P Block (II) Flashcards
1
Q
Sulphur is seen in volcano in the form of?
What is its smell?
A
H2S. Rotten egg smell
2
Q
Po is radioactive and exist as decay product of
A
Thirium and uranium minerals
3
Q
Oxygen shows +2 in
A
OF2
4
Q
Oxygen shows -1 in
A
Peroxides. H2O2. Na2O2. BaO2
5
Q
Oxygen show -(1/2) in
A
Superoxides. Ko2. RbO2. CsO2
6
Q
Sulphur compounds in which oxidation state are covalent
A
+4 and +6
7
Q
What can you say about electron gain enthalpy of group of 16 elements
A
They have negative values. It becomes less negative from S to Po and oxygen has least negative electron gain enthalpy.
8
Q
Structure of allotropes of S
A
Alpha S- rhombic/octahedral.
Beta S- monoclinic/prismatic
Gamma S- plastic
9
Q
In oxides of group 16, ___ and ___ are gases while others are ___
A
O3, So2, solids.
10
Q
Reducing property of grp 16 oxides?
A
Dtg Decrease. EO3 are all O.A.
11
Q
Geometry of Tetrafluorides and dichlorides of group 16
A
Tetraflourides:-
•Sp3d hybridisation.
•Trigonal bipyramidal.
•Sea saw geometry.
Dichlorides:-
•Sp3
•tetrahedral
12
Q
Dimeric monohalides of group 16 undergo disproportionation to form
A
EX4 and E
13
Q
Preparation of oxygen?
A
1)thermal decomposition of :-
- oxygen containing salts.
- oxides of metals low in reactivity series and higher oxides of some metals.
2) decomposition of H2O2.
Catalyst: MnO2 or finely divided metals (pt).
3) industrially:-
•fractional distillation of liquid air in claude’s apparatus.
•electrolysis of acidified or alkaline water using pt electrode.
14
Q
Magnetic nature of oxygen?
A
Paramagnetic inspite having even electrons. This is due to unpaired e in pi2px and pi2py mooecular Orbital
15
Q
Deacon’s process?
A
4 HCl + O2 → 2 Cl2 + 2H2O.
In the presence if CuCl2 and at 723K
16
Q
Give some simple and mixed oxides
A
Simple- MgO, Al2O3
Mixed- Pb3O4, Fe3O4
17
Q
How is the following formed and why are they called so.
a) basic oxides
b) acidic oxides ? excpetion?
c) amphoteric oxides with eg
d) neutral oxides
A
Basic oxides: formed by metals
Give a base with water
Give salt with acid
Acidic oxides: formed by non metals
Give an acid with water
Give salt with base
Note: oxides of some transition metals in high oxidation state( +5,+6,+7) also are acidic. V2O5, CrO3, Mn2O7
Amphoteric oxides: by metals or metalloids.
Form salt with both acid and base.
BeO, Al2O3, SnO, SnO2, PbO, PbO2, AsO3, Sb2O3, ZnO….
Neutral oxide: by some non metals
According to bronstef lowry concept, water is amphoteric.
18
Q
Reaction of Al2O3 with acid and base
A
Al2O3(s)+6NaOH(aq)+3H2O(l)→
2Na3 Al(OH)6
Al2O3+6HCl(aq)+9H2O(l)→2[Al(H2O)6]Cl3
19
Q
What is the preparation of ozone?
What to do if conc of ozone greater than 10% is neede?
A
Subjecting pure dry steam of oxygen to a silent electric discharge in a siemen’s ozoniser.
Use battery of ozonisers.
20
Q
Why is it necessary To use a silent electric discharge in the preparation of ozone?
A
O2 gives O3. The forward reaction is endothermic. To prevent the decomposition of ozone back into oxygen we use silent electric discharge. 
21
Q
Physical properties of ozone? (3)
A
Pale blue gas
Dark blue liquid
Violet black solid
22
Q
Above what concentration ozone becomes harmful
A
Above 100ppm.
23
Q
Why is decomposition of ozone spontaneous?
A
1) ozone is thermodynamically unstable and decomposes to give oxygen with the liberation of heat. Delta H= -ve
2) During the decomposition there is increase in entropy. Delta S= +ve
These two factors result in large
-ve delta G
24
Q
Give three example for the oxidation reaction using ozone
A
Ozone oxidises
black PbS to white PbSO4
KI solution to I2
Certain metals to their oxides.
25
Give the quantitative method for estimation of ozone gas
Ozone reacts with excess of KI solution liberating I2. This oxygen can be titrated against a standard solution of Na2S2O3(sodium thiosulphate)
26
Give the reaction used for detection of ozone. what is it called?
