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P Block (II) Flashcards

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1
Q

Sulphur is seen in volcano in the form of?

What is its smell?

A

H2S. Rotten egg smell

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2
Q

Po is radioactive and exist as decay product of

A

Thirium and uranium minerals

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3
Q

Oxygen shows +2 in

A

OF2

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4
Q

Oxygen shows -1 in

A

Peroxides. H2O2. Na2O2. BaO2

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5
Q

Oxygen show -(1/2) in

A

Superoxides. Ko2. RbO2. CsO2

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6
Q

Sulphur compounds in which oxidation state are covalent

A

+4 and +6

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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.

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8
Q

Structure of allotropes of S

A

Alpha S- rhombic/octahedral.
Beta S- monoclinic/prismatic
Gamma S- plastic

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9
Q

In oxides of group 16, ___ and ___ are gases while others are ___

A

O3, So2, solids.

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10
Q

Reducing property of grp 16 oxides?

A

Dtg Decrease. EO3 are all O.A.

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11
Q

Geometry of Tetrafluorides and dichlorides of group 16

A

Tetraflourides:-
•Sp3d hybridisation.
•Trigonal bipyramidal.
•Sea saw geometry.

Dichlorides:-
•Sp3
•tetrahedral

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12
Q

Dimeric monohalides of group 16 undergo disproportionation to form

A

EX4 and E

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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.

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14
Q

Magnetic nature of oxygen?

A

Paramagnetic inspite having even electrons. This is due to unpaired e in pi2px and pi2py mooecular Orbital

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15
Q

Deacon’s process?

A

4 HCl + O2 → 2 Cl2 + 2H2O.

In the presence if CuCl2 and at 723K

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16
Q

Give some simple and mixed oxides

A

Simple- MgO, Al2O3

Mixed- Pb3O4, Fe3O4

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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.

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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

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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.

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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. 

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21
Q

Physical properties of ozone? (3)

A

Pale blue gas
Dark blue liquid
Violet black solid

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22
Q

Above what concentration ozone becomes harmful

A

Above 100ppm.

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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

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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.

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25
Q

Give the quantitative method for estimation of ozone gas

A

Ozone reacts with excess of KI solution liberating I2. This oxygen can be titrated against a standard solution of Na2S2O3(sodium thiosulphate)

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26
Q

Give the reaction used for detection of ozone. what is it called?

A

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. 

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27
Q

What is the reaction of ozone with nitric oxide(NO)?

A

It gives NO2 and O2

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28
Q

What is the structure of ozone give the bond length and bond angle

A

Angular or bent
Both single and double bond has 128pm
Bond angle 117 degrees

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29
Q

Give three uses of ozone

A

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

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30
Q

What is the colour of Alpha S

A

Yellow

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31
Q

What is the colour of beta S

A

Colourless

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32
Q

What is the solubility of alpha S

A

Insoluble in water but highly soluble in CS2. Also slightly soluble in benzene alcohol and ethers.

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33
Q

What is the solubility of beta S

A

Insoluble in water. soluble in CS2

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34
Q

What is the preparation of alpha S

A

By evaporating a solution of roll S in CS2

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35
Q

What is the stable temperature of alpha S

A

It is stable below 369K, above 369K it transforms to beta S

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36
Q

What is preparation of beta S

A

By melting alpha S followed by cooling. 

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37
Q

What is the stable temperature of beta S

A

Stable above 369K. below it, it transforms to Alpha S.

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38
Q

Compare the melting point and the specific gravity of alpha and beta S

A

Mp : alpha less than beta

SG: alpha greater than beta

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39
Q

What is the structure of alpha and beta S

A

Both exist as S8 the molecules having puckered ring or crown like a structure.

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40
Q

What is the bond length and the bond angle in puckered ring structure of alotrope of S

A

Bond length: 204pm

Bond angle: 107 degree

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41
Q

What are the other modifications of sulphur allotropes structure

A

6-20 S atoms per ring structure.

Eg: Cyclo S6 molecules have a chain shape

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42
Q

What is the Bond angle and bond length in cyclo s6 molecules

A

Bondle length: 205.7pm

Bond angle: 102.2 degree

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43
Q

Magnetic nature of diatomic S2

A

Paramagnetic like O2.

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44
Q

Sulphur is mined from underground deposits by

A

Frasch process

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45
Q

Give three preparation of sulphur dioxide

A

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.

