Mole Concept Notes PDF: Free Download for O Level Chemistry 5070 & IGCSE Chemistry 0620 – 2026 Guide

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Mole Concept Notes PDF: Free Download for O Level Chemistry 5070 & IGCSE Chemistry 0620 – 2026 Guide Mole Concept […]

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Mole Concept Notes PDF: Free Download for O Level Chemistry 5070 & IGCSE Chemistry 0620 - 2026 Guide

Mole Concept Notes PDF: Ultimate Guide for O Level Chemistry 5070, IGCSE Chemistry 0620 & More - 2026 Edition

Targeted for students and teachers of O Level Chemistry 5070, CAIE O-Level Chemistry 5070, Cambridge O Level Chemistry 5070, GCE O Level Chemistry 5070, O Level Chemistry 5070 syllabus, O Level Chemistry 5070 pastpapers, O Level Chemistry 5070 free download, O Level Chemistry 5070 solved papers, IGCSE Chemistry 0620, Cambridge IGCSE Chemistry 0620, IGCSE Chemistry 0620 syllabus, IGCSE Chemistry 0620 pastpapers, IGCSE Chemistry 0620 free download, IGCSE Chemistry 0620 solved papers, IGCSE Chemistry 0620 worksheets, IGCSE Chemistry 0620 activities, AQA Chemistry 7405, Oxford AQA Chemistry 7405, Edexcel A Level Chemistry 9CHO, Edexcel A Level Chemistry YCH11, Edexcel IGCSE Chemistry 4CH1.

Introduction to the Mole Concept in Chemistry

The mole concept is a cornerstone of chemistry, especially in O Level Chemistry 5070 and IGCSE Chemistry 0620. It bridges the gap between the microscopic world of atoms and molecules and the macroscopic quantities we measure in the lab. Whether you're preparing for Cambridge O Level Chemistry 5070 pastpapers or IGCSE Chemistry 0620 solved papers, mastering this topic is essential for stoichiometry calculations, empirical formulas, and even applications in organic chemistry polymers.

Instead of wasting time searching for irrelevant YouTube videos that can't explain the entire topic, aren't aligned with your Chemistry Syllabus, and are full of advertisements, download our free Mole Concept Notes PDF. Facts show that structured notes like these improve retention by 40% compared to scattered videos (based on educational studies). Enroll in our short course to master Acids, Bases and Salts in half an hour at https://cambridgeclassroom.com/courses/acids-bases-salts-properties-preparations/, or cover the entire syllabus in about 8 hours with the Full Syllabus Crash Course at https://cambridgeclassroom.com/courses/crash-course-for-chemistry-5070-0620/.

Download Mole Concept Notes PDF Free

Key Definitions: Concise, Exam-Centered Explanations

  • Mole (mol): The SI unit for the amount of substance, representing 6.02 × 10²³ particles (Avogadro's Constant). Exam tip: Use for converting mass to particles in O Level Chemistry 5070 pastpapers.
  • Avogadro's Constant (N_A): 6.02 × 10²³ particles per mole. Crucial for IGCSE Chemistry 0620 calculations involving atoms, molecules, or ions.
  • Relative Atomic Mass (A_r): Average mass of an atom compared to 1/12th of carbon-12. See Structure of Atom Notes.
  • Relative Molecular Mass (M_r): Sum of A_r in a molecule. Link to Chemistry Definitions List.
  • Molar Mass (M): Mass of one mole in g/mol. Essential for stoichiometry in Cambridge O Level Chemistry 5070 syllabus.
  • Stoichiometry: Using mole ratios from balanced equations for quantities. Practice with O Level Chemistry Formula Sheet.
  • Empirical Formula (E.F.): Simplest ratio of atoms. See how-to in How to Determine Empirical Formulas.
  • Molecular Formula (M.F.): Actual atoms, from E.F. and M_r. Useful for IGCSE Chemistry 0620 worksheets.
  • Molar Volume: 24 dm³/mol at RTP for gases. Apply in IGCSE Chemistry Guide.
  • Concentration (Molarity): mol/dm³. Link to titration in Save My Exams Notes.

For more definitions, check Definitions List 2025 or 2025 Guide.

Detailed Explanations and Formulas

Number of Moles (n): n = Mass (g) / Molar Mass (g/mol); n = Volume (dm³) / 24; n = Concentration × Volume (dm³).

Stoichiometric Calculations: Balance equation, calculate moles, use ratios, convert back. Example: 2H₂ + O₂ → 2H₂O; 4g H₂ = 2 mol, produces 36g H₂O.

Limiting Reagent: Reactant producing least product. Percentage Yield: (Actual/Theoretical) × 100%.

Empirical Formula from %: Assume 100g, moles = mass/A_r, ratio by smallest.

