Solid State

In an ionic solid anions are arranged in hcp array and cations occupy $\frac{2}{3}$ of octahedral voids.
What is the formula of ionic compound? [consider $\mathrm{A}=$ cation; $\mathrm{B}=$ anion]

Calculate the edge length of bcc unit cell if radius of a particle present in it is 186 pm .

The compound forming ccp structure contains $9.6 \times 10^{23}$ atoms. Find the number of tetrahedral voids formed in it.

What is the coordination number of a particle in simple cubic close packed structure?

The attractive interactions between cations and mobile electrons in metallic solid is called

Calculate the radius of an atom of an element in pm if it forms bcc unit cell structure having edge length $4.3 \times 10^{-8} \mathrm{~cm}$.

Calculate the number of unit cells in $1 \mathrm{~cm}^3$ of an element if unit cell edge length is $2.0 \times 10^{-8} \mathrm{~cm}$.

Calculate the edge length of unit cell if a metal with atomic radius 128 pm forming fcc unit cell structure.

Calculate the number of particles present per unit cell if mass of a particle is $8.0 \times 10^{-23} \mathrm{~g} \left[\rho \times a^3=3.2 \times 10^{-22} \mathrm{~g}\right]$

Which of the following dopant is used in silicon to produce p-type semiconductor?

Calculate the total volume occupied by all particles in fcc unit cell if volume of unit cell is $6.4 \times 10^{-23} \mathrm{~cm}^3$

What is the total number of unit cells shared by each corner particle of bcc unit cell?

Calculate the number of unit cells in $1 \mathrm{~cm}^3$ volume of metal if unit cell edge length is $1.25 \times 10^{-8} \mathrm{~cm}$.

Calculate the volume occupied by all particles in bcc unit cell if the volume of unit cell is $8.0 \times 10^{-23} \mathrm{~cm}^3$.

Calculate the number of atoms in 1 g metal if it forms fcc crystal structure.
$\left[\rho \times \mathrm{a}^3=1.728 \times 10^{-22} \mathrm{~g}\right]$

Which from following pair of compounds exhibits isomorphism?

Which from following is nonconductor of electricity?

Calculate the number of unit cells in 0.79 g metal if product of density and volume of unit cell is $1.58 \times 10^{-22} \mathrm{~g}$.

Calculate the volume of bcc unit cell if radius of an atom present in it is $1.86 \times 10^{-3} \mathrm{~cm}$.

Calculate the volume occupied by all particles in fcc unit cell if volume of unit cell is $1.6 \times 10^{-23} \mathrm{~cm}^3$.

Which from following dopants is used in germanium to produce p-type semiconductor?

Calculate the number of unit cell in $1 \mathrm{~cm}^3$ volume of metal if volume of unit cell is $3.448 \times 10^{-23} \mathrm{~cm}^3$

Calculate the number of atoms present in 1 g of an element if it forms fcc unit cell structure. $\left[\rho \times \mathrm{a}^3=6.8 \times 10^{-22} \mathrm{~g}\right]$

Identify the type of defect in brass alloy.

Calculate the volume occupied by a particle in fcc unit cell if volume of unit cell is $1.6 \times 10^{-23} \mathrm{~cm}^3$.

Identify the defect that develops when the ratio of number of cations to anions become different from that indicated by its chemical formula.

The mass of an atom present in unit cell is $4.4 \times 10^{-23} \mathrm{~g}$ and the product of density and volume of unit cell is $1.792 \times 10^{-22} \mathrm{~g}$. What is the type of cubic unit cell?

Calculate the total number of tetrahedral and octahedral voids in 0.4 mol compound having such voids in it.

Calculate the number of atoms present per unit cell if product of density and volume of unit cell is $1.8 \times 10^{-22} \mathrm{~g}$.
[Mass of an atom $=4.5 \times 10^{-23} \mathrm{~g}$ ]

Identify the defect developed when an ion of an ionic compound is missing from its regular site and occupies interstitial position between lattice points.

Calculate the volume of fcc unit cell in $\mathrm{cm}^3$ if void volume of it is $4.16 \times 10^{-24} \mathrm{~cm}^3$.

Identify the type of defect from following in stainless steel.

Calculate the molar mass of an element if it forms fcc unit cell structure [mass of unit cell $=1.8 \times 10^{-22} \mathrm{~g}, \mathrm{~N}_{\mathrm{A}}=6.022 \times 10^{23} \mathrm{~mol}^{-1}$ ]

Calculate the total number of tetrahedral and octahedral voids formed in 0.6 mol of a compound if it forms hcp structure.

Calculate the volume occupied by a particle in bcc unit cell if the volume of unit cell is $8.2 \times 10^{-23} \mathrm{~cm}^3$.

Which of the following dopants is used in germanium to form n-type semiconductor?

Calculate the number of unit cells in $1 \mathrm{~cm}^3$ volume of an element if unit cell edge length is $4.0 \times 10^{-8} \mathrm{~cm}$.

Calculate the number of atoms present in 1.58 g metal if it forms bcc structure.
\(\left[\rho \times \mathrm{a}^3=1.58 \times 10^{-22} \mathrm{~g}\right]\)

Which from following solids is isotropic?

Calculate the volume of unit cell having atomic radius 141.4 pm forming fcc unit cell.

Which of the following statements is NOT correct regarding voids in lattice structure?

In ionic solid, anions are arranged in ccp array and cations occupy $1 / 3$ tetrahedral voids. What is the formula of ionic compound?
[Consider $\mathrm{A}=$ cation; $\mathrm{B}=$ anion]

The volume of simple unit cell is $x \times 10^{-23} \mathrm{~cm}^3$. Calculate the value of $x$ if volume occupied by a particle in it is $2.1 \times 10^{-23} \mathrm{~cm}^3$.

What is the relation between edge length and total volume occupied by atoms in bec unit cell?

What is the total number of atoms present in fcc unit cell?

Calculate the volume of unit cell when metal having density $1 \mathrm{~g} \mathrm{~cm}^{-3}$ and molar mass $23 \mathrm{~g} \mathrm{~mol}^{-1}$ crystallises to form bec structure.

What is the coordination number of a particle in fcc structure?

Calculate the molar mass of an element having density $5.6 \mathrm{~g} \mathrm{~cm}^{-3}$ that forms bcc structure $\left[\mathrm{a}^3 \times \mathrm{N}_{\mathrm{A}}=75 \mathrm{~cm}^3 \mathrm{~mol}^{-1}\right]$

Calculate the volume of fcc unit cell if radius of a particle in it is 106.05 pm.

Calculate molar mass of an element having density $8.6 \mathrm{~g} \mathrm{~cm}^{-3}$ if it forms bec structure $\left[\mathrm{a}^3 \times \mathrm{N}_{\mathrm{A}}=22.0 \mathrm{~cm}^3 \mathrm{~mol}^{-1}\right]$