Q.Using IUPAC norms write the systematic names of the following:
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🔒 Start your 14-day free trial to unlock the full solution →Concept understanding — Werner Coordination Theory
Werner Coordination Theory: The Idea That Changed Inorganic Chemistry
Imagine you're looking at a salt like cobalt(III) chloride. The formula is written as CoClX3, and when you dissolve it in water, you expect to find CoX3+ and ClX− ions. But something strange happens: when you add silver nitrate (which precipitates chloride ions), only some of the chlorine comes out as silver chloride. Not all of it. And the amount that precipitates depends on how you made the compound.
This was the puzzle that faced chemists in the late 1800s. Compounds like CoClX3⋅6NHX3 (orange-yellow) and CoClX3⋅5NHX3 (purple) had the same metal and the same ligands (ammonia), but different colours, different conductivities in solution, and different numbers of chloride ions that could be precipitated. The old ideas of fixed valency couldn't explain it.
Alfred Werner proposed a radical solution in 1893. He said: a metal ion has two kinds of valency.
The Core Intuition
Think of a metal ion like a king in a castle. The king has two types of relationships:
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Primary valency (today: oxidation state) — this is the king's royal authority. It's fixed, non-directional, and satisfied by negative ions. For cobalt(III), this is +3. It's like the king's crown: it doesn't change.
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Secondary valency (today: coordination number) — this is the king's personal bodyguard. The king can have a fixed number of guards (usually 4 or 6) who stand in specific positions around him. These guards can be neutral molecules (like ammonia) or negative ions (like chloride). The key: these guards are directly attached to the metal, forming a stable cluster called the coordination sphere.
The revolutionary idea: the chloride ions that act as bodyguards (inside the coordination sphere) do not behave like free ions. They don't precipitate with silver nitrate. They don't conduct electricity. They are "locked" to the metal.
The Precise Statement
Werner Coordination Theory (1893)
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Every metal atom has two types of valency:
- Primary valency (ionisable): corresponds to the oxidation state. It is satisfied by negative ions. These ions are outside the coordination sphere and behave as free ions in solution.
- Secondary valency (non-ionisable): corresponds to the coordination number. It is satisfied by neutral molecules or negative ions directly bonded to the metal. These are inside the coordination sphere and do not dissociate.
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The secondary valencies are directional — they point to fixed positions in space around the metal, giving the complex a definite geometry (e.g., octahedral for coordination number 6, square planar for 4).
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The primary valency is non-directional — it is just a number, not a spatial arrangement.
How It Explains the Puzzle
Take the compound CoClX3⋅6NHX3 (orange-yellow). Werner said:
- Cobalt has primary valency +3 (needs three negative charges to satisfy it).
- Cobalt has secondary valency 6 (can hold six ligands around it).
- The six ammonia molecules satisfy all six secondary valencies. So the chloride ions cannot be inside the coordination sphere — they must be outside, as free ions.
- Structure: [Co(NHX3)X6]ClX3. All three chlorides precipitate with AgNOX3.
Now take CoClX3⋅5NHX3 (purple):
- Again, primary valency +3, secondary valency 6.
- Five ammonia molecules satisfy five secondary valencies. One chloride ion must fill the sixth spot — it becomes a ligand inside the sphere.
- The other two chlorides are outside as free ions.
- Structure: [Co(NHX3)X5Cl]ClX2. Only two chlorides precipitate.
The number of free ions in solution determines the conductivity and the number of precipitable chlorides. Werner's theory predicted exactly these numbers — and experiments confirmed them.
The Geometry Insight …
Why this formula?
Werner Coordination Theory: Why the Key Formulas Hold
Werner Coordination Theory (1893) revolutionized inorganic chemistry by explaining how metal ions bind ligands. Let's build the reasoning from first principles — not just memorize formulas.
1. The Core Observation: Primary vs. Secondary Valence
Werner noticed that metal compounds had two types of bonding capacity:
- Primary valence (now oxidation state): Satisfies the metal's charge — ionic in nature.
- Secondary valence (now coordination number): Determines how many ligands attach — directional, spatial in nature.
Why this distinction?
Consider CoClX3 ⋅6NHX3 (one of Werner's classic compounds).
- The compound is electrically neutral overall.
- Adding AgNOX3 precipitates all 3 Cl⁻ as AgCl — meaning all chlorides are free ions.
- Therefore, the NHX3 molecules must be directly bonded to Co, not the chlorides.
This forces the idea: Co has a fixed capacity for direct ligand attachment (secondary valence = 6 here), separate from its charge balance (primary valence = +3).
