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AQA Chemistry > Inorganic 1 Section 2 - Unit 10: Halogens > Flashcards

Inorganic 1 Section 2 - Unit 10: Halogens Flashcards

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1
Q

State the equation for the reaction between chlorine and water (1 mark)

A
  • Cl2 + H2O → HOCl + HCl
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2
Q

When a pool has a pH of over 7.0, explain how adding chlorine to water affects the equilibrium (2 marks)

A
  • Alkaline ions react with acid

- So equilibrium shifts to the right

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3
Q

Explain why chlorine is used to kill bacteria in swimming pools, even though chlorine is toxic (2 marks)

A
  • Only used in small amounts

- Health benefits outweigh the risk

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4
Q

Which substance reacts most rapidly to produce a silver halide precipitate with acidified silver nitrate?

A
  • CH3l
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5
Q

Explain why chlorine has a lower boiling point than bromine (1 mark)

A
  • Chlorine is smaller than bromine

- Cl2 has weaker intermolecular forces

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6
Q

State how you could tell the difference between AgBr and AgI (3 marks)

A
  • Concentrated ammonia
  • Cream solid dissolves
  • Yellow solid does not dissolve
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7
Q

Describe fluorine (1)

A
  • Pale yellow gas
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8
Q

Describe chlorine (1)

A
  • Greenish gas
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9
Q

Describe bromine (2)

A
  • Red liquid

- Gives off brown/orange poisonous fumes

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10
Q

Describe iodine (2)

A
  • Shiny grey solid

- Purple gas

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11
Q

Explain why melting and boiling point increases down the halogen group (3 marks)

A
  • Down the group, more electrons
  • So larger VDW
  • So more energy required to break the forces
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12
Q

Role of H₂SO₄ when reacting with NaF and NaCl (1 mark)

A
  • Acid
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13
Q

Role of H₂SO₄ when reacting with NaBr and NaI (2 marks)

A
  • Acid in first step

- Then oxidising agent

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14
Q

Appearance of HI (1 mark)

A
  • White steamy fumes
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15
Q

Appearance of SO₂ (1 mark)

A
  • Colourless acidic gas
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16
Q

Appearance of H₂S (1 mark)

A
  • Gas with bad egg smell
17
Q

Equation for reaction of NaF with H₂SO₄ (1 mark)

A

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

18
Q

Observation for reaction of NaF with H₂SO₄ (1 mark)

A

White steamy fumes of HF

19
Q

Equation for reaction of NaCl with H₂SO₄ (1 mark)

A

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

20
Q

Observation for reaction of NaCl with H₂SO₄ (1 mark)

A

White steamy fumes of HCl

21
Q

Explain why redox reactions do not occur with NaF and NaCl with H₂SO₄ (2 marks)

A
  • F- and Cl- are not strong enough reducing agents

- So cannot reduce the S in H₂SO₄

22
Q

Equation for acid-base step of reaction of NaBr with H₂SO₄ (1 mark)

A

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

23
Q

Equation for redox step of reaction of NaBr with H₂SO₄ (1 mark)

A

2H+ + 2Br- + H₂SO₄ –> Br₂ + SO₂ + 2H₂O

24
Q

Overall equation for reaction of NaBr with H₂SO₄ (1 mark)

A

2NaBr + 3H₂SO₄ –> 2NaHSO₄ + Br₂ + SO₂ + 2H₂O

25
Q

Observations for reaction of NaBr with H₂SO₄ (3 marks)

A
  • White steamy fumes of HBr
  • Orange fumes of bromine
  • Colourless, acidic gas SO₂
26
Q

Equation for acid-base step of reaction of NaI with H₂SO₄ (1 mark)

A

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

27
Q

State the redox step for the reaction of NaI with H₂SO₄, when SO₂ is given off (1 mark)

A

2 H+ + 2 I- + H₂SO₄ –> I₂ (s) + SO₂ (g) + 2 H₂O(l)

28
Q

State the redox step for the reaction of NaI with H₂SO₄, when S is produced (1 mark)

A

6 H+ + 6 I- + H₂SO₄ –> 3 I₂ (s) + S (s) + 4 H₂O (l)

29
Q

State the redox step for the reaction of NaI with H₂SO₄, when H₂S is given off (1 mark)

A

8 H+ + 8 I- + H₂SO₄ –> 4 I₂ (s) + H₂S(g) + 4 H₂O(l)

30
Q

Observations for reaction of NaI with H₂SO₄ (5 mark)

A
  • White steamy fumes of HI
  • Black solid and purple fumes of iodine
  • Colourless acidic gas of SO₂
  • Yellow solid of sulfur
  • H₂S gas with bad egg smell
31
Q

State the equation for the reaction of chlorine with water in sunlight (1 mark)

A

2Cl₂ + 2H₂O –> 4HCl + O₂

32
Q

State the equation for the reaction of chlorine with water (1 mark)

A

Cl₂ + H₂O –> HCl (aq) + HClO (aq)

33
Q

State the observation when universal indicator is added to the reaction of chlorine with water (2 marks)

A
  • First turns red due to acidity of both reaction products

- Then turns colourless as the HClO bleaches the colour

AQA Chemistry (32 decks)

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