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ES- Elements of the Sea Flashcards

0
Q

What is the appearance + state of fluorine at room temperature?

A

Pale yellow gas

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1
Q

What is the appearance + state of chlorine at room temperature?

A

Green gas

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2
Q

Volatility of fluorine?

A

Gas

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3
Q

Volatility of iodine?

A

Sublimes on warming to give a purple vapour

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4
Q

Volatility of chlorine?

A

Gas

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5
Q

Volatility of bromine?

A

Liquid quickly forms brown gas on warming

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6
Q

What is the appearance + state of bromine at room temperature?

A

Dark red liquid

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7
Q

What is the appearance + state of iodine at room temperature?

A

Shiny black solid

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8
Q

Solubility of iodine in water?

A

Barely soluble, gives brown solution

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9
Q

Solubility of bromine in water?

A

Slightly soluble to give red-brown solution

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10
Q

Solubility of fluorine in water?

A

Reacts with water

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11
Q

Solubility of chlorine in water?

A

Slightly soluble to give pale green solution

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12
Q

Solubility of fluorine in organic solvents?

A

Soluble

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13
Q

Solubility of iodine in organic solvents?

A

Soluble to give a violet solution

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14
Q

Solubility of chlorine in organic solvents?

A

Soluble to give a pale green solution

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15
Q

Solubility of bromine in organic solvents?

A

Soluble to give a red solution

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16
Q

Which of the halogens is the most reactive?

A

Fluorine

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17
Q

Does fluorine react with halide ions and silver ions???

A

NO

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18
Q

What would you expect from the reaction of chlorine and silver ions?

A

White precipitate = silver chloride

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19
Q

What would you expect from the reaction of bromine and silver ions?

A

Cream precipitate = silver bromide

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20
Q

What would you expect from the reaction of iodine and silver ions?

A

Yellow precipitate = silver iodide

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21
Q

How does iodine behave in displacement reactions?

A

It does not displace anything

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22
Q

How does fluorine behave in displacement reactions?

A

It displaces everything below it in the group (Cl, Br, I)

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23
Q

Why are halogens known as oxidising agents?

A

They increase in oxidation state.

They tend to remove electrons from other elements.

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24
Q

Are all halogens reactive?

A

Yep

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25
Q

Why is fluorine the strongest oxidising agent in group 7?

A

Small atoms

Fewest shells so less shielding from nucleus + greater attraction (pull) from nucleus

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26
Q

How does fluorine need to be stored?

A

It’s too reactive

Made in situ (as needed) by electrolysing liquid hydrogen fluoride

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27
Q

Why is chlorine dangerous?

A

Toxic + volatile (gas)

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28
Q

How is chlorine transported?

A

Rail or road tanker, stored as a liquid OR produce it on site

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29
Q

How do the bond strengths of halogenoalkanes change down the group?

A

Decrease

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30
Q

How is bromine transported?

A

Convert it into Bromide compounds
Lead-lined steel tanks
Tanks are supported in strong metal frames
Transport routes planned to minimise risk of accidents

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31
Q

How do the reactivities of halogenoalkanes change down the group?

A

Increase

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32
Q

What are the conditions for homolytic fission?

A

Gas phase; high temperatures/ the presence of UV radiation (e.g. In the stratosphere)

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33
Q

What are the conditions for heterolytic fission?

A

Halogenoalkane dissolved in a polar solvent like ethanol/ water mixture

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34
Q

What is a carbocation?

A

A positively charged C group

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35
Q

What reactions do halogenoalkanes undergo?

A

Nucleophilic substitution

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36
Q

How many electrons can S hold?

A

2

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37
Q

How many electrons can P hold?

A

6

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38
Q

How many electrons can D hold?

A

10

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39
Q

How many electrons can F hold?

A

14

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40
Q

How many orbitals does S have?

41
Q

How many orbitals does P have?

42
Q

How many orbitals does D have?

43
Q

How many orbitals does F have?

44
Q

What is a cation?

A

A positive ion

45
Q

What is a giant ionic lattice?

A

Lots of ions arranged in fixed positions

46
Q

Why can an ionic lattice hold its structure?

A

The attractive forces are stronger than the repulsive forces

47
Q

What are hydrated crystals?

A

Crystals of some ionic solids with water molecules fit into the lattice just as regularly as ions

48
Q

What happens when hydrated crystals are heated?

A

Water is driven off as steam

49
Q

What is the product of heated hydrated crystals?

A

An anhydrous solid

50
Q

What is the main condition of hydration?

A

The energy needed to break the lattice is compensated by the energy released

51
Q

What are spectator ions?

A

Ions that are not involved in ionic equations

52
Q

Give an example of covalent compounds being made from mixed solutions

A

Neutralisation

53
Q

True or false? ‘All NITRATES are soluble’

54
Q

Which CHLORIDES are insoluble

A

AgCl ; PbCl2

55
Q

Most SULFATES are soluble in water. What are the exceptions to this rule?

A

BaSO4 ; PbSO4 ; SrSO4

56
Q

All CARBONATES are insoluble. What are the exceptions to this rule?

