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Chemistry A level (Edexcel) > TOPIC 4 - Inorganic chemistry and the Periodic Table > Flashcards

TOPIC 4 - Inorganic chemistry and the Periodic Table Flashcards

1
Q

What is the general equation for the reaction between group 2 metals and water?

A

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

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2
Q

What is the equation for the reaction of magensium with steam?

A

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

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3
Q

Why does reactivity increase down group 2?

A

Atom is larger so electron is further away from the nucleus and there is more shielding.

Therefore the electrostatic forces of attraction between the outer electrons and the nucleus decreases.

Therefore it is easier to remove the outer electrons and reactivity increases.

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4
Q

What is the general equation for group 2 metals with oxygen?

A

2X + O2 > 2XO

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5
Q

What appearance do group 2 oxides have?

A

White solids.

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6
Q

What is the general reaction for group 2 metals with chlorine?

A

X + Cl2 > XCl2

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7
Q

Why do group 2 metal oxides create an alkaline solutions?

A

XO + H2O > X(OH)2

X(OH)2 > X2++ 2OH-

The OH- ion creates the alkaline solution.

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8
Q

Which group 2 oxides don’t create alkaline solutions?

A
  • Magnesium oxide - reacts very slowly with water and magnesium hydroxide is barely soluble.
  • Beryllium oxide - doesn’t react with water and the hydroxide is insoluble.
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9
Q

Why do group 2 metal oxide solutions get more alkaline as we go down the group?

A

They are more reactive with water.

The hydroxide salt is more soluble so it dissociates more.

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10
Q

How does solubility of group 2 hydroxides change as we go down the group?

A

Increases

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11
Q

How does solubility of group 2 sulfates change as we go down the group?

A

Decreases.

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12
Q

What is the general equation for the thermal decomposition of group 2 carbonates?

A
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13
Q

What is the general formula for the thermal decomposition of group 2 nitrates?

A
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14
Q

Why does thermal stability of carbonates/nitrates increase as we go down group 1 or 2?

A

Bigger metal cation so lower charge density.

Therefore the electron cloud in the anion (sulfate/carbonate) is less distorted.

The less distortion, the more thermal stability.

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15
Q

Do group 1 carbonates decompose under bunsen flame?

A

No. Only Lithium carbonate.

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16
Q

What is the general equation for the thermal decomposition of group 1 nitrates?

A
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17
Q

What is the equation for the thermal decomposition of of lithium nitrate?

A

4LiNO3 > 2Li2O + 4NO2 + O2

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18
Q

Why are group 1 carbonates/nitrates more stable than in group 2?

A

Group 1 ions have a lower charge than group 2 (+1 vs +2) so they have a lower charge density.

Therefore the electron cloud in the anion is distorted less.

The less distortion, the more stability.

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19
Q

How can you test for thermal stability?

A

Measuring how much and how fast gas is produced from thermal decomposition.

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20
Q

Why do flame tests give different colours?

A
  1. Electrons absorb energy from the flame and become excited so they move to a higher energy level.
  2. When they drop back to their ground level, and emit a specific amount of energy through electromagnetic radiation.
  3. This electromagnetic has a specific wavelength and so the part of the spectrum that falls into visible light, has different colours.
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21
Q

What is the procedure for a flame test?

A
  1. Dip nichrome wire in HCl.
  2. Dip nichrome wire into sample.
  3. Place the loop into a blue bunsen flame and observe the colour.
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22
Q

What is the flame test colour of Li+?

A

Crimson red

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23
Q

What is the flame test colour of Na+?

A

Yellow/orange

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24
Q

What is the flame test colour of K+​?

A

Lilac

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25
Q

What is the flame test colour of Rb+?

A

Red

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26
Q

What is the flame test colour of Cs+​?

A

Blue

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27
Q

What is the flame test colour of Ca2+​?

A

Dark red

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28
Q

What is the flame test colour of Sr2+​?

A

Crimson red

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29
Q

What is the flame test colour of Ba2+?

A

Green

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30
Q

What is the flame test colour of Be2+?

A

No colour (radiation emitted doesn’t fall in the visible spectrum).

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31
Q

What is the flame test colour of Mg2+?

A

No colour. Radiation emitted doesn’t fall into the visible spectrum.

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32
Q

What is the appearance of Fluorine?

A

Pale yellow gas

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33
Q

What is the appearance of Chlorine?

A

Pale green gas

34
Q

What is the appearance of Bromine?

A

Brown-orange liquid

35
Q

What is the appearance of Iodine?

A

Grey solid

36
Q

Why do mpt/bpt increase as we go down group 7?

A

Bigger atoms therefore diatomic molecules have more electrons and so stronger london forces between molecules and therefore more energy needed to overcome them.

37
Q

Why does electronegativity decrease down group 7?

A

Atoms get larger so larger distance between bonding electrons and nucleus.

More shielding

This offsets the increase in nuclear charge.

Therefore the attraction between nucleus and the bonding electrons is less and therefore electronegativity decreases.

38
Q

What would be seen when Cl2 is added to a KBr solution with a layer of hexane?

Give ionic eqt.

A

Cl2+ 2Br- > 2Cl- + Br2

Aqueous layer turns yellow.

Organic layer turns orange.

39
Q

What would be seen when Cl2 is added to a KI solution with a layer of hexane?

Give ionic eqt.

A

Cl2 + 2I- > 2Cl- + I2

Aqueous turns brown

Organic turns purple

40
Q

What would be seen when Br2 is added to a KCl solution with a layer of hexane?