Ozone oxidides Hg to Hg2O. Due to formation of Hg2O, Hg loses its mobility and sticks to glass surface. This is called tailing of mercury. 
27
What is the reaction of ozone with nitric oxide(NO)?
It gives NO2 and O2
28
What is the structure of ozone give the bond length and bond angle
Angular or bent
Both single and double bond has 128pm
Bond angle 117 degrees
29
Give three uses of ozone
1) as a germicide , disinfectant and for sterilising water.
2) as a bleaching agent for fat ,oil ,starch flour et..
3) as an oxidising agent in manufacture of KMnO4 from K2MnO4
30
What is the colour of Alpha S
Yellow
31
What is the colour of beta S
Colourless
32
What is the solubility of alpha S
Insoluble in water but highly soluble in CS2. Also slightly soluble in benzene alcohol and ethers.
33
What is the solubility of beta S
Insoluble in water. soluble in CS2
34
What is the preparation of alpha S
By evaporating a solution of roll S in CS2
35
What is the stable temperature of alpha S
It is stable below 369K, above 369K it transforms to beta S
36
What is preparation of beta S
By melting alpha S followed by cooling. 
37
What is the stable temperature of beta S
Stable above 369K. below it, it transforms to Alpha S.
38
Compare the melting point and the specific gravity of alpha and beta S
Mp : alpha less than beta
| SG: alpha greater than beta
39
What is the structure of alpha and beta S
Both exist as S8 the molecules having puckered ring or crown like a structure.
40
What is the bond length and the bond angle in puckered ring structure of alotrope of S
Bond length: 204pm
| Bond angle: 107 degree
41
What are the other modifications of sulphur allotropes structure
6-20 S atoms per ring structure.
Eg: Cyclo S6 molecules have a chain shape
42
What is the Bond angle and bond length in cyclo s6 molecules
Bondle length: 205.7pm
| Bond angle: 102.2 degree
43
Magnetic nature of diatomic S2
Paramagnetic like O2.
44
Sulphur is mined from underground deposits by
Frasch process
45
Give three preparation of sulphur dioxide
1) lab preparation:by acidifying sulphite (SO3 2-) with dilute H2SO4
SO3 2-(aq)+2H+ (aq)→H2O(l)+SO2 (g)
2) industrial: as a by-product of the roasting of sulphide ores.
4FeS2 (s) +11O2 (g) → 2Fe2O3 (s) + 8SO2
3) it is formed together with a little (6-8%) sulphur trioxide when sulphur is burnt in air or oxygen.
46
What is the physical property of sulphur dioxide
Colourless gas with pungent smell
47
What is the solubility of sulphur dioxide
Highly soluble in water forming sulphurous acid H2SO3
48
What is the reaction of sulphur dioxide with bases
Being acidic, It forms salt
49
What is the reaction of sulphur dioxide with chlorine and oxygen
Directly react with chlorine in the presence of charcoal forming sulphonyl chloride( SO2Cl2)
With oxygen in the presence of V2O5 forming SO3
50
What is the oxidising or reducing nature of sulphur dioxide
Moist sulphur dioxide act as reducing agent
51
What is the test for sulphur dioxide. why is this test used
Reduction of MnO4-(purple) to Mn2+(colourless). it decolourises permagnate MnO4-
52
What is the structure of sulphur dioxide
Angular / V shape/ bent
Similar to oxygen
A resonance hybrid of two canonical structures. 
53
Give five uses of sulphur dioxide
1) for refining of petrol and sugar
2) as a disinfectant, preservative and Anti-chlor
3) bleaching agent for wool, silk et..
Bleaching action due to reducing action
4) manufacture of sulphuric acid (by contact process), NaHSO3, Ca(HSO3)2
5) liquid sulphur dioxide is a good solvent for many organic and inorganic chemicals.
54
Sulphurous acid formula
H2SO3
55
Formula of thiosulphurous acid
H2S2O2
56
Formula of hyposulphurous acid
H2S2O4
57
Formula of pyrosulphurous acid
H2S2O5
58
Name of H2SO3
Sulphurous acid
59
Name of H2S2O2
Thiosulphurous acid
60
Name of H2S2O4
Hyposulphurous acid
61
Name of H2S2O5
Pyrosulphurous acid.
