FSc Chemistry Formulas
All FSc Chemistry formulas, chapter by chapter, with search and a printable layout.
This page covers both years of FSc/ICS. The formulas are listed by chapter and are not split into Part-I and Part-II.
Atomic Structure (10)
| Formula | Expression |
|---|---|
| Bohr's Energy | Eₙ = -13.6/n² eV |
| Rydberg Equation | 1/λ = R(1/n₁² - 1/n₂²) |
| Number of Electrons in Shell | max e⁻ = 2n² |
| Bohr Radius | rₙ = n²h²/(4π²mke²) |
| Energy Levels (Bohr) | Eₙ = −13.6/n² eV |
| de Broglie Wavelength | λ = h/mv |
| Heisenberg's Uncertainty Principle | Δx·Δp ≥ h/4π |
| Frequency-Wavelength Relation | c = νλ |
| Principal Quantum Number | n = 1, 2, 3... defines the energy level |
| Azimuthal Quantum Number | l = 0 to (n−1) |
Gas Laws (15)
| Formula | Expression |
|---|---|
| Ideal Gas | PV = nRT |
| Boyle's Law | P₁V₁ = P₂V₂ |
| Charles's Law | V₁/T₁ = V₂/T₂ |
| Gay-Lussac's Law | P₁/T₁ = P₂/T₂ |
| Avogadro's Law | V₁/n₁ = V₂/n₂ |
| Graham's Law of Diffusion | r₁/r₂ = √(M₂/M₁) |
| Dalton's Law | Pₜ = P₁+P₂+P₃+... |
| Combined Gas Law | P₁V₁/T₁ = P₂V₂/T₂ |
| Kinetic Energy of Gas | KE = (3/2)RT (per mole) |
| Root Mean Square Speed | vrms = √(3RT/M) |
| Real Gas Deviation (Z) | Z = PV/nRT |
| Molar Mass from Gas Density | M = dRT/P |
| Universal Gas Constant Value | R = 0.0821 L·atm/(mol·K) |
| Standard Temperature and Pressure | STP: 0°C (273 K), 1 atm |
| Partial Pressure (Mole Fraction Form) | Pi = xi × Ptotal |
Thermodynamics (8)
| Formula | Expression |
|---|---|
| 1st Law | ΔU = q + w |
| Enthalpy | H = U + PV |
| Gibbs Free Energy | ΔG = ΔH - TΔS |
| Entropy Change | ΔS = qrev/T |
| Work Done (expansion) | w = −PΔV |
| Bond Enthalpy Calculation | ΔH = Σ(bonds broken) − Σ(bonds formed) |
| Specific Heat Capacity | c = Q/(mΔT) |
| Molar Heat Capacity (Ideal Monatomic Gas) | Cv = (3/2)R |
Equilibrium (11)
| Formula | Expression |
|---|---|
| Equilibrium Constant | Kc = [C]ᶜ[D]ᵈ/[A]ᵃ[B]ᵇ |
| Kp & Kc Relation | Kp = Kc(RT)^Δn |
| Kp-Kc Relation | Kp = Kc(RT)^Δn |
| Le Chatelier's Principle | system shifts to counter applied stress |
| Solubility Product | Ksp = [Aⁿ⁺]ᵐ[Bᵐ⁻]ⁿ |
| Common Ion Effect (concept) | adding common ion shifts equilibrium, lowers solubility |
| Degree of Dissociation | α = moles dissociated/initial moles |
| Ionic Product of Water | Kw = [H⁺][OH⁻] = 10⁻¹⁴ |
| Reaction Quotient Q | Q = [Products]/[Reactants] at any time |
| Relationship Between Q and K (concept) | Q<K forward shift, Q>K reverse shift, Q=K equilibrium |
| Solubility from Ksp (AB type salt) | s = √Ksp |
Kinetics (10)
| Formula | Expression |
|---|---|
| Rate Law | Rate = k[A]ᵐ[B]ⁿ |
| Arrhenius | k = Ae^(-Ea/RT) |
| First Order Half-life | t½ = 0.693/k |
| Zero Order Half-life | t½ = [A]₀/2k |
| Second Order Integrated Rate | 1/[A] = kt + 1/[A]₀ |
| Arrhenius Equation | k = Ae^(−Ea/RT) |
| Third Order Half-life | t½ = 3/(2k[A]₀²) |
| Activation Energy (two-point) | ln(k₂/k₁) = −Ea/R(1/T₂ − 1/T₁) |
| Collision Theory Rate Constant | k = PZ_A e^(−Ea/RT) |
| Overall Reaction Order | order = sum of exponents (m + n) in rate law |
Electrochemistry (13)
