UNIT#05 SOLIDS Flashcards
1
Q
The transition temperature is shown by which of the following pairs:
A
➡Allotrope
➡Polymorph
(different crystalline forms of compounds)
2
Q
Lattice energy decreases with the increase in the size of ion because oppositely charged ions
A
become less tight
3
Q
Ionic solids are called true solids :
A
Crystalline
4
Q
Which ionic solid has the lowest lattice energy
A
CsCl
5
Q
Which of the following intermolecular forces are present in solid iodine:
(Iodine is non-polar)
A
London Dispersion force
6
Q
Which one of the following is not amorphous solid:
A
Table salt
7
Q
Ionic solids are called true solids
A
Crystalline
8
Q
The transition temperature of sulphur is:
A
95.5 °C
9
Q
Which of the following is isotropic property?
A
Metallic conduction
10
Q
When an element exists in more than one crystalline form, it is known as:
A
Allotropy
11
Q
A solid may be made up of:
A
➡Atoms
➡Molecuels
➡Ions
12
Q
Which one has the highest melting point and boiling point
A
Covalent crystal
(Network Structure)
13
Q
In a crystal, the atoms are located at the position of:
A
Minimum Potential Energy
(in order to gain maximum stability)
14
Q
Which of the following is anisotropic
A
Quartz
(Crystalline)
15
Q
Crystalline parts of otherwise amorphous solids are known as:
A
Crystallites
16
Q
Coinage metals are Cu, Ag and Au and they have ___ crystalline system
A
Cubic
17
Q
In the crystal structure of NaCl, the arrangement of Cl- ions are:
A
Face centred cubic
18
Q
In a crystal lattice the correct sequence of bond angles is:
A
bc=α, ca=β, ab=γ
19
Q
Total unit cell dimensions are;
A
SIx
20
Q
The cubic crystal system has the following unit cell dimensions
A
a=b=c and α=β=γ=90°
21
Q
The crystalline form of white tin is:
A
Tetragonal
22
Q
Molecular crystals are;
A
Soft
Formed by intermolecular forces
23
Q
The crystals formed due to London forces of interaction are:
A
Molecular
24
Q
The number of Cl- ions per units cell of a simple cubic lattice at the corer is/are:
A
1
25
Which is incorrect about the structure of iodine
I-I (g) > I-I (s)
Bond length
26
The coordination number of each ion in NaCl is:
6
27
The best conductors of electricity are;
Metallic solids
28
Independent molecule of NaCl may exist in:
Vapour Phase
29
Which of the following is an example of a polar molecular solids
Sugar
(have hydrogen bonding)
30
Solid CO2 (Dry ice) is an example of ___crystal
Molecular
(non-polar)
31
The coordination number of Na in the NaCl crystal is;
6
32
In the structure of NaCl, each sodium ion is surrounded by chloride ions
6
33
Which one of the following has the highest lattice energy
LiCl
34
The electrical conductivity of graphite is greater in one direction than in another due to;
Anisotropy
35
In diamond, each o the four outer electrons on every carbon atom is involved in covalent bonding. This means that there are no free electrons available. Which of the following property is explained by this statement
Diamond does not conduct heat and electricity
36
Graphite is one of the allotropic forms of Carbon it is;
➡Anisotrpic
➡Good conductor of electricity
37
A substance that has a sharp melting point in the following is
Diamond
(Crystalline solid)
38
The lattice energy is also called:
Crystal Energy
39
Which of the following is also an isomorph o copper?
Ag
40
Highest vapour pressure
Molecular solids
41
The molecular theory for metallic solids is;
Electron Gas Theory
42
Position of particles in crystalline solids represented by:
Lattice Point
43
The shape of iodine unit cells
Cubic
44
Radius ratio has units
Unitless
45
CuSO4.5H2O is an example of a crystal system
Triclinic
46
Which of the following solids is isotropic?
Amorphous solids
47
Properties due to a change of direction are called ___
Anisotropy
48
Which of the following has a transition temperature equal to 128 degrees celsius?