2. The Key Formula: Coordination Number = Number of Ligands Attached
Formula:
Coordination number=number of donor atoms directly bonded to the metal
Why this holds:
- Werner's experiments showed that only a fixed number of ligands could be replaced without breaking the compound's identity.
- For CoClX3 ⋅6NHX3, adding acid doesn't remove NHX3 easily — they are coordinated.
- The maximum number of such tightly bound ligands is the coordination number — a property of the metal ion, not the counterions.
Derivation from data:
If you have [Co(NHX3)X6]ClX3, conductivity measurements show 4 ions in solution ([Co(NHX3)X6]X3+ + 3 Cl⁻).
If you had [Co(NHX3)X5Cl]ClX2, conductivity shows 3 ions.
The number of chlorides inside the coordination sphere (non-precipitable) plus those outside must sum to the total chlorides. This gives the coordination number directly.
3. The Geometry Formula: Coordination Number Determines Shape
Werner proposed that secondary valences are directed in space — leading to specific geometries.
| Coordination Number | Geometry | Why? |
|---|---|---|
| 2 | Linear | Minimizes repulsion between 2 ligands |
| 4 | Tetrahedral or Square planar | 4 points in space — two arrangements possible |
| 6 | Octahedral | 6 ligands at 90° angles — most symmetric |
Why octahedral for 6?
- 6 ligands around a central atom must be placed to maximize separation.
- The octahedron (6 vertices, all equidistant from center, 90° between adjacent bonds) is the only regular polyhedron with 6 vertices.
- This explains why [Co(NHX3)X6]X3+ is octahedral — no other arrangement gives equal bond angles and distances.
4. The Isomer Counting Formula: Why 2n or n! Appears
Werner used isomer counts to confirm geometry. For an octahedral complex [MaX2bX2cX2]:
Number of geometrical isomers = 5 (not 6, not 4)
Why this formula?
- Place the two 'a' ligands: they can be cis (90°) or trans (180°).
- For each, place 'b' and 'c' in remaining positions — but symmetry reduces duplicates. …
Concept: Werner Coordination Theory — ligands are named before the metal, oxidation state in Roman numerals in parentheses, and the complex is named as one word (cation/anion order).
(i) [Co(NH3)6]Cl3
Hexaamminecobalt(III) chloride
(ii) [Pt(NH3)2Cl(NH2CH3)]Cl
Diamminechlorido(methanamine)platinum(II) chloride
(iii) [Ti(H2O)6]3+
Hexaaquatitanium(III) ion
(iv) [Co(NH3)4Cl(NO2)]Cl
Tetraamminechloridonitrito-κN-cobalt(III) chloride
(v) [Mn(H2O)6]2+
Hexaaquamanganese(II) ion
(vi) [NiCl4]2−
Tetrachloridonickelate(II) ion
(vii) [Ni(NH3)6]Cl2
Hexaamminenickel(II) chloride
(viii) [Co(en)3]3+
Tris(ethane-1,2-diamine)cobalt(III) ion
(ix) [Ni(CO)4] …
Werner’s coordination theory tells us that the central metal’s primary valence (oxidation state) is satisfied by the counter ions outside the coordination sphere, while the secondary valence (coordination number) is satisfied by the ligands inside the square brackets. The systematic name follows: ligands in alphabetical order (ignoring prefixes), then the metal with its oxidation state in Roman numerals in parentheses, and finally the counter ion if any.
The core idea: In coordination compounds, the species inside the square brackets is the coordination entity — the metal ion plus the ligands directly bonded to it. Everything outside the brackets is a counter ion that balances charge. The IUPAC naming rules are:
- Name the ligands first, in alphabetical order (prefixes like di-, tri- are ignored for alphabetisation).
- Anionic ligands end in -o, neutral ligands keep their name (except water = aqua, ammonia = ammine, carbon monoxide = carbonyl).
- Write the metal’s name, then its oxidation state in Roman numerals in parentheses.
- If the complex is an anion, the metal name ends in -ate.
- Finally, name the counter ion (cation first, then anion).
Let’s apply this step by step to each compound.
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[Co(NH3)6]Cl3
- Ligand: six ammines → “hexaammine”.
- Metal: cobalt. The complex is a cation (inside brackets is positive, three chlorides outside give total charge −3, so the complex cation is +3). Oxidation state of Co: x+0=+3⇒x=+3.
- Name: Hexaamminecobalt(III) chloride.
