Inorganic Chemistry
Summary

Transition metals and complexes. From coordination chemistry to ligand field theory.

Transition Metals

Properties

• Variable oxidation states
• Colored compounds
• Catalytic activity
• Complex ion formation
• Magnetic properties

Electronic Configuration

[Ar] 3d¹-¹⁰ 4s¹-²
Loss: 4s before 3d
Cu: [Ar] 3d¹⁰ 4s¹ (exception)
Cr: [Ar] 3d⁵ 4s¹ (exception)

Coordination Chemistry

Complex Ions

[M(L)ₙ]ˣ⁺
M = central metal ion
L = ligand
n = coordination number
x = charge on complex

Ligands

Monodentate: NH₃, H₂O, Cl⁻
Bidentate: en (ethylenediamine)
Polydentate: EDTA (hexadentate)
Ligand strength: I⁻ < Br⁻ < Cl⁻ < F⁻ < OH⁻ < H₂O < NH₃ < en < NO₂⁻ < CN⁻ < CO

Ligand Field Theory

Crystal Field Splitting

Octahedral: t₂g and eₐ
Tetrahedral: e and t₂
Square planar: complex splitting

Δ = 10Dq (splitting energy)

Color

E = hν = hc/λ
Complementary colors absorbed
Small Δ: absorb red → appear blue-green
Large Δ: absorb violet → appear yellow

Download

Print this page or save as PDF for quick reference.

Tip: Use Ctrl+P (Cmd+P on Mac) to print or save as PDF.