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Cambridge OLevel Chemistry Crash Course

Welcome to our Cambridge OLevel Chemistry Crash Course! Are you ready to ace your chemistry exam with flying colors? Look no further! Our intensive crash course is tailor-made to equip you with everything you need to succeed. Led by experienced educators, our course is designed to simplify complex chemistry concepts and make learning engaging and effective.

Why Choose Our Course:

Comprehensive Learning: Our crash course covers all the essential topics from the Cambridge O-Level Chemistry syllabus. From atoms and molecules to chemical reactions and beyond, we’ve got you covered.
Expert Guidance: Learn from experienced instructors who are passionate about chemistry and dedicated to helping you succeed. Our teachers break down difficult concepts into easy-to-understand explanations, ensuring you grasp every concept with ease.
Interactive Classes: Engage in dynamic lessons that bring chemistry to life! Our crash course includes interactive activities, demonstrations, and experiments to make learning fun and memorable.
Practical Practice: Reinforce your learning with plenty of practice exercises and hands-on experiments. Our crash course includes regular quizzes and tests to help you track your progress and identify areas for improvement.
Flexible Schedule: We understand that you have a busy schedule, which is why our crash course offers flexible scheduling options. Whether you prefer weekday or weekend classes, we’ve got you covered.
Convenient Location: Our institute is conveniently located, making it easy for you to attend classes without any hassle. With our comfortable and conducive learning environment, you can focus on your studies and excel in chemistry.

Course Structure:

Our Cambridge O-Level Chemistry Crash Course is designed to make learning easy and effective. Here’s an overview of what to expect:

Duration: The crash course spans [4 weeks/months], with classes held [3 times] per week.
Content Coverage: We cover all topics included in the Cambridge O-Level Chemistry syllabus, focusing on core concepts and exam-specific strategies.
Class Format: Each class combines simple explanations with practical examples, ensuring you understand every concept thoroughly.
Assessments: Throughout the course, you’ll have the opportunity to complete quizzes, tests, and mock exams to assess your progress and readiness for the real exam.

Enroll Now:

Don’t let the fear of chemistry hold you back! Enroll in our Cambridge O-Level Chemistry Crash Course today and take the first step towards exam success. For inquiries and enrollment, contact us at [email protected] or call us at +8801327331903. Let us help you unlock your potential and achieve your goals in chemistry!

Fundamental principles of Chemistry
Periodic table and elements
Chemical reactions and equations
Acids, bases, and salts
Organic chemistry
Inorganic chemistry
Physical chemistry
Laboratory skills and safety
Problem-solving techniques
Real-world applications of Chemistry
Exam preparation strategies
Self-learning skills and research abilities

Course Content

Introduction

Introduction

10:00

Chapter-1. The particulate nature of matter.
• State the distinguishing properties of solids, liquids and gases • Describe the structure of solids, liquids and gases in terms of particle separation, arrangement and types of motion • Describe changes of state in terms of melting, boiling, evaporation, freezing, condensation and sublimation • Describe qualitatively the pressure and temperature of a gas in terms of the motion of its particles • Show an understanding of the random motion of particles in a suspension (sometimes known as Brownian motion) as evidence for the kinetic particle (atoms, molecules or ions) model of matter • Describe and explain diffusion

Assignments-1.1
Lesson-1.1.5- Show an understanding of the random motion of particles in a suspension (sometimes known as Brownian motion) as evidence for the kinetic particle (atoms, molecules or ions) model of matter. Describe and explain diffusion.

40:00
Lesson-1.1.4- Describe qualitatively the pressure and temperature of a gas in terms of the motion of its particles.

40:00
Lesson-1.1.3- Describe changes of state in terms of melting, boiling, evaporation, freezing, condensation and sublimation.

40:00
Lesson-1.1.2- Describe the structure of solids, liquids and gases in terms of particle separation, arrangement and types of motion.

40:00
Lesson-1.1.1- State the distinguishing properties of solids, liquids and gases.

40:00
Quiz-1.1

Chapter-2. Experimental techniques.
• Name appropriate apparatus for the measurement of time, temperature, mass and volume, including burettes, pipettes and measuring cylinders • Demonstrate knowledge and understanding of paper chromatography • Interpret simple chromatograms • Identify substances and assess their purity from melting point and boiling point information • Understand the importance of purity in substances in everyday life, e.g. foodstuffs and drugs • Describe and explain methods of purification by the use of a suitable solvent, filtration, crystallisation and distillation (including use of a fractionating column). (Refer to the fractional distillation of petroleum in section 14.2 and products of fermentation in section 14.6.) • Suggest suitable purification techniques, given information about the substances involved

Assignments-2.1
Lesson-2.1.6- Suggest suitable purification techniques, given information about the substances involved.