A

NH4 ; Group 1 elements

57
Q

Are all GROUP 1 salts soluble or insoluble in water?

58
Q

Name the three types of salts that are always soluble in water

A

SODIUM, POTASSIUM, AMMONIUM

59
Q

At room temperature and pressure what is the volume that 1 mole of any gas occupies?

60
Q

At standard temperature and pressure what is the volume that 1 mole of any gas occupies?

61
Q

Why do chemists usually prefer to measure out quantities in moles rather than grams?

A

Moles tells us the number of particles actually present

62
Q

How does ATOMIC RADIUS affect the size of ionisation enthalpies?

A

The bigger the atoms, the weaker the electronegative pull (from the nucleus)

63
Q

How does NUCLEAR CHARGE affect the size of ionisation enthalpies?

A

The more protons in the nucleus, the stronger the pull from the nucleus

64
Q

How does ELECTRON SHIELDING affect the size of ionisation enthalpies?

A

The more inner shells the weaker the electrongeative pull (from the nucleus)

65
Q

What is the first ionisation enthalpy?

A

The energy needed to remove 1 electron from each atom in 1 mole of GASEOUS ATOMS to form 1 mole of GASEOUS 1+ IONS

66
Q

What is the second ionisation enthalpy?

A

The energy needed to remove 1 electron from each atom in 1 mole of 1+ GASEOUS IONS to form 1 mole of GASEOUS 2+ IONS

67
Q

What is the effect of having more electrons on ionisation enthalpy? (For elements within the same period)

A

More electrons = More protons. This means a stronger electronegative pull from the nucleus of the atom.

68
Q

What is important about the mole of gaseous atoms/ ions being ionized?

A

They must be ISOLATED.

69
Q

Why does it get harder to remove electrons from ions?

A

Once an electron has been removed from the atom/ ion, the electronegative pull increases

70
Q

What is important to note about a graph showing ionisation enthalpies?

A

A sharp increase in the enthalpy when electrons are taken from the next outer shell. This is because the next shell is closer to the nucleus…

71
Q

How do you identify a spectator ion?

A

It will be anything that hasn’t changed in oxidation state during the reaction.

72
Q

What are oxoanions?

A

Negative ions with oxygen in them

73
Q

‘Electrons in atoms have a spin’ What does this mean?

A

They can only occupy the same orbital with opposite/ paired spins (spinning in opposite directions)

74
Q

What are sub-shells filled with electrons known as?

A

CLOSED - SHELL ARRANGEMENTS

75
Q

What are halogens more soluble in: organic solvents, or water?

A

ORGANIC SOLVENTS

76
Q

True or false? Different halogens can covalently bond with each other

A

True. The less reactive one has a positive oxidation state.

77
Q

What do you add to the test for halide ions FIRST and why?

A

DILUTE NITRIC ACID - Removes ions which might interfere with the reaction

78
Q

What is the test for halide ions and what would you see?

A

Silver nitrate - A precipitate of the silver halide

79
Q

What colour is the Chloride precipitate?

80
Q

What colour is the Fluoride precipitate?

A

Trick question: No precipitate would be formed in the presence of silver nitrate because SILVER FLUORIDE is SOLUBLE IN WATER.

81
Q

What colour is the Iodide precipitate?

82
Q

What is the main way of extracting halogens (excl. fluorine)?

A

Electrolysis of halide solutions

83
Q

What happens when solutions containing I- or Br- ions are electrolysed?

A
  1. Halogen released at anode

2. Halogen oxidised to atoms which form molecules

84
Q

What condition must chloride be extracted from in its halide solution?

A

CONCENTRATION

85
Q

In a chloride solution what two CATIONS are present?

86
Q

In a chloride solution what two ANIONS are present?

87
Q

If the chloride solution is dilute, what is released at the cathode?

A

H2 (Hydrogen)

88
Q

If the chloride solution is concentrated, what is released at the cathode?

A

H2 (Hydrogen)

89
Q

If the chloride solution is dilute, what is released at the anode?

A

OH- —> O2 (Oxygen)

90
Q

If the chloride solution is concentrated, what is released at the anode?

A

Cl- —> Cl2

91
Q

True or false? Regardless of whether the solution is concentrated or dilute, HYDROGEN is always produced at the CATHODE

92
Q

Why can’t fluorine be extracted from electrolysis?

A

Hydroxide ions are discharged regardless of the concentration of the solution

93
Q

What is the atom economy of electrolysis?

94
Q

How is Fluorine transported?

A

Just avoid using it

95
Q

How is Iodine transported?

A

This is fairly easy to transport

96
Q

What reactions with halide ions are IRREVERSIBLE?

A

DISPLACEMENT and REDOX

97
Q

What STATE are molecular dipoles at room temperature and pressure?

98
Q

What is the importance of silver halides?

A

Used in PHOTOCHROMIC LENSES

99
Q

Silver bromide is decomposed by light. What is it soluble in and why is this useful?

A

SODIUM THIOSULFATE - It clears silver bromide crystals from films

Chemistry (12 decks)

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