This lesson continues the discussion of acids and bases started in Lesson 6. You will learn how to identify the difference between acids, bases, and salts, including their structure, formula, physical properties, and the substances they interact with. You will also learn about integral role of neutralization reactions as well as hydrogen and water. You will then learn the importance of knowing the difference between dangerous and safe acids and bases. Your perception of weak and strong will be altered along the way, and you will finish this lesson with a better awareness of how to safely handle these substances that are everywhere around you. Show Less
We come into contact with a variety of different acids and bases every day. In this video, students will learn about some of the common acids and bases that they use and interact with on a daily basis.
Acids and bases are all around us. This programme features the following: - Early theories of Arrenhius and Lowry-Bronsted. - Valence structures. - Exposed protons and proton transfer. - Diprotic and triprotic acids linked to structures. - Amphiprotic example given by hydrogen sulphate ion. - The pH scale and the use of indicators to measure pH. - Conjugate pairs and strengths of acids with strong acids giving weak conjugate bases. - Standard reactions: acid + metal, acid + oxide, acid + carbonate, acid + hydrogen carbonate. Show Less
This programme familiarises students with the features of acids and bases, and discusses their physical and chemical properties. The pH scale is introduced with examples of strong and weak acids and bases and the concept of neutral substances is explored. The use of indicators to test the pH of acids and bases is explained, as well as showing the variety of indicators available and their specific uses. Students are shown how to make their own red cabbage indicator in the kitchen, and examples of acids and bases commonly found in the home are discussed. A description of neutralisation reactions and their products concludes the programme. Show Less
Objective: To learn about air. Learning outcomes - students will be able to: 1. Define air and its composition 2. Discuss the percentage of different gases present in air 3. Explain that air occupies space
Radioisotopes are unstable atoms that emit radiation, and decay to form stable atoms. Some of their uses are as nuclear fuel and as tracers in medicinal fields.
This video defines colloids and explains their importance in pharmaceutical preparations.
The programme covers Le Chatelier's principle, the equilibrium law, calculating K. It examines how K changes when the temperature of exothermic and endothermic reactions changes, with a focus on sulphuric acid manufacture.
Objective: To understand the arrangement of electrons in atoms. Learning outcomes: Students will be able to 1. Explain the Bohr-Bury Scheme of distribution of electrons in an atom. 2. Give the electronic distribution of elements such as boron, oxygen and calcium. Show Less
Chemical analysis is integral to modern society. The testing of consumer goods, industrial products and food relies upon a number of different techniques. This program will investigate the analytical techniques of chromatography, mass spectrometry and spectroscopy. This program will address the theory behind how a range of analytical techniques work and how the data produced by these techniques is interpreted. Specific examples will be used to demonstrate the qualitative and quantitative applications of chromatography, mass spectrometry, flame testing, atomic absorption spectrometry, infrared spectrometry and nuclear magnetic resonance spectrometry. Show Less
Objective: To learn about Dalton’s Atomic Theory, molecules and ions, how to write the chemical formulae of compounds, the laws of chemical combination, and the mole concept. Learning outcomes - students will be able to: 1. State the postulates of Dalton’s Atomic Theory 2. State the limitations of Dalton’s Atomic Theory 3. Explain the Law of Multiple Proportion 4. Tell how the molecules of an element or a compound are formed 5. Define 'molecule' 6. Define 'atomicity of molecule' 7. Write the atomicity of different elements 8. Define 'ions' 9. Explain the formation of ions 10. Define cation and an anion 11. Distinguish between simple ions and polyatomic ions 12. Define 'chemical formula' 13. Identify the symbols given by Dalton and Berzelius 14. Memorise the modern symbols used to represent elements 15. Define 'valency' 16. Write the chemical formulae of some compounds 17. Define a polyatomic ion 18. Define the term 'electronegativity' 19. State the laws of chemical combination 20. Explain the Law of Conservation of Mass 21. Explain the Law of Definite Proportion 22. Define the concept of mole 23. State what Avagadro’s number is 24. Explain the molar mass of elements and compounds 25. Define gram atomic mass, gram molecular mass, and formula unit mass Show Less
Avogadro’s Law describes the relationship between the volume of a gas and the number of molecules in it, at constant temperature and pressure. Students will learn how to prove the law in this video.
