This chapter explores coordination compounds, which are essential in modern inorganic chemistry. Understanding these compounds enhances knowledge of chemical bonding and their applications in various fields.
Coordination Compounds – Formula & Equation Sheet
Essential formulas and equations from Chemistry - I, tailored for Class 12 in Chemistry.
This one-pager compiles key formulas and equations from the Coordination Compounds chapter of Chemistry - I. Ideal for exam prep, quick reference, and solving time-bound numerical problems accurately.
Key concepts & formulas
Essential formulas, key terms, and important concepts for quick reference and revision.
Formulas
Coordination Number (CN) = Number of Ligands directly bonded to the central atom
CN is defined by the number of donor atoms in ligands directly bonded to the metal ion. E.g., in [Co(NH3)6]3+, CN = 6.
Primary Valence + Secondary Valence = Total Valence of Metal Ion
Primary valence relates to the ionizable links (usually anions), while secondary valence refers to the coordination number.
[M(L)n]^(z) = M + L_1 + L_2 + ... + L_n
A general representation of coordination complexes, where M is the metal, L are ligands, and z is the charge of the complex.
Isomer Count = 1/2(n(n-1)) for Geometrical Isomers
For complex ions with n identical pairs of ligands, the formula estimates the number of geometrical isomers.
Absorbance (A) = ε * c * l
A relates to the concentration (c) of the complex and path length (l), relevant in colorimetric determination of metal concentrations.
Crystal Field Splitting Energy: Δ = h * c / λ
Used to calculate the energy difference between d-orbital sets in octahedral or tetrahedral complexes, relevant for determining colors.
Formation Constant (Kf) = [Complex] / ([Metal]^a * [Ligand]^b)
Defines the stability of a coordination complex. Higher Kf indicates more stability of the complex.
Stability Constant Kst = (complex ion concentration) / (concentration of reactants)
Describes the stability of a coordination compound; greater Kst suggests more stable complexes with ligands.
m = (Number of moles disassociated) / (Initial moles of complex)
Useful in determining the degree of dissociation and the effective concentration of resulting ions.
Ligand field strength: I- < Br- < Cl- < OH- < H2O < NH3 < en < CN- < CO
Reflects the increasing ability of ligands to cause splitting of d-orbitals; affects the inner/outer orbital complex formation.
Equations
[Co(NH3)6]Cl3 → [Co(NH3)6]3+ + 3Cl-
An example of dissociation in coordination compounds where 3 chloride ions are released.
Kf = [Complex] / {Cation}^p[Anion]^q
The formation constant equation used in coordination chemistry to determine the stability of complexes.
Color change: [Fe(H2O)6]3+ (orange) + CN- → [Fe(CN)6]3- (yellow)
Illustrates a reaction resulting in a visible color change, indicating the formation of a new complex.
Optical Isomerism: [Co(en)3]Cl3 ⇌ [Co(en)3]Cl3 (enant. pairs)
Describes the formation of optical isomers in coordination compounds.
[Ag(NH3)2]+ + AgCl → [Ag(NH3)2]Cl + Cl-
Proof of equilibrium in coordination reactions demonstrating ligand exchange.
Δo = E_g - E_t2
Energy difference calculation in octahedral field theory, crucial for predicting the magnetism of the complex.
[MnO4]- + 8H+ + 5e- → Mn2+ + 4H2O
Half-equation showing the reduction of permanganate ion, relevant in redox reactions involving coordination complexes.
Absorption: A = log10(I0/I)
Beer-Lambert Law for measuring the absorbance of complexes in solution.
[Co(NH3)4Cl2]+ + H2O → [Co(NH3)4Cl(H2O)]+ + Cl-
Example of ligand substitution reaction and its effect on the complex's properties.
Oxidation State: Co in [Co(NH3)6]Cl3 = +3
Identifying the oxidation state of the metal in coordination complexes.
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