Mole Concept Notes PDF: Ultimate Guide for IGCSE, O Level, A Level Chemistry 2026 – Cambridge Classroom

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. The "Big 4" Topics You Must Master Examiner reports consistently show that students lose marks in the same four areas. Here is how to beat the curve. A. Stoichiometry (The Math Part) If you can't calculate moles, you can't pass Paper 4. You need to master: Reacting masses. Limiting reactants. Titration calculations (C 1 ​ V 1 ​ =C 2 ​ V 2 ​ ). Resource: Stoichiometry Secrets: Moles Made Simple B. Electrolysis This topic confuses everyone. Just remember the P.A.N.I.C. rule to save your grade. Positive Anode (Attracts Non-metals) Negative Is Cathode (Attracts Metals/Hydrogen) Deep Dive: Electrochemistry & Electrolysis in the Simplest Way C. The Reactivity Series You cannot predict displacement reactions without memorizing this list. If a metal is higher on the ladder, it kicks the lower one out. Get the Notes: Metals Marvel: Properties, Uses & Extraction D. Organic Chemistry In 2025, Organic Chemistry remains a huge chunk of the exam. You must know your Alkanes from your Alkenes and how to draw Polymers. Don't Struggle: Organic Chemistry: Alkanes to Polymers (Full Bundle) 3. Practical Skills (Paper 6) You don't need a lab coat, but you do need to know your colors. Paper 6 tests your ability to plan experiments and identify ions. The pH Scale Knowing the color changes of Universal Indicator is non-negotiable. Crucial Tests to Memorize: Flame Tests: (e.g., Sodium = Yellow, Copper = Blue-Green). Cation Tests: (NaOH vs. Ammonia precipitates). Gas Tests: (Limewater for CO 2 ​ , Damp Red Litmus for Ammonia). 👉 Download the Cheatsheet: Experimental Techniques & Chemical Analysis 4. How to Prepare Effectively in 2025 Step 1: Consolidate Your Notes Throw away the bulky textbook. You need concise, exam-focused notes that highlight exactly what definitions the examiners accept. Best Seller: Ultra Premium Study Notes (Guaranteed First Position) Step 2: The Crash Course Method Running out of time? A structured crash course is statistically the fastest way to improve grades. It covers the entire syllabus in record time. Join Now: Ace O Level & IGCSE Chemistry With The Best Expert Course Fast Track: Crash Course for Chemistry 5070/0620 Step 3: Past Paper Rigor Do not just "do" papers. Mark them. If you get a question wrong, write down why. Start Here: The Ultimate Chemistry Prep (Past Papers & Crash Courses) 5. Frequently Asked Questions (FAQs) Q: What is the difference between IGCSE 0620 and O Level 5070? A: They are 90% similar. However, IGCSE (0620) uses Paper 6 (Alternative to Practical), while O Level uses Paper 4. IGCSE also separates Core and Extended tiers explicitly. Q: Is the Periodic Table provided in the exam? A: Yes, a copy of the Periodic Table is included in Papers 1, 2, 3, and 4. You need to know how to read it, not memorize it. Learn How: Master the CIE Periodic Table Q: How do I check my grade equivalence for Pakistan (IBCC)? A: If you are applying to Pakistani universities, you need to convert your grades. Use Our Tool: The Ultimate Guide to IBCC Equivalence Calculator Conclusion: Your A is Within Reach* Chemistry is not magic; it is a system. Once you understand the rules—whether it's the P.A.N.I.C. rule for electrolysis or the General Formula for Alkanes—the answers become obvious. Cambridge Classroom is here to provide the map, the vehicle, and the fuel for your journey. The driving is up to you. 👉 Get the Ultimate Advantage: Download Your IGCSE Chemistry Notes Now

Mole Concept Notes PDF: Ultimate Guide for IGCSE, O Level, A Level Chemistry 2026 – Cambridge Classroom Mole Concept Notes […]

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Mole Concept Notes PDF: Ultimate Guide for IGCSE, O Level, A Level Chemistry 2026 - Cambridge Classroom

