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3d block chemistry of zinc revision notes for Advanced level pre-university inorganic chemistry students

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colourless hexaaquazinc ion octahedral complex with waterInorganic chemistry Part 10. Transition Metals 3d–block

10.12 Zinc Chemistry  - a 3d block element (not a transition element)

[Author ©  Dr Phil Brown PhD: Doc Brown's Chemistry exam revision notes suitable for students of advanced pre-university A level inorganic chemistry for AQA, Edexcel, OCR, Salters, WJEC, CCEA, IB and US grade 11-12 courses: Periodic Table - 3D block and 1st transition metal series: chemistry of zinc and its compounds [page updated May 4th 2026 *]

Sub-index for this page on the chemistry of zinc - a 3d block element

1. Introduction to the chemistry of zinc

2. Data tables for the chemistry of zinc

3. Uses of zinc and its biological role

4. The colour of zinc compounds

5. Electron configuration, oxidation states and electrode potentials

6. The chemistry of zinc and its simple compounds and complexes

7. The extraction and purification of zinc

8. The vertical connection of zinc with the other d-block elements of Group 12 (IUPAC designation)

9. Learning objectives for the chemistry of zinc

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1. Introduction to the chemistry of zinc - a 3d block element

Zinc is the head-top element of Group 12 of the periodic table (modern IUPAC assignment).

Zinc is a member of the 3d–block of elements BUT why isn't zinc a true transition metal?

Zinc cannot form a stable ion with an incomplete d sub–shell and is therefore not a true transition element. Zinc's chemistry is determined solely by the formation of compounds in its +2 oxidation state, but it does form many complexes, though not as many as other transition metals.

The only oxidation state of zinc is +2, so there is a much more limited chemistry in terms of redox reactions of zinc, ligand substitution displacement reactions of zinc, balanced equations of zinc chemistry, formula of zinc complex ions, shapes colours of zinc complexes, formula of compounds compared to true transition metals.

2. Data for 10.12. Chemistry of Zinc Zn, Z=30, 1s22s22p63s23p63d104s2 

Data comparison of zinc 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
EŘ M(s)/M2+(aq) na –1.63V –1.18V –0.90V –1.18V –0.44V –0.28V –0.26V +0.34V –0.76V
EŘ M(s)/M3+(aq) –2.03V –1.21V –0.85V –0.74V –0.28V –0.04V +0.40 na na na
EŘ 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 zinc (EŘ at 298K/25oC, 101kPa/1 atm.)

na = data not applicable to zinc

Extended data table for ZINC

property of zinc/unit value for Zn
melting point Zn/oC 420
boiling point Zn/oC 907
density Zn/gcm–3 7.13
1st Ionisation Energy/kJmol–1 906
2nd IE/kJmol–1 1733
3rd IE/kJmol–1 3832
4th IE/kJmol–1 5730
5th IE/kJmol–1 7970
Zn atomic radius/pm 133
Zn2+ ionic radius/pm 74
Relative polarising power Zn2+ ion 2.7
oxidation state of Zn +2 only
simple electron configuration of Zn 2,8,18,2
outer electrons of Zn [beyond argon core] [Ar]3d104s2
Electrode potential Zn(s)/Zn2+(aq) –0.76V
Electronegativity of Zn 1.65

3. Uses of zinc and its biological role

  • Uses of ZINC

    • Zinc is a greyish silvery white metal which is quite brittle at room temperature.

    • Zinc is a good conductor of heat and electricity.

    • Zinc slowly reacts with oxygen and water, but quite fast with acids.

    • Zinc is used in zinc–carbon batteries, as is zinc chloride, ZnCl2. (in the 'paste')

    • Zinc is alloyed with copper to make brass.

    • Zinc sulfide, ZnS, is used in paint manufacture.

    • Zinc oxide, ZnO is used in rubber manufacture.

    • Covalent organometallic zinc compounds (ZnR2) are used as catalysts in polymer production.

    • A solution of zinc sulfate, ZnSO4, is used in zinc plating as anti–corrosion treatment of other metals like steel.

    • Zinc chloride is also used in wood preservatives.

    • The phosphor Zn2SiO4:Mn is involved in the manufacture of night vision devices.

  • Biological role of zinc

    • Zinc is an essential trace element and is a co–factor in the operation of many enzymes such as lactic dehydrogenase.

