IGCSE Chemistry Last Minute Revision Plan: Your Path to A* in O Level Chemistry 5070 & IGCSE Chemistry 0620
Welcome to the most comprehensive IGCSE Chemistry Last Minute Revision Plan designed specifically for students and teachers of O Level Chemistry 5070, IGCSE Chemistry 0620, CAIE O-Level Chemistry 5070, Cambridge O Level Chemistry 5070, GCE O Level Chemistry 5070, and related syllabi like Edexcel IGCSE Chemistry 4CH1. This igcse chemistry revision plan is exam-centered, concise, and packed with facts to help you ace your exams in 2025-2026. Instead of wasting time on irrelevant YouTube videos that aren't aligned with your syllabus, contain ads, and fail to cover topics fully, opt for structured courses that guarantee results. For example, 95% of students who enrolled in our crash courses scored A or higher, based on internal surveys from 2023-2024.
Why This IGCSE Chemistry Revision Plan Beats Random YouTube Searches
YouTube videos often lack syllabus alignment for IGCSE Chemistry 0620 syllabus or O Level Chemistry 5070 syllabus, bombard you with ads, and don't provide complete topic coverage. Our plan, however, is tailored to Cambridge and Edexcel standards, with 100% syllabus-matched content. Facts show that students using structured revision like our Full Syllabus Crash Course improve grades by 2 levels on average (data from 500+ students in 2024).
Revision Timeline for Last Minute Success
| Day | Focus Topics | Activities |
|---|---|---|
| Day 1-2 | States of Matter, Atomic Structure | Review Structure of Atom O Level Notes, solve 5 past papers from P1 Past Papers Session. |
| Day 3-4 | Stoichiometry, Mole Concept | Practice with Mole Concept Notes, download Moles PDF. |
| Day 5-6 | Organic Chemistry, Bonding | Enroll in Organic Chemistry Crash Course, use Chemical Bonding PDF. |
| Day 7 | Full Mock & Review | Take 20 mocks from P1 Course, analyze with Grade Thresholds 2025. |
Exam-Centered Definitions List (Concise & Useful)
- Atom: Smallest unit of an element; consists of protons, neutrons, electrons. (From Structure of Atom Notes)
- Mole: 6.02 x 10^23 particles; key for calculations in stoichiometry.
- Redox: Oxidation (loss of electrons) and reduction (gain); essential for electrolysis. (Download Redox PDF)
- Organic Chemistry: Carbon-based compounds; alkanes to polymers. Master via crash course.
- All definitions from IGCSE Chemistry Definitions List.
Downloadable Resources for IGCSE Chemistry Revision
- Oxygen and Air PDF
- Chemical Bonding PDF
- Chemical Energetics PDF
- Experimental Techniques PDF
- Formula PDF
- Formulae PDF
- Metals PDF 1
- Metals PDF 2
- Moles PDF
- Organic Chemistry PDF
- Reactions PDF
- Redox PDF
- States of Matter PDF 1
- The Periodic Table PDF
- States of Matter PDF 2
- Atoms, Elements and Compounds PDF
- Organic Chem PDF
- Acids, Bases and Salts PDF
- Electrolysis PDF
- Hydrogen and Water PDF
These are aligned with O Level Chemistry Formula Sheet PDF and Ultimate Pack Notes.
Demo Videos & Embedded Content
Watch this demo: Chemistry Crash Course 10% Off Now Cover Complete Syllabus of O Level Chemistry & IGCSE Chemistry
IGCSE 0620_m22_qp_62 SOLVED by Prof. Faisal Janjowa
O Level Chemistry 5070_s23_qp_42 Solved by Professor Faisal Janjowa
Chemistry Cheat Sheet for Cations and Anions Test Gas and Ion Identification
Learn Periodic Table by O/A-Level, IGCSE, AQA, Edexcel Hack Periodic Table Learn Groups 1-8 in one Song
Mood Booster Songs for Revision Breaks
Teacher Profile: Professor Faisal Janjowa (The Chemistry Guru)
Prof. Faisal Janjowa has 15+ years teaching CAIE, Edexcel, and AQA Chemistry. He has helped 10,000+ students achieve A* grades. Specializes in Paper 4 ATP Guides.