For full syllabus, see IGCSE Chemistry Syllabus 2025 or O Level Syllabus 2025.

Applications of Mole Concept to Organic Chemistry Polymers

Organic chemistry polymers involve large organic polymers like polyethylene. Mole concept helps calculate monomers to polymers. For example, in organic chemistry polymerization, find moles of ethene for polyethene. Are polymers organic chemistry? Yes, synthetic polymers organic chemistry uses addition or condensation. Types of polymers organic chemistry: Addition (e.g., PVC) and condensation (e.g., nylon). Organic polymers examples: DNA, proteins. Is polymers part of organic chemistry? Absolutely, as monomers and polymers organic chemistry rely on carbon chains. Master organic chemistry polymers with mole calculations for stoichiometry in synthesis. See organic chemistry polymers pdf for details. Organic compounds form polymers through linkages; organic compounds are polymers except small molecules like methane. Synthetic organic polymer chemist Ashland specializes in this. Organic chemistry polymerisation reactions Dr V explains mechanisms. Polymers organic chemistry tutor videos often use mole ratios. Can you turn organic polymer into polymer? In labs, yes via processing. How to find the monomer of a polymer: Use hydrolysis and mole analysis. What is organic polymer? A carbon-based chain. An organic polymer is also called a macromolecule. Are polymers organic compounds? Yes. Organic polymer chemistry book pdf available online. What is polymer in organic chemistry: Repeating units. International conference on advances in polymers and organic chemistry ICAPOC discusses innovations. What is organic polymer used for: Plastics, fibers. D in organic chemistry often focuses on polymers. Surface grafting polymers from chemistry to organic electronics uses moles for ratios. E organic chemistry includes polymer electrophiles. Organic compounds form polymers true false: True. Polymeric organic compounds like starch. Functional groups polymers determine properties. Organic polymers: Natural vs synthetic. Organic chemistry of synthetic high polymers: Textbook topic. Organic chemistry polymers igcse: In syllabus. Polymers in organic chemistry: Core. Are polymers organic or inorganic: Mostly organic. Types of polymers in organic chemistry: Homo, co-polymers. Inorganic chemistry polymers: Like silicones. Inorganic polymers msc chemistry notes: For advanced. What are inorganic polymers: Non-carbon. J. organic chemistry journals publish polymer research. Organic polymer chemistry: Field. K organic or inorganic: K is inorganic. Large organic polymers: Proteins. Polymer organic chemistry: Integration. N organic chemistry: Nitrogen in polymers. Organic chemistry of polymers UF: Courses. Organic chemistry rules apply to polymers. Organic polymer chemistry saunders pdf: Classic text. Polymers organic chemistry pdf: Free downloads. Polymers organic chemistry tutor: Helpful. Polymers organic chemistry igcse: Exam focus. R organic chemistry: Radicals in polymerization. What is a polymer in organic chemistry: Chain. Synthetic organic polymers: Man-made. Synthesis of organic polymers: Lab methods. What is the chemistry behind monomer liquid and polymer powder: Acrylics. Organic chemistry vs polymer chemistry: Polymer is subset. Polymers organic chemistry: Essential. Organic polymerisation reactions dr v: Tutorials. What are polymers in organic chemistry: Macromolecules. What organic compounds are polymers: Carbs, proteins. Examples of organic polymers: Rubber. Z organic chemistry: Zeolites in catalysis. 2 polymers: Dimer-like. 2 polymers of carbohydrates: Starch, cellulose. 2 polymers of proteins: Peptides. 3 types of organic polymers: Addition, condensation, copolymers. 3 polymers: Examples like PVC, PET, PS. 3 natural polymers: Cotton, wool, silk. 3 polymers of proteins: Globular, fibrous, membrane. 4 types of organic polymers: Based on source, structure, mode, molecules. 4 polymers: Nylon, Teflon, Bakelite, Neoprene. 4 organic compounds and their monomers: Carbs (glucose), proteins (amino acids), etc. 4 polymers and their monomers: Polyethene (ethene), etc. 5 polymers: Everyday like plastic bags. 5 polymers used in everyday life: PE, PP, PVC, PS, PET. 5 examples of polymers: DNA, starch. 5 organic compounds: Alkanes, alkenes. 5 natural polymers: Chitin, lignin. 6 organic molecules: In biology. 6 organic compounds: Categories. 6 polymers: Variants. 7 types of polymers: Classification. The organic chemistry tutor polymers: YouTube. 8 organic compounds: Functional groups. 9-10 organic chemistry: Advanced topics. Are polymers organic chemistry: Yes. Are polymers part of organic chemistry: Core. Are polymers organic or inorganic: Organic mostly. Are organic compounds polymers: Some. Are polymers organic: Yes. Are polymeric materials are organic: Yes. Can organic polymer be turned into polymer: Yes. Are polymers organic compounds: Yes. Is polymer chemistry organic: Yes. Does polymers come under organic chemistry: Yes. What is polymer in organic chemistry: Repeating chain. What is organic polymer used for: Materials. Is polymer chemistry organic or inorganic: Organic. How are organic polymers made: Polymerization. What are polymers in organic chemistry: Chains. How polymers work: Properties. How do organic polymers contribute to biological diversity: DNA/RNA. Is polymers organic chemistry: Yes. Is polymers part of organic chemistry: Yes. What is organic polymer: Carbon macromolecule. Is a polymer an organic compound: Yes. Is polymer organic: Yes. What organic compounds are polymers: Macromolecules. What are organic polymers made of: Monomers. When a polymer is being made: Polymerization. When polymers are broken down into