    • In plants, zinc ions activate carboxylases and leaves may be malformed if there is a zinc deficiency in a plant.

4. The colour of zinc compounds

  • Most zinc compounds and complex ions (Zn only exhibits a +2 oxidation state in them) are white or colourless.

  • You can add different ligands, apart from water [Zn(H2O)4]2+, like ammonia [Zn(NH3)4]2+, or chloride ion [ZnCl4]2- , or cyanide ion [Zn(CN)4]2-, but no coloured complex is observed, simple experiments to do (but NOT with cyanide!).

  • Even with hydroxide ions, the initial hydroxide precipitate complex is white, and with excess alkali you get the colourless 'zincate' ion [Zn(OH)4]2-.

  • The lack of scope for a variety of coloured compounds arises from the fundamental electronic configuration of the Zn2+ ion, namely [Ar]3d10, giving a completely filled 3d sub–shell.

  • i.e. there is no electron that can be promoted to a higher level when the 3d sub–shell is split when the central metal ion interacts with the ligands. See 1st electronic diagram below.

  • Bottom right shows the ground state of the zinc(II) ion, and clearly, no electron can be promoted in the 3d sub-levels, so no absorption of visible light photons, no colour from transmitted visible light!

  • diagram showing the 3d orbital splitting in the zinc(II) ion, Zn2+

  • The 2nd electronic diagram (above), shows the possible electronic transitions, whose ∆E photon absorption is in the visible region of the electromagnetic spectrum.

  • Even though zinc is a member of the 3d block of elements, this is why zinc is NOT a true member of the first transition metal series, it forms no ion with a partly filled 3d sub–shell.

  • For more details see Appendix 4. Electron configuration & complex ion colour theory

5. The Chemistry of ZINC - electron configuration, oxidation states and electrode potentials

Some basic reactions of zinc metal, oxide and carbonate are on the GCSE Reactivity Series of Metals Notes

Pd s block d blocks (3d block zinc) and f blocks of metallic elements p block elements
Gp1 Gp2 Gp3/13 Gp4/14
1

1H
2 3Li 4Be Part of the modern Periodic Table of Elements: ZSymbol, z = atomic or proton number

Sc to Zn are now considered the head-top elements of groups 3 to 12

3d block of metallic elements: Scandium to Zinc Sc-Zn focus on zinc

5B 6C
3 11Na 12Mg 13Al 14Si
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
5 37Rb 38Sr 39Y 40Zr 41Nb 42Mo 43Tc 44Ru 45Rh 46Pd 47Ag 48Cd 49In 50Sn
6 55Cs 56Ba 57,58-71 72Hf 73Ta 74W 75Re 76Os 77Ir 78Pt 79Au 80Hg 81Tl 82Pb
7 87Fr 88Ra 89,90-103 104Rf 105Db 106Sg 107Bh 108Hs 109Mt 110Ds 111Rg 112Cn 113Nh 114Fl

 

Summary of oxidation states of the 3d block metals (least important) Ti to Cu are true transition metals
Group 3 Group 4 Group 5 Group 6 Group 7 Group 8 Group 9 Group 10 Gp 11 Group 12
Sc Ti V Cr Mn Fe Co Ni Cu Zn
                +1  
  (+2) (+2) (+2) +2 +2 +2 +2 +2 +2 (3d10)
+3 +3 +3 +3 (+3) +3 +3 (+3) (+3)  
  +4 +4   +4     (+4)    
    +5              
      +6 (+6) (+6)        
        +7          
3d14s2 3d24s2 3d34s2 3d54s1 3d54s2 3d64s2 3d74s2 3d84s2 3d104s1 3d104s2
Outer electron configurations beyond [Ar] for the ground state of the simple atom (ion configuration)

Note that when 3d block elements form ions, the 4s electrons are 'lost' first.

The oxidation state (+2 only) and electron configuration of zinc in the context of the 3d block of elements

Electrode potential chart for zinc the context of the 3d block transition metals

electrode potential chart diagram show position of Zn/Zn2+ in the context of the 3d block transition metalszinc

The electrode potential chart highlights the value for the one positive oxidation state of zinc.

PLEASE note: The electrode potentials (EŘ) for zinc chemistry in the text sometimes vary from the chart above - apologies, but data sources for zinc chemistry can vary! Any discrepancy shouldn't significantly affect any electrode potential calculation outcomes e.g feasibility (email if concerned?).

