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Chemistry > 4: Inorganic Chemistry and the Periodic Table > Flashcards

4: Inorganic Chemistry and the Periodic Table Flashcards

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1
Q

What is the trend of reactivity in Group 2

A

Reactivity increases down Group 2 elements

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2
Q

Why does reactivity increase down Group 2

A
  • First and second ionisation energies decrease down Group 2
  • Therefore it is easier for the elements to lose their two valance electrons down the group
  • This is due to the attraction of the nucleus and valance electrons decreasing down the group due to increasing atomic radii and the increasing shielding
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3
Q

How do Group 2 elements behave in redox reactions

A
  • Each metal atom is oxidised, losing its two valance electrons, forming a +2 ion
  • Another species gains these electrons and is reduced
  • Therefore Group 2 elements are reducing agents
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4
Q

How can the reactivity of Group 2 elements be tested

A
  • Reacting with dilute HCl: bubbles of hydrogen gas are given off much faster down the group (more vigorous)
  • Reacting with oxygen: more reactive with oxygen down the group
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5
Q

What is the general equation for the reaction between Group 2 metals and oxygen

A
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6
Q

What is the general equation for the reaction between Group 2 metals and water

A
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7
Q

Why is magnesium oxide sometimes formed when magnesium reacts with water

A
  • Magnesium reacts extremely slowly with cold water, and the solution formed is only slightly soluble
  • When magnesium is heated in steam, it reacts vigorously to make magnesium oxide
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8
Q

What is the general equation for the reaction of Group 2 metals and chlorine gas

A
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9
Q

Are Group 2 oxides acidic or basic

A
  • All are basic
  • Apart from BeO which is amphoteric
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10
Q

Define amphoteric

A

A substance that can act as both an acid (proton donor) and a base (proton acceptor)

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11
Q

What happens when Group 2 oxides react with water

A
  • They form alkaline solutions which become more alkaline down the group
    Oxide + water ➡️ hydroxide
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12
Q

What is the general equation of the reaction between a Group 2 oxide and dilute hydrochloric/sulphuric acid

A

Metal oxide + dilute acid ➡️ metal salt (chloride/sulphate) + water

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13
Q

What happens when Group 2 metal hydroxides react with dilute acids

A
  • Form colourless solutions of metal salts
  • Except barium sulphate which is insoluble, making a white precipitate
    Metal hydroxide + dilute hydrochloric/sulphuric acid ➡️ metal salt (chloride/sulphate) + water
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14
Q

What is the ionic reaction that takes place when Group 2 oxides react with water

A
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15
Q

What is the trend in alkalinity in Group 2 solutions

A

Increases down the group

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16
Q

Why does alkalinity of Group 2 hydroxides increase down the group

A
  • Solubility of Group 2 hydroxides increases down the group,
  • So the concentration of OH- ions in the solution increases, increasing the pH of the solution
  • Making it more alkaline
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17
Q

What is the general equation for Group 2 hydroxides dissolving in water

A
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18
Q

What is the trend of solubility in Group 2 sulphates

A

Solubility decreases down the group

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19
Q

What is the trend of solubility of Group 1 hydroxides and sulphates

A

They are all soluble in water

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20
Q

Are Group 1 or 2 hydroxides more soluble

A

Group 1 hydroxides are more soluble

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21
Q

What is thermal decomposition

A

The breakdown of a compound into two or more different substances using heat

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22
Q

What is the only Group 1 carbonate that decomposes

A
  • Only lithium carbonate can be thermally decomposed at Bunsen temperatures
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23
Q

What is the general equation for the thermal decomposition of Group 2 carbonates

A
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24
Q

What is the only Group 1 nitrate that thermally decomposes

A
  • Lithium nitrate
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25
Q

What is the general equation for the incomplete decomposition of Group 1 nitrates (not lithium)

A
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26
Q

What is the general equation for the thermal decomposition of Group 2 nitrates

A
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27
Q

What is the trend in thermal stability in Group 1 and 2 carbonates and nitrates

A

Thermal stability increases down both groups

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28
Q

Why does thermal stability increase down Group 1 and 2 carbonates and nitrates

A
  • Ionic radius of the cations increases down the groups
  • Positive ions with larger ionic radii have lower polarising power and distort the electron clouds of the anions less
  • Positive ions with smaller ionic radii have higher polarising power and distort the electron clouds one the anions more
  • The more polarised the anion is, the more likely it is to be thermally decomposed as the bonds in the carbonate and nitrate ions become weaker and less heat is needed to free CO2 and NO2
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29
Q

