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P blocks Flashcards

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1
Q

Metallic characteristics in Group 15

A

Nitrogen and phosphorus : Non metal
Arsenic Antimony : Metalloids
Bismuth : Metal

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2
Q

Composition of Nitrogen in atmosphere

A

78%

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3
Q

Electronic configuration of Group 15

A

ns2 np3

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4
Q

Why are group 15 elements extra stable?

A

Due to presence of half filled p orbitals (np3)

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5
Q

Atomic and Ionic radii trend in group 15

A

Increases down the group

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6
Q

Considerable increase in covalent radius from N to P, but small increase from As to Bi

A

Due to presence of completely filled d or f orbitals in heavier members

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7
Q

Anomality in Atomic radius trend in Group 15

A

Considerable increase from N to P but small increase from As to Bi

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8
Q

Ionisation enthalpy trend in group 15

A

Decreases down the group

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9
Q

Why does ionisation enthalpy decrease down the group 15?

A

Due to gradual increase in atomic size

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10
Q

Ionisation enthalpy of group 15 is much greater than group 14

A

Due to extra stable half filled p

orbitals

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11
Q

Electronegativity trend in group 15

A

Decreases down the group

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12
Q

Physical state of Group 15

A

N2 is gas,

other all are solids

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13
Q

Metallic character trend in group 15

A

Increases down the group

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14
Q

Why is N and P non metals
As and Sb metalloids
Bi metal??

A

Due to decrease in ionisation enthalpy down the group and increased atomic size

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15
Q

Boiling point and melting point trend in Group 15 with exception

A

Increases from top to bottom

Exception : Mp increases upto arsenic and then decreases upto Bismuth

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16
Q

Which group 15 element does not show allotrophy?

A

Nitrogen

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17
Q

Common Oxidation state of group 15

A

-3, +3, +5

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18
Q

Tendency to exhibut -3 Oxidation state decreases down the group

A

Due to increase in size and Mettalic character

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19
Q

Which element of Group 15 hardly shows -3 oxidation state

A

Bismuth

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20
Q

The stability of +5 Oxidation state increases / decreases down the group?

A

Decreases

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21
Q

Only well characterized Bi(V) compound?

A

BiF5

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22
Q

Stability of +5 state decreases and +3 state increases down the group.

A

Due to Inert Pair Effect

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23
Q

Oxidation states displayed by N when it reacts with O

A

+1, +2, +4

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24
Q

Oxidation state of Phosphorus in oxoacids

A

+1, +4

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25
Q

What happens to Oxidation state of nitrogen from +1 to +4 in acid solution?

A

Disproportionates

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26
Q

In which solution does the oxidation state of +1 to +4 of N disproportionates?

A

Acid solution

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27
Q

What happens to Phosphorus in alkali and acid solution?

A

All Oxidation states disproportionates to +5 and -3 state

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28
Q

In which solution does the Oxidation state of Phosphorus disproportionates to -5 and +3 states?

A

Alkali and Acid

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29
Q

Which oxidation state of As, Sb, and Bu becomes increasingly more stable wrt disproportionation

A

+3

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30
Q

Nitrogen is restricted to maximum of __ Covalency

A

4

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31
Q

Why is Nitrogen restricted to Maximum of 4 covalency

A

Due to absence of d orbitals

only four orbitals (s and 3 p) are available for bonding

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32
Q

Why does N differ from rest of the members of the group?

A

Small size
High Electronegativity
High ionization Enthalpy
Absence of d orbital

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33
Q

Why can Heavier members of group 15 not form pπ-pπ multiple bonds with itself?

A

As their atomic orbitals are large and diffuse and cannot have effective overlapping

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34
Q

Why does nitrogen exist as diatomic molecule with triple bond?

A

Due to its ability to form pπ-pπ multiple bonds

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35
Q

Bond Enthalpy of N is very high

A

Due to formation of Triple bond between the Nitrogen atoms of its molecule

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36
Q

Which bond does Bi form in its elemental state?