40:00
Lesson-2.1.5- Describe and explain methods of purification by the use of a suitable solvent, filtration, crystallisation and distillation (including use of a fractionating column).

40:00
Lesson-2.1.4- Understand the importance of purity in substances in everyday life, e.g. foodstuffs and drugs.

40:00
Lesson-2.1.3- Identify substances and assess their purity from melting point and boiling point information.

40:00
Lesson-2.1.2- Demonstrate knowledge and understanding of paper chromatography • Interpret simple chromatograms.

40:00
Lesson-2.1.1- Name appropriate apparatus for the measurement of time, temperature, mass and volume, including burettes, pipettes and measuring cylinders.

40:00
Quiz-2.1

Chapter-3. Atoms, elements and compounds.
• State the relative charges and approximate relative masses of protons, neutrons and electrons • Define proton number (atomic number) as the number of protons in the nucleus of an atom • Define nucleon number (mass number) as the total number of protons and neutrons in the nucleus of an atom • Use proton number and the simple structure of atoms to explain the basis of the Periodic Table (see section 9), with special reference to the elements of proton number 1 to 20 • Define isotopes as atoms of the same element which have the same proton number but a different nucleon number • State the two types of isotopes as being radioactive and non-radioactive • State one medical and one industrial use of radioactive isotopes • Describe the build-up of electrons in ‘shells’ and understand the significance of the noble gas electronic structures and of the outer shell electrons. (The ideas of the distribution of electrons in s and p orbitals and in d block elements are not required.) • Describe the differences between elements, mixtures and compounds, and between metals and non-metals • Describe an alloy, such as brass, as a mixture of a metal with other elements • Describe the formation of ions by electron loss or gain • Describe the formation of ionic bonds between elements from Groups I and VII • Describe the formation of single covalent bonds in H 2, Cl2, H2O, CH4, NH3 and HCl as the sharing of pairs of electrons leading to the noble gas configuration • Describe the differences in volatility, solubility and electrical conductivity between ionic and covalent compounds • Describe the giant covalent structures of graphite and diamond • Relate their structures to their uses, e.g. graphite as a lubricant and a conductor, and diamond in cutting tools • Describe metallic bonding as a lattice of positive ions in a ‘sea of electrons’ and use this to describe the electrical conductivity and malleability of metals

Assignments-3.1
Lesson-3.1.13- Describe metallic bonding as a lattice of positive ions in a ‘sea of electrons’ and use this to describe the electrical conductivity and malleability of metals.

40:00
Lesson-3.1.12- Describe the differences in volatility, solubility and electrical conductivity between ionic and covalent compounds.

40:00
Lesson-3.1.11- Describe the differences in volatility, solubility and electrical conductivity between ionic and covalent compounds.

40:00
Lesson-3.1.10- Describe the formation of single covalent bonds in H 2, Cl2, H2O, CH4, NH3 and HCl as the sharing of pairs of electrons leading to the noble gas configuration.

40:00
Lesson-3.1.9- Describe the formation of ions by electron loss or gain • Describe the formation of ionic bonds between elements from Groups I and VII.

40:00
Lesson-3.1.8- Describe the differences between elements, mixtures and compounds, and between metals and non-metals • Describe an alloy, such as brass, as a mixture of a metal with other elements.

40:00
Lesson-3.1.7- Describe the build-up of electrons in ‘shells’ and understand the significance of the noble gas electronic structures and of the outer shell electrons. (The ideas of the distribution of electrons in s and p orbitals and in d block elements are not required.)

40:00
Lesson-3.1.6- State the two types of isotopes as being radioactive and non-radioactive. State one medical and one industrial use of radioactive isotopes.

40:00
Lesson-3.1.5- Define isotopes as atoms of the same element which have the same proton number but a different nucleon number.

40:00
Lesson-3.1.4- Use proton number and the simple structure of atoms to explain the basis of the Periodic Table, with special reference to the elements of proton number 1 to 20.

40:00
Lesson-3.1.3- Define nucleon number (mass number) as the total number of protons and neutrons in the nucleus of an atom.

40:00
Lesson-3.1.2- Define proton number (atomic number) as the number of protons in the nucleus of an atom.

40:00
Lesson-3.1.1- State the relative charges and approximate relative masses of protons, neutrons and electrons.

