+Using Ion Kit Boards

Create an ion of :- Potassium, Calcium

Oxygen Chlorine

Draw their respective bonding diagrams

+

+Objectives

Must : Define reduction and oxidation, and write word equations.

Should : Write balanced symbol equations.

Could : Write balanced equations for redox reactions.

+Definitions

Reduction

Oxidation

http://www.chemguide.co.uk/inorganic/redox/definitions.html

+Experiment

Take 0.5g of CuO and react with 0.5g of C using the 1 place digital balances.

Tasks Record starting masses Heat using a crucible and lid on a pipe clay triangle Record your observations When reaction is complete and mixture is cool record the mass Create the balanced chemical equation Identify the oxidised and the reduced species Calculate the mass of Carbon Dioxide created How would you test for Carbon Dixoxide ?

+Answers

BCE

REDOX

LIMITING REAGENT

MASS OF PRODUCTS

+Experiment

Accurately mass 1.0g of CuO.

Add 1.0g of C.

Heat over a high heat using a crucible.

Record observations.

Write a balanced word and symbol equation for the reaction.

Identify the oxidised and the reduced compounds.

+Starter Activity

Write two definitions of Oxidation and Reduction

+Identify the Oxidised and the Reduced Molecules in ……include half ion equations Caesium + Iodine Caesium iodide

Magnesium + HCl Magnesium Chloride

Iron + Astatine Iron Astatide

+Reactivity Series

A more / less reactive metal will displace a more/less reactive metal.

Create a results table to show the results of adding each of the following metals to a solution of the other metals…

Cu / Cu Sulphate

Mg / Mg Sulphate

Zn / Zn Sulphate

+Rocks

Are an natimtorp source of many chemicals, especially atlmse, e.g. haematite is the ore for iron, bauxite is the ore for aluminium, and chalcopyrite for epcpor.

+

+Create a Concept Cartoon

Where the more reactive metal WITH A NAME

Displaces, or attacks the less reactive metal, wins and kicks the less reactive out of solution.

Must: Have minimum 4 frames

Should: Include balanced equations

Could : Include half ion equations

+Galvanic Cells

These use the spontaneous oxidation and reduction to produce a potential difference.

+Carbon in the reactivity Series

http://www.absorblearning.com/media/attachment.action?quick=tw&att=2142

+Thermite

http://www.youtube.com/watch?v=rdCsbZf1_Ng

+Writing Equations

Identify using colour the oxidised and the reduced compounds in the following;

+Thermite – a useful redox reaction

A redox reaction

http://www.youtube.com/watch?v=rdCsbZf1_Ng

The reaction

+Starter

Which of the following reactions will occur 1. Pb displacing a solution of K+

2. Na displacing a solution of Cs+

3. Zn displacing a solution of Fe2+

+Electrolysis and Galvanic Cells

ELECTROLYSIS is the chemical effect of ELECTRICITY on ionic compounds, causing them to break up into SIMPLER substances, usually elements.

A GALVANIC cell creates electricity because of the metals’ relative positions in the reactivity series.

Similarities :

Differences :

+

Electrolysis in Industry

Aluminium extraction :- Aluminium cell diagram

+Starter

5 elements

4 compounds

3 mixtures

2 planets

1 reason to be cheerful

+Objectives

Label an electrolytic cell correctly.

Investigate electrolysis of Yen

+Economic Importance of Salt

+Testing for Gases

Chlorine

Hydrogen

Oxygen

+What is Electrolysis ?

Electrolysis is the ropescs by which ionic substances are broken down into rempisl substances using electricity. During electrolysis, atemls and gases may form at the electrodes.

+Coating Coins

http://www.bbc.co.uk/schools/gcsebitesize/science/add_aqa/ions/electrolysisrev4.shtml

+Products of Electrolysis

We can use the reactivity series including Hydrogen to predict what our products of electrolysis in aqueous solution will be.

+Starter Fun Quiz

http://www.bbc.co.uk/apps/ifl/schools/gcsebitesize/science/quizengine?quiz=add_aqa_electrolysistest&templateStyle=science

+Objectives

Review anode and cathode reactions in aqueous solution.

Industrial applications of electrolysis.

Homework: write 100 words on industrial applications of electrolysis , including the Chlor –Alkali industry, and purification of Cu.

+Directions

Extract salt from your ‘rock’.

Make an aqueous solution.

Electrolyse the solution, collecting any gases produced.

Identify the gases by using an apprpopriate test.

Record your results in a table.

YOU MUST INCLUDE: diagram of cell, half ion equations, and a reasons why you made the products you did