The CFSE for octahedral $[CoCl_6]^{4-}$ is $18,000\ \text{cm}^{-1}$. The CFSE for tetrahedral $[CoCl_4]^{2-}$ will be (i) $18,000\ \text{cm}^{-1}$ (ii) $16,000\ \text{cm}^{-1}$ (iii) $8,000\ \text{cm}^{-1}$ (iv) $20,000\ \text{cm}^{-1}$

The CFSE for octahedral [CoCl₆]⁴⁻ is 18,000cm⁻¹. The CFSE for tetrahedral [CoCl₄]²⁻ will be (i) 18,000cm⁻¹ (ii

NCERT Exemplar · Q8

[CoCl_6]^{4-}

(i)

18,000\ \text{cm}^{-1}

(ii)

16,000\ \text{cm}^{-1}

(iii)

8,000\ \text{cm}^{-1}

(iv)

20,000\ \text{cm}^{-1}

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Concept understanding — Crystal Field Splitting

Crystal Field Splitting: From Intuition to Precision

Imagine you are a negatively charged electron sitting on a metal ion. All around you, the space is perfectly spherical — every direction feels the same. Your energy depends only on how far you are from the nucleus, not on which way you face.

Now imagine that six negative ions (or the negative ends of polar molecules) march in from the $x$ , $y$ , and $z$ axes and stop close to you. Suddenly, the space around you is no longer uniform. If you try to move straight toward one of these approaching ions, you feel a strong repulsion — that path costs extra energy. If you move between the axes (say, along a diagonal), you feel less repulsion because you are farther from the incoming charges.

This is the core intuition: when ligands approach a metal ion, they break the spherical symmetry of the space around the metal. Different directions in space are no longer equivalent. Electrons in orbitals that point directly at the ligands get pushed up in energy; electrons in orbitals that point between the ligands stay lower.

The Precise Statement

d

For the most common geometry — octahedral — here is what happens:

Six ligands sit at the corners of an octahedron, along the $+x$ , $-x$ , $+y$ , $-y$ , $+z$ , $-z$ axes.
The $d_{x^2-y^2}$ and $d_{z^2}$ orbitals point their lobes directly along these axes. These are the $e_g$ set. They feel maximum repulsion → higher energy.
The $d_{xy}$ , $d_{xz}$ , and $d_{yz}$ orbitals point their lobes between the axes (into the octahedral faces). These are the $t_{2g}$ set. They feel less repulsion → lower energy.

The energy gap between these two sets is denoted by $\Delta_o$ (or $10\,Dq$ ). The $t_{2g}$ set drops by $0.4\Delta_o$ and the $e_g$ set rises by $0.6\Delta_o$ , keeping the average energy unchanged (the "barycentre" rule).

Note

The labels $e_g$ and $t_{2g}$ come from group theory — they describe how the orbitals transform under the symmetry operations of an octahedron. You do not need to memorise the derivation, but the notation is standard in every exam.

Why This Matters

Crystal field splitting explains three things you will see repeatedly:

Colour — electrons can jump from $t_{2g}$ to $e_g$ by absorbing visible light. The gap $\Delta_o$ determines the colour you see.
Magnetism — if $\Delta_o$ is large, electrons pair up in the lower $t_{2g}$ set (low spin). If $\Delta_o$ is small, electrons spread out (high spin). This changes the number of unpaired electrons. …

Why this formula?

Crystal Field Splitting: Why the Energy Splitting Occurs

Crystal Field Theory (CFT) explains how the d-orbitals of a transition metal ion split in energy when placed in an electrostatic field created by surrounding ligands (anions or polar molecules). The key result is that five degenerate d-orbitals split into two or more sets with different energies. Let's understand why this happens.

1. The Starting Point: Degenerate d-Orbitals

In a free transition metal ion (no ligands), all five d-orbitals have the same energy (degenerate). Their shapes are:

$d_{xy}$ , $d_{xz}$ , $d_{yz}$ — lobes lie between the x, y, z axes (called $t_{2g}$ set in octahedral symmetry)
$d_{x^2-y^2}$ , $d_{z^2}$ — lobes point directly along the x, y, z axes (called $e_g$ set)

Key idea: The spatial orientation of each orbital determines how it interacts with approaching ligands.

2. The Octahedral Case: Why $e_g$ Orbitals Are Higher in Energy

Imagine six ligands approaching along the +x, –x, +y, –y, +z, –z axes (octahedral geometry).

What happens to $d_{x^2-y^2}$ and $d_{z^2}$ ?

Their lobes point directly at the ligands.
The negatively charged ligands repel the electron density in these orbitals.
This repulsion raises the energy of these orbitals — they become less stable (higher energy).

What happens to $d_{xy}$ , $d_{xz}$ , $d_{yz}$ ?