40:00
Quiz-3.1

Chapter-4. Stoichiometry.
• Use the symbols of the elements and write the formulae of simple compounds • Deduce the formula of a simple compound from the relative numbers of atoms present • Deduce the formula of a simple compound from a model or a diagrammatic representation • Construct word equations and simple balanced chemical equations • Define relative atomic mass, A r, as the average mass of naturally occurring atoms of an element on a scale where the 12C atom has a mass of exactly 12 units • Define relative molecular mass, M r, as the sum of the relative atomic masses. (Relative formula mass or M r will be used for ionic compounds.) (Calculations involving reacting masses in simple proportions may be set. Calculations will not involve the mole concept.) • Define the mole and the Avogadro constant • Use the molar gas volume, taken as 24 dm3 at room temperature and pressure • Calculate stoichiometric reacting masses, volumes of gases and solutions, and concentrations of solutions expressed in g / dm3 and mol / dm3. (Calculations involving the idea of limiting reactants may be set. Questions on the gas laws and the conversion of gaseous volumes to different temperatures and pressures will not be set.) • Calculate empirical formulae and molecular formulae • Calculate percentage yield and percentage purity

Assignments-4.1
Lesson-4.1.7- Calculate empirical formulae and molecular formulae • Calculate percentage yield and percentage purity.

40:00
Lesson-4.1.6- Calculate stoichiometric reacting masses, volumes of gases and solutions, and concentrations of solutions expressed in g / dm3 and mol / dm3. (Calculations involving the idea of limiting reactants may be set. Questions on the gas laws and the conversion of gaseous volumes to different temperatures and pressures will not be set.)

40:00
Lesson-4.1.5- Define the mole and the Avogadro constant • Use the molar gas volume, taken as 24 dm3 at room temperature and pressure.

40:00
Lesson-4.1.4- Define relative molecular mass, M r, as the sum of the relative atomic masses. (Relative formula mass or M r will be used for ionic compounds.).

40:00
Lesson-4.1.3- Define relative atomic mass, A r, as the average mass of naturally occurring atoms of an element on a scale where the 12C atom has a mass of exactly 12 units.

40:00
Lesson-4.1.2- Deduce the formula of a simple compound from a model or a diagrammatic representation • Construct word equations and simple balanced chemical equations.

40:00
Lesson-4.1.1- Use the symbols of the elements and write the formulae of simple compounds • Deduce the formula of a simple compound from the relative numbers of atoms present.

40:00
Quiz-4.1

Chapter-5. Electricity and chemistry.
• Define electrolysis as the breakdown of an ionic compound, molten or in aqueous solution, by the passage of electricity • Describe the electrode products and the observations made during the electrolysis of: – molten lead(II) bromide – concentrated hydrochloric acid – concentrated aqueous sodium chloride – dilute sulfuric acid between inert electrodes (platinum or carbon) • State the general principle that metals or hydrogen are formed at the negative electrode (cathode), and that non-metals (other than hydrogen) are formed at the positive electrode (anode) • Predict the products of the electrolysis of a specified binary compound in the molten state • Describe the electroplating of metals • Outline the uses of electroplating • Describe the transfer of charge during electrolysis to include: – the movement of electrons in the metallic conductor – the removal or addition of electrons from the external circuit at the electrodes – the movement of ions in the electrolyte • Describe the production of electrical energy from simple cells, i.e. two electrodes in an electrolyte. (This should be linked with the reactivity series in section 10.2 and redox in section 7.4.) • Describe, in outline, the manufacture of: – aluminium from pure aluminium oxide in molten cryolite (refer to section 10.3) – chlorine, hydrogen and sodium hydroxide from concentrated aqueous sodium chloride (Starting materials and essential conditions should be given but not technical details or diagrams.)

Assignments-5.1
Lesson-5.1.9- Describe, in outline, the manufacture of: – aluminium from pure aluminium oxide in molten cryolite – chlorine, hydrogen and sodium hydroxide from concentrated aqueous sodium chloride.

40:00
Lesson-5.1.8- Describe the production of electrical energy from simple cells, i.e. two electrodes in an electrolyte.

40:00
Lesson-5.1.7- Describe the transfer of charge during electrolysis to include: – the movement of electrons in the metallic conductor – the removal or addition of electrons from the external circuit at the electrodes – the movement of ions in the electrolyte.

40:00
Lesson-5.1.6- Describe the electroplating of metals • Outline the uses of electroplating.

40:00
Lesson-5.1.5- Predict the products of the electrolysis of a specified binary compound in the molten state.

