IGCSE/O-Level/Oxford/Edexcel Organic Chemistry: Plastic Made Easy in 2026
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Introduction to Plastics in Organic Chemistry
In 2026, mastering plastics (polymers) in organic chemistry is key for IGCSE Chemistry 0620 and O Level Chemistry 5070 exams. Organic chemistry polymers involve large molecules from monomers, essential for understanding everyday materials. Instead of wasting time on irrelevant YouTube videos that don't cover the full syllabus and are ad-filled, opt for structured resources. Studies show 70% of students improve grades with syllabus-aligned courses (educational data 2025). Enroll in our Organic Chemistry Crash Course at https://cambridgeclassroom.com/courses/organic-chemistry-alkanes-to-polymers/, P1 Past Papers Session at https://cambridgeclassroom.com/courses/past-papers-session-for-the-o-level-chemistry-5070-course/, or Full Syllabus Crash Course at https://cambridgeclassroom.com/courses/crash-course-for-chemistry-5070-0620/.
Key Definitions: Concise, Exam-Centered
- Polymer: Large molecule from many monomers (repeating units). What is polymer in organic chemistry? Core for IGCSE/ O-Level.
- Monomer: Small molecule joining to form polymer. Monomers and polymers organic chemistry key relation.
- Addition Polymerization: Alkenes form polymers by adding without byproducts. Organic chemistry polymerization example: poly(ethene).
- Condensation Polymerization: Monomers with functional groups join, releasing water. Types of polymers organic chemistry include this.
- Poly(ethene): Addition polymer from ethene, used in plastics. Organic polymers examples.
- Nylon: Condensation polymer from diamine and dicarboxylic acid. Synthetic polymers organic chemistry.
- Biodegradable Polymer: Breaks down naturally. Properties implications for disposal in syllabus.
For more, see Definitions List or 2025 Guide.
Detailed Explanations of Plastics (Polymers)
Organic chemistry polymers: Are polymers organic chemistry? Yes, carbon-based. Is polymers part of organic chemistry? Core in IGCSE organic chemistry polymers. Master organic chemistry polymers with examples.
Types of polymers in organic chemistry: Addition (e.g., PVC) and condensation (e.g., polyester). Synthetic polymers organic chemistry vs natural. Organic chemistry polymerisation: Addition uses alkenes; condensation functional groups polymers.
What is a polymer in organic chemistry: Chain from monomers. How are organic polymers made: Polymerization organic chemistry. Examples of organic polymers: Polyethene, starch (natural).
Are polymers organic or inorganic: Mostly organic. Organic vs inorganic polymers: Carbon vs silicon-based. What are inorganic polymers: Siloxanes in inorganic chemistry polymers.
Polymers in organic chemistry: Large organic polymers like DNA. How to find the monomer of a polymer: Look for repeating unit.
Organic compounds form polymers: True. Organic compounds are polymers except small molecules. What organic compounds are polymers: Carbs, proteins.
2 polymers of carbohydrates: Starch, cellulose. 2 polymers of proteins: Fibrous, globular. 3 types of organic polymers: Homo, co, block. 3 natural polymers: Rubber, silk, wool. 3 polymers: PE, PP, PS. 4 types of organic polymers: Based on origin, tacticity, etc. 4 polymers: Nylon, Teflon, PVC, PET. 4 organic compounds and their monomers: Nucleic acids (nucleotides), etc. 4 polymers and their monomers: Polyethene (ethene), etc.
5 polymers: Bakelite, etc. 5 polymers used in everyday life: Plastic bags (PE), bottles (PET). 5 examples of polymers: DNA, nylon. 5 organic compounds: Alkanes to esters. 5 natural polymers: Chitin, lignin.
6 organic molecules: In bio. 6 organic compounds: Groups. 6 polymers: Variants. 7 types of polymers: Classifications.
The organic chemistry tutor polymers: Helpful. 8 organic compounds: Functional. 9-10 organic chemistry: Advanced.
Are polymers organic compounds: Yes. Is polymer chemistry organic: Yes. Does polymers come under organic chemistry: Yes. What is organic polymer used for: Packaging.
Is polymer chemistry organic or inorganic: Organic. How polymers work: Chains entangle. How do organic polymers contribute to biological diversity: DNA codes.
What is organic polymer: Macromolecule. Is a polymer an organic compound: Yes. Is polymer organic: Yes. What are organic polymers made of: Carbon monomers.
When a polymer is being made: Polymerization. When polymers are broken down into monomers: Hydrolysis. Where do organic polymers come from: Petrochemicals or bio.
Where are polymers found: Products. Which organic compound is not a polymer: Ethanol. Which organic molecule is not a polymer: Glucose.
Which organic compounds share a monomer to polymer relationship: 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: Cellulose. Why organic molecules are important: Life. Why is organic chemistry so important: Materials.
Organic chemistry of polymers: Study. Organic chemistry of polymers uf: Course. List of polymers and their uses: PE for bags.
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: Subset. Organic chemistry vs chemistry: Branch.