Na2CO3
49
Polymorphs have different:
Physical Properties
50
Allotropy is for:
Elements
51
HF has a higher boiling point than HCl due to:
Hydrogen bonding
52
Isomorphism is shown by:
➡Ionic solid
➡Metallic solid
➡Coinage metal
53
Current in electrolysis is carried through:
➡Postive ions
➡Negative ions
54
The most asymmetrical crystal system:
Cubic
55
Which one of the characteristics of ionic solids?
Solubility in polar solvents
56
The size and shape of the crystal depend upon some crystallographic elements which are:
6
57
The deliquescence is a property in which a solid
Absorbs moisture and turns to liquid form
58
Which one of them is known as supercooled liquids?
Glass
59
To conduct electricity through ionic solid, ions should be
Free
60
The smallest part of the crystal lattice has all the properties of the entire crystal this is called:
Unit cell
61
Lattice points are also called:
Lattice sites
62
The definite shape of NaCl crystal is its:
Habit
63
Which of the following are isomorphs
NaNO3, KNO3
64
Symmetry is the repetition of ___ when a crystal rotates at 360 ° along its axis
➡Faces
➡Angles
➡Edge
65
Which of the following is a directional bond?
H-bond
66
The thermal conductivity of graphite is greater when a mobile electron is moving to its layers
Parallel
67
Which of the following is true regarding polymorphism
same chemical properties
68
Types of solids on basis of bonds present in them
4
69
Ionic solids are;
Brittle
70
The coordination of a number of Na in NaCl
6
71
NaNO3 as unit cell
Rhombohedral
72
2 sides of the unit cell and 3 angles are equal in;
Tetragonal
73
Molecular solids are:
Bad conductors of electricity
74
The lattice energy of NaCl:
-787 kJ/mol
75
Metallic solids are:
Good conductor
76
Which is true about copper:
Can be easily bent
77
Lattice energy decrease when:
Charge to-size ratio decreases
78
Which one of the following is a giant molecule
SiO2
79
Molecular crystals are
Soft
80
The overall structure of diamond looksIce occupies more space than liquid water
Hexagonal
81
Ice occupies more space than liquid water
9%
82
The crystals formed due to London forces of interaction are
Molecular
83
The number of chloride ions per units cell of a simple cubic lattice at the corner is/are
1
84
Ionic solids are characterized by
Solubility in polar solvents
85
Which is incorrect about Structure of Iodine
I-I(g) < I-I(s) bond length
86
Overall ratio of silicon to oxygen atoms in silicon (IV) oxide is
1: 2
87
C-C Bond length in Diamond crystal are
154 pm
88
In interior of silicon (IV) oxide crystal, each Silicon atom is directly connected with
Four oxygen atoms
89
Iodine is a molecular solid because the forces between its molecules are
Van der Waals forces
90
The coordination number of each ion in NaCl is
6
91
The best conductors of electricity are
Metallic solids
92
Which of the following statement is incorrect about silica
Has very high thermal expansion
93
During which process empty spaces between particles become minimum
Condensation
94
A solid maybe made up of
Atoms, Ions or molecules
95
A malleable solid is one which can be
Converted into thin sheets
96
Which solids are called true solids
Crystalline solid
97
The arrangement ABC,ABC... is referred as
cubic close packing
98
Crystalline solids are classified on the basis of bonding into ______ types
4
99
Ionic crystals are characterized by
Solubility in polar solvents
100
NaCl crystal is
Cubic
101
Which element exists as discrete small molecule in the solid state
Iodine
102
Ice floats on the liquid water because
Water freezes at 0°C and is less dense than liquid water
103
Number of tetrahedral carbon atoms in unit cell of diamond is
4
104
The number of chloride ions per unit cell of NaCl are
4
105
The Crystal of diamond is
Covalent
106
1 unit cell of NaCl contains ion pairs
4
107
Which is not the property of silica
High thermal expansion
108
Silicon(IV) oxide crystal is an example of
Covalent crystal
109
Carbon atom in diamond is
sp3 hybridized
110
The given crystal lattice is for
Iodine
111
The volume of ice on freezing 200cm3 of water will be
218cm3
112
I - I Bond distance difference between i2(g) and i2(s) is
4.9 pm
113
Which one of the following contains maximum hydrogen bonding
H2O
114
Ammonia shows the maximum boiling point because of
Enhanced electronegativity character of nitrogen
115
The boiling point of H2O is 100°C while that of C2H5OH is 78.37°C. The reason is that
The number of hydrogen bonds per water molecule is greater than C2H5OH
116
All are crystalline solids except
Glass
117
Which is a pseudo solid?