40:00
Lesson-5.1.4- State the general principle that metals or hydrogen are formed at the negative electrode (cathode), and that non-metals (other than hydrogen) are formed at the positive electrode (anode).

40:00
Lesson-5.1.3- Describe the electrode products and the observations made during the electrolysis of: – concentrated aqueous sodium chloride – dilute sulfuric acid.

40:00
Lesson-5.1.2- Describe the electrode products and the observations made during the electrolysis of: – molten lead(II) bromide – concentrated hydrochloric acid.

40:00
Lesson-5.1.1- Define electrolysis as the breakdown of an ionic compound, molten or in aqueous solution, by the passage of electricity.

40:00
Quiz-5.1

Chapter-6. Chemical energetics
• Describe the meaning of exothermic and endothermic reactions • Interpret energy level diagrams showing exothermic and endothermic reactions • Describe the release of heat energy by burning fuels • State the use of hydrogen as a fuel • Describe radioactive isotopes, such as 235U, as a source of energy

Chapter-7. Chemical reactions.
• Identify physical and chemical changes, and understand the differences between them • Describe and explain the effect of concentration, particle size, catalysts (including enzymes) and temperature on the rate of reactions • Describe the application of the above factors to the danger of explosive combustion with fine powders (e.g. flour mills) and gases (e.g. methane in mines) • Demonstrate knowledge and understanding of a practical method for investigating the rate of a reaction involving gas evolution • Interpret data obtained from experiments concerned with rate of reaction Understand that some chemical reactions can be reversed by changing the reaction conditions. (Limited to the effects of heat and water on hydrated and anhydrous copper(II) sulfate and cobalt(II) chloride.) (Concept of equilibrium is not required.) Define oxidation and reduction in terms of oxygen loss/gain. (Oxidation state limited to its use to name ions, e.g. iron(II), iron(III), copper(II), manganate(VII).)

Assignments-7.1
Lesson-7.1.9- Identify oxidising agents and reducing agents from simple equations.

40:00
Lesson-7.1.8- Define oxidising agent as a substance which oxidises another substance during a redox reaction. Define reducing agent as a substance which reduces another substance during a redox reaction.

40:00
Lesson-7.1.7- Define redox in terms of electron transfer • Identify redox reactions by changes in oxidation state and by the colour changes involved when using acidified potassium manganate(VII), and potassium iodide. (Recall of equations involving KMnO 4 is not required.).

40:00
Lesson-7.1.6- Understand that some chemical reactions can be reversed by changing the reaction conditions. (Limited to the effects of heat and water on hydrated and anhydrous copper(II) sulfate and cobalt(II) chloride.) (Concept of equilibrium is not required.).

40:00
Lesson-7.1.5- Interpret data obtained from experiments concerned with rate of reaction.

40:00
Lesson-7.1.4- Demonstrate knowledge and understanding of a practical method for investigating the rate of a reaction involving gas evolution.

40:00
Lesson-7.1.3- Describe the application of the above factors to the danger of explosive combustion with fine powders (e.g. flour mills) and gases (e.g. methane in mines).

40:00
Lesson-7.1.2- Describe and explain the effect of concentration, particle size, catalysts (including enzymes) and temperature on the rate of reactions.

40:00
Lesson-7.1.1- Identify physical and chemical changes, and understand the differences between them.

40:00
Quiz-7.1

Chapter-8. Acids, Bases, Salts

Lesson-8.1.1- Describe the characteristic properties of acids as reactions with metals, bases, carbonates and effect on litmus and methyl orange.

00:00
Lesson-8.1.2- Describe the characteristic properties of bases as reactions with acids and with ammonium salts and effect on litmus and methyl orange.

00:00
Lesson-8.1.3-Describe neutrality and relative acidity and alkalinity in terms of pH measured using universal indicator paper (whole numbers only).

00:00
Lesson-8.1.4- Describe and explain the importance of controlling acidity in soil.

00:00
Lesson-8.1.5- Classify oxides as either acidic or basic, related to metallic and non-metallic character.

00:00
Lesson-8.1.6- Demonstrate knowledge and understanding of preparation, separation and purification of salts.

00:00
Lesson-8.1.7- Describe the following tests to identify: aqueous cations: aluminum, ammonium, calcium, chromium(III), copper(II), iron(II), iron(III) and zinc (using aqueous sodium hydroxide and aqueous ammonia as appropriate).

00:00
Assignments-8.1
Quiz-8.1

Chapter-9. The Periodic Table

Lesson-9.1.1- Describe the Periodic Table as a method of classifying elements and its use to predict properties of elements.

