Solid State

In an ionic crystalline solid, atoms of element Y forms hcp structure. The atoms of element X occupy one third of tetrahedral voids. What is the formula of compound?

Calculate the volume of unit cell if an element having molar mass \(56 \mathrm{~g} \mathrm{~mol}^{-1}\) that forms bcc unit cells.
$$\left[\rho \cdot \mathrm{N}_{\mathrm{A}}=4.8 \times 10^{24} \mathrm{~g} \mathrm{~cm}^{-3} \mathrm{~mol}^{-1...

Calculate the density of metal having molar mass \(210 \mathrm{~g} \mathrm{~mol}^{-1}\) that forms simple cubic unit cell. \(\left(\mathrm{a}^3 \cdot \mathrm{N}_{\mathrm{A}}=21.5 \mathrm{~cm}^3 \mathrm{~mol}^{-1}\right)\)

Which from following combinations is an example for construction of n-type semiconductor?

Calculate the edge length of bcc unit cell if radius of metal atom is \(227 \mathrm{~pm}\).

Calculate the number of atoms present in unit cell if an element having molar mass \(23 \mathrm{~g} \mathrm{~mol}^{-1}\) and density \(0.96 \mathrm{~g} \mathrm{~cm}^{-3}\).
$$[\mathrm{a}^3 \cdot \mathrm{N}_{\mathrm{A}}=48 \mathrm{~cm}^3 \ma...

Calculate the radius of metal atom in bcc unit cell having edge length \(287 \mathrm{~pm}\).

Which from following metal has hcp crystal structure?

Calculate the volume of unit cell if an element having molar mass \(180 \mathrm{~g} \mathrm{~mol}^{-1}\) forms fcc unit cell. \(\left[\rho \cdot N_A=120 \times 10^{21} \mathrm{~g} \mathrm{~cm}^{-3} \mathrm{~mol}^{-1}\right]\)

Find the radius of metal atom in bcc unit cell having edge length \(450 \mathrm{~pm}\).

Which statement from following about nano-material is NOT correct?

Identify the good conductor of electricity from following band gap energy values of solids.

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Identify the example of zero-dimensional nanostructure from following.

Calculate the molar mass of an element having density \(7.8 \mathrm{~g} \mathrm{~cm}^{-3}\) that forms bcc unit cell. \(\left[\mathrm{a}^3 \cdot \mathrm{N}_{\mathrm{A}}=16.2 \mathrm{~cm}^3 \mathrm{~mol}^{-1}\right]\)

What are the number of octahedral and tetrahedral voids in 0.3 mole substance respectively if it forms hcp structure?

Calculate the edge length of simple cubic unit cell if radius of an atom is \(167.3 \mathrm{~pm}\).

What type of following solids the ice is

Calculate the density of an element having molar mass \(27 \mathrm{~g} \mathrm{~mol}^{-1}\) that forms fcc unit cell. \(\left[\mathrm{a}^3 \cdot \mathrm{N}_{\mathrm{A}}=38.5 \mathrm{~cm}^3 \mathrm{~mol}^{-1}\right]\)

What is the number of unit cells present in a cubic pack crystal lattice having 4 atoms per unit cell and weighing \(0.60 \mathrm{~g}\) (molar mass \(\left.60 \mathrm{~g} \mathrm{~mol}^{-1}\right)\) ?

What is atomic mass of an element with \(\mathrm{BCC}\) structure and density \(10 \mathrm{~g} \mathrm{~cm}^{-3}\) having edge length \(300 \mathrm{~pm}\) ?

Which formula is used to calculate edge length in bcc structure?

Find the radius of an atom in fcc unit cell having edge length \(405 \mathrm{pm}\).

Calculate the molar mass of metal having density \(9.3 \mathrm{~g} \mathrm{~cm}^{-3}\) that forms simple cubic unit cell. \(\left[\mathrm{a}^3 \cdot \mathrm{N}_{\mathrm{A}}=22.6 \mathrm{~cm}^3 \mathrm{~mol}^{-1}\right]\)

Which from following is NOT an example of amorphous solid?

