Do now! Can you read through the blast furnace equations?

Slides:

Advertisements

Similar presentations

Can you think of some uses for aluminium?

Advertisements

31/03/2017 Reactivity of Metals.

1 Secondary 4 Chemistry Extraction of Aluminium via electrolysis JT 2009 Raffles Programme.

Electrolysis Electrolysis breaks down ionic substances into simpler substances by using electricity!

1 Negative Ions - Bromine Negative ions are attracted to the positive electrode. The positive electrode is called the anode. Negative ions are called anions.

Properties of metals Chemical properties Form oxides when they react with oxygen Metal oxides are bases Form positive ions Transition metals have a variable.

Starter 1. The following metals were reacted with water. Put them in order of reactivity, with the least reactive metal first. Lithium, potassium, calcium,

What is an ore? Why do we have to use chemical reactions to extract most metals? What is the name given to the group of metals in the centre of the periodic.

Chemicals of the Natural Environment. C5 Lesson 8.

The Extraction Of Metals and The Preparation and Collection Of Non-Metals. Ashvini Jagassar- 5C Chemistry. Mr. Dookoo.

ALUMINIUM Extraction and uses. BACKGROUND Aluminium is the most common metal in the Earth’s crust. It comprises approximately 7.5% of the crust by mass.

Purifying Metals Aims:

Electrolysis. –A redox reaction that is made to occur by passing a direct electric current through an electrolyte Electrolyte –is a liquid that conducts.

Production and Uses of Metals CHEMISTRY 2 Additional Science Chapter 8.

Cairo University Faculty of Engineering 2nd year Dept of Metallurgy.

Extraction of Aluminium I know how aluminium is extracted from its ore. L.O.

Write down the Reactivity Series from Potassium to Gold.

ELECTROLYSIS Decomposition using an electric current.

The Extraction Of Metals

APPLICATIONS of REDOX REACTIONS. ELECTROPLATING Electroplating is the use of electrolysis to apply a thin layer of one metal over another.

Extraction of Aluminium Aluminium is extracted using electrolysis because it is too reactive to be extracted using carbon.

Definition The Process Examples

Explain the process of electrolysis and its uses

Splitting up ionic compounds (F) Molten compounds

Metals, Making Electricity and Corrosion. Metals The job that a metal is used for is determined by its physical and chemical properties. Physical properties.

METALS. Introducing metal extraction 1.First, substances other than the metal compound are removed (concentration). 2.Next, the metal itself is extracted.

Metals. Learning Objectives Use reactivity data to determine a reactivity series Relate extraction method to reactivity of metals Write word/symbol equations.

The purpose of electrolysis is to split up ionic compounds using electricity to produce useful products. Electrolysis is used a lot in industry and is.

Chemical effect of electric current How things work.

Electrolysis L.O: To be able to describe the uses and predict the products of electrolysis.

Aluminium It is a metal with a low density which means it is lightweight for its size Aluminium is used for aircraft, trains, overhead power cables, saucepans.

One plus, two plus, three plus, NO Three minus, two minus, one minus, NO.

What are atoms like??? By Alex Hulbert. An atom is made up of a nucleus that is surrounded by electrons. The nucleus of a atom is made up of protons and.

Electrolysis – background

Making aluminium.

Electrolysis Noadswood Science, 2012.

Title: Lesson 6 Electrolytic Cells Learning Objectives: – Describe electrolytic cells – Identify at which electrode oxidation and reduction takes place.

Aluminium Extraction and Uses.

Revision lesson.  Metals found in the ground are normally found as a METAL ORE – combined with other elements in compounds  Metals found on their own.

Extracting metals. Methods of extracting metals The Earth's crust contains metals and metal compounds such as gold, iron oxide and aluminium oxide, but.

Conductors and non-conductors Conductors are materials that conduct electricity. Non-conductors or insulators are materials that do not conduct electricity.

ELECTROLYSIS BONDING, STRUCTURE & PROPERTIES. After completing this topic you should be able to : BONDING, STRUCTURE & PROPERTIES ELECTROLYSIS Explain.