6. The chemistry of zinc and its simple compounds and complexes

  • Although a member of the 3d–block, zinc is NOT a true transition metal.

  • Zinc metal readily dissolves in dilute hydrochloric acid or dilute sulfuric acid reducing hydrogen ions to hydrogen gas.

    • Zn(s) + 2H+(aq) ===> Zn2+(aq) + H2(g)

  • The Zn2+ ion has a full sub–shell, 3d10, which does not allow the electronic transitions which account for the colour in transition metal compounds.

  • In aqueous solution zinc forms the colourless stable hydrated zinc ion, [Zn(H2O)6]2+(aq) and most complexes of the zinc ion have a co–ordination number of 6.

    • Solutions of zinc sulfate ZnSO4(aq) or zinc chloride ZnCl2(aq) are suitable for laboratory experiments for investigating the aqueous chemistry of the zinc ion..

  • The alkalis sodium hydroxide or ammonia, produce the hydrated white gelatinous zinc hydroxide precipitate. There is a further reaction with excess of NaOH or NH3.

    • Zn2+(aq) + 2OH–(aq) ===> Zn(OH)2(s)  (can be written as [Zn(OH)2(H2O)2]0

    • or  [Zn(H2O)6]2+(aq)  + 2OH–(aq) rev Zn(OH)2(aq) +  6H2O(l)

    •  A precipitation reaction which you can expression via various equations!

  • Zinc ions with excess sodium hydroxide:

    • (i) [Zn(H2O)6]2+(aq)  + 4OH–(aq) rev [Zn(OH)4]2–(aq) + 6H2O(l)  (from original aqueous ion)

    • or (ii) Zn(OH)2(s) + 2OH–(aq) rev [Zn(OH)4]2–(aq)  (from hydroxide ppt.)

      • For (i) the formation of tetrahydroxozincate ion is a ligand exchange reaction (hydroxide ion for water) with change in shape (octahedral to tetrahedral), change in co-ordination number (from 6 to 4), but no change in oxidation state of zinc (+2). However the overall charge on the zinc complex changes from 2+ to 2- (2+ 4x-1).

    • In fact zinc oxide is a classic amphoteric oxide e.g. giving a 'zincate' ion with alkali and a chloride salt with hydrochloric acid.

      • ZnO(s) + 2NaOH(aq) + H2O(l) ===> Na2Zn(OH)4(aq)

      • ZnO(s) + 2HCl(aq) ===> ZnCl2(aq) + H2O(l)

  • Zinc ions with excess ammonia:

    • [Zn(H2O)6]2+(aq) + 4NH3(aq) rev [Zn(NH3)4]2+(aq) + 6H2O(l) 

    • (formation from original aqueous ion)

    • The formation of the tetraammine zinc(II) ion is a ligand exchange reaction (ammonia for water) with change in shape (octahedral to tetrahedral), co-ordination number changes (from 6 to 4), but no change in the oxidation state of zinc (+2) or overall change in the net charge on the zinc complex ion (2+, since both ligands involved are neutral).

    • or  Zn(OH)2(s)  + 4NH3(aq) rev [Zn(NH3)4]2+(aq) + 2OH–(aq) (from hydroxide precipitate)

      • The ammonia ligand displaces the water/hydroxide ion ligands.

  • With aqueous of sodium carbonate zinc ion solutions produce a precipitate of white zinc carbonate, but its a basic carbonate, i.e. the carbonate precipitate is mixed with zinc hydroxide, Zn(OH)2.

    • Zn2+(aq) + CO32–(aq) ===> ZnCO3(s) 

    • better prepared using less alkaline NaHCO3:

    • Zn2+(aq) + 2HCO3–(aq) ===> ZnCO3(s) + H2O(l) + CO2(g) 

  • Some examples of zinc complex ion formation

    • The variation of the stability constant with change in ligand is illustrated with the zinc ion.

    • The data set for zinc compares five different monodentate ligands and the polydentate ligand EDTA.

    • Apart from the EDTA complex the stability constant (Kstab) equilibrium expression is

    • Kstab = [[ZnL4]2+/2–(aq)] / [[Zn(H2O)4]2+(aq)] [[L(aq)]4] mol–4dm12  (equations below)

    • Remember [H2O] is not included in the equilibrium expression.

    • The data also assumes a ligand coordination number of 4 for all the complexes involved.

