Grades 7-8,
Grades 9-10,
Grades 11-12
November 15, 2025
Registration deadline
November 13, 2025
December 20, 2025
Registration deadline
December 18, 2025
March 24-30, 2026
Registration deadline
February 1, 2026
Welcome to the Brainiacs Chemistry Olympiad!
In a world driven by innovation and discovery, chemistry stands as the cornerstone of understanding the matter that shapes our universe. Often referred to as the “central science,” chemistry bridges the physical and biological realms, offering insights into everything from the structure of atoms to the reactions that fuel life and technology. Whether it’s developing sustainable materials, advancing medicine, or creating solutions to global challenges, chemistry is at the forefront of progress.
The Brainiacs Chemistry Olympiad is designed to spark curiosity and deepen understanding in students. This competition goes beyond equations and formulas—it’s about unraveling the secrets of matter, solving intricate problems, and exploring the forces that drive chemical transformations. Participants will enhance their critical thinking, embrace creativity, and build skills that pave the way for a world of possibilities.
Chemistry empowers us to innovate and create a sustainable future and inspire the next generation of chemists and problem-solvers to lead the way in shaping a better tomorrow. Let’s unlock the brainiac in every student!
Experience the thrill of competition and the joy of achievement.
20 Q Preliminary
20+2 Q Global Final
75 min Preliminary
120+120 min Global Final
English, Russian,
French, and Spanish
MECHANICS
Brainiacs Chemistry Olympiad Mechanics
The Brainiacs Chemistry Olympiad is a competition aimed at encouraging creativity, innovation, and academic excellence in students from Grade 7 to Grade 12. The Olympiad is structured into two main stages: the Preliminary Round and the Global Round.
PRELIMINARY ROUND
Registration
Students can register for the Olympiad through the official Brainiacs Olympiad website or via authorized representatives in their respective countries.
Dates
The online qualifying exams for the Preliminary Round are scheduled for:
- Round I: – November 15, 2025 (Registration deadline: November 14, 2025)
- Results: November 20, 2025
- Round II: – December 20, 2025 (Registration deadline: December 19, 2025)
- Results: – December 25, 2025
The two online rounds are the same, but feature different questions.
Those who did not qualify for the global round in the first online round, along with those who were absent from the first round, can participate in the second round.
Format
The exam consists of 20 questions divided into three levels of difficulty:
- Easy: 5 questions
- Normal: 10 questions
- Difficult: 5 questions
The exam consists of 20 multiple-choice questions to be completed within 75 minutes.
Questions are tailored to the participant’s educational level and divided into the following categories:
- Category 1: Grades 7 and 8
- Category 2: Grades 9 and 10
- Category 3: Grades 11 and 12
Scoring
- Easy Questions: +4 points for each correct answer
- Normal Questions: +5 points for each correct answer
- Difficult Questions: +6 points for each correct answer
- Incorrect Answer: No negative marking for any question
- Unanswered Question: No points deducte
Qualification
Participants scoring at least 40% in the Preliminary Round qualify for the Global Round. Every participant receives a Certificate of Participation.
Recognition
In the Preliminary Round, medals are awarded based on the points earned by the participants:
- 40 to 49 : Honorable Mention Certificate
- 50 to 74 : Bronze Medal
- 75 to 89 : Silver Medal
- 90 to 100 : Gold Medal
GLOBAL ROUND
The Global Round is the final stage of the competition, where participants showcase their knowledge and ability.
Registration
Students can register for the Olympiad through the official Brainiacs Olympiad website or via authorized representatives in their respective countries.
Dates and Venue
The Global Round of Brainiacs Olympiad will take place in Xiamen University Malaysia from March 24 to 30, 2026.
- Normal Registration Deadline: 28 February 2026
- Late Registration: March 1, 2026
Exam Days
Global Round exam format is different from Preliminary Round. It has both Theoretical and Practical parts separated in two consecutive examination days.
