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P block elements Flashcards

1
Q

2Al(s) + 6HCl(aq)

A

2AlCl3(aq) + 3H2(g)

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2
Q

2Al(s) + 2OH ̅(aq) + 6H2O(l)

A

2[Al(OH)4] ̅(aq) + 3H2(g)

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3
Q

[Al(OH2)6]3+(aq) + H2O(l)

A

[Al(OH2)5(OH)]2+(aq) + H3O+(aq)

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4
Q

[Al(OH2)5(OH)]2+(aq) + H2O(l)

A

[Al(OH2)4(OH)2]+(aq) + H3O+(aq)

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5
Q

Al3+(aq) + 3OH ̅(aq)

A

Al(OH)3(s) (white gelatinous ppt)

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6
Q

Al(OH)3(s) + OH ̅(aq)

A

[Al(OH)4] ̅ (aq) or AlO2 ̅(aq) + 2H2O(l)

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7
Q

allotropic forms of carbon

A

Graphite, diamond and fullerenes

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8
Q

Carbon monoxide is mostly used as

A

a reducing agent in the production of iron. Also, CO

plays an important role in many catalytic reactions as a ligand due to the lone pair of electrons on the C atom

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9
Q

CO2(aq) + H2O(l)

A

H2CO3(aq)

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10
Q

H2CO3(aq) + H2O(l)

A

HCO3-(aq) + H3O+(aq)

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11
Q

HCO3-(aq) + H2O(l)

A

CO3 2-(aq) + H3O+(aq)

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12
Q

CO2(g) + 2NaOH(aq)

A

Na2CO3(aq) + H2O(l)

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13
Q

Na2CO3(aq) + excess CO2(g) + H2O(l)

A

2NaHCO3(aq)

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14
Q

N2(g) + 2O2(g)

A

2NO2(g)

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15
Q

3HNO2(aq)

A

HNO3(aq) + 2NO(g) + H2O(l)

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16
Q

2NO(g) + O2(g)

A

2NO2(g)

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17
Q

4HNO3(aq)

A

4NO2(g) + O2(g) + 2H2O(l)

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18
Q

Mg(s) + dil. 2HNO3(aq)

A

Mg(NO3)2(aq) + H2(g)

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19
Q

Mg(s) + conc. 4HNO3(l)

A

Mg(NO3)2(aq) + 2NO2(g) + 2H2O(l)

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20
Q

3Cu(s) + dil. 8HNO3(aq)

A

3Cu(NO3)2(aq) + 2NO(g) + 4H2O(l)

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21
Q

Cu(s) + conc. 4HNO3(l)

A

Cu(NO3)2(aq) + 2NO2(g) + 2H2O(l)

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22
Q

C(s) + conc. 4HNO3(l)

A

CO2(g) + 4NO2(g) + 2H2O(l)

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23
Q

S(s) + conc. 6HNO3(l)

A

H2SO4(l) + 6NO2(g) + 2H2O(l)

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24
Q

NH3(g) + H2O(l)

A

NH4OH(aq)

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25
Q

NH4OH(aq)

A

NH4+(aq) + OH ̅(aq)

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26
Q

2NH4OH(aq) + dil. H2SO4(aq)

A

(NH4)2SO4(aq) + 2H2O(l)

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27
Q

NH4+(aq) + H2O(l)

A

NH3(aq) + H3O+(l)

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28
Q

NH4Cl(aq) + NaOH(aq)

A

NaCl(aq) + NH3 (g) + H2O(l)

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29
Q

excess ammonia, 2NH3(g) + 3Cl2(g)

A

N2(g) + 6HCl(g)

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30
Q

Excess 3Cl2(g) + NH3(g)

A

3HCl(g) + NCl3(l)

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31
Q

NCl3(l) + 3H2O(l)

A

NH3(g) + 3HOCl(aq)

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32
Q

NH3(g) + HCl(g)

A

NH4Cl(s)

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33
Q

3CuO(s) + 2NH3(g)

A

N2(g) + 3Cu(s) + 3H2O(g)

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34
Q

2Na(s) + 2NH3(l)

A

2NaNH2(l) + H2(g)

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35
Q

3Mg(s) + 2NH3(l)

A

Mg3N2(l) + 3H2(g)

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36
Q

(NH4)2CO3(s)

A

2NH3(g) + CO2(g) + H2O(g)

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37
Q

NH4Cl(s)

A

NH3(g) + HCl(g)

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38
Q

(NH4)2SO4(s)

A

NH3(g) + H2SO4(g)*

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39
Q

NH4NO2(s)

A

N2(g) + 2H2O(g)

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40
Q

NH4NO3(s)

A

N2O(g) + 2H2O(g)

41
Q

(NH4)2Cr2O7(s)

A

N2(g) + Cr2O3(s) + 4H2O(g)

42
Q

NH4+(aq) + OH¯(aq)

A

NH3(g) + H2O(l)

43
Q

NH3(g) + HCl(g)

A

NH4Cl(s) white fumes

44
Q

2NO3ˉ (aq) + 4H2SO4(l) + 6Fe2+(aq)

A

6Fe3+(aq) + 2NO(g) + 4SO42ˉ (aq) + 4 H2O(l)

45
Q

Fe2+(aq)+ NO(g)

A

[Fe(NO)]2+(aq) brown colour

46
Q

3NO3ˉ (aq) + 8Al(s) + 5OHˉ(aq) + 18H2O(l)

A

3NH3(g) + 8[Al(OH)4]ˉ(aq)

