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Chemistry Y12 > Group 2 > Flashcards

Group 2 Flashcards

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1
Q

Why does reactivity increase as we go down group 2?

A
  • down group 2 atomic radii increases
  • due to more filled energy levels
  • so outer electron is futher away from the nucleus
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2
Q

why does ionisation energy decrease as we go down group 2?

A
  • due to greater atomic radii
  • there is greater shielding
  • therefore the outer electron is attracted less strongly so less energy is required to remove an electron
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3
Q

why does the melting point generally decrease as we go down group 2?

A
  • due to increase in ionic radii
  • so decrease in charge/size ratio of the ion
  • so weaker metallic bonding
  • so less energy required to break the metallic bonds
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4
Q

reactions of group 2 with water

A
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5
Q

when group 2 elements react with water they form what ions?
They’re oxidised from..? to..?

A

M2+ ions , oxidised from 0 -> +2

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6
Q

describe solubility with group 2 elements and hydroxide ions?

A

solubility increases as you go down group 2 when reacted with OH- ions

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7
Q

group 2 metals + cold water –> makes?

A

metal hydroxide and hydrogen

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8
Q

describe what happens in the reaction between magnesium and cold water?

what happens when the rest of group 2 elements react with cold water?

A
  • Mg reacts very slowly to form magnesium hydroxide and hydrogen
    Mg (s) + H2O (l) —-> Mg(OH)2 (aq) + H2 (g)
  • they react more vigorously with cold water
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9
Q

group 2 metal + steam —> makes?

A

metal oxide and hydrogen

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10
Q

describe the reaction between magnesium and steam.
what observations can be made from this reaction?

A
  • reacts to form magnesium oxide and hydrogen
    Mg (s) + H2O (g) —> MgO (s) + H2 (g)
  • glows a bright orange, white solid MgO formed
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11
Q

describe the reaction between calcium and cold water?
why is a cloudy white mixture formed?

A
  • reacts to form calcium hydroxide and hydrogen
  • because ca(OH)2 is sparingly soluble in water
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12
Q

what happens when strontium and barium react with cold water.
why is a colourless solution formed?

A
  • react tor form their metal hydroxide which is a colourless solution and hydrogen
  • barium hydroxide and strontium hydroxide is soluble in water
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13
Q

the more soluble the hydroxide the…?
why is this?

A

the stronger the alkali, as there is a higher content of hydroxide (OH-) ions

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14
Q

uses of metal hydroxides

A
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15
Q

what is Mg(OH)2 used as?

A
  • an indigestion cure as its a weak alkali so neutralises excess stomach acid. safe to use as it’s not corrosive or toxic
  • also used as a laxative
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16
Q

what is Ca(OH) used for?

A
  • used by farmers in agriculture to add to soils to increase pH, neutralise acidic soils
  • = limewater used to test for co2
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17
Q

2 word equation to show magnesium hydroxide neutralising HCL

A
  • Mg(OH)2 (s) + 2HCL (l) —-> MgCl2 (aq) + 2H2O (l)
  • Mg(OH)2 + 2H+ (aq) —> Mg2+ (aq) + 2H2O (l)
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18
Q

group 2 sulphates

A
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19
Q

describe solubility of group 2 sulphates down the group?

A

solubility decreases so Mg is the most soluble and Barium is insoluble in water (because it’s a solid)

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20
Q

most barium compounds are..? but..?

A

toxic but BaSO4 is not toxic as its’s insoluble so passes straight out of the body

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21
Q

how can we test for sulphate ions?

A

using acidified barium chloride (BaCl2) solution

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22
Q

if sulphate ions are present what will the solution form..?
why does it form a white precipitate?

A

will form a white precipitate of barium sulphate (BaSO4)
- because BaSO4 is insoluble

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23
Q

when do we need to make sure we add ACIDIFIED BaCl2?

A

needs to be acidified in order to remove carbonate ions from the solution. as CO3(2-) carbonate ions would interfere with the test and so form a false positive result of a white precipitate of BaCO3

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24
Q

draw the equation to show how carbonate ions interfere with the test and how carbonate ions are removed

A
  • Ba 2+ (aq) + CO3(2-) (aq) —-> BaCO3 (s)
  • CO3(2-) (aq) + 2H+ (aq) —–> CO2 + h20
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25
Q

equation to show the test for sulphate ions

A

Ba2+ (aq) + SO4(2-) (aq) —–> BaSO4 (s)

26
Q

what can we use to acidify Barium chloride solution?

A

dilute hydrochloric acid or nitric acid

27
Q

why can we not use dilute sulphuric acid?

A

as sulphuric acid contains sulphate ions which will interfere with the test and form a false positIve result of a white precipitate of BaSO4

28
Q

what are the uses of barium sulphate in medicine?