    • Many of the species involving the hydrated zinc ion can be partially substituted and hydrated and exist as octahedral complexes, but I've ignored these complications and denoted the end product in terms of the ligand substitution i.e. the water ligand exchanged for CN-, NH3, X- (halide).

Ligand substitution reaction to give new complex ion Kstab lg Kstab
[Zn(H2O)4]2+(aq) + 4CN–(aq) ==> Zn(CN)4]2–(aq) + 4H2O(l) 5.0 x 1016 16.7
[Zn(H2O)4]2+(aq) + 4NH3(aq) ==> Zn(NH3)4]2–(aq) + 4H2O(l) 3.8 x 109 9.58
[Zn(H2O)4]2+(aq) + 4Cl–(aq) ==> [ZnCl4]2–(aq) + 4H2O(l) 1.0 0.0
[Zn(H2O)4]2+(aq) + 4Br–(aq) ==> [ZnBr4]2–(aq) + 4H2O(l) 10–1 –1.0
[Zn(H2O)4]2+(aq) + 4I–(aq) ==> [ZnI4]2–(aq) + 4H2O(l) 10–2 –2.0
[Zn(H2O)4]2+(aq) + EDTA4–(aq) ==> [ZnEDTA]2–(aq) + 4H2O(l) 3.2 x 1016 16.5

  • The very high value for the tetracyanozincate(II) in reflects the strong of central metal ion (Zn2+) - ligand (CN) bond.

  • The lower Kstab value for ammonia indicates on average a weaker dative covalent bond.

  • The ligand bonds are even weaker for the halide ions possibly due to their larger radius, since there is a steady decrease in Kstab as the halide radius increases, making the Zn–X dative covalent bond longer and weaker.

  • The stability constant for the zinc–EDTA complex is a very high value, typical for a polydentate ligand (see Appendix 8).

7. The Extraction and Purification of Zinc

  • Zinc is extracted from either zinc blende/sphalerite ore (zinc sulfide) or sometimes calamine/Smithsonite ore (zinc carbonate).
  • (1) The zinc sulfide ore is roasted in air to give impure zinc oxide.
    • 2ZnS(s) + 3O2(g) ==> 2ZnO(s) + 2SO2(g)
    • Note: calamine ore can be used directly in a zinc smelter because on heating it also forms zinc oxide.
      • ZnCO3(s)  ==> ZnO(s) + CO2(g) (endothermic thermal decomposition)
  • (2) The impure zinc oxide can be treated in two ways to extract the zinc:
    • (a) It is roasted in a smelting furnace with carbon (coke, reducing agent) and limestone (to remove the acidic impurities).
      • C(s) + O2(g) ==> CO2(g) (very exothermic oxidation, raises temperature considerably)
      • C(s) + CO2(g) ==> 2CO(g) (C oxidised, CO2 reduced)
      • ZnO(s) + CO(g) ==> Zn(l) + CO2(g) (zinc oxide reduced by CO, Zn undergoes O loss)
      • or direct reduction by carbon:
      • ZnO(s) + C(s) ==> Zn(l) + CO(g) (ZnO reduced, C oxidised)
      • The carbon monoxide acts as the reducing agent i.e. it removes the oxygen from the oxide.
      • The impure zinc is  then fractionally distilled from the mixture of slag and other metals like lead and cadmium out of the top of the furnace in an atmosphere rich in carbon monoxide which stops any zinc from being oxidised back to zinc oxide.
      • The slag and lead (with other metals like cadmium) form two layers which can be tapped off at the base of the furnace.
      • The zinc can be further purified by a 2nd fractional distillation or more likely by dissolving it in dilute sulfuric acid and purified electrolytically as described below.
    • (b) Two stages
      • (i) It is dissolved and neutralised with dilute sulfuric acid to form impure zinc sulfate solution.
      • ZnO(s) + H2SO4(aq) ==> ZnSO4(aq) + H2O(l)
      • or using calamine ore/zinc carbonate directly:
        • ZnCO3(s) + H2SO4(aq) ==> ZnSO4(aq) + H2O(l)+ CO2(g)
      • (ii) Quite pure zinc is produced from the solution by electrolysis. It can be deposited on a pure zinc negative electrode (cathode) in the same way copper can be purified. The other electrode, must be inert e.g. for laboratory experiments, carbon (graphite) can be used and oxygen is formed.
      • Zn2+(aq) + 2e– ==> Zn(s)
      • A reduction process, electron gain, as zinc metal is deposited on the (–) electrode.
      • You can't use solid zinc oxide directly because its insoluble and the ions must free to carry the current and migrate to the electrodes in some sort of solution.
      • For more details of the type of electrolysis system used, see purification of copper (just swap Zn for Cu in the method/diagram).
      • PLEASE note: In the industrial production of zinc by electrolysis (called electro–winning) the negative (–) cathode is made of aluminium (Al, where zinc deposits) and the positive (+) electrode is made of a lead–silver alloy (Pb–Ag, where oxygen gas is formed). Why these particular electrode metals are used in this 'electrowinning' process I'm not quite sure, but aluminium is so unreactive that it is effectively inert, and lead and silver are also of low activity, but ... ???

