Year 10 Chemistry: Reactivity Topic

Vocabulary flashcards covering the reactivity series, extraction methods, reactions with water, acids, and oxygen, displacement, rusting, and redox chemistry from Year 10 Chemistry notes.

Reactivity Series

A list of metals ordered from most to least reactive (Potassium, Sodium, Lithium, Calcium, Magnesium, Aluminium, Zinc, Iron, Copper, Silver, Gold), where metals higher in the series react more easily.

Displacement Reaction

A reaction in which a more reactive metal replaces or displaces a less reactive metal from its compound.

Carbon Reduction

A method often used to extract metals positioned below carbon in the reactivity series.

Electrolysis

A metal extraction method usually required for metals positioned above carbon in the reactivity series.

Reaction of Metals with Water

A chemical reaction following the general word equation: $\text{Metal} + \text{Water} \rightarrow \text{Metal hydroxide} + \text{Hydrogen}$.

Reaction of Metals with Oxygen

A chemical reaction following the general word equation: $\text{Metal} + \text{Oxygen} \rightarrow \text{Metal oxide}$.

Reaction of Metals with Acids

A reaction following the general equation: $\text{Metal} + \text{Acid} \rightarrow \text{Salt} + \text{Hydrogen}$, occurring only for metals positioned above hydrogen in the reactivity series.

Rusting

The corrosion of iron that occurs only when both oxygen and water/moisture are present.

Rust

Hydrated iron(III) oxide.

Galvanising

A rust prevention method that coats iron with zinc, preventing oxygen and water from reaching the iron and reacting first because zinc is more reactive.

Sacrificial Protection

A rust prevention method where a more reactive metal is used to protect iron.

Oxidation

The gain of oxygen or the loss of electrons.

Reduction

The loss of oxygen or the gain of electrons.

Redox Reactions

Reactions in which oxidation and reduction take place together simultaneously.

Observation Questions (Exam Rule)

Exam questions requiring only visible occurrences (e.g., fizzing/effervescence, gas bubbles, colour changes, deposits, solids forming or dissolving) and strictly avoiding unseen chemical statements such as "hydrogen is produced".

Explain Questions (Exam Rule)

Exam questions requiring three specific parts: a reactivity comparison, a displacement or electron explanation, and the product formed.

Reactivity Series

A ranking of metals from most to least reactive (Potassium, Sodium, Lithium, Calcium, Magnesium, Aluminium, Zinc, Iron, Copper, Silver, Gold), where the higher a metal is, the more easily it reacts.

Displacement Reaction

A chemical reaction in which a more reactive metal replaces or displaces a less reactive metal from its compound.

Carbon Reduction

A method used to extract less reactive metals positioned below carbon in the reactivity series.

Electrolysis

An extraction method usually required for very reactive metals that are positioned above carbon in the reactivity series and form strong compounds.

Metals above Hydrogen

Metals in the reactivity series (such as magnesium, zinc, and iron) that react with dilute acids to produce a salt and hydrogen gas.

Metals below Hydrogen

Metals in the reactivity series (such as copper and silver) that do not react with dilute acids.

Metal Reaction with Water

A reaction following the general equation: $\text{Metal} + \text{Water} \rightarrow \text{Metal hydroxide} + \text{Hydrogen}$.

Combustion of Magnesium

A reaction with oxygen where magnesium burns with a bright white flame to form a white powder called magnesium oxide ($2\text{Mg} + \text{O}_2 \rightarrow 2\text{MgO}$).

Oxidation of Copper

A slow reaction with oxygen that produces black copper oxide.

Metal Reaction with Acid

A reaction following the general equation: $\text{Metal} + \text{Acid} \rightarrow \text{Salt} + \text{Hydrogen}$.

Observations in Acid-Metal Reactions

Visible signs of reaction including fizzing/effervescence, bubbles of gas, the metal getting smaller/dissolving, and a potential increase in temperature.

Rusting

The corrosion of iron that takes place only when both oxygen and water/moisture are present.

Rust

The reddish-brown substance formed during the corrosion of iron, chemically known as hydrated iron(III) oxide.

Galvanising

A rust prevention method that coats iron with zinc; the zinc prevents oxygen and water from reaching the iron and reacts first because it is more reactive.

Oxidation

A chemical process characterized by the gain of oxygen or the loss of electrons.

Reduction

A chemical process characterized by the loss of oxygen or the gain of electrons.

Redox Reactions

Reactions in which oxidation and reduction occur simultaneously together.

Mass Gain during Heating of Magnesium

An observed increase in mass caused by oxygen from the air combining with magnesium to produce solid magnesium oxide.

Observations (Exam Question Rule)

What can be directly seen during a reaction (e.g., bubbles/fizzing, colour changes, deposits, solids forming or dissolving) rather than non-visible inferences such as stating 'hydrogen is produced'.