| Formula | Expression |
|---|---|
| Nernst Equation | E = E° - (RT/nF)lnQ |
| Faraday's Law | m = ZIt |
| Standard Cell Potential | E°cell = E°cathode − E°anode |
| Gibbs–Cell Potential | ΔG° = −nFE° |
| Faraday's Second Law | m/M = Q/(nF) |
| Faraday Constant | F = 96500 C/mol |
| Molar Conductivity | Λm = κ/C |
| Conductivity Cell Constant | κ = G × (l/A) |
| Kohlrausch's Law | Λm° = λ°+ + λ°− |
| Standard Hydrogen Electrode | E°(SHE) = 0.00 V (reference) |
| Number of Electrons Transferred (n) | from balanced half-reaction |
| Electrolysis Mass Deposited | m = (ItM)/(nF) |
| Cell Notation Convention (concept) | anode | anode solution || cathode solution | cathode |
Solutions (13)
| Formula | Expression |
|---|---|
| Molarity | M = mol solute / L solution |
| Molality | m = mol solute / kg solvent |
| Raoult's Law | P = P°X |
| Freezing Point | ΔTf = Kf × m |
| Boiling Point | ΔTb = Kb × m |
| Osmotic Pressure | π = MRT |
| Dilution Formula | M₁V₁ = M₂V₂ |
| Mole Fraction | X_A = nₐ/(nₐ+n_b) |
| Parts per Million | ppm = (mass solute/mass solution) × 10⁶ |
| Percent by Mass | % = (mass solute/mass solution) × 100 |
| Percent by Volume | % = (vol solute/vol solution) × 100 |
| Colligative Property (Relative Lowering) | ΔP/P° = mole fraction of solute |
| Van't Hoff Factor | i = 1 + α(n−1) |
Acid-Base (13)
| Formula | Expression |
|---|---|
| pH | pH = -log[H⁺] |
| pOH | pOH = -log[OH⁻] |
| pH + pOH | pH + pOH = 14 |
| Henderson-Hasselbalch | pH = pKa + log([A⁻]/[HA]) |
| Ka-Kb Relation | Ka × Kb = Kw |
| Buffer Capacity (concept) | resists pH change on addition of acid/base |
| Percent Ionization | %ionization = [H⁺]/[HA]₀ × 100 |
| Common Ion Effect on Ionization (concept) | a common ion suppresses ionization of a weak acid or base |
| pH of Strong Acid | pH = −log[H+] |
| pOH of Strong Base | pOH = −log[OH−] |
| Kw at 25°C | Kw = [H+][OH−] = 1×10⁻¹⁴ |
| Conjugate Acid-Base Pair (concept) | acid loses a proton to form its conjugate base |
| Amphoteric Species (concept) | a substance that can act as both an acid and a base |
Organic (1)
| Formula | Expression |
|---|---|
| Degree of Unsaturation | DoU = (2C + 2 + N - H)/2 |
Nuclear Chemistry (2)
| Formula | Expression |
|---|---|
| Mass Defect | Δm = Zmₚ + Nmₙ − M |
| Half-life (nuclear) | N = N₀(½)^(t/t½) |
Titration (3)
| Formula | Expression |
|---|---|
| Normality | N = molarity × n-factor |
| Titration Equation | N₁V₁ = N₂V₂ |
| Equivalence Point (concept) | moles of acid equal moles of base at stoichiometric ratio |
Organic Chemistry (33)
| Formula | Expression |
|---|---|
| General Alkane Formula | CₙH₂ₙ₊₂ |
| General Alkene Formula | CₙH₂ₙ |
| General Alkyne Formula | CₙH₂ₙ₋₂ |
| Degree of Unsaturation (alt) | DoU = (2C+2−H)/2 (no N) |
| Empirical Formula (organic) | simplest whole-number mole ratio of elements |
| General Alcohol Formula | CₙH₂ₙ₊₁OH |
| Percentage of Element (Organic) | %C = (mass CO₂ × 12/44 × 100)/sample mass |
| General Cycloalkane Formula | CₙH₂ₙ |
| IUPAC Parent Chain Rule (concept) | longest continuous carbon chain determines the parent name |