IGCSE CHEMISTRY SECTION 5 LESSON 1. Content The iGCSE Chemistry course Section 1 Principles of Chemistry Section 2 Chemistry of the Elements Section 3.

AQA GCSE C2.7.  When an ionic substance is melted or dissolved in water (to make a solution) the ions become free to move.  Electrolysis can then be.

Learning objective: demonstrate electrolysis as the decomposition of a molten salt by an electric current see patterns in the changes at the electrodes.

3.17 Uses of electrolysis Purification of copper:

Chapter 17.  Which metals were discovered earliest?  Gold, copper, silver = less reactive metals  Found “native” ie. as pure metal  More reactive.

Some metals react with;

Recycle or raw materials?

The Extraction Of Metals 1

The ionic compound is called an electrolyte.

Starter Under what conditions do ionic compounds conduct electricity?

Redox Reactions and Electrolysis

Make sure you revise the following:

extraction of metals extraction of aluminium -

A complete circuit is required for electric current to flow

Knowledge Organiser – Chemical Changes

C6.2 Changes at the electrodes

C4 – Chemical changes Key Concepts.

Chemistry 4: Chemical Changes

Title: Electrolysis Complete the activities listed below

The reactivity of metals

Presentation transcript:

Do now! Can you read through the blast furnace equations?

Last lesson The reduction of copper oxide using carbon.

Extracting copper from copper oxide 2CuO + C 2Cu + CO 2

Today’s lesson The extraction of aluminium from aluminium oxide (Bauxite)

Reactivity Series

Electrolysis of aluminium oxide CO 2

Electrolysis of aluminium oxide Aluminium oxide has a high melting point (2054°C) (EXPENSIVE)

Electrolysis of aluminium oxide Aluminium oxide will dissolve in molten cryolite which melts at “only” 959°C (CHEAPER)

Electrolysis of aluminium oxide The molten liquid is put into a large chamber, the walls of which are connected to the negative side of a circuit (cathode). Large positive electrodes (anodes) made of graphite are lowered into the mixture.

Electrolysis of aluminium oxide Aluminum oxide is an ionic compound. The positive aluminium ions drift to the negative electrode (cathode) and the negative oxygen ions to the positive electrodes (anodes).

Electrolysis of aluminium oxide At the cathode the aluminium ions gain electrons and become aluminium atoms. 4Al e - 4Al

Electrolysis of aluminium oxide At the anodes the oxygen ions lose electrons and become oxygen atoms. 6O 2- 3O e -

Electrolysis of aluminium oxide The oxygen immediately reacts with the hot graphite to form carbon dioxide. This means the graphite electrodes have to be replaced occasionally as they wear away.

Electrolysis of aluminium oxide Molten aluminium is tapped from the bottom of the chamber

Electrolysis of aluminium oxide This all requires LOTS of electricity so is an expensive process.

Electrolysis of Aluminium Aluminium oxide has a high melting point (2054°C) (EXPENSIVE) Aluminium oxide will dissolve in molten cryolite which melts at “only” 959°C (CHEAPER) The molten liquid is put into a large chamber, the walls of which are connected to the negative side of a circuit (cathode). Large positive electrodes (anodes) made of graphite are lowered into the mixture. Aluminum oxide is an ionic compound. The positive aluminium ions drift to the negative electrode (cathode) and the negative oxygen ions to the positive electrodes (anodes). At the cathode the aluminium ions gain electrons and become aluminium atoms. 4Al e-4Al At the anodes the oxygen ions lose electrons and become oxygen atoms. 6O 2- 3O e- The oxygen immediately reacts with the hot graphite to form carbon dioxide. This means the graphite electrodes have to be replaced occasionally as they wear away. Molten aluminium is tapped from the bottom of the chamber Maximum two words per drawing - numbers allowed

Homework Can you complete the “Draw the sentence” exercise for Wednesday 23 rd September?