Describe the flame test process

A
  • Dip an unreactive metal wire (in chrome/platinum) in concentrated HCl, then hold it in the blue flame of the Bunsen burner until there is no colour change (cleans to avoid contamination)
  • Dip the wire in the solid metal sample and place it on the edge of the blue Bunsen flame
  • Observe the colour
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30
Q

Why are are colours produced in flame tests

A
  • Heat causes electrons in the sample to jump to a higher energy level
  • The electron is unstable at this energy level, so falls back down
  • As it falls energy is emitted in the form of visible light
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31
Q

Mg2+ flame test

A

Bright white flame

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32
Q

Ba2+ flame test

A

Apple green

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33
Q

Ca2+ flame test

A

Brick red

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34
Q

Sr2+ flame test

A

Strong red

35
Q

Cu2+ flame test

A

Blue-green

36
Q

K+ flame test

A

Lilac

37
Q

Na+ flame test

A

Yellow

38
Q

Li+ flame test

A

Scarlett red

39
Q

Rb+ flame test

A

Red

40
Q

Cs+ flame test

A

Blue

41
Q

What is the name of Group 7 elements

A

Halogens

42
Q

What is the trend in colour of Group 7 elements

A

Colour gets darker down the group

43
Q

What is the colour and standard state of fluorine

A

Pale yellow gas

44
Q

What is the colour and standard state of chlorine

A

Green/yellow gas

45
Q

What is the colour and standard state of bromine

A

Orange/brown liquid

46
Q

What is the colour and standard state of iodine

A

Black solid (purple vapour)

47
Q

Define volatility

A

How easily a substance can evaporate

48
Q

What is the trend in volatility in Group 7

A

Volatility of the halogens decreases down the group

49
Q

What is the trend in melting/boiling points in Group 7 elements

A

Melting/boiling point of the elements increases down the group

50
Q

Why does the boiling point of halogens increase down the group

A
  • Halogens are diatomic molecules with simple molecular structures, with instantaneous dipoles caused by uneven spread of electrons within the molecule
  • There are weak London forces between the diatomic molecules caused by instantaneous dipole induced dipole forces
  • The more electrons in a molecule, the greater the instantaneous dipole induced dipole forces, and the stronger the London forces between molecules
  • This causes more energy needed to separate the molecules, causing the melting/boiling points to increase down the group
51
Q

What is the trend in electronegativity in Group 7 elements

A

Electronegativity decreases down the group

52
Q

Define electronegativity

A

The electronegativity of an atom refers to how strongly it attracts electrons towards itself in a covalent bond

53
Q

Why does electronegativity decrease down Group 7

A
  • Going down the group, atomic radii of the elements increases, so valance electrons get further from the nucleus as there are more shells in between it
  • Incoming electrons experience more shielding from the attraction of the positive nuclear charge
  • Making it harder for the elements to accept an electron (oxidising power) down the group
54
Q

What is the trend in reactivity in Group 7 elements

A

Reactivity decreases down the group

55
Q

Why does reactivity decrease down Group 7

A
  • When halogens react they gain 1 electron, and are reduced as they act as oxidising agents
  • As atomic radii increases down the group, valance electrons are further away from the nucleus, and are shielded from the positive nucleus
  • This makes it harder for the elements to attract an electron down the group
56
Q

Describe the reaction of fluorine and hydrogen

A

Reacts explosively even in cool, dark conditions

57
Q

Describe the reaction of chlorine and hydrogen

A

Reacts explosively in sunlight

58
Q

Describe the reaction of bromine and hydrogen

A

Reacts slowly on heating

59
Q

Describe the reaction of iodine and hydrogen

A

Forms an equilibrium mixture on heating

60
Q

What is shown by halogen displacement reactions

A
  • The reactivity of the halogens
  • The more reactive halogen can displace a less reactive halogen from a halide solution of the less reactive halogen
61
Q

What is the overall equation and ionic equation of chlorine water being added to a solution of bromine water

A
62
Q

Write the overall equation and ionic equation of chlorine water being added to a solution of iodine water

A
63
Q

What happens when chlorine is added to bromine solution

A
  • Chorine is more reactive, so displaces the bromine ions in the solution
  • Therefore the solution turns yellow-orange as Br2 is formed
64
Q

