6092 Chapter 15 The Reactivity Series

Open Ended

What is reactivity of metals?

Explanation Slide...

Tendency (How readily) of an atom of metal to lose one or more electron(s) to form its positive ion.

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The ​

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reactive a metal, the greater the tendency for an atom of a metal to

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electron(s) to another reactant to form its positive

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and hence the greater the tendency for the metal to be

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. Hence a more reactive metal is a stronger

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.

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The ​

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reactive a metal, the ​

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the tendency for an atom of a metal to ​

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electron(s) to another reactant to form its positive ion and hence the lower the tendency for the metal to be ​

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. Hence a less reactive metal is a weaker ​​

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.

Multiple Select

Which of the following are the products when metals react with water?

• metal hydroxide

• hydrogen gas

• metal oxide

• salt

• oxygen gas

Multiple Select

Which of the following are the products when metals react with steam?

• metal hydroxide

• hydrogen gas

• metal oxide

• salt

• oxygen gas

Multiple Select

Which of the following are the products when metals react with acid?

• metal hydroxide

• hydrogen gas

• metal oxide

• salt

• oxygen gas

Match

Match the following observation for the respective reaction between metal and water.

• Reacts explosively with cold water. Potassium darts around rapidly on the water surface and burns with a lilac flame.

• Reacts violently with cold water. Reaction may be explosive. Sodium darts around on the water surface and burns with an orange flame.

• Reacts rapidly with cold water. Vigorous bubbling is observed.

• Reacts very slowly with water.

• No visible change

potassium

sodium

calcium

magnesium

zinc

• potassium

• sodium

• calcium

• magnesium

• zinc

Match

Match the following observation for the respective reaction between metal and steam.

• Reactions are highly explosive. These reactions should not be conducted in the school laboratory.

• reacts violently with steam. A bright white glow is observed during the reaction

• reacts readily with steam.

• reacts slowly with steam under continuous heating.

• No visible change

calcium

magnesium

zinc

iron

lead

• calcium

• magnesium

• zinc

• iron

• lead

Match

Match the following observation for the respective reaction between metal and acids.

• Reactions are highly explosive. These reactions should not be conducted in the school laboratory.

• Reacts rapidly with dilute hydrochloric acid. Vigorous bubbling is observed.

• Reacts violently with dilute hydrochloric acid.

• Reacts moderately fast with dilute hydrochloric acid.

  Effervescence is observed.

• Reacts slowly with dilute hydrochloric acid.

sodium

magnesium

calcium

zinc

iron

• sodium

• magnesium

• calcium

• zinc

• iron

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Zinc is a

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metal which reacts readily with

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in air to form zinc oxide. Thus

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is not observed immediately when zinc is mixed with dilute acid as zinc is coated with a layer of zinc oxide. Zinc oxide will react with acid first to form a solution of

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and water before zinc can react with the acid to form

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.

Categorize

Options (9)

Mg

K

Ca

Na

Zn

Fe

Cu

Pb

Ag

Select from the following metals: Mg, K, Ca, Na, Zn, Fe, Cu, Pb, Ag.

Which metals can react with cold water?        

Reactive with cold water

non-reactive with cold water

Categorize

Options (9)

Mg

K

Ca

Na

Cu

Pb

Ag

Zn

Fe

Select from the following metals: Mg, K, Ca, Na, Zn, Fe, Cu, Pb, Ag.

Which metals can react with steam?                    

Reactive with steam

non-reactive with steam

Categorize

Options (9)

Mg

K

Ca

Na

Cu

Ag

Zn

Fe

Pb

Select from the following metals: Mg, K, Ca, Na, Zn, Fe, Cu, Pb, Ag.

Which metals can react with acids?                    

Reactive with cold acid

non-reactive with acids

Multiple Select

Which of the following statements are true?

• Magnesium forms positive ions more readily than copper.

• Magnesium has a stronger metallic bond than copper.

• Magnesium gives away electrons more readily than copper.

• Magnesium is a stronger oxidizing agent than copper.

• Magnesium is a strong reducing agent than copper.

Open Ended

Predict what will be observed when aluminum is added to cold water. Explain your answer. [2]

Explanation Slide...

No visible change.[1]Aluminium is a reactive metal which reacts readily with oxygen in air to form an *insoluble layer of aluminium oxide which coats aluminium. This layer of oxide does not react with water and also prevents aluminium beneath from reacting with water.[1]

Open Ended

When aluminum is mixed with dilute hydrochloric acid, effervescence is only observed after a few seconds. Explain why. [2]

Explanation Slide...