A
  • barium meal to block x-rays. As barium sulphate is insoluble in water and bodily fluids we can use it to investigate problems in the digestive and bowel systems. the barium sulphate coats the tissue, making them show up on the x-rays
29
Q

why can we not use other barium compounds?

A

because other barium compounds are toxic as aqueous Ba2+ ions are toxic

30
Q

group 2 metal + sulphuric acid –> makes?

A

metal sulphate + hydrogen

31
Q

describe what would be seen when magnesium reacts with sulphuric acid?

A
  • Mg (s) + H2SO4 (l) —–> MgSO4 (aq) + H2 (l)
  • reacts vigorously fizzing, bubbles of h2 produced. colourless solution is formed as magnesium sulphate is highly soluble in water
32
Q

describe what happens when calcium reacts with sulphuric acid?

A
  • Ca (s) + H2SO4 (l) —-> CaSO4 (aq) + H2 (l)
  • reacts violently, exothermic reaction, bubbles formed. cloudy white mixture formed as calcium sulphate is sparing soluble
33
Q

extraction of titanium

A
34
Q

why can’t titanium be extracted by the reduction of minerals by carbon?
what does titanium carbide do?

A

because titanium carbide forms
titanium carbide makes the metal brittle and useless

35
Q

why can’t titanium be reduced with more reactive metals?

A
  • reduction of titanium with more reactive metals produces impurity problems and it is difficult and expensive to eliminate the reducing agent from the titanium
36
Q

titanium is obtained from it’s oxide in two steps?

A

step 1 - conversion of titanium oxide into titanium (IV) chloride
step 2 - reduction of titanium (IV) chloride by a reactive metal

37
Q

explain how titanium oxide is converted into titanium (IV) chloride?

A
  • by reacting with chlorine and coke at 900C
  • TiO2 (aq) + 2C (s) + 2Cl2 (g) —> TiCl4 (l) + 2CO (g)
38
Q

why can titanium chloride be purified by fractional distillation from any other chlorides

A

because titanium chloride is a liquid a room temperature

39
Q

after the 1st step how can we reduce titanium chloride by a reactive metal?

A
  • (in UK) titanium chloride is reduced by sodium at high temperature via the following exothermic displacement reaction:
  • TiCl4 (l) + 4Na (l) —-> Ti (s) + 4NaCl (s)
40
Q

what temperature is the sodium initially set to and why does it end up being raised?

A
  • the temperature of the sodium is initially set to 550C but the exothermic reaction raises it to nearly 1000C during the reaction
41
Q

what reaction conditions does this have to be set in and why?

A
  • the reaction has to be carried out in an inert atmosphere of argon to prevent any contamination of the metal with oxygen or nitrogen
42
Q

what is the by-product formed? And how is it removed to get titanium?

A

sodium chloride is removed by washing with dilute hydrochloric acid leaving granules of titanium behind

43
Q

what is used as the reducing agent in this reaction? show this in an equation?

A
  • magnesium is used as the reducing agent (high temperature and inert argon atmosphere)
  • TiCl4 () + 2Mg (l) —-> Ti (s) + 2MgCl2 (s)
44
Q

how is the magnesium chloride by-product removed from titanium?

A

by vaccum distillation at high temperatures

45
Q

the reactions of ethanoic acid?

A
46
Q

what type of acids are carboxylic acids?

A

weak acids

47
Q

(ethanoic) acid + metal —-> makes?

A

salt + hydrogen

48
Q

(ethanoic) Acid + metal hydrogencarbonate —–> makes?

A

salt + water + carbon dioxide

49
Q

(ethanoic) Acid + metal carbonate —-> makes?

A

salt + water + carbon dioxide

50
Q

(ethanoic) acid + alkali —-> makes?

A

salt + water

51
Q

what can ethanoic acid not be oxidised by?

A

Acidified potassium dichromate (VI)

52
Q

Carboxylic acid + Alcohol ⇌ makes?

A

ester and water

53
Q

draw this reaction above

A
54
Q

what is the standard test for carboxylic acids?

A

sodium hydrogen carbonate

55
Q

what is the pH of ethanol?

A

neutral - green 7

56
Q

what is the pH of ethanoic acid?

A

acidic - redish - 0

57
Q

reaction of magnesium and ethanol vs ethanoic acid?

A

ethanol - no reaction
ethanoic acid - bubbles, fizzes, hydrogen produced

58
Q

explain what happens when ethanol and ethanoic acid react with sodium hydrogencarbonate?

A

ethanol - no reaction, powder sinks
ethanoic acid - reacts violently bubbles, rises carbon dioxide produced

59
Q

what happens when ethanol and ethanoic acid react with acidified dichromate?

A

ethanol - orange to green
ethanoic acid - ethanal made , apple smell produced

60
Q

DONE!!!

A

Chemistry Y12 (11 decks)

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