Watch out“Ammine” (with two m’s) is used for NH₃ as a ligand, not “amine” (which is for organic −NH₂ groups). A common slip.
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[Pt(NH3)2Cl(NH2CH3)]Cl
- Ligands: two ammines, one chloride (anionic → “chlorido”), one methanamine (NH2CH3, neutral — NCERT's preferred IUPAC name; “methylamine” is the common synonym). Alphabetical order: ammine, chlorido, methanamine.
- Oxidation state of Pt: inside bracket charge = x+0+(−1)+0=+1 (since one Cl⁻ outside). So x−1=+1⇒x=+2.
- Name: Diamminechlorido(methanamine)platinum(II) chloride.
TipWhen a ligand carries a compound organic name (like methanamine), enclose it in parentheses so it cannot merge confusingly with the neighbouring ligand names and prefixes.
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[Ti(H2O)6]3+
- Ligand: six water molecules → “hexaaqua”.
- Metal: titanium. Charge on complex is +3, water is neutral, so Ti is +3.
- Name: Hexaaquatitanium(III) ion. (Since it’s a cation, no counter ion named.)
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[Co(NH3)4Cl(NO2)]Cl
- Ligands: four ammines, one chloride (chlorido), one nitrite (NO₂⁻ can bind through N or O; here it’s likely through N → “nitrito-N” or simply “nitrito” if unambiguous). Alphabetical: ammine, chlorido, nitrito.
- Oxidation state of Co: inside charge = x+0+(−1)+(−1)=+1 (one Cl⁻ outside). So x−2=+1⇒x=+3.
- Name: Tetraamminechloridonitrito-N-cobalt(III) chloride.
NoteThe nitrite ligand is ambidentate; if the bonding atom is not specified, “nitrito” usually means O-bonded, but in many exam contexts NO₂⁻ bonded through N is called “nitro”. Here we follow IUPAC: “nitrito-N” for N-bonded, “nitrito-O” for O-bonded. The formula itself writes the ligand N-first (NO2), which indicates N-bonding — hence nitrito-N.
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[Mn(H2O)6]2+
- Ligand: hexaaqua.
- Metal: manganese. Complex charge +2, water neutral → Mn is +2.
- Name: Hexaaquamanganese(II) ion.
-
[NiCl4]2− …
Systematic Naming of Coordination Compounds (IUPAC)
Method: IUPAC Nomenclature Rules for Coordination Compounds
Steps to Follow
- Identify the complex ion — separate cationic and anionic parts.
- Name the ligands first (alphabetical order, ignoring prefixes like di-, tri-).
- Name the central metal atom/ion:
- If the complex is cationic or neutral: use the metal name as is.
- If the complex is anionic: add the suffix -ate to the metal name.
- Specify the oxidation state of the metal in Roman numerals in parentheses.
- Name the counter ions (outside the coordination sphere) last.
Solutions
(i) [Co(NH3)6]Cl3
- Complex ion: [Co(NH3)6]3+ (cationic)
- Ligand: hexaammine (6 × NH₃)
- Metal: cobalt
- Oxidation state: Co is +3 (since 6 NH₃ are neutral, charge +3 from Cl₃)
- Counter ion: chloride
Answer: Hexaamminecobalt(III) chloride
(ii) [Pt(NH3)2Cl(NH2CH3)]Cl
- Complex ion: [Pt(NH3)2Cl(NH2CH3)]+ (cationic)
- Ligands (alphabetical order):
- ammine (NH₃) — 2 → diammine
- chloride (Cl) — 1 → chlorido
- methanamine (NH₂CH₃) — 1 → methanamine (common synonym: methylamine)
- Metal: platinum
- Oxidation state: Pt is +2 (2 NH₃ neutral, Cl⁻, NH₂CH₃ neutral → overall +1, so Pt = +2)
- Counter ion: chloride
Answer: Diamminechlorido(methanamine)platinum(II) chloride
(iii) [Ti(H2O)6]3+
- Complex ion: [Ti(H2O)6]3+ (cationic)
- Ligand: hexaaqua (6 × H₂O)
- Metal: titanium
- Oxidation state: Ti is +3 (6 H₂O neutral, charge +3)
Answer: Hexaaquatitanium(III) ion
(iv) [Co(NH3)4Cl(NO2)]Cl
- Complex ion: [Co(NH3)4Cl(NO2)]+ (cationic)
- Ligands (alphabetical order):
- ammine (NH₃) — 4 → tetraammine
- chlorido (Cl) — 1 → chlorido
- nitrito (NO₂⁻) — 1 → the NO₂⁻ formula written in the complex ion shows it is bonded through nitrogen, so the modern IUPAC name uses nitrito-N (older textbooks call this "nitro")
