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CHEMISTRY 🌡️ > INORGANIC 🌡️ > Flashcards

INORGANIC 🌡️ Flashcards

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1
Q

Reaction of beryllium with water

A

No reaction with water or steam

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2
Q

Reaction of magnesium with water

A

WATER - Mg(s) + 2H2O(l) -> Mg(OH)2(s) + H2(g) very slow
STEAM - Mg(s) + H2O(g) -> MgO(aq) +H2(g)

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3
Q

Reaction of calcium with water

A

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

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4
Q

Reaction of strontium with water

A

Sr(s) + 2H2O(l) -> Sr(OH)2(aq) + H2(g) fairly quick, exothermic, stored in oil to prevent reaction

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5
Q

Reaction of barium with water

A

Ba(s) + 2H2O(l) -> Ba(OH)2(aq) + H2(g) rapid, exothermic, stored in oil to prevent reaction

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6
Q

Solubility of Mg(OH)2 in water

A

Insoluble / sparingly soluble

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7
Q

Solubility of Ca(OH)2 in water

A

Slightly soluble, forming cloudy alkaline solution

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8
Q

Solubility of Sr(OH)2 in water

A

Soluble, forms cloudy alkaline solution

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9
Q

Solubility of Ba(OH)2 in water

A

Soluble, forms alkaline solution

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10
Q

Solubility of MgSO4 in water

A

Soluble

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11
Q

Solubility of CaSO4 in water

A

Slightly soluble

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12
Q

Solubility of SrSO4 in water

A

Insoluble

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13
Q

Solubility of BaSO4 in water

A

Insoluble

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14
Q

Test for sulfate ions

A

Add acidified BaCl2 to solution (acidify with HCl to get rid of sulfites or carbonates which also produce white ppt)
If SO4 is present, white ppt forms
eg BaCl2(aq) + FeSO4(aq) -> BaSO4(s) + FeCl2(aq)

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15
Q

Use of magnesium

A

Extraction of titanium from its ore
TiO2 converted to TiCl4 by heating with carbon in stream of chlorine gas
TiCl4 purified by fractional distillation
Then reduced by magnesium in furnace at ~1000°c
TiCl4(g) + 2Mg(l) -> Ti(s) + 2MgCl2(l)

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16
Q

Use of calcium

A

Remove sulfur dioxide
Burning fossil fuels produces sulfur dioxide which pollutes atmosphere
Acidic SO2 can be removed from flue gases by reacting with alkali - wet scrubbing
Powdered CaO and CaCO3 can both be used
Slurry is made by mixing CaO or CaCO3 with water
Slurry sprayed onto flue gases
CaO(s) + 2H2O(l) + SO2(g) -> CaSO3(s) + 2H2O(l)
CaCO3(s) + 2H2O(l) +SO2(g) -> CaSO3(s) + 2H2O(l) + CO2(g)

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17
Q

Colour of fluorine gas

A

Pale yellow

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18
Q

Colour of chlorine gas

A

Green

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19
Q

Colour of liquid bromine

A

Red-brown

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20
Q

Colour of solid iodine

A

Grey

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21
Q

How to make bleach

A

Mix chlorine gas with cold dilute aqueous NaOH
Forming sodium chlorate (I) solution
2NaOH(aq) + Cl2(g) -> NaClO(aq) + NaCl(aq) + H2O(l)

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22
Q

Chlorine in water treatment

A

Mix chlorine with water, disproportionation:
Cl2(g) + H2O(l) <=> 2H+(aq) + Cl-(aq) + ClO-(aq)
Mix chlorine and water in sunlight:
2Cl2(g) + 2H2O(l) <=> 4H+(aq) + 4Cl-(aq) + O2(g)

