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Y12 Chem > Metals And Reactivity Series > Flashcards

Metals And Reactivity Series Flashcards

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1
Q

Reactions of Na and K when left in air

A

These soft metals can be cut easily with knife to give a shiny surface which quickly tarnishes

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2
Q

Reactions of K and Na when heated in air

A

Burns with a lilac flame, forming a white solid

Burns with a yellow/orange flame, forming a white solid

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3
Q

Reactions of Ca, Mg, Al, Zn when left in air

A

Reacts slowly with the air forming a layer of oxide

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4
Q

Ca when heated in air

A

Burns with a brick red flame, leaving a white solid

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5
Q

Mg reacted when heated in air

A

Burns with a bright white flame leaving a white ash

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6
Q

Al reaction when heated in air

A

Sheets of aluminium do not burn easily. Powdered aluminium burns with white peaks leaving a white solid

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7
Q

Zn reaction when heated in air

A

Burns steadily, forming a yellow solid which when cooled changes to white

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8
Q

Reactions Fe and Cu when left in air

A

Oxide layer is easily rubbed off

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9
Q

Fe heated in air

A

Sheets of iron do not burn easily. Iron wool or iron filings burn with yellow/orange sparks forming a black solid

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10
Q

Cu heated in air

A

Sheets of red brown copper glows red and forms a black layer of copper oxide but does not burn. There may be a blue - green flame observed

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11
Q

Na reaction with water

A

Floats, moves rapidly around the surface. So much heat is released that Na melts and forms a sphere of molten metal

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12
Q

General equation for metal and water

A

Metal + water —> metal hydroxide + hydrogen

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13
Q

K reaction with water

A

Floats, moves rapidly around the surface. Bursts into lilac flame. Bubbles of gas released. Colourless solution formed. Heat is released. Potassium disappears at the end.

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14
Q

Further tests for K

A

Solution changes Universal Indicator from green to blue.

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15
Q

Ca reaction with water

A

Ca granules will sink initially then rises. Bubbles of gas evolved. Beaker feels warm to the touch as heat is evolved. Calcium disappears. Colourless solution with a white ppt (due to Ca(OH)2 which is only slightly soluble).

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16
Q

Mg reaction with water

A

Very few bubbles are observed even after leaving for several days.

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17
Q

Al, Fe, Zn and Cu reaction with water

A

No reaction

Iron will rust after a few days

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18
Q

General equation for reaction between water and metal

A

METAL + WATER —>METAL HYDROXIDE + HYDROGEN

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19
Q

Mg reaction with steam

A

Reacts when heated. Produces a very bright white light. Heat given out. A white powder remains.

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20
Q

Al reaction with steam

A

Aluminium foil will not react. Small pieces will react when the oxide layer is taken off. Aluminium powder reacts when heated to form a white powder. Heat is given out.

21
Q

Zn reaction with steam

A

Reacts when heated. Glows as steam is passed over producing a yellow powder. Heat is given out. Yellow powder becomes white when it is left to cool.

22
Q

Fe reaction with steam

A

Iron must be heated until it glows red before the steam is passed over. Reacts to form a black solid.

23
Q

General equation for metal and steam

A

METAL + STEAM —> METAL OXIDE + HYDROGEN

24
Q

Does copper react with water or steam?

A

Copper does not react with cold water or steam. It is used in plumbing.
Also metals below copper in the reactivity series, for example, silver and gold do not react with cold water or steam.

25
Q

Mnemonic for reactivity series

A 
Please - K
Send- Na
Little - Li
Charlie's - Ca
Monkeys - Mg
And - Al
Coloured - C 
Zebras - Zinc
In - Fe
Tin - Sn
Cages - Cu
Securely - Ag 
Guarded - Au
26
Q

Write the half equation for this :

Symbol equation Zn + 2HCl —> ZnCl2 + H2

A

Zn —> Zn 2+ + 2e-

27
Q

Write the half equation for this

Symbol equation 2Mg + O2 —> 2MgO

A

Mg —> Mg 2+ + 2e-

28
Q

Explain what happens to the calcium atoms in the reaction of water and metal in terms
of electrons.