Aluminium is a reactive metal which reacts readily with oxygen in air to form a layer of aluminium oxide which coats aluminium.[1]This layer of oxide will react with dilute hydrochloric acid first to form a solution of aluminium chloride and water before aluminium beneath the oxide layer can react with the acid to form hydrogen gas.[1]

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• The greater the tendency for metal to

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to form its positive ions achieve stable electronic configuration of

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, the

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the metal. Thus, a more reactive metal has a greater tendency to undergo reactions to form compound than a ​

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metal. In the compound of a reactive metal, the metal ions have stable electronic configuration of noble gas. Thus, these ions do not take part in further chemical reactions readily.

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• Hence, the

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a metal is, the ​

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the compounds of a metal to chemical reactions thus the

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for these compounds to undergo chemical reactions. The ​

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a metal is, the less stable the compounds of a metal to chemical reactions thus the ​

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for these compounds to undergo chemical reactions.

Open Ended

What is a displacement reactions of a metal? (Redox reaction)

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+ compound of ​

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--> ​

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of less reactive metal + ​

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of more reactive metal

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more reactive metal

less reactive metal

element

compound

mixture of gases

solid solution

aqueous solution

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General Ionic Equation of Displacement Reactions of Metals:



atoms of ​

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metal + cation of ​

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metal --> ​

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of less reactive metal + ​

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of more reactive metal

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more reactive

less reactive

atom

cation

anion

ion

inert

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Atoms of more reactive metal are ​

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to form cations (positive ions) by ​

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electrons to the cations of ​

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metal in the compound. The cations of less reactive metal in the compound are ​

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to form atoms by ​

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electrons from the atoms of more reactive metal.

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oxidized

losing

less reactive

reduced

gaining

more reactive

inert

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Reactions of ​

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metals with aqueous solutions of ​

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(contains cations of less reactive metals)

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Reactions of ​

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metals with ​

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of ​

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metals. This type of reaction is also known as ​

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reaction.

Match

Match the metals / compounds of metal with their physical appearance.

• silver solid

• pink solid (when freshly formed) or red-brown solid

• silver liquid

• white solid, colourless solution

• white solid (when cold) & yellow solid (when hot)

most metals

copper

mercury

Compound of Group I – III metals

zinc oxide

• most metals

• copper

• mercury

• Compound of Group I – III metals

• zinc oxide

Match

Match the metals / compounds of metal with their physical appearance.

• yellow solution (colour intensity increases as concentration of ions of metal increases)

• red- brown solid (red-brown precipitate)

• green solution (colour intensity increases as concentration of ions of metal increases)

• dark green solid (dark green precipitate)

• white solid, colorless solution

aqueous compounds of iron(III)

Iron(III) oxide/hydroxide

aqueous compounds of iron(II)

Iron(II) hydroxide

other compounds of zinc

• aqueous compounds of iron(III)

• Iron(III) oxide/hydroxide

• aqueous compounds of iron(II)

• Iron(II) hydroxide

• other compounds of zinc

Match

Match the metals / compounds of metal with their physical appearance.

• blue solid, blue solution

• white solid, colourless solution (aq)

• white solid

• black powdery solid

• purple solution

other compounds of copper

silver nitrate

silver chloride

manganese(IV) oxide

acidified potassium

 manganate(VII)

• other compounds of copper

• silver nitrate

• silver chloride

• manganese(IV) oxide

• acidified potassium

   manganate(VII)

Multiple Select

Which statements describe what was observed when magnesium is placed in a beaker of copper(II) sulfate solution.

• Magnesium metal is coated with pink/reddish-brown deposit.

• Blue solution turns colourless.

• colourless solution turn blue

• Reaction mixture becomes warm.

• Reaction mixture becomes cold.

Open Ended

Explain the observations when magnesium is placed in a beaker of copper(II) sulfate solution. A chemical change occurred. [4]

Explanation Slide...

Magnesium is a more reactive metal than copper as magnesium loses electrons to form its positive ions more readily. A displacement reaction will take place between Mg and CuSO4.[1]Magnesium displaces copper from blue copper(II) sulfate solution to form colourless magnesium sulfate solution and copper which is the pink deposit. [1]The blue colour of copper(II) sulfate solution fades gradually as the concentration of copper(II) ions in the reaction mixture decreases as reaction progresses. [1]As displacement reactions are *exothermic thus this reaction gives out heat to the surroundings causing the reaction mixture to become warm. [1]

Open Ended

zinc reacted with copper(II) oxide to produce a reddish-brown solid.

This reaction gives out a lot of light energy and heat. Explain the observations. [4]

Multiple Select

When a piece of magnesium ribbon is added to aqueous iron(III) sulfate, a chemical change

occurred. Predict the observation

• Magnesium ribbon is coated with silver deposit.

• Yellow solution turns colourless.

• Reaction mixture becomes warm.

• colorless solution turn yellow.

