Group 7 Flashcards

1
Q

natural appearance & properties of halogens:

A

Fluorine (F2): very pale yellow gas. It is highly reactive
Chlorine : (Cl2) greenish, reactive gas, poisonous in high concentrations
Bromine (Br2) : orange brown liquid
Iodine (I2) : black/grey solid & brown in (aq)

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2
Q

oxidising strength down G7:

A

The oxidising strength decreases down the group.
Oxidising agents are electron acceptors.

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3
Q

displacement

The colour of the solution in the test tube shows which free halogen is present in solution.

A

Chlorine = very pale green solution (often colourless),
Bromine = yellow solution
Iodine = brown solution (sometimes black solid present)

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4
Q

natural state of halogens:

A

f2 & cl2: gasses
br2: liquid
i2: solid

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5
Q

disproportionation reaction:

A

one substance is both reduced and oxidised simultaneously

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6
Q

reaction of Cl2 with water:

hint: alkali + acid

A

cl2 + h2o <—> hcl + hclo

hclo kills bacteria in water preventing cholera

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7
Q

why no sunlight when cl2 reacts with water?

A

cl2 will decomopose to form hcl and o2

so no clo (I) ions so no benefits

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8
Q

testing for halide ions

How to test for halides?

A

HNO3 & AgNO3:
AgF: no visible change
AgCl: white ppt
AgBr: cream ppt
AgI: yellow ppt

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9
Q

when testing for halide ions why acidify?

A

to remove any other ions that could give a ppt with silver nitrate (aq)

if CO3- present, effervescence

would prod. false +ve white ppt

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10
Q

how to differentiate betw/ white (cl-) ppt and cream (br-) ppt

A
  • use dilute NH3 solution, if Cl- then ppt should dissolve
  • with con. NH3 solution, Br- ppt dissolves
  • no visible change with I-
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11
Q

test for SO2

A

filter paper soaked in k2cr2o7
changes from orange to green

prod. when h2so4 reacts with NaBr

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12
Q

products formed when I- reduces S in H₂SO₄

very strong reducing agent

A
  • S (S gets reduced, gaining 6 e-)
  • H₂S (eggy smell, reduced by 8 e-)
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13
Q

test for CO₂

A
  • bubble through limewater
  • white ppt forms
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14
Q

reaction for silver chloride with NH3 (to differentiate between cream and white solution)

A

AgCl(s) + 2 NH₃ (aq) –> [Ag(NH₃ )₂]+ + Cl-(aq)

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15
Q

testing for halides: method overview

A
  • make a solution of a solid halide salt
  • acidify with dilute nitric acid
    -> prevents the precipitation of other insoluble silver salts such as Ag₂CO3
  • add a few drops of silver nitrate solution
  • treat any precipitate with dilute ammonia solution
  • if a precipitate still exists, add concentrated ammonia solution
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16
Q

why can’t F- ions be tested for using Ag?

A

AgF is soluble in water (solubility decreases down the group) so
* no observable change

17
Q

A colourless solution contains a mixture of sodium chloride and sodium bromide.
Using aqueous silver nitrate and any other reagents of your choice, develop a procedure to prepare a pure sample of silver bromide from this mixture.
Explain each step in the procedure and illustrate your explanations with equations, where appropriate.
(6 marks)

A

Stage 1: formation of precipitates
*Add silver nitrate
*to form precipitates of AgCl and AgBr
*AgNO₃ + NaCl → AgCl + NaNO₃
*AgNO₃ + NaBr → AgBr + NaNO₃

Stage 2: selective dissolving of AgCl
*Add excess of dilute ammonia to the mixture of precipitates
*the silver chloride precipitate dissolves
*AgCl + 2NH → [Ag(NH₃)2]+ + Cl−

Stage 3: separation and purification of AgBr
*Filter off the remaining silver bromide precipitate
*Wash to remove soluble compounds
*Dry to remove water

18
Q

NaCO₃ +2HNO₃

A

—> CO₂ +H₂O +2NaNO₃

19
Q

Separate unlabelled solid samples of three anhydrous sodium compounds are provided for a student to identify.
These compounds are known to be sodium carbonate, sodium fluoride and sodium chloride but it is not known which sample is which.
Outline a logical sequence of test-tube reactions that the student could carry out to identify each of these compounds.
Include the observations the student would expect to make. Give equations, including state symbols, for any reactions that would take place.

A
  • Add nitric acid to all three
  • add water to make solution
  • add AgNo3.
  • Na2CO3 will fizz with acid
  • NaCl gives white precipitate with AgNO3
  • NaF shows no visible change (no ppt formed).
    ….
  • Na2CO3(s)+ 2HNO3(aq)→ 2NaNO3 + CO2 (g)+ H2O(l)
  • AgNO3(aq) + NaCl(s) → AgCl(s) + NaNO3(aq)
20
Q

Write equation of reaction betw/ cold Cl2 + dilute NaOH.
Give two uses of resulting solution. (3)

A

Cl 2 + NaOH ⟶ NaC l + NaClO3 + H2O
* bleach
* disinfectant / kills bacteria

21
Q

observation for reaction forming gaseous hydrogen halides

A

steamy fumes

22
Q

reaction between potassium bromide and sulfuric acid

redox

A

KBr + H2SO4 –> KHSO4 + HBr + Br2 + SO2 (steamy fumes)

23
Q

products formed when H2SO4 reacted with Br- and I- :

A
  • Br- : only strong enough to reduce to SO₂
  • I- : can reduce to SO₂, or S or H₂S
24
Q

Give the equation for solid NaBr with H2SO4

A

Acid- base step: NaBr(s) + H2SO4(l) ⟶ NaHSO4(s) + HBr(g)
Redox step: 2H+ + 2Br - + H2SO4 ⟶ Br2(g) + SO2(g) + 2 H2O(l)

Overall equation: combining two steps above:
2 NaBr + 3 H2SO4 ⟶ 2 NaHSO4 + SO2 + Br2 + 2 H2O