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AQA A Level Chemistry > Group 2 and Group 7 > Flashcards

Group 2 and Group 7 Flashcards

1
Q

Test for Halide Ions

A

Add Nitric Acid (to remove carbonate Ions)
Add Silver Nitrate

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2
Q

Test for Group 2 Metal Ions

A

Add Sodium Hydroxide in excess
white precipitate (Ca + Mg)
or
Add Sulfuric Acid in excess
white precipitate (Ba + Sr)
or
Dip nichrome wire loop in concentrated HCl (to clean it)
Dip in unknown compound
Hold in blue Bunsen Flame
Observe colour

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3
Q

Test for Sulfate Ions

A

Add Dilute HCl
Add Barium Chloride
White Precipitate

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4
Q

Test for Hydroxide Ions

A

Add dilute Magnesium Chloride
White Precipitate

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5
Q

Test for Ammonium Ions

A

Add Sodium Hydroxide
Shake and heat gently
Test fumes with Damp Red Litmus Paper
Blue

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6
Q

Equation for reaction between Magnesium and Steam

A

Mg(s) + H2O(l) -> MgO(s) + H2 (g)

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7
Q

Trend in solubility of Group 2 Hydroxides down the group

A

Increasing
Mg= insoluble
Ca= slightly soluble
Sr= soluble
Ba= soluble

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8
Q

Trend in solubility of Group 2 Sulfates down the group

A

Decreasing
Mg= soluble
Ca= slightly soluble
Sr= insoluble
Ba= insoluble

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9
Q

Equations for using Magnesium to extract Titanium from its Ore

A

TiO2 + 2C + 2Cl2 -> TiCl4 + 2CO
TiCl4 + 2Mg -> Ti + 2MgCl2

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10
Q

Use for Calcium Hydroxide and Calcium Carbonate

A

Neutralise Fields

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11
Q

Use for Calcium Oxide

A

Remove Sulfur Dioxide from Flue Gas

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12
Q

Use for Barium Sulfate

A

Barium Meal for X-Rays of the Digestive System

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13
Q

Equation for reaction between Group 2 Metal (X) and Water

A

X + 2H2O -> Ca(OH)2 + H2

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14
Q

The colour of the Precipitate formed by Magnesium Hydroxide

A

White

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15
Q

The Group 7 Element that is the best Oxidising Agent

A

Fluorine (too dangerous to use in school)

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16
Q

The colour formed by Br- + Cl2(aq)

A

Orange

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17
Q

The colour formed by I- + Cl2(aq)

A

Brown

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18
Q

The colour formed by I- + Br2(aq)

A

Brown

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19
Q

Use of Fluorine

A

Making Plastics

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20
Q

Use for Chlorine

A

Bleach and Disinfectants

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21
Q

Use for Bromine

A

Testing saturation + Water Purification

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22
Q

Use for Iodine

A

Antiseptics and Mineral Supplements

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23
Q

State of Fluorine at Room Temperature

A

Gas

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24
Q

State of Chlorine at Room Temperature

A

Gas

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25
Q

State of Bromine at Room Temperature

A

Liquid

26
Q

State of Iodine at Room Temperature

A

Solid

27
Q

First Equation for Reducing Power of Iodine

A

H2SO4 (l) + NaI (s) -> NaHSO4 (s) + HI (g)

28
Q

Second Equation for Reducing Power of Iodine

A

2HI (g) + H2SO4 (l) -> I2 (g) + SO2 (g) + 2H2O (l)

29
Q

Third Equation for Reducing Power of Iodine

A

6HI (g) + H2SO4 (l) -> 3I2 (g) + S (s) + 4H2O (l)

30
Q

Fourth Equation for Reducing Power of Iodine

A

8HI (g) + H2SO4 (l) -> 4I2 (s) + H2S (g) + 4H2O (l)

