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(B - GCSE) Chemistry > C4 > Flashcards

C4 Flashcards

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1
Q

What are the properties of alkali metals
(Group 1)

A

They react with water to form alkaline solutions

They have the typical properties of metals

They are shiny when freshly cut and good condictors of electricity

They are all soft enough to be cut with a knife

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2
Q

What does the trend going down the alkali metals show

A

They get softer to cut
Their density increases
Their melting point decreases
Reactivity increases

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3
Q

How do lithium, sodium and potassium react with water

A

Lithium - fizzes steadily and slowly disappears
sodium - melts into a silvery ball, fizzes vigorously then quickly disappears
Potasium - immediatkey ignites and burns with a lilac flame, the dissapears very quickly

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4
Q

Why does reactivity increase going down group 1

A

It becomes easier to lose electrons from the outer shell

(Force of attraction to the nucleus is lower, the more electron shells there are)

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5
Q

What is group 2 called

A

The alkaline earth metals

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6
Q

What are the elements in group 7 called

A

The halogen

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7
Q

What are the properties of the halogens

A

They are brittle
Poor conductors of electricity

(Typical non metals)

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8
Q

What are the physical properties of each halogen at room temperature

A

Fluorine - pale yellow gas
Chlorine - green gas
Bromine - orange / brown liquid
Iodine - shiny grey/black crystalline solid

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9
Q

What trends can be seen going down the group (halogens)

A

Reactivity decreases
Melting + boiling points increase
Density increases

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10
Q

Why are they called group 7 (halogens

A

They react with metals to form salts

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11
Q

Why does the reactivity decrease going down the group (non metals)

A

Going down the group they have more electron shells so the force of attraction between electrons and the nucleus is weaker

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12
Q

What is a displacement reaction

A

A reaction where a more reactive element displaces a less reactive element from its compound

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13
Q

How can you confirm the order of the halogens reactivitu

A

Using displacement reactions.
The most reactive will displace all but itself (etc)

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14
Q

What is group 8/0 called

A

The nobel gasses

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15
Q

What are the properties of the nobel gasses

A

They are unreactive
All in the gas state at room temperature
They are very light, as their atoms are far apart
They are monatomic, with weak forces of attraction - easily broken

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16
Q

What trends are shown going down group 0

A

Boiling point increases (forces between atoms get stronger)
Density increased

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17
Q

What does monatomic mean

A

Existing as single atoms

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18
Q

What does diatomic mean

A

Containing two atoms

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19
Q

What is the IUPAC group

A

A numbering system of all groups (including transition metals) 1-18

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20
Q

Why are nobel gasses unreactive

A

They have full outer shell

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21
Q

What are the properties of the transition metals

A

Shiny when freshly cut
Good conductor of electricity
Strong
Malleable (can be hammered into shape)

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22
Q

How do the transition metals compare to g1 metals

A

They are stronger / harder
Have higher densities
Higher melting points

Less reactive than g1 metals

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23
Q

What are the transition metals useful for

A

Making everyday objects, like copper wire

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24
Q

What are the chemical properties of transition metals

A

They react very slowly

Iron reacts with oxygen and water to produce rust (hydrated iron (3) oxide

Gold platinum and iridium dont react with oxygen and water

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25
Q

How / where is platinum (trans metal) used as a catalyst

A

In catalytic converters - convert harmful gasses in car exhausts into less harmful fumes

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26
Q

How many different types of ions can transition metals form

A

Multiple

E.g iron(II) and iron(III)

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27
Q

How do metals react with water / acids

A

A metal hydroxide and hydrogen is formed /
//
A salt and hydrogen is produced

28
Q

What does the rate of reaction tell you

A

The time the reaction takes shows how reactive the metal is

The quicker the reaction takes the more reactive the metal

29
Q

How do you test for carbon dioxide

A

Using limewater (calcium hydroxide solution)

Limewater tuens cloudy white when carbon dioxide is bubbled theough it

This happens as the calcium hydroxide and carbon dioxide react to form water and a white precioitate

30
Q

How do you test for chlorine

A

Get a damp piece of blue litmus paper

Hold the container near your substance

If chlorine is present the litmus paper will turn red then bleach white

31
Q

How should you smell substances in a labratory

A

With the container away from you, breathe enough air to almost fill your lungs

Then waft the substance towards you and take a small cautious sniff

32
Q

How do you test for hydrogen

A

Place a lighted splint near the container
If hydrogen is present it will ignitw with a squeaky pop

33
Q

How do you test for oxygen

A

Place a glowing splint in the tube.