Calculate the molar mass of an element with density \(2.7 \mathrm{~g} \mathrm{~cm}^{-3}\) that forms fcc structure. \(\left[\mathrm{a}^3 \cdot \mathrm{N}_{\mathrm{A}}=40 \mathrm{~cm}^3 \mathrm{~mol}^{-1}\right]\)

What is the total number of Bravais lattices present for different crystal systems?

Calculate the edge length of unit cell of metal which crystallises to bcc structure.
(Radius of metal atom \(=173 \mathrm{~pm}\) )

Which of the following characteristic properties is NOT true for crystalline solid?

Calculate the number of atoms present in unit cell of an element having molar mass \(190 \mathrm{~g} \mathrm{~mol}^{-1}\) and density \(20 \mathrm{~g} \mathrm{~cm}^{-3}\).
$$\left[\mathrm{a}^3 \cdot \mathrm{N}_{\mathrm{A}}=38 \mathrm{~cm}^3...

Find the radius of an atom in fcc unit cell having edge length \(393 \mathrm{pm}\).

Calculate the density of metal having volume of unit cell \(64 \times 10^{-24} \mathrm{~cm}^3\) and molar mass of metal \(192 \mathrm{~g} \mathrm{~mol}^{-1}\) containing 4 particles in unit cell.

What is the total volume occupied by atoms in bcc unit cell ?

Calculate the number of atoms in 5 gram metal that crystallises to form simple cubic unit cell structure having edge length \(336 \mathrm{~pm}\). (Density of metal \(=9.4 \mathrm{~g} \mathrm{~cm}^{-3}\) )

What is the volume occupied by particles in \(\mathrm{BCC}\) structure if '\(\mathrm{a}\)' is edge length of unit cell?

The FCC unit cell of a compound contains ions of \(\mathrm{A}\) at the corner and ions of \(\mathrm{B}\) at the centre of each face, what is the formula of the compound?

A metal has \(\mathrm{BCC}\) structure with edge length of unit cell \(400 \mathrm{~pm}\). Density or metal is \(4 \mathrm{~g} \mathrm{~cm}^{-3}\). What is molar mass of metal?

Which of the following pairs of compounds is isomorphous?

The density of chromium metal is 7 g cm\(^{-3}\). If edge length of unit cell is 300 pm, identify the type of unit cell. (At mass Cr = 52)

An element has \(\mathrm{BCC}\) structure with edge length of unit cell \(600 \mathrm{~pm}\). What is the atomic radius of element?

An element with BCC structure has edge length of \(500 \mathrm{~pm}\). If it's density is \(4 \mathrm{~g} \mathrm{~cm}^{-3}\), find atomic mass of the element?

How many particles per unit cell are present in \(\mathrm{BCC}\) structure?

What is the atomic radius of polonium if it crystallises in a simple cubic structure with edge length of unit cell \(336 \mathrm{~pm}\) ?

Edge length of unit cell of BCC structure is 352 pm. What is radius of the atom?

For simple cubic crystal edge length is expressed as

An element is found to crystallize with \(\mathrm{BCC}\) structure having density \(8.55 \mathrm{~g} \mathrm{~cm}^{-3}\). What is the edge length of unit cell? (At. mass of element \(=93\))

How many lattice points are present in a face centred cubic unit cell?

What is the molar mass of a metal having density 8.57 g cm\(^{-3}\) and edge length 3.3 \(\mathop A\limits^o\) ? (packing efficiency = 68%)

What is the number of octahedral and tetrahedral voids presents respectively in 0.25 mole of a substance having hcp structure?

Identify the type of unit cell that has particles at the centre of each face in addition to the particles at eight corners of a cube?

How many atoms of niobium are present in \(2.43 \mathrm{~g}\) if it forms bcc structure with density \(9 \mathrm{~g} \mathrm{~cm}^{-3}\) and volume of unit cell \(2.7 \times 10^{-23} \mathrm{~cm}^3\) ?