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A-Level Chemistry > 3.2.2/3.2.3 - Group 2 and Group 7 > Flashcards

3.2.2/3.2.3 - Group 2 and Group 7 Flashcards

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1
Q

Define a reducing agent

A

An electron donor

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2
Q

Describe the trend in the reducing strength of halides

A
  • Increases down the group
  • Ionic radius increases
  • Weaker attraction between outer electron and nucleus
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3
Q

What is the observation for SO2?

A

(Acidic) Choking gas

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4
Q

What is the observation for S?

A

Yellow solid

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5
Q

What is the observation for H2S

A

Smell of bad eggs

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6
Q

What forms SO2?

A

Br- and I-

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7
Q

What forms S?

A

I-

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8
Q

What forms H2S?

A

I-

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9
Q

What is the observation for this reaction:
2I- -> I2 + 2e-

A

Black solid

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10
Q

What is the observation for this reaction:
2Br- -> Br2 + 2e-

A

Brown fumes

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11
Q

What do F and Cl undergo when they react with H2SO4?

A

Acid-base reactions

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12
Q

What is the ionic equation for H2SO4 reaction with F and Cl?

A

H+ + F- -> HF
H+ + Cl- -> HCl

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13
Q

What is the observation for H2SO4 and F?

A

Misty fumes of HF gas

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14
Q

What is the observation for H2SO4 and Cl?

A

Misty fumes of HCl gas

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15
Q

What are the steps for the halide test?

A
  1. Dissolve sample in water
  2. Add HNO3
  3. Add AgNO3(aq) solution
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16
Q

What are the observations from adding HNO3 and AgNO3 in a halide test?

A
  • Fluoride: No precipitate
  • Chloride: White precipitate
  • Bromide: Cream precipitate
  • Iodide: Yellow precipitate
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17
Q

What are the observations after adding dilute NH3?

A
  • Chloride: White precipitate dissolves
  • Bromide: Cream precipitate insoluble
  • Iodide: Yellow precipitate insoluble
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18
Q

What are the observations after adding concentrated NH3?

A
  • Bromide: Cream precipitate dissolves
  • Iodide: Yellow precipitate insoluble
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19
Q

Equation for AgCl and NH3

A

AgCl(s) + 2NH3 -> [Ag(NH3)2]+(aq) + Cl-(aq)

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20
Q

Equation for AgBr and NH3

A

AgBr(s) + 2NH3 -> [Ag(NH3)2]+(aq) + Br-(aq)

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21
Q

Define oxidising reagent

A

Electron acceptor

22
Q

What is the trend in oxidising ability of halogens?

A
  • Decrease down the group
  • Larger radius = weaker attraction between nucleus and outer electron
23
Q

What is the ionic equation for:
Chlorine + Sodium Bromide -> Bromine + Sodium Chloride

A

Cl2 + 2Br- -> Br2 + 2Cl-

24
Q

Observation when Cl2 reacts with Br-

A

Br2 produced - orange solution

25
Q

Observation when Cl2 reacts with I-

A

I2 produced - brown solution (black solid)

26
Q

Observation when Br2 reacts with I-

A

I2 produced - brown solution (black solid)

27
Q

Why is chlorine added to water?

A

Sterilises water by killing bacteria

28
Q

Why must chlorine be added in low concentrations?

A

It is toxic

29
Q

What is the reaction between chlorine and water?

A

H2O + Cl2 <–> HCl + HClO

30
Q

What is disproportionation?

A

A reaction in which a substance is simultaneously oxidized and reduced, giving two different products

31
Q

What is the trend in the reactivity of group 2 metals down the group?

A

Increases

32
Q

Equation for a group 2 metal reacting with liquid water

A

X(s) + H2O(l) -> X(OH)2 + H2(g)

33
Q

Equation for a group 2 metal reacting with steam

A

X(s) + H2O(g) -> XO(s) + H2(g)

34
Q

What are the observations of reaction with group 2 metals and water?

A
  • White solid produced
  • Bright white light
35
Q

Equation for when Mg is used in the extraction of Ti from TiCl4

A

TiCl4 + 2Mg -> 2MgCl2 + Ti

36
Q

What agent is Mg during its use in the extraction of Ti

A

Reducing agent

37
Q

What is the trend of the solubility of group 2 hydroxides?

A

Increases down the group

38
Q

Ionic equation for the formation of Magnesium Hydroxide

A

Mg2+ + 2OH- -> Mg(OH)2

39
Q

What is the observation for reaction between Mg and OH-?

A

White precipitate forms

40
Q

What can be used to test for the presence of Mg2+ ions in a solution?

A

NaOH

41
Q

What can be used to test for the presence of OH- ions in a solution?

A

Mg(NO3)2

42
Q

Uses of Magnesium Hydroxide?

A
  • Indigestion relief (neutralises stomach acid)
  • Often called “milk of magnesia”
43
Q

What is the trend in the solubility of group 2 sulphates?

A

Decreases down the group

44
Q

Ionic equation for the formation of Barium Sulphate

A

Ba2+ + SO4 2- -> BaSO4

45
Q

What can be used to test for the presence of Ba2+ ions in a solution?

A

H2SO4 or Na2SO4

46
Q

What is the observation for reaction between Ba and SO4 2-?

A

Formation of a white precipitate

47
Q

What can be used to test for the presence of SO4 2- ions in a solution?

A

Acidified BaCl2

48
Q

Uses of Barium Sulphate

A
  • Stomach X-rays (barium meal)
49
Q

What are the dangers of using Ba2+ ions?

A

They are toxic

50
Q

Observation with the reaction with carbonate impurities

A

Effervescence

A-Level Chemistry (5 decks)

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