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C4 Flashcards

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1
Q

What are the Group 1 elements known as?

A

Alkali Metals

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2
Q

Why do alkali metals have similar properties?

A

They all have 1 outer electron

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3
Q

What are the physical properties of alkali metals?

A

Very soft - can be cut with a knife

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4
Q

How can you test for alkali metals?

A

Flame tests

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5
Q

Why are alkali metals very reactive?

A

They readily lose their single outer electron to form a positive ion - the more readily a metal becomes an ion, the more reactive it is.

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6
Q

Why do alkali metals get increasingly reactive as you move down the group?

A

The outer electron is easier to lose when the outer shell is further away from the nucleus (the atomic radius is larger).

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7
Q

How do alkali metals in general behave in water?

A

They react vigorously. The reaction produces hydrogen gas and a hydroxide of the metal.

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8
Q

How does Lithium behave in water?

A

It moves around the surface, fizzing furiously

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9
Q

How do Sodium and Potassium behave in water?

A

Similarly to Lithium, but they also melt in the heat of the reaction

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10
Q

How do Rubidium and Caesium behave in water?

A

They react violently with water, tending to explode when they get wet.

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11
Q

What is produced when alkali metals react with dilute acids?

A

A salt and hydrogen gas. This reaction is very violent.

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12
Q

What are Group 7 elements known as?

A

Halogens

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13
Q

Why do halogens have similar properties?

A

They all have 7 electrons in their outer shell.

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14
Q

Halogens exist as diatomic molecules - what does this mean?

A

They are made up of two atoms of the element eg. Cl₂

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15
Q

How do halogens gain a stable electronic structure?

A

They share one pair of electrons in a covalent bond, giving both atoms involved a full outer shell.

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16
Q

What happens to the melting and boiling point of halogens as you move down the group?

A

The melting points of the halogens increase.

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17
Q

How does chlorine behave at room temperature?

A

It is fairly reactive, poisonous, green gas.

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18
Q

How does bromine behave at room temperature?

A

It is a poisonous, red-brown liquid, which gives off an orange vapour at room temperature.

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19
Q

How does iodine behave at room temperature?

A

It is a dark grey crystalline solid, which gives off purple vapour when heated.

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20
Q

Why do halogens become less reactive as you move down the group?

A

It is harder for them to attract an extra neutron to fill their outer shell when it’s further away from the nucleus (the atomic radius is larger).

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21
Q

What happens when halogens react with alkali metals?

A

They react vigorously and form salts known as metal halides.

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22
Q

What is a displacement reaction?

A

It is where a more reactive element “pushes out” (displaces) a less reactive element from a compound

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23
Q

What does it mean if there is a colour change when you mix a halide salt and a halogen solution?

A

It means that the halogen has displaced the halide ions from the salt.

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24
Q

What happens when you react Chlorine with Potassium Chloride, Potassium Bromide and Potassium Iodide?

A

Potassium Chloride: No reaction
Potassium Bromide: Orange solution formed (Bromide displaced)
Potassium Iodide: Brown solution formed (Iodide

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25
Q

What happens when you react Bromine with Potassium Chloride, Potassium Bromide and Potassium Iodide?

A

Potassium Chloride: No reaction
Potassium Bromide: No reaction
Potassium Iodide: Brown solution formed (Iodide displaced)

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26
Q

What happens when you react Iodine with Potassium Chloride, Potassium Bromide and Potassium Iodide?

A

Potassium Chloride: No reaction
Potassium Bromide: No reaction
Potassium Iodide: No reaction

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27
Q

What are Group 0 elements known as?

A

Noble gases.

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28
Q

How do noble gases behave at room temperature?

A

They are all colourless gases.

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29
Q

Noble gases are monatomic - what does monatomic mean?

A

It means that they are made up of single atoms.

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30
Q

What does inert mean?

A

It means that something doesn’t react.

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31
Q

Why are noble gases inert?

A

They have a full outer shell and therefore they don’t easily give up or gain electrons.

32
Q

Why are noble gasses non-flammable?

A

Because they are inert.

33
Q

What happens to the boiling point, melting point and density of noble gases as you move down the group?

A

They increase.

34
Q

What are the properties of transition metals?

A

They are hard, strong and shiny materials that conduct heat and electricity. They have high melting points (except mercury) and densities.

35
Q

How are transition metals used as catalysts?

A

Vanadium pentoxide is the catalyst for making sulfuric acid in the Contact Process.

36
Q

What is the colour of transition metals like?

A

They are all colourful. What colour they are depend on what transition metal ion they contain.

37
Q

What is the reactivity of transition metals like in comparison to Group 1 and 2 metals?

A

They are much less reactive.

38
Q

What’s an easy experiment that you can use to show that some metals are more reactive than others?

A

Place them into hydrochloric acid

39
Q

How do magnesium, aluminium, zinc, iron and copper react in hydrochloric acid?

A 
Magnesium - loud squeaky pop
Aluminium - squeaky pop
Zinc - quiet squeaky pop
Iron - very quiet squeaky pop
Copper - no reaction
40
Q

What does the volume of the “squeaky pop” relate to when reacting metals with hydrochloric acid?

A

The amount of hydrogen produced.

41
Q

What is produced when you react metal with water?

A

Metal + Water → Metal Hydroxide + Hydrogen

42
Q

What can you react less reactive metals with instead of water?

