JEE Main Chemistry - State of Matter Solid State
Exam Duration: 60 Mins Total Questions : 30
Which of the following is not characteristic of crystalline solids?
- (a)
They have a regular geometry
- (b)
They have sharp melting points
- (c)
They are isotropic
- (d)
They undergo a clean cleavage
Which of the following is not a crystalline solid?
- (a)
Naphthalene
- (b)
Benzoic acid
- (c)
Copper
- (d)
Fibre glass
Solid carbon dioxide is an example of
- (a)
metallic crystal
- (b)
cavalent crystal
- (c)
molecular crystal
- (d)
ionic crystal
An example of a substance possessing giant covalent structure is
- (a)
Solid \(CO_2\)
- (b)
silica
- (c)
iodine crystal
- (d)
white phosphorus
In face centred cubic cell, an atom at the face centre is shared by
- (a)
4 unit cells
- (b)
2 unit cells
- (c)
1 unit cell
- (d)
6 unit cells
A monoclinic crystal has dimensions
- (a)
\(a\neq b \neq c, \alpha = \gamma = 90^o; \beta\neq 90^o\)
- (b)
\(a= b = c, \alpha = \beta = \gamma = 90^o\)
- (c)
\(a= b = c, \alpha = \beta = 90^o; \gamma = 120^o\)
- (d)
\(a\neq b = c, \alpha = \beta = \gamma= 120^o\)
The ABAB... packing and ABCABC.... packing are respectively called as
- (a)
hep and ccp
- (b)
ccp and hcp
- (c)
bcc and hep
- (d)
hep and bcc
At the limiting value of radius ratio \({r^+\over r^-},\)
- (a)
forces of attraction are larger than the forces of repulsion
- (b)
forces of attraction are smaller
- (c)
than the forces of repulsion
- (d)
None of the above
For an ionic crystal of the general formula AX and coordination number 6, the value of radius ratio will be
- (a)
greater than 0.73
- (b)
in between 0.73 and 0.41
- (c)
in between 0.14 and 0.22
- (d)
less than 0.22
Edge length of \(M^+X^-\) (fcc structure) is \(7.2 \mathring { A } \) and radius of cation is \(1.6 \mathring { A } \) Assuming \(M^+-X^-\) contact along cell edge, radius of \(X^-\) ion is
- (a)
\(2.0 \mathring { A } \)
- (b)
\(5.6 \mathring { A } \)
- (c)
\(2.8 \mathring { A } \)
- (d)
\(3.8 \mathring { A } \)
In \(A^+\ B^-\) ionic compound, radii of \(A^+\) and \(B^-\) ions are 180 and 187 pm respectively. The crystal structure of the compound will be
- (a)
NaCl type
- (b)
CsCl type
- (c)
ZnS type
- (d)
Similar to diamond
The structure of \(Na_2O\) crystal is
- (a)
NaCl type
- (b)
CsCl type
- (c)
ZnS type
- (d)
antifluorite type
Mathc the following and choose the correct option.
Type of packing | Voild volume |
A. hcp | p. 0.38 |
B. sc | q. 0.48 |
C. bcc | r. 0.22 |
D. dc(diamond cubic) | s. 0.66 |
- (a)
A B C D p r q s - (b)
A B C D r q p s - (c)
A B C D r p q s - (d)
A B C D p q r s
KCL crystallises in the same type of lattice as does NaCl. Given, \({r_{Na^+}\over r_{cl^-}}=0.5\) and \({r_{Na\ +}\over r_{K^+}}=0.7.\) Then ratio of the side of the unit cell for NaCl to that for KCl is
- (a)
1 : 1.172
- (b)
1 ; 1.143
- (c)
1 : 1.1413
- (d)
1 : 1.732
Calculate the wavelength of X-rays which produces a diffraction angle \(2\theta\) equal to \(16.80^o\) for a crystal. Assume first order diffraction with inter- particle distance in crystal of 0.2 nm.