00:00
Lesson-9.1.2- Describe and explain the relationship between Group number, number of outer shell electrons and metallic/non-metallic character.

00:00
Lesson-9.1.3- Describe lithium, sodium and potassium in Group I as a collection of relatively soft metals showing a trend in melting point, density and reaction with water.

00:00
Lesson-9.1.4- Predict the properties of other elements in Group I, given data, where appropriate.

00:00
Lesson-9.1.5- Describe the halogens, chlorine, bromine and iodine in Group VII, as a collection of diatomic non-metals showing a trend in colour and density and state their reaction with other halide ions.

00:00
Lesson-9.1.6- Predict the properties of other elements in Group VII, given data where appropriate.

00:00
Lesson-9.1.7- Describe the transition elements as a collection of metals having high densities, high melting points and forming coloured compounds, and which, as elements and compounds, often act as catalysts.

00:00
Lesson-9.1.8- Describe the noble gases, in Group VIII or 0, as being unreactive, monoatomic gases and explain this in terms of electronic structure.

00:00
Lesson-9.1.9- State the uses of the noble gases in providing an inert atmosphere, i.e. argon in lamps, helium for filling balloons.

00:00
Assignments-9.1
Quiz-9.1

Chapter-10. Metals

Lesson-10.1.1- List the general physical properties of metals • Describe the general chemical properties of metals, e.g. reaction with dilute acids and reaction with oxygen.

00:00
Lesson-10.1.2- Explain in terms of their properties why alloys are used instead of pure metals.

00:00
Lesson-10.1.3- Identify representations of alloys from diagrams of structure.

00:00
Lesson-10.1.4- Place in order of reactivity: potassium, sodium, calcium, magnesium, zinc, iron, (hydrogen) and copper, by reference to the reactions, if any, of the metals with: – water or steam.

00:00
Lesson-10.1.5- Place in order of reactivity: potassium, sodium, calcium, magnesium, zinc, iron, (hydrogen) and copper, by reference to the reactions, if any, of the metals with: – dilute hydrochloric acid and the reduction of their oxides with carbon.

00:00
Lesson-10.1.6- Deduce an order of reactivity from a given set of experimental results.

00:00
Lesson-10.1.7- Describe the ease in obtaining metals from their ores by relating the elements to the reactivity series.

00:00
Lesson-10.1.8- Describe and state the essential reactions in the extraction of iron from hematite.

00:00
Lesson-10.1.9- Describe the conversion of iron into steel using basic oxides and oxygen.

00:00
Lesson-10.1.10- Know that aluminum is extracted from the ore bauxite by electrolysis.

00:00
Lesson-10.1.11- Discuss the advantages and disadvantages of recycling metals, limited to iron/steel and aluminum.

00:00
Lesson-10.1.12- Name the uses of aluminum: – in the manufacture of aircraft because of its strength and low density – in food containers because of its resistance to corrosion.

00:00
Lesson-10.1.13- Name the uses of copper related to its properties (electrical wiring and in cooking utensils).

00:00
Lesson-10.1.14- Name the uses of mild steel (car bodies and machinery) and stainless steel (chemical plant and cutlery).

00:00
Assignments-10.1
Quiz-10.1

Chapter-11. Air and Water

Lesson-11.1.1- Name the uses of mild steel (car bodies and machinery) and stainless steel (chemical plant and cutlery).

00:00
Lesson-11.1.2- Describe, in outline, the treatment of the water supply in terms of filtration and chlorination.

00:00
Lesson-11.1.3- Name some of the uses of water in industry and in the home.

00:00
Lesson-11.1.4- State the composition of clean, dry air as being approximately 78% nitrogen, 21% oxygen and the remainder as being a mixture of noble gases and carbon dioxide.

00:00
Lesson-11.1.5- Name the common pollutants in the air as being carbon monoxide, sulfur dioxide, oxides of nitrogen and lead compounds.

00:00
Lesson-11.1.6- Name the common pollutants in the air as being carbon monoxide, sulfur dioxide, oxides of nitrogen and lead compounds.

00:00
Lesson-11.1.7- State the source of each of these pollutants: – carbon monoxide from the incomplete combustion of carbon-containing substances – sulfur dioxide from the combustion of fossil fuels which contain sulfur compounds (leading to ‘acid rain’).

00:00
Lesson-11.1.8- State the source of each of these pollutants: – oxides of nitrogen from car engines – lead compounds from leaded petrol.

