This chapter covers the properties, electronic configurations, and significance of the d-and f-block elements in the periodic table, highlighting their applications and roles in various processes.
The d-and f-Block Elements – 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 The d-and f-Block Elements 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
E = nRT
E represents energy (in joules), n is the number of moles, R is the universal gas constant (8.314 J/(mol·K)), and T is the temperature (in Kelvin). This formula relates the energy of an ideal gas to the number of moles and temperature.
ΔG = ΔH - TΔS
ΔG is the Gibbs free energy change, ΔH is the enthalpy change, T is the temperature (in Kelvin), and ΔS is the entropy change. It indicates the spontaneity of a reaction.
n = (V × P) / (R × T)
n is the number of moles, V is the volume in liters, P is the pressure in atm, R is the gas constant (0.0821 L·atm/(mol·K)), and T is the temperature in Kelvin. This equation is derived from the ideal gas law.
[M(n-H2O)x]y+ + zL → [M(n-H2O)xLz] + yH2O
This represents a general formation of a complex between a metal ion (M) and a ligand (L). It indicates the substitution of water molecules in a hydration sphere by ligands.
Ksp = [Ag+]^2[Br^-]^2
Ksp is the solubility product constant for a salt, where [Ag+] and [Br^-] are the molar concentrations of the respective ions at saturation. This relationship is crucial in determining the solubility of ionic compounds.
ΔH ≈ TΔS
This approximation applies when a reaction is at equilibrium. The Gibbs energy change is zero, indicating that the forward and reverse processes occur at equal rates.
E°(MnO4−/Mn2+) = +1.51 V
This standard electrode potential value indicates the relative strength of the MnO4− ion as an oxidizing agent.
E°(Cr2O7^2−/Cr^3+) = +1.33 V
This standard electrode potential signifies the ability of dichromate to act as an oxidizing agent in acidic solutions.
Fe3+ + e− ↔ Fe2+ (E° = +0.77 V)
This equation represents the half-reaction of iron reduction, critical for understanding redox processes.
5C2O4^2− → 10CO2 + 10e−
This equation shows the oxidation of oxalate ion to carbon dioxide, significant in redox reactions with potassium permanganate.
Equations
K2Cr2O7 + 14H+ + 6e− → 2Cr3+ + 7H2O (E°= 1.33 V)
This reaction depicts the reduction of dichromate in acidic medium, illustrating its role as a strong oxidizing agent.
MnO4− + 8H+ + 5e− → Mn2+ + 4H2O (E°= 1.51 V)
This equation represents the reduction of permanganate ion to manganese(II) ion, useful in redox titrations.
2Cu+ → Cu2+ + Cu (disproportionation)
This disproportionation reaction demonstrates the tendency of Cu+ to oxidize itself to Cu2+ and reduce to Cu metal.
5Fe2+ + MnO4− + 8H+ → 5Fe3+ + Mn2+ + 4H2O
This is the overall reaction for the oxidation of iron(II) ions by permanganate in acidic conditions.
2Cr2O7^2− + 14H+ + 6e− → 4Cr^3+ + 7H2O
This chemical equation illustrates the reduction of dichromate to chromium ions, highlighting its oxidative properties.
Mn2O7 + 4H2O → 2MnO4− + 8H+ + 6e−
This reaction shows the transformation of manganese oxides, relevant in understanding manganese chemistry.
C2O4^2− + 2MnO4− + 16H+ → 2Mn2+ + 8H2O + 10CO2
This redox reaction highlights how oxalate acts as a reducing agent for permanganate.
2Mn4+ + 3I− → 2Mn2+ + I2
In this redox reaction, manganese is reduced, showcasing the electron transfer processes in transition metals.
NO3− + 2Fe2+ + 2H+ → 2Fe3+ + H2O + NO
This reaction demonstrates the reduction of nitrate by iron(II), useful in determining oxidation states.
5Mn2+ + 2MnO4− + 16H+ → 7Mn3+ + 8H2O
This illustrates the redox reaction of manganous ions with permanganate, stressing manganese's versatile oxidation states.
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