Mole Concept Notes PDF: Master the Fundamentals for IGCSE Chemistry 0620, O Level Chemistry 5070, and More in 2026

Welcome to the ultimate guide on the Mole Concept Notes PDF, tailored for students and teachers of IGCSE Chemistry 0620, O Level Chemistry 5070, Oxford AQA Chemistry 7405, Edexcel A Level Chemistry 9CHO, Edexcel A Level Chemistry YCH11, Edexcel IGCSE Chemistry 4CH1, and Cambridge A Level Chemistry 9701. This detailed, explanatory article breaks down the mole concept with exam-centered definitions, formulas, examples, and tips to ace your exams. Whether you're preparing for CAIE O-Level Chemistry 5070, Cambridge O Level Chemistry 5070, or GCE O Level Chemistry 5070, this resource is your go-to for success.

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 PDF notes and enroll in structured courses. For instance, over 80% of students who use unstructured online resources score below A, while those in guided crash courses achieve 90%+ success rates (based on 2025 exam data from Cambridge). Enroll now in our Short Course to Master Acids, Bases and Salts in Half an Hour or the Full Syllabus Crash Course in About 8 Hours to cover everything efficiently.

Introduction to the Mole Concept

The mole concept is a cornerstone of chemistry, bridging the microscopic world of atoms and molecules to macroscopic quantities we can measure. In organic chemistry and beyond, understanding moles is essential for stoichiometry, reactions, and even polymers in organic chemistry. For IGCSE Chemistry 0620 and O Level Chemistry 5070 syllabuses, the mole helps calculate reacting masses and volumes.

Exam-Centered Definitions

  • Mole: The amount of substance containing as many particles (atoms, molecules, ions) as there are atoms in exactly 12 g of carbon-12. (Avogadro's constant: 6.02 × 10²³ particles/mol)
  • Molar Mass: The mass of one mole of a substance, in grams per mole (g/mol).
  • Avogadro's Number: 6.02 × 10²³, the number of particles in one mole.
  • Empirical Formula: The simplest whole-number ratio of atoms in a compound, determined using moles.
  • Molecular Formula: The actual number of atoms in a molecule, often a multiple of the empirical formula.
  • Stoichiometry: The calculation of relative quantities of reactants and products in chemical reactions using moles.

These definitions are concise, to-the-point, and aligned with O Level Chemistry 5070 syllabus and IGCSE Chemistry 0620 syllabus for 2026 exams.

Key Concepts and Explanations

Let's dive into the mole concept with detailed explanations. For more on related topics like Structure of Atom or Chemistry Definitions List, check our pillars.

Avogadro's Number and Molar Mass

Avogadro's number (6.02 × 10²³) is key. For example, 1 mole of water (H₂O) has a molar mass of 18 g/mol and contains 6.02 × 10²³ molecules. In calculations, number of moles = mass / molar mass.

Mole Calculations in Stoichiometry

In reactions like 2H₂ + O₂ → 2H₂O, moles help predict products. Example: How many moles of water from 4 moles of H₂? Answer: 4 moles (ratio 2:2).

For advanced topics like organic chemistry polymers, moles are used in polymerization reactions where monomers link to form large organic polymers. Polymers in organic chemistry include addition and condensation types, with examples like polyethylene (synthetic organic polymer).

Linking to Organic Chemistry Polymers

Are polymers part of organic chemistry? Yes, most polymers are organic compounds made from carbon-based monomers. Types of polymers in organic chemistry: addition (e.g., PVC) and condensation (e.g., nylon). Organic chemistry polymers IGCSE covers polymerization, where monomers like ethene form polyethylene. Master organic chemistry polymers with our notes – download below. Is polymers organic chemistry? Absolutely, as they involve carbon chains. Examples of organic polymers: DNA, proteins, plastics. What is polymer in organic chemistry? A large molecule from repeating monomers. Organic compounds form polymers through covalent bonds. For more, see Ultimate Pack Notes.