00:00
Lesson-11.1.9- State the adverse effect of these common pollutants on buildings and on health and discuss why these pollutants are of global concern.

00:00
Lesson-11.1.10- State the conditions required for the rusting of iron • Describe and explain methods of rust prevention, specifically paint and other coatings to exclude oxygen.

00:00
Lesson-11.1.11- Describe the need for nitrogen-, phosphorus- and potassium-containing fertilizers • Describe the displacement of ammonia from its salts.

00:00
Lesson-11.1.12- State that carbon dioxide and methane are greenhouse gases and explain how they may contribute to climate change.

00:00
Lesson-11.1.13- State the formation of carbon dioxide: – as a product of complete combustion of carbon-containing substances – as a product of respiration.

00:00
Lesson-11.1.14- State the formation of carbon dioxide: – as a product of the reaction between an acid and a carbonate – from the thermal decomposition of a carbonate.

00:00
Lesson-11.1.15- State the sources of methane, including decomposition of vegetation and waste gases from digestion in animals.

00:00
Assignments-11.1
Quiz-11.1

Chapter-12. Sulfur

Chapter-13. Corbonates

Chapter-14. Organic Chemistry

Lesson-14.1.1- Name and draw the structures of methane, ethane, ethene, ethanol, ethanoic acid and the products of the reactions.

00:00
Lesson-14.1.2- State the type of compound present, given a chemical name ending in -ane, -ene, -ol, or -oic acid or a molecular structure.

00:00
Lesson-14.1.3- Name the fuels: coal, natural gas and petroleum • Name methane as the main constituent of natural gas.

00:00
Lesson-14.1.4- Describe petroleum as a mixture of hydrocarbons and its separation into useful fractions by fractional distillation.

00:00
Lesson-14.1.5- Describe the properties of molecules within a fraction.

00:00
Lesson-14.1.6- Name the uses of the fractions as: – refinery gas for bottled gas for heating and cooking – gasoline fraction for fuel (petrol) in cars – naphtha fraction for making chemicals – kerosene/paraffin fraction for jet fuel.

00:00
Lesson-14.1.7- Name the uses of the fractions as:– diesel oil/gas oil for fuel in diesel engines – fuel oil fraction for fuel for ships and home heating systems – lubricating fraction for lubricants, waxes and polishes – bitumen for making roads.

00:00
Lesson-14.1.8- • Describe the general characteristics of a homologous series • Recall that the compounds in a homologous series have the same general formula • Describe and identify structural isomerism.

00:00
Lesson-14.1.9- Describe the properties of alkanes (exemplified by methane) as being generally unreactive, except in terms of burning • Describe the bonding in alkanes.

00:00
Assignments-14.1
Quiz-14.1
Lesson-14.2.1- Describe the manufacture of alkenes and of hydrogen by cracking.

00:00
Lesson-14.2.2-Distinguish between saturated and unsaturated hydrocarbons: – from molecular structures – by reaction with aqueous bromine.

00:00
Lesson-14.2.3- Describe the formation of poly(ethene) as an example of addition polymerization of monomer units.

00:00
Lesson-14.2.4- Describe the manufacture of ethanol by fermentation and by the catalytic addition of steam to ethene.

00:00
Lesson-14.2.5- Describe the properties of ethanol in terms of burning • Name the uses of ethanol as a solvent and as a fuel.

00:00
Lesson-14.2.6- Describe the formation of ethanoic acid by the oxidation of ethanol by fermentation and with acidified potassium manganate(VII).

00:00
Lesson-14.2.7- Describe ethanoic acid as a typical weak acid • Describe the reaction of a carboxylic acid with an alcohol in the presence of a catalyst to give an ester.

00:00
Assignments-14.2
Quiz-14.2
Lesson-14.3.1- • Define polymers as large molecules built up from small units (monomers).

00:00
Lesson-14.3.2- Explain the differences between condensation and addition polymerisation • Deduce the structure of the polymer product from a given alkene and vice versa.

00:00
Lesson-14.3.3- Describe the formation of nylon (a polyamide) and Terylene (a polyester) by condensation polymerization, the structure of nylon being represented.

00:00
Lesson-14.3.4- Describe proteins as possessing the same (amide) linkages as nylon but with different units.

00:00
Lesson-14.3.5- Describe the hydrolysis of proteins to amino acids. (Structures and names are not required.) • Describe complex carbohydrates in terms of a large number of sugar units, considered as HO OH, joined together by condensation polymerization.

00:00
Lesson-14.3.6- Describe the hydrolysis of complex carbohydrates (e.g. starch), by acids or enzymes to give simple sugars.

