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AQA A-Level Chemistry > 2.2 Group 2 > Flashcards

2.2 Group 2 Flashcards

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1
Q

Melting point of group 2 elements

A

High
- Giant mettalic lattice
- Strong electrostatic forces of attraction
- Lots of energy to break metalic bonds

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2
Q

Density of group 2 (relative to group 1)

A

Higher density
- Group 2 ions are smaller
- Pack closer together

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3
Q

Reactivity of group 2 elements

A

All reactive metals (similar reactions as they have the same number of electrons in their outer shell)

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4
Q

Appearance of group 2 compounds

A

White crystalline ionic solids

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5
Q

Trend in atomic radius down group 2

A

Increases
- Atoms become larger
- More shellls + shielding
- Nuclear attraction to outer electron is less

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6
Q

Trend in first ionisation energy down group 2

A

Decreases
- More main shells + shielding
- Weaker attraction between nucleus and electron being removed

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7
Q

Trend in melting point down group 2

A

Decreases
- Metallic ions get bigger
- Less attraction between ions and delocalised electrons

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8
Q

Trend in reactivity down group 2

A

Increases
- React by losing electrons
- More shells + shielding
- Less nuclear attraction to the 2 outer electrons

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9
Q

Use of Magnesium

A

Extracting Ti from TiCl₄

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10
Q

Two reactions used to extract titanium from titanium oxide

A

React titanium oxide with chlorine and carbon
Reduce titanium chloride with magnesium

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11
Q

What makes titanium chloride easy to purify?

A

It is a liquid (distillation can be used)

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12
Q

Why is titanium difficult to extract from ores?

A

Reduction with carbon cannot be used (forms TiC, a brittle titanium carbide)

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13
Q

Trend in solubility down group 2 hydroxides

A

Increases

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14
Q

Solubility of Magnesium hydroxide

A

Sparingly soluable

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15
Q

Solubility of Barium hydroxide

A

Fully soluable

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16
Q

Trend in pH down group 2 hydroxides

A

Increases

17
Q

Why does pH change down group 2 hydroxides?

A

Differences in solubility changes the number of hydroxide ions released into a solution

18
Q

pH of Magnesium hydroxide

A

Around 8

19
Q

pH of Barium hydroxide

A

Around 13

20
Q

Use of Magnesium hydroxide

A

As an antacid to neutralise excess stomach acid

21
Q

Use of calcium hydroxide

A

In agriculture to neutralise acidic soil

22
Q

Trend in solubility down group 2 sulfates

A

Decreases

23
Q

Solilubility of Magnesium sulfate

A

Fully soluable

24
Q

Solubility of Barium sulfate

A

Insoluable

25
Q

Solubility of Calcium sulfate

A

Sparingly soluable

26
Q

Use of Barium sulfate

A

Used in medicine (Barium meal) as it absorbs x-rays allowing soft tissue to be seen.

27
Q

Why is Barium sulfate used in medicine despite Barium ions being toxic?

A

It is insoluble so cannot be absorbed into the blood

28
Q

Uses of calcium compounds

A

To remove sulfur dioxide from flue gas (flue gas desulfurizarion)

29
Q

Reaction of Mg with water

A
  • Cold water: Forms Mg(OH)₂(s) + H₂(g) in a very slow reaction
  • With steam: Forms MgO(s) + H₂(g) and a bright white light
30
Q

Reaction of Ca with water

A
  • Forms Ca(OH)₂(s) + H₂(g)
  • Calcium hydroxide is slightly soluble and gives an alkaline solution
  • White solid is still seen
    (cold water)
31
Q

Reaction of Sr with water

A
  • Forms Sr(OH)₂(aq) + H₂(g)
  • Strontium hydroxide forms an alkaline solution
  • Some white solid is still seen
    (cold water)
32
Q

Reaction of Ba with water

A
  • Forms Ba(OH)₂(aq) + H₂(g)
  • Barium hydroxide forms a strongly alkaline solution
  • No white solid is seen
    (cold water)
33
Q

Trend in reactivity with water as you go down group 2

A

Increases

34
Q

Equation for forming titanium(IV) chloride from titanium ore

A

TiO₂ + 2Cl₂ + 2C –> TiCl₄ + 2CO

35
Q

Equation for reducing titanium(IV) chloride with magnesium

A

TiCl₄ + 2Mg –> 2MgCl₂ + Ti

36
Q

Test for Mg²⁺(aq) ions

A

Add aqueous sodium hydroxide, a thick white precipitate will form as Mg(OH)₂ is sparingly soluble

37
Q

Test for Ba²⁺(aq) ions

A

Add sulfuric acid or aqueous sodium sulfate, a thick white precipitate will form as BaSO₄ is insoluable

38
Q

What can barium salts be used for?

A

Testing for SO₄²⁻ ions (will form precipitate of BaSO₄ if present)

39
Q

What can magnesium salts be used for?

A

Testing for OH⁻ ions (will form precipitate of Mg(OH)₂ if present)

AQA A-Level Chemistry (13 decks)

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