8. The vertical connection of zinc with the other d-block elements of Group 12 (IUPAC designation)

Modern IUPAC group numbers of 3-12 Outer electron structure of d-block elements which includes the transition metals

Zinc is the head element of Group 12 plus Cadmium, Mercury and Copernicium

Their outer electron configurations are nd10(n+1)s2 (n = 3 to 6)
[e- core] Gp 3 Group 4 Group 5 Group 6 Group 7 Group 8 Group 9 Group 10 Group 11 Gp 12
P'd 4, 3d block [Ar] core 21Sc

3d14s2

 22Ti

3d24s2

 23V

3d34s2

 24Cr

3d54s1

 25Mn

3d54s2

 26Fe

3d64s2

 27Co

3d74s2

 28Ni

3d84s2

 29Cu

3d104s1

 30Zn

3d104s2
P'd 5, 4d block (Kr] core 39Y

4d15s2

 40Zr

4d25s2

 41Nb

4d45s1

 42Mo

4d55s1

 43Tc

4d55s2

 44Ru

4d75s1

 45Rh

4d85s1

 46Pd

4d10

 47Ag

4d105s1

 48Cd

4d105s2
P'd 6, 5d b'k  [Xe] core 57La

5d16s2

 72Hf

4f145d26s2

 73Ta

4f145d36s2

 74W

4f145d46s2

 75Re

4f145d56s2

 76Os

4f145d66s2

 77Ir

4f145d76s2

 78Pt

4f145d96s1

 79Au

4f145d106s1

 80Hg

4f145d106s2
P'd 7, 6d b'k [Rn] core 89Ac

6d17s2

 104Rf

5f146d27s2

 105Db

5f146d37s2

 106Sg

5f146d47s2

 107Bh

5f146d57s2

 108Hs

5f146d67s2

 109Mt

5f146d77s2

 110Ds

5f146d87s2

 111Rg

5f146d97s2

 112Cn

5f146d107s2

You would expect some similarities between the chemistry of zinc, cadmium and mercury, but there are many significant differences too.

They have an outer electron configuration of d10s2.

Learning objectives for the chemistry of the 3d block metal zinc

Zinc is the top-head element of group 3 (modern IUPAC convention).

Know that zinc is a 3d block element because it has an electron in the 3d inner shell.

Know that zinc has relatively high melting point, boiling point and density.

Zinc does NOT comply with the definition of a transition metal, because it cannot form at least one ion with partially filled d sub–shell containing at least one electron.

Know how to work out the electron configurations of zinc and its ion, Zn2+.(the only +2 oxidation state)

Know that zinc does NOT display compounds or ions in several oxidation states.

Be able to relate the oxidation state of zinc to its electron configuration.

Know that most zinc ions/compounds are usually colourless because the Zn2+ has a 3d10 configuration and absorption in the visible spectrum is not possible, any colour will be due to a coloured anion or ligand.

It is quite electropositive metal and readily dissolves in acids to give zinc salts.

Zinc sulfate is used in electroplating to provide an anti-rusting coated on iron/steel surfaces.

The zinc ion is an important ingredient in our diet and is at the heart of the active site in several enzymes.

Know that zinc can form complex ions, but not with the variety of ligands and colours of true transition metal ions.

Know that aqueous solutions of zinc salts give a white hydroxide precipitate that dissolves in excess hydroxide ion or ammonia, and be able to write equations for these reactions.

Know that zinc and its compounds do NOT display the catalytic properties of true transition metals.

WHAT NEXT?

