Chemistry AS Cambridge

Examine van der Waals (London) forces from instantaneous and induced dipoles, and how permanent dipole interactions and hydrogen bonding govern boiling points through molecular size, shape, and lone pairs.

Explore how electron repulsion shapes molecular geometry using lone and bond pairs, learn common shapes and bond angles, and examine dipoles, polarity, and hydrogen bonding.

Explore enthalpy changes in reactions, distinguish endothermic and exothermic processes, and apply Hess's law to calculate delta H from products and reactants using standard enthalpy changes.

Explore activation energy and Boltzmann distribution concepts, and apply Hess's law to standard enthalpy of formation and combustion for key reactions like methanol and carbon dioxide.

Learn to calculate enthalpy changes using formation data and bond energies from the data booklet, including the exothermic formation of CH3Cl from CH4 and Cl2 and reaction pathways with intermediates.

Explore standard enthalpy changes and formation enthalpies using Hess's law and Hess triangle to calculate enthalpy of reaction for methanol, water, ammonia, and CS2.

Explore enthalpy changes and Hess's triangle through practical calculations of formation enthalpies, bond energies, and redox examples, including sodium and aluminium oxide reactions.

Explore enthalpy changes by applying Q=mcΔT to calculate the enthalpy of combustion of ethanol in kilojoules per mole, using water's 4.2 J kg-1 K-1 and mole calculations.

Explore enthalpy changes in chemical reactions, including endothermic and exothermic processes, standard enthalpy changes of formation, solution, atomization, and hydration, and apply Hess's law via alternative routes.

Explore redox reactions, define oxidation and reduction, and learn to balance half-reactions and overall equations through practical examples and oxidation-number rules.

Reversible reactions in a closed system reach equilibrium as forward and backward rates balance, while Le Chatelier's principle explains how concentration, pressure, and temperature shifts affect KC, with units varying.

learn to construct the equilibrium constant of concentration using products over reactants, derive its formula, calculate Kc from initial and equilibrium concentrations, and examine stoichiometry and temperature effects.

Calculate KP for gas equilibria using partial pressures in a closed system, with N2 + 3 H2 ⇌ 2 NH3, and learn how each gas shapes the equilibrium.

Master equilibria through Brønsted-Lowry acid-base concepts, reversible reactions, and equilibrium constants Kc and Kp, with worked examples on sulfuric and nitric acids, nitrogen–hydrogen–ammonia systems, and gas-phase shifts.

Explore chemical equilibrium and reversible reactions, dynamic equilibrium, Le Chatelier's principle, and how pressure, temperature, and catalysts shift equilibria, plus KC and KP calculations.

Explains how to calculate kc and kp from equilibrium concentrations and partial pressures, using Haber and contact processes, acid base equilibria, and practice with dynamic equilibrium and unit analysis.

Review bronsted-lowry acids and bases, conjugate pairs, amphoteric water, and strong vs weak acids and bases, with applications to titration curves and Haber process and contact process.

Discover organic chemistry fundamentals by exploring hydrocarbons, saturated and unsaturated bonds, including sigma and pi bonds. Master naming, functional groups, and common formula types with practical examples.

Introduce the basics of organic chemistry, naming rules, and isomerism. Cover structural isomerism (chain, position, functional) and stereoisomerism (geometric cis/trans and optical enantiomers) with chiral centers.

Explore how pentanol's four primary alcohol structural isomers are analyzed to identify which contain chiral carbons, using the elimination of functional, chain, branched, and positional isomer possibilities.

Learn to complete skeletal structures, identify chiral carbons on rings, rule out nonchiral centers, and analyze isomerism, including cis/trans and optical isomers, with examples from halogenated alkanes.

Explore alkane structure, properties and sources from crude oil, fractional distillation, cracking, reforming, and pollution controls; then examine alkenes and their electrophilic addition reactions and tests for double bonds.

Explore carbonyl compounds, including aldehydes and ketones, their naming, oxidation of primary alcohols, reduction to alcohols, diagnostic tests like Tollens, Fehling, dinitrophenylhydrazine, and infrared spectroscopy.

Explore alcohols: structure with the hydroxyl group, primary–secondary–tertiary classification, core reactions such as combustion, halogenation, esterification, dehydration, oxidation, and carbon neutral ethanol as a biofuel.

Identify organic compounds using infrared spectroscopy with a spectrophotometer, interpreting absorption bands and functional groups from a data booklet and corroborate findings with mass spectrometry and NMR.

Explore mass spectrometry fundamentals, including ionization, molecular ion (M+), and fragmentation patterns; use M+1, M+2 peaks and halogen isotopes to identify organic compounds and determine carbon content.

Explain the mechanism of hydrogen bromide adding to propane to form the major product 2-bromopropane via a secondary carbocation, including heterolytic fission and electrophilic addition, plus mass spectrometry basics.

Explore stereoisomerism, including optical isomerism and geometric considerations, and predict oxidation and reduction products of aldehydes and ketones; analyze alkene reactions, reagents, and mass spectrometry in organic chemistry.

Explore organic chemistry basics from hydrocarbons in naphtha to cracking and subsequent oxidation, addition, and polymerization reactions, including tests for carboxylic acids, bromine water, and the fate of pollutants.

This lecture derives the empirical formula of a hydrocarbon from combustion data using mole ratios and reviews core organic topics like dipole moments, alkenes, and structural isomers.

Explore periodicity on the periodic table, including atomic and ionic radii, ionization energy, and how melting points and conductivity relate to nuclear charge, shielding, and bonding.

Explore how ionization energy trends across a period rise, with dips at group 2–3 and group 5–6 explained by orbital energy levels, shielding, and electron configurations.

This lecture explains trends in group two, the alkaline earth metals, including radius and reactivity, and outlines their reactions with water, oxygen, acids, and carbonates.

Explore trends in group seven halogens, including physical properties, van der Waals forces, decreasing electronegativity, and reactivity with metals and non-metals, color changes in displacement reactions.

Explores trends in group 7 reactivity and displacement, and identifying halogens via cyclohexane extraction. Covers halide ion tests with silver nitrate and sulfuric acid reactions.

Explore nitrogen and sulfur chemistry, including nitrogen's nonreactive N2, nitrogen oxides, ammonia synthesis via the Haber process, and the environmental impact of acid rain and fertilizers.

Tackle inorganic chemistry questions on reducing agents, oxide and hydroxide reactions with water, amphoteric aluminum oxide, acid-base and redox reactions, and qualitative halide tests, with balanced equations and explanations.

Explores ionization energy and group placement, isoelectronic reasoning, and electron configurations while analyzing melting point trends, hydrolysis versus dissolution, and coordinate bonding in key inorganic systems.

Examine chlorine's role as an oxidizing agent in water purification, and analyze period three first ionization energy trends and halide reactions in this inorganic chemistry lesson.

Identify unknown inorganic samples through solubility and pH tests, classify barium hydroxide, sodium chloride, phosphorus oxide, and silicon tetrachloride, and explore related oxide properties and bonding.

Analyze how rate of reaction depends on concentration, temperature, pressure, and catalysts, using collision theory and Boltzmann distribution to explain activation energy and collision frequency.

Delve into rate of reaction concepts, concentration versus rate, collision theory, and activation energy, applying these ideas to real chemistry questions and related thermodynamics and gas law problems.