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Chemistry Form 1 - Form 4 notes (56)

All high school notes Chemistry notes from Form 1 to Form 4.

Chemistry Notes 

Topical revision questions

ALL CHEMISTRY PRACTICALS FOR SECONDARY SCHOOLS

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Chemistry Notes Form 1 - Summarized Notes Easy Elimu

Chemistry Notes Form 1 - Summarized Notes Easy Elimu (5)

Get the complete Form 1 chemistry notes based on the CBC curriculum for free on Easy Elimu to help you prepare for local and national exams.

The chemistry form 1 notes in this category are obtained from the numerous high school approved text books, including KLB chemistry, and others. For the purpose of preparing for both national and local exams, it includes the complete chemistry approved notes for form 1 based on the latest curriculum (CBC).

You can get these form one Chemistry notes for free without having to pay a cent on our Easy Elimu Study App, which you can get from Google Playstore here. 
As a bonus, each chemistry topic and subtopic has summarized notes, so you won’t have to stress over writing that mwakenya, which makes passing that summative Chemistry form 1 term 3 exam easy. No matter the term—term 1, term 2, or term 3—these free chemistry form 1 summary notes will get you an A.

How to optimally use this page (Get chemistry form 1 all notes here.)

  1. Find the topic you're looking for by scrolling down.
  2. When you locate the information you seek, click on the chapter heading to explore the numerous subtopics.

Best chemistry revision notes form 1 per topic - Easy Elimu

Chemistry notes form 1 introduction 1

Topic 1: Introduction to Chemistry - Form 1 Chemistry Summarized Notes

  • Topic Review
    • Matter
    • Separation of mixture
    • Metals and non metals
    • conductors and non-conductors of electricity
    • Drugs and Drug Abuse
  • Chemistry and the Society
    • Definition of chemistry and its role in the society
  • Chemistry laboratory
    • Apparatus
    • The Bunsen Burner
    • Safety in the Laboratory
    • Laboratory Safety Rules.

Topic 2: Simple Classification of Substances - Form 1 Chemistry Revision Notes

  • Types of Mixtures
    • Solutions/solid-liquid dissolved mixture
    • Suspension/ precipitates/solid-liquid mixture which do not dissolve
    • Miscibles /Liquid-liquid mixtures
    • Immiscibles/Liquid-liquid mixtures
    • Solid-solid mixtures/Alloys
    • Common alloys of metal.
  • Methods of separating mixtures
    • Decantation
    • Filtration
    • Evaporation
    • Distillation
    • Fractional distillation
    • Separation of immiscibles (Using a separating funnel)
    • Sublimation/deposition
    • Chromatography
    • Solvent extraction
    • Crystallization
  • Physical/Temporary and Chemical changes
    • Heating ice
    • Examples of Physical and Chemical Processes

Topic 3: Air and Combustion - Form 1 Chemistry Revision Notes

  • The Atmosphere
    • To find the composition of air supporting combustion using a candle stick
    • To find the composition of active part of air using heated copper turnings.
    • To find the composition of active part of air using alkaline pyrogallol
    • To establish the presence of carbon (IV) oxide in air using lime water
  • Oxygen
    • Occurrence
    • School laboratory preparation.
    • Uses of Oxygen
  • Chemical properties of Oxygen /combustion
    • Reaction of metals with Oxygen/air
    • Reaction of non metals with Oxygen/air
    • Reactivity series/competition for combined Oxygen.

Topic 4: Water and Hydrogen - Form 1 Chemistry Revision Notes

  • Water
    • Tests for Presence of Water
    • Burning a candle in air
    • Water pollution
    • Reaction of water with metals
  • Hydrogen
    • Occurrence
    • School laboratory Preparation
    • Properties of Hydrogen gas
    • Water as an Oxide of Hydrogen
    • Uses of Hydrogen gas

Topic 5: Acids, Bases and Indicators - Form 1 Chemistry Revision Notes

  • Introduction to Acids, Bases and Indicators
  • Properties of acids
    • Physical properties of acids
    • Chemical properties of acids

After you are done reading these summarized Chemistry notes, you can test yourself with our chemistry form 1 questions and answers, which you can access here.

Moreover, if you are having a problem with a specific topic or want to practice more, you can practice with our chemistry Form 1 topical revision questions and answers, which you can access here.

Download the Easy Elimu chemistry Notes Form 1. Get them in PDF format on the Easy Elimu Study App.

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KCSE and MOCKS Chemistry Practicals Notes

KCSE and MOCKS Chemistry Practicals Notes (7)

Get the best chemistry practicals notes to help with your revision.

These notes explain the most commonly set chemistry practicals questions for Kenyan Schools.

The best KCSE and MOCKS chemistry practicals notes in Kenya

The above are all the chemistry practical notes with revision questions and answers that you need to pass your KCSE and MOCKS Chemistry Practicals.

ALL CHEMISTRY PRACTICALS FOR SECONDARY SCHOOLS - Easy Elimu

chem practicals 1
KCSE Chemistry Practicals

Titration/volumetric analysis Summary Notes - Easy Elimu

titration 1

What you get;

  1. Glossary of terms including:
    • Titration
    • Indicator
    • Quantitative
    • Acid-alkali
    • Neutralises
    • Valid
    • Precise
    • Accurate
    • Pipette
    • End-point
    • Repeatable
    • Titre
    • Meniscus
  2. Aims of titration
  3. Practical activity 1 - Sample Titration table format
  4. Practical activity 2 - carrying out a titration
    • Sample results titration
    • Analysis of results of titration
  5. Evaluation of learner's understanding
    • Titration general questions and answers
  6. Hazards, risks and precautions when carrying out titration

Get these complete Titration revision notes with set questions and answers here.

Thermochemistry(energy changes) Summary Notes - Easy Elimu

heat

What you get;

  1.  Glosssary of terms including:
    • Energy
    • Endothermic
    • Exothermic
    • Rise in temperature (-ΔH)
    • Fall in temperature (+ΔH)
    • Physical changes
    • Chemical changes
    • Melting/liquidification/fusion
    • Freezing/fusion/solidification
    • Boiling/vaporization/evaporation
    • Kinetic Theory of matter
    • Neutralization
    • Condensation/liquidification
    • Extrapolation point
    • Standard enthalpy/heat of displacement
    • Standard enthalpy/heat of neutralization
    • Standard enthalpy/heat of solution/dissolution
  2. Quick tips (practically section)
  3. Energy changes in physical processes
  4. Experiments for energy changes in physical processes.
    1. To determine the boiling point of water
      1. Procedure
      2. Sample question 1 (graph and table of temperature and time)
      3. Sample question 2
      4. Sample question 3 (Calculation of molar heat of vaporization of water)
    2. To determine the melting point of candle wax
      1. Procedure
      2. Sample question (table and graph of temperature and time)
  5. Energy changes in chemical processes
    1. Standard enthalpy/heat of displacement ΔHod
      1. Examples of displacement reactions
      2. Experiments I showing how to determine the molar standard enthalpy/heat of displacement copper
        • Sample question 1 (Calculating average change in temperature of reaction)
        • Sample question 2 (Calculating the percentage enthalpy change)
        • Sample question 3 (Writing the ionic equation)
        • Sample question 4 (Observations)
      3. Experiments II showing the graphical determination of molar enthalpy of displacement
    2. Standard enthalpy/heat of neutralization ΔHon
      1. Simplified notes on what standard enthalpy/heat of neutralization
      2. Experiment to determine the molar enthalpy of neutralization of Hydrochloric acid
        1. Procedure
        2. Theoretical revision questions with answers
    3. Standard enthalpy/heat of solution/dissolution ΔHos
      1. Simplified notes on what  standard enthalpy of solution
      2. Experiment to determine the heat of dissolution of ammonium nitrate (V)
        1. Procedure
        2. Theoretical revision questions with answers

Get these complete thermochemistry / energy changes revision notes with set questions and answers here.

