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Inorganic Chemistry > Group 7 - The Halogens > Flashcards

Group 7 - The Halogens Flashcards

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1
Q

What does F2 look like

A

Pale yellow gas

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2
Q

What does Cl2 appear as

A

A pale green gas

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3
Q

How does Br2 appear

A

Dark red/ brown/ orange liquid

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4
Q

How does I2 appear

A

Dark purple/ black solid

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5
Q

What is the trend in atomic radius for group 7

A

Increases down the group

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6
Q

What is the trend in electronegativity for group 7

Why?

A

Decreases down the group

Size increases
More shielding
So ability of nucleus to attract electrons is reduced

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7
Q

What is the trend in boiling point for group 7

Why

A

Boiling point increases down the group

All halogens are diatomic and as you go down the group the size of the atom increases and there are more Van der Waals forces between molecules

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8
Q

Halogens act as oxidising agents

True or false?

A

True

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9
Q

What happens when a halogen acts as an oxidising agent

A

Each halogen Atom gains an electron

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10
Q

What is the trend in the ability as an oxidising agent in group 7

Why

A

Decreases down the group

Atomic radius increases down the group and shielding increases
Halogen atom gains an electron less readily

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11
Q

Method to test displacement reaction

A

Aqueous solutions of the halogens are added drop-wise to a colourless solution containing halide ions; solutions of Potassium Chloride, Potassium bromide, and potassium iodide are usually added as the salts

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12
Q

What observations are seen when Cl2 is added to potassium bromide
Why?

Ionic equation for this reaction

A

Yellow/ brown solution of Br2
Cl2 oxides Br-

2Br- +Cl2 —>2Cl- +Br2

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13
Q

Observation for Cl2 added to potassium iodide
Why
Give ionic equation

A

Brown solution/ black PPT
Cl2 oxides I-
2I- +Cl2 —> 2Cl- +I2

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14
Q

Observations for Br2 + KCl

Why

A

No visible change

Br2 is not able to oxidise Cl2

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15
Q

Observation for Br2 + KI

A

Brown solution/ black PPT
Br2 oxidises I-
2I- + Br2 —> 2Br- + I2

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16
Q

Observation for I2 added to KCl

A

No visible change

I2 is not able to oxidise Cl-

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17
Q

What can chlorine oxidise

A

Br- and I-

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18
Q

What can Bromine oxidise

A

I- but not Cl-

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19
Q

What will iodine oxidise

A

Neither Cl- nor Br-

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20
Q

Which halogens are the strongest and weakest oxidising agents

A

F2 is the strongest

I2 is the weakest

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21
Q

Trend in ability of a halide ion to act as a reducing agent

A

Increases down group 7

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22
Q

How is trend in reducing powers of halide ions shown?

A

Reaction of solid halide salts with concentrated sulphuric acid

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23
Q

Oxidation state of S in H2SO4

A

+6

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24
Q

What can the S in H2SO4 be reduced to

A

+4, 0, or -2 depending on reducing power of the halide ion

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25
What is produced from NaF + H2SO4 What redox reaction occurs
Na2SO4 + 2HF No redox reaction occurs as F- is not a strong enough reduction agent to reduce S in H2SO4 Cl- is the same
26
Acid-base reaction for NaBr + H2SO4 Redox reaction of NaBr to give SO2 and half equation
2NaBr + H2SO4—> Na2SO4 + 2HBr 2H+ + H2SO4 + 2Br- —> Br2 + SO2 + 2H2O 2e- +2H+ +H2SO4 —> SO2 + H2O
27
Equation for NaI + H2SO4 acid base reaction
2NaI + H2SO4–> Na2SO4 +2HI
28
What are the 3 different products from the 3 redox reactions for NaI + H2SO4
SO2 - choking gas S - yellow solid H2S - smell of rotten eggs
29
How to identify HF, HCl, HBr, and HI (observation)
Misty fumes
30
Observation for production of Br2 I2?
Brown gas Black solid/ purple gas
31
Equation for redox reaction including I- to produce SO2
2H+ + H2SO4 + 2I- —> SO2 + 2H2O + I2
32
I- redox reaction to produce S
6H+ + H2SO4 + 6I- —> S +4H2O + 3I2
33
I- redox reaction to produce H2S
H2SO4 + 8H+ +8I- —> 4I2 + H2S + 4H2O
34
Strongest and weakest reducing agents of Halogens
``` Strongest = I- Weakest = F- ```
35
Which silver halides are soluble and insoluble
Soluble: Silver fluoride Insoluble: silver chloride, bromide, iodide
36
Why is HNO3 added to an aqueous halide solution before silver nitrate test
To remove hydroxides and carbonates that would form a precipitate
37
What colour PPT does each halide produce when added to AgNO3 and how soluble are they in NH3
F- : none as AgF is soluble Cl-: white; soluble in dilute NH3 Br-: cream; partially soluble in dilute NH3, soluble in conc NH3 I-: yellow; insoluble in conc NH3
38
What is formed when Cl2 is dissolved in water
HCl and chloric acid (HClO)
39
Equation for Cl2 dissolving in water Is Cl2 oxidised or reduced? What is the equilibrium mixture called and what colour is it
Cl2+H2O (equilibrium sign) HCl + HClO Both this is called disproportionation Chlorine water Pale green
40
What colour does litmus paper turn in chlorine water | Why
Red as Both reaction products are acidic Red then disappears and the UI turns white because HClO is a v effective bleach
41
Equation for chlorine and water in bright sunlight What is oxidised and reduced
2Cl2 + 2H2O—> 4HCl + O2 Chlorine oxidises water to O2 Chlorine is reduced to chloride ions
42
Why does chlorine water’s green colour fade in bright sunlight
Cl2 is converted to HCl and O2 which are colourless
43
Chlorine is toxic. Why is it still used to disinfect water
Health benefits outweigh the risks
44
Equations for chlorine reacting with cold dilute NaOH
Cl2 +2NaOH—> H2O + NaCl + NaClO Cl2 +2OH- —> H2O + Cl- +ClO- (ionic equation)
45
Why is Cl2 + NaOH of great commercial importance
NaClO is the active ingredient in household bleach
46
Test for CO3 2- ions
Add HCl | CO2 gas given off (effervescence)
47
Test for NH4+
Warm carefully Do not allow to spit Ammonia gas given off Which will turn damp litmus blue
48
Test for Ba2+
Add sulphuric acid | White ppt of barium sulphate produced
49
Test for OH-
Add magnesium chlorine White ppt of magnesium hydroxide formed Or Add universal indicator Turn blue
50
What must always be included when writing equations for group two metals and water
State symbols
51
When testing for halides what state must they be in
Aqueous
52
If a procedure asks the product to be pure what must you include
Filter Wash Dry
53
2 things to mention when discussing reducing ability
Size of ion | Attraction of nucleus to e-
54
Colour of Br(2) as gas
BROWN gas
55
Colour of I2(g)
PURPLE gas
56
Normal reaction of chlorine and water
Cl2 + water —-> HCl + HClO | Disproportionation
57
What are the products of mixing Cl2 and water
``` HCl Chloric acid (a weak acid) ```
58
Chlorine in sunlit water
Cl2 + H2O —-> HCl + O2 | Pale Green Colourless
59
Products of Cl2 + water in sunlight
HCl | O2
60
Observation when Cl2 is added to KBr
Yellow/ brown solution
61
Observation when Cl2 is added to I-
Black PPT | dark brown solutions
62
Observation when Br2 is added KI solution
Black PPT | Dark brown solution

Inorganic Chemistry (6 decks)

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