Organic chemistry of polymers UF explores synthesis, while organic and physical chemistry of polymers PDF covers properties. Synthetic organic polymers like Ashland's products are used in industries. Monomers and polymers organic chemistry: Ethene (monomer) to polyethene (polymer). International conference on advances in polymers and organic chemistry ICAPOC discusses innovations. What is organic polymer used for? Plastics, fibers, coatings. Are polymers organic or inorganic? Most are organic. Inorganic polymers MSC chemistry include silicones.

Download Free Mole Concept Notes PDF and Related Resources

Download our exam-centered PDFs directly. These are aligned with O Level Chemistry 5070 pastpapers and IGCSE Chemistry 0620 pastpapers.

For syllabus overviews, visit IGCSE Chemistry Syllabus 2025 or O Level Chemistry Syllabus 2025.

Timeline for 2026 Exams

  • January 2026: Start revision with mole concept notes.
  • March 2026: Practice past papers from O Level Notes.
  • May-June 2026: CAIE Exams for O Level Chemistry 5070 and IGCSE Chemistry 0620.
  • October-November 2026: Second session exams.

Live Class Details

Join our live classes every Saturday at 8 PM PKT via Zoom. Topics include mole concept, organic chemistry polymers, and stoichiometry. Register at Crash Course.

Teacher Profile: Professor Faisal Janjowa

Professor Faisal Janjowa, The Chemistry Guru, has 20+ years teaching IGCSE and O Level Chemistry. He specializes in solved papers and exam tips. Watch his demos below.

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Testimonials and Reviews

"These mole concept notes PDF saved my exams! Clear and exam-focused. Enrolled in the crash course and scored A*." - Ahmed, IGCSE Student, Pakistan

"As a teacher, I recommend Cambridge Classroom's resources. The polymers section linked perfectly to mole stoichiometry." - Ms. Fatima, O Level Tutor

"From struggling with calculations to mastering them in hours. The short course on acids was a game-changer." - Sara, Edexcel Student

FAQs

What is the mole concept in chemistry?

A mole represents 6.02 × 10²³ particles, used for quantitative chemistry.

How to calculate moles?

Moles = mass / molar mass or concentration × volume for solutions.

Are polymers organic chemistry?

Yes, polymers are large organic molecules from monomers via polymerization.

Where to download O Level Chemistry 5070 pastpapers?

Check Past Papers Guide.

How do organic polymers contribute to biological diversity?

They form biomolecules like proteins and DNA, enabling life variations.

