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Chemistry GCSE > Chemical Analysis > Flashcards

Chemical Analysis Flashcards

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1
Q

How do you test for chlorine (gas)?

A

Bleach damp litmus paper - turning it white

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2
Q

How do you test for oxygen?

A

A glowing splint relit when put inside a test tube containing oxygen

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3
Q

How do you test for hydrogen?

A

A lit splint causes a squeaky pop when placed at end of a test tube containing hydrogen

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4
Q

How do you test for carbon dioxide?

A

Limewater turns cloudy when carbon dioxide bubbled through

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5
Q

What are flame tests used to identify?

A

Some metal ions that burn with distinctive flame

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6
Q

What metal makes a crimson flame?

A

Lithium

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7
Q

What metal makes a yellow flame?

A

Sodium

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8
Q

What metal makes a lilac flame?

A

Potassium

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9
Q

What metal makes a orange-red flame?

A

Calcium

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10
Q

What metal makes a green flame?

A

Copper

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11
Q

What colour flame for lithium?

A

Crimson flame

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12
Q

What colour flame for sodium?

A

Yellow flame

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13
Q

What colour flame for potassium?

A

Lilac flame

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14
Q

What colour flame for calcium?

A

Orange-red flame

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15
Q

What colour flame for copper?

A

Green flame

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16
Q

What is the problem of using a sample containing a mixture of metal ions?

A

Some flame colours might be masked by stronger ions

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17
Q

What solution helps identify some metal ions?

A

Sodium hydroxide solution

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18
Q

What colour precipitate does calcium form?

A

White precipitate - check using flame test

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19
Q

What colour precipitate does copper form?

A

Blue precipitate

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20
Q

What colour precipitate does magnesium form?

A

White precipitate

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21
Q

What colour precipitate does aluminium form?

A

White precipitate - redissolves in excess to form colourless solution

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22
Q

What colour precipitate does iron (II) form?

A

Green precipitate

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23
Q

What colour precipitate does iron (III) form?

A

Brown precipitate

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24
Q

Which metal ion forms a blue precipitate?

A

Copper

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25
Q

Which metal ion forms a white precipitate and can be checked using a flame test?

A

Calcium

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26
Q

Which metal ion forms a white precipitate?

A

Magnesium

27
Q

Which metal ion forms a white precipitate that redissolves in excess to form a colourless solution?

A

Aluminium

28
Q

Which metal ion forms a green precipitate?

A

Iron (II)

29
Q

Which metal ion forms a brown precipitate?

A

Iron (III)

30
Q

How do you test for carbonates?

A

Add dilute acid to solution
Connect test tube to limewater
Limewater turns cloudy if carbonate ions present - carbon dioxide released

31
Q

What do you add to a solution to test for carbonates?

A

Dilute acid

32
Q

What do you connect the solution to to test for carbonates?

A

Limewater

33
Q

Why do you connect the solution to limewater when testing for carbonates?

A

To see if the limewater turns cloudy, to see if carbon dioxide is produced

34
Q

How do you test for sulfates?

A

Add dilute hydrochloric acid
Add barium chloride solution
A white precipitate of barium sulfate will form if sulfate ions present

35
Q

What do you add to the solution to test for sulfates?

A

Dilute hydrochloric acid then barium chloride solution

36
Q

What do you add to a solution to test for a halide ion?

A

Dilute nitric acid and then silver nitrate solution

37
Q

How do you test for a halide ion in a solution?

A

Add dilute nitric acid
Add silver nitrate solution
See colour of precipitate if formed

38
Q

What colour precipitate does chloride form when testing for halides?

A

White precipitate - silver chloride

39
Q

What colour precipitate does bromide form when testing for halides?

A

Cream precipitate - silver bromide

40
Q

What colour precipitate does iodide form when testing for halides?

A

Yellow precipitate - silver iodide

41
Q

What halide ion is present if yellow precipitate formed?

A

Iodide

42
Q

What halide ion is present if cream precipitate formed?

A

Bromide

43
Q

What halide ion is present if white precipitate formed?

A

Chloride

44
Q

Why are instrumental methods a great way to identify elements and compounds?

A

They are accurate, sensitive and rapid

45
Q

What is flame emission spectroscopy used to analyse?

A

Metals ions in a solution

46
Q

How does flame emission spectroscopy work?

A

Sample put into a flame
When ions heat up, the electrons become excited
When electrons drop back to normal level of energy, they transfer energy as light
Light is passed through spectroscope
Spectroscope detects different wavelengths of light
Produces line spectrum

47
Q

Why do different ions emit different wavelengths of light during flame emission spectroscopy?

A

Because each ion has a different charge and electron arrangement

48
Q

Why is flame emission spectroscopy more useful than flame tests?

A

Flame emission spectroscopy can be used to detect different ions in mixtures - more useful than flame tests

49
Q

What is meant by purity in chemistry?

A

A singe element or compound

50
Q

What type of elements/compounds melt and boil at specific temperatures?

A

Pure elements and compounds

51
Q

What is the mobile phase in chromatography?

A

Where the molecules can move

52
Q

What is the stationary phase in chromatography?

A

Where the molecules can’t move

53
Q

The _____ phase moves through the _________ phase and anything dissolved in the ______ phase moves with it

A

Mobile
Stationary
Mobile

54
Q

Chemicals that spend more time in the ______ phase than the ________ phase, will move further through the _________ phase

A

Mobile
Stationary
Stationary

55
Q

What do components on a mixture normally separate through during chromatography?

A

The stationary phase

56
Q

How many spots will be formed by a pure substance during chromatography?

A

1

57
Q

The amount of time the molecules spend in each phase depends on:

A

How soluble they are in the solvent

How attracted they are to the paper

58
Q

Molecules with a higher solubility in the solvent and which are less attracted to the pare will spend more time in the ______ phase

A

Mobile

59
Q

If a dye has a higher attraction to the mobile phase, they move…

A

Further up

60
Q

If a dye has a stronger attraction to the stationary phase, they move…

A

Don’t move as much

61
Q

What is the Rf value?

A

The ration between the distance travelled by the dissolved substance and the distance travelled b the solvent

62
Q

Rf =

A

Distance travelled by solvent

63
Q

The further up the stationary phase you move, the _______ the Rf value

A

Larger

Chemistry GCSE (10 decks)

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