Inorganic 1 Section 2 - Unit 10: Halogens

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Total cards: 24•Content version: v4•Public deck•Updated: 8/1/2026

Card preview (24)

Front (Question)

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

Back (Answer)

• Cl2 + H2O → HOCl + HCl

Front (Question)

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

Back (Answer)

• Alkaline ions react with acid - So equilibrium shifts to the right

Front (Question)

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

Back (Answer)

• Only used in small amounts - Health benefits outweigh the risk

Front (Question)

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

Back (Answer)

• CH3l

Front (Question)

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

Back (Answer)

• Chlorine is smaller than bromine - Cl2 has weaker intermolecular forces

Front (Question)

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

Back (Answer)

• Concentrated ammonia • Cream solid dissolves • Yellow solid does not dissolve

Front (Question)

Describe fluorine (1)

Back (Answer)

• Pale yellow gas

Front (Question)

Describe chlorine (1)

Back (Answer)

• Greenish gas

Front (Question)

Describe bromine (2)

Back (Answer)

• Red liquid - Gives off brown/orange poisonous fumes

#10

Front (Question)

Describe iodine (2)

Back (Answer)

• Shiny grey solid - Purple gas

#11

Front (Question)

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

Back (Answer)

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

#12

Front (Question)

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

Back (Answer)

• Acid

#13

Front (Question)

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

Back (Answer)

• Acid in first step - Then oxidising agent

#14

Front (Question)

Appearance of HI (1 mark)

Back (Answer)

• White steamy fumes

#15

Front (Question)

Appearance of SO₂ (1 mark)

Back (Answer)

• Colourless acidic gas

#16

Front (Question)

Appearance of H₂S (1 mark)

Back (Answer)

• Gas with bad egg smell

#17

Front (Question)

Equation for reaction of NaF with H₂SO₄ (1 mark)

Back (Answer)

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

#18

Front (Question)

Observation for reaction of NaF with H₂SO₄ (1 mark)

Back (Answer)

White steamy fumes of HF

#19

Front (Question)

Equation for reaction of NaCl with H₂SO₄ (1 mark)

Back (Answer)

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

#20

Front (Question)

Observation for reaction of NaCl with H₂SO₄ (1 mark)

Back (Answer)

White steamy fumes of HCl

#21

Front (Question)

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

Back (Answer)

• F- and Cl- are not strong enough reducing agents - So cannot reduce the S in H₂SO₄

#22

Front (Question)

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

Back (Answer)

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

#23

Front (Question)

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

Back (Answer)

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

#24

Front (Question)

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

Back (Answer)

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