Their lobes point between the axes (e.g., $d_{xy}$ lobes lie in the xy-plane but at 45° to x and y).
They avoid the ligands — less repulsion.
Their energy is lower than the $e_g$ set.

The Splitting Pattern

\Delta_{\text{oct}} = E(e_g) - E(t_{2g})

Where:

$E(e_g)$ = energy of $d_{x^2-y^2}$ and $d_{z^2}$ (higher)
$E(t_{2g})$ = energy of $d_{xy}$ , $d_{xz}$ , $d_{yz}$ (lower)
$\Delta_{\text{oct}}$ is called the crystal field splitting energy (CFSE)

Why the name? The $e_g$ orbitals are "doubly degenerate" (2 orbitals), $t_{2g}$ are "triply degenerate" (3 orbitals). The letters come from group theory symmetry labels.

3. The Energy Conservation Rule

The total energy of all five d-orbitals must remain constant (no energy is created or destroyed). So:

The center of gravity (average energy) of the split set equals the original degenerate energy.
For octahedral splitting:
- 2 $e_g$ orbitals go up by $+0.6\Delta_{\text{oct}}$ each
- 3 $t_{2g}$ orbitals go down by $-0.4\Delta_{\text{oct}}$ each

Check:

2 \times (+0.6\Delta) + 3 \times (-0.4\Delta) = 1.2\Delta - 1.2\Delta = 0

This conservation of energy is a fundamental constraint — the splitting is not arbitrary.

4. The Tetrahedral Case: Why It's Opposite and Smaller

In a tetrahedral complex, four ligands approach from alternate corners of a cube. The axes are different:

The $d_{xy}$ , $d_{xz}$ , $d_{yz}$ orbitals now point closer to the ligands (more repulsion).
The $d_{x^2-y^2}$ and $d_{z^2}$ orbitals point away from ligands (less repulsion).

Result:

$e$ set ( $d_{x^2-y^2}$ , $d_{z^2}$ ) — lower energy
$t_2$ set ( $d_{xy}$ , $d_{xz}$ , $d_{yz}$ ) — higher energy

The splitting is inverted compared to octahedral.

Magnitude:

\Delta_{\text{tet}} \approx \frac{4}{9} \Delta_{\text{oct}}

Why smaller?

Only 4 ligands (vs. 6) → less total repulsion.
Ligands are not directly along axes → weaker interaction. …

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Using the standard relation $\Delta_t = \tfrac{4}{9}\,\Delta_o$ , the tetrahedral stabilization scales as $\tfrac{4}{9}$ of the octahedral value: $\tfrac{4}{9}\times 18{,}000 = 8{,}000\ \text{cm}^{-1}$ . The answer is (iii).

Setup. In both complexes the metal is $\text{Co}^{2+}$ ( $d^7$ ) with the same weak-field $\text{Cl}^-$ ligands. The only quantity that changes on going from octahedral to tetrahedral geometry is the size of the crystal-field splitting.

Key relation. For the same metal ion and the same ligands,

$\Delta_t = \frac{4}{9}\,\Delta_o.$ …

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Common Mistakes Students Make on This CFSE Problem

Mistake 1: Forgetting the Geometry Factor (Δₜ = 4/9 Δₒ)

The error: Students directly use the same CFSE value for tetrahedral as octahedral, or apply a wrong ratio.

Why it’s wrong:

Crystal Field Splitting in tetrahedral complexes is smaller than in octahedral. The relationship is:

\Delta_t = \frac{4}{9} \Delta_o

Here, $\Delta_o = 18,000\ \text{cm}^{-1}$ , so:

\Delta_t = \frac{4}{9} \times 18,000 = 8,000\ \text{cm}^{-1}

How to avoid: Always recall: tetrahedral splitting is always $\frac{4}{9}$ of octahedral splitting for the same metal and ligand.

Mistake 2: Ignoring the d-electron Count and CFSE Formula

The error: Students calculate $\Delta_t$ but forget that CFSE depends on how electrons fill the $t_2$ and $e$ orbitals.

Why it’s wrong:

For $[CoCl_6]^{4-}$ , Co is in +2 state → $d^7$ configuration.

In octahedral: $t_{2g}^5 e_g^2$ (high spin, weak field ligand Cl⁻).

CFSE = $[5 \times (-0.4) + 2 \times (0.6)] \Delta_o = (-2 + 1.2) \Delta_o = -0.8 \Delta_o$

For tetrahedral $[CoCl_4]^{2-}$ (also $d^7$ , weak field):

Configuration: $e^4 t_2^3$

CFSE = $[4 \times (-0.6) + 3 \times (0.4)] \Delta_t = (-2.4 + 1.2) \Delta_t = -1.2 \Delta_t$

So CFSE (tet) = $-1.2 \times 8,000 = -9,600\ \text{cm}^{-1}$ — but the question asks for $\Delta_t$ , not CFSE.