- (a)
\(7.04\times 10^{-9}m\)
- (b)
\(5.84\times 10^{-11}\ m\)
- (c)
\(3.4\times 10^{-10}\ m\)
- (d)
\(5.84\times 10^{-9}\ m\)
The anions (A) form hexagonal close packing and atoms (M) occupy only two-third of the octahedral voids. The general formula of the compound is
- (a)
\(M_2A_3\)
- (b)
MA
- (c)
\(MA_2\)
- (d)
\(M_3A_2\)
The NaCl structure can be converted into CsCl structure
- (a)
by application of high pressure
- (b)
by heating to 760 K
- (c)
both by heat and pressure
- (d)
the conversion is not possible
The number of atoms in 100g of an fcc crystal with density \(d = 10 g cm^{-3}\) and cell edge as 200 pm is equal to
- (a)
\(3\times 10^{25}\)
- (b)
\(0.5\times 10^{25}\)
- (c)
\(1\times 10^{25}\)
- (d)
\(2\times 10^{25}\)
Edge length of face centred cubic unit cell is 508 pm. Then, radius of atom is
- (a)
179.6 pm
- (b)
288 pm
- (c)
618 pm
- (d)
398 pm
The pykometric density of sodium chloride crystal is \(2.165\times 10^3\ kgm^{-3}.\) While its X-rays density is \(2.178\times 10^3\ kgm^{-3}\) The fraction of unoccupied sites in NaCl crystal is
- (a)
5.97
- (b)
\(5.97\times 10^{-2}\)
- (c)
\(5.97\times 10^{-1}\)
- (d)
\(5.97\times 10^{-3}\)
If 'a' stands for the edge length of the cubic systems simple cubic, body centred cubic and face centred cubic, then the ratio of radii of the spheres in these system will be respectively
- (a)
\({1\over 2}a:\sqrt3 a:{1\over \sqrt 2}a\)
- (b)
\({1\over 2}a:{\sqrt3\over 2}a:{\sqrt2\over 2}a\)
- (c)
\(1a:\sqrt3a:\sqrt2\ a\)
- (d)
\({1\over 2}a:{\sqrt3 \over 4}a:{1\over 2\sqrt 2}a\)
Calcium metal crystallises in fcc lattice with edge length 556 pm. Calculate the denstity (in g \(cm^{-3}\)) of metal if it contains 0.2% Schottky defects.
- (a)
3.992
- (b)
1.5455
- (c)
1.5427
- (d)
1.4987
If NaCl is doped with \(10^{-3}\) mol % \(SrCl_2,\) then concentration of cation vacancies will be
- (a)
\(1\times 10^{-3}\ mol\) %
- (b)
\(2\times 10^{-3}\ mol\) %
- (c)
\(3\times 10^{-3}\ mol\) %
- (d)
\(4\times 10^{-3}\ mol\) %
which of the following exists as covalent crystals in the solid state?
- (a)
Iodine
- (b)
Silicon
- (c)
Sulphur
- (d)
Phosphorus
Lithium forms body central cubic structure. The length of the side of its unit cell is 351 pm. Atomic radius of lithium will be
- (a)
175 pm
- (b)
300 pm
- (c)
240 pm
- (d)
152 pm
Copper crystallises in fcc lattice with a unit cell edge of 361 pm. The radius of copper atoms is
- (a)
181 pm
- (b)
108 pm
- (c)
128 pm
- (d)
157 pm
Percentage of fee space in cubic close - packed structure and in body-centred packed structure are respectively
- (a)
48% and 26%
- (b)
30% and 26%
- (c)
26% and 32%
- (d)
32% and 48%
In a compound, atoms of element Y form cubical - closest packing and those of elements X occupy 2/3 of tetrahedral voids. The formula of the compound will be
- (a)
\(X_3Y\)
- (b)
\(X_4Y_3\)
- (c)
\(X_2Y_3\)
- (d)
\(X_2Y\)
Total volume of atoms present in a face-centred cubic unit cell of a metal is (r is atomic radius)
- (a)
\(16\over 3\pi r^3\)
- (b)
\({20\over 3}\pi r^3\)
- (c)
\({24\over 3}\pi\ r^3\)
- (d)
\({12\over 3}\pi r^3\)
How many unit cells are present in a cube-shaped ideal crystal of NaCl mass 1.00 g?
- (a)
\(1.71\times 10^{21}\)
- (b)
\(2.57\times 10^{21}\)
- (c)
\(5.14\times 10^{21}\)
- (d)
\(1.28\times 10^{21}\)