Glue
118
____ may be isotropic under ordinary conditions:
Bromine
119
NaCl and CsF have same geometry because:
They have similar radii ratio
120
K2SO4 and K2CrO4 are isomorphic substances they have similar properties except one:
Chemical Properties
121
In structure of NaCl, the number of formula units per unit cell is:
4
122
Ionic solids are mostly of high density due to:
Close packing of ions
123
The molecuels of CO2 in dry ice form the:
Molecular Crystals
124
The arrangement of particles as a points in a crystal is called:
➡Crystal Lattice
➡Space Lattice
125
Unit cell is the smallest part and represented all features of the entire ____
Crystal
126
Crystalline solids have different properties;
1. Allotropy
2. Isomorphism
3. Polymorphism
Ionic compounds show which of the above properties:
➡II
➡III
127
Which property is incorrect about silica:
➡High transparency of light❌
➡Very low thermal expansion❌
➡Excellent insulator❌
➡Soluble in water✅
128
Which of the following is wrong?
➡Water has maximum density at 4°C❌
➡Molecular solids are relatively soft and volatile❌
➡In graphite carbon atom has tetrahedral geometry✅
➡Graphite is a good conductor of electricity❌
129
Which one is not the anisotropic behaviour:
➡Cleavage of crystal❌
➡Electrical Conductivity❌
➡Co-efficient of thermal expansion❌
➡Melting Point and Boiling Point✅
130
Which of the following is anisotropic?
Crystalline Solid
131
The lattice energy is maximum for:
MgF2
132
Ionic solids do not conduct the electrical current because:
Ions dont have translatory motion
133
The number of ion pairs per unit cell of NaCl are:
4
134
Crystalline solids are classified on the basis of bonding into;
Four types
135
In a crystal lattice the correct sequence of bond angles is:
bc=α, ca=β, ab=γ
136
The number of Cl-1 ions per unit cell of NaCl is;
4
137
The crystal of a diamond is;
Covalent
138
One unit cell of NaCl contains ion pairs:
Four
139
The share of Na+ ion on each edge in the NaCl unit cell is;
1/4
140
Silicon (IV) oxide crystal is an example of;
Covalent Crystal
141
The carbon atom in a diamond is;
sp3 hybridized
142
The given crystal lattice is for:
Iodine
143
The volume of ice on freezng 200 cm^3 of water will be:
218 cm^3
144
I-I bond distance difference between I2 and I2 is:
4.9 pm
145
Molecules in dry ice forms:
Covalent Crystal
146
Ionic solids are characterized by:
Solubility in a polar solvent
147
The lattice energy of NaCl is;
-787 kJ/mol
148
Which of the following is layered covalent crystalline solid
Cadmium Iodide
149
Maximum lattice energy is shown by:
LiCl
150
One unit cell of NaCl contains ion pairs;
Four
151
Which is incorrect about the structure of iodine;
➡Face-Centered Cubic❌
➡Metallic Appearance❌
➡I-I(g) > I-I(s)✅
➡I-I(g) < I-I(s)❌
152
The overall ratio of silicon to oxygen atoms in silicon (IV) oxide is;
1:2
153
C-C bond lengths in the diamond crystals are;
154 pm
154
The rate of evaporation of a liqui d does not depend on:
Material of container
155
Type of hybridization in diamond:
sp3
156
The overall structure of the diamond looks;
Face-centred cubic
157
The number of Cl-1 ions per unit cell of NaCl is;
4
158
The crystal of a diamond is;
Covalent
159
The crystals formed due to London forces of interaction are:
Molecular
160
The number of Cl-1 ions per unit cell of a simple cubic lattice at the corner is/are:
1