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46
Q

What is the physical property of sulphur dioxide

A

Colourless gas with pungent smell

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47
Q

What is the solubility of sulphur dioxide

A

Highly soluble in water forming sulphurous acid H2SO3

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48
Q

What is the reaction of sulphur dioxide with bases

A

Being acidic, It forms salt

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49
Q

What is the reaction of sulphur dioxide with chlorine and oxygen

A

Directly react with chlorine in the presence of charcoal forming sulphonyl chloride( SO2Cl2)

With oxygen in the presence of V2O5 forming SO3

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50
Q

What is the oxidising or reducing nature of sulphur dioxide

A

Moist sulphur dioxide act as reducing agent

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51
Q

What is the test for sulphur dioxide. why is this test used

A

Reduction of MnO4-(purple) to Mn2+(colourless). it decolourises permagnate MnO4-

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52
Q

What is the structure of sulphur dioxide

A

Angular / V shape/ bent
Similar to oxygen
A resonance hybrid of two canonical structures. 

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53
Q

Give five uses of sulphur dioxide

A

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.

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54
Q

Sulphurous acid formula

A

H2SO3

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55
Q

Formula of thiosulphurous acid

A

H2S2O2

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56
Q

Formula of hyposulphurous acid

A

H2S2O4

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57
Q

Formula of pyrosulphurous acid

A

H2S2O5

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58
Q

Name of H2SO3

A

Sulphurous acid

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59
Q

Name of H2S2O2

A

Thiosulphurous acid

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60
Q

Name of H2S2O4

A

Hyposulphurous acid

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61
Q

Name of H2S2O5

A

Pyrosulphurous acid.

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62
Q

Formula of thiosulphuric acid

A

H2S2O3

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63
Q

Name of H2S2O3

A

thiosulphuric acid

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64
Q

Formula of pyrosulphuric acid

A

H2S2O7

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65
Q

Name of H2S2O7

A

pyrosulphuric acid

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66
Q

Pyrosulphuric acid is also called

A

Fusing sulphuric acid/ oleum

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67
Q

Formula of dithionic acid

A

H2S2O6

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68
Q

Name of H2S2O6

A

dithionic acid

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69
Q

Formula of polythionic acid

A

H2S(n)O6

n=3,4,5,6

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70
Q

Name of H2S(n)O6

A

Polythionic acid.

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71
Q

Formula of peroxomonosulphuric acid

A

H2SO5

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72
Q

Name of H2SO5

A

peroxomonosulphuric acid

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73
Q

Name of H2s2O8

A

Peroxodisulphuric acid.

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74
Q

Formula of Peroxodisulphuric acid.

A

H2s2O8

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75
Q

Peroxodisulphuric acid. Also called

A

Marshalli acid

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76
Q

Peroxomonosulphuric acid is also called

A

Corous acid

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77
Q

Corous acid is

A

Peroxomonosulphuric acid

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78
Q

Marshalli acid is

A

Peroxodisulphuric acid

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79
Q

Blue vitrol?

A

CuSO4.5H2O

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80
Q

green vitrol?

A

FeSO4.7H2O

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81
Q

White vitrol?

A

ZnSO4.7H2O

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82
Q

Describe first step of contact process

A

Sulphur or pyrites burned in air or oxygen to get So2

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83
Q

Contact process is what type of catalysis

A

Heterogenous

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84
Q

Contact process is favoured at hig/low P and hig/low temp?

A

High P

Low T

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85
Q

2nd step of contact process

A

Oxidation of SO2 in the presence of V2O5 at 720k and 2 bar pressure to give SO3

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86
Q

3rd process and last process of contact process

A

SO3 absorbed in 98% H2SO4 to get oleum. Oleun is diluted with water to get H2SO4 of any strength.

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87
Q

Sulphuric acid produced through contact process is how much % pure

A

96-98%

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88
Q

What type of catalysis is lead chamber process

A

Homogenous

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89
Q

Describe lead chamber process

A

Sulphur dioxide+ oxygen+ water (in the presence of NO(g) gives sulphuric acid

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90
Q

Lead chamber process is used in the preparation of

A

Sulphuric acid

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91
Q

Physical properties of sulphuric acid

A

Colourless dense oily liquid.

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92
Q

Mp and bp of h2SO4

A

Mp: 283k
Bp: 611k

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93
Q

types of chemical reactions given by sulphuric acid are due to? (4)

A

Strong acidic character
Great affinity for water(dehydration)
Less volatility
Oxidising action

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94
Q

H2SO4 ionises in how many steps

A

Two

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95
Q

Ka1 for first step and Ka2 for second step of ionisation of h2so4 are in the order

A

Ka1>ka2

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96
Q

First step of ionisation of h2so4 gives

A

Hso4^-

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97
Q

Second step of ionisation of h2so4 gives

A

So4^2-

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98
Q

How many series of salts are produces by h2so4 with bases like naoh?What are they?

A

Two.

Acidic salt hso4^-
Normal sal so4^2-

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99
Q

What does h2so4 do in a reaction due to its low volatility

A

Displace volatile acids from their salts

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100
Q

Oxidising action of h2so4 is intermediate of?