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23
Q

Reaction of NaCl with H2SO4

A

NaCl(s) + H2SO4(l) -> NaHSO4(s) + HCl(g)
Steamy fumes - HCl
Not redox

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24
Q

Reaction of NaBr with H2SO4

A

NaBr(s) + H2SO4(l) -> NaHSO4(s) + HBr(g)
Steamy fumes - HBr
Not redox

2HBr(aq) + H2SO4(l) -> Br2(g) + SO2(g) + 2H2O(l)
Brown fumes - Br2
Colourless choking gas - SO2
Redox (HBr is strong reducing agent)

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25
Q

Reaction of NaI with H2SO4

A

NaI(s) + H2SO4(l) -> NaHSO4(s) + HI(g)
Steamy fumes - HI
Not redox

2HI(g) + H2SO4(l) -> I2(s) + SO2(g) + 2H2O(l)
Purple fumes - I2(g) or black solid - I2(s)
Colourless choking gas - SO2

6HI(g) + SO2(g) -> H2S(g) + 3I2(s) +2H2O(l)
Gas smells of bad eggs - H2S
Redox (HI is very strong reducing agent)

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

8HI(g) + H2SO4(l) -> 4I2(s) + H2S(g) + 4H2O(l)
Toxic gas which smells of bad eggs - H2S
Redox

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26
Q

Flame test procedure

A

Dip loop of nichrome wire in conc HCl
Dip wire loop into unknown compound
Hold loop in clear blue part of Bunsen burner flame
Observe colour change

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27
Q

Flame test result for calcium ion

A

Brick red flame

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28
Q

Flame test result for strontium ion

A

Red flame

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29
Q

Flame test result for barium ion

A

Pale green flame

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30
Q

Test for group 2 with NaOH procedure

A

Add dilute NaOH dropwise
Observe ppt formed
Add NaOH until in excess
Observe changes

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31
Q

Result for magnesium ions with NaOH

A

DROPS OF OH - slight white ppt
EXCESS OH - white ppt

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32
Q

Result for calcium ions with NaOH

A

DROPS OF OH - slight white ppt
EXCESS OH - slight white ppt

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33
Q

Result for strontium ions with NaOH

A

DROPS OF OH - slight white ppt
EXCESS OH - slight white ppt

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34
Q

Result for barium ions with NaOH

A

DROPS OF OH - no change
EXCESS OH - no change

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35
Q

Reaction of sodium with oxygen

A

4Na(s) + O2(g) -> 2Na2O(s)
Vigorous
Burns with yellow-orange flame to give white power

36
Q

Reaction of magnesium with oxygen

A

2Mg(s) + O2(g) -> MgO(s)
Vigorous
Burns with white flame to produce white powder

37
Q

Reaction of aluminium with oxygen

A

4Al(s) + 3O2(g) -> 2Al2O3(s)
Slow, faster if powdered
Burns with white flame to produce white powder

38
Q

Reaction of silicon with oxygen

A

Si(s) + O2(g) -> SiO2(g)
Slow
Burns with white flame to produce white powder

39
Q

Reaction of phosphorus with oxygen

A

P4(s) + 5O2(g) -> P4O10(s)
Spontaneously combusts
Burns with very bright white flame to produce white powder

40
Q

Reaction of sulfur with oxygen

A

S(s) + O2(g) -> SO2(g)
Burns steadily
Burns with blue flame and gives off choking gas

41
Q

Reaction of sodium with water

A

2Na(s) + 2H2O(l) -> 2NaOH(aq) + H2(g)
Floats and moves about on water
Fizzes
May catch fire with yellow orange flame

42
Q

Reaction of magnesium with water

A

Mg(s) + H2O(l) -> MgO(aq) + H2(g)
Steam:
Burns with white flame giving white powder
Water:
Very slow

43
Q

Reaction of chlorine with water

A

Cl2(g) + H2O(l) <=> HCl(aq) + HClO(aq)
Dissolves giving very pale green solution

44
Q

Reaction of sodium oxide with water

A

Na2O(aq) + H2O(l) -> 2NaOH(aq)
Na+ and O2- dissolve in water
Then O2- react with water:
O2- + H2O -> 2OH-
pH 12-14

