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HALOGENS Flashcards

1
Q

Describe fluorine (F2)

A

Pale yellow

Gas

Highly reactive

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2
Q

Describe chlorine (Cl2)

A

Greenish

Gas

Reactive

Poisonous in high concentrations

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3
Q

Describe bromine (Br2)

A

Red

Liquid

Gives off brown/orange poisonous fumes

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4
Q

Describe iodine (I2)

A

Shiny grey

Solid

Sublimes to purple gas

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5
Q

Describe the trend in melting point and boiling point in halogens

A

Increase down the group

As the molecules become larger they have more electrons

Larger Van Der Waals forces between molecules

More energy required to break the forces

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6
Q

Describe the trend in electronegativity of halogens

A

Decreases down the group

Increased atomic radii

Increased number of shells

Nucleus less able to attract bonding pairs of electrons

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7
Q

Describe the trend of halogens as oxidising agents

A

Decreases down the group

Strong halogen oxidising agents displace halogens with lower oxidising agents

From one of its compounds

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8
Q

Describe the reaction between aqueous chlorine and aqueous potassium chloride

A

Pale green solution

No reaction

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9
Q

Describe the reaction between aqueous chlorine and aqueous potassium bromide

A

Yellow solution

Cl displaces Br

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10
Q

Describe the reaction between aqueous chlorine and aqueous potassium iodide

A

brown solution

Cl displaces I

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11
Q

Describe the reaction between aqueous bromine and aqueous potassium chloride

A

Yellow solution

No reaction

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12
Q

Describe the reaction between aqueous bromine and aqueous potassium bromide

A

Yellow solution

No reaction

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13
Q

Describe the reaction between aqueous bromine and aqueous potassium iodide

A

Brown solution

Br displaces I

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14
Q

Describe the reaction between aqueous iodine and aqueous potassium chloride

A

Brown solution

No reaction

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15
Q

Describe the reaction between aqueous iodine and aqueous potassium bromide

A

Brown solution

No reaction

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16
Q

Describe the reaction between aqueous iodine and aqueous potassium iodide

A

Brown solution

No reaction

17
Q

Outline the reactions of halide ions with silver nitrate

A

Fluoride = no precipitate

Chloride = white precipitate

Bromide = Cream precipitate

Iodide = Pale yellow precipitate

18
Q

Describe the role of nitric acid in the reaction of halide ions with silver nitrate

A

Halide ion is dissolved in nitric acid

To react with any carbonates present

And prevent formation of Ag2CO3

Which would mask the desired observations

19
Q

Describe the reactions of silver halide precipitates and ammonia

A

AgCl = dissolves in dilute ammonia but not concentrated

AgBr = dissolves in dilute and concentrated ammonia

AgI = does not react with ammonia

20
Q

Describe the trend of halides as reducing agents

A

Increases down the group

Larger ion

Easier to donate outer electrons

Weaker attraction to nucleus

21
Q

Outline the reaction of fluoride salts with concentrated sulphuric acid

A

Acid-base reaction

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

White steamy fumes

22
Q

Outline the reaction of chloride salts with concentrated sulphuric acid

A

Acid-base reaction

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

White steamy fumes

23
Q

Outline the reaction of bromide salts with concentrated sulphuric acid

A

Acid-base reaction
NaBr(s) + H2SO4 (l) > NaHSO4(s) + HBr(g)
White steamy fumes

Redox reaction
2HBr + H2SO4 > Br2(g) + SO2(g) + 2H2O(l)
Red bromine fumes
Colourless acidic gas

24
Q

What are the two half equations or the redox step in bromine salts reacting with concentrated sulphuric acid

A

OX: 2Br- > Br2 + 2e-

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

25
Q

Outline the reactions of iodide salts with concentrated sulphuric acid

A

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

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

6HI + H2SO4 > 3I2(s) + S(s) + 4H2O(l)

8HI + H2SO4 > 4I2(s) + H2S(g) + 4H2O(l)

26
Q

Outline the observations of iodide salts with concentrated sulphuric acid

A

White steamy fumes

Black solid
Purple fumes

Colourless acidic gas

Yellow solid

Bad egg smell

27
Q

Define disproportionation

A

A reaction where an element simultaneously oxidises and reduces

28
Q

Reaction of chlorine with water

A

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

29
Q

Reaction of chlorine with water in the presence of sunlight

A

2Cl2 + 2H2O > 4H+ + 4Cl- + O2

30
Q

What is the use of a disproportionation reaction between chlorine and water

A

Treatment to kill bacteria

Drinking water

Swimming pools

Health outweighs toxic effects

31
Q

Reaction of chlorine with old dilute NaOH(aq)

A

Fades to colourless

Cl2(aq) + 2NaOH(aq) > NaCl(aq) + BaClO(aq) + H2O

32
Q

What is NaCl and NaClO used for

A

Bleach

To disinfect

And kill bacteria

33
Q

Name the chlorates and sulphates

A

NaClO sodium chlorate(I)
NaClO3 sodium chlorate (V)

K2SO4 potassium sulphate (VI)
K2SO3 potassium sulphate (IV)

AS CHEMISTRY (17 decks)

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