A

Hno3 (strong) and h2po4 (weak).

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101
Q

During the oxidising action of h2so4, it gets reduced to

A

So2

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102
Q

What happens in the reaction of h2so4 with cl2

A

OH group in h2so4 gets substituted by Cl atom forming chlorosubstituted products.

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103
Q

Manufacturing of nitrocellulose products and pickiling agents is a use of

A

Sulphuric acid

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104
Q

Which is used as an electrolyte in lead storage battery

A

Sulphuric acid

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105
Q

Flourine occurs as

A

Insoluble flourides like flourspar (CaF2), cryolite, flourapatite.

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106
Q

Chlorine bromine and iodine is present as

A

Cl- Br- I- of Na,K,Mg,Ca in sea water.

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107
Q

Formula of sylvine?

A

Kcl

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108
Q

Formula of carnallite

A

KCl.MgCl2.6H2O

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109
Q

Iodine is present in? Give with %

A

Sea weeds—-0.5%

Chile saltpeter—— 0.2% as NaIO3

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110
Q

Iodine is present in chile saltpetee as

A

NaIO3

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111
Q

Physical occurrence and colour of F2?

A

Pale yellow gas

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112
Q

Physical occurrence and colour of Cl2

A

Greenish yellow gas

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113
Q

Physical occurrence and colour of Br2?

A

Reddish brown liquid

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114
Q

Physical occurrence and colour of I2?

A

Dark violet solid

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115
Q

The only liquid non metal?

A

Br2

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116
Q

Name of HClO

A

Hypochlorous acid

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117
Q

Formula of Hypochlorous acid

A

HClO

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118
Q

Name of HClO2

A

Chlorous acid

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119
Q

Formula of chlorous acid

A

HClO2

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120
Q

Name of HClO3

A

Chloric acid

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121
Q

Formula of chloric acid

A

HClO3

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122
Q

Name of HClO4

A

Perchloric acid

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123
Q

Formula of perchloric acid

A

HClO4

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124
Q

The only oxidation state shown by flourine

A

-1

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125
Q

Cl and Br also shows ___ and ___ oxidation state in their certain oxides

A

+4 and +6

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126
Q

Which two halogens show +4 and +6 in their oxides

A

Cl and Br

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127
Q

Which group has largest -ve electron gain enthalpy values. Give reason

A

Halogens. Because they are short of inly one elctron.

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128
Q

Dtg, electron gain enthalpy values of halogens become

A

Less negative

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129
Q

Order of negative value of electron gain enthalpy of halogens

A

Cl>F>Br>I.

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130
Q

Why does F has lesser negative electron gain enthalpy value than chlorine

A

Because of its small size and hence string interelectronic repulsion.

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131
Q

Down the group, order of mp and bp of halogens ___

A

Increases

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132
Q

Dtg, density of halogens ___

A

Increases

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133
Q

What is the order of bond dissociation enthalpy of halogens

A

Cl2 > Br2 > F2 > I2.

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134
Q

Lesser bond enthalpy of flourine is due to

A

Large electron -electron repulsion among the lone pairs.

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135
Q

Dtg, solubility of halogens in water ___

A

Decreases.

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136
Q

F2 dissolves in water forming

A

HF and ozonised oxygen

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137
Q

Which two halogens undergo disproportionation in water

A

Chlorine and bromine.

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138
Q

chlorine with water forms?

A

Hcl and HOCl

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139
Q

Solubility of iodine in water?

A

Almost insoluble.

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140
Q

How do you make iodine soluble in water

A

Iodine dissolves in water containing Ki due to formation of ionic complex KI3

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141
Q

Which complex is formed when iodine dissolves in water containing KI?

A

Potassium triiodide. KI3

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142
Q

Oxidation of I- using O2 in acid medium forms

A

I2 and water

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143
Q

Oxidation of I- using O2 in acid medium is equivalent to which reaction

A

Recerse of reaction of F2 with water

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144
Q

Order of mp of halides of hydrogen/hydride of halogen

A

HCl< HBr< HF< HI

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145
Q

Order of bp of halides of hydrogen/hydride of halogen

A

HCl< HBr< HI< HF

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146
Q

Higher mp and bp of HF is due to

A

Hydrogen bonding

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147
Q

HF exists as ___ due to H-bonding

A

Liquid

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148
Q

HF exists as liquid due to ___

A

H-bonding

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149
Q

Oxides of F

A

No oxides but oxygen flourides. OF2 and O2F2

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150
Q

O.s of halides except florine varies from

A

+1 to +7

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151
Q

Give three charecteristics of chlorine oxides

A

Powerful OA
Highly reactive
Tend to exlplode

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152
Q

Which chlorine oxide is a good bleaching agent

A

ClO2

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153
Q

Which chlorine oxide is used in water treatment

A

ClO2

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154
Q

Euchlorine is a mixture of

A

ClO2 and Cl2

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155
Q

Euchlorine is used as

A

Bleaching agent

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156
Q

Mixture of ClO2 and Cl2 is called

A

Euchlorine

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157
Q

Which halogen oxides are the least stable

A

Bromine oxides

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158
Q

Which halogen oxide is most stable

A

Iodine oxides

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159
Q

Iodine oxides are most stable soluble/insoluble gases/liquids/solids?

