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P block elements Flashcards

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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
NH4OH(aq)
NH4+(aq) + OH ̅(aq)
26
2NH4OH(aq) + dil. H2SO4(aq)
(NH4)2SO4(aq) + 2H2O(l)
27
NH4+(aq) + H2O(l)
NH3(aq) + H3O+(l)
28
NH4Cl(aq) + NaOH(aq)
NaCl(aq) + NH3 (g) + H2O(l)
29
excess ammonia, 2NH3(g) + 3Cl2(g)
N2(g) + 6HCl(g)
30
Excess 3Cl2(g) + NH3(g)
3HCl(g) + NCl3(l)
31
NCl3(l) + 3H2O(l)
NH3(g) + 3HOCl(aq)
32
NH3(g) + HCl(g)
NH4Cl(s)
33
3CuO(s) + 2NH3(g)
N2(g) + 3Cu(s) + 3H2O(g)
34
2Na(s) + 2NH3(l)
2NaNH2(l) + H2(g)
35
3Mg(s) + 2NH3(l)
Mg3N2(l) + 3H2(g)
36
(NH4)2CO3(s)
2NH3(g) + CO2(g) + H2O(g)
37
NH4Cl(s)
NH3(g) + HCl(g)
38
(NH4)2SO4(s)
NH3(g) + H2SO4(g)*
39
NH4NO2(s)
N2(g) + 2H2O(g)
40
NH4NO3(s)
N2O(g) + 2H2O(g)
41
(NH4)2Cr2O7(s)
N2(g) + Cr2O3(s) + 4H2O(g)
42
NH4+(aq) + OH¯(aq)
NH3(g) + H2O(l)
43
NH3(g) + HCl(g)
NH4Cl(s) white fumes
44
2NO3ˉ (aq) + 4H2SO4(l) + 6Fe2+(aq)
6Fe3+(aq) + 2NO(g) + 4SO42ˉ (aq) + 4 H2O(l)
45
Fe2+(aq)+ NO(g)
[Fe(NO)]2+(aq) brown colour
46
3NO3ˉ (aq) + 8Al(s) + 5OHˉ(aq) + 18H2O(l)
3NH3(g) + 8[Al(OH)4]ˉ(aq)
47
2H2O(l)
H3O+(aq) + OH-(aq)
48
H2O(l) + HCl(aq)
H3O+(aq) + Cl-(aq)
49
H2O(l) + NH3(aq)
NH4+(aq) + OH-(aq)
50
2H2O2(aq)
O2(g) + 2H2O(l)
51
2KClO3(s)
2KCl(s) + 3O2(g), heating in the presence of MnO2 or Pt
52
NaOH(aq) + excess H2S(g)
NaHS(s) + H2O(l)
53
2NaOH(aq) + limited H2S(g)
Na2S(s) + 2H2O(l)
54
2Na(s) + excess 2H2S(g)
2NaHS(s) + H2(g)
55
2Na(s) + limited H2S(g)
Na2S(s) + H2(g)
56
Mg(s) + H2S(g)
MgS(s) + H2(g)
57
2Mg(s) + SO2(g)
2MgO(s) + S(s)
58
3Mg(s) + SO2(g)
2MgO(s) + MgS(s)
59
SO3(g) + H2O(l)
H2SO4(aq)
60
H2SO4(aq) + H2O(l)
HSO4-(aq) + H3O+(aq)
61
HSO4-(aq) + H2O(l)
SO42-(aq) + H3O+(aq)
62
S(s) + 2H2SO4(l)
3SO2(g) + 2H2O(l)
63
C(s) + 2H2SO4(l)
CO2(g) + 2SO2(g) + 2H2O(l)
64
H2SO4(aq) + 2H2O(l)
SO42-(aq) + 2H3O+(aq)
65
H2S2O3(aq)
S(s) + SO2(g) + H2O(l)
66
C6H12O6(s) with conc.H2SO4
6C(s) + 6H2O(g)
67
C2H5OH(l) with conc.H2SO4
C2H4(g) + H2O(l)
68
Cl2(aq) + 2Br-(aq)
2Cl-(aq) + Br2(aq)
69
Br2(aq) + 2I-(aq)
2Br-(aq) + I2(aq)
70
AgCl | Colour and solubility in ammonia
White | Dissolves in dil. aqueous ammonia
71
AgBr | Colour and solubility in ammonia
Pale yellow | Dissolves in conc. aqueous ammonia
72
AgI | Colour and solubility in ammonia
Yellow | Insoluble in both dil. and conc. aqueous ammonia
73
Oxidizing power of oxoacids of chlorine
HClO > HClO2 > HClO3 > HClO4
74
SiCl4(l) + less 2H2O(l)
4HCl(aq) + SiO2(s)
75
PCl5(l) + H2O(l)
POCl3(aq) + 2HCl(aq)
76
SiCl4 (l) +excess 3H2O(l)
4HCl(aq) + H2SiO3(aq)
77
NCl3(l) + 3H2O(l)
NH3(aq) + 3HOCl(aq)
78
PCl3(l) + 3H2O(l)
H3PO3(aq) + 3HCl(aq)
79
PCl5(l) + 4H2O(l)
H3PO4(aq) + 5HCl(aq)
80
AsCl3(s) + 3H2O(l)
H3AsO3(aq) + 3HCl(aq)
81
SbCl3(aq) + H2O(l)
SbOCl(s) + 2HCl(aq)
82
BiCl3(aq) + H2O(l)
BiOCl(s) + 2HCl(aq)
83
Cl2(g) + H2O(l)
HOCl(aq) + HCl(aq)
84
Cl2(g) + cold and dil. 2NaOH(aq)
NaCl(aq) + NaOCl(aq) + H2O(l)
85
3Cl2(g) + conc. 6NaOH(aq)
5NaCl(aq) + NaClO3(aq) + 3H2O(l)
86
Lime water composition
Ca(OH)2
87
Nitrous acid
HNO2 | Weak acid
88
Binary acids
Acids containing H+ groups only O is absent
89
Allotropes of Phosphrous
White, red and black
90
Amphiprotic compound
They can either donate or accept a proton. Therefor it can act as an acid or base. e.g: water
91
NH3 + limited H2S =
(NH4)2S
92
NH3 + excess H2S
NH4HS
93
Variation of boiling points of hydrides of group 17
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
Gases having characteristics smells
SO2 - burnt matches H2S - rotten egg smell NH3
95
Which anion is responsible for giving out a gas with a pungent smell and a yellow turbidity
S2O3 2-
96
Although a reaction should take place spontaneously according to calculation, this does not happen practically, what will be the reason?
The activation energy of the reaction having a larger value
97
Excess NH3 + Cl2
N2 + NH4Cl
98
Dimers of nitogen
N204 | N205
99
Classification of S
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

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