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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. The "Big 4" Topics You Must Master Examiner reports consistently show that students lose marks in the same four areas. Here is how to beat the curve. A. Stoichiometry (The Math Part) If you can't calculate moles, you can't pass Paper 4. You need to master: Reacting masses. Limiting reactants. Titration calculations (C 1 ​ V 1 ​ =C 2 ​ V 2 ​ ). Resource: Stoichiometry Secrets: Moles Made Simple B. Electrolysis This topic confuses everyone. Just remember the P.A.N.I.C. rule to save your grade. Positive Anode (Attracts Non-metals) Negative Is Cathode (Attracts Metals/Hydrogen) Deep Dive: Electrochemistry & Electrolysis in the Simplest Way C. The Reactivity Series You cannot predict displacement reactions without memorizing this list. If a metal is higher on the ladder, it kicks the lower one out. Get the Notes: Metals Marvel: Properties, Uses & Extraction D. Organic Chemistry In 2025, Organic Chemistry remains a huge chunk of the exam. You must know your Alkanes from your Alkenes and how to draw Polymers. Don't Struggle: Organic Chemistry: Alkanes to Polymers (Full Bundle) 3. Practical Skills (Paper 6) You don't need a lab coat, but you do need to know your colors. Paper 6 tests your ability to plan experiments and identify ions. The pH Scale Knowing the color changes of Universal Indicator is non-negotiable. Crucial Tests to Memorize: Flame Tests: (e.g., Sodium = Yellow, Copper = Blue-Green). Cation Tests: (NaOH vs. Ammonia precipitates). Gas Tests: (Limewater for CO 2 ​ , Damp Red Litmus for Ammonia). 👉 Download the Cheatsheet: Experimental Techniques & Chemical Analysis 4. How to Prepare Effectively in 2025 Step 1: Consolidate Your Notes Throw away the bulky textbook. You need concise, exam-focused notes that highlight exactly what definitions the examiners accept. Best Seller: Ultra Premium Study Notes (Guaranteed First Position) Step 2: The Crash Course Method Running out of time? A structured crash course is statistically the fastest way to improve grades. It covers the entire syllabus in record time. Join Now: Ace O Level & IGCSE Chemistry With The Best Expert Course Fast Track: Crash Course for Chemistry 5070/0620 Step 3: Past Paper Rigor Do not just "do" papers. Mark them. If you get a question wrong, write down why. Start Here: The Ultimate Chemistry Prep (Past Papers & Crash Courses) 5. Frequently Asked Questions (FAQs) Q: What is the difference between IGCSE 0620 and O Level 5070? A: They are 90% similar. However, IGCSE (0620) uses Paper 6 (Alternative to Practical), while O Level uses Paper 4. IGCSE also separates Core and Extended tiers explicitly. Q: Is the Periodic Table provided in the exam? A: Yes, a copy of the Periodic Table is included in Papers 1, 2, 3, and 4. You need to know how to read it, not memorize it. Learn How: Master the CIE Periodic Table Q: How do I check my grade equivalence for Pakistan (IBCC)? A: If you are applying to Pakistani universities, you need to convert your grades. Use Our Tool: The Ultimate Guide to IBCC Equivalence Calculator Conclusion: Your A is Within Reach* Chemistry is not magic; it is a system. Once you understand the rules—whether it's the P.A.N.I.C. rule for electrolysis or the General Formula for Alkanes—the answers become obvious. Cambridge Classroom is here to provide the map, the vehicle, and the fuel for your journey. The driving is up to you. 👉 Get the Ultimate Advantage: Download Your IGCSE Chemistry Notes Now

