Mastering Edexcel OLevel Chemistry with Ease online

About Course

Mastering Edexcel OLevel Chemistry with Ease online.

Students can learn Edexcel O-Level Chemistry concepts by taking this online course. All topics covered in the course, such as Atomic Structure, Chemical Bonding, States of Matter, Chemical Energetics, and others, are those that must be covered for the O-Level Chemistry exam. Through interactive quizzes, practice problems, and entertaining video lectures, students will learn the principles of chemistry.

Goals of the course:

to give pupils a thorough comprehension of Edexcel O-Level Chemistry
through practice tasks, assist pupils in developing their problem-solving abilities
in order to get kids ready to pass the O-Level Chemistry exam

Course Advantages:

all topics necessary for the O-Level Chemistry exam are fully covered
engaging lectures on the video to boost learning
Students can practice exercises and take interactive tests to improve their problem-solving abilities.
access to knowledgeable chemistry instructors for help and direction
Online learning is flexible and convenient

The overall goal of the online course “Mastering Edexcel O-Level Chemistry with Ease” is to assist students in building a solid foundation in chemistry and getting ready to pass the O-Level Chemistry exam.

Course Content

Introduction

Chapter-1. States of matter
1.1 understand the three states of matter in terms of the arrangement, movement and energy of the particles 1.2 understand the interconversions between the three states of matter in terms of: • the names of the interconversions • how they are achieved • the changes in arrangement, movement and energy of the particles. 1.3 understand how the results of experiments involving the dilution of coloured solutions and diffusion of gases can be explained 1.4 know what is meant by the terms: • solvent • solute • solution • saturated solution. 1.5C know what is meant by the term solubility in the units g per 100 g of solvent 1.6C understand how to plot and interpret solubility curves 1.7C practical: investigate the solubility of a solid in water at a specific temperature

Chapter-2. Elements, compounds and mixtures.
2.1.1 understand how to classify a substance as an element, compound or mixture 2.1.2understand that a pure substance has a fixed melting and boiling point, but that a mixture may melt or boil over a range of temperatures 2.1.3 describe these experimental techniques for the separation of mixtures: • simple distillation • fractional distillation • filtration • crystallisation • paper chromatography. 2.1.4 understand how a chromatogram provides information about the composition of a mixture 2.1.5 understand how to use the calculation of Rf values to identify the components of a mixture 2.1.6 practical: investigate paper chromatography using inks/food colourings

Chapter-3. Atomic structure
3.1.1 know what is meant by the terms atom and molecule 3.1.2 know the structure of an atom in terms of the positions, relative masses and relative charges of sub-atomic particles 3.1.3 know what is meant by the terms atomic number, mass number, isotopes and relative atomic mass (Ar) 3.1.4 be able to calculate the relative atomic mass of an element (Ar) from isotopic abundances

Chapter-4. The Periodic Table.
4.1.1 understand how elements are arranged in the Periodic Table: • in order of atomic number • in groups and periods. 4.1.2 understand how to deduce the electronic configurations of the first 20 elements from their positions in the Periodic Table 4.1.3 understand how to use electrical conductivity and the acid-base character of oxides to classify elements as metals or non-metals 4.1.4 identify an element as a metal or a non-metal according to its position in the Periodic Table 4.1.5 understand how the electronic configuration of a main group element is related to its position in the Periodic Table4.1.6 understand why elements in the same group of the Periodic Table have similar chemical properties 4.1.7 understand why the noble gases (Group 0) do not readily react

Chapter-5. Chemical formulae, equations and calculations.
5.1.1 write word equations and balanced chemical equations (including state symbols): • for reactions studied in this specification • for unfamiliar reactions where suitable information is provided. 5.1.2 calculate relative formula masses (including relative molecular masses) (Mr) from relative atomic masses (Ar) 5.1.3 know that the mole (mol) is the unit for the amount of a substance 5.1.4 understand how to carry out calculations involving amount of substance, relative atomic mass (Ar) and relative formula mass (Mr) 5.1.5 calculate reacting masses using experimental data and chemical equations 5.1.6 calculate percentage yield 5.1.7 understand how the formulae of simple compounds can be obtained experimentally, including metal oxides, water and salts containing water of crystallisation 5.1.8 know what is meant by the terms empirical formula and molecular formula 5.1.9 calculate empirical and molecular formulae from experimental data 5.1.10 understand how to carry out calculations involving amount of substance, volume and concentration (in mol/dm3) of solution 5.1.11 understand how to carry out calculations involving gas volumes and the molar volume of a gas (24 dm3 and 24 000 cm3 at room temperature and pressure (rtp)) 5.1.12 practical: know how to determine the formula of a metal oxide by combustion (e.g. magnesium oxide) or by reduction (e.g. copper(II) oxide)

Chapter-6. Group 1 (alkali metals) – lithium, sodium and potassium
6.1.1 understand how the similarities in the reactions of these elements with water provide evidence for their recognition as a family of elements 6.1.2 understand how the differences between the reactions of these elements with air and water provide evidence for the trend in reactivity in Group 1 6.1.3 use knowledge of trends in Group 1 to predict the properties of other alkali metals 6.1.4 explain the trend in reactivity in Group 1 in terms of electronic configurations