47
Q

2H2O(l)

A

H3O+(aq) + OH-(aq)

48
Q

H2O(l) + HCl(aq)

A

H3O+(aq) + Cl-(aq)

49
Q

H2O(l) + NH3(aq)

A

NH4+(aq) + OH-(aq)

50
Q

2H2O2(aq)

A

O2(g) + 2H2O(l)

51
Q

2KClO3(s)

A

2KCl(s) + 3O2(g), heating in the presence of MnO2 or Pt

52
Q

NaOH(aq) + excess H2S(g)

A

NaHS(s) + H2O(l)

53
Q

2NaOH(aq) + limited H2S(g)

A

Na2S(s) + 2H2O(l)

54
Q

2Na(s) + excess 2H2S(g)

A

2NaHS(s) + H2(g)

55
Q

2Na(s) + limited H2S(g)

A

Na2S(s) + H2(g)

56
Q

Mg(s) + H2S(g)

A

MgS(s) + H2(g)

57
Q

2Mg(s) + SO2(g)

A

2MgO(s) + S(s)

58
Q

3Mg(s) + SO2(g)

A

2MgO(s) + MgS(s)

59
Q

SO3(g) + H2O(l)

60
Q

H2SO4(aq) + H2O(l)

A

HSO4-(aq) + H3O+(aq)

61
Q

HSO4-(aq) + H2O(l)

A

SO42-(aq) + H3O+(aq)

62
Q

S(s) + 2H2SO4(l)

A

3SO2(g) + 2H2O(l)

63
Q

C(s) + 2H2SO4(l)

A

CO2(g) + 2SO2(g) + 2H2O(l)

64
Q

H2SO4(aq) + 2H2O(l)

A

SO42-(aq) + 2H3O+(aq)

65
Q

H2S2O3(aq)

A

S(s) + SO2(g) + H2O(l)

66
Q

C6H12O6(s) with conc.H2SO4

A

6C(s) + 6H2O(g)

67
Q

C2H5OH(l) with conc.H2SO4

A

C2H4(g) + H2O(l)

68
Q

Cl2(aq) + 2Br-(aq)

A

2Cl-(aq) + Br2(aq)

69
Q

Br2(aq) + 2I-(aq)

A

2Br-(aq) + I2(aq)

70
Q

AgCl

Colour and solubility in ammonia

A

White

Dissolves in dil. aqueous ammonia

71
Q

AgBr

Colour and solubility in ammonia

A

Pale yellow

Dissolves in conc. aqueous ammonia

72
Q

AgI

Colour and solubility in ammonia

A

Yellow

Insoluble in both dil. and conc. aqueous ammonia

73
Q

Oxidizing power of oxoacids of chlorine

A

HClO > HClO2 > HClO3 > HClO4

74
Q

SiCl4(l) + less 2H2O(l)

A

4HCl(aq) + SiO2(s)

75
Q

PCl5(l) + H2O(l)

A

POCl3(aq) + 2HCl(aq)

76
Q

SiCl4 (l) +excess 3H2O(l)

A

4HCl(aq) + H2SiO3(aq)

77
Q

NCl3(l) + 3H2O(l)

A

NH3(aq) + 3HOCl(aq)

78
Q

PCl3(l) + 3H2O(l)

A

H3PO3(aq) + 3HCl(aq)

79
Q

PCl5(l) + 4H2O(l)

A

H3PO4(aq) + 5HCl(aq)

80
Q

AsCl3(s) + 3H2O(l)

A

H3AsO3(aq) + 3HCl(aq)

81
Q

SbCl3(aq) + H2O(l)

A

SbOCl(s) + 2HCl(aq)

82
Q

BiCl3(aq) + H2O(l)

A

BiOCl(s) + 2HCl(aq)

83
Q

Cl2(g) + H2O(l)

A

HOCl(aq) + HCl(aq)

84
Q

Cl2(g) + cold and dil. 2NaOH(aq)

A

NaCl(aq) + NaOCl(aq) + H2O(l)

85
Q

3Cl2(g) + conc. 6NaOH(aq)

A

5NaCl(aq) + NaClO3(aq) + 3H2O(l)

86
Q

Lime water composition

87
Q

Nitrous acid

A

HNO2

Weak acid

88
Q

Binary acids

A

Acids containing H+ groups only O is absent

89
Q

Allotropes of Phosphrous

A

White, red and black

90
Q

Amphiprotic compound

A

They can either donate or accept a proton. Therefor it can act as an acid or base.
e.g: water

91
Q

NH3 + limited H2S =

92
Q

NH3 + excess H2S

93
Q

Variation of boiling points of hydrides of group 17

A

HF will have the highest boiling point due to the presence of hydrogen bonds.
HCl to HI boiling point increases due to the increasing molar mass. So that the London forces will be greater when going down the group.

94
Q

Gases having characteristics smells

A

SO2 - burnt matches
H2S - rotten egg smell
NH3

95
Q

Which anion is responsible for giving out a gas with a pungent smell and a yellow turbidity

96
Q

Although a reaction should take place spontaneously according to calculation, this does not happen practically, what will be the reason?

A

The activation energy of the reaction having a larger value

97
Q

Excess NH3 + Cl2

A

N2 + NH4Cl

98
Q

Dimers of nitogen

99
Q

Classification of S

A

2 main types known as crystalline and amorphous

Crystalline structures are rhombic sulfur and monoclinic sulfur

Amorphous structures are plastic, colloidal and milk of sulfur

Chemistry (15 decks)

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