A

Steam

43
Q

What is produced when you react a less reactive metal with steam?

A

Less reactive metal + Steam → Metal Oxide + Hydrogen

44
Q

What is the reactivity series?

A 
Potassium
Sodium
Lithium
Calcium
Magnesium
Aluminium
Carbon
Zinc
Iron
Hydrogen
Copper
Silver
Gold
45
Q

How do more reactive metals interact with less reactive metals?

A

The more reactive metal displaces the less reactive metal.

46
Q

How do you test for carbon dioxide?

A

You can test to see a gas is carbon dioxide by bubbling it through limewater. If the gas is carbon dioxide, the limewater will become cloudy.

47
Q

How do you test hydrogen?

A

Hydrogen makes a “squeaky pop” when it interacts with a lighted splint. This noise comes from the hydrogen burning with the oxygen in the air to form water.

48
Q

How can you test for oxygen?

A

You can put a glowing splint into a test tube and if it relights, oxygen is present.

49
Q

How can you test for chlorine?

A

When you hold a piece of damp blue litmus paper over chlorine, it bleaches the paper, turning it white.

50
Q

How can you test for halide ions?

A

You can test for halide ions by adding dilute nitric acid (HNO₃) and silver nitrate solution (AgNO₃)

51
Q

Why do you add nitric acid when testing for halide ions?

A

To remove any carbonate ions which may interfere or confuse the colour change/result.

52
Q

How does chloride react to the silver nitrate test?

A

It produces a white precipitate of silver chloride.

53
Q

How does bromide react to the silver nitrate test?

A

It produces a cream precipitate of silver bromide.

54
Q

How does iodide react to the silver nitrate test?

A

It produces a yellow precipitate of silver iodide.

55
Q

How can you test for carbonates?

A

Add barium chloride solution, and then dilute hydrochloric acid.

56
Q

What should happen if a carbonate is present when you add barium chloride to the solution?

A

If carbonate ions are present, a white precipitate of barium carbonate will be produced.

57
Q

What should happen if a carbonate is present when you add hydrochloric acid to the solution, after adding barium chloride?

A

The mixture should fizz, as a result of the carbonate reacting with the acid to produce carbon dioxide gas.

58
Q

What is the product of barium carbonate reacting with hydrochloric acid?

A

A colourless solution containing Ba²⁺ ions.

59
Q

How can you test for sulfate ions?

A

The same way you test for carbonates - you add barium chloride and then dilute hydrochloric acid.

60
Q

What should happen if sulfate ions are present when you add barium chloride to the solution?

A

If carbonate ions are present, a white precipitate of barium sulfate will be produced.

61
Q

Why do you add hydrochloric acid when testing for sulfate ions?

A

Barium sulfate will not react with hydrochloric acid, which proves that you’ve got sulfate ions and not carbonate ions.

62
Q

How does Lithium react in a flame?

A

Produces a crimson red flame

63
Q

How does Sodium react in a flame?

A

Produces a yellow flame

64
Q

How does Potassium react in a flame?

A

Produces a lilac flame

65
Q

How does Calcium react in a flame?

A

Produces a brick red flame

66
Q

How does Copper react in a flame?

A

Produces a blue-green flame

67
Q

How do you perform a flame test for metal?

A

Clean a nichrome wire loop by dipping it in hydrochloric acid and then rinsing it in deionised water.
Dip the wire loop into a sample of the metal compound and put the loop into the flame.

68
Q

How can you test some metal ions with sodium hydroxide?

A

You add a few drops of sodium hydroxide to a solution of the mystery compound. If a hydroxide precipitate forms, you can use its colour to tell which metal ion is present.

69
Q

What colour precipitate does Calcium, Ca²⁺ produce when reacted with Sodium Hydroxide? What is the Ionic Equation?

A

White

Ca²⁺ + 2OH⁻ → Ca(OH)₂

70
Q

What colour precipitate does Copper, Cu²⁺ produce when reacted with Sodium Hydroxide? What is the Ionic Equation?

A

Blue

Cu²⁺ + 2OH⁻ → Cu(OH)₂

71
Q

What colour precipitate does Iron(II), Fe²⁺ produce when reacted with Sodium Hydroxide? What is the Ionic Equation?

A

Green

Fe²⁺ + 2OH⁻ → Fe(OH)₂

72
Q

What colour precipitate does Iron(III), Fe³⁺ produce when reacted with Sodium Hydroxide? What is the Ionic Equation?

A

Brown

Fe³⁺ + 3OH⁻ → Fe(OH)₃

73
Q

What colour precipitate does Zinc, Zn²⁺ produce when reacted with Sodium Hydroxide? What is the Ionic Equation?

A

White at first, but then redissolves in excess sodium hydroxide to form a colourless solution.
Zn²⁺ + 2OH⁻ → Zn(OH)₂
Then: Zn(OH)₂ + 2OH⁻ → ZN(OH)₄²⁻

74
Q

What is an instrumental method?

A

A method which involves using machines rather than a person doing chemical tests manually.

75
Q

What are the advantages of instrumental methods?

A

They are very accurate - they don’t involve human error.

76
Q

What are some examples of instrumental methods?

A

Mass spectrometry - technique which can find the relative molecular mass of a mystery compound

OCR chemistry (6 decks)

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