10.Group 7, the halogens Flashcards

1
Q

Describe the trend in size of atoms going down group 7

A
  • going down the group atoms get bigger

- each element has one extra filled main level of electrons

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2
Q

Describe the trend in electronegativity going down in group 7

A
  • electronegativity is the power of an atom to attract shared electrons in a covalent bond
  • going down the group electronegativity decreases
  • atoms get bigger and more shielding, going down a group
  • less nuclear attraction between halogen nucleus and shared electrons electrons in the covalent bond
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3
Q

Describe the trend in melting and boiling points going down in group 7

A
  • increase as you go down a group
  • larger atoms have more electrons
  • larger van der Waal forces
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4
Q

Define volatile

A

Easily evaporated at normal temperatures

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5
Q

Which is more volatile chlorine or iodine

A
  • the lower the boiling point the more volatile the element

- so chlorine is more volatile

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6
Q

Describe the trend in oxidising ability going down a group

A
  • going down a group the oxidising ability decreases
  • shielding and atom radii increases going down
  • nuclear attraction decreases
  • this reduces the ability for atom to attract (accept) electrons
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7
Q

How do halogens react with metal halides

A

By displacement reaction. Halide in the compound will be displaced by a more reactive halogen.

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8
Q

Write the ionic equation for the extraction of bromine from sea water

A

Cl2 (aq) + 2Br- (aq) —> Br2 (aq) + 2Cl- (aq)

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9
Q

Describe how iodine is extracted from kelp

A
  • salts such as NaCl KCL and K2S04 are removed by washing with water
  • residue is then heated with manganese dioxide and conc. sulfuric acid and iodine is liberated
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10
Q

Write the ionic equation for the extraction of iodine from kelp

A

2I- +MnO2 + 4H+ —-> Mn2+ + 2H2O +I2

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11
Q

Describe the trend in reducing ability going down a group

A
  • going down a group the oxidising ability increases
  • shielding and atomic radii increases
  • reducing nuclear attraction
  • this increases the ability for atom to lose (donate) electrons
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12
Q

What reactions shows the trend in reducing ability

A

Reaction of solid sodium halides with conc. sulfuric acid

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13
Q

Name a observation when conc. sulfuric acid is added to NaCl

A

Steamy fumes of hydrogen chloride

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14
Q

Name the solid product when conc. sulfuric acid is added to NaCl

A

Hydrogensulfate

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15
Q

Write the equation for when conc. sulfuric acid is added to NaCl

A

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

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16
Q

Is the reaction between conc. sulfuric acid and NaCl a redox reaction

A
  • no
  • as no oxidation state has changed
  • the chlorine ion is too weak a reducing agent to reduce the sulphur
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17
Q

What kind of reaction is the reaction between conc. sulfuric acid and NaCl

A

Acid-base reaction

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18
Q

Name a observation when conc. sulfuric acid is added to NaBr

A

Steamy fumes of hydrogen bromide and brown fumes of bromine

19
Q

What colour is bromine gas

20
Q

Describe two reactions that occur when conc. sulfuric acid is added to NaBr

A
  • first sodium hydrogensulfate and HBr are produced in an acid-base reaction
  • bromide ions are strong enough reducing agents to reduce sulfuric acid to sulfur dioxide
21
Q

Write the equations for when conc. sulfuric acid is added to NaBr and what reactions they are

A

1) NaBr (s) + H2SO4 (l) —-> NaHSO4 (s) + HBr (g)
an acid base reaction
2) 2H+ +2Br- + H2SO4 (l) —-> SO2 (g) + 2H2O (l) + Br2 (l)
a redox reaction

22
Q

Name a observation when conc. sulfuric acid is added to NaI

A
  • steamy fumes of HI
  • black solid of iodine
  • bad egg smell of hydrogen sulfide
23
Q

Describe two reactions that occur when conc. sulfuric acid is added to NaI

A
  • first sodium hydrogensulfate and HI are produced in an acid-base reaction
  • iodine ions are better reducing agents so reduce the sulfuric acid even further to sulfur dioxide sulfur and hydrogen sulfide are produced
24
Q

Write the equations for when conc. sulfuric acid is added to NaI and what reactions they are

A

1) NaI (s) + H2SO4 (l) —-> NaHSO4 (s) + HI (g)
an acid base reaction
2) 8H+ + 8I- + H2SO4 (l) —-> H2S (g) + 4H2O (l) + 4I2 (l)
a redox reaction

25
Write an ionic equation for reaction of metal chlorides with silver ions
Cl- (aq) +Ag+ (aq) ---->AgCl (s)
26
Describe the steps in identifying metal halides with silver ions
- dilute nitric acid is added to the solution to get rid of any soluble carbonate or hydroxide impurities - add a few drops of silver nitrate which forms the halide precipitate
27
How would carbonates or hydroxides interfere with identifying metal halides with silver ions
-forming silver carbonate 2Ag+ (aq) + CO3 2- (aq) ----> Ag2CO3 (s) -forming silver hydroxide Ag+ (aq) + OH- (aq) ----> AgOH (s)
28
Write the equations for getting rid of soluble carbonate or hydroxide impurities
CO3 2- (aq) + 2H+ (aq) ----> CO2 (g) + H2O (l) | OH- (aq) + H+ (aq) ----> H2O (l)
29
What are the results form the identifying metal halides with silver ions test
- silver fluoride :no precipitate - silver chloride: white precipitate - silver bromide: cream precipitate - silver iodide: pale yellow precipitate
30
What further test can be done to distinguish silver halides
- add a few drop of a dilute ammonia - then add a few drops of concentrated ammonia - silver chloride: dissolves in dilute ammonia - silver bromide: dissolves in conc. ammonia - silver iodide: insoluble in conc. ammonia
31
Write the equation for the reaction between chlorine and water
Cl2 (g) +H2O (l) ---> HClO (aq) + HCl (aq)
32
What kind of reaction is the reaction between chlorine and water
Disproportionation
33
What is a disproportionation reaction
Describes a redox reaction in which the oxidation number of some atoms of a particular element increases and that of other atoms of the same atom decrease
34
Name a use for the reaction between chlorine and water
Purify drinking water and swimming baths as the chloric acid kills bacteria by oxidation (as it is an oxidising agent) It is also a bleach
35
Describe the reaction between chlorine and water in sunlight
2Cl2 (g) +2H2O (l) ----> 4HCl (aq) + O2 (g) | pale green ----> colourless
36
Describe an alternative to the direct chlorination of swimming pools
-add solid sodium (or calcium) chlorate (I). This dissolves in water to form chloric acid, HClO (aq)
37
Write an equation for sodium chlorate and water
NaClO (s) + H2O Na+ (aq) + OH- + HClO (aq)
38
Why do swimming pools with sodium chlorate dissolved need to be slightly acidic
-in alkaline solution the equilibrium moves to the left and the HClO is removed as ClO-
39
Write the equation for the reaction with chlorine and alkali
Cl2 (g) + 2NaOH (aq) ----> NaClO (aq) + NaCl (aq) + H2O (l)
40
Describe the reaction for the reaction with chlorine and alkali
Chlorine reacts with cold, dilute sodium hydroxide to form sodium chlorate (I), NaClO.
41
What is NaClO
- oxidising agent | - active ingredient in household bleach
42
What kind reaction of is the reaction with chlorine and alkali
Disproportionation
43
Name two disproportionation reactions
- chlorine + alkali | - chlorine + water