Solid State · Chemistry · KCET
MCQ (Single Correct Answer)
Which of the following crystals has the unit cell such that $a=b \neq c$ and $\alpha=\beta=90^{\circ}$, $\gamma=120^{\circ}$ ?
The number of atoms in 4.5 g of a face-centred cubic crystal with edge length 300 pm is (Given : Density $=10 \mathrm{~g} \mathrm{~cm}^{-3}$ and $N_A=6.022 \times 10^{23}$)
If '$$a$$' stands for the edge length of the cubic systems. The ratio of radii in simple cubic, body centred cubic and face centred cubic unit cells is
Match the column A (type of crystalline solid) with the column B (example for each type)
| A | B | ||
|---|---|---|---|
| P. | Molecular solid | i. | SiC |
| Q. | Ionic solid | ii. | Mg |
| R. | Metallic solid | iii. | H$$_2$$O |
| S. | Network solid | iv. | MgO |
A metal crystallises in a body centred cubic lattice with the metallic radius $$\sqrt3\mathop A\limits^o $$. The volume of the unit cell in $$\mathrm{m}^3$$ is
In solid state, $$\mathrm{PCl}_5$$ is a/an
Vacant space in body centered cubic lattice unit cell is about
How many number of atoms are there in a cube based unit cell, having one atom on each corner and 2 atoms on each body diagonal of cube?
Which of the following is not true about the amorphous solids?
Alkali halides do not show dislocation defect because
In chrysoberyl, a compound containing beryllium, aluminium and oxygen, oxide ions form cubic close packed structure. Aluminium ions occupy $$\frac{1}{4}$$th of octahedral voids. The formula of the compound is
The correct statement regarding defects in solid is
A metal crystallises in bcc lattice with unit cell edge length of $$300 \mathrm{~pm}$$ and density $$615 \mathrm{~g~cm}^{-3}$$. The molar mass of the metal is
A metal crystallises in face centred cubic structure with metallic radius $$\sqrt{2} \mathop A\limits^o$$. The volume of the unit cell (in $$\mathrm{m}^3$$ ) is
Silicon doped with gallium forms
Which of the following is a network crystalline solid?
The number of atoms in $$2.4 \mathrm{~g}$$ of body centred cubic crystal with edge length $$200 \mathrm{pm}$$ is (density $$=10 \mathrm{~g} \mathrm{~cm}^{-3}, \mathrm{~N}_A=6 \times 10^{23}$$ atoms$$/ \mathrm{mol}$$)
1 mole of $$\mathrm{NaCl}$$ is doped with $$10^{-5}$$ mole of $$\mathrm{SrCl}_2$$. The number of cationic vacancies in the crystal lattice will be