45
Q

Reaction of magnesium oxide with water

A

MgO(aq) + H2O(l) -> Mg(OH)2(aq)
Slightly soluble
Some Mg2+ and O2- dissolve in water
Then O2- react with water
O2- + H2O -> 2OH-
pH 9-10

46
Q

Reaction of aluminium oxide with water

A

No reaction because Al2O3 cannot dissolve
Due to very high lattice enthalpy

47
Q

Reaction of silicon dioxide with water

A

Insoluble
Due to lattice of atoms linked by strong covalent bonds which would have to be broken

48
Q

Reaction of phosphorus (V) oxide with water

A

P4O10(s) + 6H2O(l) -> 4H3PO4(aq)
Reacts violently
Forms phosphoric (V) acid (strong acid)
H2O molecules attack delta+ P atoms, leading to release of H+ from water
pH 0

49
Q

Reaction of sulfur dioxide with water

A

SO2(g) + H2O(l) -> H2SO3(aq)
Forms sulfurous acid / sulfuric(IV) acid
H2O attacks delta+ S atom, leading to release of H+ from water molecules
pH 3

50
Q

Reaction of sulfur trioxide with water

A

SO3(l) + H2O(l) -> H2SO4(aq)
Reacts violently
Forms sulfuric (VI) acid
H2O attacks delta+ S atom, leading to release of H+ from water
pH 0

51
Q

Which period 3 oxides are basic

A

Na2O
MgO
Al2O3

52
Q

Which period 3 oxides are acidic

A

Al2O3
SiO2
P4O10
SO2
SO3

53
Q

Reaction of sodium oxide with acid

A

Na2O(s) + 2HCl(aq) -> 2NaCl(aq) + H2O(l)

54
Q

Reaction of magnesium oxide with acid

A

MgO(s) + 2HCl(aq) -> MgCl2(aq) + H2O(l)

55
Q

Reaction of aluminium oxide with acid

A

Al2O3(s) + 6HCl(aq) -> 2AlCl3(aq) + 3H2O(l)

56
Q

Reaction of aluminium oxide with base

A

Al2O3(s) + 2NaOH(aq) + 3H2O(l) -> 2NaAl(OH)4(aq)

57
Q

Reaction of silicon dioxide with base

A

SiO2(s) + 2NaOH(aq) -> Na2SiO3(aq) + H2O(l)

58
Q

Reaction of phosphorus (V) oxide with base

A

P4O10(s) + 12NaOH(aq) -> 4Na3PO4(aq) + 6H2O(l)

59
Q

Reaction of sulfur dioxide with base

A

SO2(g) + 2NaOH(aq) -> Na2SO3(aq)+ H2O(l)

60
Q

Reaction of sulfur trioxide with base

A

SO3(g) + 2NaOH(aq) -> Na2SO4(aq) + H2O(l)

61
Q

Vanadium (V) to vanadium (IV)

A

2(VO2)+(aq) + Zn(s) + 4H+(aq) -> 2(VO)2+(aq) + Zn2+(aq) + 2H2O(l)

62
Q

Vanadium (IV) to vanadium (III)

A

2(VO)2+(aq) + Zn(s) + 4H+(aq) -> 2V3+(aq) + Zn2+(aq) + 2H2O(l)

63
Q

Vanadium (III) to vanadium (II)

A

2V3+(aq) + Zn(s) -> 2V2+(aq) + Zn2+(aq)

64
Q

Colour of vanadium (V) ion / (VO2)+

A

Yellow

65
Q

Colour of vanadium (IV) ion / (VO)2+

A

Blue

66
Q

Colour of vanadium (III) ion / V3+

A

Green

67
Q

Colour of vanadium (II) ion / V2+

A

Violet (purple?)