- Metal: cobalt
- Oxidation state: Co is +3 (4 NH₃ neutral, Cl⁻, NO₂⁻ → overall +1, so Co = +3)
- Counter ion: chloride
Answer: Tetraamminechloridonitrito-N-cobalt(III) chloride
(v) [Mn(H2O)6]2+
- Complex ion: [Mn(H2O)6]2+ (cationic)
- Ligand: hexaaqua
- Metal: manganese
- Oxidation state: Mn is +2
Answer: Hexaaquamanganese(II) ion
(vi) [NiCl4]2−
- Complex ion: [NiCl4]2− (anionic)
- Ligand: tetrachlorido (4 × Cl⁻)
- Metal: nickel → nickelate (anionic suffix)
- Oxidation state: Ni is +2 (4 Cl⁻ = −4, overall −2, so Ni = +2)
Answer: Tetrachloridonickelate(II) ion
(vii) [Ni(NH3)6]Cl2
- Complex ion: [Ni(NH3)6]2+ (cationic)
- Ligand: hexaammine
- Metal: nickel
- Oxidation state: Ni is +2
- Counter ion: chloride
Answer: Hexaamminenickel(II) chloride
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Common Mistakes in Naming Coordination Compounds (Werner Theory)
Students frequently lose marks on IUPAC nomenclature. Here are the most common errors and how to avoid each:
1. Wrong Order of Ligands (Alphabetical vs. Charge)
Mistake: Listing anionic ligands after neutral ligands, or writing ligands in order of charge (negative → neutral → positive).
Example from (ii): Writing "chloridodiammine(methylamine)platinum(II) chloride" (chlorido placed first because it is anionic) instead of the correct alphabetical order.
How to Avoid:
- Always arrange ligands alphabetically by ligand name (ignoring prefixes like di-, tri-, tetra-).
- Anionic ligands come first only if they start with an earlier letter.
- Also do not drop the multiplying prefix once the ligands are reordered — there are still two ammine ligands, so the prefix di- must stay.
- For (ii): ammine (a) → chlorido (c) → methanamine (m) → diamminechlorido(methanamine)platinum(II) chloride
2. Incorrect Oxidation State (Roman Numeral)
Mistake: Guessing the oxidation state without calculation, especially when counter ions are present.
Example from (i): Writing cobalt(0) or cobalt(III) without checking.
How to Avoid:
- Always calculate oxidation state using: Charge of complex = sum of charges on metal + ligands
- For (i): [Co(NH3)6]Cl3 → complex ion [Co(NH3)6]3+ → x+6(0)=+3 → x=+3 → cobalt(III)
- For (iv): [Co(NH3)4Cl(NO2)]Cl → complex ion [Co(NH3)4Cl(NO2)]+ → x+4(0)+(−1)+(−1)=+1 → x=+3 → cobalt(III)
3. Confusing Anionic Ligand Names
Mistake: Using the neutral name instead of the anionic form (e.g., chlorine instead of chlorido, nitrite instead of nitrito).
Example from (iv): Writing nitrite instead of nitrito or nitro.
How to Avoid:
- Memorise the anionic ligand endings:
- -ide → -ido (chlorido, bromido, iodido)
- -ite → -ito (nitrito, sulfito)
- -ate → -ato (sulfato, carbonato)
- For (iv): the formula writes the ligand N-first (NO2), which indicates N-bonding — so the modern IUPAC (and NCERT) name is nitrito-N; the O-bonded form would be nitrito-O (written ONO in the formula). The older style called the N-bonded form nitro — recognise it, but write the NCERT locant style in the exam.
4. Forgetting to Name the Counter Ion
Mistake: Naming only the complex ion and omitting the counter ion.
Example from (i): Writing hexaamminecobalt(III) instead of hexaamminecobalt(III) chloride.
How to Avoid:
- Always check the overall formula — if there are ions outside the square brackets, name them last.
- For (i): [Co(NH3)6]Cl3 → complex cation + three chloride ions → hexaamminecobalt(III) chloride
- For (ii): [Pt(NH3)2Cl(NH2CH3)]Cl → complex cation + one chloride ion → diamminechlorido(methylamine)platinum(II) chloride
5. Wrong Prefix for Polydentate Ligands
Mistake: Using di-, tri- for chelating ligands like en (ethylenediamine) instead of bis-, tris-.