• Magnesium ribbon is coated with red-brown deposit

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Reduction of metal oxides with carbon



​

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​ + ​ ​

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--> ​ + ​ ​

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​

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carbon

metal oxide

metal

carbon dioxide

oxygen

metal carbonate

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Reduction of metal oxides with hydrogen gas



​

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+ ​

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--> ​

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+ ​

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metal oxide

hydrogen

metal

steam

water

oxygen

carbon

metal hydroxide

Categorize

Options (9)

Zn

Fe

Cu

Pb

Ag

Mg

K

Ca

Na

Organize the following metals: Mg, K, Ca, Na, Zn, Fe, Cu, Pb, Ag into the right categories.

metal whose oxide can be reduced by C

metal whose oxide cannot be reduced by C

Categorize

Options (9)

Fe

Cu

Pb

Ag

Mg

K

Ca

Na

Zn

Organize the following metals: Mg, K, Ca, Na, Zn, Fe, Cu, Pb, Ag into the right categories.

metal whose oxide can be reduced by H

metal whose oxide cannot be reduced by H

Multiple Choice

Which oxide can be reduced to the metal by heating with carbon?

• calcium oxide    

• magnesium oxide

• potassium oxide

• zinc oxide  

Multiple Select

Which oxides can be reduced to the metal by heating with hydrogen gas?

• copper(II) oxide

• iron(III) oxide

• lead(II) oxide

• zinc oxide

Open Ended

The reaction between copper(II) oxide and hydrogen gas is a redox reaction. Predict what will be observed when this reaction takes place.

Explanation Slide...

Black powdery solid [copper(II) oxide)] turned pink (freshly formed copper) or reddish – brown.

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The reaction between copper(II) oxide and hydrogen gas is a redox reaction. Identify the oxidising and reducing agents in this reaction. Explain your reasoning in terms of oxidation state.

CuO is an ​

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agent.

CuO caused H₂ to be oxidised by ​

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the oxidation state of

hydrogen from ​

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in H₂ to ​

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in H₂O. [1]

Drag and Drop

The reaction between copper(II) oxide and hydrogen gas is a redox reaction. Identify the oxidising and reducing agents in this reaction. Explain your reasoning in terms of oxidation state.

H₂ is a ​

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agent.

H₂ caused copper in CuO to be ​

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by ​

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the oxidation state of

copper from ​

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in CuO to ​

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in Cu. [1]

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reducing

reduced

decreasing

+2

0

oxidized

oxidizing

increasing

-2

+1

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Thermal Decomposition of Metal Carbonates

General Equation (include SS) does not apply to silver carbonate

metal carbonate (s)  -->  ​

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(s)  +  ​

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(g)

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metal oxide

carbon dioxide

metal hydroxide

hydrogen gas

oxygen gas

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Carbonates of these ​

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metals are less stable to thermal decomposition. These metal carbonates will decompose to form ​

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and ​

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upon strong heating. As reactivity of metals ​

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, thermal stability of metal carbonates decreases thus ease of thermal decomposition of metal carbonates ​

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.

Categorize

Options (9)

Silver

calcium

magensium

zinc

iron

lead

copper

potassium

sodium

Organize these options into the right categories

No decomposition of metal carbonate

decomposition of metal carbonates

decomposed to form metal, oxygen and CO2

Drag and Drop

A sample of silver carbonate is heated strongly and a chemical change occurs. Is this a redox reaction? Explain your reasoning in terms of oxidation state.



Oxygen in Ag₂CO₃ is ​

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as the oxidation state of oxygen ​

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from ​

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in Ag₂CO₃ to ​

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in O₂. [1] 

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oxidised

increases

-2

0

-1

+2

decrease

reduced

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We learnt previously that compounds of more reactive metals are more stable compared to compounds of less reactive metals. Hence ​

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metals are more difficult to extract and ​

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metals are easier to extract from their ores. ​

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of the molten compounds/ores is used to extract more reactive metals.

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more reactive

less reactive

Electrolysis

less stable metals

more stable metals

Chemical reduction

Categorize

Options (10)

gold

silver

zinc

iron

lead

copper

potassium

sodium

calcium

magnesium

Organize these metals into the recommended method of extraction

electrolysis of molten compound/ore

reduce metal oxide in ore with carbon

heating the ore alone

usually found naturally uncombined

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The slow ​

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of iron to form hydrated ​

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. Rusting is also known as the ​

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of iron

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oxidation

iron(III) oxide

corrosion

iron(II) oxide

reduction

decomposition

Multiple Choice

What is rust?

• Hydrated iron(III) oxide

• Hydrated iron(II) oxide

• Hydrated copper(II) oxide

• Hydrated copper(I) oxide

Open Ended

What is the conditions required for rusting to occur?

Explanation Slide...

(i)             Water (ii)           oxygen

Multiple Select

Which factors which increases the speed of rusting?

• Presence of salt

• Presence of acidic substances

• Increased pressure

• increased concentration