Live Class Details
Weekly live sessions in our Full Syllabus Crash Course: Sundays 8 PM PKT, covering topics like Empirical Formulas.
Testimonials & Reviews
"This IGCSE Chemistry Revision Plan saved my exams! Enrolled in the Full Crash Course and scored A*." - Ahmed, Student, Pakistan (5/5)
"Better than YouTube – no ads, full syllabus coverage. Highly recommend!" - Sara, Teacher, UAE (4.8/5)
"Past papers session boosted my confidence. 90% improvement in mocks." - Ali, Student, UK (5/5)
Relaxation Tips with Google Trends Integration
During breaks in your igcse chemistry revision plan, relax with trends like watching pakistan national cricket team vs united states national cricket team match scorecard or uae vs new zealand cricket highlights on Star Sports. Follow players like Babar Azam, Saurabh Netravalkar, Haider Ali, Ehsan Adil, Harmeet Singh, Monank Patel, Faheem Ashraf, Sahibzada Farhan. Check namibia vs netherlands, south africa national cricket team vs canada national cricket team standings, pakistan women vs south africa women, pakistan vs usa, pak vs usa, man united, man united vs west ham. Non-sports: solar net metering, whatsapp web video calls, lahore 1947, ebo taylor, ottis gibson, my co, gta6, ali dar, jana nayagan movie, sanae takaichi japan election, جوهر نبيل, dubai weather fog, hind alowais, تراكتور ضد السد, ترند السبعينات, درب, يوم التأسيس السعودي, اليونايتد, كريستيانو رونالدو, اسيا ٢, التعديل الوزاري الجديد, فياريال ضد إسبانيول, علي لاريجاني, كأس الاتحاد الآسيوي, lutnick, rachel zoe, tony yayo, michelle randolph, rivian r2, ben ogden, dancing with the stars, alex hall, tps nepal honduras nicaragua, casey wasserman, isaiah stewart, jeff johnson, sultan ahmed bin sulayem, grizzlies vs warriors, thunder vs lakers, mcnugget caviar.com, arizona vs kansas, cavaliers vs nuggets, gordie howe bridge, les wexner, noah kahan presale, tibia bone, eishockey olympia 2026 frauen, rügen, ribery, wetter karneval, lena kesting, groenlo, justin engel, donald trump halftime show, natalie geisenberger, katrin müller-hohenstein, philipp nawrath, sturla holm lægreid, jan-lennard struff, starlink ukraine russland, hertha freiburg, philipp horn, meningokokken, biathlon olympia, karin prien, birk ruud, olympia aktuell, xbox game pass, schrozberg, sports, six, pakistan match.
Enroll Now: Logical Reasons with Facts
Don't waste time – enroll in our courses: 8-hour Full Syllabus Crash Course covers everything (90% student satisfaction). Or master Organic Chemistry Crash Course (covers 30% of syllabus efficiently). Practice with P1 Past Papers (20 Mocks).
Enroll in Organic Chemistry Crash Course Enroll in P1 Past Papers Session Enroll in Full Syllabus Crash CourseFAQs for IGCSE Chemistry Last Minute Revision Plan
- How to revise for IGCSE Chemistry effectively?
- Use our Last Minute Revision Notes and crash courses.
- What is the best IGCSE Chemistry Revision Guide?
- Our IGCSE Chemistry 0620 Guide with past papers.
- Are Save My Exams Notes free?
- Download free from Save My Exams Notes IGCSE Chemistry.
- How to calculate moles simply?
- Follow this guide.
- What are grade thresholds for 2025?
- Check Grade Thresholds 2025.
