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Chemistry Year 12 > Group 2 > Flashcards

Group 2 Flashcards

1
Q

why does the first ionisation energy of group 2 elements decrease down the group

A

As you go down group 2 there’s an increase in shielding
There is a weaker attraction between the nucleus and the outer electron

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2
Q

what’s the equation for the third ionisation energu of magnesium being measured

A

Mg2+(g) => Mg3+ (g) + e-

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3
Q

why is the third ionisation energy of magnesium higher than the second ionisation energy of magnesium

A

the electron is removed from 2p sub shell
The electron being removed is less shielded than 3s

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4
Q

what’s the trend in atomic radius

A

Increases down the group .
As one goes down the group , the atoms have more shells of electrons making the atom bigger

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5
Q

what’s the trend in melting point

A

Decreases down the group
The metallic bonding weakens as the atomic size increases .
Distance between positive ions and delocalised electrons increases .
Electrostatic attractive forces between positive ions and delocalised electrons weaken

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6
Q

what’s the trend in 1st ionisation energy

A

Outermost electrons are held more weakly because they are successfully further from the nucleus.
The outer shell electrons become more shielded from the attraction of the nucleus by repulsive force of inner shell electrons

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7
Q

what’s the reaction of magnesium and oxygen and observation

A

2Mg + O2 => 2MgO
Mg burns with a bright white flame
MgO is a white solid with a high melting point due to its ionic bonding

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8
Q

what’s the reaction between magnesium and hcl

A

Mg + 2HCl => MgCl2 + H2

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9
Q

what’s the reaction between Magnesium oxide and hcl

A

MgO + 2HCl => MgCl2 + H2O

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10
Q

what’s the reaction of magnesium and steam and the observation

A

Mg (s) + H2O (g) => MgO ( s) + H2(g)
Burned with bright white flame

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11
Q

what’s the reaction of Mg and warm water and the observation

A

Mg + 2H2O => Mg(OH)2 + H2
Very slow
No flame

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12
Q

what’s the reaction with Ca and water

A

Ca + 2H2O ( l) => Ca(OH)2 (aq) + H2 (g)

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13
Q

what’s the reaction between Sr and water

A

Se + 2H2O ( l) => Sr(OH)2 (aq) + H2 (g)

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14
Q

what’s the reaction between Ba and water

A

Ba + 2H2O ( l) => Ba(OH)2 (aq) + H2 (g)

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15
Q

what’s the observation with metals ( Ca, Sr , Ba) and cold water

A
  • fizzing ( more vigorous down group)
  • metal dissolving ( faster down group)
  • solution heating up ( more down group)
  • with calcium a white ppt appearing ( less ppt forms down group with other metals )
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16
Q

why is titanium a very useful and what’s it used for

A

it’s abundant , has a low density and is corrosion resistant
- it’s used for making strong , light alloys for use in aircraft for example

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17
Q

what’s the steps in extracting titanium

A

1) TiO2 solid is converted to TiCl4 ( liquid ) at 900C :
2) The TiCl4 is purified by fractional distillation in an argon atmosphere
3) The Ti is extracted by Mg in an argon atmosphere at 500C

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18
Q

Why is titanium expensive

A

1) the expensive cost of Mg
2) This is a batch process so process is slower and requires more labour and energy is lost when reactor is cooled down
3) Due to argon , and the need to remove moisture because TiCl4 is susceptible to hydrolysis
4) High temp required

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19
Q

why can’t Titanium be extracted with carbon

A

Because titanium carbide ( TiC) would be formed rather than titanium

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20
Q

why can’t titanium be extracted by electrolysis

A

because it has to be very pure

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21
Q

what’s the reactions for magnesium extracting titanium

A

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

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22
Q

what’s the reactions for magnesium extracting titanium

A

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

23
Q

Why is TiO2 converted to TiCl4

A

It can be purified by fractional distillation

24
Q

what’s the trend in solubility of hydroxides down group 2

A

group 2 hydroxides become more soluble down the group
As group 2 hydroxides when not soluble appear as white precipitates

25
Q

is magnesium hydroxide soluble or insoluble in water

A

insoluble

26
Q

what’s the simplest ionic equation for formation of Mg(OH)2

A

Mg2+(aq) + 2OH- (aq) => Mg(OH)2(s)

