3.1.3: The halogens Flashcards

1
Q

Test for halide ions

A

Add a few drops of aqueous silver nitrate

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2
Q

Results for halide ions test

A

Chloride - white ppt
Bromide - cream ppt
Iodide - yellow ppt

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3
Q

Add what to halide ppt as a further test?

A

Aqueous ammonia

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4
Q

Results of adding aqueous ammonia to halide ion ppt?

A

Chloride - white ppt - dissolves in dilute ammonia

Bromide - cream ppt - dissolves in aqueous ammonia

Iodide - yellow ppt - does not dissolve even in conc NH3

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5
Q

Displacement of halogens method

A
  • Add an aqueous solution of the halogen
  • To an aqueous solution of the halide
  • Record the colour of the top (displaced) layer

e.g. KBr⁻ + Cl₂ –> 2KCl + Br₂

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6
Q

Ionic equation for halide ions test

A

Ag+ + X- —> AgX

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7
Q

Displacement of halogens - test results

A
  • Organic layer orange - bromine has been displaced

* Organic layer violet/purple - iodine has been displaced

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8
Q

Displacement of halogens - most reactive to least reactive

A

Most = chlorine
Bromine
Least = Iodine

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9
Q

Reactivity of Group 7 elements __________ down group

A

decreases

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10
Q

Why does reactivity of Group 7 elements decrease down group?

A
  • Larger atomic radius, more shielding means reduced force of positive charge felt by outermost shell of e-
  • Harder to attract electron to outer shell (lower e- affinity)
  • Less reactive
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11
Q

Boiling point _______ down Group 7

A

increases

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12
Q

Why does boiling point increase down Group 7?

A
  • Greater n(e-)

* Greater London forces between molecules

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13
Q

Bond enthalpy _______ down Group 7

A

decreases

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14
Q

Why does bond enthalpy decrease down Group 7?

A
  • Halogen atom gets larger so X-X bond gets longer and weaker
  • Fluorine is anomalous –> so small that e- repel
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15
Q

Electronegativity ______ down Group 7

A

decreases

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16
Q

Why does electronegativity decrease down Group 7?

A
  • Atom of X gets larger
  • More shells of e- means better shielding
  • Harder to attract the e- in a covalent bond
17
Q

Disproportionation reaction

A

where both oxidation and reduction occur to the same element in a redox reaction.