Complete Revision of Coordination Compounds Class 12th JEE & NEET
Basic Concepts
1.Q:What is a coordination compound?
A:A compound containing a central metal atom/ion bonded to ligands via coordinate bonds.
2. Q: What is a ligand?
A: An ion or molecule that donates a lone pair of electrons to the central metal atom/ion.
3. Q:What is coordination number?
A:The number of ligand donor atoms directly bonded to the central metal ion.
4. Q:What are monodentate ligands?
A:Ligands that donate only one pair of electrons (e.g., NH₃, H₂O, Cl⁻).
5. Q:Give an example of a polydentate ligand.
A: Ethylenediamine (en), Oxalate (C₂O₄²⁻).
6. Q:What is a chelating ligand?
A: A ligand that forms two or more coordinate bonds with the same central metal ion.
7. Q:What is the oxidation number of Co in [Co(NH₃)₆]Cl₃?
A: +3.
8. Q:What is the difference between inner and outer orbital complexes?
A:Inner orbital uses (n-1)d orbitals, outer orbital uses nd orbitals for hybridization.
9. Q: What is EAN rule?
A:Effective Atomic Number = Atomic number of metal + electrons donated by ligands – oxidation state.
10. Q: Which law explains isomerism in coordination compounds?
A: Werner’s coordination theory.
Nomenclature
11. Q: What is the name of [Cr(H₂O)₆]Cl₃?
A: Hexaaquachromium(III) chloride.
12. Q:Write the formula of potassium ferrocyanide.
A: K₄[Fe(CN)₆].
13. Q:Name [Ni(CO)₄].
A:Tetracarbonylnickel(0).
14. Q:Give the name of [Pt(NH₃)₂Cl₂].
A: Diamminedichloroplatinum(II).
15. Q: Name [Cu(NH₃)₄]SO₄.
A: Tetraamminecopper(II) sulfate.
Isomerism
16.Q: What type of isomerism is shown by [Co(NH₃)₅Cl]SO₄ and [Co(NH₃)₅SO₄]Cl?
A: Ionization isomerism.
17. Q: Name the isomerism in [Co(en)₃]Cl₃.
18. Q: [Pt(NH₃)₂Cl₂] shows which type of isomerism?
A:Geometrical isomerism (cis/trans).
19. Q:What type of isomerism is shown when one ligand changes its point of attachment?
20. Q:Give an example of coordination isomerism.
A: [Co(NH₃)₆][Cr(CN)₆] and [Cr(NH₃)₆][Co(CN)₆].
Hybridization and Structures
21. Q:Hybridization of Ni in [Ni(CN)₄]²⁻?
A:dsp² (square planar).
22. Q:Hybridization in [NiCl₄]²⁻?
A:sp³ (tetrahedral).
23. Q:What is the geometry of [Fe(CN)₆]³⁻?
A:Octahedral.
24. Q:Magnetic moment of [Ti(H₂O)₆]³⁺? (d¹ system)
A:√1(1+2) = 1.73 BM.
25. Q:Which has more unpaired electrons: [Fe(CN)₆]³⁻ or [FeF₆]³⁻?
A: [FeF₆]³⁻ (weak ligand field).
Crystal Field Theory
26. Q:What is crystal field splitting?
A:Splitting of d-orbitals of a metal ion in presence of ligands.
27.Q:Why is [Fe(CN)₆]⁴⁻ diamagnetic?
A:CN⁻ is a strong field ligand causing pairing of electrons.
28. Q:Why is [FeF₆]³⁻ paramagnetic?
A: F⁻ is a weak field ligand, no pairing of electrons.
29. Q: In octahedral field, d-orbitals split into which sets?
A: t₂g (lower energy) and eg (higher energy).
30. Q:Write the electronic configuration of Co³⁺ in [CoF₆]³⁻.
A: t₂g⁴ eg² (high spin).
Color, Spectra, and Properties
31.Q:Why are transition metal complexes often colored?
A:Due to d-d transitions absorbing visible light.
32. Q:Why is [Ti(H₂O)₆]³⁺ purple?
A: d-d transition in d¹ system absorbs green light.
33. Q:Why is [Cu(H₂O)₆]²⁺ blue?
A:Absorption of red light causes complementary blue color.
34. Q:What is the magnetic nature of [Ni(CO)₄]?
A:Diamagnetic (all electrons paired).
35. Q: State the reason why [Mn(H₂O)₆]²⁺ is pale pink.
A:Weak d-d transitions (d⁵ high spin).
