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Chemistry Content > Group 7 Halogens And Redox > Flashcards

Group 7 Halogens And Redox Flashcards

1
Q

What is oxidising power

A

The ability to remove an electron

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2
Q

Oxidising power trend

A

Cl2> Br2 > I2

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3
Q

The reaction table of halogens for oxidising power

A
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4
Q

The equation of Cl2 and KCl

A

There is no reaction

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5
Q

The reaction between Br2 and KCl

A

There is no reaction

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6
Q

The reaction of KCl and I2

A

There is no reaction

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7
Q

Why is there no reaction of KCl with the halides

A

As Br2 and I2 are not a good oxidising powers. They have a bigger atomic radius than Cl2 which mean it cannot remove an electron from the potassium as easily as Cl2 can.

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8
Q

The reaction of KBr and Cl2

A
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9
Q

The ionic equation of KBr and Cl2

A
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10
Q

What is the observation we see with the reaction of KBr and Cl2

A

Orange solution

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11
Q

The reaction of KI and Cl2 including ionic

A
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12
Q

The observation of KI and Cl2

A

Brown solution

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13
Q

The reaction of KI and Br2 including ionic

A
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14
Q

The observation of KI and Br2

A

Brown solution

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15
Q

Formation of bleach reaction

A
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16
Q

What is bleach, chemical formula

A

NaClO

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17
Q

What is bleach used for

A

Cleaning agent

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18
Q

What is the reaction of bleach called and why

A

Disproportionation as the chlorine is being oxidised and reduced at the same time

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19
Q

The reaction of Cl2 and H20

20
Q

The reaction of Cl2 and H20 in UV light

21
Q

Is Cl2 and H20 reaction a disproportionation reaction

22
Q

Why is chlorine used for water treatment even though it is toxic

A

The benefits outweighs the risks

23
Q

Reducing power of halides

A

I2>Br2>Cl2

24
Q

What is reducing power

A

The ability to lose an electron

25
Q

Why is Iodine a good reducing agent

A

It can easily lose its electron because there is a weaker force of attraction between nucleus and outer electron compared to chlorine

Iodine can easily be oxidised (lose and electron) so it acts as a reducing agent. Something oxidised is a reducing agent and something reduced is an oxidising agent

26
Q

Reaction of NaCl and H2SO4

27
Q

Reaction of NaF with H2SO4

28
Q

Observation of NaCl and H2SO4

A

Misty white fumes (HCl produced)

29
Q

Observation of NaF and H2SO4

A

Misty white fumes (HF produced)

30
Q

Reaction of NaBr and H2SO4 the two equations

31
Q

Observation of NaBr and H2SO4

A 
Misty white fumes (HBr produced) 
Brown fumes (Br2 gas produced)
32
Q

Reaction of NaI and H2SO4 four reactions

A
  1. 8HI + H2SO4 —-> 4I2 +H2S +4H2O
33
Q

Observation of NaI and H2SO4

A

Misty white fumes (HI produced)
Black solid/ purple fumes (I2 produced)
Bad egg smell, toxic (H2S produced)
Yellow solid (sulfur produced)

34
Q

Test for halides

A

Add HNO3 which is acid that removes unwanted ions such as Carbonate ions
Add Silver Nitrate (AgNO3)

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

35
Q

Ionic equation for test of halides

36
Q

Ionic equation for halide Cl2

37
Q

Ionic equation for halide test Br2

38
Q

Ionic equation for halide test Br2

39
Q

Trend of atomic radius in group 7

A

Increases
More shells
More shielding
So bigger atoms

40
Q

Trend of electronegativity in group 7

A

Decreases
More shells
More shielding
Weaker attraction b/w nucleus and two electrons in covalent bond

41
Q

Trend of boiling/melting group 7

A 
Increases
More electrons 
Bigger atomic radius 
More vdw 
Higher melting and boiling between molecules as halogens are SCM
42
Q

Ionisation energy trend of group 7

A

Decreases
More shells
More shielding
Weaker forces of attraction b/w nucleus and electron in outer shell

43
Q

Displacement in aqueous solutions table of halides in an organic layer

44
Q

Oxidation state of H2

A

+1 unless joined to a metal - becomes -1

45
Q

Oxidation state of O2

A

-2 always unless joined to H2O2 (hydrogen peroxide) - becomes -1

46
Q

Table of reactions for reducing power along with equations

Chemistry Content (31 decks)

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