 GCSE Level Notes on Transition Metals (for the basics)

The chemistry of Scandium * Titanium * Vanadium * Chromium * Manganese

The chemistry of 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, Eř * 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 Some pages have a matching sub-index

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

Group numbering and the modern periodic table

The original group numbers of the periodic table ran from group 1 alkali metals to group 0 noble gases. To account for the d block elements and their 'vertical' similarities, in the modern periodic table, groups 3 to group 0 are numbered 13 to 18. So, the p block elements are referred to as groups 13 to group 18 at a higher academic level, though the group 3 to 0 notation is still used, but usually at a lower academic level. The 3d block elements (Sc to Zn) are now considered the head (top) elements of groups 3 to 12.

keywords redox reactions ligand substitution displacement balanced equations formula complex ions complexes ligands colours oxidation states: zinc ions Zn(0) Zn2+ Zn(+2) ZnSO4 ZnCl2 ZnO [Zn(H2O)4]2+ + 4 OH– [Zn(OH)4]2– Zn(OH)2 + 2OH– [Zn(OH)4]2– [Zn(H2O)4]2+ + 4 NH3 [Zn(NH3)4]2+ + 4H2O Zn(OH)2 + 4NH3 [Zn(NH3)4]2+ + 2OH– Zn2+ + 2 HCO3– ==> ZnCO3 + H2O + CO2 Ligand substitution reaction to give new complex ion [Zn(H2O)4]2+ + 4CN– ==> Zn(CN)4]2– + 4H2O [Zn(H2O)4]2+ + 4NH3 ==> Zn(NH3)4]2– + 4H2O [Zn(H2O)4]2+ + 4Cl– ==> [ZnCl4]2– + 4H2O [Zn(H2O)4]2+ + 4Br– ==> [ZnBr4]2– + 4H2O [Zn(H2O)4]2+ + 4 CN– ==> [Zn(CN)4]2– + 4H2O [Zn(H2O)4]2+ + EDTA4– ==> [ZnEDTA]2– + 4H2O oxidation states of zinc, redox reactions of zinc, ligand substitution displacement reactions of zinc, balanced equations of zinc chemistry, formula of zinc complex ions, shapes colours of zinc complexes  Na2CO3 NaOH NH3 Website content © Dr Phil Brown 2000+. All copyrights reserved on revision notes, images, quizzes, worksheets etc. Copying of website material is NOT permitted. Doc Brown's Chemistry inorganic chemistry revision notes for pre-university level students on 3d-block elements including the physical and chemical properties reactions equations and trends explained for the 3d-block of transition metals series Explaining the importance of chemistry of zinc in inorganic chemistry, What you need to know about chemistry of zinc for inorganic chemistry, Explaining the use of chemistry of zinc knowledge in inorganic chemistry, Examples of chemistry of zinc explained when studying inorganic chemistry, What is the significance of chemistry of zinc in inorganic chemistry, What is the use of chemistry of zinc in inorganic chemistry  Describing and explaining the theory of chemistry of zinc when studying inorganic chemistry, exam revision notes for chemistry of zinc in exams, online help for chemistry of zinc, revision notes for chemistry of zinc, what do I need to learn for chemistry of zinc in exams? revision summary for chemistry of zinc, help in teaching chemistry of zinc, learning notes for chemistry of zinc, help to pass the chemistry of zinc exam, how to prepare for examination questions on chemistry of zinc? Website content © Dr Phil Brown 2000+. All copyrights reserved on revision notes, images, quizzes, worksheets etc. Copying of website material is NOT permitted. Exam revision summaries & references to science course specifications are unofficial. Website content © Dr Phil Brown 2000+. All copyrights reserved on these organic chemistry exam revision notes on chemistry of zinc, these A level chemistry revision notes are suitable for use of pre-university students studying AQA advanced A level inorganic chemistry revision notes on chemistry of zinc, Edexcel advanced A level inorganic chemistry revision notes on chemistry of zinc, OCR advanced A level inorganic chemistry revision notes on chemistry of zinc, IB advanced A level inorganic chemistry revision notes on chemistry of zinc, WJEC (Eduqas) advanced A level inorganic chemistry revision notes on chemistry of zinc, CIE Cambridge advanced A level inorganic chemistry revision notes on chemistry of zinc, CCEA advanced A level inorganic chemistry revision notes on chemistry of zinc, and useful for US grade 11 grade 12 AP honors inorganic chemistry courses involving chemistry of zinc

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