A

Insoluble solids

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160
Q

Iodine oxides decompose only on

A

Heating

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161
Q

Which haligen oxide is used for estimation of CO?

A

I2O5

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162
Q

I2O5 is used in the estimation of

A

CO

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163
Q

Order of stablity of halogen oxides?This order obtained is due to

A

I oxides > Cl oxides > Br oxides.

Due to combined effect of kinetic and thermodynamic factors

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164
Q

Oxygen flourides are good

A

Flourinating agents just like IHC

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165
Q

Order of ionic character of metal halides

A

MF > MCl > MBr > MI

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166
Q

If a metal exhibits more than one o.s, halides in which o.s will be more covalent

A

Halides in higher o.s will be more covalent

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167
Q

Which is more covalent SnCl4 or SnCl2

A

SnCl4

168
Q

Which is more covalent PbCl4 or PbCl2

A

PbCl4

169
Q

Which is more covalent SbCl5 or SbCl3

A

SbCl5

170
Q

Which is more covalent UF6 or UF4

A

UF6

171
Q

Metals halides are covalent/ionic

A

Ionic

172
Q

Non metal halides are covalent/ionic

A

Covalent

173
Q

Chlorine discovered by

A

Sheele

174
Q

Cl first prepared by

A

Sheele

175
Q

The name chlorine was coined by

A

Davy

176
Q

Give two lab preparations of chlorine

A

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
Q

Name two manufacture methods for prep of chlorine

A 
Deacons process
Electrolytic process (of brine)
178
Q

What are the byproducts obtained by electrolysis of brine in Down’s process

A

Na and Cl2

179
Q

What are the byproducts obtained by electrolysis of brine in Caster-kellner process

A

NaOH , H2 and Cl2

180
Q

Smell, colour, and physical property of chlorine

A

Greenish yellow gas with suffocating smell

181
Q

Which halogen has a suffocating smell

A

Chlorine

182
Q

Which halogen is denser than air

A

Chlorine

183
Q

Is chlorine very hard to liquify?

A

No, it can be easily liquified

184
Q

Solubility of chlorine in water?

A

Soluble in water

185
Q

With NaOH, chlorine undergoes

A

Disproportionation

186
Q

Chlorine with cold conc NaOH gives

A

NaCl and NaClO(sodium hypochlorite) and water.

187
Q

Cl2 with hot conc NaOH gives

A

NaCl , NaClO3 (sodium chlorate) and water

188
Q

Name of sodium chlorate

A

NaClO3

189
Q

Name of sodium hypochlorite

A

NaClO

190
Q

Dry chlorine passed through dry slaked lime gives

A

Bleaching powder:-

A mixture of CaCl2 and Ca(OCl)2

191
Q

Formula Calcium chlorohypochlorite?

A

CaOCl2

192
Q

Formula of calcium oxychloride

A

CaOcl2

193
Q

Give three names of CaOCl2

A

Calcium oxychloride / calcium hypochlorite / chloride of lime

194
Q

Chloride of lime is

A

CaOCl2

195
Q

Actual formula of bleaching powder

A

CaCl2 . Ca(OCl)2 . Ca(OH)2 . 2H2O

196
Q

Give four examples for oxidation action of chlorine

A

Fe2+ to Fe3+

Sulphite(SO3^2-) to sulphate(SO4^2-)

SO2 to H2SO4

I2 to HIO3

197
Q

During oxidation action of chlorine, it gets reduced to

A

HCl

198
Q

What about the oxidation action of moist Cl2 on organic compounds

A

It oxidises(bleaches) coloured organic compounds to colourless

199
Q

Bleaching effect of chorine is temporary or permanent?

A

Permanent

200
Q

Chlorine has great affinity for

A

Hydrogen

201
Q

Manufacture of insecticides like DDT, BHC is a use of

A

Chlorine

202
Q

Solvents like westron, is a made using

A

Chlorine

203
Q

Which haligen is used for sterilising water

A

Chlorine

204
Q

Poisonous gases like phosgene, tear gas, mustard gas are made using

A

Chlorine

205
Q

Formula of tear gas

A

CCl3NO2

206
Q

Nitrochloroform is also called (2)

A

Tear gas or chloropierin

207
Q

Mustard gas is also called

A

War gas

208
Q

HCl was first prepared by

A

Glauber

209
Q

Who showed that HCl is made of H2 and Cl2

A

Davy

210
Q

Give two prep of HCl. Along with their temp of prep

A

1) common salt with conc h2so4 : 420k

2) common salt with NaHSO4 : 820k

211
Q

Colour, property and smell of HCl?