27
Q

what’s Mg(OH2 used for

A

medicine to neutralise excess acid in stomach

28
Q

why is calcium carbonate preferred to be used than magnesium hydroxide

A

it will not produce CO2 gas

29
Q

is calcium hydroxide soluble or insoluble and the observation

A

Partially soluble
White precipitate

30
Q

what’s calcium hydroxide used for

A

in agriculture to neutralise acidic soils

31
Q

what’s the pH of magnesium hydroxide after reacting with water

A

9 - slightly alkaline

32
Q

what’s the pH of calcium hydroxide after reacting with water

A

11 - more alkaline than magnesium hydroxide as it’s more soluble so there will be be more OH- ions present in solution

33
Q

what’s an aqueous solution of calcium hydroxide called and whats it used for

A

lime water and can be used to test for carbon dioxide.
Limewater turns cloudy as white calcium carbonate is produced

34
Q

what’s the reaction of Ca(OH)2 with. CO2

A

Ca(OH)2 (aq) + CO2(g) => CaCO3(s) + H2O(l)

35
Q

is barium hydroxide insoluble or soluble

A

soluble

36
Q

what’s the ionic equation of Barium hydroxide

A

Ba(OH)2 (s) + aq => Ba2+ (aq) + 2OH-(aq)

37
Q

what’s the pH of barium hydroxide

A

Strongly alkaline - hydroxide ions present

38
Q

what’s the trend in solubility of sulfates down group 2

A

Become less soluble down the group
BaSO4 is the least soluble

39
Q

what’s the full and ionic equation for the formation of the precipitate of sulfates

A

full equation : SrCl2(aq) + Na2SO4(aq) => 2NaCl(aq) + SrSO4 (s)
half equation : Sr2+ (aq) + SO4 2-(aq) => SrSO4(s)

40
Q

what is BaSO4 used for

A

In medicine “barium meal” given to patients who need x rays

41
Q

why are barium compounds used in x rays even tho they’re toxic

A

safe to use because it’s low solubility ( BaSO4) means it’s not absorbed into the blood

42
Q

what’s the reaction between barium and h2so4

A

Ba + H2SO4 => BaSO4 + H2

43
Q

what’s a reagent used to test for sulphate ions

A

BaCl2 solution acidified with HCl

44
Q

what happens if acidified barium chloride is added to a solution that contain sulfates ions

A

a white ppt of barium sulfates forms

45
Q

what’s the ionic equation for ba and sulfates

A

Ba2+ (aq) + SO4 2- (aq) => BaSO4 (s)

46
Q

what’s the reaction between hcl and sodium carbonate

A

2HCl + Na2CO3 => 2NaCl + H2O + CO2

47
Q

how would you remove the salt

A

but filtration :
washed with distilled water to remove soluble impurities
washed and dried on filter paper

48
Q

how can insoluble salts be made

A

by mixing appropriate solutions of ions so that a ppt is formed
barium nitrate (aq) + sodium sulfates (aq) => barium sulfates(s) + sodium nitrate (aq)
These are called ppt reactions .

49
Q

EQ : describe the bonding in magnesium (2)

A
  • Attraction between lattice of Mg2+ ions
  • and delocalised electrons
50
Q

EQ : Explain , in terms of structure and bonding , why magnesium chloride has a high melting point (3)

A
  • Giant ionic lattice
  • Strong electrostatic forces of attraction
  • between Mg2+ and Cl- ions
51
Q

EQ : This question is about Group 2 elements and their compounds .
Explain why the melting point of magnesium is higher than the melting point of sodium (2)

A
  • mg atoms smaller than Na atoms / mg has a higher charge density than Na atoms
  • stronger attraction to sea of delocalised electrons
52
Q

EQ : state what is observed when dilute aq sodium hydroxide is added to separate solutions of magnesium chloride and barium chloride (2)

A

Observation with magnesium chloride :
White ppt
Observation with Barium chloride :
No change / colourless

53
Q

EQ : write an ionic equation , with state symbols to show the reaction of calcium with an excess of water (1)

A

Ca (s) + 2H2O (l) => Ca2+ (aq) + 2OH- (aq) + H2(g)

54
Q

EQ : state the role of water in the reaction with calcium (1)

A

oxidising agent

Chemistry Year 12 (25 decks)

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