Chapter 15 - The Reactivity Series Flashcards
In the reactivity series, how are metals arranged?
From most reactive to least reactive
State all the metals of the reactivity series (include the 2 non metals)
1) Potassium Please
2) Sodium Stop
3) Calcium Calling
4) Magnesium Me
5) Aluminium A
6) Carbon Cute
7) Zinc Zebra
8) Iron I
9) Tin Totally
10) Lead Like
11) Hydrogen Hwa
12) Copper Chong
13) Silver Sexy
14) Gold Girls
15) Platinum Period
The order of reactivity can be determined by the ____ of reactions of metal with ____, ____, ____?
1) Cold water
2) Steam
3) Dilute hydrochloric acid
When a metal reacts with cold water what are the products?
Metal hydroxide + Hydrogen
What is a hydroxide?
A compound that contains a metal ion (e.g., Na⁺, K⁺, Ca²⁺) and hydroxide ions (OH⁻)
What are the 4 metals that react with cold water?
Potassium, Sodium, Calcium, Magnesium
Zinc to silver no reaction
How does potassium react with cold water?
Reacts extremely violently to form potassium hydroxide and hydrogen gas. Enough heat is produced to cause hydrogen gas to catch fire and explode
2K(s) + 2H2O (l) –> 2KOH (aq) + H2 (g)
How does sodium react with cold water?
Reacts violently to form sodium hydroxide and hydrogen gas. Hydrogen gas may catch fie and explode
2Na(s) + 2H2O(l) —> 2NaOH (aq) + H2 (g)
How does calcium react with cold water?
Reacts readily to form calcium hydroxide and hydrogen gas
Ca(s) + 2H2O(l) —> Ca (OH)2(aq) + H2(g)
How does magnesium react with cold water?
Reacts very slowly with cold water to form magnesium hydroxide and hydrogen gas. A test tube of hydrogen gas is produced after a few days
Mg(s) + 2H2O (l) —> Mg(OH)2(s) + H2(g)
Most reactive metals can react with ____ and ____
Moderate reactive metals can only react with ____
Least reactive metals cant react with ____
Most reactive metals can react with cold water and steam
Moderate reactive metals can only react with steam
Least reactive metals cant react with both
What are the products when metal and steam react?
Metal oxide + Hydrogen gas
What is a metal oxide?
A metal oxide is a compound containing a metal ion (e.g., Mg²⁺, Fe²⁺, Al³⁺) and oxygen (O²⁻) ions
How does potassium react with steam?
Reacts explosively
How does sodium react with steam?
Reacts explosively
How does calcium react with steam?
Reacts explosively
How does magnesium react with steam?
Hot magnesium reacts violently with steam to form magnesium oxide and hydrogen gas. A bright white glow is produced during the reaction
Mg(s) + H2O(g) —> MgO(s) + H2(g)
How does zinc react with steam?
Hot zinc reacts readily with steam to produce zinc oxide and hydrogen. Zinc oxide is yellow when hot and white when cold
Zn(s) + H2O(g) —> ZnO(s) + H2(g)
How does iron react with steam?
Red-hot iron reacts slowly with steam to form iron oxide. The iron must be constantly heated for the reaction to progress
3Fe(s) + 4H2O(g) <—–> Fe3O4(s) + 4H2
What are the metals that react with steam?
Potassium, sodium, calcium, magnesium, zinc, iron
Lead to silver no reaction
What are the metals that react with dilute hydrochloric acid?
Potassium, sodium, calcium, magnesium, zinc, iron
Lead to silver no reaction
How does potassium react with HCl?
Reacts explosively
How does sodium react with HCl?
Reacts explosively
How does calcium react with HCl?
Reacts violently to give hydrogen gas
How does magnesium react with HCl?
Reacts rapidly to give hydrogen gas
How does zinc react with HCl?
Reacts moderately fast to give hydrogen gas
How does iron react with HCl?
Reacts slowly to give hydrogen gas
How does lead react with HCl?
The initial reaction between lead and HCl forms an insoluble layer of lead(II) chloride which coats the lead and prevents further rection. Hence lead does not appear to react with HCl
All metals above ____ react with dilute HCl to produce ____ ____
hydrogen, hydrogen gas
What can the reactivity series be used to predict?
1) The behavior of a metal from its position in the reactivity series
2) Position of an unfamiliar metal in the reactivity series from a given set of experimental results
What is reduction of metal with carbon?
- This process is used to extract metals from their oxides by removing oxygen from the metal oxide.
- Carbon is more reactive than some metals, so it can take away oxygen from metal oxides, leaving behind pure metal.
- Carbon is oxidised (gains oxygen and metal is reduced (lose oxygen)
What is the word equation to represent the reduction of metal oxides with carbon?
Metal oxide + carbon —>(heat) —> Metal + Carbon dioxide
Only metal oxides below ____ can be reduced by carbon
carbon
What is the relationship between position of metal in the reactivity series and how readily the reduction of metal occurs?
The lower the metal is in the reactivity series from carbon ,the more readily the reduction of metal oxide will occur
What is reduction of metal with hydrogen?
- Hydrogen can also be used to reduce metal oxides.
- Instead of carbon taking the oxygen, hydrogen does takes oxygen, forming water (H₂O) instead of CO₂ or CO.
- Used for metals that react too easily with carbon
- Carbon is oxidised (gains oxygen) and metal oxide is reduced (lose oxygen)
What is the word equation to represent reduction of metal oxides with hydrogen?
Metal oxide + hydrogen —> Metal + steam
Hydrogen is able to reduce oxides of metals from ____ and below
iron
A ____ reactive metal has a ____ tendency to form ____ compared to a less reactive metal
A more reactive metal has a greater tendency to form cations compared to a less reactive metal. (This is why when potassium reacts with water, it loses electrons readily to form positive ions
What kind of metals can displace what kind of metal from its salt solution?
