Reactivity Series and Rusting in Metals - Edexcel IGCSE Chemistry

These flashcards cover key concepts related to the reactivity series of metals, rusting of iron, and the definitions of chemical reactions and terms as instructed in the Edexcel IGCSE Chemistry syllabus.

What are the products when a reactive metal reacts with cold water?

Metal hydroxide and hydrogen gas.

Which metal is known for being extremely unreactive and does not react with water, acids, or oxygen?

Gold.

What do you observe when metals react with acid?

Bubbles of hydrogen gas are given off.

What is the order of the reactivity series ?

Potassium > Sodium > Lithium > Calcium > Magnesium > Aluminium > Zinc > Iron > Copper > Silver > Gold.

How can the relative reactivity of metals be deduced?

By observing their reactions with water, acids, and oxygen.

What happens in a displacement reaction between metals?

A more reactive metal displaces a less reactive metal from its compound.

Define oxidation in terms of oxygen and electrons.

Gain of oxygen or loss of electrons.

Define reduction in terms of oxygen and electrons.

Loss of oxygen or gain of electrons.

What is a redox reaction?

A reaction in which both oxidation and reduction occur.

What is the role of an oxidising agent?

It causes another reactant to be oxidised and is itself reduced.

What is the effect of water and air on iron rusting?

Both air and water are necessary for iron to rust.

Name two methods to prevent rusting in iron.

Barriers (like painting) and galvanising.

How does galvanizing prevent rust?

A more reactive metal coats the iron, rusting first and preventing water and oxygen from reaching the iron.

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

The more reactive metal gradually disappears, and the less reactive metal coats its surface.

What are some barrier methods to prevent rusting?

Painting, coating with plastic, and using oil or grease.

Explain the term 'sacrificial protection'.

A more reactive metal is used to protect a less reactive metal from rusting.

What is a desiccant and how can it help prevent rusting?

A substance that absorbs moisture, keeping water away from the metal.

Describe the reaction of metals with dilute hydrochloric acid.

Metal + acid → hydrogen + salt, with observable H2 gas bubbles.

What is a characteristic observation when zinc reacts with dilute hydrochloric acid?

Large amounts of H2 gas bubbles.

What are the components of a reactivity series?

Metals arranged according to their reactivity with water, acids, and other substances.

Which metals primarily react with dilute acids?

Up to iron, only the more reactive metals will react with dilute acids.

Why is it important to understand metal reactivity?

To predict how metals will behave in various chemical reactions.

How are metal ions formed during a reaction?

When metal atoms lose electrons, they form positive ions.

What distinguishes metals from non-metals in the reactivity series?

Metals form positive ions and exhibit different reactivity profiles compared to non-metals.

Define the term 'metal oxide'.

A compound formed when a metal reacts with oxygen.

What is the significance of hydrogen in the context of metals and reactivity?

Hydrogen is included in the reactivity series, often as a reference point.

What do you need to remember about the reaction of gold in the reactivity series?

Gold does not react with water, acids, or oxygen due to its low reactivity.

How does temperature affect the rusting of iron?

Higher temperatures generally increase the rate of rusting due to increased reaction rates.

Why can potassium and sodium be considered very reactive metals?

Because they react vigorously with cold water to form hydroxides and release hydrogen gas.