Chemical kinetic(rates of reaction) Summary Notes - Easy Elimu

What you get:

  1. Defination of terms
  2. Examples
  3. Instructions on how to use a stop watch/clock
  4. Factors that theoretically and practically influence the rate or reactions including:
    1. Concentration of reactants
    2. Temperature
    3. Nature of reactants
    4. Physical state of reactants
    5. Surface area of reactants
    6. Effect of solvent
    7. The presence of a catalyst
  5. Lab safety/precautions for chemical kinetics reactions

Get these complete chemical kinetic / rate of reaction revision notes with set questions and answers here.

Read on the Reaction Rates and Reversible Reactions - Form 4 Chemistry notes that are related to the chemical kinetics practical on the Easy Elimu Website here.

Remember: You can access all these notes on the Easy Elimu app for free. Download it now!

Qualitative analysis(organic/inorganic) Summary Notes - Easy Elimu

Get these complete qualitative analysis revision notes with set questions and answers here.

What you get; 

  1. Process of identifying unknown inorganic compounds
    1. When using 2M sodium hydroxide
    2. When using 2M aqueous ammonia
    3. When using Barium(II)nitrate(V)/Barium chloride solution
  2. Process of identifying unknown organic compounds
    1. Identified through burning-a substance
    2. When using bromine water
    3. When using chlorine water
    4. When using acidified KMnO4
    5. When using acidified K2Cr2O7
    6. Using litmus paper test

The inorganic compunds tested and formed include; K+, Na+, Nh4+, Zn2+ Pb2+ Al3+ , Ba2+ Mg2+ Ca2+, Cu2+, Fe2+, Fe3+, PbSO4 ,PbSO3 ,PbCO3, PbS, PbI2,PbCl2, SO42- ,SO32- ,CO32- Cl-, I-, S2-, CO32-, BaSO4 ,BaSO3 , BaCO3,  from SO42- ,SO32- 

Flame test Summary Notes - Easy Elimu

flame test

Get these questions answered with these Easy Elimu flame test notes.

  1. What is a flame test?
  2. Why use flame test?
  3. Why do different metal ions produce different flame colours?
  4. How do you carry out a flame test?

Also get notes on:

  • What you need to do to conduct a valid flame experiment
  • The distinct flame coloration of some compounds including:
    • Lithium
    • Sodium
    • Potassium
    • calcium
    • Barium
    • Copper

Finally you get some revision questions with answers to test your grasp of flame test experiment.

Get these complete flame test revision notes with set questions and answers here.

Physical / general chemistry Summary Notes - Easy Elimu

Get these complete physical chemistry revision notes with set questions and answers here.

Chemistry practicals FAQs navigator

Chemistry practicals FAQs

How many practicals are required for chemistry?

In KCSE chemistry paper 3, there are usually 3 practical questions set. These three questions can be derived from any of the above-mentioned practicals, such as titration/volumetric analysis, thermochemistry (energy changes), chemical kinetics (rates of reaction), qualitative analysis (organic/inorganic), solubility and solubility curves, flame test, and physical/general chemistry. 

How do I pass the KCSE chemistry practicals?

To pass the chemistry practicals, whether they are KCSE chemistry practicals or MOCK chemistry practicals, you need to first know the kinds of experiments that can be examined. The table below shows the kinds of experiments that were tested from KCSE 2010 up to now so that you can be able to deduce the practical that will be tested in your year.

To get the specific papers with marking schemes for the various KCSE practicals, click on the highlighted KCSE year in the table.

 KCSE Year  Types of Experiments Tested
KCSE Chemistry Practicals 2010
  1. Titration/volumetric analysis
  2. Qualitative analysis (had section a & b)
KCSE Chemistry Practicals 2011
  1. Titration/Volumetric analysis
  2. Thermochemistry
  3. Qualitative analysis
KCSE Chemistry Practicals 2012
  1. Titration/Volumetric analysis
  2. Solubility
  3. Qualitative analysis
KCSE Chemistry Practicals 2013
  1.                            
    1. Thermochemistry
    2. Volumetric analysis/Titration
  2. Qualitative analysis
  3. Qualitative analysis
KCSE Chemistry Practicals 2014
  1.                        
    1. Volumetric analysis/Titration
    2. Thermochemistry
  2. Qualitative analysis of inorganic compounds
  3. Qualitative analysis of organic compounds
KCSE Chemistry Practicals 2015
  1.                    
    1. Thermochemistry
    2. Volumetric analysis/Titration
  2. Qualitative analysis of inorganic compounds
  3. Qualitative analysis of organic compounds
KCSE Chemistry Practicals 2016
  1. Chemical kinetics
  2. Qualitative analysis of organic compounds
  3. Qualitative analysis of inorganic compounds
KCSE Chemistry Practicals 2017
  1.                    
    1. Thermochemistry
    2. Volumetric analysis
  2. Qualitative analysis of inorganic compounds
  3. Qualitative analysis of organic compounds
KCSE Chemistry Practicals 2018
  1.                
    1. Thermochemistry
    2. Volumetric analysis
  2. Qualitative analysis of inorganic compounds
  3. Qualitative analysis of organic compounds
KCSE Chemistry Practicals 2019
  1. Chemical kinetics
  2. Qualitative analysis of inorganic compounds
  3. Qualitative analysis of organic compounds
KCSE Chemistry Practicals 2020
  1.                 
    1. Thermochemistry
    2. Volumetric analysis
  2. Qualitative analysis of inorganic compounds
  3. Qualitative analysis of organic compounds
KCSE Chemistry Practicals 2021
  1.                              
    1. Titration/Volumetric analysis
    2. Titration/Volumetric analysis
  2. Chemical kinetics
  3. Qualitative analysis of inorganic compounds
KCSE Chemistry Practicals 2022
  1.  
    1.                    
      1. Solubility - physical properties
      2. Titration/volumetric analysis
    2. Thermochemistry
  2. Qualitative analysis of organic compounds
  3. Qualitative analysis of inorganic compounds

Based on the table above you can see the most common practical exams given for each KCSE exam since 2010. 

This table is suppose to help you revise as you can now know the probability of each practical test being examined.