62
Formula of thiosulphuric acid
H2S2O3
63
Name of H2S2O3
thiosulphuric acid
64
Formula of pyrosulphuric acid
H2S2O7
65
Name of H2S2O7
pyrosulphuric acid
66
Pyrosulphuric acid is also called
Fusing sulphuric acid/ oleum
67
Formula of dithionic acid
H2S2O6
68
Name of H2S2O6
dithionic acid
69
Formula of polythionic acid
H2S(n)O6
n=3,4,5,6
70
Name of H2S(n)O6
Polythionic acid.
71
Formula of peroxomonosulphuric acid
H2SO5
72
Name of H2SO5
peroxomonosulphuric acid
73
Name of H2s2O8
Peroxodisulphuric acid.
74
Formula of Peroxodisulphuric acid.
H2s2O8
75
Peroxodisulphuric acid. Also called
Marshalli acid
76
Peroxomonosulphuric acid is also called
Corous acid
77
Corous acid is
Peroxomonosulphuric acid
78
Marshalli acid is
Peroxodisulphuric acid
79
Blue vitrol?
CuSO4.5H2O
80
green vitrol?
FeSO4.7H2O
81
White vitrol?
ZnSO4.7H2O
82
Describe first step of contact process
Sulphur or pyrites burned in air or oxygen to get So2
83
Contact process is what type of catalysis
Heterogenous
84
Contact process is favoured at hig/low P and hig/low temp?
High P
| Low T
85
2nd step of contact process
Oxidation of SO2 in the presence of V2O5 at 720k and 2 bar pressure to give SO3
86
3rd process and last process of contact process
SO3 absorbed in 98% H2SO4 to get oleum. Oleun is diluted with water to get H2SO4 of any strength.
87
Sulphuric acid produced through contact process is how much % pure
96-98%
88
What type of catalysis is lead chamber process
Homogenous
89
Describe lead chamber process
Sulphur dioxide+ oxygen+ water (in the presence of NO(g) gives sulphuric acid
90
Lead chamber process is used in the preparation of
Sulphuric acid
91
Physical properties of sulphuric acid
Colourless dense oily liquid.
92
Mp and bp of h2SO4
Mp: 283k
Bp: 611k
93
types of chemical reactions given by sulphuric acid are due to? (4)
Strong acidic character
Great affinity for water(dehydration)
Less volatility
Oxidising action
94
H2SO4 ionises in how many steps
Two
95
Ka1 for first step and Ka2 for second step of ionisation of h2so4 are in the order
Ka1>ka2
96
First step of ionisation of h2so4 gives
Hso4^-
97
Second step of ionisation of h2so4 gives
So4^2-
98
How many series of salts are produces by h2so4 with bases like naoh?What are they?
Two.
Acidic salt hso4^-
Normal sal so4^2-
99
What does h2so4 do in a reaction due to its low volatility
Displace volatile acids from their salts
100
Oxidising action of h2so4 is intermediate of?
Hno3 (strong) and h2po4 (weak).
101
During the oxidising action of h2so4, it gets reduced to
So2
102
What happens in the reaction of h2so4 with cl2
OH group in h2so4 gets substituted by Cl atom forming chlorosubstituted products.
103
Manufacturing of nitrocellulose products and pickiling agents is a use of
Sulphuric acid
104
Which is used as an electrolyte in lead storage battery
Sulphuric acid
105
Flourine occurs as
Insoluble flourides like flourspar (CaF2), cryolite, flourapatite.
106
Chlorine bromine and iodine is present as
Cl- Br- I- of Na,K,Mg,Ca in sea water.
107
Formula of sylvine?
Kcl
108
Formula of carnallite
KCl.MgCl2.6H2O
109
Iodine is present in? Give with %
Sea weeds—-0.5%
| Chile saltpeter—— 0.2% as NaIO3
110
Iodine is present in chile saltpetee as
NaIO3
111
Physical occurrence and colour of F2?
Pale yellow gas
112
Physical occurrence and colour of Cl2
Greenish yellow gas
113
Physical occurrence and colour of Br2?
Reddish brown liquid
114
Physical occurrence and colour of I2?
Dark violet solid
115
The only liquid non metal?
Br2
116
Name of HClO
Hypochlorous acid
117
Formula of Hypochlorous acid
HClO
118
Name of HClO2
Chlorous acid
119
Formula of chlorous acid
HClO2
120
Name of HClO3
Chloric acid
121
Formula of chloric acid
HClO3
122
Name of HClO4
Perchloric acid
123
Formula of perchloric acid
HClO4
124
The only oxidation state shown by flourine
-1
125
Cl and Br also shows ___ and ___ oxidation state in their certain oxides
+4 and +6
126
Which two halogens show +4 and +6 in their oxides
Cl and Br
127
Which group has largest -ve electron gain enthalpy values. Give reason
Halogens. Because they are short of inly one elctron.