Day 1. Theoretical Part
This is the traditional portion of a chemistry exam it evaluates understanding of chemical concepts, reasoning, and the ability to solve theoretical problems.
Examples:
- Solving stoichiometric and chemical equation problems
- Explaining reaction mechanisms or trends in the periodic table
- Predicting products or outcomes of reactions
- Conceptual and multiple-choice questions on atomic structure, bonding, or thermodynamics
Purpose:
To test chemical knowledge, logical reasoning, and the ability to apply theoretical concepts to explain and predict chemical behavior.
Day 1. Exam Format
The exam consists of 20 questions divided into three levels of difficulty:
- Easy: 5 multiple-choice questions
- Normal: 5 multiple-choice questions
- Difficult: 5 multiple-choice questions
- Open-ended (difficult): 5 questions
The exam consists of 15 multiple-choice and 5 open-ended questions to be completed within 120 minutes.
Day 1. Exam Scoring
- Easy Questions: +4 points for each correct answer
- Normal Questions: +5 points for each correct answer
- Difficult Questions: +6 points for each correct answer
- Open-ended: +7 points for full correct solution and answer
- Incorrect Answer: No negative marking for any question
- Unanswered Question: No points deducted
Day 2. Practical Part
The practical part checks how students can apply chemical knowledge in experimental or problem-solving situations (laboratory and data-analysis tasks).
Examples:
- Performing simple chemical reactions and observing changes (color, gas, temperature)
- Identifying substances through tests (e.g., flame test, pH test)
- Analyzing data from experiments such as titrations or rate-of-reaction studies
Purpose:
To test students’ ability to plan, conduct, and interpret chemical experiments safely and logically, linking theory with observable results.
Day 2. Exam Format and Scoring
The exam consists of two tasks, each worth 50 points, to be completed within 120 minutes. Each task includes several questions that test a range of skills, including conceptual understanding, analytical thinking, and practical application.
Global Round Recognition
In the Global Round, medals are awarded based on the percentage distribution according to the number of participants.
- The top 10% (0-10%) of participants receive gold medals.
- The next 20% (11-30%) of participants receive silver medals.
- The next 30% (31-60%) of participants receive bronze medals.
- The next 15% (61-75%) receive honorable mentions.
Languages
All of the questions in Preliminary and Global Rounds will be in 4 languages:
English, Russian, French, and Spanish
SYLLABUS
1. INTRODUCTION TO CHEMISTRY
1.1 What is Chemistry?
1.1.1 Definition
1.1.2 Branches of chemistry (organic, inorganic, physical, analytical, biochemistry)
1.1.3 Historical milestones in chemistry discovery
1.2 Importance of Chemistry in Daily Life
1.2.1 Food, medicine, energy, environment, materials
1.2.2 Role in technology and innovation
1.3 Chemistry and Safety
1.3.1 Laboratory safety rules
1.3.2 Common safety symbols and their meanings
2. STATES OF MATTER
2.1 Solids, Liquids, and Gases
2.1.1 Properties
2.1.2 Particle arrangement