Note:

  • Though some chemistry practicals are not exclusively indicated as the main question, you may find that they appear in the other practicals. Take for example solubility experiments. Solubility is tested in qualitative analysis where in the inference you can note whether the products of the reactants are either soluble or insoluble.

How do you do chemistry practicals?

Depending on the type of chemistry practical you are being tested on, clear and well-defined instructions will be given on the paper/instruction sheet.

First, one is given a list of chemicals and tools that you are provided with to conduct the test or experiment.

Then clear instructions or steps on how to conduct the experiment are given in the procedure section.

Note: You do not have to cram the instructions/steps for conducting an experiment as they will be provided in the paper. What you need to know is simply the theory behind the experiment.

Read the instructions twice. The first time is to get a general sense of what the test wants you to do. The second time, read as you underline the main ideas and questions of the practical. Doing this will ensure that you do not miss anything.

Remember: As you conduct the experiments, you need to record the data fast. Accurate data recording will ensure that you are able to answer the questions accurately based on your calculations.

With Easy Elimu, either through this website or the Easy Elimu Study app, you will be able to access all the chemical practicals you need to practice and make sure that you pass that KCSE practical exam.

How do I prepare a chem lab practical?

  1. Quick tips to pass those chemistry paper 3 exams:
  • If you see a table showing time and temperature that is a thermochemistry experiment that tests the changes in heat of a chemical reaction
    Example:

    evtemp
    Table for thermochemistry practical
  • If the table that appears in a question contains final and initial burette readings and volume of solution that is most probably a titration/volumetric analysis experiment
    Example:

    burettetable
    table for titration/volumetric analysis practical
  •  When you get a stop watch to test the rate of reaction that is most probably a Chemical kinetics experiment.

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Chemistry Notes Form 2 - Easy Elimu

Chemistry Notes Form 2 - Easy Elimu (7)

Get the complete Form 2 chemistry notes based on the CBC curriculum for free on Easy Elimu to help you prepare for local and national exams.

The chemistry form 2 notes in this category are obtained from the numerous high school approved text books, including KLB chemistry, and others. For the purpose of preparing for both national and local exams, it includes the complete chemistry approved notes for form 2 based on the latest curriculum (CBC).

You can get these form two Chemistry notes for free without having to pay a cent on our Easy Elimu Study App, which you can get from Google Playstore here. 
As a bonus, each chemistry topic and subtopic has summarized notes, so you won’t have to stress over writing that mwakenya, which makes passing that summative Chemistry form 2 term 3 exam easy. No matter the term—term 1, term 2, or term 3—these free chemistry form 2 summary notes will get you an A.

How to optimally use this page (Get chemistry form 2 all notes here.)

  1. Find the topic you're looking for by scrolling down.
  2. When you locate the information you seek, click on the chapter heading to explore the numerous subtopics.

Best chemistry revision notes form 2 per topic - Easy Elimu
form 2

Topic 1: Structure of the Atom and the Periodic Table - Form 2 Summarized Chemistry Notes

  • The Atom
    • Parts of an Atom
    • Structure of the Atom
    • Atomic Number and Mass Number
    • Notation of Atomic Number and Mass Number
    • Atomic Properties of the First 20 Elements
    • Isotopes
  • Energy Levels and Electron Arrangements
    • Energy Levels
    • Electron Arrangement.
    • Dot and Cross Diagrams
  • The Periodic Table
    • Design of the Modern Periodic Table
    • Placing an Element in the Periodic Table
    • The Period:
    • Group:
  • Relative Atomic Mass and Isotopes.
    • Introduction:
    • Definition:
    • Measurement of Relative Atomic Mass
  • Ion Formation
    • Introduction
    • Ion
    • Electron Transfer During Chemical Reactions
    • Radicals
    • Oxidation Number
    • Chemical Formulae
    • Deriving the Chemical Formula of Compounds.
    • Chemical Equations
    • Balancing Chemical Equations
    • Types of State Symbols.

Topic 2: Chemical Families: Patterns in Properties - Form 2 Summarized Chemistry Notes

  • Introduction
    • Characteristics of a Chemical Family
    • Main Chemical Families
  • The Alkali Metals
    • Electron Arrangement of the First Three Alkali Metals
    • Diagram: Part of Periodic Table Showing the Alkali Metals
    • Gradation in Properties of Alkali Metals
    • Physical Properties of Alkali Metals
    • Chemical Properties of Alkali Metals
    • The General Trend in Reactivity of Alkali Metals.
    • Similarity of Ions and Formulae of Some Compounds of Alkali Metals.
    • Uses of Alkali Metals and their Compounds.
  • The Alkaline Earth Metals
    • Electron Arrangement of the First Three alkaline Earth Metals.
    • Diagram: Part of Periodic Table Showing the Alkaline Earth Metals 
    • Dot and Cross Diagram for the First Three Alkaline Earth Metals
    • Gradation in Properties of Alkaline Earth Metals.
    • Physical Properties of Alkaline Earth Metals.
    • Chemical Properties of Alkaline Earth Metals.
    • Trend in Reactivity in Alkaline Earth Metals.
    • Similarity of Ions and Formulae of Some Compounds of Alkaline Earth Metals.
    • Uses of Some Alkaline Earth Metals and their Compounds
  • The Halogens
    • Electron Arrangement of the First Three Halogens.
    • Diagram: Part of Periodic Table Showing the Halogens
    • Gradation in Properties of Halogens.
    • Laboratory Preparation of Chlorine.
    • Physical Properties of Halogens.
    • Chemical Properties of Halogens.
    • Some Uses of Halogens and their Compounds.
  • The Noble Gases.
    • Electron Arrangement of the First Three Noble Gases.
    • Diagram: Part of Periodic Table Showing the Noble Gases
    • Dot and Cross Diagrams for the First three Noble Gases
    • Physical Properties of Noble Gases
    • Chemical Properties of Noble Gases.
    • Uses of Some Noble Gases.

Topic 3: Properties and Trends Across a Period - Form 2 Summarized Chemistry Notes

  • Introduction:
  • The Period Three of the Periodic Table.
    • Part of Periodic Table Showing Period 3 of the Periodic Table. 
  • Trends in Physical Properties of Elements in Period 3.
    • Electrical Conductivity.
    • The Atomic and Ionic Radii.
    • Melting and Boiling Points
    • Summary: Some Physical Properties of Elements in Period 3.
  • Trends in Chemical Properties of the Elements in Period 3.
    • Trends in Reactivity.
    • Summary: Chemical Properties of Period 3 Elements.