How to avoid: Read carefully — does the question ask for CFSE or Δ? Here it asks for CFSE of tetrahedral, which is not simply $\frac{4}{9} \times$ octahedral CFSE.

Mistake 3: Confusing Δ with CFSE

The error: Students treat $\Delta$ and CFSE as the same quantity.

Why it’s wrong:

$\Delta$ is the splitting energy between $t_2$ and $e$ sets.

CFSE is the net energy stabilization after placing electrons, given by:

\text{CFSE} = \left[ -0.4 \times n(t_{2g}) + 0.6 \times n(e_g) \right] \Delta_o \quad \text{(octahedral)}

\text{CFSE} = \left[ -0.6 \times n(e) + 0.4 \times n(t_2) \right] \Delta_t \quad \text{(tetrahedral)}

How to avoid: Always write the electron configuration and apply the correct CFSE formula — never skip this step.

Mistake 4: Using the Wrong d-Orbital Splitting Pattern

The error: Students apply octahedral orbital labels ( $t_{2g}, e_g$ ) to tetrahedral geometry.

Why it’s wrong:

In tetrahedral, the splitting is inverted:

Lower energy: $e$ set ( $d_{x^2-y^2}, d_{z^2}$ ) …

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Same / Similar Concept — real previous-year questions on the same or a closely similar concept, not this exact question.

GSEB Higher Secondary Certificate (HSC) Examination 2026Set ANNUAL1 markMCQ
$Q. The crystal field splitting energy for octahedral (delta o) and tetrahedral (delta t) complexes is related as$
(a) delta t = 1/2 delta o
(b) delta t = 4/9 delta o
(c) delta t = 3/9 delta o
(d) delta t = 3/2 delta o
›Reveal solutionSolution

By crystal field theory, the tetrahedral crystal field splitting energy is always 4/9 of the octahedral splitting energy for the same metal ion and ligands.

In an octahedral field, 6 ligands point directly at the d-orbitals, producing a relatively large splitting (Δo). In a tetrahedral field, only 4 ligands are present and none point directly at any d-orbital (they approach between the axes), which weakens the splitting considerably. Crystal field theory shows the two splittings are rela …

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GUJCET 2025Set 031 markMCQ
$\Delta_{0}$
›Reveal solutionSolution
[!TLDR]

$[Co(CN)_6]^{3-}$ has the maximum $\Delta_0$ because $CN^-$ is the strongest-field ligand.

Concept

For a given metal and oxidation state, the crystal-field splitting energy $\Delta_0$ increases with the field strength of the ligands, ordered by the spectrochemical series: $Cl^- < H_2O < NH_3 < CN^-$ .

Solution

Cobalt is $Co^{3+}$ ( $d^6$ ) in every option, so compare ligand fields:

$[CoCl(NH_3)_5]^{2+}$ : one weak $Cl^-$ plus five $NH_3$ — lowered field.

$[Co(NH_3)_5(H_2O)]^{3+}$ : one $H_2O$ (weaker than $NH_3$ ) plus five $NH_3$ . …
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GUJCET 2023Set 091 markMCQ
$t_{2g}^4 e_g^0$
›Reveal solutionSolution

Electrons pair in $t_{2g}$ (low spin) only when the splitting exceeds the pairing energy: $\Delta_0 > P$ .

Concept: For a $d^4$ octahedral ion, the fourth electron either enters $e_g$ (high spin, $t_{2g}^3e_g^1$ ) or pairs in $t_{2g}$ (low spin, $t_{2g}^4e_g^0$ ). Pairing is favoured when …
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GSEB Higher Secondary Certificate (HSC) Examination 2022Set ANNUAL1 markMCQ
$Q. For a high-spin complex, which relation is correct (comparing crystal field splitting energy Delta and pairing energy P)?$
(a) Delta < P
(b) Delta = P
(c) Delta > P
(d) Delta0 >= P
›Reveal solutionSolution

Whether electrons pair up in the lower t2g set or spread out with parallel spins into eg depends on comparing the crystal field splitting energy (Delta) with the pairing energy (P).

If Delta (the energy gap created by the ligand field) is SMALLER than the pairing energy P, it costs less energy for electrons to occupy the higher eg orbitals singly (Hund's rule) than to pair up in t2g - this gives the maximum number of unpaired electro …

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GUJCET 2020Set 071 markMCQ
$[Co(NH_3)_6]^{3+}$
›Reveal solutionSolution

Longest $\lambda$ ⇔ smallest crystal-field split $\Delta_o$ ; $[\text{CoCl(NH}_3)_5]^{2+}$ has the weakest-field set.

