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Chemistry Inorganic 1 > Chapter 10 (Group 7) > Flashcards

Chapter 10 (Group 7) Flashcards

1
Q

How does fluorine appear?

A

Pale yellow gas which is highly reactive

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2
Q

How does chlorine appear?

A

Green, reactive gas, poisonous in high concentrations

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3
Q

How does bromine appear?

A

Red liquid, that gives off dense brown/orange poisonous fumes

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4
Q

How does iodine appear?

A

Shiny grey solid which sublimes to purple gas

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5
Q

State and explain the trend in boiling point down the group

A

Increases down the group

The molecules become larger as they have more electron shells so have larger Van Der Waals forces between molecules . As the intermolecular forces become larger, they require more energy to break.

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6
Q

Define electronegativity

A

The relative tendancy of an atom in a molecule to attract electrons in a covalent bond to itself.

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7
Q

State and explain the trend in electronegativity down the group

A

Decreases down the group

The atomic radius increases as there are more shells and more shielding. The nucleus is less able to attract a bonding pair of electrons.

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8
Q

How does the oxidising power of a halogen change down the group?

A

Weaker oxidising power

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9
Q

What halide ions is chlorine able to displace?

A

Iodide and Bromide

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10
Q

What halide ion is bromine able to displace?

A

Iodide

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11
Q

How does free bromine appear?

A

Yellow solution

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12
Q

How does free iodine appear in a solution?

A

Brown solution

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13
Q

How do you identify halide ions?

A

Add nitric acid and silver nitrate solution and a precipitate should form

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14
Q

Why do you add an acid before identifying halide ions?

A

To get rid of other negative ions e.g. carbonates

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15
Q

What colour is the precipitate of silver chloride?

A

White

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16
Q

What colour is the precipitate of silver bromine?

A

Cream

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17
Q

What colour is the precipice of silver iodide?

A

Yellow

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18
Q

What is added to help to distinguish between the silver halide precipitates and what is the observation?

A

Ammonia

Silver Chloride dissolves in dilute ammonia

Silver Bromide dissolves in concentrated ammonia

Silver Iodide does not dissolve/is insoluble in ammonia

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19
Q

How does the reducing power of a halide change down the group and why?

A

Stronger reducing agent

As the ions get bigger it is easier for the outer electrons to be given away as the electrostatic attraction from the nucleus becomes weaker.

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20
Q

What is a reducing agent?

A

A species which donate electrons

21
Q

What type of reaction happens between F- and Cl- and Sulphuric acid and why?

A

Acid based (proton donor) as the ions are not strong enough reducing agents to reduce the S in sulphuric acid.

22
Q

What is the equation for sodium fluoride and sulphuric acid and what is the observation?

A

NaF(s) + H2SO4(l) > NaHSO4(s) + HF(g)

White steamy fumes of HF

23
Q

What is the equation for sodium chloride and sulphuric acid and what is the observation?

A

NaCl(s) + H2SO4(l) > NaHSO4(s) + HCl(g)

White steamy fumes of HCl

24
Q

What is the observation when bromide ions are added to Sulphuric Acid?

A

White steamy fumes of HBr, Red Fumes of Bromide, Colourless, acidic, chocking gas of SO2.

25
Q

What is the equation of the acid based step when sodium bromide is added to Sulphuric Acid?

A

NaBr(s) + H2SO4(l) > NaHSO4(s) + HBr(g)

26
Q

What is the equation for the Redox step when Hydrogen Bromide reacts with Sulphuric Acid?

A

2HBr + H2SO4 > Br2(g) + SO2(g) + 2H2O(l)

27
Q

What is the half equation for the oxidation of Bromide?

A

2Br- > Br2 +2e-

28
Q

What is the half equation for the reduction of Sulphuric Acid to form Sulphur Dioxide?

A

H2SO4 +2H+ + 2e- > SO2 + 2H2O

29
Q

What is the change of oxidation state of sulphur in H2SO4 > SO2?

A

6+ > 4+

reduced

30
Q

What is the change of oxidation state of sulphur in H2SO4 > S?

A

6+ > 0

reduced

31
Q

What is the change of oxidation state of sulphur in H2SO4 > H2S?

A

6+ > 2-

reduced

32
Q

What is the half equation for the oxidation of iodide?

A

2I- > I2 + 2e-

33
Q

What is the equation for the acid-based reaction of Sodium Iodide with Sulphuric Acid?

A

NaI(s) + H2SO4(l) > NaHSO4(s) + HI(g)

34
Q

What is the half equation for the reduction of Sulphuric Acid to Sulphur?

A

H2SO4 + 6H+ + 6e- > SO2 + 4H2O

35
Q

What is the half equation for the reduction of Sulphuric Acid to Hydrogen Sulphide?

A

H2SO4 + 8H+ + 8e- > H2S + 4H2O

36
Q

What is the equation when Hydrogen Iodide reacts with Sulphuric Acid to form Sulphur Dioxide?

A

2HI + H2SO4 > I2(s) + SO2(g) + 2H2O(l)

37
Q

What is the equation when Hydrogen Iodide reacts with Sulphuric Acid to form Sulphur?

A

6HI + H2SO4 > 3I2(s) + S(s) + 4H20(l)

38
Q

What is the equation when Hydrogen Iodide reacts with Sulphuric Acid to form Hydrogen Sulphide?

A

8HI + H2SO4 > 4I2(s) + H2S(g) + 4H20(l)

39
Q

What is the reduction product when Bromide is added to H2SO4?

A

Sulphur Dioxide

40
Q

What are the reduction products when Iodide is added to H2SO4?

A

Sulphur Dioxide, Sulphur and Hydrogen Sulphide

41
Q

What are the observations when Sodium Iodide is added to H2SO4?

A

White steamy fumes of HI, Black solid and purple fumes of iodine, colourless and acidic chocking gas of SO2, yellow solid of sulphur and H2S gas with bad egg smell

42
Q

What is a disproportionation reaction?

A

A reaction where an element is simultaneously oxides and reduced.

43
Q

What is the equation for when chlorine is added to water?

A

Cl2(g) + H2O(l) <> HClO(aq) + HCl(aq)

44
Q

What is the equation for when chlorine is added to water with sunlight?

A

2Cl2 + 2H2O > 4HCl (4H+ + 4Cl-) + O2

45
Q

How is HClO tested for?

A

Universal indicator/Blue litmus paper will first turn red due to the acidity and then turn colourless as HClO bleaches the colour.

46
Q

What are the uses for NaClO?

A

Bleach/Disinfectant

47
Q

Why can chlorine be added to pools even though it is toxic?

A

Only added in small quantities to kill bacteria to health benefits outweigh the toxic effects.

48
Q

What is the equation for the reaction with Chlorine and cold, dilute NaOH?

A

Cl2(aq) + NaOH(aq) > NaCl(aq) + NaClO(aq) + H2O(l)

Chemistry Inorganic 1 (3 decks)

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