00:00
Lesson-14.3.7- Describe the fermentation of simple sugars to produce ethanol (and carbon dioxide). (Candidates will not be expected to give the molecular formulae of sugars.).

00:00
Lesson-14.3.8- Describe, in outline, the usefulness of chromatography in separating and identifying the products of hydrolysis of carbohydrates and proteins.

00:00
Assignments-14.3
Quiz-14.3

Test Yourself

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Final Mock-6
Final Mock-7
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Final Mock-10

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About Course

Cambridge OLevel Chemistry Crash Course

What Will You Learn?

Course Content

Introduction

Introduction

Assignments-1.1

Lesson-1.1.5- Show an understanding of the random motion of particles in a suspension (sometimes known as Brownian motion) as evidence for the kinetic particle (atoms, molecules or ions) model of matter. Describe and explain diffusion.

Lesson-1.1.4- Describe qualitatively the pressure and temperature of a gas in terms of the motion of its particles.

Lesson-1.1.3- Describe changes of state in terms of melting, boiling, evaporation, freezing, condensation and sublimation.

Lesson-1.1.2- Describe the structure of solids, liquids and gases in terms of particle separation, arrangement and types of motion.

Lesson-1.1.1- State the distinguishing properties of solids, liquids and gases.

Quiz-1.1

Assignments-2.1

Lesson-2.1.6- Suggest suitable purification techniques, given information about the substances involved.

Lesson-2.1.5- Describe and explain methods of purification by the use of a suitable solvent, filtration, crystallisation and distillation (including use of a fractionating column).

Lesson-2.1.4- Understand the importance of purity in substances in everyday life, e.g. foodstuffs and drugs.

Lesson-2.1.3- Identify substances and assess their purity from melting point and boiling point information.

Lesson-2.1.2- Demonstrate knowledge and understanding of paper chromatography • Interpret simple chromatograms.

Lesson-2.1.1- Name appropriate apparatus for the measurement of time, temperature, mass and volume, including burettes, pipettes and measuring cylinders.

Quiz-2.1

Assignments-3.1

Lesson-3.1.13- Describe metallic bonding as a lattice of positive ions in a ‘sea of electrons’ and use this to describe the electrical conductivity and malleability of metals.

Lesson-3.1.12- Describe the differences in volatility, solubility and electrical conductivity between ionic and covalent compounds.

Lesson-3.1.11- Describe the differences in volatility, solubility and electrical conductivity between ionic and covalent compounds.

Lesson-3.1.10- Describe the formation of single covalent bonds in H 2, Cl2, H2O, CH4, NH3 and HCl as the sharing of pairs of electrons leading to the noble gas configuration.

Lesson-3.1.9- Describe the formation of ions by electron loss or gain • Describe the formation of ionic bonds between elements from Groups I and VII.

Lesson-3.1.8- Describe the differences between elements, mixtures and compounds, and between metals and non-metals • Describe an alloy, such as brass, as a mixture of a metal with other elements.

Lesson-3.1.7- Describe the build-up of electrons in ‘shells’ and understand the significance of the noble gas electronic structures and of the outer shell electrons. (The ideas of the distribution of electrons in s and p orbitals and in d block elements are not required.)

Lesson-3.1.6- State the two types of isotopes as being radioactive and non-radioactive. State one medical and one industrial use of radioactive isotopes.

Lesson-3.1.5- Define isotopes as atoms of the same element which have the same proton number but a different nucleon number.

Lesson-3.1.4- Use proton number and the simple structure of atoms to explain the basis of the Periodic Table, with special reference to the elements of proton number 1 to 20.

Lesson-3.1.3- Define nucleon number (mass number) as the total number of protons and neutrons in the nucleus of an atom.

Lesson-3.1.2- Define proton number (atomic number) as the number of protons in the nucleus of an atom.

Lesson-3.1.1- State the relative charges and approximate relative masses of protons, neutrons and electrons.

Quiz-3.1

Assignments-4.1

Lesson-4.1.7- Calculate empirical formulae and molecular formulae • Calculate percentage yield and percentage purity.

Lesson-4.1.5- Define the mole and the Avogadro constant • Use the molar gas volume, taken as 24 dm3 at room temperature and pressure.

Lesson-4.1.4- Define relative molecular mass, M r, as the sum of the relative atomic masses. (Relative formula mass or M r will be used for ionic compounds.).

Lesson-4.1.3- Define relative atomic mass, A r, as the average mass of naturally occurring atoms of an element on a scale where the 12C atom has a mass of exactly 12 units.