Example from (viii): Writing diethylenediamine instead of bis(ethylenediamine).
How to Avoid:
- Use bis-, tris-, tetrakis- for ligands that already contain di-, tri- in their name, or for chelating ligands.
- For (viii): [Co(en)3]3+ → tris(ethane-1,2-diamine)cobalt(III) ion (en = ethane-1,2-diamine, commonly called ethylenediamine)
- For simple ligands like NH3, the ordinary prefixes are correct: six NH3 → hexaammine (no bis/tris needed)
6. Incorrect Ending for Complex Ion (Cation vs. Anion)
Mistake: Using -ate for a cationic complex, or omitting -ate for an anionic complex.
Example from (vi): Writing tetrachloronickel(II) instead of tetrachloridonickelate(II).
How to Avoid:
- If the complex is an anion, add -ate to the metal name (and use the Latin name for some metals).
- For (vi): [NiCl4]2− → anionic → tetrachloridonickelate(II) ion
- Common Latin names: ferrate (Fe), cuprate (Cu), argentate (Ag), aurate (Au), stannate (Sn), plumbate (Pb)
7. Omitting the Word "Ion" for Charged Complexes
Mistake: Writing hexaaquatitanium(III) instead of hexaaquatitanium(III) ion.
Example from (iii): [Ti(H2O)6]3+ → hexaaquatitanium(III) ion
How to Avoid:
- If the complex has a charge and no counter ion is shown, add "ion" at the end.
- For (iii): hexaaquatitanium(III) ion
- For (v): hexaaquamanganese(II) ion
- For (viii): tris(ethylenediamine)cobalt(III) ion
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Showing the 12 most recent of 25 on this concept.
- AP EAPCET 2026Set eng-2026-05-12-AN1 markMCQQ.Aqueous solutions of which of the following compounds do not form AgCl precipitate with excess AgNO3 solution? I. PtCl4.2HCl II. PtCl2.2NH3 III. CoCl3.4NH3 IV. PdCl2.4NH3 The correct answer is (only = only) (A) I , II only (B) III , IV only (C) I , II , III only (D) I , II , IV only
›Reveal solutionSolution
Only the chloride ions OUTSIDE the coordination sphere (ionisable) precipitate as AgCl; ligand (coordinated) chlorides do not. Complexes I and II have zero free Cl−.
Concept and Intuition
This is the classical Werner coordination-number test: dissolve the complex, add excess AgNO3, and see how much AgCl precipitates. Chlorine atoms bonded directly to the metal as ligands are held too tightly to react; only chloride counter-ions (outside the coordination sphere, present as free Cl− in solution) react with Ag+.
Step-by-Step Solution
- I. PtCl4.2HCl: rewrite as the ionic formula H2[PtCl6] — Pt(IV), coordination number 6, all six chlorides are ligands inside [PtCl6]2−; the two H+ are the counter-ions. Free Cl−=0 → no precipitate.
- II. PtCl2.2NH3: [Pt(NH3)2Cl2], Pt(II), coordination number 4 (square planar), both Cl are ligands, complex is neutral overall (no counter-ions at all). Free Cl−=0 → no precipitate.
- III. CoCl3.4NH3: Co(III), coordination number 6 is satisfied by 4 NH3 + 2 Cl as ligands, giving [Co(NH3)4Cl2]+; the third Cl is a free counter-ion: [Co(NH3)4Cl2]Cl. Free Cl−=1 per formula unit → gives precipitate (though only a third of the total chlorine). …
- AP EAPCET 2026Set eng-2026-05-13-FN1 markMCQQ.The metal ion, ligands present in Wilkinson catalyst are respectively (A) Rh3+ , Cl− , PPh3 (B) Rh+ , Cl− , PPh3 (C) Rh2+ , Br− , PH3 (D) Re+ , I− , P(CH3)3
›Reveal solutionSolution
Wilkinson's catalyst, [RhCl(PPh₃)₃], is built from Rh in the +1 state, a chloride ligand, and neutral triphenylphosphine ligands.
Concept and Intuition
Wilkinson's catalyst is one of the classic homogeneous hydrogenation catalysts, a square-planar 16-electron Rh(I) complex. To find the metal's oxidation state in a coordination complex, sum the charges of the ligands and set the whole species' charge (here, neutral, since it's written without any counter-ion) equal to metal charge + ligand charges.
Step-by-Step Solution
- The formula is [RhCl(PPh3)3] — an overall neutral complex.
- PPh3 (triphenylphosphine) is a neutral, two-electron-donor ligand (donates via the lone pair on P) — contributes 0 charge, and there are three of them.
