Navigating Chemistry OLevel CAIE Success Online

About Course

A complete online course called Chemistry Expedition was created to give O-Level CAIE (Cambridge Assessment International Education) students the knowledge and abilities they need to flourish in Chemistry. According to the specifications of the O-Level CAIE curriculum, this subject offers a thorough examination of the fundamental ideas, concepts, and uses of chemistry.

Students will have an exciting learning journey throughout the course as they delve into the intriguing realm of chemistry through interactive lessons, interesting multimedia materials, and practical exercises. The O-Level CAIE Chemistry syllabus’s main topics and learning objectives are meticulously covered throughout the course material.

Atomic structure, chemical bonding, and chemical reactions are introduced at the start of the course as its foundational ideas. The periodic table, chemical equations, and stoichiometry will all be deeply understood by the students.

Students will learn about the various subfields of chemistry as the course goes along, including organic, inorganic, and physical chemistry. They will explore the characteristics, reactions, and uses of a variety of substances and elements, including metals, hydrocarbons, acids, and bases. It will also include practical laboratory skills such as safe laboratory procedures, experimental methods, and data analysis.

Critical thinking and problem-solving abilities are highly valued in this course. To hone their analytical skills and get ready for the O-Level CAIE Chemistry exams, students will be exposed to a variety of practice problems and problem-solving situations. In order to perform at their best, they will discover efficient approaches to various question kinds and exam methodologies.

The course includes virtual experiments, simulations, and interactive demos to improve the learning experience. To help them comprehend the material better, students will be given the chance to simulate experiments, watch chemical processes, and visualize challenging ideas.

The course incorporates real-world applications of chemistry in addition to the fundamentals, stressing the importance of chemistry in a variety of fields and daily life. In order to help them understand how important chemistry is to everyday life, students will learn about how it is used in medicine, energy production, consumer goods, and environmental sustainability.

Students will have access to a range of learning resources during the course, such as course notes, practice questions, exams, and interactive conversations. Instructors will provide timely feedback to students in order to track their development and offer suggestions for improvement.

Students can learn at their own speed and have access to the course materials whenever and wherever they want thanks to the flexibility and convenience of the Chemistry Expedition course. The user-friendly online learning environment offers a seamless learning environment that encourages interaction and involvement with the course material and other students.

By the end of the course, students will have improved their problem-solving abilities, gained confidence in taking the O-Level CAIE Chemistry exams, and developed a thorough understanding of chemistry subjects. Students who successfully complete the course will be well-equipped to excel in their Chemistry coursework and seek postsecondary education or professions in scientific fields.

Explore the mysteries of chemistry by setting off on the Chemistry Expedition. Join us for this comprehensive online learning experience, and let us help you prepare for and succeed on the O-Level CAIE Chemistry exams. Enroll right away to start a life-changing adventure of learning!

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

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

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

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

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.)

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).)

Chapter-8. Acids, Bases, Salts

Chapter-9. The Periodic Table

Chapter-10. Metals

Chapter-11. Air and Water

Chapter-12. Sulfur

Chapter-13. Corbonates

Chapter-14. Organic Chemistry

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