128
Dtg, electron gain enthalpy values of halogens become
Less negative
129
Order of negative value of electron gain enthalpy of halogens
Cl>F>Br>I.
130
Why does F has lesser negative electron gain enthalpy value than chlorine
Because of its small size and hence string interelectronic repulsion.
131
Down the group, order of mp and bp of halogens ___
Increases
132
Dtg, density of halogens ___
Increases
133
What is the order of bond dissociation enthalpy of halogens
Cl2 > Br2 > F2 > I2.
134
Lesser bond enthalpy of flourine is due to
Large electron -electron repulsion among the lone pairs.
135
Dtg, solubility of halogens in water ___
Decreases.
136
F2 dissolves in water forming
HF and ozonised oxygen
137
Which two halogens undergo disproportionation in water
Chlorine and bromine.
138
chlorine with water forms?
Hcl and HOCl
139
Solubility of iodine in water?
Almost insoluble.
140
How do you make iodine soluble in water
Iodine dissolves in water containing Ki due to formation of ionic complex KI3
141
Which complex is formed when iodine dissolves in water containing KI?
Potassium triiodide. KI3
142
Oxidation of I- using O2 in acid medium forms
I2 and water
143
Oxidation of I- using O2 in acid medium is equivalent to which reaction
Recerse of reaction of F2 with water
144
Order of mp of halides of hydrogen/hydride of halogen
HCl< HBr< HF< HI
145
Order of bp of halides of hydrogen/hydride of halogen
HCl< HBr< HI< HF
146
Higher mp and bp of HF is due to
Hydrogen bonding
147
HF exists as ___ due to H-bonding
Liquid
148
HF exists as liquid due to ___
H-bonding
149
Oxides of F
No oxides but oxygen flourides. OF2 and O2F2
150
O.s of halides except florine varies from
+1 to +7
151
Give three charecteristics of chlorine oxides
Powerful OA
Highly reactive
Tend to exlplode
152
Which chlorine oxide is a good bleaching agent
ClO2
153
Which chlorine oxide is used in water treatment
ClO2
154
Euchlorine is a mixture of
ClO2 and Cl2
155
Euchlorine is used as
Bleaching agent
156
Mixture of ClO2 and Cl2 is called
Euchlorine
157
Which halogen oxides are the least stable
Bromine oxides
158
Which halogen oxide is most stable
Iodine oxides
159
Iodine oxides are most stable soluble/insoluble gases/liquids/solids?
Insoluble solids
160
Iodine oxides decompose only on
Heating
161
Which haligen oxide is used for estimation of CO?
I2O5
162
I2O5 is used in the estimation of
CO
163
Order of stablity of halogen oxides?This order obtained is due to
I oxides > Cl oxides > Br oxides.
| Due to combined effect of kinetic and thermodynamic factors
164
Oxygen flourides are good
Flourinating agents just like IHC
165
Order of ionic character of metal halides
MF > MCl > MBr > MI
166
If a metal exhibits more than one o.s, halides in which o.s will be more covalent
Halides in higher o.s will be more covalent
167
Which is more covalent SnCl4 or SnCl2
SnCl4
168
Which is more covalent PbCl4 or PbCl2
PbCl4
169
Which is more covalent SbCl5 or SbCl3
SbCl5
170
Which is more covalent UF6 or UF4
UF6
171
Metals halides are covalent/ionic
Ionic
172
Non metal halides are covalent/ionic
Covalent
173
Chlorine discovered by
Sheele
174
Cl first prepared by
Sheele
175
The name chlorine was coined by
Davy
176
Give two lab preparations of chlorine
1) oxidation of concentrated Hcl using MnO2
Instead of HCl, a mixture of NaCl and conc H2SO4 also can be heated with MnO2
2) oxidation of HCl using KMnO4
177
Name two manufacture methods for prep of chlorine
```
Deacons process
Electrolytic process (of brine)
```
178
What are the byproducts obtained by electrolysis of brine in Down’s process
Na and Cl2
179
What are the byproducts obtained by electrolysis of brine in Caster-kellner process
NaOH , H2 and Cl2
180
Smell, colour, and physical property of chlorine
Greenish yellow gas with suffocating smell
181
Which halogen has a suffocating smell
Chlorine
182
Which halogen is denser than air
Chlorine
183
Is chlorine very hard to liquify?
No, it can be easily liquified
184
Solubility of chlorine in water?
Soluble in water
185
With NaOH, chlorine undergoes
Disproportionation
186
Chlorine with cold conc NaOH gives
NaCl and NaClO(sodium hypochlorite) and water.