Chapter-7. Group 7 (halogens) – chlorine, bromine and iodine.
7.1.1 know the colours, physical states (at room temperature) and trends in physical properties of these elements 7.1.2 use knowledge of trends in Group 7 to predict the properties of other halogens 7.1.3 understand how displacement reactions involving halogens and halides provide evidence for the trend in reactivity in Group 7 7.1.4 explain the trend in reactivity in Group 7 in terms of electronic configurations

Chapter-8. Gases in the atmosphere
8.1.1 know the approximate percentages by volume of the four most abundant gases in dry air 8.1.2 understand how to determine the percentage by volume of oxygen in air using experiments involving the reactions of metals (e.g. iron) and non-metals (e.g. phosphorus) with air 8.1.3 describe the combustion of elements in oxygen, including magnesium, hydrogen and sulfur 8.1.4 describe the formation of carbon dioxide from the thermal decomposition of metal carbonates, including copper(II) carbonate 8.1.5 know that carbon dioxide is a greenhouse gas and that increasing amounts in the atmosphere may contribute to climate change 8.1.6 practical: determine the approximate percentage by volume of oxygen in air using a metal or a non-metal

Chapter-9. Reactivity series.
9.1.1 understand how metals can be arranged in a reactivity series based on their reactions with: • water • dilute hydrochloric or sulfuric acid. 9.1.2 understand how metals can be arranged in a reactivity series based on their displacement reactions between: • metals and metal oxides • metals and aqueous solutions of metal salts. 9.1.3 know the order of reactivity of these metals: potassium, sodium, lithium, calcium, magnesium, aluminium, zinc, iron, copper, silver, gold 9.1.4 know the conditions under which iron rusts 9.1.5 understand how the rusting of iron may be prevented by: • barrier methods • galvanising • sacrificial protection. 9.1.6 understand the terms: • oxidation • reduction • redox • oxidising agent • reducing agent in terms of gain or loss of oxygen and loss or gain of electrons.9.1.7 practical: investigate reactions between dilute hydrochloric and sulfuric acids and metals (e.g. magnesium, zinc and iron)

Chapter-10. Acids, alkalis and titrations.
10.1.1 describe the use of litmus, phenolphthalein and methyl orange to distinguish between acidic and alkaline solutions 10.1.2 understand how to use the pH scale, from 0–14, can be used to classify solutions as strongly acidic (0–3), weakly acidic (4–6), neutral (7), weakly alkaline (8–10) and strongly alkaline (11–14) 10.1.3 describe the use of universal indicator to measure the approximate pH value of an aqueous solution 10.1.4 know that acids in aqueous solution are a source of hydrogen ions and alkalis in a aqueous solution are a source of hydroxide ions 10.1.5 know that alkalis can neutralise acids 10.1.6 describe how to carry out an acid-alkali titration

Chapter-11. Acids, bases and salt preparations.
11.1.1 know the general rules for predicting the solubility of ionic compounds in water: • common sodium, potassium and ammonium compounds are soluble • all nitrates are soluble • common chlorides are soluble, except those of silver and lead(II) • common sulfates are soluble, except for those of barium, calcium and lead(II) • common carbonates are insoluble, except for those of sodium, potassium and ammonium • common hydroxides are insoluble except for those of sodium, potassium and calcium (calcium hydroxide is slightly soluble). 11.1.2 understand acids and bases in terms of proton transfer 11.1.3 understand that an acid is a proton donor and a base is a proton acceptor 11.1.4 describe the reactions of hydrochloric acid, sulfuric acid and nitric acid with metals, bases and metal carbonates (excluding the reactions between nitric acid and metals) to form salts 11.1.5 know that metal oxides, metal hydroxides and ammonia can act as bases, and that alkalis are bases that are soluble in water 11.1.6 describe an experiment to prepare a pure, dry sample of a soluble salt, starting from an insoluble reactant 11.1.7 describe an experiment to prepare a pure, dry sample of a soluble salt, starting from an acid and alkali 11.1.8 describe an experiment to prepare a pure, dry sample of an insoluble salt, starting from two soluble reactants 11.1.9 practical: prepare a sample of pure, dry hydrated copper(II) sulfate crystals starting from copper(II) oxide 11.1.10 practical: prepare a sample of pure, dry lead(II) sulfate

Chapter-12. Ionic Bonding

Chapter-13. Covalent Bonding

Chapter-14. Metallic Bonding

Chapter-15. Electrolysis

Chapter-16. Extraction and Uses of Metals

Chapter-17. Chemical Tests

Chapter-18. Energetics

Chapter-19. Rates of Reactions

Chapter-20. Reversible Reactions and Equilibria

Chapter-21. Introduction of Organic Chemistry

Chapter-22. Crude Oil

Chapter-23. Alkanes

Chapter-24. Alkenes

Chapter-25. Alcohols

Chapter-26. Carboxylic Acids

Chapter-27. Esters

Chapter-28. Synthetic Polymers

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