2.1.3 Compressibility
2.1.4 Diffusion in different states of matter
2.2 Changes in States of Matter
2.2.1 Melting, freezing, boiling, condensation, sublimation, deposition
2.2.2 Effect of pressure and temperature on states (gas laws intro)
2.3 Other States of Matter
2.3.1 Plasma (intro)
2.3.2 Bose–Einstein Condensate (intro)
3. ELEMENTS, COMPOUNDS, AND MIXTURES
3.1 Definitions and Examples
3.1.1 Metals, nonmetals, and metalloids
3.2 Differences Between Elements, Compounds, and Mixtures
3.2.1 Physical vs. chemical properties
3.3 Separation Techniques
3.3.1 Filtration
3.3.2 Distillation
3.3.3 Evaporation
3.3.4 Crystallization
3.3.5 Chromatography
3.3.6 Magnetic separation
3.3.7 Decantation
3.3.8 Centrifugation
3.4 Applications of Separation Methods in Industry
4. ATOMIC STRUCTURE
4.1 Introduction to Atoms
4.1.1 Dalton’s atomic theory (limitations & modern view)
4.2 Subatomic Particles
4.2.1 Proton, neutron, electron – relative mass & charge
4.2.2 Nucleus and electron cloud
4.3 Simple Atomic Models
4.3.1 Thomson’s model
4.3.2 Rutherford’s model
4.3.3 Bohr’s model (basic)
4.4 Atomic Number and Mass Number
4.4.1 Isotopes and their real-life uses (medicine, archaeology, energy)
5. THE PERIODIC TABLE
5.1 Introduction & History
5.1.1 Mendeleev and modern periodic table
5.2 Groups and Periods
5.2.1 Trends in properties (atomic size, metallic character, reactivity – intro level)
5.3 Common Elements and Their Symbols
5.3.1 First 20 elements
5.3.2 Transition metals (Fe, Cu, Zn, Ag, Au)
5.4 Special Element Families
5.4.1 Alkali metals
5.4.2 Alkaline earth metals
5.4.3 Halogens
5.4.4 Noble gases
6. ACIDS, BASES, SALTS, AND INDICATORS
6.1 Properties of Acids and Bases
6.1.1 Taste, feel, conductivity
6.1.2 pH scale
6.2 Natural and Synthetic Indicators
6.2.1 Litmus
6.2.2 Phenolphthalein
6.2.3 Methyl orange
6.2.4 Red cabbage extract
6.3 Neutralization Reactions
6.3.1 Everyday examples (medicine for acidity, soil treatment)
6.4 Acid Rain – Causes and Effects
6.4.1 Environmental impact
7. MATTER AND ITS CLASSIFICATION
7.1 Pure Substances and Mixtures
7.1.1 Homogeneous mixtures
7.1.2 Heterogeneous mixtures
7.2 Colloids
7.2.1 Types: sols, gels, emulsions, aerosols
7.2.2 Tyndall effect
8. ATOMIC STRUCTURE (ADVANCED)
8.1 Electronic Configuration
8.1.1 First 20 elements
8.1.2 Orbital concept (basic s & p orbitals)
8.2 Mass Number & Isotopic Abundance Calculations
8.3 Isotopes in Medicine & Industry
9. CHEMICAL BONDING
9.1 Ionic Bonds
9.1.1 Properties of ionic compounds
9.2 Covalent Bonds
9.2.1 Single, double, triple bonds
9.2.2 Properties of covalent compounds
9.3 Metallic Bonding (Intro)
9.3.1 Explanation of conductivity and malleability
9.4 Polar vs. Non-polar Molecules
10. CHEMICAL REACTIONS
10.1 Types of Chemical Reactions
10.1.1 Combination
10.1.2 Decomposition
10.1.3 Displacement
10.1.4 Double displacement
10.2 Balancing Equations
10.2.1 Step-by-step method
10.3 Law of Conservation of Mass
10.4 Factors Affecting Reaction Rate
10.4.1 Temperature
10.4.2 Concentration
10.4.3 Catalysts
10.4.4 Surface area
10.5 Catalysts in Industry and Nature
10.5.1 Enzymes
11. THERMOCHEMICAL & REDOX REACTIONS
11.1 Thermochemical Reactions