Give ionic eqt.

A

No reaction.

aqueous turns yellow

organic turns orange

41
Q

What would be seen when Br2 is added to a KI solution with a layer of hexane?

Give ionic eqt.

A

Br2 + 2I- > 2Br- + I2

Aqueous turns brown

Organic turns purple

42
Q

What would be seen when I2 is added to a KCl solution with a layer of hexane?

Give ionic eqt.

A

No reaction.

Aqueous turns brown.

Organic turns purple

43
Q

What would be seen when I2 is added to a KBr solution with a layer of hexane?

Give ionic eqt.

A

No reaction.

Aqueous turns brown.

Organic turns purple.

44
Q

What is the colour of Br2 in an aqueous solution?

45
Q

What is the colour of Br2 in an organic solution?

46
Q

What is the colour of I2 in an aqueous solution?

47
Q

What is the colour of I2 in an organic solution?

48
Q

What is the formula of the chlorate(I) ion?

Give oxidation state of Cl.

A

ClO-

Cl is +1.

49
Q

What is the formula of the Bromate(I) ion?

Give oxidation state of Br.

A

BrO-

Br is +1

50
Q

What is the formula of the Bromate(III) ion?

Give oxidation state of Br.

A

BrO2-

Br is +3.

51
Q

What is the formula of the iodate(V) ion?

Give oxidation state of Iodine.

A

IO3-

I is +5

52
Q

What is the formula of the iodate(VII) ion?

Give oxidation state of Iodine.

A

IO4-

I is +7.

53
Q

What is the general equation for the halogens with cold alkali?

54
Q

What is the general equation for the halogens with hot alkalis?

55
Q

What is the equation for the reaction between chlorine and sodium hydroxide to give bleach?

56
Q

What are the uses of sodium chlorate(I) (bleach)?

A

Treating water

Bleaching paper and fabrics

Cleaning agents

57
Q

What is the reaction of water with chlorine?

58
Q

What are the uses of adding chlorine to water?

A

Drinking water and swimming pools (ClO- ions kill bacteria)

59
Q

What is the equation for the dissociation of chloric(I) acid in water?

60
Q

Why does the reducing power of the halide ions increase as you go down the group?

A

Larger distance between electrons and nucleus

More shielding

Therefore there’s a weaker force of attraction and so it is easier to loose the electron.

61
Q

Which sulfur-containing products can Cl- ions form when reacted with sulfuric acid?

62
Q

Which sulfur-containing products can Br- ions form when reacted with sulfuric acid?

Give oxidation number of Sulfur.

A

NaHSO4(+6), SO2(+4)

63
Q

Which sulfur-containing products can I- ions form when reacted with sulfuric acid?

Give oxidation number of sulfur

A

NaHSO4(+6), SO2(+4), S(0), H2S(-2)

64
Q

What is the general equation for the reaction of halide ions with H2SO4 to give NaHSO4?

What observation can be made?

A

White misty fumes

65
Q

What is the equation for the reduction of sulfuric acid to SO2 by Br- ions?

What observation can be made?

A

Orange vapour (Br2)

66
Q

What is the equation for the reduction of sulfuric acid to dulfur by I-?

What observations can be made?

A

Yellow solid (S) produced.

67
Q

What is the equation for the reduction of sulfuric acid to hydrogen sulfide by I-?

What observations can be made?

A

Rotten egg smell (H2S)

68
Q

What is the name of the acid produced when HCl is dissolved in water?

A

Hydrochloric acid

69
Q

What is the name of the acid produced when HBr is dissolved in water?

A

Hydrobromic acid

70
Q

What is the name of the acid produced when HI is dissolved in water?

A

Hydroiodic acid

71
Q

What is the general formula for the reaction between hydrogen halides and ammonia?

A

NH3 + HX > NH4X

72
Q

What is the positive result for chloride ions in the test with silver nitrate?

Give ionic equation and solubility in ammonia.

A

White ppt

Ag+ (aq) + Cl- (aq) > AgCl (s)

Dissolves in dilute and excess ammonia.

73
Q

What is the positive result for bromide ions in the test with silver nitrate?

Give ionic equation and solubility in ammonia.

A

Cream ppt.

Ag+ + Br- > AgBr

Dissolves only in concentrated ammonia.

74
Q

What is the positive result for iodide ions in the test with silver nitrate?

Give ionic equation and solubility in ammonia.

A

Yellow ppt.

Ag+ + I- > AgI

Insoluble in Ammonia.

75
Q

Why is nitric acid added before the silver nitrate test for halide ions?

A

To react with other anions and ensure none of them react with Ag+.

The acid shouldn’t contain halide ions present.

76
Q

Why isn’t there a silver nitrate test for fluoride ions?

A

AgF is soluble, so doesn’t form a precipitate.

77
Q

What is the test for carbonates?

A

Add acid and test for CO2 (turns limewater cloudy)

78
Q

What is the test for sulfates?

A

Add HCl to remove any carbonates that could react.

Add BaCl

Barium sulfate is formed - white ppt is formed.

79
Q

What is the test for ammonium salts?

A

Add NaOH + gently heat.

Test for ammonia gas - turns damp red litmus paper blue.

80
Q

What can be used as a test for hydroxides?

A

Turns red litmus paper blue (although this is for every alkali, so further tests should be done).

Chemistry A level (Edexcel) (19 decks)

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