A

Metallic Bond

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37
Q

Single N-N bond is weaker than P-P bond

A

High interelectronic repulsion of the non bonding electrons

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38
Q

Catenation tendency is weaker in N

A

Due to weak single N-N bond

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39
Q

Nitrogen cannot form dπ-pπ bond

A

Due to absence of d orbitals

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40
Q

Group 15 Elements

A 
Nitrogen (N)
Phosphorus(P)
Arsenic (As)
Antimony (Sb)
Bismuth (Bi)
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41
Q

Why does stability of Hydrides decrease from NH3 to BiH3

A

Due to Decreasing Bond dissosiation enthalpy between E-H bond

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42
Q

Reducing character of hydrides of group 15

A

Increases from NH3 to BiH3

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43
Q

Which is the stronger reducing agent : NH3 or BiH3?

A

BiH3

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44
Q

Basicity trend of Group 15 Hydides

A

Decreases from NH3 to BiH3

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45
Q

Reactivity of Group 15 Elements towards Oxygen

A

E2O3

E2O5

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46
Q

Trend of Acidic Character of group 15 oxides

A

Decreases down the group

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47
Q

Reactivity towards Halogen of Group 15

A

EX3

EX5

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48
Q

Which trihalide of N are stable

A

NF3 only

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49
Q

Reactivity of group 15 elements toward Hydrogen

A

They form hydrides of the type EH3

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50
Q

pH nature of E2O3 in group 15

A

N2O3 P2O3 : Acidic
As2O3 Sb2O3 : Amphoteric
Bi2O3 : Basic

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51
Q

Trihalides of group 15 : covalent or ionic (with exception)

A

Covalent except BiF3

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52
Q

Reactivity of group 15 towards metal

A

group 15 elements will show -3 oxidation state

53
Q

PH3 has lower boiling point than NH3

A

Due to formation of H bond in NH3

54
Q

Group 15 More covalent : pentahalide or trihalide? Why?

A

PentaHalide

higher covalency due to higher oxidation state

55
Q

Which Oxide is more acidic? Higher oxidation state or lower oxidation stye?

A

Higher Oxidation Stae

56
Q

What type of agent is NH3

A

Mild Reducing Agent

57
Q

Stability of Hydrides of group 15

A

Stability decreases from NH3 to BiH3

58
Q

Trend in Bond Dissociation Enthalpy of E-H bond in group 15 Hydrides

A

Decreases from NH3 to BiH3

59
Q

Stability of triHalides in group 15

A

All trihalides are stable except those of N

60
Q

Nitrogen Does not form Pentahalida

A

Due to Absence of d orbital

61
Q

Strongest reducing agent among Group 15 hydrides

A

BiH3

62
Q

How to obtain Very Pure Nitrogen?

A

Thermal Decomposition of Barium/Sodium Azide
Ba(N3)2 -> Ba + 3 N2
Na(N3)2

63
Q

Properties of Nitrogen (N2)

A

Colourless
Odourless
Tasteless
Non-toxic gas

64
Q

Stable Isotopes of N

A

N-14

N-15

65
Q

Solubility of N2 in water

A

Very low

66
Q

B pt and F pt of N2

A

Low

67
Q

N2 is inert in room temperature

A

Due to high bond enthalpy of N-N triple bond

68
Q

Trend of Reactivity of N2 with temp

A

Increases rapidly with increase in temperature

69
Q

Reactivity of N2 with metal, hydrogen and oxygen

A

It reacts with them at high temp
Metal : M3N
Hydrogen : NH3
Oxygen : NO ( N2 + O2 -> 2NO )

70
Q

Use of N2

A

Production of NH3
Used where inert atmosphere is required
Liq. N2 used as refrigerant
In cryosurgery

71
Q

Properties of Ammonia

A

Colorless
Pungent Odour
Highly Soluble in water
Weak Base

72
Q

State of Ammonia in room temp

A

Gas

73
Q

Why is the Mp and Bp of ammonia higher than expected (by its molecular mass)

A

Due to formation of H bond in Liquid and solid phase

74
Q

Shape of ammonia

A

Trigonal Pyramidal with N at apex

75
Q

Nature of aqueous solution of Ammonia (Acid, Base, Neutral)

A

Weakly Basic

76
Q

Why is ammonia a base

A

Presence of a lone pair of e on N atom making it Lewis Base

77
Q

N2O Physical appearance n nature

A

colorless

Neutral

78
Q

NO Physical appearance n nature

A

Colorless Neutral

79
Q

N2O3 Physical appearance n nature

A

Blue solid

Acidic

80
Q

NO2 Physical appearance n nature

A

Brown Gas

Acidic

81
Q

N2O4 Physical appearance n nature

A

Colorless Solid/liquid

Acidic

82
Q

N2O5 Physical appearance n nature

A

Colorless Solid

Acidic

83
Q

Why does NO2 Dimerise

A

Due to presence of odd number of Valence electron (by making lewis dot structure it will be clear)

