with ammonia, oxidation of cobalt(II) ion Co2+ to the cobalt(III) ion Co3+ with hydrogen peroxide, tetrahedral complex of Co2+ with chloride ion, colour and structure of cobalt(III) Co3+ complexes, formula of EDTA complexes of cobalt physical and chemical properties of the 3d block transition metal cobalt, oxidation and reduction reactions of cobalt ions, outer electronic configurations of cobalt, principal oxidation states of cobalt, shapes of cobalt's complexes, octahedral complexes of cobalt, tetrahedral complexes of cobalt, square planar complexes of cobalt, stability data for cobalt's complexes, aqueous chemistry of cobalt ions, redox reactions of cobalt ions, physical properties of cobalt, melting point of cobalt, boiling point of cobalt, electronegativity of cobalt, density of cobalt, atomic radius of cobalt, ion radius of cobalt, ionic radii of cobalt's ions, common oxidation states of cobalt, standard electrode potential data for cobalt, ionisation energies of cobalt, polarising power of cobalt ions, industrial applications of cobalt compounds, chemical properties of cobalt compounds, why are cobalt complexes coloured?, isomerism in the complexes of cobalt, formulae of cobalt compounds, tests for cobalt ions keywords redox reactions ligand substitution displacement balanced equations formula complex ions complexes ligand exchange reactions redox reactions ligands colours oxidation states: cobalt ions Co(0) Co2+ Co(+2) Co(II) Co3+ Co(+3) Co(III) CoCl2 CoSO4 Co2+ + 2OH– ==> Co(OH)2 Co2+ + CO32– ==> CoCO3  [Co(H2O)6]2+ + 6NH3 ==> [Co(NH3)6]2+ + 6H2O  4[Co(NH3)6]2+ + O2(g/aq) + 4H+ ==> 4[Co(NH3)6]3+ + 2H2O (ii) 2[Co(NH3)6]2+ + H2O2(g/aq) + 2H+ ==> 2[Co(NH3)6]3+ + 2H2O +1.82V for [Co(H2O)6]3+ + e– [Co(H2O)6]2+ +0.10V for [Co(NH3)6]3+ + e– [Co(NH3)6]2+ [Co(H2O)6]2+ + 6NH3 ==> [Co(NH3)6]2+ + 6H2O Kstab = {[Co(NH3)6]2+} / {[Co(H2O)6]2+} [NH3]6 Kstab = 7.7 x 104 mol–6 dm18 [lg(Kstab) = 4.9] [Co(H2O)6]3+ + 6NH3 ==> [Co(NH3)6]3+ + 6H2O Kstab = {[Co(NH3)6]3+} / {[Co(H2O)6]3+} [NH3]6 Kstab mol–6 dm18 [lg(Kstab) = 33.7] [Co(H2O)6]2+ + 4Cl– [CoCl4]2– + 6H2O [Co(NH3)6]3+ [Co(NO2)6]3– [Co(CN)6]3– [Co(NH3)6]3+(Cl–)3 [Co(NH3)5Cl]2+(Cl–)2 [Co(NH3)4Cl2]+Cl– [Co(H2O)6]2+ + EDTA4– ===> [Co(EDTA)]2– + 6H2O Kstab = {[Co(EDTA)3]2–} / {[Co (H2O)6]2+} [EDTA4–] Kstab = 2.0 x 1016 mol–1 dm3 [lg(Kstab) = 16.3] [Co(H2O)6]3+ + EDTA4– ===> [Co(EDTA)]– + 6H2O Kstab = {[Co(EDTA)3]–} / {[Co(H2O)6]3+} [EDTA4–] Kstab = 1.0 x 1036 mol–1 dm3 [lg(Kstab) = 36.0] [Co(H2O)6]2+ + 3en ==> [Co (en)3]2+ + 6H2O Kstab = {[Co(en)3]2+} / {[Co(H2O)6]2+} [en]3 [Co(H2O)6]2+ + 3en ==> [Co(en)3]2+ + 6H2O Kstab = {[Co(en)3]2+} / {[Co(H2O)6]2+} [en]3 [Co(OOCCH(OH)CH(OH)COO)3]4– ==via H2O2==> [Co(OOCCH(OH)CH(OH)COO)3]3– [Co(OOCCH(OH)CH(OH)COO)3]3– ==> [Co(H2O)6]2+,H2O,HCOO–,CO2 oxidation states of cobalt, redox reactions of cobalt, ligand substitution displacement reactions of cobalt, balanced equations of cobalt chemistry, formula of cobalt complex ions, shapes colours of cobalt complexes  Na2CO3 NaOH NH3 cobalt chemistry for AQA AS chemistry, cobalt chemistry for Edexcel A level AS chemistry, cobalt chemistry for A level OCR AS chemistry A, cobalt chemistry for OCR Salters AS chemistry B, cobalt chemistry for AQA A level chemistry, cobalt chemistry for A level Edexcel A level chemistry, cobalt chemistry for OCR A level chemistry A, cobalt chemistry for A level OCR Salters A level chemistry B cobalt chemistry for US Honours grade 11 grade 12 cobalt chemistry for pre-university chemistry courses pre-university A level revision notes for cobalt chemistry  A level guide notes on cobalt chemistry for schools colleges academies science course tutors images pictures diagrams for cobalt chemistry A level chemistry revision notes on cobalt chemistry for revising module topics notes to help on understanding of cobalt chemistry university courses in science careers in science jobs in the industry laboratory assistant apprenticeships technical internships USA US grade 11 grade 11 AQA A level chemistry notes on cobalt chemistry Edexcel A level chemistry notes on cobalt chemistry for OCR A level chemistry notes WJEC A level chemistry notes on cobalt chemistry CCEA/CEA A level chemistry notes on cobalt chemistry for university entrance examinations


ALPHABETICAL SITE INDEX for chemistry     

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, Eø * 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


PLEASE NOTE this page on the 3d block transition metal cobalt is for Advanced A Level students ONLY!

Therefore it is IMPORTANT for GCSE/IGCSE/O Level students studying iron chemistry to go to  ...

(c) doc b GCSE/IGCSE Periodic Table Revision Notes  or   (c) doc b GCSE/IGCSE Transition Metals Revision Notes including cobalt

 Doc Brown's Chemistry 

*

For latest updates see https://twitter.com/docbrownchem

TOP OF PAGE

visits since January 2000