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D.Chem 4- Inorganic + PT > Group 7 - Halogens > Flashcards

Group 7 - Halogens Flashcards

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1
Q

At room temp what is fluorine

A

Pale yellow gas

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2
Q

At room temp what is bromine

A

Brown/ orange liquid

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3
Q

At room temp what is chlorine

A

Pale green gas

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4
Q

At room temp what is iodine

A

Grey solid

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5
Q

Trend in boiling point group 7

A

Increase down group = more electrons = increase in London forces

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6
Q

Trend in electronegativity ( ability to attract electrons ) / reactivity

A

Decrease down group = atom gets larger = distance between nucleus and electrons increases = harder to attract electrons
( also more e shielding )

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7
Q

2NaI + Cl2 = 2NaCl + I2
What is happening in this reaction
What can you add to these reaction to make a observation

A

Displacement reaction
Less reactive halogen is replaced by more reactive halogen
Chlorine is the stronger oxidising agent
Adding hexane/organic solvent= makes it easier to see colour change as halogen present will dissolve readily in organic solvents
- coloured band forms above aqueous layer

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8
Q

Trend in oxidising strength down group 7

A
  • oxidising strength decreases down group 7
  • A halogen that is a strong oxidising agent will displace a halogen that has a lower oxidising power
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9
Q

Will chlorine displace potassium iodide

A

Yes
Brown solution then iodine forms ( grey solid)

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10
Q

Will bromine displace potassium chloride

A

No - chlorine is the stronger oxidising agent
- yellow solution due to bromine

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11
Q

What does the colour in the solution show

A
  • the free halogen present in solution
    Eg: BromINE not BromIDE
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12
Q

What colours are
Chlorine
Bromine
Iodine
In solution without organic solvent

A

Chlorine = pale green
Bromine = yellow
Iodine = brown/yellow solution

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13
Q

What are oxidising agents in terms of electrons

A

Electron acceptors

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14
Q

What colours are
Chlorine
Bromine
Iodine
In solution WITH organic solvent
Where are these colours ?

A

Chlorine= colourless
Bromine = yellow
Iodine = purple
Solvent layer forms on top of solution

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15
Q

What is the name of
HClO

A

Bleach

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16
Q

Reaction of halogens/Chlorine with cold NaOH

A

-Colour of halogen solution for all turn colourless= bleach formed
- mixture of NaCl + NaClO = bleach
Eg: Cl2 + NaOH = NaCl + NaClO + H2O

17
Q

Reactions of halogens with hot dilute NaOH

A

Basically same as cold
- however halogen that is oxidised goes to a higher oxidation state
Eg: Cl2 + NaOH = NaCl + NaClO3 + H2O

18
Q

Trend in reducing power of halides

A
  • down group reducing power of halides increases
  • as ions get bigger it is easier for outer electrons to be given away
19
Q

What do we use to see the difference in reducing power of halides

A
  • reaction between halide salts + sulphuric acid
    Eg: NaF + H2SO4
    To see how far halide can reduce sulphur
20
Q

Fluoride and chloride + sulphuric acid (H2SO4) results ?

A

Fluoride and chloride are not strong enough reducing agents to reduce H2SO4 .
No redox reaction occurs just acid-base
NaCl+ H2SO4 = NaHSO4 + HCl
Observation = steamy white fumes

21
Q

Bromide + sulphuric acid reaction

A

Bromide ions are stronger reducing agents than Cl- + F-
- br- reduces sulphur in H2S04 = SO2
Oxidation state of sulphur from +6 - +4

Observation= steamy white fumes(HBr)
- orange fume of Br2 gas

22
Q

Iodide ions + sulphuric acid

A

-iodide ions are the strongest halide reducing agents
- iodide reduces sulphur from +6 in H2S04 =
+4 in SO2
0 in S
-2 in H2S
Observations= white steamy fumes
- yellow solid of sulphur
- rotten egg smell H2S
- grey solid + purple fumes of iodine

23
Q

Test for halide ions procedure

A

1- add nitric acid = react and get rid of any carbonates
2- add silver nitrate solution
= forms coloured precipitate

24
Q

Colour of silver halides

A

Silver chloride = white
Silver bromide = cream
Silver iodide = yellow

25
Q

Solubility of silver halides in ammonia to further test for identity of halide present

A

Silver chloride = dissolves in dilute ammonia

Silver bromide = dissolves in conc ammonia

Silver iodide = does not dissolve

26
Q

Producing hydrogen halides
Reactants and observable

A

Solid sodium Halide salt + phosphoric acid= sodium phosphate + HCl

Observation = steamy white fumes = HCl dissolved in moisture in air

Phosphoric acid is used instead of sulphuric acid as there are no extra reactions / no other products

27
Q

Are hydrogen halides more or less dense than air

A

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D.Chem 4- Inorganic + PT (3 decks)

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