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CCEA AS Chemistry Units 1, 2 And 3 > (U1) Halogens > Flashcards

(U1) Halogens Flashcards

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1
Q

What colour and state is Fluorine

A

Yellow gas

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2
Q

what colour and state is Chlorine

A

Yellow-Green gas

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3
Q

what colour and state is Bromine

A

Red-Brown liquid

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4
Q

what colour is solid Iodine

A

Grey-Black

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5
Q

what colour is Iodine vapor

A

Purple

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6
Q

what colour is Chlorine water

A

Pale Green/Colourless

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7
Q

what colour is Bromine water

A

Brown

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8
Q

what colour is Iodine in POLAR solvents

A

Yellow-Brown

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9
Q

what colour is Iodine in NON-POLAR Solvents

A

Purple

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10
Q

What is the observation for reactions between:

  • Fluorides and
  • Concentrated Sulfuric Acid

(Not needed as much)

A

Steamy/Misty Fumes (of HF)

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11
Q

What is the observation for reactions between:

  • Chlorides and
  • Concentrated Sulfuric Acid
A

Steamy/Misty Fumes (of HCI)

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12
Q

What are the observations for reactions between:

  • bromides and
  • Concentrated Sulfuric Acid
    (3)
A
  • Steamy/Misty Fumes ( HBr)
  • Red-Brown Vapour (Br 2 )
  • pungent smell
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13
Q

What are the observations for reactions between:

  • Iodides and
  • Concentrated Sulfuric Acid
    (7)
A

3 reactions:

1.

  • Steamy/misty fumes (of HI)
    • Purple Vapour (I2)
    • pungent smell (SO2)
    • Yellow solid (S)
    • Smell of Rotten Eggs (H2S)
    • Grey-Black solid (on the sides of the test tube) (I2)
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14
Q

What is the observation for reactions between:

  • solid fluorides and
  • Concentrated phosphoric Acid
A

Steamy/misty fumes (of HF)

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15
Q

What is the observation for reactions between:

  • Chlorides and
  • Concentrated phosphoric Acid
A

Steamy/misty fumes (of HCI)

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16
Q

What is the observation for reactions between:

  • Bromides and
  • Concentrated phosphoric Acid
A

Steamy/misty fumes (of HBr)

17
Q

What is the observation for reactions between:

  • Iodides and
  • Concentrated phosphoric Acid
A

Steamy/misty fumes (of HI)

18
Q

State every reaction between sodium iodide and sulphuric acid in order

A
  • NaI + H2SO4 —> HI + NaHSO4
  • HI + H2SO4 —> SO2 + I2 + 2H2O
  • 6HI + H2SO4 —> S + I2 + 4H2O
  • HI + H2SO4 —> H2S + I2 + H2O

Last 2 reactions occur because iodide ions are greater reducing agents than halides up the group

19
Q

What happens to the oxidising ability of halogens down the group?

A

Oxidising ability decreases

20
Q

What happens to the reducing ability of halides down the group?

A

Reducing ability increases

21
Q

Why are halide ions reducing agents while atoms are oxidising agents? (3)

A
  • ions lose electrons more readily
  • larger atomic radius + greater shielding make this easier
  • also halogen atoms would rather gain electrons than lose (oxidising agents), ions are stable

CCEA AS Chemistry Units 1, 2 And 3 (22 decks)

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