68
Q

Fe2+ catalyst

A

Catalyses reaction:
(S2O8)2-(aq) + 2I-(aq) -> I2(aq) + 2(SO4)2-(aq)
Slow as both are negatively charged (repulsion)
(S2O8)2-(aq) + 2Fe2+(aq) -> 2Fe3+(aq) + 2(SO4)2-(aq)
2Fe3+(aq) + 2I-(aq) -> I2(aq) + 2Fe2+(aq)
Homogeneous catalyst

69
Q

Autocatalysis example

A

2(MnO4)-(aq) + 16H+(aq) + 5(C2O4)2-(aq) -> 2Mn2+(aq) +8H2O(l) +10CO2(g)
Both negatively charged
So repel - initial reaction is slow
Product of reaction, Mn2+, can act as catalyst
(MnO4)-(aq) + 4Mn2+(aq) +8H+(aq) -> 5Mn3+(aq) + 4H2O(l)
2Mn3+(aq) + (C2O4)-(aq) -> 2Mn2+(aq) + 2CO2(g)
Reforming Mn2+
Homogeneous catalyst

70
Q

Catalyst in contact process

A

V2O5(s) + SO2(g) -> V2O4(s) +SO3(g)
Vanadium oxidises SO2 to SO3 and reduces itself
V2O4(s) + 0.5O2(g) -> V2O5(s)
Vanadium oxidised by oxygen to its original state
Overall:
SO2(g) + 0.5O2(g) -> SO3(g)
With heterogeneous V2O5 catalyst

71
Q

Colour of aqueous iron (II) ion

A

Green solution
[Fe(H2O)6]2+

72
Q

Colour of aqueous copper (II) ion

A

Blue solution
[Cu(H2O)6]2+

73
Q

Colour of aqueous iron (III) ion

A

Purple solution
[Fe(H2O)6]3+
May look yellow-brown due to some [Fe(H2O)5(OH)]2+

74
Q

Colour of aqueous aluminium (III) ion

A

Colourless solution
[Al(H2O)6]3+

75
Q

Action of limited and excess NaOH on aqueous iron (II) ion

A

LIMITED:
Green ppt, goes brown on standing in air
Fe(H2O)4(OH)2
EXCESS:
No further change

76
Q

Action of limited and excess NaOH on aqueous copper (II) ion

A

LIMITED:
Blue ppt
Cu(H2O)6(OH)2
EXCESS:
No further change

77
Q

Action of limited and excess NaOH on aqueous iron (III) ion

A

LIMITED:
Brown ppt, may look orange-brown
Fe(H2O)3(OH)3
EXCESS:
No further change

78
Q

Action of limited and excess NaOH on aqueous aluminium (III) ion

A

LIMITED:
White ppt
Al(H2O)3(OH)3
EXCESS:
Colourless solution
[Al(OH)4]-

79
Q

Action of limited and excess ammonia on aqueous iron (II) ion

A

LIMITED:
Green ppt, goes brown on standing in air
Fe(H2O)4(OH)2
EXCESS:
No further change

80
Q

Action of limited and excess ammonia on aqueous copper (II) ion

A

LIMITED:
Blue ppt
Cu(H2O)4(OH)2
EXCESS:
Deep blue solution
[Cu(H2O)2(NH3)4]2+

81
Q

Action of limited and excess ammonia on aqueous iron (III) ion

A

LIMITED:
Brown ppt, may look orange-brown
Fe(H2O)3(OH)3
EXCESS:
No further change

82
Q

Action of limited and excess ammonia on aqueous aluminium (III) ion

A

LIMITED:
White ppt
Al(H2O)3(OH)3
EXCESS:
No further change

83
Q

Action of Na2CO3 on aqueous iron (II) ion

A

Green ppt
FeCO3

84
Q

Action of Na2CO3 on aqueous copper (II) ion

A

Blue-green ppt
CuCO3

85
Q

Action of Na2CO3 on aqueous iron (III) ion

A

Brown ppt, may look orange-brown
CO2 gas evolved
Fe(H2O)3(OH)3

86
Q

Action of Na2CO3 on aqueous aluminium (III) ion

A

White ppt
CO2 gas evolved
Al(H2O)3(OH)3

CHEMISTRY 🌡️ (4 decks)

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