What happens when chlorine and cyclohexane are added to bromine solution

A
  • Chlorine is more reactive so it displaces bromine in the solution
  • Cyclohexane will form an organic layer on top of the solution, and it will be yellow-orange as Br2 is formed
65
Q

Why is cyclohexane used in halogen displacement reactions

A

Halogens are more soluble in the organic layer created by the cyclohexane, so the colour changes can be observed more easily

66
Q

What happens when chlorine and cyclohexane are added to iodine solution

A
  • Chlorine is more reactive so it displaces iodine in the solution
  • The cyclohexane forms an organic layer on top of the solution, and it turns purple as I2 is formed
67
Q

What happens when chlorine is added to iodine solution

A
  • Chlorine is more reactive so it replaces iodine in the solution
  • Therefore the solution turns brown as I2 is formed
68
Q

Write the full equation and the ionic equation of bromine water and iodine water

A
69
Q

What is the general formula for halogens reacting with metals

A

Halogen + metal ➡️ metal halide salt

  • Where the metal is oxidised
  • The halogens act as oxidising agents
70
Q

What are the halogens reactions with iron (II)

A
  • Chlorine and bromine can oxidise iron(II) to iron(III)
  • Iodine isn’t a strong enough oxidising agent, and is instead oxidised itself from iodide ions to iodine by iron(III)
71
Q

What is the reaction, ionic equation, and half equations of chlorine in dilute hot alkali (70 degrees C)

A
  • Disproportion reaction, as chlorine is simultaneously reduced and oxidised
72
Q

What is the reaction, ionic equation, and half equations of chlorine in dilute cold alkali (15 degrees C)

A
73
Q

Why is chlorine added to drinking water, and what is the reaction

A
  • Chlorine used to clean water and make it drinkable
  • Disproportionation reaction
  • Chloric(I) acid (HClO) sterilises water by killing bacteria
  • HClO can further dissociate in water to form ClO- which also acts as a sterilising agent
74
Q

What generally happens in the reaction between halide ions and concentrated sulphuric acid

A
  • React to produce toxic gases, so should happen in a fume cupboard
75
Q

What happens when chloride ions react with concentrated sulphuric acid

A
  • Conc. H2SO4 is added dropwise to sodium chloride crystals
  • Producing hydrogen chloride gas
  • The HCl gas produces steamy white fumes
76
Q

What happens when bromide ions react with concentrated sulphuric acid

A
  • After the reaction has occurred and HBr has been formed, the conc. sulphuric acid oxidises HBr
  • The HBr decomposes into bromine and hydrogen gas, and the sulphuric acid is reduced to sulphur dioxide gas
  • Bromine makes a reddish-brown gas
77
Q

What happens when iodide ions react with concentrated sulphuric acid

A
  • The reaction occurs, and the HI produced is oxidised by the sulphuric acid
  • The HI can be oxidised by sulphuric acid into iodine, and itself is reduced to sulphur
  • Iodine has a purple vapour, and sulphur is a yellow solid
  • The sulphuric acid can also oxidise HI to iodine, and itself is reduced to hydrogen sulphide
  • Hydrogen sulphide smells of rotten eggs
78
Q

Describe the test for halide ions

A
  • Unknown halide solution is dissolved in nitric acid
  • Silver nitrate solution is added
  • A precipitate of silver halide is formed
  • Dilute ammonia is added to the solution
  • Concentrated ammonia is added to the solution
79
Q

Silver ion test for chloride results

A
  • If chloride is present, ions form a white precipitate
  • When dilute ammonia is added, precipitate dissolves
  • When concentrated ammonia is added, precipitate dissolves
80
Q

Silver ions test for bromide results

A
  • If bromide is present, precipitate turns cream
  • When dilute ammonia is added, precipitate remains insoluble
  • When concentrated ammonia is added, precipitate dissolves
81
Q

Silver ions test for iodide results

A
  • If iodide is present, precipitate turns pale yellow
  • When dilute ammonia is added, solution remains insoluble
  • When concentrated ammonia is added, solution remains insoluble
82
Q

What is the equation for the reaction between halogens and hydrogen

A
  • Reaction produces a hydrogen halide
83
Q

What is the equation for the reaction between hydrogen halides and ammonia gas

A
  • Produces ammonium halides
84
Q

What is the equation for hydrogen halides reacting with water

A
  • Dissolve in water to form acids

Chemistry (19 decks)

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