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GCSE Chemistry > Metals And Reactivity Series > Flashcards

Metals And Reactivity Series Flashcards

1
Q

What is the general equation for a metal reacting with air?

A

Metal + oxygen = metal oxide

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2
Q

How does K (potassium) react with air when heated?

A

Burns with lilac flame

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3
Q

How does Na (sodium) react with air when heated?

A

Burns with a bright yellow flame

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4
Q

How does Ca (calcium) react with air when heated?

A

Burns with a brick red flame

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5
Q

How does Mg (magnesium) react with air when heated?

A

Burns with a bright white flame leaving a white ash

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6
Q

How does Al (aluminium) react with air when heated?

A

Sheets do not burn easily.

Powdered aluminium burns with white sparks leaving a white solid.

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7
Q

How does Zn (zinc) react with air when heated?

A

Burns leaving a yellow solid which turns white when cooled.

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8
Q

How does Fe (iron) react with air when heated?

A

Sheets of iron do not burn quickly.

Iron wool or iron filings burn with yellow sparks leaving a black solid.

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9
Q

How does Cu (copper) react with air when heated?

A

Sheets of red brown copper glows red and forms a black layer of copper oxide.

May also be a blue-green flame.

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10
Q

What is the general equation for when more reactive metals react with water?

A

Metal + water -> metal hydroxide + hydrogen

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11
Q

How does K (potassium) react 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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12
Q

How does Na (sodium) react with water?

A

Floats, moves rapidly around the surface. So much heat released that Na melts into a sphere of molten metal. Sodium disappears. Colourless solution formed.

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13
Q

How does Ca (calcium) react with water?

A

Ca granules burn, bubbles of gas evolved. Beaker feels warm. Calcium disappears. Colourless solution with a white ppt Ca(OH)2

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14
Q

How does Mg (magnesium) react with water?

A

Very few bubbles even after several days.

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15
Q

How does Al (aluminium) react with water?

A

No reaction

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16
Q

How does Zn (zinc) react with water?

A

No reaction

17
Q

How does Cu (copper) react with water?

A

No reaction

18
Q

How does Fe (iron) react with water?

A

Rusts after a few days.

19
Q

What is the general equation for when a metal reacts with steam?

A

Metal + steam -> metal oxide + hydrogen

20
Q

How does Mg (magnesium) react with steam?

A

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

21
Q

How does Al (aluminium) react 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.

22
Q

How does Zn (zinc) react with steam?

A

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

23
Q

How does Fe (iron) react with steam?

A

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

24
Q

How is reactivity of metal related to their tendency to form positive ions?

A

More reactive metals have a greater tendency to lose electrons and form positive ions. The further the outer electron is from the nucleus then the more easily it is lost and the more reactive the metal is.

25
Q

What is a displacement reaction?

A

When a more reactive metal takes the place of a less reactive metal in a compound.

26
Q

List the reactivity series

A

K (please)
Na (send)
Li (little)
Ca (Charlie’s)
Mg (monkeys)
Al (and)
Zn (zebras)
Fe (in)
Sn (tin)
Cu (cages)

27
Q

What is an ore?

A

A rock which contains a metal compound from which the metal can be extracted.

28
Q

What two processes can be used to extract metals from ore?

A

Electrolysis (for metals more reactive than carbon).

Reduction via heating with carbon (for metals less reactive than carbon).

29
Q

What is Phytomining?

A

The use of plants to absorb metal compounds from soil as part of metal extraction.

30
Q

What steps are involved in phytomining?

A

Plants (e.g. rapeseed) are grown on ground that contains low-grade ores, 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. For example, to extract copper.

Fe (s) + Cu 2+ (aq) -> Fe 2+ (aq) + Cu (s)

The iron is more reactive than the copper and so the copper is displaced my the iron.

31
Q

What ire the advantages and disadvantages to phytomining?

A

Phytomining avoids the noise and dust pollen, and the large amount of energy required for traditional mining, thus is better for the environment. Energy is also produced as the plants are burned.

However, it is a slow process. Plants take time to grow and can only be harvested at certain times of the year.

32
Q

Explain how you would carry out an experiment testing how different metals react with water.

A

Cut a piece of sodium and place it in water. It is very soft and shiny when freshly cut. It shoot’s across the surface of the water, forms a small ball, floats, fizzes and dissolves.

Drip indicator solution into the water. Green blue, pH 7.7

Repeat with lithium and potassium. Lithium is less reactive than sodium and potassium is more reactive than sodium.

Collect a test tube and half fill with water. Add 4 granules of calcium and hold a second, dry test tube over it upside down to collect the gas evolved. Bubbles of gas are released and the test tube feels warm, exothermic reaction. Calcium sinks and rises.

Test the gas by inserting a lit splint into the test tube. Makes a squeaky pop, hydrogen.

Add 3 drops of indicator into the solution. It is green blue, an alkali.

Repeat the experiment using magnesium. Less reactive, bubbles of hydrogen gas form slower. More vigorous with steam.

33
Q

How would you test the reactivity of iron?

A

Half full separate test tubes with copper (II) sulfate, magnesium sulfate and zinc sulfate solutions.

Add a piece of iron to each tube.

Leave for 3 minutes, record observations.

34
Q

How would you test the reactivity of Zinc?

A

Half fill separate test tubes with copper (II) sulfate, magnesium sulfate, and iron (II) sulfate solutions.

Add a piece of zinc to each test tube.

Leave for 3 minutes and record observations.

35
Q

How would you test the reactivity of copper?

A

Half fill test tubes with zinc sulfate, magnesium sulfate and iron (II) sulfate solutions.

Add a piece of copper to each test tube.

Leave for 3 minutes.

36
Q

How would you test the reactivity of magnesium?

A

Half-fill separate test tubes with copper (II) sulfate, zinc sulfate and iron sulfate solutions.

Add a piece of magnesium to each test tube.

Leave for 3 minutes and record observations.

GCSE Chemistry (21 decks)

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