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Chemistry > Reactivity Series > Flashcards

Reactivity Series Flashcards

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1
Q

Define a metal

A

Metals are elements which lose electrons to form positive ions

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2
Q

Define a metallic bond

A

A metallic bond is the electrostatic forces of attraction formed between positive metal ions and a ‘sea’ of free-moving valence electrons

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2
Q

Why are alloys used over pure metals

A
  • Alloys are harder and stronger
  • Alloys do not corrode when reacting with oxygen and water
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3
Q

Define an alloy

A

An alloy is a mixture of a metal and one or more other elements

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3
Q

Name the reactivity series

A

PSCMAZILCSG

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3
Q

What are the properties of a metal ‘high up’ in the reactivity series

A
  • Reacts quickly and vigorously
  • Corrodes easily
  • Loses electrons readily to form positive ions
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4
Q

Why are alloys harder and stronger than pure metals

A
  • Atoms of added element have different size than atoms of pure metal
  • This disrupts the orderly arrangement of atoms in pure metal
  • Much harder for atoms to slide over one another without orderly arrangement of atoms
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5
Q

What are the properties of a metal ‘low down’ in the reactivity series

A
  • React slowly
  • Do not corrode easily
  • Do not lose electrons readily to form positive ions
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5
Q

What is formed when a metal reacts with cold water

A
  • Hydrogen gas
  • Metal hydroxide
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6
Q

What is formed when a metal reacts with steam

A
  • Hydrogen gas
  • Metal oxide
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7
Q

Why does aluminium not react with water or steam

A

Aluminium is covered in a layer of non-porous aluminium oxide, which adheres strongly to the metal and prevents it from reacting

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8
Q

Which metals do not react with cold water or steam

A
  • Aluminium
  • Lead
  • Copper
  • Silver
  • Gold
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8
Q

What forms when iron reacts with steam

A
  • Hydrogen gas
  • Iron (II,III) oxide (Fe3O4)
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9
Q

Why does aluminium not react at first with HCl, and what happens after

A
  • Aluminium is covered in a layer of non-porous aluminium oxides, which adheres strongly to the metal and prevents it from reacting
  • HCl will react with aluminium oxide to form water and soluble aluminium chloride
  • Aluminium metal is exposed once oxide layer is washed away
  • Reaction between acid and aluminium metal is rapid
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10
Q

Why does reaction between lead and HCl stop before completion

A
  • Insoluble lead(II)chloride will form
  • It will coat onto surface of lead metal and prevent further reaction between acid and metal
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11
Q

Give an example of a thermit reaction

A

A more reactive metal will displace a less reactive metal from its metal oxide

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11
Q

Reaction for decomposition of metal carbonates

A

Metal carbonate
–> Metal oxide + Carbon dioxide
Exception: Silver

11
Q

What is a thermit reaction

A

A thermit reaction is when a great amount of heat is released during a reaction

11
Q

Explain the displacement of metals from metal salt solution

A

A more reactive metal will displace a less reactive metal from its salt solution

12
Q

Reaction for reduction with carbon

A

Metal oxide + Carbon
–> Metal + Carbon dioxide

12
Q

Which metal carbonates cannot be decomposed by heat

A
  • K2CO3
  • Na2CO3
13
Q

Reaction for reduction with hydrogen

A

Metal oxide + Hydrogen
–> Metal + Water

13
Q

Which metal carbonates require very strong heating to decompose

A
  • CaCO3
14
Q

Which metal carbonates require moderate heating to decompose

A
  • MgCO3
  • ZnCO3
  • FeCO3
  • PbCO3
14
Q

Which metal carbonates require gentle heating to decompose

A
  • CuCO3
  • Ag2CO3
15
Q

What does silver carbonate decompose into

A
  • Silver metal
  • Oxygen
  • Carbon dioxide
16
Q

What are ores

A

Ores are compounds of metals mixed with large amounts of impurities

16
Q

How does reactivity affect thermal stability of its carbonate

A

The more reactive the metal, the more thermally stable its carbonate is

17
Q

What are the methods for extraction of metals

A
  • Electrolysis
  • Reduction of metal oxide with carbon
18
Q

Which metals can only be extracted by electrolysis

A
  • Potassium
  • Sodium
  • Calcium
  • Magnesium
  • Aluminium
19
Q

Which metals are extracted by reduction of their metal oxides with carbon

A
  • Zinc
  • Iron
  • Lead
  • Copper
  • Silver
20
Q

What does it mean when gold is unreactive

A

Gold is found naturally uncombined in the ground as an element

20
Q

Which metals are unreactive

A

Gold

21
Q

How are very reactive metals extracted

A
  • Always exist in compounds with strong chemical bonds
  • Electrolysis is used to break down molten ionic compounds
21
Q

How are moderately reactive metals extracted

A
  • Found as oxides or sulfides
  • Sulfides heated in air to form oxides
  • Oxides reduced with carbon to form the metal and carbon dioxide
22
Q

Define rusting

A

Rusting is the slow oxidation of iron to form hydrated iron(III)oxide in the presence of air and water

22
Q

What is needed for rusting to occur

A
  • Air
  • Water
23
Q

What can be added to increase the speed of rusting

A
  • Sodium chloride
  • Acidic substances
24
Q

What are the main methods of rust prevention

A
  • Protective layer
  • Sacrificial metal
  • Alloys
25
Q

How to use a protective layer to prevent rusting

A
  • Painting
  • Oiling
  • Plastic coating
  • Chrome plating
26
Q

How can a sacrificial metal prevent rusting

A

Galvanising (Zinc plating)
- Zinc, being more reactive than iron, loses electrons more readily than iron hence zinc corrodes in place of iron

27
Q

How can using alloys prevent rusting

A

Stainless steel

Chemistry (16 decks)

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