Lesson-4.1.2- Deduce the formula of a simple compound from a model or a diagrammatic representation • Construct word equations and simple balanced chemical equations.

Lesson-4.1.1- Use the symbols of the elements and write the formulae of simple compounds • Deduce the formula of a simple compound from the relative numbers of atoms present.

Quiz-4.1

Assignments-5.1

Lesson-5.1.9- Describe, in outline, the manufacture of: – aluminium from pure aluminium oxide in molten cryolite – chlorine, hydrogen and sodium hydroxide from concentrated aqueous sodium chloride.

Lesson-5.1.8- Describe the production of electrical energy from simple cells, i.e. two electrodes in an electrolyte.

Lesson-5.1.7- Describe the transfer of charge during electrolysis to include: – the movement of electrons in the metallic conductor – the removal or addition of electrons from the external circuit at the electrodes – the movement of ions in the electrolyte.

Lesson-5.1.6- Describe the electroplating of metals • Outline the uses of electroplating.

Lesson-5.1.5- Predict the products of the electrolysis of a specified binary compound in the molten state.

Lesson-5.1.4- State the general principle that metals or hydrogen are formed at the negative electrode (cathode), and that non-metals (other than hydrogen) are formed at the positive electrode (anode).

Lesson-5.1.3- Describe the electrode products and the observations made during the electrolysis of: – concentrated aqueous sodium chloride – dilute sulfuric acid.

Lesson-5.1.2- Describe the electrode products and the observations made during the electrolysis of: – molten lead(II) bromide – concentrated hydrochloric acid.

Lesson-5.1.1- Define electrolysis as the breakdown of an ionic compound, molten or in aqueous solution, by the passage of electricity.

Quiz-5.1

Assignments-6.1

Lesson-6.1.4- Describe radioactive isotopes, such as 235U, as a source of energy.

Lesson-6.1.3- Describe the release of heat energy by burning fuels • State the use of hydrogen as a fuel.

Lesson-6.1.2- Interpret energy level diagrams showing exothermic and endothermic reactions.

Lesson-6.1.1- Describe the meaning of exothermic and endothermic reactions.

Quiz-6.1

Assignments-7.1

Lesson-7.1.9- Identify oxidising agents and reducing agents from simple equations.

Lesson-7.1.8- Define oxidising agent as a substance which oxidises another substance during a redox reaction. Define reducing agent as a substance which reduces another substance during a redox reaction.

Lesson-7.1.7- Define redox in terms of electron transfer • Identify redox reactions by changes in oxidation state and by the colour changes involved when using acidified potassium manganate(VII), and potassium iodide. (Recall of equations involving KMnO 4 is not required.).

Lesson-7.1.6- Understand that some chemical reactions can be reversed by changing the reaction conditions. (Limited to the effects of heat and water on hydrated and anhydrous copper(II) sulfate and cobalt(II) chloride.) (Concept of equilibrium is not required.).

Lesson-7.1.5- Interpret data obtained from experiments concerned with rate of reaction.

Lesson-7.1.4- Demonstrate knowledge and understanding of a practical method for investigating the rate of a reaction involving gas evolution.

Lesson-7.1.3- Describe the application of the above factors to the danger of explosive combustion with fine powders (e.g. flour mills) and gases (e.g. methane in mines).

Lesson-7.1.2- Describe and explain the effect of concentration, particle size, catalysts (including enzymes) and temperature on the rate of reactions.

Lesson-7.1.1- Identify physical and chemical changes, and understand the differences between them.

Quiz-7.1

Chapter-8. Acids, Bases, Salts

Lesson-8.1.1- Describe the characteristic properties of acids as reactions with metals, bases, carbonates and effect on litmus and methyl orange.

Lesson-8.1.2- Describe the characteristic properties of bases as reactions with acids and with ammonium salts and effect on litmus and methyl orange.

Lesson-8.1.3-Describe neutrality and relative acidity and alkalinity in terms of pH measured using universal indicator paper (whole numbers only).

Lesson-8.1.4- Describe and explain the importance of controlling acidity in soil.

Lesson-8.1.5- Classify oxides as either acidic or basic, related to metallic and non-metallic character.

Lesson-8.1.6- Demonstrate knowledge and understanding of preparation, separation and purification of salts.

Lesson-8.1.7- Describe the following tests to identify: aqueous cations: aluminum, ammonium, calcium, chromium(III), copper(II), iron(II), iron(III) and zinc (using aqueous sodium hydroxide and aqueous ammonia as appropriate).