Internal Links: Mole Concept, Atom Structure, Atom Notes 2025, Definitions List 1, Definitions List 2, Definitions 2025, Definitions Guide, Syllabus 2025, Formula Sheet 2025, Free Formula Sheet, Physics Formula (Related), Formula 2026, 0620 Guide, Physics SME Notes, Ultimate Pack, IGCSE Physics SME, SME Chemistry 0620, SME O Level 5070, SME 2026 O Level, SME 2026 IGCSE, SME 2026 Onwards, SME 2026 Download, SME 2025, 0620 Syllabus 2026, Latest Syllabus 2026, 5070 Syllabus 2025, 0620 Complete Guide, Topic List 2025, 5070 Breakdown PDF, Thresholds Predictions, Thresholds June Nov, Thresholds 2025, ATP Guide Solved, ATP Guide, Last Minute Notes, Notes All Chapters 2025, Notes 2026, Free Download 2025, Free Download 2026, Complete Guide 2025, Empirical Formulas, Computer Science Tips (Related), O Level Equivalence, Paper 2 Prep, Study Tips, Purity Measurement, Master Syllabus, Reactivity, IBCC Equivalence, Predict Products, Equivalence Certificate, Moles Calculation.
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![Fundamental Concepts & States of Matter • Atom: The smallest particle of an element that can exist, made of a nucleus (protons and neutrons) and electrons orbiting it. • Element: A pure substance consisting of only one type of atom, which cannot be broken down into simpler substances by chemical means. • Compound: A substance formed when two or more different elements are chemically bonded together in a fixed ratio. • Mixture: A substance containing two or more elements or compounds not chemically bonded together. Can be separated by physical means. • Molecule: A group of two or more atoms held together by chemical bonds. • Proton: A subatomic particle found in the nucleus with a relative mass of 1 and a charge of +1. • Neutron: A subatomic particle found in the nucleus with a relative mass of 1 and no charge (0). • Electron: A subatomic particle orbiting the nucleus with a negligible relative mass and a charge of -1. • Atomic Number (Z): The number of protons in the nucleus of an atom. Defines the element. • Mass Number (A): The total number of protons and neutrons in the nucleus of an atom. • Isotopes: Atoms of the same element (same atomic number) but with different mass numbers due to a different number of neutrons. • Relative Atomic Mass ($A_r$): The weighted average mass of an atom of an element compared to $1/12$th the mass of a carbon-12 atom. • Relative Molecular Mass ($M_r$): The sum of the relative atomic masses of all atoms in one molecule of a compound. • Relative Formula Mass ($M_r$): The sum of the relative atomic masses of all atoms in the formula unit of an ionic compound. • Mole: The amount of substance that contains $6.02 \times 10^{23}$ particles (Avogadro's number). • Molar Mass: The mass of one mole of a substance, expressed in g/mol. Numerically equal to $A_r$ or $M_r$. • Empirical Formula: The simplest whole number ratio of atoms of each element in a compound. • Molecular Formula: The actual number of atoms of each element in a molecule. • Solid: Particles are closely packed in a fixed, regular arrangement, vibrate about fixed positions. Definite shape and volume. • Liquid: Particles are closely packed but randomly arranged, can slide past each other. Definite volume, no definite shape. • Gas: Particles are far apart and arranged randomly, move rapidly and randomly. No definite shape or volume. • Melting Point: The specific temperature at which a solid changes into a liquid at a given pressure. • Boiling Point: The specific temperature at which a liquid changes into a gas (vaporizes) at a given pressure. • Sublimation: The direct change of state from solid to gas without passing through the liquid phase (e.g., solid $\text{CO}_2$). • Diffusion: The net movement of particles from a region of higher concentration to a region of lower concentration, due to random motion. • Osmosis: The net movement of water molecules across a partially permeable membrane from a region of higher water potential to a region of lower water potential. 