187
Cl2 with hot conc NaOH gives
NaCl , NaClO3 (sodium chlorate) and water
188
Name of sodium chlorate
NaClO3
189
Name of sodium hypochlorite
NaClO
190
Dry chlorine passed through dry slaked lime gives
Bleaching powder:-
| A mixture of CaCl2 and Ca(OCl)2
191
Formula Calcium chlorohypochlorite?
CaOCl2
192
Formula of calcium oxychloride
CaOcl2
193
Give three names of CaOCl2
Calcium oxychloride / calcium hypochlorite / chloride of lime
194
Chloride of lime is
CaOCl2
195
Actual formula of bleaching powder
CaCl2 . Ca(OCl)2 . Ca(OH)2 . 2H2O
196
Give four examples for oxidation action of chlorine
Fe2+ to Fe3+
Sulphite(SO3^2-) to sulphate(SO4^2-)
SO2 to H2SO4
I2 to HIO3
197
During oxidation action of chlorine, it gets reduced to
HCl
198
What about the oxidation action of moist Cl2 on organic compounds
It oxidises(bleaches) coloured organic compounds to colourless
199
Bleaching effect of chorine is temporary or permanent?
Permanent
200
Chlorine has great affinity for
Hydrogen
201
Manufacture of insecticides like DDT, BHC is a use of
Chlorine
202
Solvents like westron, is a made using
Chlorine
203
Which haligen is used for sterilising water
Chlorine
204
Poisonous gases like phosgene, tear gas, mustard gas are made using
Chlorine
205
Formula of tear gas
CCl3NO2
206
Nitrochloroform is also called (2)
Tear gas or chloropierin
207
Mustard gas is also called
War gas
208
HCl was first prepared by
Glauber
209
Who showed that HCl is made of H2 and Cl2
Davy
210
Give two prep of HCl. Along with their temp of prep
1) common salt with conc h2so4 : 420k
| 2) common salt with NaHSO4 : 820k
211
Colour, property and smell of HCl?
Colourless gas with pungent smell
212
Can HCl be easily liquified?
Yes
213
Solubility of HCl in water
Highly soluble
214
HCl in water gives
H3O+ and Cl-
215
Aq solution of HCl is called
Hydrochloric acid
216
Hydrochloric acud is also called
Muriatic acid
217
HCl can _____ salts of weaker acids
Decompose
218
What is aquaregia
3:1 mixture of HCl and HNO3
219
HCl is used in which named process?
Deacon process
220
Extracting glue from animal bones is done using
HCl
221
Purifying bone black is done using
HCl
222
Which acid is used in the preparation of medicines
HCl
223
How many oxoacids are formed by flourine?
One
224
Which is the oxoacid formed by F2
HOF
225
How many oxoacids are formed by bromine and iodine?
Three
226
Which oxoacid is not formed by bromine and iodine
halous acid
227
Order of acidic Strength of halogen oxoacids in +1 o.s
HClO > HBrO > HIO
228
Order of acidic Strength of halogen oxoacids in +5 o.s
HClO3 > HBrO3 > HIO3
229
Order of acidic Strength of halogen oxoacids in +7 o.s
HClO4 > HBrO4 > HIO4
230
Order Acidic Strength of oxoacides of chlorine
HClO < HClO2 < HClO3 < HClO4
231
Order Acidic Strength of oxoacides of bromine
HBrO < HBrO3 < HBrO4
232
Order Acidic Strength of oxoacides of iodine
HIO < HIO3 < HIO4
233
Which IHC has the max number of atoms
IF7
234
The only IHC formed by flourine is
IF7
235
In the representation of IHC, XX’
| What can you say about X and X’ (2)
X is heavier/bigger than X’
| X is more electropositive than X’
236
hybridisation and number of lp in XX’
Sp3 / 3lp
237
hybridisation and number of lp in XX’3
Sp3d / 2lp
238
hybridisation and number of lp in XX’5
Sp3d2 / 1lp
239
hybridisation and number of lp in XX’7
Sp3d3 / 0 lp
240
What is the geometry of XX’
Linear
241
What is the geometry of XX’3
Bent T shape
242
What is the geometry of XX’5
Square pyramidal
243
What is the geometry of XX’7
Pentagonal bipyramidal
244
IHC are more/less reactive than elemental halogen?