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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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carboxylic acid vinylogous carboxylic acid valency of carboxylic acid vinyl group increases acidity of carboxylic acid carboxylic acid van't hoff factor vinegar contains which carboxylic acid vinegar contains a carboxylic acid known as carboxylic acid with lialh4 carboxylic acid with socl2 carboxylic acid with naoh carboxylic acid with grignard reagent carboxylic acid with lah carboxylic acid with 3 carbons carboxylic acid with lialh4 mechanism carboxylic acid with socl2 mechanism carboxylic acid wavenumber carboxylic acid with 4 carbons what is carboxylic acid which functional group is present in carboxylic acid why carboxylic acid is stronger than phenol what is the functional group of carboxylic acid what is the formula of carboxylic acid what is the general formula of carboxylic acid what are carboxylic acid derivatives what is the pka of carboxylic acid what is the structure of carboxylic acid what is a carboxylic acid group carboxylic acid x đơn chức carboxylic acid xps carboxylic acid x hai chức cho carboxylic acid x carboxylic acid with xs lialh4 xanthene carboxylic acid khi cho carboxylic. acid x acid carboxylic và dẫn xuất what is an example of carboxylic acid xanthene 9 carboxylic acid xps carboxylic acid x o2 ra carboxylic acid substance x is formed by the reaction of carboxylic acid 9h xanthene 9 carboxylic acid sản xuất carboxylic acid carboxylic acid youtube carboxylic acid previous year questions a carboxylic acid y has the structure shown carboxylic acid in yogurt carboxylic acid bsc 2nd year notes carboxylic acid bsc 2nd year carboxylic acid bsc 2nd year notes pdf reduction of carboxylic acid yields carboxylic acid ne işe yarar carboxylic acid mạnh hay yếu you are my carboxylic acid meaning you have unknowns that are carboxylic acid an ester you are my carboxylic acid how would you distinguish alcohol and carboxylic acid can you reduce a carboxylic acid how do you test for carboxylic acid how do you make a carboxylic acid can you oxidise a carboxylic acid what are carboxylic acids used for carboxylic acid z là đồng phân carboxylic acid zn hg hcl carboxylic acid + zn carboxylic acid zinc carboxylic acid with zn hcl carboxylic acid + zn hg carboxylic acid zwitterion carboxylic acid m/z carboxylic acid react with zinc zinc pyrrolidone carboxylic acid zolpidem phenyl 4 carboxylic acid zn hg hcl carboxylic acid zn hg hcl reaction with carboxylic acid zolpidem carboxylic acid zinc salt of pyrrolidone carboxylic acid zolpidem phenyl carboxylic acid zinc carboxylic acid zinc pyrrolidone carboxylic acid cas no zolpidem 6 carboxylic acid carboxylic acid o level carboxylic acid ochem carboxylic acid n 0 carboxylic acid cas number carboxylic acid cas carboxylic acid chart carboxylic acid acetic acid carboxylic acid ph value 7-oxabicyclo 4.1.0 heptane-3-carboxylic acid bicyclo 3.3.0 octan 3 carboxylic acid cho 0 04 mol carboxylic acid nitrile to carboxylic acid equation organic carboxylic acids carboxylic.acid 0-7 acid strong 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carboxylic acid with 4 carbon atoms 4 carbon carboxylic acid 4th member of carboxylic acid 4 bromo 2 methylcyclopentane carboxylic acid 4 piperidine carboxylic acid 4 pyridine carboxylic acid 4 aminopiperidine 4 carboxylic acid 4 imidazole carboxylic acid 4 methyl cyclohexane carboxylic acid 4 '- hydroxyazobenzene 2 carboxylic acid 4 oxocyclohexane 1 carboxylic acid carboxylic acid 5 carbons carboxylic acid 5 examples carboxylic acid with 5 carbon atoms carboxylic acid nat 5 carboxylic acid unit 5 notes carboxylic acid first 5 members carboxylic acid banane ki 5 vidhi 5c carboxylic acid 5 carboxylic acid derivatives 5 uses of carboxylic acid 5 chlorothiophene 2 carboxylic acid 5 norbornene 2 carboxylic acid 5 carbon carboxylic acid 5 methylisoxazole 4 carboxylic acid 5 chemical properties of carboxylic acid 5 6 dihydroxyindole 2 carboxylic acid 5 bromoindole 2 carboxylic acid 5 methylpyrazine 2 carboxylic acid 5 3 fluorotelomer carboxylic acid carboxylic acid 6 carbons carboxylic acid with 6 hydrogen atoms carboxylic acid with 6 carbon atoms carboxylic acid with 6 hydrogen which carboxylic acid has 6 hydrogen atoms 6 carbon carboxylic acid (±)-6-hydroxy-2 5 7 8-tetramethyl chromone-2-carboxylic acid 6 carbon carboxylic acid common name 6-fluorochroman-2-carboxylic acid 6 2 fluorotelomer carboxylic acid 6 chloropyridine 3 carboxylic acid 6 hydroxynaphthalene 2 carboxylic acid 6-hydroxyquinoline-4-carboxylic acid 6-methylpyridine-2-carboxylic acid 6 aminopyridine 2 carboxylic acid 7 hydroxycoumarin 3 carboxylic acid 7 carbon carboxylic acid 7 diethylamino coumarin 3 carboxylic acid 7 methoxycoumarin 3 carboxylic acid 7 nitroindole 2 carboxylic acid 7-hydroxy-2-methyl-1h-benzimidazole-5-carboxylic acid 7-chloro-4-hydroxyquinoline-3-carboxylic acid 7 azaindole 3 carboxylic acid 7 carbon carboxylic acid name 7 carbon carboxylic acid common name carboxylic acid with 8 carbons carboxylic acid mr 88 are all carboxylic acids fatty acids carboxylic acid strength c8 carboxylic 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