Important Compounds and Uses
36. Q: Formula of EDTA?
A:Ethylenediaminetetraacetic acid.
37. Q: Name one use of EDTA.
A: Used in complexometric titrations for hardness of water.
38. Q:What is cisplatin used for?
A: Anti-cancer drug.
39. Q: Name the active species in Vitamin B₁₂.
A:Co(III) coordination complex.
40.Q:Which coordination compound is known as Prussian Blue?
A: Fe₄[Fe(CN)₆]₃.
Advanced and Conceptual
41Q: Define stability constant.
A:Equilibrium constant for the formation of a complex.
42.Q:Between [Fe(CN)₆]³⁻ and [FeCl₆]³⁻, which is more stable?
A:[Fe(CN)₆]³⁻ (due to strong field ligand CN⁻).
43.Q:Which follows chelate effect: EDTA or NH₃?
A:EDTA.
44.Q:Write IUPAC name of [Fe(H₂O)₅NO]SO₄.
A:Pentaaquanitrosyliron(II) sulfate.
45. Q: What is the charge on [MnO₄]⁻?
A:–1.
46. Q:Why are low spin complexes more stable than high spin sometimes?
A: Higher crystal field stabilization energy (CFSE).
47. Q: Which complex is low spin: [Fe(CN)₆]³⁻ or [Fe(H₂O)₆]³⁺?
A: [Fe(CN)₆]³⁻.
48. Q:What is the coordination number in [Cr(C₂O₄)₃]³⁻?
A: 6 (oxalate is bidentate).
49. Q: Write geometry of [Cu(NH₃)₄]²⁺.
A:Square planar or distorted tetrahedral.
50. Q:Which rule helps predict absorbance in coordination compounds?
A:Selection rules (Laporte and spin selection rules).
Structural and Conceptual
1.Q:Why does [Ni(CN)₄]²⁻ have square planar geometry while [NiCl₄]²⁻ has tetrahedral geometry?
A:CN⁻ is a strong field ligand (dsp² hybridization), while Cl⁻ is weak field (sp³ hybridization).
2. Q:Which complex is diamagnetic: [CoF₆]³⁻ or [Co(NH₃)₆]³⁺?
A: [Co(NH₃)₆]³⁺, because NH₃ induces pairing (low spin).
3. Q:Why does [Ti(H₂O)₆]³⁺ show color, but [Sc(H₂O)₆]³⁺ is colorless?
A:Ti³⁺ has d¹ electron (d-d transition possible), Sc³⁺ is d⁰ (no d-d transition).
4.Q:Between [Fe(CN)₆]³⁻ and [Fe(CN)₆]⁴⁻, which one is more stable and why?
A:[Fe(CN)₆]³⁻ is more stable due to stronger CFSE of d⁵ low spin.
5. Q:Why is tetraamminecopper(II) sulfate solution blue?
A: It absorbs orange-red light due to d-d transitions, reflecting blue.
Isomerism
6. Q: Can a tetrahedral complex show geometrical isomerism?
A: No, only square planar and octahedral complexes show it.
7. Q:Which complex shows optical isomerism: [Co(en)₃]³⁺ or [Co(NH₃)₆]³⁺?
A: [Co(en)₃]³⁺ (chiral due to bidentate ligands).
8. Q:Why does [PtCl₂(NH₃)₂] have two isomers but [NiCl₄]²⁻ does not?
A:Square planar geometry of Pt complex allows cis/trans; Ni complex is tetrahedral.
9. Q: Which type of isomerism is shown by [Co(NO₂)(NH₃)₅]Cl₂ and [Co(ONO)(NH₃)₅]Cl₂?
A:Linkage isomerism (NO₂⁻ vs ONO⁻).
10. Q:Differentiate coordination and ionization isomers with one example.
A: [Cu(NH₃)₄][PtCl₄] vs [Pt(NH₃)₄][CuCl₄]; [Co(NH₃)₅Br]SO₄ vs [Co(NH₃)₅SO₄]Br.
Crystal Field Theory
11.Q:Why are d⁰ and d¹⁰ complexes usually colorless?
A:No d-d transitions possible.
12. Q:Arrange [Ti(H₂O)₆]³⁺, [V(H₂O)₆]³⁺, [Cr(H₂O)₆]³⁺ in increasing CFSE.
A: Ti³⁺ < V³⁺ < Cr³⁺ (increasing d-electrons).