More
245
IHC are weaker/stronger o.a than elemental halogen
Stronger
246
IHC are more reactive and stronger OA than elemental halogen except
Flourine
247
IHC are covalent/ionic and para/diamagnetic
Covalent diamagnetic
248
The _______ in second period and _______ in heavier elements(starting from__period onwards) have significant effects on the properties of elements
Absence of d orbital
Presence of d or d and f orbitals
Third period
249
From which period onwards presence of d or d and f orbitals is seen
Third period
250
Which are the non metals of group 15
N and P
251
Which are the metalloids of group 15
As and Sb
252
Which are the metals of group 15
Bi and Mo
253
Nitrogen conprises ___ % by vilume of the earth ___
78%
| Atmosphere
254
Formul of sodium nitrate
NaNO3
255
Sodium nitrate also called
Chile saltpeter
256
Formula of potassium nitrate
KNO3
257
Potassium nitrate also called
Indian saltpeter
258
General formula of apatite family
Ca9(PO4)6 . CaX2
Where X= F, Cl or OH
259
Flourapatite formula
3Ca3(PO4)2 . CaF2
260
Arsenic antimony and bismuth are found mainly as
Sulphide minerals
261
Mo has very short/long half life
Short
262
Why is Mo available in very little amount
Due to very short half life
263
Order of IE1 of group 15
Regualr decrease
264
Order of IE2 of grp 15
N > P > As > Bi > Sb
265
Order of IE3 of grp 15
N >> P > As > Bi > Sb
266
Order and values of electronegativity of grp 15
N(3.0) > P(2.1) > As(2.0) > Sb(1.9)= Bi(1.9)
267
order of covalent and ionic radii of grp 15
regular increase.
268
what can you say about the increase in covalent radius in grp 15. give reason
there is considerable increase from N to P. from As to Bi only small increase is seen.
reason : presence of completely filled d or/and f orbitals in heavier metals
269
order mp of grp 15 elements
N < P < Bi < Sb < As
270
order of bp of grp 15 elements
N < P < As < Bi < Sb
271
density of group 15 elements
increases
272
common oxidation states shown by group 15
-3 , +3, +5
273
in grp 15 tendancy to show -3 dtg
decreases
274
why does tendancy to show -3 in group 15 dtg decreases
increase in size and metallic character
275
Bi hardly forms any compound in ___ oxidation state
-3
276
stability of +5 state in grp 15 dtg
decreases
277
the only well characterised Bi(V) compound is
BiF5
278
stability of +3 in grp 15 dtg
increases
279
why does stability of +3 state of grp 15 dtg increase
inert pair effect
280
besides +5, N exhibits __, ___, __ oxidation state when it reacts with oxygen
+1, +2, +4
281
besides +5, N exhibits +1, +2, +4 oxidation state when it reacts with
oxygen
282
N doesnt form componds in ___ oxidation state with halogens. reason?
+5. no d orbitals
283
N doesnt form componds in +5 oxidation state with
halogens
284
phosphorous shows __ and __ oxidation states in some oxoacids
+1 and +4
285
phosphorous shows +1 and +4 oxidation states in some
oxoacids
286
in the case of nitrogen, all the oxidation states from __ to __ tend to disproportionate in acid solution
+1 to +4
287
in the case of nitrogen, all the oxidation states from +1 to +4 tend to disproportionate in ___ solution
acid
288
in the case of nitrogen, all the oxidation states from +1 to +4 tend to ______ in acid solution
disproportionate
289
in the case of P, all the intermediate oxidation states disproportionate into __ and __ in both alkali and acid
+5 and -3
290
in the case of P, all the ____ oxidation states disproportionate into +5 and -3 in both alkali and acid
intermediate
291
in the case of P, all the intermediate oxidation states disproportionate into +5 and -3 in both ____ and ___
acid and alkali
292
+3 oxidation state of As, Sb and Bi becomes increasingly stable with respect to
disproportionation
293
+3 oxidation state of As, Sb and Bi becomes increasingly/decreasingly stable with respect to disproportionation
increasingly
294
+3 oxidation state of ___, __ and ___ becomes increasingly stable with respect to disproportionation
As, Sb and Bi
295
___ oxidation state of As, Sb and Bi becomes increasingly stable with respect to disproportionation
+3
296
N is restricted to a maximum covalency of
four
297
why is macimum covalency of N four?
since only four (one s and three p) orbitals are available for bonding.