A

Colourless gas with pungent smell

212
Q

Can HCl be easily liquified?

A

Yes

213
Q

Solubility of HCl in water

A

Highly soluble

214
Q

HCl in water gives

A

H3O+ and Cl-

215
Q

Aq solution of HCl is called

A

Hydrochloric acid

216
Q

Hydrochloric acud is also called

A

Muriatic acid

217
Q

HCl can _____ salts of weaker acids

A

Decompose

218
Q

What is aquaregia

A

3:1 mixture of HCl and HNO3

219
Q

HCl is used in which named process?

A

Deacon process

220
Q

Extracting glue from animal bones is done using

A

HCl

221
Q

Purifying bone black is done using

A

HCl

222
Q

Which acid is used in the preparation of medicines

A

HCl

223
Q

How many oxoacids are formed by flourine?

A

One

224
Q

Which is the oxoacid formed by F2

A

HOF

225
Q

How many oxoacids are formed by bromine and iodine?

A

Three

226
Q

Which oxoacid is not formed by bromine and iodine

A

halous acid

227
Q

Order of acidic Strength of halogen oxoacids in +1 o.s

A

HClO > HBrO > HIO

228
Q

Order of acidic Strength of halogen oxoacids in +5 o.s

A

HClO3 > HBrO3 > HIO3

229
Q

Order of acidic Strength of halogen oxoacids in +7 o.s

A

HClO4 > HBrO4 > HIO4

230
Q

Order Acidic Strength of oxoacides of chlorine

A

HClO < HClO2 < HClO3 < HClO4

231
Q

Order Acidic Strength of oxoacides of bromine

A

HBrO < HBrO3 < HBrO4

232
Q

Order Acidic Strength of oxoacides of iodine

A

HIO < HIO3 < HIO4

233
Q

Which IHC has the max number of atoms

A

IF7

234
Q

The only IHC formed by flourine is

A

IF7

235
Q

In the representation of IHC, XX’

What can you say about X and X’ (2)

A

X is heavier/bigger than X’

X is more electropositive than X’

236
Q

hybridisation and number of lp in XX’

A

Sp3 / 3lp

237
Q

hybridisation and number of lp in XX’3

A

Sp3d / 2lp

238
Q

hybridisation and number of lp in XX’5

A

Sp3d2 / 1lp

239
Q

hybridisation and number of lp in XX’7

A

Sp3d3 / 0 lp

240
Q

What is the geometry of XX’

A

Linear

241
Q

What is the geometry of XX’3

A

Bent T shape

242
Q

What is the geometry of XX’5

A

Square pyramidal

243
Q

What is the geometry of XX’7

A

Pentagonal bipyramidal

244
Q

IHC are more/less reactive than elemental halogen?

A

More

245
Q

IHC are weaker/stronger o.a than elemental halogen

A

Stronger

246
Q

IHC are more reactive and stronger OA than elemental halogen except

A

Flourine

247
Q

IHC are covalent/ionic and para/diamagnetic

A

Covalent diamagnetic

248
Q

The _______ in second period and _______ in heavier elements(starting from__period onwards) have significant effects on the properties of elements

A

Absence of d orbital
Presence of d or d and f orbitals
Third period

249
Q

From which period onwards presence of d or d and f orbitals is seen

A

Third period

250
Q

Which are the non metals of group 15

A

N and P

251
Q

Which are the metalloids of group 15

A

As and Sb

252
Q

Which are the metals of group 15

A

Bi and Mo

253
Q

Nitrogen conprises ___ % by vilume of the earth ___

A

78%

Atmosphere

254
Q

Formul of sodium nitrate

A

NaNO3

255
Q

Sodium nitrate also called

A

Chile saltpeter

256
Q

Formula of potassium nitrate

A

KNO3

257
Q

Potassium nitrate also called

A

Indian saltpeter

258
Q

General formula of apatite family

A

Ca9(PO4)6 . CaX2

Where X= F, Cl or OH

259
Q

Flourapatite formula

A

3Ca3(PO4)2 . CaF2

260
Q

Arsenic antimony and bismuth are found mainly as

A

Sulphide minerals

261
Q

Mo has very short/long half life

A

Short

262
Q

Why is Mo available in very little amount

A

Due to very short half life

263
Q

Order of IE1 of group 15

A

Regualr decrease

264
Q

Order of IE2 of grp 15

A

N > P > As > Bi > Sb

265
Q

Order of IE3 of grp 15

A

N&raquo_space; P > As > Bi > Sb

266
Q

Order and values of electronegativity of grp 15

A

N(3.0) > P(2.1) > As(2.0) > Sb(1.9)= Bi(1.9)

267
Q

order of covalent and ionic radii of grp 15

A

regular increase.