In this resource, you learn a great deal about the depth to which chemistry explains every part and process related to the human body. As you know, chemistry often deals with small, almost invisible substances, and in this resource you will focus on the cell. You will also explore in detail how much our body is affected by the various sources of energy you eat, such as carbohydrates, fats, and proteins. As you will discover, your body and your health are not solely determined by how much you exercise and what you eat. Genetics, in the form of DNA, helps explain who you are and even who you may become, including the types of diseases you may inherit that have afflicted the people you are related to. Why are fats not all bad? Why should you not cut out carbohydrates completely, even when on a diet? How can a disease from your grandfather pass on to you? Show Less
In a secret location, Copper and Silver separate Chlorine from Potassium. Gold and Chlorine return to Carbon’s secret school – but cannot find Fluorine and Oxygen. Carbon appears, and Gold and Chlorine flee to a nearby bond shop where they meet Oxygen – now an Ozone molecule. Carbon has followed them and calls in Cyanide to dissolve Gold, and our hero is taken to the DNA coding hideout. Show Less
This programme covers: * Electrons in clouds around atoms. * The electrons of halogens outer shell. * The electrons of alkali metal outer shell. * Carbon diamond and graphite share electrons. * Chlorine combining with the third row, a range of bonds. * Metallic bond * Ionic bond * Ionic solutions dissolving in water. Show Less
This film takes you from discussing the elements in isolation to exploring how these elements interact with each other at the atomic level, and how chemists, including you, can predict these interactions. As we move our focus to bonding in this lesson you will shift your focus to the electrons, since they define how elements interact with each other. Show Less
In the hideout, Chlorine is trapped in Carbon’s buckyball, and Gold is put behind bars. When released, Ethanol takes him on a guided tour of the completed Project D. It’s giant DNA molecule, which will bring Planet Earth to life. Gold’s final attempt at destroying the molecule has little effect. Carbon’s heavies throw Gold and Chlorine into some aqua regia – and the pair finally bond. Show Less
Carboxylic acids are carbon compounds containing polar carboxyl functional groups. Carboxylic acids form strong intermolecular hydrogen bonds and have high boiling points . The hydrogen bonding is also responsible for the high solubility of smaller carboxylic acid molecules in water. Show Less
Sodium hydroxide is produced by the electrolysis of sodium chloride solution. During electrolysis, hydrogen gas evolves at the cathode and chlorine gas evolves at the anode.
Objective: To learn about the changes in the states of matter. Learning outcomes - students will be able to: 1. Identify the three states of matter; 2. Understand how ice, water, and water vapour are formed.
What happens when you turn up the heat in an equilibrium? This video demonstrates how changing temperature affects reaction rates in accordance with Le Chatelier’s principle. Students will observe the colour of a solution of cobaltous chloride at different temperatures. Footage of a real lab demonstration makes this essential viewing for senior secondary chemistry students. Show Less
What happens when you add more product to an equilibrium? This video demonstrates how an increase in products affects reaction rates in accordance with Le Chatelier’s principle. Students will observe how the appearance of a solution of sodium chloride changes when products are added. Footage of a real lab demonstration makes this essential viewing for senior secondary chemistry students. Show Less
What happens when you add more reactant to an equilibrium? This video demonstrates how an increase in reactants affects reaction rates in accordance with Le Chatelier’s principle. Students will observe how the colour of a solution of ferric thiocyanate changes when reactants are added. Footage of a real lab demonstration makes this essential viewing for senior secondary chemistry students. Show Less
What happens when you increase the pressure on an equilibrium? This video demonstrates how changing pressure affects reaction rates in accordance with Le Chatelier’s principle. Students will observe the colour of a gaseous mixture of nitrogen dioxide and dinitrogen tetroxide under different pressure conditions. Footage of a real lab demonstration makes this essential viewing for senior secondary chemistry students. Show Less