More reactive metals can displace any less reactive metal
What is the relationship between the reactiveness of a metal whether they gain or lose electrons
- The atoms of a more reactive metal loses electrons to form positive ions that enter the solution
- The ions of a less reactive metal in the solution gain electrons and are discharged as atoms of an element
(e.g. Iron displaces copper from copper(II) sulfate, forms iron (II) sulfate. BUT if copper foil is dipped into iron (II) sulfate, no reaction occurs)
A more ____ metal in the reactivity series can displace a less ____ metal from its oxide
reactive
- Atoms of a more reactive metal loses electrons to form positive ions to combine with oxygen
- ions of the less reactive metal in the oxide gains electrons and are discharged as atoms of an element
How does magnesium react with zinc nitrate?
Solution remains colourless. Grey deposit of zinc formed on magnesium
How does magnesium react with copper(II) nitrate?
Solution remains colourless. Red-brown deposit of copper formed on magnesium
How does magnesium react with lead(II) nitrate?
Solution remains colourless. Grey deposited of lead formed on a magnesium
How does magnesium react with iron(II) nitrate?
Pale green solution turns colourless. Grey deposit of iron formed on magnesium
How does zinc react with magnesium nitrate?
No change is observed
How does zinc react with copper (II) nitrate?
Blue solution turns colourless. Red-brown deposit of copper formed on zinc
How does zinc react with lead (II) nitrate?
Solution remains colourless. grey deposit of lead formed on zinc
How does zinc react with iron (II) nitrate?
Pale green solution turns colourless. Grey deposit of iron formed on zinc
How does copper react with any nitrate?
No change is observed
How does lead react with magnesium nitrate?
No change is observed
How does lead react with zinc nitrate?
No change is observed
How does lead react with copper (II) nitrate?
Blue solution turns colourless. Red-brown deposit of copper formed on lead
How does lead react with lead (II) nitrate?
No change is observed
How does lead react with iron (II) nitrate?
No change is observed
How does iron react with magnesium nitrate?
No change is observed
How does iron react with zinc nitrate?
No change is observed
How does iron react with copper (II) nitrate?
Blue solution turns pale green. Red-brown deposit of copper formed iron
How does iron react with lead (II) nitrate?
Colourless solution turns pale green. Green deposit of lead formed on iron
Why is a metal displacement reaction a redox reaction?
The more reactive metal is oxidised while the less reactive metal is reduced
(e.g.
Mg(s) + Cu2(aq) + –> Mg2+ (aq) + Cu(s)
Magnesium oxidised, copper reduced)
When a displacement of metal occurs, what changes can be observed?
1) Deposit of solid metal
2) Colour of solution changes
A more reactive metal can ____the oxide of a less reactive metal
reduce
The atoms of a ____ reactive metal will lose electrons to form ____ to combine with oxygen
more, cations
The ions of a ____ reactive metal in the oxide will gain electrons and are ____ as atoms of an element
less, discharged
(e.g. Zinc forms cations more readily than copper. So in an experiment with a mixture of zinc powder and copper (II) oxide, zinc ions react with oxygen ions from copper (II) oxide to form zinc oxide. If zinc oxide and copper powder were added together no reaction would occur. The more reactive metal DISPLACES the less reactive metal from its oxide)
If a carbonate compound is decomposed upon strong heating, what does it produce?
Oxide and carbon dioxide
(metal + carbonate (s) —> metal oxide (s) + carbon dioxide (g))
The more reactive the metal in the carbonate, the ____ the resistance to decompose by heating
greater. They are very heat stable
Carbonates containing ____ ____ ____/ higher up in the reactivity series are generally heat stable and do not ____ easily upon strong heating
Carbonates containing group 1 metals are generally heat stable and do not decompose easily upon strong heating
The carbonates of metals below ____ in the RS decompose to form ____ and ____
The carbonates of metals below sodium in the RS decompose to form oxides of metals and carbon dioxide
For ____ carbonate, the ____ oxide is thermally unstable which further decomposes to form ____
silver
Ores exist as what?
Oxides, carbonates, sulfides
What are the 2 ways to extract metals from ores?
Reducing the metal compound to the metal using carbon
Electrolysis
Metals ____ in the RS, compounds are very ____ to break down
high, difficult (only done by electrolysis). While those in the mid to bottom can be extracted by reducing their oxides with carbon
What is the word equation for reduction of metallic oxides with carbon?
Oxide of metal + Carbon —> Metal + Carbon dioxide
What is the chemical name for rust?
Hydrated iron (III) oxide
Rust only occurs in the presence of ____ and ____
Water and oxygen
What is the word equation for rusting?
Iron + Oxygen + water —> Hydrated iron (III) oxide
Is rusting oxidation or reduction?
Oxidation. Iron gains oxygen
Rust is formed on the surface of iron and steel objects that ….
easily crumbles into a powder. When the rust flakes are off, more iron exposed to form rust until metal is destroyed
When does speed of rusting increase?
When salt or acidic condition is present
What are the 2 ways to prevent rusting?
1) Barrier method
2) Sacrificial protection
What are the methods to provide a barrier by forming a protective layer by preventing water and oxygen from coming into contact with iron?
1) Painting (large objects)
2) Greasing (machinery)
3) Plastic coating (small objects)
4) Tin-Plating (used in food containers)
5) Chrome-Plating
What is sacrificial protection?
Protection of iron and steel against rusting by using a more reactive metal like zinc
What are some sacrificial protection methods?
1) Galvanising (dip iron into molten zinc to coat the iron and protect the iron by corroding in place of the iron)
2) Attaching a more reactive metal (attaching blocks of more reactive metal such as zinc to iron to corrode in place of iron)