- Cl here is bound as the anionic chloride ligand, Cl−.
- Charge balance: (charge on Rh) + (−1 from Cl⁻) + 3×(0 from PPh₃) = 0 ⟹ charge on Rh = +1, i.e. Rh+.
- So metal ion = Rh+; ligands = Cl− and PPh3 — matching option (B).
Common Mistakes …
- AP EAPCET 2026Set eng-2026-05-14-FN1 markMCQQ.Identify the correct set containing only ambidentate ligands (A) NO2−,CN−,SCN− (B) NH3,CN−,C2O42− (C) SO42−,SCN−,CO (D) C2O42−,(CH3)3P,CO
›Reveal solutionSolution
Ambidentate ligands offer two different donor atoms; the classic textbook trio is NO2−, CN−, SCN−.
Concept and Intuition
An ambidentate ligand has two different atoms, either of which can coordinate to the metal (though not simultaneously, unlike a chelating bidentate ligand). The identity of the coordinating atom can even change the name of the complex (e.g. nitro vs nitrito).
Step-by-Step Solution
- NO2− can bind through N (nitro) or through O (nitrito) — ambidentate.
- CN− can bind through C (cyano) or N (isocyano) — ambidentate.
- SCN− (thiocyanate) can bind through S (thiocyanato) or N (isothiocyanato) — ambidentate. …
- AP EAPCET 2025Set eng-2025-05-24-FN1 markMCQQ.The co-ordination number of chromium in K[Cr(H2O)2(C2O4)2] is (A) 5 (B) 4 (C) 6 (D) 3
›Reveal solutionSolution
This tests counting coordination number from a mixed-ligand complex; oxalate's bidentate nature is the key, giving coordination number 6.
Concept and Intuition
Coordination number counts the total number of donor-atom bonds to the central metal, not the number of ligand molecules/ions. A ligand like oxalate (C2O42−) is bidentate — it uses two oxygen atoms to bond to the metal simultaneously, forming a five-membered chelate ring — so each oxalate contributes 2 to the coordination number, not 1.
Step-by-Step Solution
- Identify ligands in [Cr(H2O)2(C2O4)2]−: 2 water molecules (monodentate) and 2 oxalate ions (bidentate).
- Donor atoms from water: 2×1=2. …
- AP EAPCET 2025Set eng-2025-05-26-FN1 markMCQQ.Which of the following exhibit ionization isomerism? (only = మాత్రమే) I) [Cr(NH3)4Cl2]Cl II) [Ti(H2O)5Cl](NO3)2 III) [Pt(en)(NH3)Cl]NO3 IV) [Co(NH3)4(NO3)2]NO3 (A) II & III only (B) I & II only (C) II & IV only (D) III & IV only
›Reveal solutionSolution
This tests when ionization isomerism is actually possible. The answer is (A): only II and III have two chemically different anions available to swap between the coordination sphere and the counter-ion position.
Concept and Intuition
Ionization isomers are compounds with the same overall formula that give different ions in solution because an anionic ligand and the counter-ion have exchanged positions (one moves from inside the coordination sphere to outside, and vice versa). For this to produce a genuinely different, distinguishable compound, the ligand-anion and the counter-anion must be chemically different species. If a complex only contains ONE kind of extra anion (split between 'inside' and 'outside' just to satisfy the coordination number and overall charge), then any rearrangement of identical anions gives back an indistinguishable compound — so no real isomerism is possible.
Step-by-Step Solution
- I: [Cr(NH3)4Cl2]Cl. Cr(III) is octahedral (CN 6); 4 NH3 occupy 4 sites, so exactly 2 more anionic ligands are needed to complete the sphere — and Cl− is the only anion present (3 total: 2 in, 1 out). The split (2 in / 1 out) is forced by the coordination number, and since all three anions are identical Cl−, no alternative arrangement gives a distinguishable compound. No ionization isomerism.
- II: [Ti(H2O)5Cl](NO3)2. Ti(III) is octahedral; 5 H2O + 1 Cl− fill the sphere, with 2 NO3− outside. Here TWO different anions exist (Cl− and NO3−). Swapping the ligand Cl− for one of the counter NO3− ions gives [Ti(H2O)5(NO3)]Cl(NO3) — a genuinely different, distinguishable compound. Shows ionization isomerism. …
- AP EAPCET 2025Set eng-2025-05-27-FN1 markMCQQ.Identify the set which does not have ambidentate ligand (s) (A) NO2−,CN−,C2O42− (B) C2O42−,H2O,SO42− (C) SCN−,NH3,CH3COO− (D) CN−,SCN−,CH3NH2
›Reveal solutionSolution
Ambidentate ligands can coordinate through two different atoms (e.g. NO2−, CN−, SCN−). Only set (B) contains none of these classic ambidentate ligands.