| General Formula of Carboxylic Acids | CnH2nO2 |
| General Formula of Aldehydes | CnH2nO |
| General Formula of Ketones | CnH2nO |
| General Formula of Ethers | CnH2n+2O |
| General Formula of Amines | CnH2n+3N |
| General Formula of Esters | CnH2nO2 |
| Homologous Series (concept) | members differ by a -CH2- unit and share similar properties |
| Markovnikov's Rule (simple statement) | H adds to carbon with more H atoms already attached |
| Isomers Count (concept) | compounds with same molecular formula, different structure |
| General Formula of Alkanes | CₙH₂ₙ₊₂ |
| General Formula of Alkenes | CₙH₂ₙ |
| General Formula of Alkynes | CₙH₂ₙ₋₂ |
| Degree of Unsaturation | DoU = (2C + 2 + N − H)/2, C = carbons, N = nitrogens, H = hydrogens |
| Isomers (concept) | compounds with the same molecular formula but different structural arrangements |
| Functional Group (concept) | a specific group of atoms within a molecule responsible for its characteristic chemical reactions |
| Nucleophilic Substitution (SN1/SN2) (concept) | reactions where a nucleophile replaces a leaving group; SN1 is stepwise, SN2 is a single concerted step |
| Electrophilic Addition (concept) | an electrophile adds across a double or triple bond, typical of alkene/alkyne reactions |
| Elimination Reaction (E1/E2) (concept) | a reaction that removes atoms from a molecule to form a double bond, releasing a small byproduct |
| Markovnikov's Rule (concept) | in addition to an unsymmetrical alkene, H adds to the carbon with more hydrogens already attached |
| Esterification Reaction (concept) | Carboxylic Acid + Alcohol ⇌ Ester + Water (catalyzed by acid) |
| Saponification Reaction (concept) | Ester + Strong Base → Soap (carboxylate salt) + Alcohol |
| Aromaticity (Hückel's Rule) | a ring is aromatic if it is planar, cyclic, fully conjugated, and has (4n+2) π electrons |
| Chirality / Optical Isomerism (concept) | a molecule with a carbon bonded to four different groups can exist as non-superimposable mirror images |
| Polymerization (concept) | the process of joining many small monomer molecules together to form a large polymer chain |
Environmental Chemistry (7)
| Formula | Expression |
|---|---|
| Hardness of Water | as CaCO₃ (mg/L) |
| BOD | Biochemical Oxygen Demand (mg/L) |
| Carbon Footprint (concept) | total CO₂-equivalent emissions from an activity |
| Total Dissolved Solids (concept) | sum of all dissolved minerals and salts in water, in mg/L |
| pH Scale of Rainwater (concept) | normal rainwater has pH about 5.6 due to dissolved CO2 |
| COD (Chemical Oxygen Demand) | amount of oxygen required to oxidize organic matter chemically |
| Ozone Depletion Reaction (concept) | Cl radicals catalytically destroy ozone: Cl + O3 → ClO + O2 |
Thermochemistry (10)
| Formula | Expression |
|---|---|
| Enthalpy Change | ΔH = H_products − H_reactants |
| Hess's Law | ΔH_total = ΣΔH_steps |
| Gibbs Free Energy | ΔG = ΔH − TΔS |
| Enthalpy of Reaction | ΔH_rxn = ΔH_products − ΔH_reactants |
| Enthalpy of Formation (concept) | the heat change when 1 mole of a compound forms from its elements in their standard states |