31
Q

Another name for Sulfur Dioxide

A

Choking Gas

32
Q

The Colour of Solid Sulfur

A

Yellow

33
Q

The Colour of Solid Iodine

A

Black

34
Q

The scent of Dihydrogen Sulfide

A

Rotton Egg

35
Q

Colour of Silver Chloride Precipitate

A

White

36
Q

Colour of Silver Bromide Precipitate

A

Cream

37
Q

Colour of Silver Iodide Precipitate

A

Yellow

38
Q

The Silver (Group 2) compounds that dissolve in Dilute Ammonia Solution

A

Silver Chloride

39
Q

The Silver (Group 2) compounds that dissolve in Concentrated Ammonia Solution

A

Silver Chloride and Silver Bromide

40
Q

Equation for the reaction between Sodium Hydroxide and Chlorine to form Bleach

A

2NaOH (aq) + Cl2 (g) -> NaCl (aq) + NaClO (aq) + H2O (l)

41
Q

Product for reaction between Sodium Hydroxide and Chlorine

A

Salty Bleach Water
(NaCl + NaClO + H2O)

42
Q

Definition of Disproportionation Reaction

A

One Element in a reaction is both Oxidised and Reduced

43
Q

Benefits of using Chlorine to treat water

A

Cl- kills bacteria
Prevents Algae growth
Prevents Cholera Epidemic

44
Q

Risks of using Chlorine to treat water

A

Chlorine is a Toxic Gas
Increases risk of cancer when reacts with organic compounds (carcinogenic)

45
Q

Ionic Equation for Barium Sulfate

A

Ba 2+ (aq) + SO4 2- (aq) -> BaSO4 (s)

46
Q

Ionic Equation for Magnesium Hydroxide

A

Mg 2+ (aq) + 2OH- (aq) -> Mg(OH)2 (s)

47
Q

Test for carbonate Ions

A

Add Any Acid
Bubble gas produced through Limewater
Cloudy Limewater

48
Q

Trend in Atomic Radius down Group 2

A

Increasing

49
Q

Trend in First Ionisation Energy down Group 2

A

Decreasing
As you go down, shells are gained- so it is easier to lose an electron

50
Q

Trend in Melting Point down Group 2

A

Decreasing
Going down the group, metal ions get bigger, but the number of delocalised electrons does not change

51
Q

The equations for the use of Calcium Compounds to remove Sulfur Dioxide from Flue Gas

A

CaO (s) + 2H2O (l) + SO4 (g) -> CaSO3 (s) + 2H2O (l)
CaCO3 (s) + 2H2O (l) + SO2 (g) -> CaSO3 (s) + 2H2O (l) + CO2 (g)

52
Q

Trend in Boiling Point down Group 7

A

Increasing
Increasing strength of Van der Waals as size and relative mass of the molecules increases

53
Q

Trend in Electronegativity down Group 7

A

Decreasing
Atomic radius increases and Electron Shielding Increases

54
Q

Equation for the reaction between Chlorine and Water
Name this type of reaction
Name the Chlorine Product

A

Cl2 (g) + H2O (l) -><- 2H+ (aq) + Cl- (aq) + ClO- (aq)
Disproportination
Chloride Ions and Chlorate (I) Ions

55
Q

Equation for the reaction between Chlorine and Water in the presence of Sunlight

A

Cl2 (g) + H2O (l) -><- 2H+ (aq) + 2Cl- (aq) + 1/2O2 (g)

56
Q

Use for Chlorate (I) Ions

A

To treat water, kill bacteria

57
Q

Risks of using Chlorate (I) Ions to treat water

A

Chlorine Gas is harmful to breathe in
Liquid Chlorine on skin or eyes causes severe chemical burns
When combined with Organic Matter, carcinogenic

58
Q

The colour flame Calcium Ions would produce

A

Brick Red

59
Q

The colour flame Strontium Ions would produce

A

Red

60
Q

The colour flame Barium Ions would produce

A

Pale Green

AQA A Level Chemistry (9 decks)

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