84
Q

Covalence of N in N2O5

A

4

85
Q

H2N2O2 name

A

HypoNitrous acid

86
Q

Hyponitrous acid formula

A

H2N2O2

87
Q

Nitrous acid formula

A

HNO2

88
Q

Nitric acid formula

A

HNO3

89
Q

Process to prepare Nitric acid (name)

A

Ostwald’s Process

90
Q

Concentration of Lab grade Nitric acid

A

68% by mass

91
Q

How does HNO3 exist in gaseous state

A

HNO3 exists as a Planar Molecule in Gaseous Phase

92
Q

Conc. HNO3 is oxidising or reducing agent??

A

Strong Oxidising agent

93
Q

Why does some metals (such as Al and Cr) not dissolve in Nitric acid

A

Dueto the formation of passive film of oxide on the surface

94
Q

Does conc HNO3 react with non metals??

A

Yes, it oxideses then to their corresponding acid (except C oxidising it to CO2)
I->HIO3
S-> H2SO4
P-> H3PO4

95
Q

Allotropes of Phosphorus

A

White, Red and Black (α , β)

96
Q

appearance of White Phosphorous

A

White waxy translucent solid

97
Q

Is white phosphorus poisonous?

A

Yes

98
Q

Solubility of White Phosphorus

A

Insoluble in water but soluble in CS2 (carbon disulphide)

99
Q

Does White Phosphorus glow in dark? what is the phenomenon called ?

A

Yes, Chemiluminescence

100
Q

Why is White phosphorus more reactive

A

Due to angular strain in P4 molecule

101
Q

Angle in White phosphorous

A

60°

102
Q

What happens to white phosphorus in air

A

It readily catches fire and gives white fumes of P4O10

103
Q

Lusture of Red Phosphorus

A

Iron grey lusture

104
Q

Properties of Red Phosphorus

A

Odourless

Non poisonous

105
Q

Solubility of Red Phosphorous

A

Insoluble in water as well as CS2 (Carbon Disulphide)

106
Q

Which is more reactive? red or white phosphorous??

A

White

107
Q

Does Red phosphorous show Chemiluminescence

A

No

108
Q

Structure of White P

A

Discrete Tetrahedral P4 molecules

109
Q

Shape of Red P

A

Polymeric chain of P4 tetrahedra

110
Q

Reactivity Order of Phosphorous

A

White > Red > Black

111
Q

Which phosphorous upon heating gives α - Black Phosphorous

A

Red P

112
Q

Which P upon heating gives β-Black Phosphorous ?

A

White P

113
Q

Why is impure Phosphine Immflamable

A

Due to presence of P2H4 or P4 vapours

114
Q

Properties of Phosphine

A

Colorless
Rotten fish Odour
Highly Poisonous

115
Q

What happens when PH3 comes in contact with oxidising agent

A

Explodes

116
Q

Solubility of PH3 in water

A

Slightly soluble in water

117
Q

Nature of PH3

A

weakly Basic

118
Q

What happens to aq. PH3 in the presence of light

A

It decomposes to red P and H2

119
Q

Bond angle of PH4+ ion is greater thn PH3

A

Due to lower bp-bp repulsion thn lp-bp repulsion

120
Q

Properties of PCl3

A

Colorless oily liquid

121
Q

Properties of PCl5

A

Yellowish white powder

122
Q

Shape of PCl5 in gaseous and Liquid phase

A

Trigonal bipyramidal

123
Q

Two axial bonds are longer than three equitorial bonds of PCl5 .. why?

A

The two axial bond pairs suffer more repulsion as compared to equatorial bond pairs

124
Q

How does PCl5 exist in Solid state

A

As an Ionic Solid with [PCl4]+ [PCl6]- ions

125
Q

Shpae of [PCl4]+

A

Tetrahedral

126
Q

Shape of [PCl6]-

A

Octahedral

127
Q

Why does PCl3 fume in moisture

A

PCl3 Hydrolyses in the presence of moisture giving fumes of HCl

128
Q

What happens when PCl5 is heated

A

It decomposes to PCl3 and Cl2

129
Q

Are all five bonds of PCl5 equivalent?

A

No, two axial bonds are longer thn three equatorial bonds

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