Topic 4: Structure and Bonding - Form 2 Summarized Chemistry Notes

  • Meaning of Structure and Bond.
    • Bond
    • Structure
  • Nature of the Chemical Bond.
  • Types of Bonds.
    • Ionic Bonds/Electrovalent Bond.
    • The Covalent Bond.
    • The Coordinate Bond.
    • The Molecular Structures.
  • Types of Bonds Across a Period.
    • Variation in Bond Types in Oxides of Period Three Elements.
    • Effect of Bond Types of Properties of Chlorides of Period 3 Elements
    • Trends in Bond Types and Properties of Chlorides of Elements in Period 3
  • Summary: Characteristics of Bonds

Topic 5: Salts - Form 2 Summarized Chemistry Notes

  • Introduction to salts
    • Table Showing Normal and Acid Salts Derived from Common Acids
    • Table Showing Some Examples of Salts.
    • Table Showing Some Hydrated Salts.
    • Table of Some Complex Salts
    • Table of Some Double Salts
    • Table of Solubility of Salts
  • Preparation of Salts
    • Soluble Salts
    • Insoluble Salts
  • Effect of Heat on Salts
    • Effect of Heat on Chlorides
    • Effect of Heat on Nitrate(V)
    • Effect of Heat on Sulphate(VI)
    • Effect of Heat on Carbonates(IV) and Hydrogen Carbonate(IV).

Topic 6: Effect of an Electric Current on Substances - Form 2 Summarized Chemistry Notes

  • Introduction
  • Conductors and Insulators
    • Summary of Common Electrical Conductors
  • Electrolytes and Non-electrolytes
    • Strong Electrolyte
    • Weak Electrolyte
    • Non-electrolyte
  • Ionisation
  • Electrolytic Dissociation
    • Theory of Electrolytic Dissociation
  • Electrolysis of a Compound
  • Metallic Conductivity
  • Electrolytic Conductivity
  • Electrolysis Circuit
    • Electrode Reactions
  • Factors that Determine Products of Electrolysis
  • Electrolysis of Dilute Sulphuric Acid (Electrolysis of Water)
  • Electrolysis of Copper(II)Sulphate Solution
  • Electroplating
    • Electrolysis of Copper(II)sulphate Solution using Copper Electrodes
  • Electrolysis of Lead Bromide.

Topic 7: Carbon and it's Compounds - Form 2 Summarized Chemistry Notes

  • Introduction
    • Occurrence
    • Allotropes of Carbon
  • Properties of Carbon
    • Physical Properties of Carbon
    • Chemical properties of Carbon
  • Compounds of Carbon
    • Carbon(IV)Oxide (CO2)
    • Carbon(II)Oxide (CO)
    • Carbonate(IV) (CO32-)and Hydrogen Carbonate(IV)(HCO3-)
    • Sodium Carbonate(Na2CO3)

After you are done reading these summarized Chemistry notes, you can test yourself with our chemistry form 2 questions and answers, which you can access here.

Moreover, if you are having a problem with a specific topic or want to practice more, you can practice with our chemistry Form 2 topical revision questions and answers, which you can access here.

Download the Easy Elimu chemistry Notes Form 2. Get them in PDF format on the Easy Elimu Study App.

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Chemistry Notes Form 3 - Easy Elimu

Chemistry Notes Form 3 - Easy Elimu (6)

Get the complete Form 3 chemistry notes based on the CBC curriculum for free on Easy Elimu to help you prepare for local and national exams.

The chemistry form 3 notes in this category are obtained from the numerous high school approved text books, including KLB chemistry, and others. For the purpose of preparing for both national and local exams, it includes the complete chemistry approved notes for form 3 based on the latest curriculum (CBC).

You can get these form three Chemistry notes for free without having to pay a cent on our Easy Elimu Study App, which you can get from Google Playstore here. 
As a bonus, each chemistry topic and subtopic has summarized notes, so you won’t have to stress over writing that mwakenya, which makes passing that summative Chemistry form 3 term 3 exam easy. No matter the term—term 1, term 2, or term 3—these free chemistry form 3 summary notes will get you an A.

How to optimally use this page (Get chemistry form 3 all notes here.)

  1. Find the topic you're looking for by scrolling down.
  2. When you locate the information you seek, click on the chapter heading to explore the numerous subtopics.

Best chemistry revision notes form 3 per topic - Easy Elimu

chemistry form 3

Topic 1: Gas Laws - Form 3 Chemistry Summarized Notes

  • Kinetic Particle Theory
  • Diffusion and Kinetic Energy
    • Diffusion of Ammonia and Hydrogen Chloride
    • Graham's Law of Diffusion
  • Evaporation, Boiling and Kinetic Theory
    • Differences Between Evaporation and Boiling
    • Factors that Affect the Rate of Evaporation
  • Kinetic Theory and Gas Laws
    • Boyle's Law
    • Charles' Law
    • Pressure Law
  • Gases and the Kinetic Theory

Topic 2:The Mole: Formulae And Chemical Equations - Form 3 Chemistry Summarized Notes

  • Mole Concept
    • What is a Mole?
    • Relative Atomic Mass (R.A.M) and Moles
    • Relative Formula Mass (R.F.M) of a Compound
  • Stoichiometric and Ionic Equations
    • Chemical Word Equations
    • Stoichiometric Equations
    • Ionic Equations
  • Molarity
  • Titration: Acid and Alkali
    • How to Carry Out a Titration
    • Volumetric Analysis Titrations
    • Titration Technique

Topic 3: Organic Chemistry I - Form 3 Chemistry Summarized Notes

  • Products from Oil
    • Coal, Oil and Natural Gas Formation - Fossil Fuels
    • Hydrocarbons
    • Fractional Distillation of Crude Oil
  • Families of Organic Compounds
    • Homologous Series
    • Alkanes
    • Alkenes
    • Alkynes

Topic 4: Nitrogen and its Compounds - Form 3 Chemistry Summarized Notes

  • Nitrogen
    • Composition of Air
    • Preparation of Nitrogen from Air
    • Uses of Nitrogen
  • Nitrous Oxide
  • Nitric Oxide
  • Nitrogen Dioxide
  • Ammonia
    • Preparation of Ammonia
    • Chemical Properties of Ammonia
    • Physical Properties of Ammonia
    • Uses of Ammonia
  • Nitric Acid 
    • Oswald Process
    • Reactions of Nitric Acid
    • Nitrates

Topic 5: Sulphur and its Compounds - Form 3 Chemistry Summarized Notes

  • Sulphur
    • Extraction of pure Sulphur: Frasch Process
    • Physical Properties of Sulphur
    • Chemical Properties of Sulphur
    • Effect of Heat on Sulphur
    • Vulcanization of Rubber
    • Uses of Sulphur
  • Sulphur Dioxide
    • Occurence
    • Preparation of Sulphur Dioxide
    • Properties of Sulphur Dioxide
    • Chemical Properties of Sulphur Dioxide
    • Uses of Sulphur Dioxide
  • Sulphuric Acid
    • The Contact Process
    • Propertis of Sulphuric Acid
    • Industrial Uses

Topic 6: Chlorine and its Compounds - Form 3 Chemistry Summarized Notes

  • Chlorine
    • Laboratory Preparation
    • Manufacture of Chlorine
    • Products and Uses
    • Properties of Chlorine
    • Uses of Chlorine
  • Hydrogen Chloride
    • Preparation of Hydrogen Chloride
    • Properties of Hydrogen Chloride
    • Summary of Properties of Hydrogen Chloride

After you are done reading these summarized Chemistry notes, you can test yourself with our chemistry form 3 questions and answers, which you can access here.

Moreover, if you are having a problem with a specific topic or want to practice more, you can practice with our chemistry Form 3 topical revision questions and answers, which you can access here.