Concept — spectrochemical series. $\lambda_{max}\propto 1/\Delta_o$ . Field strength: $\text{CN}^->\text{NH}_3>\text{H}_2\text{O}>\text{Cl}^-$ . Replacing an NH₃ with the weak-field Cl⁻ gives the lowest $\Delta_o$ of the set, hence absorption …
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GUJCET 2019Set 131 markMCQ
$d_{x^2-y^2} > d_{z^2} > d_{xy} \cong d_{yz} \cong d_{z^2}$
›Reveal solutionSolution

Tetrachloridonickelate(II) is tetrahedral, so $t_2 (d_{xy}, d_{yz}, d_{zx})$ are HIGHER in energy than $e (d_{x^2-y^2}, d_{z^2})$ .

Concept: $[NiCl_4]^{2-}$ has $Cl^-$ (weak field) around $Ni^{2+}$ ; it is tetrahedral. In a tetrahedral field the d-orbital splitting is the inverse of octahedral: the three $t_2$ orbitals ( $d_{xy}, d_{yz}, d_{zx}$ ) point closer to the ligand approach directions and are raised, while the two $e$ orbitals ( $d_{x^2-y^2}, d_{z^2}$ ) are lowered.

Thus the correct energy order is: …
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GSEB Higher Secondary Certificate (HSC) Examination 2019Set ANNUAL1 markMCQ
$Q. For which complex from following value of delta-o (crystal field splitting energy) will be lowest?$
(a) [Co(NH3)6]3+
(b) [Co(CN)6]3-
(c) [Co(H2O)6]3+
(d) [Co(C2O4)3]3-
›Reveal solutionSolution

Crystal field splitting energy (delta-o) depends on the field strength of the coordinated ligand, ranked by the spectrochemical series.

The spectrochemical series (increasing field strength, hence increasing delta-o) relevant here is approximately:

C2O4^2- (oxalate) < H2O < NH3 < CN- …

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GUJCET 2015Set C1 markMCQ
$SCN^- < F^- < NH_3 < en < CO$
›Reveal solutionSolution
[!TLDR] Correct increasing field strength: SCN $^-$ < F $^-$ < NH $_3$ < en < CO.

Concept

The spectrochemical series ranks ligands by the crystal-field splitting they produce. A commonly used ordering (weak to strong field) is:

$I^- < Br^- < SCN^- < Cl^- < F^- < OH^- < ox < H_2O < NH_3 < en < CN^- < CO$ .

Solution

Place the given ligands on this scale:

SCN $^-$ (S-bonded, thiocyanate) — weak field, lowest here.

F $^-$ — stronger than SCN $^-$ .

NH $_3$ — stronger than F $^-$ . …
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←Previous questionQ7 — Indicate the complex ion which shows geometrical isomerism. (i) [Cr(H₂…→Next questionQ9 — Due to the presence of ambidentate ligands coordination compounds show…

Q.The CFSE for octahedral $[CoCl_6]^{4-}$ is $18,000\ \text{cm}^{-1}$ . The CFSE for tetrahedral $[CoCl_4]^{2-}$ will be

Concept understanding — Crystal Field Splitting

Crystal Field Splitting: From Intuition to Precision

The Precise Statement

Why This Matters

Why this formula?

Crystal Field Splitting: Why the Energy Splitting Occurs

1. The Starting Point: Degenerate d-Orbitals

2. The Octahedral Case: Why $e_g$ Orbitals Are Higher in Energy

What happens to $d_{x^2-y^2}$ and $d_{z^2}$ ?

What happens to $d_{xy}$ , $d_{xz}$ , $d_{yz}$ ?

The Splitting Pattern

3. The Energy Conservation Rule

4. The Tetrahedral Case: Why It's Opposite and Smaller

Result:

Magnitude:

Method: Crystal Field Splitting Ratio Rule for Tetrahedral vs Octahedral Complexes

Why this method works

Steps to solve

Common Mistakes Students Make on This CFSE Problem

Mistake 1: Forgetting the Geometry Factor (Δₜ = 4/9 Δₒ)

Mistake 2: Ignoring the d-electron Count and CFSE Formula

Mistake 3: Confusing Δ with CFSE

Mistake 4: Using the Wrong d-Orbital Splitting Pattern

Concept

Solution

Concept

Solution

Q.The CFSE for octahedral [CoCl6]4−[CoCl_6]^{4-}[CoCl6​]4− is 18,000 cm−118,000\ \text{cm}^{-1}18,000 cm−1. The CFSE for tetrahedral [CoCl4]2−[CoCl_4]^{2-}[CoCl4​]2− will be

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Q.The CFSE for octahedral $[CoCl_6]^{4-}$ is $18,000\ \text{cm}^{-1}$ . The CFSE for tetrahedral $[CoCl_4]^{2-}$ will be

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