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C4 Flashcards

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1
Q

What are the group 1 elements also known as?

A

Alkali metals

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2
Q

Why are the elements in group 1 called alkali metals?

A

They react with water to form alkaline solutions

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3
Q

What are the typical properties of the group 1 elements?

A

They are shiny when freshly cut
Good conductors of electricity

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4
Q

What state of matter are the group 1 elements at room temp and what is odd about that?

A

They are all solid at room temp but are soft enough to cut with a knife

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5
Q

Why are the group 1 metals only shiny when freshly cut?

A

They oxidise with air and lose their shiny colour

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6
Q

What is the trend as you go down group 1?

A

Density increases (sodium is more dense than expected)
Melting point decreases
They get softer
The reactivity increases

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7
Q

What do the alkali metals react with water to produce?

A

Metal hydroxide and hydrogen

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8
Q

What is the general half equation for group 1?

A

M = the symbol of the element

M = M^+ + E^-
M = M plus (plus) e minus

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9
Q

How do the first 3 element of group 1 react?

A

Lithium - fizzes steadily and slowly disappears
Sodium - melts to form a silvery ball, fizzes vigorously, quickly disappears
Potassium - immediately ignites, burns with a lilac flame, very quickly disappears

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10
Q

Why does the reactivity of group 1 increase as you go down?

A

Because it becomes easier to lose their outer electrons as the electrons get further and further away from the nucleus

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11
Q

Why does the density increase as you go down group 1?

A

The atom gets bigger (mass increases) due to the increase of electron shells

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12
Q

Why does the melting point decrease as you go down group 1?

A

The forces of attraction decrease as you go down the group

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13
Q

What is fluorine at room temp?

A

A pale yellow gas

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14
Q

What is chlorine at room temp?

A

A green gas

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15
Q

What is bromine at room temp?

A

An orange-brown liquid that vaporises easily

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16
Q

What is iodine at room temp?

A

A shiny grey-black crystalline solid that sublimes to form a purple vapour

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17
Q

What are the physical properties of the elements in group 7?

A

They are brittle when solid and are poor conductors of electricity

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18
Q

What do group 7 elements exist as?

A

Diatomic molecules

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19
Q

What are the group 7 elements known as?

A

The halogens

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20
Q

What is the trend as you go down group 7?

A

The density increases
The melting and boiling points increase
The reactivity decreases

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21
Q

Why are the group 7 elements called halogens?

A

They react with metals to produce salts
They react vigorously with the alkali metals especially if the metal is heated first

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22
Q

What is the half equation for the halogens?

A

X is the symbol of a halogen
X (lower) 2 + 2e- —> 2X-
X lower 2 + 2e minus goes to 2x minus

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23
Q

Why does the reactivity of the halogens decrease as you go down the group?

A

It becomes more difficult to gain an electron due to the higher energy level

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24
Q

Why does the melting and boiling point increase as you go down group 7?

A

The atoms increase in size as they gain extra electron shells and the intermolecular forces become stronger

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25
Q

Why does the density increase as you god own group 7?

A

The molecules get larger due to the extra electron shells

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26
Q

What happens in a halogen displacement reaction?

A

A halogen will displace a less reactive halogen from its halide ions

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27
Q

What would happen if the halogens tried to displace each other?

A

Chlorine displaces bromine from bromides
Bromine would displace iodine from iodides
Iodine cannot displace anything

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28
Q

How can you prove the order of reactivity of the halogens?

A

Use halogen displacement reactions

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29
Q

What type of reaction is a halogen displacement reaction?

A

A redox reaction

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30
Q

What is a redox reaction?

A

A reaction in which oxidation and reduction both take place

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31
Q

Why are the element of group 0 called noble gases?

A

They are so unreactive

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32
Q

What are all the elements of group 0 like at room temp?

A

They are all gases at room temp

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33
Q

Why are the noble gases so unreactive?

A

They have complete electron shells so that have no tendency to lose or gain electrons to form ions.

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34
Q

What word describes the noble gases?

A

Monatomic

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35
Q

What is the trend as you go down group 0?

A

The attractive forces between atoms get stronger
The boiling point increases
The densities increase

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36
Q

Why does the boiling point increase as you go down group 0?

A

The atoms get bigger meaning the forces of attraction become stronger

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37
Q

What are the typical properties of the transition metals?

A

Shiny when freshly cut
Good conductors if electricity
Malleable

38
Q

What are the properties of the transition metals compared to the alkali metals of group 1?

A

Stronger and harder
Higher densities
Have higher melting points (except for mercury)
Less reaction

39
Q

How do the transition metals react?

A

Slowly

40
Q

How does iron react with water and oxygen?

A

To produce rust - hydrated iron(III) oxide

41
Q

How do gold, platinum and iridium react with water and oxygen?

A

They don’t react at all

42
Q

What is different about the transitions metals compared to the alkali metal?

A

Transition metals can form more than 1 type of ion - the Roman numbers in brackets shows the charge

43
Q

What do metals form in reactions?

A

Positive ions

44
Q

How would you know how reactive a metal is during a reaction?

A

The more easily metals form ions, the more reactive the metal is

45
Q

How do you know if a metal can react with water or dilute acids?

A

If they are more reactive than hydrogen

46
Q

What is the descending reactivity series of metals (with hydrogen)?

A

Potassium
Sodium
Calcium
Magnesium
Aluminium
Zinc
Iron
Tin
Lead
(Hydrogen)
Copper
Silver
Gold
Platinum

47
Q

What do the electrons on the right of a half equation mean for metals mean?