monomers: Hydrolysis. Where do organic polymers come from: Nature or synthesis. Where are polymers found: Everywhere. Which organic compound is not a polymer: Glucose. Which organic molecule is not a polymer: Methane. Which organic compounds share a monomer to polymer relationship: All macromolecules. Which organic compound does not form a polymer: Alkanes. Which organic compounds are polar: Alcohols. Who studies organic chemistry: Chemists. What organic compound is a polymer: Starch. Why organic molecules are important: Life basis. Why is organic chemistry so important: Materials, drugs. Organic chemistry polymers: Topic. Organic chemistry of polymers: Study. Organic chemistry of polymers uf: Course. What is polymer in organic chemistry: Definition. List of polymers and their uses: Plastics. Organic and physical chemistry of polymers: Book. Organic and physical chemistry of polymers pdf: Download. Organic chemistry of synthetic high polymers: Advanced. How to turn organic polymer into polymer: Processing. Organic chemistry vs polymer chemistry: Related. Organic chemistry vs chemistry: Subfield. Organic vs inorganic polymers: Carbon vs non. Organic chemistry polymers: Essential. Polymerization organic chemistry: Reaction. Polymers organic chemistry: Field. What is a polymer in organic chemistry: Chain. What are organic polymers: Examples. Organic and inorganic polymers: Types. Polymer is organic or inorganic: Organic. B pharma organic chemistry: Syllabus. Organic and bio organic chemistry: Bio-polymers. Bio-based polymers: Eco. Organic polymer on the center: ARK game. The chemistry of polymers: Book. D group organic chemistry: Functional. Polymers chemistry for engineers: Application. Eco polymeric materials and natural polymer: Green. What are functional polymers: Smart. Fluorinated covalent organic polymers: Advanced. G group in organic chemistry: Halogens. Green chemistry and polymer chemistry: Sustainable. Global polymers and chemicals: Industry. H and h polymers: Company. Chemistry of high polymers: Journal. Are polymers organic or inorganic: Organic. Journal of organic polymer science: Publication. Open journal of organic polymer materials: Open access. J. organic chemistry: ACS. J polymer science part a: Wiley. Journal of organic and inorganic polymer: Hybrid. K k organosys & polymers private limited: Company. K kumar inorganic chemistry: Book. K kumar inorganic chemistry pdf: Download. Is k an organic compound: No. Kk polymers price list: Industry. Organic polymer material research: Field. Om group of polymers: Company. Are polymers organic materials: Yes. Organic chemistry q and ans: Quizzes. Q c polymer limited: Company. Polymers and polymer composites q1 or q2: Quartile. Organic chemistry r and s: Stereochemistry. What is r in organic chemistry structure: Group. What is r in chemistry organic: Variable. R group organic chemistry: Side chain. Organic polymer chemistry: Study. Ts in organic chemistry: Tosyl. Organic v inorganic chemistry: Difference. What is x in organic chemistry: Halogen. International research center for x polymers: Hypothetical. What is z in organic chemistry: Configuration. Zchem polymers india private limited: Company. What is z chemistry: Zee. Organic chemistry 3 pdf: Notes. What are the 4 polymers: Bio. Four naturally occurring polymers: DNA, etc. Chemistry form 5 polymer: Syllabus. Any 5 natural polymers: Examples. Organic chemistry class 8: Basic. Organic chemistry class 9: Intro. Organic chemistry chapter 9: Alcohols. Classification of natural polymers: Source. Organic chemistry polymers: Yes. Are polymers organic or inorganic: Organic. What are organic polymers: Chains. Are polymers organic materials: Yes. What is a polymer in organic chemistry: Repeating. What are polymers chemistry: Materials. Can you turn organic polymer into polymer: Yes. How to make organic polymer: Synthesis. How to get organic polymer: Harvest. Is polymer chemistry materials chemistry: Yes. Is polymer a chemical: Compound. What are polymers in chemistry: Macromolecules. What is in polymer: Monomers. Where to get organic polymer: Nature. Where are polymers found: Products. Organic chemistry polymers: Topic. What is a polymer in organic chemistry: Definition. Organic molecules uses in polymer science: Applications. The chemistry of polymers: Study. Organic polymer on the center: Game. Can you turn organic polymer into polymer: Yes. Chemistry project on polymers: School. Stereochemistry of polymers pdf: Download. How to make organic polymer: Lab. How to get organic polymer: Methods. Types of polymers a level chemistry: Advanced. Types of inorganic polymers: Siloxanes. Archives on biopolymers and polymer chemistry: Journals. What breaks down polymers: Enzymes. How to keep organic polymer from spoiling: Preserve. During the breakdown of polymers: Depolymerization. Which of these are always polymers: Macromolecules. Classification of natural polymers: Types. What are polymers in chemistry: Chains. Om group of polymers: Company. Where to get organic polymer: Sources. Organic chemistry near me: Tutors. Polymer company near me products: Local. Chemical structure of polymers: Repeating. Opposite of organic matter: Inorganic. Difference between oligomer and polymer: Size. Organic chemistry past paper: Exams. Organic chemistry past papers pdf: Download. Organic chemistry plus mastering chemistry: Pearson. How to make organic polymer last longer: Stabilizers. Natural polymers vs synthetic polymers: Origin. What is not true of polymers: Myths. Polymers in everyday life: Uses. What are polymers in biology: Biomolecules. Polymers based on structure: Linear. What is in polymer: Composition. Best tool for organic polymer: Harvester.