13. Q:Why is [Fe(H₂O)₆]²⁺ strongly paramagnetic, but [Fe(CN)₆]⁴⁻ is diamagnetic?
A: H₂O is weak ligand (high spin d⁶), CN⁻ is strong ligand (low spin d⁶).
14. Q:Explain Jahn–Teller distortion in [Cu(H₂O)₆]²⁺.
A:Unequal occupancy of eg orbitals (d⁹ system) leads to elongation along z-axis.
15.Q:Which is the stronger ligand, en or NH₃?
A:en, due to chelate effect and stronger field strength.
Stability and Reactions
16. Q:Between [Ag(NH₃)₂]⁺ and [Ag(CN)₂]⁻, which is more stable?
A:[Ag(CN)₂]⁻ (cyanide forms very stable complexes).
17.Q:Why is EDTA a better ligand than NH₃?
A:It is hexadentate (chelating effect gives higher stability).
18. Q:Why does [Fe(CO)₅] have strong metal-ligand bonds?
A:CO shows synergic bonding (σ donation + π backbonding).
19.Q:Why is [Cr(NH₃)₆]³⁺ violet, but [Cr(H₂O)₆]³⁺ green?
A:Different ligand field strengths cause different absorption frequencies.
20.Q:Which is thermodynamically more stable: [Co(en)₃]³⁺ or [Co(NH₃)₆]³⁺?
A:[Co(en)₃]³⁺ due to chelation.
Conceptual Traps
21. Q:Why does [Zn(NH₃)₄]²⁺ not show color?
A:Zn²⁺ is d¹⁰, no d-d transitions.
22.Q: In [Mn(H₂O)₆]²⁺, why is CFSE = 0?
A:High spin d⁵, equal filling of t₂g and eg
23.Q:Why is [Fe(CN)₆]³⁻ less stable than [Fe(CN)₆]⁴⁻?
A:Fe³⁺ has higher charge density than Fe²⁺, so faces more repulsion with 6 CN⁻ ligands.
24.Q:Why do d-d transitions violate Laporte’s rule in [Ti(H₂O)₆]³⁺?
A:Vibronic coupling relaxes selection rule.
25.Q:Why is [Ni(CO)₄] diamagnetic despite Ni(0) being d⁸?
A:Strong CO field causes pairing → dsp² hybridization, no unpaired e⁻.
Applications
26.Q:Why is K₂[HgI₄] used in Nessler’s reagent?
A:It detects NH₃ by forming a brown complex.
27.Q:How does cisplatin act as an anticancer drug?
A:It binds to DNA and prevents replication.
28. Q:Why is EDTA used in water softening?
A: It binds strongly to Ca²⁺ and Mg²⁺ ions.
29.Q:Which coordination compound is used in photography fixing?
A:Sodium thiosulfate (Na₂S₂O₃).
30. Q:What gives the deep blue color in the Cu²⁺–NH₃ complex test?
A:Formation of [Cu(NH₃)₄]²⁺.
Advanced/Competitive Edge
31.Q:Which complex shows both linkage and geometrical isomerism?
A: [Co(NO₂)₂(NH₃)₄]⁺.
32. Q:Out of [Fe(H₂O)₆]²⁺ and [Fe(H₂O)₆]³⁺, which is more easily oxidized?
A:Fe²⁺ → Fe³⁺, because Fe³⁺ is more stable in water.
33. Q:Write CFSE expression for high spin octahedral complexes.
A:CFSE = –0.4xΔ₀ + 0.6yΔ₀, where x = no. of e⁻ in t₂g, y = e⁻ in eg
34.Q:Which shows greater magnetic moment: [CoF₆]³⁻ or [Co(NH₃)₆]³⁺?
A: [CoF₆]³⁻ (weak field, high spin, more unpaired e⁻).
35.Q: Why is [Cr(en)₃]³⁺ optically active?
A: It exists as two enantiomers (d and l forms).
Quantitative and CFSE Tricks
36. Q: Calculate CFSE of [Fe(CN)₆]⁴⁻. (Fe²⁺, d⁶, low spin)
A:CFSE = (–0.4×6Δ₀) = –2.4Δ₀ + pairing energy.
37. Q: Spin only magnetic moment of [MnF₆]³⁻ (d⁴ high spin)?
A: √4(4+2) = √24 = 4.9 BM.
38. Q: Why does NH₃ act as a ligand but not CH₄?
A:NH₃ has a lone pair on N, CH₄ has no lone pairs.
39. Q: In [Cr(H₂O)₆]³⁺, what is the color?
A:Violet-green (depends on light) due to d³ transitions.