| Enthalpy of Combustion (concept) | the heat released when 1 mole of a substance burns completely in oxygen |
| Bond Enthalpy Calculation | ΔH = Σ(Bond Energies Broken) − Σ(Bond Energies Formed) |
| Calorimetry Heat Formula | q = mcΔT, m = mass, c = specific heat capacity, ΔT = temperature change |
| Exothermic vs Endothermic (concept) | exothermic reactions release heat (ΔH negative); endothermic reactions absorb heat (ΔH positive) |
| Specific Heat Capacity (concept) | the amount of heat needed to raise the temperature of 1 g of a substance by 1°C |
Biochemistry (5)
| Formula | Expression |
|---|---|
| Peptide Bond Formation (concept) | condensation of -COOH and -NH2 groups releasing H2O |
| Glycosidic Bond (concept) | bond linking two monosaccharides formed by dehydration |
| ATP Hydrolysis Energy (concept) | ATP + H2O → ADP + Pi, releases ~30.5 kJ/mol |
| Isoelectric Point (concept) | pH at which a molecule carries no net electric charge |
| Enzyme-Substrate Rate (Michaelis-Menten) | v = Vmax[S]/(Km+[S]) |
Stoichiometry (10)
| Formula | Expression |
|---|---|
| Percent Yield | Percent Yield = (Actual Yield/Theoretical Yield) × 100 |
| Limiting Reagent (concept) | the reactant that is completely consumed first, limiting the amount of product formed |
| Theoretical Yield (concept) | the maximum amount of product that could be formed from the limiting reagent, based on stoichiometry |
| Percent Composition | Percent Composition = (Mass of Element in Compound/Molar Mass of Compound) × 100 |
| Empirical Formula (concept) | the simplest whole-number ratio of atoms of each element in a compound |
| Molecular Formula from Empirical Formula | Molecular Formula = (Empirical Formula)ₙ, n = Molar Mass/Empirical Formula Mass |
| Molar Mass | Molar Mass = Mass of Substance (g)/Number of Moles |
| Number of Moles from Mass | n = Mass (g)/Molar Mass (g/mol) |
| Number of Particles from Moles | N = n × Nₐ, Nₐ = Avogadro's Number (6.022 × 10²³) |
| Molar Volume of a Gas at STP | 1 mole of any gas occupies 22.4 L at STP |
Colligative Properties (8)
| Formula | Expression |
|---|---|
| Relative Lowering of Vapor Pressure | (P° − P)/P° = Mole Fraction of Solute |
| Elevation in Boiling Point | ΔTb = Kb × m, Kb = molal boiling point constant, m = molality |
| Depression in Freezing Point | ΔTf = Kf × m, Kf = molal freezing point constant |
| Osmotic Pressure (Van't Hoff Equation) | π = MRT, M = molarity, R = gas constant, T = temperature (K) |
| Van't Hoff Factor | i = Actual number of particles in solution/Number of formula units initially dissolved |
| Molality | m = Moles of Solute/Mass of Solvent (kg) |
| Mole Fraction | X_A = Moles of A/Total Moles of All Components |
| Isotonic Solutions (concept) | two solutions with equal osmotic pressure, causing no net water movement between them |
More class-wise formulas
Formulas are for revision. Always follow the notation and rounding used in your own textbook and board papers.
FAQ
How many FSc Chemistry formulas are on this page?
172 formulas in 17 chapters.
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