Download the Easy Elimu chemistry Notes Form 3. Get them in PDF format on the Easy Elimu Study App.

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Chemistry Notes Form 4 - Online Chemistry Summarized Notes - Easy Elimu

Chemistry Notes Form 4 - Online Chemistry Summarized Notes - Easy Elimu (7)

Get the complete Form 4 chemistry notes based on the CBC curriculum for free on Easy Elimu to help you prepare for local and national exams.

The chemistry form 4 notes in this category are obtained from the numerous high school approved text books, including KLB chemistry, and others. For the purpose of preparing for both national and local exams, it includes the complete chemistry approved notes for form 4 based on the latest curriculum (CBC).

You can get these form four Chemistry notes for free without having to pay a cent on our Easy Elimu Study App, which you can get from Google Playstore here. 
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Best chemistry revision notes form 4 per topic - Easy Elimu

chem form 4

Topic 1: Organic Chemistry II - Form 4 Summarized Chemistry Notes

  • Alcohols (Alkanols)
    • Nomenclature of Alcohols
    • Isomerism in Alkanols
    • Primary, Secondary and Tertiary Alcohols
    • Properties of Alcohols (Ethanol)
    • Uses of Ethanol
    • Tests for Primary Alkanols
    • Summary on Preparation of Alkanols(Ethanol)
    • Summary on Reactions of Alkanols
  • Akanoic Acids(Carboxylic Acids)
    • Nomenclature of Alkanoic Acids
    • Isomerism in Alkanoic Acids
    • Preparation of Alkanoic Acids
    • Properties of Alkanoic Acids
    • Uses of Alkanoic Acids (Ethanoic Acid)
    • Test for Alkanoic Acids
  • Fats and Oils
  • Soaps and Soapless Detergents
    • Soaps
    • Summary on Soap Preparation
    • Soapless Detergents
    • Summary: Manufacture of Soapless Detergents
  • Polymers
    • Natural Polymers and Fabrics
    • Synthetic Polmers
    • Advantages of Synthetic Polymers and Fibres over Natural polymers
    • Disadvantages of Synthetic Polymers and Fibres over Natural polymers
    • Methods of Polymerization

Topic 2: Acids, Bases and Salts - Form 4 Summarized Chemistry Notes

  • Acids
    • Strength of Acids
    • Role of Solvents on Acidic Properties of a Solute
    • Acidic properties
  • Bases
    • Alkalis
    • Effects of Type Of Solvent on the Properties of Ammonium Solution
  • Uses of Acids and Bases
  • Amphoteric Oxides and Hydroxides
    • Oxides
    • Reaction with Acids
    • Reaction with Alkalis
  • Salts
    • Laboratory Preparation of Salts
    • Types of Salts
    • Effects of Heat on Metal Hydroxides
    • Effects of Sodium Carbonate on Various Salt Solutions
    • Reaction of Metal Ions in Salt Solutions with Sodium Chloride, Sodium Sulphate and Sodium Sulphate
    • Uses (Importance) of Precipitation Reactions
    • Useful Information on Salts (Qualitative Analysis
    • Reduction-oxidation (Redox Reactions)
  • Solubility and Solubility Curves
    • Solubility
    • Factors Affecting Solubility
    • Solubility Curves
  • Water
    • Hardness of Water
    • Advantages of Hard Water
    • Disadvantages of Hard Water

Topic 3: Energy Changes in Chemical and Physical Processes (Thermochemistry) - Form 4 Summarized Chemistry Notes

  • Introduction
    • Specific Heat Capacity
  • The Heat Content (Enthalpy of a System)
    • Endothermic and Exothermic Reactions 
    • Activation Energy
    • Determination/Measurement of Enthalpy (Heat) Changes
  • Energy Level Diagrams,Thermochemical Cycles and Hess’s law
    • Hess's Law (The Law of Constant Heat Summation)
    • Heat of Formation and Bond Energies

Topic 4: Reaction Rates and Reversible Reactions - Form 4 Summarized Chemistry Notes

  • Reaction Rates
    • Measurements of Reaction Rates
    • Collision Theory and Activation Energy
    • Factors Affecting the Rate of Reaction
  • Reversible Reactions
    • Explanations of Reversible Reactions
    • Equilibrium
    • Le Chatelier's Principle
    • Summary: Optimum Conditions for Common Industrial Processes

Topic 5: Electrochemistry - Form 4 Summarized Chemistry Notes

  • Definition
  • Displacement and REDOX Reactions
    • Displacement Reactions among Metals
    • Oxidation and Reduction in Terms of Electron Loss and Gain
    • Summary: Strength of Reducing/Oxidizing Agent of metals
    • Summary on Displacement Reactions for metals
    • Oxidation Numbers/Oxidation State
    • Redox Reactions Involving Halide Ions and Halogens
    • Further Examples of Redox Reactions
    • Summary: Order of Oxidizing Power for Halogens
    • Terms Used in Describing Oxidation-reduction
    • The Tendency of Metals to Form Ions
    • Cell Diagram for a Voltaic Cell
  • Voltaic Cells
    • Types of Electrochemical Cell
  • Electrolysis
    • Definition of Electrolysis
    • Terminologies Used in Electrolysis
    • Electrolysis of Various Substances
    • Factors Affecting Electrolysis and Electrolytic Products
    • Applications of Electrolysis
    • Quantitative Aspects of Electrolysis

Topic 6: Metals: Extraction Properties and Uses - Form 4 Summarized Chemistry Notes

  • Introduction
  • Methods of Extraction
    • Preliminary Steps Before Extraction
  • Methods of Ore Concentration
  • The Metals
    • Sodium
    • Aluminium
    • Zinc
    • Iron
    • Copper
    • Lead

Topic 7: Radioactivity - Form 4 Summarized Chemistry Notes

  • Definitions
  • Types of Radiation from Radioactive Elements
    • Evidence for the Nature of Gamma Rays
    • Nature and Property of α, β, and γ
  • Radioactive Decay Curve
    • The Half Lives of Some Radioactive Isotopes
  • Radioactive Disintegration Equations
  • Application of Radioactivity/Using Radioactive Isotopes
  • Hazards of Radioactive Isotopes
  • Precautions

After you are done reading these summarized Chemistry notes, you can test yourself with our chemistry form 4 questions and answers, which you can access here.

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Download the Easy Elimu chemistry Notes Form 3. Get them in PDF format on the Easy Elimu Study App.

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Chemistry Form 1 Topical Revision Questions and Answers PDF

Chemistry Form 1 Topical Revision Questions and Answers PDF (5)

Get these free chemistry form 1 topical revision questions and answers for your exam preparation at national and local levels. These chemistry topical revision questions are compiled from the numerous high school KICD authorized textbooks including, KLB chemistry form 1, Finder chemistry textbook form 1, Mentors chemistry form 1, Spotlight chemistry form 1, Moran chemistry form 1, Pearsons chemistry form 1, etc. The topics covered by the topical revision questions for chemistry are shown below.

