Crystal field is the energy the crystal possesses due to the orientation of the d-orbitals of the transition metal ion and the coordinating ligands. The crystal field depends on the nature of the ligand, the metal ion's charge, and the transition metal's position in the periodic table. Crystal field theory (CFT) is an electrostatic model that assumes that the metal-ligand bond in a transition metal complex is purely ionic, formed of electrostatic interactions between the metal ion and ligand. 

Crystal Field Theory

Crystal Field Theory (CFT) was introduced by physicist Hans Bethe in 1929 to explain how metal ions behave in crystals. It helps us understand how bonding works in metal complexes, why they show certain colors, and their magnetic properties. The theory is based on the idea that when ligands( molecules or ions that surround the metal) come close to a metal ion, they create an electric field. This field affects the energy levels of the metal’s d-orbitals, which are normally all equal. Due to this interaction, the d-orbitals split into different energy levels, a process known as crystal field splitting. This explains why transition metal complexes have specific properties.

In octahedral complexes, a central metal ion is surrounded by six ligands. These ligands interact with the metal’s five d-orbitals, causing them to split into two energy levels due to repulsion.

• Higher energy (e.g. orbitals): dx2-y2 and dz2, which point directly at ligands.
• Lower energy (t2g orbitals): dxy,dxz, and dyz, which lie between ligands.

The energy difference between these two sets is called crystal field splitting energy(Δ₀)

Eg orbitals are at +0.6 Δ₀

T2g orbitals are at -0.4 Δ₀

Chemistry Notes Free PDFs

The size of Δ₀ depends on the strength of the ligands:

Weak field ligands (e.g., Cl-)→ small Δ₀, high-sign complexes (more unpaired electrons)

Strong field ligands (e.g., CN-, NH3)→ large Δ₀, low spin complexes (more electron pairing).

Examples:

• [Fe(CN)6]4– – low spin
• [CO(NH3)6]3+ – low spin

Crystal Field Splitting in Tetrahedral Complexes

Tetrahedral Complexes are formed when a central metal ion is surrounded by four ligands. Unlike octahedral complexes, the pattern of d-orbital splitting in tetrahedral complexes is reversed.

In this case:

• The dxy,dxz, and dyz orbitals face more repulsion from the ligands and move to a higher energy level.
• The dx2-y2 and dz2 orbitals face less repulsion and stay at a lower energy level.

The difference in energy between these two sets is called the crystal field splitting energy (Δt).

This energy gap is much smaller than in octahedral complexes– about 4/9 of Δ₀.

Because the energy gap is small, electrons in tetrahedral complexes usually do not pair up. This leads to high-spin configurations (more unpaired electrons).

Examples:

[Fe(H2O)6]2+

[CoF6]3-

Crystal Field Stabilization Energy (CFSE)

When ligands approach a transition metal ion, they cause the d-orbitals to split into two energy levels. The energy difference between these levels is called crystal field splitting energy. When electrons fill the lower-energy orbistals, the complex becomes more stable. The stability is called Crystal Field Stabilization Energy (CFSE).

CFSE is calculated using the formula:

CFSE= Energy of the ligand field - Energy of a regular (isotropic) field

In simple terms, it tells us how more stable the complex becomes due to the presence of ligands, CFSE values vary depending on the shape of the complex:

1. For tetrahedral complexes- the splitting is smaller, so CFSE is generally lower.

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1. For octahedral complexes- the splitting is larger, which often results in higher CFSE.

Postulates Of Crystal Field Theory

The postulates of crystal field theory are-

• In crystal field theory, we assume that the metal ion is surrounded by an electric field created by the ligands surrounding the metal ion.
• The forces of attraction between the central metal ion and the ligand are considered purely electrostatic. The metal ion is targeted by the negative end of the dipole of the neutral molecule ligand.
• The transition metal ion is a positive charge ion equal to the oxidation state.
• The transition metal atom is surrounded by a specific number of ligands, which may be negative ions or neutral molecules having lone pairs of electrons.
• Ligands act as point charges that are responsible for generating an electric field. This electric field changes the energy of the orbitals on the metal atom or ions.
• The repulsive force between the central metal ion and ligand is responsible for the electrons of the metal ion occupying the d-orbitals as far as possible from the direction of approach of the ligand.
• There is no interaction between metal orbital and ligand orbitals.
• In an isolated metal atom or ion, all the orbitals have the same energy, which means all the d-orbitals are degenerate. 
• If the central metal atom or ion is surrounded by the spherical symmetrical field of negative charges, the d-orbitals degenerate. However, the energy of orbitals is raised due to the repulsion between the field and the electron on the metal atom or ion.
•  The d-orbitals are affected differently in most transition metal complexes, and their degeneration is lost due to the field produced by the unsymmetrical ligand.

Limitations of Crystal Field Theory (CFT)

While Crystal Field Theory helps us understand many things about metal complexes, it also has some limitations:

• Doesn’t Explain Covalent Bonding: CFT only considers ionic (electrostatic) interactions between the metal ion and ligands. But in many real-life complexes, covalent bonding also happens, which this theory does not account for.
• Struggles with Spectrochemical series: CFT can’t fully explain the order of ligands in the spectrochemical series. For instance, since ligands are treated as point charges, the theory suggests that negatively charged ligands (like OH-) should cause stronger splitting than neutral ones (like H2O). But in reality, water is a stronger field ligand than hydroxide– something CFT can't explain.
• Ignores s and p Orbitals: The theory focuses only on d-orbitals of the metal and does not consider s or p orbitals, which play an important role in bonding, especially when π- bonding is involved.
• Doesn’t Include Ligand Orbitals: CFT does not take into account the orbitals of the ligands. As a result, it can’t explain how ligand orbitals are intricate with metal orbitals, which is important in understanding the full bonding picture.

Difference Between Crystal Field Theory and Ligand Field Theory

The difference between crystal field theory and ligand field theory are-

Applications of Crystal Field Theory (CFT)

1.Stability of complexes:

CFT helps calculate Crystal Field Stabilization Energy (CFSE). A higher CFSE means a more stable metal complex.

Example (low-spin d4): CFSE =-1.6 Δ₀

2.Magnetic Properties:

It explains whether a complex is magnetic (paramagnetic) or non-magnetic (diamagnetic) based on unpaired electrons.

3. Color of Complexes:

CFT explains the color of metal complexes due to d-d electron transition, used in dyes and pigments.

4. High-Spin vs Low-Spin:

Predicts if a complex is high spin or low-spin depending on ligand strength and orbital splitting.

Learn more about periodic table

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