40. Q:Which is stronger ligand according to spectrochemical series: H₂O or NH₃?
A:NH₃.
Edge Case Problems
41. Q:Why does Co²⁺ prefer tetrahedral complexes while Co³⁺ prefers octahedral?
A:Higher charge stabilizes more coordination.
42. Q:What is the CFSE of d³ octahedral high spin complex?
A: –1.2Δ₀.
43. Q:In [Ni(CN)₄]²⁻, why is Ni²⁺ using inner d-orbitals?
A:Strong field CN⁻ causes pairing into 3d.
44. Q:Is [Cu(NH₃)₄]²⁺ square planar or tetrahedral?
A:Distorted square planar (Jahn–Teller distortion).
45. Q: Why is NO considered an ambidentate ligand?
A:It can bind via N or O atom.
Miscellaneous Challenge
46. Q:Can [Zn(NH₃)₄]²⁺ be isostructural with [Cu(NH₃)₄]²⁺?
A:No, Zn²⁺ complex is perfect tetrahedral; Cu²⁺ shows distortion.
47. Q:Which has higher CFSE: strong field low spin or weak field high spin complexes?
A:Strong field low spin.
48.Q:Why do tetrahedral complexes rarely show low spin?
A:Splitting energy (Δt) is too small to cause pairing.
49.Q:Why does [Fe(CO)₅] show synergic bonding but [Fe(H₂O)₆]²⁺ does not?
A:H₂O cannot accept back-donation, CO can.
50.Q: Which complex has greater stability: [Cu(NH₃)₄]²⁺ or [Cu(H₂O)₄]²⁺?
A: [Cu(NH₃)₄]²⁺ (ligand field stabilization+stronger donor ability).
Coordination Compounds – 50 MCQs
Basics and Hybridization
1. The geometry of [Ni(CN)₄]²⁻ is:
a) Tetrahedral
b) Square Planar ✔
c) Octahedral
d) Distorted tetrahedral
2. The geometry of [NiCl₄]²⁻ is:
a) Square Planar
b) Octahedral
c) Tetrahedral ✔
d) Cubic
3. Which complex is diamagnetic?
a) [CoF₆]³⁻
b) [CoCl₆]³⁻
c) [Co(NH₃)₆]³⁺ ✔
d) [Fe(H₂O)₆]³⁺
4. Which ion is colorless?
a) [Ti(H₂O)₆]³⁺
b) [Sc(H₂O)₆]³⁺ ✔
c) [Fe(H₂O)₆]³⁺
d) [Cr(H₂O)₆]³⁺
5. Why does [Ni(CO)₄] show no unpaired electrons?
a) CO is weak field ligand
b) CO causes pairing of electrons ✔
c) Ni is d¹⁰
d) d-orbitals not involved
Isomerism
6. [PtCl₂(NH₃)₂] shows:
a) Ionization
b) Geometrical ✔
c) Optical
d) Coordination
7. Which tetrahedral complex can show geometrical isomerism?
a) [NiCl₄]²⁻
b) [Zn(NH₃)₄]²⁺
c) None ✔
d) [CuCl₄]²⁻
8. [Co(en)₃]³⁺ shows:
a) Cis-trans
b) Optical ✔
c) Ionization
d) Linkage
9. [Co(NO₂)(NH₃)₅]Cl₂ and [Co(ONO)(NH₃)₅]Cl₂ are:
a) Ionization isomers
b) Linkage isomers ✔
c) Coordination isomers
d) Optical isomers
10. [Co(NO₂)₂(NH₃)₄] shows which two types of isomerism?
a) Geometrical + Linkage ✔
b) Optical + Ionization
c) Ionization + Structural
d) Hydrate + Geometrical
Crystal Field and Color
11. Which complex is colorless?
a) [Ti(H₂O)₆]³⁺
b) [Fe(H₂O)₆]²⁺
c) [Zn(NH₃)₄]²⁺ ✔
d) [Cr(H₂O)₆]³⁺
12. d⁰ and d¹⁰ complexes are generally:
a) Strongly colored
b) Weakly colored
c) Colorless ✔
d) Magnetic
13. Jahn-Teller distortion is most common in:
a) d⁵
b) d⁹ ✔
c) d³
d) d⁸
14. Which has higher CFSE?
a) Weak field ligand
b) Strong field ligand ✔
c) Neutral ligands always
d) All equal
15. Which effect explains stability of chelates?
a) Jahn–Teller effect
b) Chelate effect ✔
c) Nephelauxetic effect
d) Crystal field theory
Stability and Ligand Strength
16. Stability of [Ag(NH₃)₂]⁺ vs [Ag(CN)₂]⁻?
a) [Ag(NH₃)₂]⁺ is more stable
b) [Ag(CN)₂]⁻ is more stable ✔
c) Both equally stable
d) Depends on temp
17. Which is better ligand for complex formation?
a) H₂O
b) NH₃
c) en (ethylenediamine) ✔
d) CO₂
18. [Fe(CO)₅] has strong M–L bonding due to:
a) π-bonding only
b) σ-bonding only
c) Synergic bonding ✔
d) Ionic bonding
19. [Cr(NH₃)₆]³⁺ is violet while [Cr(H₂O)₆]³⁺ is green due to:
a) Different geometries
b) Different oxidation states
c) Different ligand field strength ✔
d) Different magnetic properties
20. [Co(en)₃]³⁺ is more stable than [Co(NH₃)₆]³⁺ due to:
a) Larger size
b) Higher oxidation
c) Chelate effect ✔
d) Higher CFSE
Trick & Exception Based
21. Why does [Mn(H₂O)₆]²⁺ have pale pink color?
a) Strong absorption
b) Weak d-d transitions ✔
c) Charge transfer
d) No transition
22. Which has greater unpaired electrons?
a) [Fe(CN)₆]³⁻
b) [FeF₆]³⁻ ✔
c) Both equal
d) None
23. Which violates Laporte’s rule under vibronic coupling?
a) d⁰ ions
b) [Ti(H₂O)₆]³⁺ ✔
c) d¹⁰ ions
d) [Zn(NH₃)₄]²⁺
24. In square planar complexes, maximum pairing is caused by:
a) Weak field
b) Strong field ✔
c) Neutral ligands
d) Anionic ligands
25. Which has more CFSE?
a) High spin complex
b) Low spin complex ✔
c) Both equal
d) Cannot predict
Applications and Compounds
26. Which is used in water softening titrations?
a) Na₂S₂O₃
b) EDTA ✔
c) NH₃
d) CO
27. Cisplatin is used as:
a) Fertilizer
b) Dye
c) Anticancer drug ✔
d) catalyst
28. Complex in photographic fixing solution:
a) [Ag(NH₃)₂]⁺
b) [Ag(S₂O₃)₂]³⁻ ✔
c) [Cu(NH₃)₄]²⁺
d) [Fe(CN)₆]³⁻
29. Deep blue solution in Cu²⁺ with NH₃ is due to:
a) [Cu(OH)₂]