With the aid of these topical revision questions, you can review the following form 1 chemistry concepts:

  1. Introduction to Chemistry Questions and Answers - Chemistry Form 1 Topical Revision
  2. Simple Classification of Substances Questions and Answers - Chemistry Form 1 Topical Revision
  3.  Acids, Bases and Indicators Questions and Answers - Chemistry Form 1 Topical Revision
  4. Air and Combustion Questions and Answers - Chemistry Form 1 Topical Revision
  5. Water and Hydrogen Questions and Answers - Chemistry Form 1 Topical Revision

You can get the topical revision questions for free without having to pay a cent on our EasyElimu Study App, which you can get from the Google Playstore here.

As a bonus, if you need to brush up your knowledge on a topic, EasyElimu has summarized notes, so you won’t have to stress over writing that MwaKenya, which makes passing that summative chemistry form 1 term 3 exam easy. Whether it’s term 1, 2 or 3, these free chemistry form 1 topical revision questions can help you get an A

Easy Elimu is a chemistry revision questions and answers app. Though it contains all subjects not only chemistry.

For free access to the answers to the topical revision questions, visit the EasyElimu App.
Alternatively, you can download the individual topical revision questions and answers in PDF format from this page by clicking the blue download notes icon under each topic.

KCSE Chemistry Revision Questions and Answers PDF

Introduction to Chemistry Questions and Answers - Chemistry Form 1 Topical Revision

Get PDF with Answers here.

  1. Wooden splints F and G were placed in different zones of a Bunsen burner flame.
    The diagram below gives the observations that were made
     burnt wooden splints
    1. Explain the difference between F and G
    2. Name the type of flame that was used in the above experiment
  2. The diagrams below represent a list of apparatus which are commonly used in a chemistry laboratory:-
     lab apparatus
    1. Give the correct order of the apparatus, using the letters only, to show the correct arrangement that can be used to prepare and investigate the nature of PH of a sample of onion solution
    2. Name one chemical substance and apparatus that is needed in this experiment
  3.  
    1. When the air-hole is fully opened, the bunsen burner produces a non-luminous flame. Explain
    2. Draw a labelled diagram of a non-luminous flame
    1. What is a drug?
    2. Give two drugs that are commonly abused by the youth.
  5. The diagram below shows three methods for collecting gases in the laboratory
     downward delivery
    1. Name the methods A and B
    2. From the methods above, identify one that is suitable for collecting sulphur (IV) oxide. Explain
  6. A mixture of hexane and water was shaken and left to separate as shown in the diagram below:
     mixturesseparation
    State the identity of;
    (i) P ………………………………..…….. (ii) W ………………………………….….
  7. The diagrams below are some common laboratory apparatus. Name each apparatus and state its use
    Diagram  Name Use
     mortar (½mk )  (½mk)
     crucible (½mk) (½mk)
  8. The diagram below shows some parts of a Bunsen burner
     Bunsen Burner
    Explain how the parts labelled T and U are suited to their functions
  9. The diagram below shows the appearance of two pieces of paper placed in different parts of a non-luminous flame of a Bunsen burner and removed quickly before they caught fire.
     burnt pieces of paper
    1. What do the experiments show about the outer region of the flame?
    2. From the above experiment, which part of the flame is better to use for heating?Give a reason
  10. A crystal of copper (II) sulphate was placed in a beaker of water. The beaker was left standing for two days without shaking. State and explain the observations that were made.
  11. Study the information in the table below and answer questions that follow. (Letters given are not real symbols)
    Ions  Electron arrangement  Ionic radius (nm)
    A+
    B+
    C2+    		 2.8
    2.8.8
    2.8    		 0.95
    0.133
    0.065
    Explain why the ionic radius of :-
    1. B+ is greater than that of A+
    2. C2+ is smaller than the of A+

Simple Classification of Substances Questions and Answers - Chemistry Form 1 Topical Revision

Get PDF with Answers here.

  1. The diagram below shows the heating curve of a pure substance. Study it and answer the questions that follow:
     heating curve of pure substance
    1. What physical changes are taking place at points X and Z?
    2. Explain what happens to the melting point of sodium chloride added to this substance
    1. State two differences between luminous flame and non-luminous flame
    2. It is advisable to set a Bunsen burner to luminous flame prior to an experiment. Explain
  3. The paper chromatography of a plant extract gave the following results:
    Solvent  Number of spots
    X 6
    Y 2
    Z 3
    1. Which is the most suitable solvent for purifying the extract? Explain
    2. Ball pen cannot be used to mark solvent front in the above chromatography. Explain
  4. Name the process which takes place when:
    1. Solid Carbon (Iv) Oxide (dry ice) changes directly into gas
    2. A red litmus paper turns white when dropped into chlorine water
    3. Propene gas molecules are converted into a giant molecule
  5. A sample of copper turnings was found to be contaminated with copper (II) oxide. Describe how a sample of copper metal can be separated from the mixture
  6. Copper (II) oxide and charcoal are black solids. How would you distinguish between the two solids?
    1. What is chromatography?
    2. Give two applications of chromatography
  8. The two elements P and R were separately burned in air, the products gave the results recorded in the table below:
    ELEMENTS PHYSICAL STATE AT ROOM TEMPERATURE P SOLID R SOLID
    Physical states of products White solid powder only  Colourless gases L and M
    Nature of solutions in water Basic L strongly acidic M slightly acidic
    1. Suggest the identity of element R. ……………………………………………..……..
    2. Describe how the nature of the solutions of the of the oxides were determined
  9. The diagram below represents a paper chromatography for the three brands of soft drinks containing banned artificial food additives.
     chromatogram for food additives
    A and C found to contain the banned artificial food additives. Which numbers indicate the banned artificial food additives?
  10. Without using any laboratory chemical, describe a simple laboratory experiment to distinguish between calcium hydrogen carbonate and sodium hydrogen carbonate
  11. Substance Q has a melting point of 15oC and boiling point of 70oC.
    1. On the same axes, draw the melting point and boiling point graph for Q and the room temperature
       graph of temp against time
    2. State the physical state of substance Q at room temperature
  12. Cooking oils comprise of a mixture of compounds which have a boiling point range of 23oC to 27oC.
    1. What evidence is then to support the statement that cooking oil is a mixture?
    2. Name another experimental technique that could be used to confirm your answer in part (i) above
  13. A form 1 student carried out the separation as shown in the set-up below:-
     evaporation
    1. Identify the method above.................................................................................
    2. Give one of its disadvantages
    3. Name a mixture which can be separated by the set-up above
  14. What is meant by melting point and boiling point of a substance?
  15. The apparatus below were used by a student to study the effect of heat on hydrated copper II sulphate
     effect of heat on copper sulphate
    1. What is the role of the ice cold water
    2. Name liquid P
    3. What observation is made in the boiling tube
  16. The diagram below shows chromatograms of blood samples obtained from three athletes. One athlete used illegal drug to improve performance in competition.
     chromatogram of blood samples
    1. Name the line marked M ………………………………………………….
    2. Identify the athlete who used illegal drug ……………... ……………………….
  17. Classify the following processes as chemical changes or physical change
    Process physical or chemical
    Neutralization ………………………………………
    Sublimation ………………………………………
    Fractional distillation ………………………………………..
    Displacement reaction …………………………………………
  18. Give two reasons why a luminous flame is not used for heating purposes
  19. State two criteria for determining the purity of a substance
  20. Study the information in the table below and answer the questions.
    A mixture contains ethene, Hydrogen and ammonia gases. Explain how a sample of hydrogen gas can be obtained from this mixture.
      1. The diagram below show spots of a pure substance A, B, and C on a chromatography paper. Spot D is that of a mixture
         spots of pure substances
        After development A, B, and C were found to have moved 8cm, 3cm and 6cm respectively. D had separated into two spots which had moved 6cm and 8cm
        On the diagram above;
        1. Label the baseline (origin)
        2. Show the positions of all the spots after development
      2. Identify the substances present in mixture D
    2. Describe how solid ammonium chloride can be separated from a solid mixture of ammonium chloride and anhydrous calcium chloride
    3. The table below shows liquids that are miscible and those that are immiscible
      Liquid  L3 L4
      L1 Miscible  Miscible
      L2 Miscible  Immiscible
      Use the information given in the table to answer that questions that follow;
      1. Name the method that can be used to separate L1 and L2 from a mixture of the two
      2. Describe how a mixture of L2 and L4 can be separated
  22. A student left some crushed fruit mixture with water for some days. He found the mixture had fermented. He concluded that the mixture was contaminated with water and ethanol with boiling point of 100oC and 78oC respectively. The set-up of apparatus below are used to separate the mixture.
     fractional distillation
    1. Name the piece of apparatus labelled W
    2. What is the purpose of the thermometer in the set-up?
    3. At which end of the apparatus W should tap water be connected?……………………………
    4. Which liquid was collected as the first distillate? Explain
    5. What is the name given to the above method of separating mixture?
    6. State two applications of the above method of separating mixtures
    7. What properties of the mixture makes it possible for the component to be separated by the above methods?
  23. The set-up below was used to separate a mixture:-
     evaporation method
    1. Name the apparatus missing in the set-up
    2. Give one example of mixture T
    3. What is the name of this method of separation