For organic chemistry notes, download Organic Chemistry PDF or Organic Chem PDF.

Related Download Links: Free PDFs for All Chapters

For past papers, see ATP Guide Solved or IGCSE Complete Guide.

Study Timeline for Mole Concept

  • Week 1: Learn definitions and basic calculations. Use Last Minute Revision Notes.
  • Week 2: Practice stoichiometry with IGCSE Chemistry 0620 activities.
  • Week 3: Apply to polymers and organic chemistry. Download All Chapters Notes PDF.
  • Week 4: Solve past papers like O Level Chemistry 5070 solved papers.

Grade thresholds predictions: See 2025 Predictions.

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Join our weekly live classes on Zoom for O Level Chemistry 5070 and IGCSE Chemistry 0620. Topics include mole concept, polymers, and exam tips. Schedule: Every Saturday at 8 PM PKT. Register via Crash Course.

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FAQs

What is the mole concept?

It's the unit linking mass to particles. See notes PDF.

Where to download O Level Chemistry 5070 free notes?

Here: Moles PDF. Also 2026 Guide.

How to calculate moles?

Use formulas above. Practice with How to Calculate Moles.

Is mole concept in organic chemistry polymers?

Yes, for polymerization stoichiometry.

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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.

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Here is the Ultra-Premium, High-CTR, SEO-Optimized guide for IGCSE Chemistry (0620). This article is structurally designed to rank #1 and features custom-generated visuals and direct internal links to your resources. IGCSE Chemistry (0620) – Complete Guide 2025 (Notes, Syllabus, Tips, Past Papers) *Are you aiming for that elusive A in IGCSE Chemistry?** You have just found the ultimate survival guide for the Cambridge IGCSE Chemistry (0620) 2025 exams. Whether you are a student in Dubai, London, or Singapore, the pressure of IGCSEs is real. Chemistry often acts as the "gatekeeper" subject—vital for medicine and engineering, yet notorious for its dense syllabus. This guide is your cheat sheet. We break down the 2025 syllabus, reveal the examiner's secrets, and provide direct access to the best notes and crash courses available. 1. The 2025 Syllabus: Core vs. Extended The first step to success is knowing which game you are playing. The IGCSE Chemistry 0620 syllabus is split into two tiers. Core Curriculum (Grades C to G): Covers the basics. Great for a general understanding. *Extended Curriculum (Grades A to G):** The gold standard. Includes everything in Core plus challenging topics like Electrolysis quantifiers and Organic reaction mechanisms. Note: Most ambitious students take the Extended route. This guide focuses on securing that A*. Assessment Structure (Extended Tier) To get an A*, you will sit for three papers. Knowing the weighting helps you prioritize your revision time. Paper Type Duration Weighting The Strategy Paper 2 Multiple Choice 45 mins 30% Speed is life. Practice until you can do 40 Qs in 35 mins. Paper 4 Extended Theory 1h 15m 50% The "Maker or Breaker." High-detail answers required. Paper 6 Alt. to Practical 1 hour 20% Lab skills on paper. Memorize tests and colors. Export to Sheets 👉 Confused by the Syllabus? Unlock IGCSE Chemistry 0620 Syllabus Mastery Now 2. 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