11.1.1 Exothermic vs. endothermic
11.1.2 Energy diagrams (intro)
11.2 Redox Reactions
11.2.1 Oxidation, reduction, oxidizing agents, reducing agents
11.2.2 Simple redox in daily life (rusting, bleaching, photosynthesis)
12. THE MOLE CONCEPT & STOICHIOMETRY
12.1 Mole Calculations
12.1.1 Mass → moles → particles conversions
12.2 Molar Mass & Avogadro’s Number
12.3 Relative Atomic & Molecular Mass
12.4 Empirical and Molecular Formula Calculations
12.5 Limiting Reagent Problems
12.6 Percentage Yield (basic level)
13. ENVIRONMENTAL CHEMISTRY
13.1 Air & Water Pollution
13.1.1 Major pollutants and sources
13.2 Greenhouse Gases & Global Warming
13.2.1 Carbon cycle (intro)
13.3 Acid Rain
13.3.1 Prevention and control
13.4 Waste Management
13.4.1 Recycling
13.4.2 Biodegradable vs. non-biodegradable materials
1. ATOMIC STRUCTURE AND THE PERIODIC TABLE
1.1 Atomic Number and Mass Number
1.1.1 Definitions
1.1.2 Differences between atomic number and mass number
1.2 Isotopes
1.2.1 Definition and examples
1.3 Electronic Configuration
1.3.1 Arrangement of electrons in shells
1.4 The Periodic Table: Groups and Periods
1.4.1 Group numbers and properties
1.4.2 Period numbers and element classification
2. BONDING, STRUCTURE, AND PROPERTIES OF MATTER
2.1 Types of Bonding
2.1.1 Ionic bonding
2.1.2 Covalent bonding
2.1.3 Metallic bonding
2.2 Properties of Compounds
2.2.1 Properties of ionic compounds
2.2.2 Properties of covalent compounds
2.3 Structures
2.3.1 Giant ionic structures
2.3.2 Giant covalent structures
2.3.3 Simple molecular substances
3. CHEMICAL REACTIONS
3.1 Types of Chemical Reactions
3.1.1 Combustion
3.1.2 Displacement
3.1.3 Decomposition
3.2 Balancing Chemical Equations
3.2.1 Rules and steps for balancing
3.3 Reaction Energy Types
3.3.1 Exothermic reactions
3.3.2 Endothermic reactions
4. ACIDS, BASES, AND SALTS
4.1 Properties of Acids and Bases
4.1.1 Physical properties
4.1.2 Chemical properties
4.2 Indicators and pH Calculations
4.2.1 Common indicators (litmus, phenolphthalein, methyl orange)
4.2.2 pH scale and calculations
4.3 Preparation of Salts
4.3.1 Neutralization method
4.3.2 Precipitation method
4.3.3 Crystallization method
5. CHEMICAL CALCULATIONS
5.1 Mole Calculations
5.1.1 Mass → moles → particles conversions
5.2 Stoichiometric Calculations
5.2.1 Reacting masses
5.2.2 Using balanced equations
5.3 Mixture Problems
5.3.1 Mass composition and separation calculations
5.4 Determination of Unknown Substances
5.4.1 Using experimental data
5.5 Solutions and Solubility
5.5.1 Solute, solvent, and types of solutions (solid, liquid, gas)
5.5.2 Definition and units of concentration
5.5.3 Molarity (mol/L) calculations
5.6 Dilution of Solutions
5.6.1 Concept
5.6.2 Mathematical expressions
5.7 Properties of Solutions
5.7.1 Factors affecting solubility
6. CHEMICAL CHANGES
6.1 Reactivity Series
6.1.1 Order of reactivity of metals
6.1.2 Displacement reactions
6.2 Extraction of Metals
6.2.1 Reduction methods
6.2.2 Electrolysis methods
6.3 Redox Reactions
6.3.1 Oxidation and reduction definitions
6.3.2 Examples in daily life
7. ENERGY CHANGES
7.1 Energy in Reactions
7.1.1 Exothermic reactions
7.1.2 Endothermic reactions