268
Q

what can you say about the increase in covalent radius in grp 15. give reason

A

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
Q

order mp of grp 15 elements

A

N < P < Bi < Sb < As

270
Q

order of bp of grp 15 elements

A

N < P < As < Bi < Sb

271
Q

density of group 15 elements

A

increases

272
Q

common oxidation states shown by group 15

A

-3 , +3, +5

273
Q

in grp 15 tendancy to show -3 dtg

A

decreases

274
Q

why does tendancy to show -3 in group 15 dtg decreases

A

increase in size and metallic character

275
Q

Bi hardly forms any compound in ___ oxidation state

A

-3

276
Q

stability of +5 state in grp 15 dtg

A

decreases

277
Q

the only well characterised Bi(V) compound is

A

BiF5

278
Q

stability of +3 in grp 15 dtg

A

increases

279
Q

why does stability of +3 state of grp 15 dtg increase

A

inert pair effect

280
Q

besides +5, N exhibits __, ___, __ oxidation state when it reacts with oxygen

A

+1, +2, +4

281
Q

besides +5, N exhibits +1, +2, +4 oxidation state when it reacts with

A

oxygen

282
Q

N doesnt form componds in ___ oxidation state with halogens. reason?

A

+5. no d orbitals

283
Q

N doesnt form componds in +5 oxidation state with

A

halogens

284
Q

phosphorous shows __ and __ oxidation states in some oxoacids

A

+1 and +4

285
Q

phosphorous shows +1 and +4 oxidation states in some

A

oxoacids

286
Q

in the case of nitrogen, all the oxidation states from __ to __ tend to disproportionate in acid solution

A

+1 to +4

287
Q

in the case of nitrogen, all the oxidation states from +1 to +4 tend to disproportionate in ___ solution

A

acid

288
Q

in the case of nitrogen, all the oxidation states from +1 to +4 tend to ______ in acid solution

A

disproportionate

289
Q

in the case of P, all the intermediate oxidation states disproportionate into __ and __ in both alkali and acid

A

+5 and -3

290
Q

in the case of P, all the ____ oxidation states disproportionate into +5 and -3 in both alkali and acid

A

intermediate

291
Q

in the case of P, all the intermediate oxidation states disproportionate into +5 and -3 in both ____ and ___

A

acid and alkali

292
Q

+3 oxidation state of As, Sb and Bi becomes increasingly stable with respect to

A

disproportionation

293
Q

+3 oxidation state of As, Sb and Bi becomes increasingly/decreasingly stable with respect to disproportionation

A

increasingly

294
Q

+3 oxidation state of ___, __ and ___ becomes increasingly stable with respect to disproportionation

A

As, Sb and Bi

295
Q

___ oxidation state of As, Sb and Bi becomes increasingly stable with respect to disproportionation

A

+3

296
Q

N is restricted to a maximum covalency of

A

four

297
Q

why is macimum covalency of N four?

A

since only four (one s and three p) orbitals are available for bonding.

298
Q

diatomic N has how many bonds

A

three

299
Q

diatomic P, As, Sb has how many bonds

A

one

300
Q

diatomic Bi has what kind of bond between it

A

metallic bond

301
Q

the single N—N is weaker/stronger than single P—P. why?

A

weaker. high interelectronic repulsion of the non bonding electrons in N

302
Q

catenation tendancy in N is weaker/stronger. why?

A

weaker. small bond length

303
Q

___ and ___ can form dpi—dpi bond with transition metals when their compounds acts as ligands

A

P and As

304
Q

P and As can form ______ bond with transition metals when their compounds acts as ligands

A

dpi—dpi

305
Q

P and As can form dpi—dpi bond with transition metals when their compounds acts as____

A

ligands

306
Q

P and As can form dpi—dpi bond with _______ when their compounds acts as ligands

A

transition metals

307
Q

all the elements in group 15 forms hydrides. true or false

A

true

308
Q

what type of hydrides are formed by grp 15

A

EH3

309
Q

hydrides of grp 15 show regular/irregular gradation in their properties

A

regular

310
Q

dtg, stability of hydrides of grp 15

A

decreases

311
Q

why does stability of grp 15 hydrided dtg decrease

A

bond dissociation enthalpy decrease

312
Q

dtg, reducing character of grp 15 hydrides

A

increases

313
Q

which hydride of grp 15 is the only mild reducing agent

A

ammonia

314
Q

dtg, basicity of hydrides of grp 15 hydrides

A

decreases. SbH3 >= BiH3

315
Q

NH3 exhibits hydrogen bonding in ___ and ___ state

A

liquid and solid.

