Reactivity Series of Metals

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Questions and Answers

What is the product of the reaction between a metal and water?

Metal oxide and oxygen

Metal hydroxide and hydrogen gas (correct)

Metal acid and oxygen

Metal oxide and hydrogen gas

Which metal does NOT react with any of the above?

Potassium

Sodium

Copper

Gold (correct)

What happens when a more reactive metal is placed in a solution of a less reactive metal salt?

The reaction does not occur

The less reactive metal coats the more reactive metal (correct)

The more reactive metal dissolves

The solution turns into water

What is the order of reactivity of the metals from most reactive to least reactive?

Potassium, sodium, lithium, calcium, magnesium, zinc, iron, copper, silver, gold Signup and view all the answers

What are the necessary conditions for iron to rust?

Both air and water Signup and view all the answers

What is the relationship between a metal's reactivity and its tendency to form positive ions?

Reactivity is directly proportional to the tendency to form positive ions Signup and view all the answers

What is the product of the reaction between a metal and acid?

Salt and hydrogen gas Signup and view all the answers

What type of reaction occurs when a more reactive metal displaces a less reactive metal from a compound?

Displacement reaction Signup and view all the answers

What is the result of oxidation in terms of oxygen?

Gain of oxygen Signup and view all the answers

Which of the following methods can prevent rusting of iron by excluding oxygen and water?

Using a desiccant in the container Signup and view all the answers

What is the purpose of sacrificial protection in preventing rusting?

To allow the more reactive metal to rust first and protect the underlying metal Signup and view all the answers

What is the definition of a reducing agent?

A substance that causes another reactant to be reduced and is oxidised itself Signup and view all the answers

What is the reaction between a metal and an acid in the reactivity series?

Metal + acid → hydrogen + salt Signup and view all the answers

Which of the following metals will react with dilute acids up to iron in the reactivity series?

Only the more reactive metals Signup and view all the answers

What is the term for a reaction in which both oxidation and reduction occur?

Redox reaction Signup and view all the answers

What is the purpose of galvanising in preventing rusting?

To provide a barrier to prevent water and oxygen from reaching the metal Signup and view all the answers

Study Notes

Metals and Reactivity

A few reactive metals react with cold water, producing a metal hydroxide and hydrogen gas (e.g., 2K + 2H2O -> 2KOH + H2 with potassium).
Most metals react with acid, producing a salt and hydrogen gas (acid + metal -> salt + H2).

Reactivity Series

Metals can be arranged in a reactivity series based on their reactions with water, dilute hydrochloric or sulfuric acid, and oxygen.
The order of reactivity is: potassium, sodium, lithium, calcium, magnesium, aluminium, zinc, iron, copper, silver, gold.
Metals can be arranged in a reactivity series based on their displacement reactions between metals and metal oxides, and metals and aqueous solutions of metal salts.

Displacement Reactions

A more reactive metal can displace a less reactive metal from a compound in a displacement reaction.
Displacement reactions can be used to determine the relative reactivity of metals.

Rusting of Iron

Iron rusts when both air and water are present, resulting in corrosion (oxidation).
Rusting can be prevented by excluding oxygen and water, such as by painting, coating with plastic, or using oil or grease.

Prevention of Rusting

Barrier methods: painting, coating with plastic, using oil or grease.
Galvanising: using a more reactive metal (e.g., zinc) to protect iron from rusting.
Sacrificial protection: using a more reactive metal to protect iron from rusting.

Oxidation and Reduction

Oxidation: gain of oxygen OR loss of electrons.
Reduction: loss of oxygen OR gain of electrons.
Redox: a reaction in which both oxidation and reduction occur.
Oxidising agent: causes another reactant to be oxidised and is reduced itself.
Reducing agent: causes another reactant to be reduced and is oxidised itself.

Investigating Reactions

Investigate reactions between dilute hydrochloric and sulfuric acids and metals (e.g., magnesium, zinc, and iron).
The reactivity series diagram shows that only more reactive metals react with dilute acids (up to iron).

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Description

This quiz covers the arrangement of metals in a reactivity series based on their reactions with water, acid, and oxygen. It includes the products of these reactions and the equations involved.