298
diatomic N has how many bonds
three
299
diatomic P, As, Sb has how many bonds
one
300
diatomic Bi has what kind of bond between it
metallic bond
301
the single N—N is weaker/stronger than single P—P. why?
weaker. high interelectronic repulsion of the non bonding electrons in N
302
catenation tendancy in N is weaker/stronger. why?
weaker. small bond length
303
___ and ___ can form dpi—dpi bond with transition metals when their compounds acts as ligands
P and As
304
P and As can form ______ bond with transition metals when their compounds acts as ligands
dpi—dpi
305
P and As can form dpi—dpi bond with transition metals when their compounds acts as____
ligands
306
P and As can form dpi—dpi bond with _______ when their compounds acts as ligands
transition metals
307
all the elements in group 15 forms hydrides. true or false
true
308
what type of hydrides are formed by grp 15
EH3
309
hydrides of grp 15 show regular/irregular gradation in their properties
regular
310
dtg, stability of hydrides of grp 15
decreases
311
why does stability of grp 15 hydrided dtg decrease
bond dissociation enthalpy decrease
312
dtg, reducing character of grp 15 hydrides
increases
313
which hydride of grp 15 is the only mild reducing agent
ammonia
314
dtg, basicity of hydrides of grp 15 hydrides
decreases. SbH3 >= BiH3
315
NH3 exhibits hydrogen bonding in ___ and ___ state
liquid and solid.
316
why does Nh3 exhibit H bonding
due to high electronegativity and small size
317
why does Nh3 have higher mp and bp than PH3
due to H bonding
318
what is the order of mp of grp 15 hydrides
PH3 < AsH3 < SbH3 < NH3
319
what is the order of bp of grp 15 hydrides
PH3 < AsH3 < NH3 < SbH3 < BiH3
320
what is the order of bond length of E—H of grp 15 hydrides
regular increase from Nh3 to SbH3
321
what is the order bond angle HEH in grp 15 hydrides
regular decrease from NH3 to SbH3
322
which hydride of grp 15 has the only -ve enthalpy of formation
Nh3
323
order of enthaly of formation of grp 15 hydrides
NH3 (-ve value) < PH3 < AsH3 < SbH3 < BiH3
324
what is the order of E—H bond dissosisiation energy of grp 15 hydrides
regular decrease from NH3 to SbH3
325
how many type of oxides are formed by group 15 elements
two
326
which are the two types of oxides formed by grp 15 elemnts
E2O3 and E2O5
327
the grp 15 oxide of higher/lower oxidation state is more acidic
higher
328
dtg, acidic character of grp 15 oxides
decreases
329
oxides of the type ___ of N and P are purely acidic
E2O3
330
oxides of the type E2O3 of __ and __ are purely acidic
N and P
331
oxides of the type E2O3 of N and P are purely ___
acidic
332
oxides of the type E2O3 of __ and __ are amphoteric
As and Sb
333
oxides of the type ___ of As and Sb are amphoteric
E2O3
334
oxides of the type E2O3 of As and Sb are ____
amphoteric
335
oxides of the type E2O3 of Bi is ___
basic
336
oxides of the type E2O3 of __ is basic
Bi
337
two type of halides formed by grp 15 elements
EX3 and EX5
338
Nitrogen does not form which type of halide. reason?
EH5. non availability of d orbitals
339
which element doesnt form halide of the type EX5
N
340
in grp 15 halides, pentahalides are more covalent/ionic than trihalides
covalent
341
in grp 15 halides, pentahalides are more covalent than trihalides. why
elements in +5 state will have more polarising power than those in +3 state
342
all the trihalides of grp 15 are stable. except
nitrogen trihalides
343
which is the only nitrogen trihalide that is stable
NF3
344
trihalides except ___ are predominantly covalent
BiF3
345
trigalides except BiF3 are predominantly
covalent
346
all the grp 15 elements react with metals forming their binary compounds, where the grp 15 elmnt will have a oxidation state of
-3
347
name of Ca3N2
calciun nitride
348
formula of calcium nitride
Ca3N2
349
formula of calcium phosphide
Ca3P2
350
name of Ca3P2
calcium phosphide
351
formula of sodium arsenide and zinc antimonide
Na3As and Zn3Sb2
352
name of Mg3Bi2
magnesium bismuthide
353
formula of magnesium bismuthide
Mg3Bi2
354
give the commercial preparation of nitrogen
liquefaction and fractional distillation of air
355
give the lab preparation of nitrogen. what are the byproducts
treating aq solution of ammonium chloride (NH4Cl) with sodium nitrite (NaNO2).