Concept and Intuition
An ambidentate ligand has two different potential donor atoms, only one of which binds the metal at a time — e.g. NO2− can bind via N (nitro) or O (nitrito); CN− via C or N; SCN− via S (thiocyanato) or N (isothiocyanato). Ligands like C2O42− (oxalate, binds via two O atoms simultaneously — bidentate but not ambidentate), H2O, SO42−, NH3, CH3COO−, CH3NH2 are not ambidentate.
Step-by-Step Solution
- List known ambidentate ligands: NO2−, CN−, SCN−.
- Check option (A): NO2−,CN−,C2O42− — contains NO2− and CN− (both ambidentate) → has ambidentate ligands, so NOT the answer.
- Check option (B): C2O42−,H2O,SO42− — none of these three is ambidentate → this IS the set without ambidentate ligands.
- Check option (C): SCN−,NH3,CH3COO− — contains SCN− (ambidentate) → NOT the answer. …
- AP EAPCET 2024Set ap-2024-05-17-AN1 markMCQQ.The sum of coordination number and oxidation number of the metal M in the complex [M(en)2(C2O4)]Cl is (en = ethylenediamine) (A) 8 (B) 6 (C) 7 (D) 9
›Reveal solutionSolution
This tests computing both the coordination number and the oxidation state of the metal in a mixed-ligand complex, then adding them.
Concept and Intuition
The counter-ion outside the coordination sphere balances the charge on the complex ion, which lets us back out the metal's oxidation state. The coordination number is the total count of donor atoms bonded to the metal, counting each ligand's denticity (en and oxalate are both bidentate).
Step-by-Step Solution
- Since one Cl− balances the complex, the complex ion [M(en)2(C2O4)]+ carries a +1 charge.
- Ethylenediamine (en) is a neutral ligand (charge 0); oxalate (C2O42−) carries a −2 charge.
- Charge balance: (oxidation number of M) +2(0)+(−2)=+1, giving oxidation number of M=+3. …
- AP EAPCET 2024Set ap-2024-05-17-FN1 markMCQQ.The number of ions present in tris (ethane-1, 2-diamine) cobalt (III) sulphate is (A) 2 (B) 4 (C) 5 (D) 3
›Reveal solutionSolution
The compound is [Co(en)3]2(SO4)3; dissolving it releases 2
complex cations and 3 sulfate anions, i.e. 5 ions total.
Concept and Intuition
Ethane-1,2-diamine ("en", H2NCH2CH2NH2) is a neutral bidentate
ligand, so it does not change the oxidation state contribution when coordinated. The
"tris(en)cobalt(III)" cation is [Co(en)3]3+ (Co is +3, en contributes 0
charge each). To form a neutral salt with sulfate (SO42−), you need the
overall positive and negative charges to balance.
Step-by-Step Solution
- Complex cation: [Co(en)3]3+, charge +3.
- To balance with SO42− (charge -2), find the LCM of 3 and 2, which is 6: need 2 cations (total +6) and 3 anions (total -6).
- Formula: [Co(en)3]2(SO4)3.
- On dissolving in water, this dissociates into its constituent ions: 2 complex cations [Co(en)3]3+ + 3 sulfate anions SO42− = 5 ions total …
- AP EAPCET 2024Set eng-2024-05-21-AN1 markMCQQ.Cobalt (III) chloride forms a green coloured complex 'X' with NH3. Number of moles of AgCl formed when excess of AgNO3 solution is added to 100 mL of 1M solution of 'X' is (A) 0.3 (B) 0.2 (C) 0.1 (D) 1
›Reveal solutionSolution
The green Co(III)-ammine complex is [Co(NH3)4Cl2]Cl, with only one ionizable chloride per formula unit, so 0.1 mol of the complex gives 0.1 mol of AgCl.
Concept and Intuition
Werner complexes of cobalt(III) chloride with ammonia give differently coloured isomers depending on how many Cl− and NH3 ligands are bound inside the coordination sphere versus left outside as free (ionizable) counter-ions: [Co(NH3)6]Cl3 (yellow/orange, luteo, 3 ionizable Cl−), [Co(NH3)5Cl]Cl2 (purple, purpureo, 2 ionizable Cl−), and [Co(NH3)4Cl2]Cl (green in the trans form — praseo — or violet in cis — violeo — 1 ionizable Cl−). Only ligands OUTSIDE the coordination sphere (free counter-ions) react instantly with AgNO3 to precipitate AgCl; ligands bound directly to the metal do not.