7.2 Bond Energy Calculations
7.2.1 Using bond energies to calculate enthalpy change (ΔH)
7.3 Applications
7.3.1 Uses of exothermic reactions
7.3.2 Uses of endothermic reactions
7.4 Energy Diagrams
7.4.1 Representation of reaction profiles
8. RATES OF REACTION
8.1 Factors Affecting Reaction Rates
8.1.1 Temperature
8.1.2 Concentration
8.1.3 Surface area
8.1.4 Catalysts
8.2 Measuring Reaction Rates
8.2.1 Gas collection method
8.2.2 Mass loss method
8.2.3 Color change observation
9. ORGANIC CHEMISTRY
9.1 Introduction to Hydrocarbons
9.1.1 Definition and classification
9.2 Alkanes, Alkenes, and Alkynes
9.2.1 Structures
9.2.2 Properties
9.2.3 Reactions
9.3 Alcohols, Aldehydes, Ketones, and Carboxylic Acids
9.3.1 Functional groups
9.3.2 Basic properties
9.4 Polymers and Their Uses
9.4.1 Addition polymers
9.4.2 Condensation polymers
10. ENVIRONMENTAL CHEMISTRY
10.1 Air and Water Pollution
10.1.1 Sources
10.1.2 Effects
10.1.3 Prevention methods
10.2 Greenhouse Gases and Global Warming
10.2.1 Causes
10.2.2 Effects on climate
10.3 Sustainable Development
10.3.1 Environmental conservation strategies
1. BASIC CONCEPTS OF CHEMISTRY
1.1 Importance and Scope of Chemistry
1.2 Atomic and Molecular Masses
1.3 Mole Concept and Molar Mass
1.4 Chemical Stoichiometry
1.5 Empirical and Molecular Formulas
1.6 Percentage Composition and Purity
1.7 Limiting Reagents and Yield Calculations
1.8 Dalton’s Atomic Theory and Modern Modifications
2. ATOMIC STRUCTURE
2.1 Dual Nature of Matter and Light
2.2 Photoelectric Effect and Wave-Particle Duality
2.3 Quantum Mechanical Model of Atom
2.4 Quantum Numbers and Their Significance
2.5 Electronic Configuration of Atoms (Aufbau, Hund’s rule, Pauli exclusion)
2.6 Shapes of Atomic Orbitals and Probability Distributions
2.7 Atomic Spectra and Line Spectra of Hydrogen
2.8 Spin-Orbit Coupling and Fine Structure
3. CHEMICAL BONDING AND MOLECULAR STRUCTURE
3.1 Ionic Bonds: Formation and Properties
3.2 Covalent Bonds: Types and Characteristics
3.3 Polar and Non-polar Covalent Bonds
3.4 Valence Bond Theory and Hybridization (sp, sp2, sp3, sp3d, sp3d2)
3.5 Molecular Orbital Theory: Bond Order, Stability, and Magnetic Properties
3.6 VSEPR Theory and Molecular Geometry
3.7 Hydrogen Bonding and Intermolecular Forces
3.8 Resonance and Formal Charge
3.9 Molecular Polarity and Dipole Moments
4. STATES OF MATTER
4.1 Gaseous State: Ideal Gas Equation and Deviations
4.2 Real Gases: van der Waals Equation and Critical Phenomena
4.3 Kinetic Molecular Theory of Gases
4.4 Liquid State: Surface Tension, Viscosity, and Vapor Pressure
4.5 Solid State: Types of Crystalline Solids (Ionic, Covalent, Metallic, Molecular)
4.6 Amorphous Solids and Glass Transition
4.7 Defects in Solids: Point, Line, and Planar Defects
4.8 Packing Efficiency and Unit Cells
4.9 Band Theory of Solids
5. THERMODYNAMICS
5.1 First Law of Thermodynamics
5.2 Internal Energy and Work
5.3 Enthalpy Changes: Combustion, Formation, Neutralization
5.4 Hess’s Law and Standard Enthalpy Changes
5.5 Second Law of Thermodynamics and Entropy
5.6 Gibbs Free Energy and Spontaneity
5.7 Thermodynamic Equations and Applications
5.8 Heat Capacity and Calorimetry
6. EQUILIBRIUM
