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(I) Topic 10 - The Halogens

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Total cards: 17•Content version: v4•Public deck•Updated: 8/1/2026

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#1
Front (Question)

Describe: The physical properties of the halogens in their standard states

Back (Answer)

Fluorine - pale yellow gas Chlorine - pale green gas Bromine - Red Liquid Iodine - Dark Grey Solid (readily sublimes into purple vapour)

#2
Front (Question)

Describe: The physical properties of the halogens in aqueous solution

Back (Answer)

Chlorine - pale green solution Bromine - Yellow/ Orange solution Iodine - Brown Solution

#3
Front (Question)

Describe: The physical properties of the halogens in organic solution

Back (Answer)

Chlorine - pale green solution Bromine - orange solution Iodine - Violet Solution

#4
Front (Question)

Describe: The trend in oxidation power in the halogens

Back (Answer)

As you go up the group the ability to oxidise increases. A halogen which is a stronger oxidising agent will displace a halogen that is a less powerful oxidising agent from a metal halide (F will always displace Cl from NaCl etc)

#5
Front (Question)

Describe: The trend in reducing powers

Back (Answer)

Increases as you go down the group.

#6
Front (Question)

Observations: when NaCl reacts with H2SO4

Back (Answer)

• HCl - white steamy fumes (damp blue litmus turns red) (acid-base reaction)

#7
Front (Question)

Observations: when NaBr reacts with H2SO4 (and type of reaction)

Back (Answer)

• HBr - white steamy fumes - (damp blue litmus turns red) (acid-base reaction) • Br2 - Orange brown vapour • SO2 - Colourless choking gas (acidified Potassium Dichromate turns from orange to green) (redox equations)

#8
Front (Question)

Observations: when NaI reacts with H2SO4

Back (Answer)

• HI - white steamy fumes - (damp blue litmus turns red) (acid- base reaction) • I2 - Purple Vapour • SO2 - Colourless choking gas (acidified potassium dichromate paper turns from orange to green) • S - Yellow Solid • H2S - Foul egg smell (wet white lead ethanoate paper) turns black (redox reactions)

#9
Front (Question)

Describe: The Halide Ion Test - Part 1

Back (Answer)

• Add nitric acid to the solution to remove any impurities • Add Silver nitrate to the solution. • If Cl- (white), Br- (Cream) or I- (Yellow) is present _____ precipitate will form

#10
Front (Question)

Describe: The Halide Ion Test Part 2

Back (Answer)

• Add ammonia (aq) to the solution, if Cl- present ppt. will redisolve • If not add ammonia (l), if Br- present ppt. will redisolve • If no ppt. redissolves I- present.

#11
Front (Question)

Write the equations of: Cl2 and H2O in different conditions

Back (Answer)

• Cl2 (g) + H2O (l) <-> HCl (aq) + HClO (aq) • (in daylight) Cl2 (g) + H2O (l) -> 2HCl (aq) + 1/2O2 (g)

#12
Front (Question)

What are pros and cons of the uses of Chlorine and Chlorate (I)

Back (Answer)

Used in swimming pools and water treatment: Pros: removes bacteria harmful to health Cons: can taste unpleasant, too much chlorine harms health, no consent

#13
Front (Question)

Write the equation for the formation of bleach

Back (Answer)

Cl2 (g) + 2NaOH (aq) -> NaCl (aq) + NaClO (aq) + H2O (l) (NaClO is bleach)

#14
Front (Question)

Equation for NaCl reacting with H2SO4

Back (Answer)

NaCl + H2SO4 -> HCl + NaHSO4 acid-base reaction

#15
Front (Question)

Equation for Bromide ions reacting with sulfide ions to form sulfur dioxide - full and ionic

Back (Answer)

ionic: 4H(+) + 2Br(-) + SO4(2-) -> SO2 + Br2 + 2H2O full: 2H2SO4 + 2NaBr -> SO2 + 2H2O + Br2 + Na2SO4

#16
Front (Question)

Equation for Iodide ions reacting with sulfuric acid to form hydrogen sulphide. Give both ionic and full

Back (Answer)

ionic: H2SO4 + 8H+ + 8I- -> H2S + 4I2 + 4H2O full: 8NaI + 5H2SO4 -> H2S + 4H2O + 4Na2SO4 + 4I2

#17
Front (Question)

Equation for Iodide reacting with sulfuric acid to form Sulfur

Back (Answer)

6NaI + 4H2SO4 -> 3I2 + 3Na2SO4 + S + 4H2O