Step-by-Step Solution
- The green colour identifies the complex as trans-[Co(NH3)4Cl2]Cl (praseocobaltic chloride), where 2 Cl− are coordinated to Co and only 1 Cl− is a free, ionizable counter-ion. …
- AP EAPCET 2024Set eng-2024-05-21-FN1 markMCQQ.Impure silver ore+CN−+H2OO2[X]−+OH− [X]−+Zn→[Y]2−+Ag (pure) The co-ordination numbers of the metals in [X], [Y] are respectively (A) 3, 4 (B) 1, 4 (C) 4, 2 (D) 2, 4
›Reveal solutionSolution
This is the cyanide (Mac Arthur–Forrest) process for silver extraction: X is the dicyanoargentate(I) ion [Ag(CN)2]− (Ag coordination number 2), and Y is the tetracyanozincate(II) ion [Zn(CN)4]2− (Zn coordination number 4).
Concept and Intuition
Silver ores are leached with aerated cyanide solution, forming a soluble silver–cyanide complex; pure silver is then recovered by displacing it with a more reactive metal (zinc), which itself forms a cyanide complex.
Step-by-Step Solution
- Leaching step: 4Ag+8CN−+O2+2H2O4[Ag(CN)2]−+4OH−. Here X−=[Ag(CN)2]−; silver is bonded to two CN⁻ ligands, so its coordination number is 2.
- Displacement (cementation) step: 2[Ag(CN)2]−+Zn→[Zn(CN)4]2−+2Ag (pure). Here Y2−=[Zn(CN)4]2−; zinc is bonded to four CN⁻ ligands, so its coordination number is 4. …
- AP EAPCET 2023Set eng-2023-05-16-FN1 markMCQQ.Which one of the following has the highest molar conductivity? (A) Diammine dichloroplatinum (II) (B) Tetraamminedichlorocobalt (III) chloride (C) Potassium hexacyano ferrate (II) (D) Hexa aquo chromium (III) chloride
›Reveal solutionSolution
Molar conductivity of an electrolyte scales with the total number of ions it dissociates into; K₄[Fe(CN)₆] gives the most ions (5) among the four choices.
Concept and Intuition
For coordination compounds, the counter ions outside the coordination sphere (square brackets) dissociate freely, while ligands inside the sphere do not contribute extra ions. More ions in solution (both in number and charge) generally means higher molar conductivity, all else being similar.
Step-by-Step Solution
- (A) [Pt(NH3)2Cl2]: both Cl are ligands (inside brackets) — complex is neutral, dissociates into 0 ions.
- (B) [Co(NH3)4Cl2]Cl: one Cl is outside as counter-ion, complex cation is +1 — dissociates into 2 ions total.
- (C) K4[Fe(CN)6]: 4 K⁺ ions plus 1 [Fe(CN)6]4− ion — 5 ions total, the most of the four. …
- AP EAPCET 2023Set eng-2023-05-18-AN1 markMCQQ.The compounds having coordinated water are CrCl3.6H2O (I) BaCl2.2H2O (II) CuSO4.5H2O (III) (A) II, III only (B) I, III only (C) I, II only (D) I, II, III
›Reveal solutionSolution
CrCl3⋅6H2O and CuSO4⋅5H2O have genuinely coordinated water; BaCl2⋅2H2O has simple water of crystallization.
Concept and Intuition
Water in a hydrate can be present in two structurally different ways: coordinated (directly bonded to the metal ion as a ligand, inside the coordination sphere) or water of crystallization (held in the crystal lattice by weaker hydrogen bonds/ionic packing forces, not bonded to the metal). Transition-metal complexes with well-defined coordination numbers (like Cr3+, Cu2+) commonly show coordinated water, whereas simple ionic salts of larger, less strongly coordinating cations like Ba2+ typically just have lattice/crystallization water.
Step-by-Step Solution
- CrCl3⋅6H2O: exists as [Cr(H2O)6]Cl3, a well-known octahedral hexaaqua complex — all six water molecules are coordinated.
- BaCl2⋅2H2O: Ba2+ is a large, weakly polarizing ion that does not form a strong discrete aqua-complex here; the two waters are water of crystallization in the lattice, not coordinated. …
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