6.1 Chemical Equilibrium and Dynamic Nature
6.2 Equilibrium Constant (Kc, Kp) and Le Chatelier’s Principle
6.3 Ionic Equilibrium in Solutions
6.4 Acid-Base Concepts: Arrhenius, Bronsted-Lowry, Lewis Theories
6.5 pH, pOH, and Buffer Solutions
6.6 Solubility Product and Common Ion Effect
6.7 Hydrolysis of Salts
6.8 Indicators and Titration Curves
6.9 Complex Ion Equilibria
7. SOLUTIONS
7.1 Types of Solutions and Concentration Terms (Molarity, Molality, Mole Fraction)
7.2 Raoult’s Law and Ideal Solutions
7.3 Colligative Properties: Boiling Point Elevation, Freezing Point Depression, Osmotic Pressure
7.4 Abnormal Molar Mass and Van’t Hoff Factor
7.5 Henry’s Law and Gas Solubility
7.6 Distribution Law
8. ELECTROCHEMISTRY
8.1 Electrochemical Cells: Galvanic and Electrolytic
8.2 Standard Electrode Potentials and Electrochemical Series
8.3 Nernst Equation and its Applications
8.4 Conductance, Molar Conductance, and Kohlrausch’s Law
8.5 Electrolysis and Faraday’s Laws
8.6 Batteries and Fuel Cells
8.7 Corrosion and Its Prevention
9. CHEMICAL KINETICS
9.1 Rate of Reaction and Rate Laws
9.2 Factors Affecting Reaction Rates
9.3 Order and Molecularity of Reactions
9.4 Integrated Rate Equations (Zero, First, Second Order)
9.5 Half-life of Reactions
9.6 Arrhenius Equation and Activation Energy
9.7 Collision Theory and Transition State Theory
9.8 Catalysis: Homogeneous and Heterogeneous Catalysts
10. COORDINATION CHEMISTRY
10.1 Coordination Compounds: Definition and Examples
10.2 Nomenclature of Coordination Compounds
10.3 Bonding in Coordination Compounds: Werner’s Theory
10.4 Crystal Field Theory and Splitting of d-Orbitals
10.5 Spectrochemical Series and Color of Complexes
10.6 Magnetic Properties of Complexes
10.7 Isomerism in Coordination Compounds
10.8 Stability Constants and Chelate Effect
11. ORGANIC CHEMISTRY BASICS
11.1 Classification and Nomenclature of Organic Compounds
11.2 Functional Groups and Their Reactions
11.3 Isomerism: Structural, Geometrical, and Optical
11.4 Mechanisms of Organic Reactions: Substitution, Addition, Elimination
11.5 Stereochemistry: Chirality, Enantiomers, Diastereomers
11.6 Reactive Intermediates: Carbocations, Carbanions, Free Radicals
12. ORGANIC CHEMISTRY ADVANCED
12.1 Aldehydes and Ketones: Preparation and Reactions
12.2 Carboxylic Acids and Their Derivatives
12.3 Amines: Classification, Preparation, and Properties
12.4 Biomolecules: Carbohydrates, Proteins, Lipids, Nucleic Acids
12.5 Polymers: Types, Polymerization Methods, and Applications
12.6 Organic Spectroscopy: IR, NMR, Mass Spectrometry
12.7 Pericyclic Reactions and Aromaticity
13. CHEMISTRY IN EVERYDAY LIFE
13.1 Drugs and Pharmaceuticals
13.2 Chemicals in Food and Agriculture
13.3 Cleaning Agents and Detergents
13.4 Cosmetics and Soaps
13.5 Metals and Alloys in Daily Use
13.6 Fuel and Combustion
14. ENVIRONMENTAL CHEMISTRY
14.1 Pollution: Air, Water, and Soil
14.2 Green Chemistry Principles and Applications
14.3 Ozone Layer and UV Radiation
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SAMPLE PAPERS & MATERIALS
Practice with these examples to understand the format, sharpen your skills, and prepare for the challenges ahead.