316
Q

why does Nh3 exhibit H bonding

A

due to high electronegativity and small size

317
Q

why does Nh3 have higher mp and bp than PH3

A

due to H bonding

318
Q

what is the order of mp of grp 15 hydrides

A

PH3 < AsH3 < SbH3 < NH3

319
Q

what is the order of bp of grp 15 hydrides

A

PH3 < AsH3 < NH3 < SbH3 < BiH3

320
Q

what is the order of bond length of E—H of grp 15 hydrides

A

regular increase from Nh3 to SbH3

321
Q

what is the order bond angle HEH in grp 15 hydrides

A

regular decrease from NH3 to SbH3

322
Q

which hydride of grp 15 has the only -ve enthalpy of formation

A

Nh3

323
Q

order of enthaly of formation of grp 15 hydrides

A

NH3 (-ve value) < PH3 < AsH3 < SbH3 < BiH3

324
Q

what is the order of E—H bond dissosisiation energy of grp 15 hydrides

A

regular decrease from NH3 to SbH3

325
Q

how many type of oxides are formed by group 15 elements

A

two

326
Q

which are the two types of oxides formed by grp 15 elemnts

A

E2O3 and E2O5

327
Q

the grp 15 oxide of higher/lower oxidation state is more acidic

A

higher

328
Q

dtg, acidic character of grp 15 oxides

A

decreases

329
Q

oxides of the type ___ of N and P are purely acidic

A

E2O3

330
Q

oxides of the type E2O3 of __ and __ are purely acidic

A

N and P

331
Q

oxides of the type E2O3 of N and P are purely ___

A

acidic

332
Q

oxides of the type E2O3 of __ and __ are amphoteric

A

As and Sb

333
Q

oxides of the type ___ of As and Sb are amphoteric

A

E2O3

334
Q

oxides of the type E2O3 of As and Sb are ____

A

amphoteric

335
Q

oxides of the type E2O3 of Bi is ___

A

basic

336
Q

oxides of the type E2O3 of __ is basic

A

Bi

337
Q

two type of halides formed by grp 15 elements

A

EX3 and EX5

338
Q

Nitrogen does not form which type of halide. reason?

A

EH5. non availability of d orbitals

339
Q

which element doesnt form halide of the type EX5

A

N

340
Q

in grp 15 halides, pentahalides are more covalent/ionic than trihalides

A

covalent

341
Q

in grp 15 halides, pentahalides are more covalent than trihalides. why

A

elements in +5 state will have more polarising power than those in +3 state

342
Q

all the trihalides of grp 15 are stable. except

A

nitrogen trihalides

343
Q

which is the only nitrogen trihalide that is stable

A

NF3

344
Q

trihalides except ___ are predominantly covalent

A

BiF3

345
Q

trigalides except BiF3 are predominantly

A

covalent

346
Q

all the grp 15 elements react with metals forming their binary compounds, where the grp 15 elmnt will have a oxidation state of

A

-3

347
Q

name of Ca3N2

A

calciun nitride

348
Q

formula of calcium nitride

A

Ca3N2

349
Q

formula of calcium phosphide

A

Ca3P2

350
Q

name of Ca3P2

A

calcium phosphide

351
Q

formula of sodium arsenide and zinc antimonide

A

Na3As and Zn3Sb2

352
Q

name of Mg3Bi2

A

magnesium bismuthide

353
Q

formula of magnesium bismuthide

A

Mg3Bi2

354
Q

give the commercial preparation of nitrogen

A

liquefaction and fractional distillation of air

355
Q

give the lab preparation of nitrogen. what are the byproducts

A

treating aq solution of ammonium chloride (NH4Cl) with sodium nitrite (NaNO2).

it gives N2, H2O and NaCl

356
Q

in which physical state is nitrogen produced during its lab preparation

A

gas

357
Q

small amounts of __ and __ are formed during the lab prep of nitrogen

A

No and HNO3

358
Q

how is NO and HNO3 produced during lab prep of nitrogen removed

A

by passing the gas through aq sulphuric acid containing potassium dichromate

359
Q

give two compounds whose thermal decomposition produces nitrogen

A 
ammonium dichromate (NH4)2CrO7
sodium or barium azide Ba(N3)2
360
Q

byproducts formed by thermal decomposition of ammonium dichromate

A

nitrogen, water and chromium oxide (Cr2O3)

361
Q

give four physical property/appearnce of nitrogen

A

colourless odourless tasteless non toxic gas

362
Q

what are the two stable isotopes of notrogen

A

14N and 15N

363
Q

how soluble is nitrogen in water

A

low solubility

364
Q

what is the solubility of N in water(give the values)