    1. The diagram below shows a set – up used by a student to find out what happens when Copper (II) sulphate crystals are heated.
       heating copperIIsulphate
      1. State the observations made when the blue copper (II) sulphate crystals are heated.
      2. Identify liquid Y and write an equation for its formation.
    2. Pellets of sodium hydrogen and anhydrous Copper (II) sulphate were put in separate Petridishes and left in the open for two hours. Explain the observation in each Petri-dish.
  25. The chromatography below shows the constituents of a flower extract using an organic solvent:-
     constituents of a flower chromatogram
    1.   
      1. Name a possible organic solvent you can use for this experiment
      2.  State one property that makes the red pigment to move the furthest distance from M
      3. Describe how one could get a sample of yellow pigment
      4. On the diagram indicate solvent front
    2. Describe how Aluminium chloride can be separated from a mixture of aluminium chloride and sodium chloride
  26. Study the information below and answer the questions that follow:
    Solid Cold water Hot water
    R Soluble Soluble
    V Insoluble Insoluble
    S Insoluble Insoluble
    Describe how the mixture of solid R, S, and V can be separated
  27. Given a mixture of lead (II) oxide, ammonium chloride and sodium chloride, describe how this mixture can be separated to obtain a sample of each.
  28. The setup below was used to separate two miscible liquids Q and T (Boling points; Q =98° C, T=78°C)
     fractional distillation method
    1. Identify the mistakes in the setup above
    2. Identify Distillate X
  29. Name the process which takes place when:
    1. Solid Carbon (IV) oxide (dry ice) changes directly into gas.
    2. A red litmus paper turns white when dropped into chlorine water.
    3. Propene gas molecules are converted into a giant molecule.
  30. The following diagram shows a paper chromatogram of substances A, B, C, and D which are coloured
     paper chromatogram of coloured substances
    1. Indicate the solvent front on the chromatogram
    2. Which substance is pure? ………………………………………..
    3. Substance E is a mixture of C and D. Indicate its chromatogram in the diagram
  31. Study the information below and answer the following questions. A mixture contains three solids A, B, and C. The solubility of these solids in different liquids is as shown below:- 
    Solid  Water Alcohol Ether
    A Soluble Insoluble  Insoluble
    B Insoluble  Soluble Very soluble
    C Soluble Soluble Insoluble
    Explain how you will obtain sample C from the mixture
  32. State and explain the observations made when iodine crystals is heated in a boiling tube?

Acids, Bases and Indicators Questions and Answers - Chemistry Form 1 Topical Revision

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  1. The table below shows solutions A, B and C are tested and observations records as shown:
    Solution  Observations on indicator
    A Methyl orange turns yellow
    B Phenolphthalein turns colourless
    C Litmus turns purple
    1. Using the table above, name an acid
    2. How does the pH value of 1M potassium hydroxide solution compare with that of 1M aqueous ammonia? Explain
  2. The information below gives PH values of solutions V, W, X, Y, Z
    Solution  PH values
    V
    W
    X
    Y
    Z    		 2
    6.5
    11
    14
    4.5
    1. Which solution is likely to be:
      1. Calcium hydroxide? 
      2. Rain water?
    2. Which solution would react most vigorously with Zinc carbonate
  3.  
    1. Complete the table below to show the colour of the given indicator in acidic and basic solutions.
      Indicator Colour in
      Methyl Orange Acidic Solution Basic Solution
         