2. Structure & Bonding • Ionic Bond: The electrostatic force of attraction between oppositely charged ions, formed by the transfer of electrons from a metal to a non-metal. • Covalent Bond: A strong electrostatic force of attraction between a shared pair of electrons and the nuclei of the bonded atoms, typically between two non-metals. • Metallic Bond: The electrostatic force of attraction between positive metal ions and delocalised electrons. • Ion: An atom or group of atoms that has gained or lost electrons, resulting in a net electrical charge. • Cation: A positively charged ion (lost electrons). • Anion: A negatively charged ion (gained electrons). • Octet Rule: Atoms tend to gain, lose, or share electrons in order to achieve a full outer electron shell, typically with eight electrons. • Giant Ionic Lattice: A regular, repeating 3D arrangement of oppositely charged ions, held together by strong electrostatic forces. • Simple Molecular Structure: Molecules held together by strong covalent bonds, but with weak intermolecular forces between molecules. • Giant Covalent Structure (Macromolecular): A large structure where all atoms are held together by strong covalent bonds in a continuous network (e.g., diamond, silicon dioxide). • Allotropes: Different structural forms of the same element in the same physical state (e.g., diamond and graphite are allotropes of carbon). • Electronegativity: The power of an atom to attract the electron pair in a covalent bond to itself. • Polar Covalent Bond: A covalent bond in which electrons are shared unequally due to a difference in electronegativity between the bonded atoms. • Hydrogen Bond: A strong type of intermolecular force that occurs between molecules containing hydrogen bonded to a highly electronegative atom (N, O, F). • Van der Waals' forces: Weak intermolecular forces of attraction between all molecules, arising from temporary dipoles. 3. Stoichiometry & Chemical Calculations • Stoichiometry: The study of quantitative relationships between reactants and products in chemical reactions. • Limiting Reactant: The reactant that is completely consumed in a chemical reaction, determining the maximum amount of product that can be formed. • Excess Reactant: The reactant present in a greater amount than required to react with the limiting reactant. • Yield: The amount of product obtained from a chemical reaction. • Theoretical Yield: The maximum amount of product that can be formed from a given amount of reactants, calculated using stoichiometry. • Actual Yield: The amount of product actually obtained from a chemical reaction, usually less than the theoretical yield. • Percentage Yield: $($Actual Yield $/$ Theoretical Yield$) \times 100\%$. • Concentration: The amount of solute dissolved in a given volume of solvent or solution. Often expressed in mol/dm$^3$ (molarity) or g/dm$^3$. • Solute: The substance that dissolves in a solvent to form a solution. • Solvent: The substance in which a solute dissolves to form a solution. • Solution: A homogeneous mixture formed when a solute dissolves in a solvent. 4. Chemical Reactions & Energetics • Chemical Reaction: A process that involves rearrangement of the atomic structure of substances, resulting in the formation of new substances. • Reactants: The starting substances in a chemical reaction. • Products: The substances formed as a result of a chemical reaction. • Word Equation: An equation that uses the names of the reactants and products. • Symbol Equation: An equation that uses chemical symbols and formulae to represent reactants and products, and is balanced. • Balancing Equation: Ensuring the number of atoms of each element is the same on both sides of a chemical equation. • Redox Reaction: A reaction involving both reduction and oxidation. • Oxidation: Loss of electrons, gain of oxygen, or loss of hydrogen. Increase in oxidation state. • Reduction: Gain of electrons, loss of oxygen, or gain of hydrogen. Decrease in oxidation state. • Oxidising Agent: A substance that causes oxidation by accepting electrons (and is itself reduced). • Reducing Agent: A substance that causes reduction by donating electrons (and is itself oxidised). • Exothermic Reaction: A reaction that releases energy to the surroundings, usually as heat, causing the temperature of the surroundings to rise. $\Delta H$ is negative. • Endothermic Reaction: A reaction that absorbs energy from the surroundings, usually as heat, causing the temperature of the surroundings to fall. $\Delta H$ is positive. • Activation Energy ($E_a$): The minimum amount of energy required for reactants to collide effectively and initiate a chemical reaction. • Catalyst: A substance that increases the rate of a chemical reaction without being chemically changed itself, by providing an alternative reaction pathway with a lower activation energy. • Enthalpy Change ($\Delta H$): The heat energy change measured at constant pressure for a reaction. • Standard Enthalpy of Formation ($\Delta H_f^\circ$): The enthalpy change when one mole of a compound is formed from its constituent elements in their standard states under standard conditions. • Standard Enthalpy of Combustion ($\Delta H_c^\circ$): The enthalpy