it gives N2, H2O and NaCl
356
in which physical state is nitrogen produced during its lab preparation
gas
357
small amounts of __ and __ are formed during the lab prep of nitrogen
No and HNO3
358
how is NO and HNO3 produced during lab prep of nitrogen removed
by passing the gas through aq sulphuric acid containing potassium dichromate
359
give two compounds whose thermal decomposition produces nitrogen
```
ammonium dichromate (NH4)2CrO7
sodium or barium azide Ba(N3)2
```
360
byproducts formed by thermal decomposition of ammonium dichromate
nitrogen, water and chromium oxide (Cr2O3)
361
give four physical property/appearnce of nitrogen
colourless odourless tasteless non toxic gas
362
what are the two stable isotopes of notrogen
14N and 15N
363
how soluble is nitrogen in water
low solubility
364
what is the solubility of N in water(give the values)
23.2 cm3 per litre of water at 273K and 1 bar pressure
365
nitrogen has high/low freezing and mp
low
366
why is dinitrogen inert at room temp
high bond enthalpy
367
how do you increase the reactivity of nitrogen
by increasing temp
368
at high temp nitrogen forms covalent/ionic nitrides with metals
ionic
369
at high temp nitrogen forms covalent/ionic nitrides with non metals
covalent
370
at what temp does N combine with Hydrogen in haber process
773K
371
formation of ammonia by habers process is endothermic/exothermic
exothermic
372
what is the enthalpy of formation of ammonia in haber process
-46.1 KJmol^-1
373
at what temp does nitrogen combine with oxygen to form NO
about 2000k
374
dinitrogen combines with oxygen at very high/low temp
high
375
calcium cyanamide is manufactured using
nitrogen
376
compound used for inert atmosphere in iron and steel industry
dinitrogen
377
which commpound is an inert diluent for reactive chemicals
dinitrogen
378
solid/liquid/gas nitrogen is used as a refrigerant
liquid
379
which compound is used in cryosurgery
diNitrogen
380
the small quantities ofammonia in air and soil is formed by
decay of nitrogenous organic matter like urea
381
give one small scale preparation of ammonia?
by decomposition of ammonium salts (NH4+)when treated with caustic alkali like caustic soda or calcium hydroxide.
382
large scale preparation of ammonia is by
haber process
383
at what. temp and pressure does haber process take place
temp: 700k
pressure: 200atm
384
what is used to increase the rate of attainment of equilibrium in haber process
catalyst iron oxide with small amounts of K2O and Al2O3
385
earlier the rate of haber process was increased using
iron as catalyst and Mb as promoter.
386
what is the colour, physical stae and smell of ammonia
colourless gas with pungent smell
387
ammonia associates through H bonding in which states
liquid and solid
388
geometry of ammonia
trigonal pyramidal
389
what is bond length and bond angle in ammonia
BA: 107.8 degrees
BL: 101.7pm
390
in the geometry of ammonia, ___ is at the apex of the structure
N atom
391
how soluble is ammonia in water
higly soluble
392
ammonia in water is a ___ solution
weakly basic
393
when salt solutions of metal reacts with aq solution of ammonia, it
precipitates the hydroxides (hydrated oxides in some metals) of the metals
394
colour of Zn(OH)2
white ppt
395
colour of Fe2O3.xH2O
brown ppt
396
presence of lp on ammonia makes it a
lewis base
397
name four nitrogenous fertilisers
ammonium nitrate
urea
ammonium phospate
ammonium sulphate
398
ammonia is used in manufacturing of inorganic/organic nitrogen compounds
inorganic
399
liquid ammonia is used as
refrigerant
400
formula of nitrous oxide
N2O
401
physical appearnace of nitrous oxide with acidic character
neutral colourless gas
402
physical appearnace of nitric oxide with acidic character
neutral colourless gas
403
physical appearnace of N2O3 with acidic character
acidic blue solid
404
physical appearnace of NO2 with acidic character
acidic brown gas
405
physical appearnace of N2O4 with acidic character
acidic colourless solid/liquid
406
physical appearnace of N2O5with acidic character
acidic colourless solid
407
preparation of nitrous oxide
thermal decomposition of NH4NO3
408
thermal decomposition of NH4NO3 gives
nitrous oxide + water
409
preparation of nitric oxide
2NaNO2 + 2FeSO4 + 3H2SO4
gives
Fe2(SO4)3 + 2NaHSO4 + 2H2O + 2NO
410
preparation of N2O3 is done at what temp
250K
411
preparation of N2O3 ?
2NO + N2O4 gives 2N2O3
412
preparation of NO2 is done at what temp
673K
413
preparation of NO2
thermal decomposition of 2Pb(NO3)2
414
thermal decomposition of 2Pb(NO3)2 gives
4NO2 + 2PbO + O2
415
preparation of N2O5
4HNO3 + P4O10 gives 4HPO3 + 2N2O5