A

23.2 cm3 per litre of water at 273K and 1 bar pressure

365
Q

nitrogen has high/low freezing and mp

A

low

366
Q

why is dinitrogen inert at room temp

A

high bond enthalpy

367
Q

how do you increase the reactivity of nitrogen

A

by increasing temp

368
Q

at high temp nitrogen forms covalent/ionic nitrides with metals

A

ionic

369
Q

at high temp nitrogen forms covalent/ionic nitrides with non metals

A

covalent

370
Q

at what temp does N combine with Hydrogen in haber process

A

773K

371
Q

formation of ammonia by habers process is endothermic/exothermic

A

exothermic

372
Q

what is the enthalpy of formation of ammonia in haber process

A

-46.1 KJmol^-1

373
Q

at what temp does nitrogen combine with oxygen to form NO

A

about 2000k

374
Q

dinitrogen combines with oxygen at very high/low temp

A

high

375
Q

calcium cyanamide is manufactured using

A

nitrogen

376
Q

compound used for inert atmosphere in iron and steel industry

A

dinitrogen

377
Q

which commpound is an inert diluent for reactive chemicals

A

dinitrogen

378
Q

solid/liquid/gas nitrogen is used as a refrigerant

A

liquid

379
Q

which compound is used in cryosurgery

A

diNitrogen

380
Q

the small quantities ofammonia in air and soil is formed by

A

decay of nitrogenous organic matter like urea

381
Q

give one small scale preparation of ammonia?

A

by decomposition of ammonium salts (NH4+)when treated with caustic alkali like caustic soda or calcium hydroxide.

382
Q

large scale preparation of ammonia is by

A

haber process

383
Q

at what. temp and pressure does haber process take place

A

temp: 700k
pressure: 200atm

384
Q

what is used to increase the rate of attainment of equilibrium in haber process

A

catalyst iron oxide with small amounts of K2O and Al2O3

385
Q

earlier the rate of haber process was increased using

A

iron as catalyst and Mb as promoter.

386
Q

what is the colour, physical stae and smell of ammonia

A

colourless gas with pungent smell

387
Q

ammonia associates through H bonding in which states

A

liquid and solid

388
Q

geometry of ammonia

A

trigonal pyramidal

389
Q

what is bond length and bond angle in ammonia

A

BA: 107.8 degrees
BL: 101.7pm

390
Q

in the geometry of ammonia, ___ is at the apex of the structure

A

N atom

391
Q

how soluble is ammonia in water

A

higly soluble

392
Q

ammonia in water is a ___ solution

A

weakly basic

393
Q

when salt solutions of metal reacts with aq solution of ammonia, it

A

precipitates the hydroxides (hydrated oxides in some metals) of the metals

394
Q

colour of Zn(OH)2

A

white ppt

395
Q

colour of Fe2O3.xH2O

A

brown ppt

396
Q

presence of lp on ammonia makes it a

A

lewis base

397
Q

name four nitrogenous fertilisers

A

ammonium nitrate
urea
ammonium phospate
ammonium sulphate

398
Q

ammonia is used in manufacturing of inorganic/organic nitrogen compounds

A

inorganic

399
Q

liquid ammonia is used as

A

refrigerant

400
Q

formula of nitrous oxide

A

N2O

401
Q

physical appearnace of nitrous oxide with acidic character

A

neutral colourless gas

402
Q

physical appearnace of nitric oxide with acidic character

A

neutral colourless gas

403
Q

physical appearnace of N2O3 with acidic character

A

acidic blue solid

404
Q

physical appearnace of NO2 with acidic character

A

acidic brown gas

405
Q

physical appearnace of N2O4 with acidic character

A

acidic colourless solid/liquid

406
Q

physical appearnace of N2O5with acidic character

A

acidic colourless solid

407
Q

preparation of nitrous oxide

A

thermal decomposition of NH4NO3

408
Q

thermal decomposition of NH4NO3 gives

A

nitrous oxide + water

409
Q

preparation of nitric oxide

A

2NaNO2 + 2FeSO4 + 3H2SO4

gives

Fe2(SO4)3 + 2NaHSO4 + 2H2O + 2NO

410
Q

preparation of N2O3 is done at what temp

A

250K

411
Q

preparation of N2O3 ?

A

2NO + N2O4 gives 2N2O3

412
Q

preparation of NO2 is done at what temp

A

673K

413
Q

preparation of NO2

A

thermal decomposition of 2Pb(NO3)2

414
Q

thermal decomposition of 2Pb(NO3)2 gives

A

4NO2 + 2PbO + O2

415
Q

preparation of N2O5

A

4HNO3 + P4O10 gives 4HPO3 + 2N2O5

Chemistry (2 decks)

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