change when one mole of a substance is completely combusted in oxygen under standard conditions. • Hess's Law: The total enthalpy change for a reaction is independent of the route taken, provided the initial and final conditions are the same. 5. Rates of Reaction & Equilibrium • Rate of Reaction: The change in concentration of a reactant or product per unit time. • Collision Theory: For a reaction to occur, reactant particles must collide with sufficient energy (activation energy) and correct orientation. • Factors Affecting Rate: Concentration, pressure (for gases), surface area, temperature, and presence of a catalyst. • Reversible Reaction: A reaction where products can react to reform the original reactants, indicated by $\rightleftharpoons$. • Chemical Equilibrium: A state in a reversible reaction where the rate of the forward reaction is equal to the rate of the reverse reaction, and the concentrations of reactants and products remain constant. • Le Chatelier's Principle: If a change in conditions (temperature, pressure, concentration) is applied to a system at equilibrium, the system will shift in a direction that counteracts the change. 6. Acids, Bases & Salts • Acid: A substance that produces hydrogen ions ($H^+$) when dissolved in water (Arrhenius definition) or a proton donor (Brønsted-Lowry definition). • Base: A substance that produces hydroxide ions ($OH^-$) when dissolved in water (Arrhenius definition) or a proton acceptor (Brønsted-Lowry definition). • Alkali: A soluble base that dissolves in water to produce hydroxide ions ($OH^-$). • Salt: A compound formed when the hydrogen ion of an acid is replaced by a metal ion or an ammonium ion. • Neutralisation: The reaction between an acid and a base (or alkali) to form a salt and water. $H^+(aq) + OH^-(aq) \rightarrow H_2O(l)$. • pH: A measure of the acidity or alkalinity of a solution, defined as $-\log_{10}[H^+]$. Scale from 0 to 14. • Strong Acid: An acid that fully dissociates (ionizes) in water (e.g., HCl, $H_2SO_4$). • Weak Acid: An acid that partially dissociates (ionizes) in water (e.g., $CH_3COOH$). • Strong Base: A base that fully dissociates in water (e.g., NaOH, KOH). • Weak Base: A base that partially dissociates in water (e.g., $NH_3$). • Amphoteric: A substance that can act as both an acid and a base (e.g., aluminium oxide, water). • Titration: A quantitative chemical analysis method used to determine the unknown concentration of a reactant using a known concentration of another reactant. • Indicator: A substance that changes colour over a specific pH range, used to detect the endpoint of a titration. 7. Electrochemistry • Electrolysis: The decomposition of an ionic compound using electrical energy. Requires molten or aqueous electrolyte. • Electrolyte: An ionic compound (molten or dissolved in a solvent) that conducts electricity due to the movement of ions. • Electrodes: Conductors (usually metal or graphite) through which electricity enters and leaves the electrolyte. • Anode: The positive electrode, where oxidation occurs (anions are attracted). • Cathode: The negative electrode, where reduction occurs (cations are attracted). • Faraday's Laws of Electrolysis: Relate the amount of substance produced at an electrode to the quantity of electricity passed through the electrolyte. • Galvanic (Voltaic) Cell: An electrochemical cell that generates electrical energy from spontaneous redox reactions. • Standard Electrode Potential ($E^\circ$): The potential difference of a half-cell compared to a standard hydrogen electrode under standard conditions (1 M concentration, 1 atm pressure for gases, 298 K). • Electrochemical Series: A list of elements arranged in order of their standard electrode potentials, indicating their relative reactivity as oxidising or reducing agents. 8. The Periodic Table • Periodic Table: An arrangement of elements in order of increasing atomic number, showing periodic trends in properties. • Group: A vertical column in the periodic table, containing elements with the same number of valence electrons and similar chemical properties. • Period: A horizontal row in the periodic table, containing elements with the same number of electron shells. • Valence Electrons: Electrons in the outermost shell of an atom, involved in chemical bonding. • Alkali Metals (Group 1): Highly reactive metals, readily lose one electron to form $+1$ ions. React vigorously with water. • Alkaline Earth Metals (Group 2): Reactive metals, readily lose two electrons to form $+2$ ions. • Halogens (Group 17/7): Highly reactive non-metals, readily gain one electron to form $-1$ ions. Exist as diatomic molecules. • Noble Gases (Group 18/0): Unreactive elements with a full outer electron shell, existing as monatomic gases. • Transition Metals: Elements in the d-block of the periodic table, characterised by variable oxidation states, coloured compounds, and catalytic activity. • Metallic Character: Tendency of an element to lose electrons and form positive ions. Increases down a group, decreases across a period. • Non-metallic Character: Tendency of an element to gain electrons and form negative ions. Decreases down a group, increases across a period. • Ionisation Energy: The energy required to remove one electron from each atom in one mole of gaseous atoms to form one mole of gaseous $1+$ ions. • Electron Affinity: The energy change when one mole of electrons is added to one mole of gaseous atoms to form one mole of gaseous $1-$ ions. 9. Organic Chemistry • Organic Chemistry: The study of carbon compounds, excluding carbonates, carbides, and oxides of carbon. • Hydrocarbon: A compound containing only carbon and hydrogen atoms. • Saturated Hydrocarbon: A hydrocarbon containing only single carbon-carbon bonds (e.g., alkanes). • Unsaturated Hydrocarbon: A hydrocarbon containing one or more carbon-carbon double or triple bonds (e.g., alkenes, alkynes). • Homologous Series: A series of organic compounds with the same general formula, similar chemical properties, and showing a gradual change in physical properties. • Functional Group: A specific group of atoms within a molecule that is responsible for the characteristic chemical reactions of that molecule. • Alkane: Saturated hydrocarbons with the general formula $C_nH_{2n+2}$. Contain only single bonds. • Alkene: Unsaturated hydrocarbons with the general formula $C_nH_{2n}$. Contain at least one carbon-carbon double bond. • Alkyne: Unsaturated hydrocarbons with the general formula $C_nH_{2n-2}$. Contain at least one carbon-carbon triple bond. • Alcohol: Organic compounds containing the hydroxyl functional group ($-OH$). General formula $C_nH_{2n+1}OH$. • Carboxylic Acid: Organic compounds containing the carboxyl functional group ($-COOH$). • Ester: Organic compounds formed from the reaction of a carboxylic acid and an alcohol, containing the ester linkage ($-COO-$). • Isomers: Compounds with the same molecular formula but different structural formulae. • Structural Isomers: Isomers that differ in the arrangement of their atoms or bonds. • Addition Reaction: A reaction where an unsaturated molecule adds across a double or triple bond, forming a single product. • Substitution Reaction: A reaction where an atom or group of atoms in a molecule is replaced by another atom or group of atoms. • Polymerisation: The process of joining many small monomer molecules together to form a large polymer molecule. • Monomer: A small molecule that can be joined together to form a polymer. • Polymer: A large molecule (macromolecule) formed from many repeating monomer units. • Addition Polymerisation: Polymerisation where monomers add to one another in such a way that the polymer contains all the atoms of the monomer. Usually involves unsaturated monomers. • Condensation Polymerisation: Polymerisation where monomers join together with the elimination of a small molecule (e.g., water). • Cracking: The process of breaking down long-chain hydrocarbons into shorter, more useful hydrocarbons using heat and/or a catalyst. • Fermentation: The anaerobic respiration of yeast, converting glucose into ethanol and carbon dioxide. 10. Analytical Chemistry • Qualitative Analysis: The identification of the components of a sample. • Quantitative Analysis: The determination of the amount or concentration of a component in a sample. • Chromatography: A separation technique based on differential partitioning between a stationary phase and a mobile phase. • Retention Factor ($R_f$): In paper/thin-layer chromatography, the ratio of the distance travelled by the spot to the distance travelled by the solvent front. • Spectroscopy: The study of the interaction of electromagnetic radiation with matter. • Infrared (IR) Spectroscopy: Used to identify functional groups in organic molecules based on their absorption of IR radiation. • Mass Spectrometry: Used to determine the relative molecular mass of a compound and its fragmentation pattern to deduce structure. • Flame Test: A qualitative test for the presence of certain metal ions, which produce characteristic colours when heated in a flame.](https://cambridgeclassroom.com/wp-content/uploads/2024/03/White-And-Purple-Modern-Online-Graphic-Design-Courses-Instagram-Post-4.png)