A

The calcium atoms lose electrons

29
Q

Write half equations for sodium and potassium

A

Na—> Na+ +e-

K —> K+ +e-

30
Q

Define a displacement reaction

A

A displacement reaction is one where a more reactive element displaces a less reactive element from its compound.

31
Q

Describe the beginning and end of an experiment using copper and silver nitrate

A

Beginning - Orange-brown copper wire placed in colourless solution.

End - The solution turns blue and the copper wire is coated with silver crystals.

32
Q

Describe the colour changes in these displacement reactions

magnesium + copper (II) sulfate

magnesium + iron (II) sulfate

iron + zinc sulfate

iron + copper (II) sulfate

zinc + copper(II) sulfate

zinc + magnesium sulfate

A

blue solution turned colourless and a
solid formed.

pale green solution turned colourless and a
solid formed

no reaction

blue solution went pale green and a solid
formed.

blue solution turned colourless and a
solid formed.

no reaction

33
Q

Which one of the four metals above forms a black layer of metal oxide when it is strongly heated in the air?

A

Copper forms a black layer of copper oxide when it is strongly heated in the air.

34
Q

Define ore

A

Definition : An ore is a rock that contains a metal compound from which the metal can be extracted.

35
Q

Two methods of extraction to obtain metals from ores:

A

Electrolysis

Reduction using carbon

36
Q

Define phytomining

A

Phytomining is the use of plants to absorb metal compounds from soil as part of metal extraction.

37
Q

Describe the process of phytomining (6)

A
  • Some plants such as rapeseed are very good at absorbing metal compounds from the ground through their roots.
  • These plants are grown on ground that contains low-grade ores, and so the metal is removed from the ore and enters the plant.
  • The plants are harvested, dried and then burned to produce an ash, which is rich in metal compounds.
  • An acid such as sulfuric acid is added to the ash and insoluble metal compounds react to produce a solution containing soluble copper compounds.
  • The solution is called a ‘leachate’.
  • The metal can then be obtained by adding scrap iron to the leachate solution, and a displacement reaction will occur
38
Q

What is the solution containing soluble metal compounds produced from phytomining called?

A

leachate

39
Q

Name two disadvantages for traditional methods

A

Traditional methods involve digging, moving and disposing of large quantities of rock.
- This involves noise and dust pollution, and uses large amounts of energy to move and transport the rock.

40
Q

Explain how the reactivity of metals is related to the tendency of a metal to form its positive ion

A

The reactivity of a metal depends on the tendency of the metal to lose outer shell electrons and form its positive ion
The greater the tendency to lose outer shell electrons the more reactive the metal

40
Q

explain and describe the displacement reactions of metals with other metal ions in solution (4)

A
  • When solid Metal compounds are heated with a solid metal, a displacement reaction can occur
  • This is a redox reaction
  • They are carried out in a crucible where both the metal and metal oxide are in powder form to increase contact between them
  • The further apart the metals in the reactivity series the faster and more exothermic the reaction
40
Q

How are metals high in the reactivity series extracted from metal ores ?

A

Metals high in the reactivity series are extracted by electrolysis

41
Q

How are metals low in the reactivity series removed from their ores ?

A

Reduction with carbon or carbon monoxide

42
Q

Which metals are extracted by electrolysis

A

Aluminium and metals above it

43
Q

Equation for reaction between scrap iron and copper ii Sulfate

A

Fe + CuSO4 —> FeSO4 + Cu

44
Q

Two advantages to phytomining

A
  • Its less destructive than traditional mining methods

- Carbon dioxide is absorbed as the plants grow

45
Q

Disadvantages of phytomining (2)

A
  • It is a slow process – time is needed for plants to grow

- Less Copper is extracted

46
Q

How must sodium, potassium and calcium be heated in air?

A

Under very careful supervision. Reactions can be dangerous

Y12 Chem (16 decks)

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