Polymer is organic or inorganic: Organic. B pharma organic chemistry: Includes polymers. Organic and bio organic chemistry: Bio-based polymers.
Organic polymer on the center: Game ref. The chemistry of polymers: Royal Society book.
D group organic chemistry: Vitamins. Polymers chemistry for engineers: Applications. Eco polymeric materials and natural polymer: Sustainable.
What are functional polymers: Responsive. Fluorinated covalent organic polymers: Materials.
G group in organic chemistry: Aldehydes. Green chemistry and polymer chemistry: Eco. Global polymers and chemicals: Industry.
H and h polymers: Company. Chemistry of high polymers: Journal.
Journal of organic polymer science: Pub. Open journal of organic polymer materials: Access.
J. organic chemistry: ACS. J polymer science part a: Wiley. Journal of organic and inorganic polymer: Hybrid.
K k organosys & polymers private limited: Firm. K kumar inorganic chemistry: Book. K kumar inorganic chemistry pdf: Download. Is k an organic compound: No. Kk polymers price list: Rates.
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: Firm. Polymers and polymer composites q1 or q2: Ranking.
Organic chemistry r and s: Stereo. What is r in organic chemistry structure: Group. What is r in chemistry organic: Variable. R group organic chemistry: Side.
Ts in organic chemistry: Tosylate. Organic v inorganic chemistry: Diff.
What is x in organic chemistry: Variable. International research center for x polymers: Hypothetical.
What is z in organic chemistry: Config. Zchem polymers india private limited: Company. What is z chemistry: Term.
Organic chemistry 3 pdf: Notes. What are the 4 polymers: Bio. Four naturally occurring polymers: Proteins, etc.
Chemistry form 5 polymer: Syllabus. Any 5 natural polymers: Examples.
Organic chemistry class 8: Basics. Organic chemistry class 9: Intro. Organic chemistry chapter 9: Polymers.
Classification of natural polymers: Source. What are polymers chemistry: Materials.
Can you turn organic polymer into polymer: Yes. How to make organic polymer: Synthesis. How to get organic polymer: Extract.
Is polymer chemistry materials chemistry: Yes. Is polymer a chemical: Yes. What are polymers in chemistry: Chains.
What is in polymer: Monomers. Where to get organic polymer: Sources.
Organic molecules uses in polymer science: Apps. Chemistry project on polymers: School.
Stereochemistry of polymers pdf: Download. Types of polymers a level chemistry: Iso, syndio.
Types of inorganic polymers: Phosphazenes. Archives on biopolymers and polymer chemistry: Journals.
What breaks down polymers: Enzymes. How to keep organic polymer from spoiling: Store.
During the breakdown of polymers: Depoly. Which of these are always polymers: Macros.
What are polymers in chemistry: Repeat. Where to get organic polymer: Labs.
Organic chemistry near me: Tutors. Polymer company near me products: Local.
Chemical structure of polymers: Chains. Opposite of organic matter: Inorganic.
Difference between oligomer and polymer: Length. Organic chemistry past paper: Exams.
Organic chemistry past papers pdf: Download. Organic chemistry plus mastering chemistry: Tool.
How to make organic polymer last longer: Additives. Natural polymers vs synthetic polymers: Origin.
What is not true of polymers: Biodegrade fast. Polymers in everyday life: Ubiquitous.
What are polymers in biology: Biomols. Polymers based on structure: Linear, branched.
What is in polymer: Composition. Best tool for organic polymer: Harvester.
For syllabus, see IGCSE Syllabus 2025 or O Level 2025.
Related Download Links: Free PDFs
- Oxygen and Air PDF
- Chemical Bonding PDF - Ultimate Pack
- Chemical Energetics PDF
- Experimental Techniques PDF
- Formula PDF - Formula Sheet
- Formulae PDF
- Metals PDF
- Metals PDF (Alt)
- Moles PDF - Mole Concept
- Organic Chemistry PDF
- Reactions PDF
- Redox PDF
- States of Matter PDF
- The Periodic Table PDF - Embed
- States of Matter PDF (Alt)
- Atoms, Elements and Compounds PDF - Atom Notes
- Organic Chem PDF
- Acids, Bases and Salts PDF
- Electrolysis PDF
- Hydrogen and Water PDF
For notes, All Chapters 2025 or Save My Exams 2025.
Study Timeline for Polymers
- Week 1: Definitions and types. Use Revision Notes.
- Week 2: Polymerization reactions. Predict Products.
- Week 3: Examples and disposal. Practice IGCSE Chemistry 0620 activities.
- Week 4: Past papers. See ATP Solved.
Thresholds: 2025 Predictions.
Live Class Details
Weekly Zoom classes for polymers in organic chemistry. Saturdays 8 PM PKT. Register via Crash Course.
Teacher Profile: Prof. Faisal Janjowa
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FAQs
What are polymers?
Large chains from monomers. See Organic Chemistry PDF.
How to master polymers for 2026 exams?
Enroll in crash course. Practice with IGCSE Guide.
What's addition polymerization?
Alkenes adding. Exam tip for IGCSE.
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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)
