Redox and electrochemistry > metals

Some metals are more reactive than others. In this experiment, a strip of metal is added to a solution of a compound of another metal. A more reactive metal displaces (pushes out) a less reactive metal from its compound. In carrying out the

Students add powdered or finely-divided metals to a copper(II) sulfate solution and measure the 

Students add powdered or finely-divided metals to hydrochloric 

A solution containing silver nitrate (Tollen’s reagent) and a 

Students heat copper(II) oxide in a glass tube while passing methane over it. The copper(II) oxide is reduced to copper. If the reactants and products are weighed carefully the formula of the copper oxide can be deduced. This could also be used simply as an example of reduction.
 

In this experiment students protect iron nails using a variety of methods including painting, greasing and sacrificial protection. The nails are placed in test-tubes and covered with corrosion indicator solution. This contains gelatine and so sets to a jelly-like consistency. The indicator changes colour from yellow to blue to show where rusting is taking place.

This experiment demonstrates that conduction is only possible where lead(II) bromide is molten, and that metallic lead and bromine are the products of electrolysis of the molten electrolyte. This is a demonstration that can be done as an introduction to studying electrolysis.
 

This demonstration is designed to find the value of the Faraday constant – the amount of electric charge carried by one mole of electrons - from the electrolysis of aqueous copper(II) sulfate solution, using weighed copper electrodes.
 

This lesson is designed to exemplify a model-based inquiry approach to practical work.