Reactivity of Metals

This section explores the reactivity series of metals explained for GCSE and Class 10 students. It covers key concepts such as oxidation, reduction, and displacement reactions.

The general equation for a metal's reaction with oxygen is presented as: metal + oxygen → metal oxide

Definition: Oxidation is when oxygen is added to an element or compound, while reduction is when oxygen is removed.

The reactivity series of metals is outlined, ranging from potassium (most reactive) to gold (least reactive):

Highlight: Potassium, Sodium, Lithium, Calcium, Magnesium, Aluminium, Carbon, Zinc, Iron, Hydrogen, Copper, Silver, Gold

The document explains displacement reactions and details the reactions of various metals with water and dilute acids.

Example: Potassium, sodium, and lithium react violently with water, while copper and silver have no reaction.

The relationship between a metal's reactivity and its tendency to form positive ions is discussed, introducing the concept of native metals.

Vocabulary: A native metal is a metal found in its pure form in nature.

Electrolysis

This final section covers the process of electrolysis, explaining key terms and concepts related to this electrochemical technique.

Vocabulary: Electrodes are solid conductors made of metal, while an electrolyte is a liquid or solution containing an ionic compound that can conduct electricity.

The document explains why ionic compounds can conduct electricity in aqueous solutions or molten states, and describes the functions of anodes and cathodes.

Highlight: The anode is the positive electrode that attracts negative ions, while the cathode is the negative electrode that attracts positive ions.

The reasons for using electrolysis in metal extraction are discussed, along with its drawbacks such as high energy consumption.

Example: Metals more reactive than carbon cannot be extracted using carbon reduction and require electrolysis.

The document concludes by explaining the products formed during electrolysis based on the reactivity of the metal and the type of negative ion present.

Highlight: If the metal is higher than hydrogen in the reactivity series, hydrogen is produced. If it's lower, the metal itself is produced.