      Phenolphthalein  Colourless  
    2. How does the PH value of 0.1M potassium hydroxide solution compare with that of 0.1M aqueous ammonia? Explain.
  4. Use the information given below to answer the questions that follow:
    Solution  G H I J K
    pH 1.5  6.5  13.0  7.0  8.0
    1. Which of the solutions would be used to relieve a stomach upset caused by indigestion?
    2. Which solution is likely to be:
      1. Dilute sulphuric acid?
      2. Sodium hydroxide solution?
  5. Solid copper (II) oxide is a base although it does not turn litmus paper to blue. Explain
  6. Below are the pH values of 4 types of medicine represented by letters P, Q, R and S
    MEDICINE pH VALUES
    P
    Q
    R
    S    		 7.0
    5.0
    8.0
    6.0
    1. It is not advisable to use S when a patient has indigestion .Explain
    2. What is the role of chemistry in drug manufacture
  7. Explain why very little Carbon (IV) oxide gas is evolved when dilute sulphuric (VI) acid is added to lead (II) carbonate
  8. State one commercial use of Calcium Oxide
  9. The following data gives the pH values of some solutions
    Solution  pH
    P
    Q
    R    		 14.0
    6.8
    2.5
    1. What colour change would occur in solution P on addition of two drops of phenolphthalein indicator?
    2. State the pH value of a resulting solution when equal moles of solution P and R react
  10. In an experiment, ammonia gas was prepared by heating ammonium salt with an alkali.
    After drying, ammonia gas was collected at room temperature and pressure.
    1. What is meant by the term alkali?
    2. Explain using physical properties of the gas why ammonia is not collected by downward delivery
  11. The table shows the colours obtained when some indicators are added to solutions:-
    Solution Blue litmus paper  Indicator W
    Distilled water ………………….. Colourless
    Calcium hydroxide  Blue Pink
    Nitric acid ………………………… Colourless
    1. Complete the table by filling in the missing colours
    2. Identify indicator W
    1. Flower extracts can be used as Acid-base indicators. Give two limitations of such indicators
    2. The diagram below shows spots of pure substances W, X, and Y on a chromatography paper. Spot Z is that of a mixture
       chromatogram of pure substance
      After development W, X, and Y were found to have moved 9cm3, 4cm3 and 7cm3 respectively. Z has separated into two spots which have moved 7cm3 and 9cm3:-
      On the diagram:-
      1. Label the baseline and solvent front
      2. Show the position of all the spots after development
      3. Identify the substances present in mixture Z
  13. A beekeeper found that when stung by a bee, application of a little solution of sodium hydrogen carbonate helped to relieve the irritation of the affected area. Explain
  14. 10g of sodium hydrogen carbonate were dissolved in 20cm3 of water in a boiling tube. Lemon juice was then added dropwise with shaking until there was no further change.
    1. Explain the observation which was made in the boiling tube when the reaction was in progress
    2. What observations would be made if the lemon juice had been added to copper turnings in a boiling tube?
  15. Complete the table below to show the colour of the given indicator in acidic and basic solutions:
    Indicator Colour in acidic solution Basic Solution
    Methyl orange Pink  
    Phenolphthalein   Pink
  16. Solutions can be classified as acids, bases or neutral. The table below shows solutions and their pH values:-
     Solutions  pH Values
     K  1.5
     L  7.0
     M  14.0
    1. Select any pair that would react to form a solution of PH 7
    2. Identify two solutions that would react with aluminium hydroxide. Explain

Air and Combustion Questions and Answers - Chemistry Form 1 Topical Revision

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  1. The set-up below was used to prepare a sample of oxygen gas. Study it and answer the questions that follow.
    1. Complete the diagram to show how Oxygen can be collected
       preparation of oxygen from hydrogen peroxide
    2. Write a chemical equation of the reaction to produce oxygen
  2. Air was passed through several reagents as shown below:
     purification of air
    1. Write an equation for the reaction which takes place in the chamber containing magnesium powder
    2. Name one gas which escapes from the chamber containing magnesium powder. Give a reason for your answer

    1. What is rust?
    2. Give two methods that can be used to prevent rusting
    3. Name one substance which speeds up the rusting process
  4. 3.0g of clean magnesium ribbon 8.0g of clean copper metal were burnt separately in equal volume of air and both metals reacted completely with air;
    1. State and explain where there was greater change in volume of air Mg =24 Cu = 64
    2. Write an equation for the reaction between dilute sulphuric acid and product of burnt copper
  5. Oxygen is obtained on large scale by the fractional distillation of air as shown on the flow chart below.
     fractional distillation of air
    1. Identify the substance that is removed at the filtration stage
    2. Explain why Carbon (IV) oxide and water are removed before liquefaction of air
    3. Identify the component that is collected at -186°C
  6. The set-up below was used to study some properties of air. 
     properties of air diagram
    State and explain two observations that would be made at the end of the experiment
  7. A form two student in an attempt to stop rusting put copper and Zinc in contact with iron as shown:-
     copper and zinc
    1. State whether rusting occurred after one week if the set-ups were left out
    2. Explain your answer in (a) above
  8. In an experiment, a piece of magnesium ribbon was cleaned with steel wool. 2.4g of the clean magnesium ribbon was placed in a crucible and completely burnt in oxygen. After cooling the product weighed 4.0g
    1. Explain why it is necessary to clean magnesium ribbon
    2. What observation was made in the crucible after burning magnesium ribbon?
    3. Why was there an increase in mass?
    4. Write an equation for the major chemical reaction which took place in the crucible
    5. The product in the crucible was shaken with water and filtered. State and explain the observation which was made when red and blue litmus paper were dropped into the filtrate
  9. In an experiment a gas jar containing some damp iron fillings was inverted in a water trough containing some water as shown in the diagram below. The set-up was left un-disturbed for three days. Study it and answer the questions that follow:
     rusting experiment
    1. Why were the iron filings moistened?
    2. State and explain the observation made after three days.
    3. State two conclusions made from the experiment.
    4. Draw a labelled set-up of apparatus for the laboratory preparation of oxygen using sodium Peroxide
    5. State two uses of oxygen
  10. The set-up below was used to collect gas F produced by the reaction between sodium peroxide and water
     prepartion of oxygen from sodium peroxide
    1. Name gas F……………………………………………………………………………
    2. At the end of the experiment, the solution in the round bottomed flask was found to be a strong base. Explain why this was so
    3. Which property of gas F makes it be collected by the method used in the set-up?
    4. Give one industrial use of gas F
  11. The set-up below was used to investigate properties of the components of air:
     componennts of air experiment
    1. State two observations made during the experiment
    2. Write two chemical equations for the reactions which occurred
    3. The experiment was repeated using burning magnesium in place of phosphorous.
      There was greater rise of water than in the first case. Explain this observation
    4. After the two experiments, the water in each trough was tested using blue and red litmus papers. State and explain the observations of each case.
      1.  Phosphorous experiment
      2. magnesium experiment
    5. Briefly explain how a sample of nitrogen gas can be isolated from air in the laboratory
  12. A group of students burnt a piece of Mg ribbon in air and its ash collected in a Petri dish. The ash was found to comprise of magnesium Oxide and Magnesium nitride
    1. Write an equation for the reaction leading to formation of the magnesium nitride
    2. A little water was added to the products in the Petri dish. State and explain the observation made.
    3. A piece of blue litmus paper was dipped into the solution formed in (b) above. 
      State the observation made.
  13. A form one class carried out an experiment to determine the active part of air. The diagram below shows the set-up of the experiment and also the observation made.
     active part of air experiment
      1. Identify substance M ...........................

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Chemistry Form 2 Topical Revision Questions and Answers

Chemistry Form 2 Topical Revision Questions and Answers (6)

Get these free chemistry form 2 topical revision questions and answers for your exam preparation at national and local levels.

These chemistry topical revision questions are compiled from the numerous high school KICD authorized textbooks including, KLB chemistry form 2, Finder chemistry textbook form 2, Mentors chemistry form 2, Spotlight chemistry form 2, Moran chemistry form 2, Pearsons chemistry form 2, etc.

All chemistry form 2 topics are covered by these EasyElimu topical revision questions.

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Chemistry Form 3 Topical Revision Questions and Answers

Chemistry Form 3 Topical Revision Questions and Answers (6)

This category contains chemistry topic by topic revision questions and answers for form 3 for the preparation of local and KCSE exams.

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Chemistry Form 4 Topical Revision Questions and Answers

Chemistry Form 4 Topical Revision Questions and Answers (7)

This category contains chemistry topic by topic revision questions and answers for form 4 for the preparation of local and KCSE exams.

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