If it relights oxygen is present

34
Q

What is a flame test

A

A test that helps identify metal ions in compounds from the colour they produce in a flame

35
Q

In a flame test what colour does lithium give off

A

Red

36
Q

In a flame test what colour does sodium give off

A

Yellow

37
Q

In a flame test what colour does potassium give off

A

Lilac

38
Q

In a flame test what colour does calcium give off

A

Orange/red

39
Q

In a flame test what colour does copper give off

A

Green/blue

40
Q

How do you do a flame test

A

First ensure the nichrome wire is clean - by dipping it in HCl until producing a clear flame

Next dip the loop of the wire into your powder or solution
Hold the wire on the edge of the bkue flame on your bunsen burner

Seeing what colour it turns tells you the ions present

41
Q

What are hydroxide precipitate tests

A

A chemical test to find the ions in a hydroxide solution by adding sodium hydroxide

42
Q

What colour is the precipitate of iron(II)

A

Green

43
Q

What colour is the precipitate of iron(III)

A

Orange-brown

44
Q

What colour is the precipitate of copper

A

Blue

45
Q

What colour is the precipitate of calcium

A

White

46
Q

What colour is the precipitate of zinc

A

White

47
Q

In precipitate tests how do you tell the difference between calcium and zinc

A

Adding excess sodium hydroxide to the zinc, the zinc hydroxide will become a colourless solution

48
Q

What type of reaction takes place in precipitate tests

A

Displacement reactions

49
Q

How do you detect sulfate ions

A

Add a few drops of hydrochloric acid to your solution
Then add barium chloride

White precipitate will be shown if sulfate ions are present

50
Q

What is a carbonate

A

A substance containing co3^2- ions

51
Q

What do metal carbonates react with acid to form

A

A salt carbon dioxide and water

52
Q

How do you test for carbonate ions

A

Add an acid (e.g hcl) to the solution
If carbonate ions are present it will bubble

During the reaction it will fizz

You can then test further by boiling it through limewater

53
Q

What is a sulfate ions

A

SO4^-2

54
Q

How do you detect halide ions

A

Add a small amount of dilute nitric acid

Then add silver nitrate
If a precipitate forms halid ions are present

55
Q

What precipitate colour is chlorine

A

White

56
Q

What precipitate colour is bromine

A

Cream

57
Q

What precipitate colour is Iodine

A

Yellow

58
Q

What are instrumental methods of analysis

A

A technique for analysing a substance that depends upon a machine

59
Q

Why is nitric acid added when finding halide ions

A

To react with any carbonate ions that may be present

60
Q

What is a mass spectrometer

A

A device that measured the masses of atoms and molecules

It analyses the relative amounts of different isotopes of an element

61
Q

What does each peak in a mass spectrum show

A

Each peak represents a fraction of the molecule

The peak on the right shows the molecular ion

62
Q

What are the advantages of instrumental methods of analysis

A

Sensitivity - instruments can analyse smaller amounts of substances

Accuracy - instruments are very accurate. They can be calibrated using internationally accepted standards

Speed - carry out analyses quickly and can run all the time

63
Q

How do you interpret a gas chromatogram

A

Each peak represents a substance present in the mixture

The areas under the peaks show the amount of each substance

64
Q

What are the axis of a gas chromatogram

A

Detector response (y)

Retention time (x)

65
Q

How does a mass spectrometer work

A

The sample molecules are ionised by the machine, to form molecular ions (e.g OH-)
These may break up to form fragments, which the machine can detect

(B - GCSE) Chemistry (7 decks)

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