A

Oxidation

48
Q

What do the electrons on the right of a half equation mean for metals mean?

A

Reduction

49
Q

What are the patterns of reactivity in the periodic table?

A

Group 0 don’t react
Reactive non-metals form covalent compounds with each other
Metals can form ionic compounds with non-metals
Group 1 and 2 metals are more reactive than other metals
Non-metals in group 7 become less reactive down the group

50
Q

How do you test for carbon dioxide?

A

Limewater (calcium hydroxide) turns cloudy when carbon dioxide is present (calcium carbonate produced)

51
Q

How do you test for chlorine?

A
  1. Dampen a piece of blue litmus paper
  2. Hold the paper near to a container that holds the substance
  3. Chlorine presence = paper turns red then white
52
Q

How do you test for hydrogen?

A

Squeaky pop test
Put a lighted splint near the container of gas
Hydrogen presence = ignite with squeaky pop

53
Q

How do you test for oxygen?

A

Put a glowing splint (lighted splint that has just been put out)
Oxygen presence = splint relights

54
Q

What happens during a flame test?

A

Heated metal ions = energy transferred to electrons
Electrons move to higher electron shells
When moved back, energy is transferred to surroundings as radiation - light

55
Q

What colour does a lithium ion make in a flame test?

A

Red

56
Q

What colour does a sodium ion make in a flame test?

A

Yellow

57
Q

What colour does a potassium ion make in a flame test?

A

Orange-red

58
Q

What colour does a copper ion make in a flame test?

A

Green-blue

59
Q

What does a hydroxide test formula look like?

A

(Metal)SO4 + 2NaOH —> Cu(OH)2 + Na2SO4

60
Q

What colour is iron(II) hydroxide precipitate?

A

Green

61
Q

What does a word equation of a hydroxide precipitate test look like?

A

(Metal) Sulfate + Sodium Hydroxide —> (metal) hydroxide + sodium sulfate

62
Q

Why is sodium hydroxide used in a hydroxide precipitate test?

A

It is insoluble

63
Q

What colour is iron(III) hydroxide precipitate?

A

Orange-brown

64
Q

What colour is copper(II) hydroxide precipitate?

A

Blue

65
Q

What colour is calcium hydroxide precipitate?

A

White

66
Q

What colour is zinc hydroxide precipitate?

A

White

67
Q

How do you tell the difference between calcium hydroxide and zinc hydroxide?

A

Add excess sodium hydroxide solution
Zinc hydroxide dissolves to a colourless solution
Calcium hydroxide doesn’t dissolve

68
Q

How do you test for sulfate ions?

A

Add a few drops of dilute hydrochloric acid
Add a few drops of barium chloride solution (BaCl2)
Sulfate ions presence = white precipitate

69
Q

How do you test for carbonate ions?

A

Add dilute hydrochloric acid
Carbonate ion presence = bubbles of gas produced
Carbon dioxide confirmation = limewater test

70
Q

Why is adding dilute hydrochloric acid a good test for carbonate ions?

A

Because it works whether the carbonate is insoluble or not

71
Q

How do you detect the presence of halide ions?

A

Add a few drops of DILUTE nitric acid
Then add a few drops of silver nitrate solution (AgNO3)
Halide ions presence = precipitate formed

72
Q

What colour precipitate do chloride ions make?

A

White

73
Q

What colour precipitate do bromide ions make?

A

Cream

74
Q

What colour precipitate do iodide ions make?

A

Yellow

75
Q

What are instrumental methods of analysis?

A

When you use machine to carry out the analysis of a substance

76
Q

What are the advantages of using instrumental methods of analysis?

A

Sensitivity - small substances
Accuracy
Speed - very fast

77
Q

What does a peak represent in a gas chromatogram?

A

A substance present in the mixture

78
Q

What do the areas under the peak mean in a gas chromatogram?

A

The relative amount of each substance in the mixture

79
Q

What is the retention time in a gas chromatogram?

A

The time taken for a substance to travel through the chromatography column

80
Q

What is a mass spectrometer?

A

A machine that can measure the masses of atoms and molecules

81
Q

What is a mass spectrometer used to analyse?

A

The relative amounts of different isotopes of an element and the structure of molecules

82
Q

Give an example of a field of science where a mass spectrometer is used and why?

A

Environmental science to detect toxic substances

83
Q

How does a mass spectrometer analyse molecules?

A

The sample molecules are ionised by the machine to form molecular ions. These break up to form fragments which the machine can separate and detect

84
Q

What does each peak in the mass spectrum represent?

A

A fragment of the molecule

85
Q

What does the peak on the far right represent in a mass spectrum?

A

The molecular ion

86
Q

What is the mass to charge ratio of the molecular ion peak equal to?

A

The relative formula mass of the molecule

87
Q

What can’t a simple flame test be used to identify two ions present in a mixture?

A

The samples might produce two very similar colours and one of the colours might be masked

88
Q

Why is Nichrome wire used in a flame test?

A

It doesn’t react or emit a colour

89
Q

How do we ensure that the Nichrome wire is clean before usage in a flame test?

A

Dip it into hydrochloric acid and hold it in the flame until no colour is seen

90
Q

How do you remove impurities when testing for sulfates?

A

You add dilute hydrochloric acid to get rid of carbonates and sulfites - they also make white precipitates with barium

91
Q

What do we add to remove impurities when testing for halide?

A

Dilute nitric acid

92
Q

What are halides?

A

Chemical compounds that contain halogen ions bonded to another ion.

Chemistry (8 decks)

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