b) [Cu(NH₃)₂]⁺
c) [Cu(NH₃)₄]²⁺ ✔
d) [Cu(H₂O)₆]²⁺
30. Prussian Blue structure is due to:
a) [Cu(NH₃)₄]²⁺
b) Fe₄[Fe(CN)₆]₃ ✔
c) [Fe(H₂O)₆]²⁺
d) [FeF₆]³⁻
Advanced Calculation Type
31. Spin-only magnetic moment of [MnF₆]³⁻? (d⁴ HS)
a) 2.8 BM
b) 3.9 BM
c) 4.9 BM ✔
d) 5.9 BM
32. CFSE for d³ octahedral (HS)?
a) –0.4Δ₀
b) –1.2Δ₀ ✔
c) –2.4Δ₀
d) 0
33. Which is stronger ligand (spectrochemical series)?
a) NH₃ ✔
b) H₂O
c) Cl⁻
d) OH⁻
34. CFSE of [Fe(CN)₆]⁴⁻ (low spin d⁶)?
a) –0.4Δ₀
b) –1.2Δ₀
c) –2.4Δ₀ ✔
d) 0
35. Which has stronger field splitting: CO or CN⁻?
a) CN⁻
b) CO ✔
c) Both equal
d) None
Trick Edge Cases
36. In [Cu(NH₃)₄]²⁺ geometry is:
a) Perfect square planar
b) Distorted square planar ✔
c) Octahedral
d) Linear
37. Why tetrahedral complexes rarely low spin?
a) Δt very small ✔
b) High CFSE
c) Jahn-Teller effect
d) High splitting
38. Which is ambidentate ligand?
a) CO
b) NO₂⁻ ✔
c) NH₃
d) H₂O
39. Which complex cannot be optical isomer?
a) [Co(en)₃]³⁺
b) [Cr(ox)₃]³⁻
c) [Co(NH₃)₆]³⁺ ✔
d) [PtCl₂(en)₂]²⁺
40. Which has maximum pairing?
a) [FeF₆]³⁻
b) [Fe(CN)₆]³⁻ ✔
c) [Fe(H₂O)₆]²⁺
d) [FeCl₆]³⁻
Energy, CFSE & Magnetism
41. Mn²⁺ in [Mn(H₂O)₆]²⁺ has CFSE:
a) 0 ✔
b) –0.6Δ₀
c) –1.2Δ₀
d) –2.4Δ₀
42. Which has higher stabilization: [CoF₆]³⁻ or [Co(CN)₆]³⁻?
a) [CoF₆]³⁻
b) [Co(CN)₆]³⁻ ✔
c) Both equal
d) None
43. Which is diamagnetic?
a) [Zn(NH₃)₄]²⁺ ✔
b) [Cu(H₂O)₆]²⁺
c) [Fe(H₂O)₆]²⁺
d) [CoF₆]³⁻
44. Which has greater absorbance in visible region?
a) Weak ligand complexes
b) Strong ligand complexes ✔
c) All equally colored
d) d¹⁰ ions
45. Why does [Fe(CO)₅] form strong complexes?
a) NO backbonding
b) Synergic bonding ✔
c) Pure ionic bonding
d) Hydrogen bonding
Final Trick Questions
46. Why does Cu²⁺ prefer distorted geometry?
a) High CFSE
b) Jahn-Teller effect ✔
c) Weak field ligands
d) Chelation
47. Which is isostructural with [Zn(NH₃)₄]²⁺?
a) [Cu(NH₃)₄]²⁺
b) [Ni(CO)₄]
c) [NiCl₄]²⁻ ✔
d) [Co(NH₃)₆]³⁺
48. Which complex has highest magnetic moment?
a) [FeF₆]³⁻ ✔
b) [Fe(CN)₆]³⁻
c) [Fe(H₂O)₆]²⁺
d) [Cu(NH₃)₄]²⁺
49. Which shows synergic bonding?
a) [Fe(CO)₅] ✔
b) [Fe(H₂O)₆]³⁺
c) [FeF₆]³⁻
d) [Zn(NH₃)₄]²⁺
50. Which is more stable: [Cu(NH₃)₄]²⁺ or [Cu(H₂O)₄]²⁺?
a) [Cu(NH₃)₄]²⁺ ✔
b) [Cu(H₂O)₄]²⁺
c) Both equal
d) Cannot predict
List of Some important ligands:
| Ligand Formula | Common Name | IUPAC Name | Coordination Type | Denticity |
|---|---|---|---|---|
| NH₃ | Ammonia | Ammine | Neutral ligand | Monodentate |
| H₂O | Water | Aqua | Neutral ligand | Monodentate |
| Cl⁻ | Chloride ion | Chloro | Anionic ligand | Monodentate |
| OH⁻ | Hydroxide ion | Hydroxo | Anionic ligand | Monodentate |
| CN⁻ | Cyanide ion | Cyano | Anionic ligand | Monodentate |
| NO₂⁻ (via N) | Nitrito (N-bound) | Nitrito-N | Anionic ligand | Monodentate |
| NO₂⁻ (via O) | Nitrito (O-bound) | Nitrito-O | Anionic ligand | Monodentate |
| SCN⁻ (via S) | Thiocyanato (S-bound) | Thiocyanato-S | Anionic ligand | Monodentate |
| SCN⁻ (via N) | Thiocyanato (N-bound) | Thiocyanato-N | Anionic ligand | Monodentate |
| CO | Carbonyl | Carbonyl | Neutral ligand | Monodentate |
| C₂O₄²⁻ | Oxalate ion | Oxalato | Anionic ligand | Bidentate (chelating) |
| en | Ethylenediamine | Ethane-1,2-diamine | Neutral ligand | Bidentate (chelating) |
| EDTA⁴⁻ | Ethylenediaminetetraacetate | Ethane-1,2-diylbis(iminodiacetato) | Anionic ligand | Hexadentate (chelating) |
| NH₂CH₂COO⁻ | Glycinate ion | Aminoacetato | Anionic ligand | Bidentate |
| SO₄²⁻ | Sulfate ion | Sulfato | Anionic ligand | Usually bidentate |
| NO₃⁻ | Nitrate ion | Nitrato | Anionic ligand | Monodentate / Bidentate |
| PPh₃ | Triphenylphosphine | Triphenylphosphane | Neutral ligand | Monodentate |
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