The unit cell of an element of atomic mass 96, and density 10.3 g cm^–3 is a cube with edge length of 314 pm. Find the structure of crystal lattice (simple cubic, F.C.C. or B.C.C.) Avogadro’s constant. N_A = 6.023 x 10²³ mol^–1?

Solution

solution:
we have given

Density of element, $ρ = 10.3 g {cm}^{- 3}$
Cell edge a= 314pm or 3.14 x 10^-10 cm

$N_{A} = 6.023 \times 10^{23} {mol}^{- 1}$

Atomic mass $= 96 g {mol}^{- 1}$

$P = \frac{Z \times M}{a^{3} \times N_{A}} Z = \frac{P \times a^{3} \times N_{A}}{M}$

$= \frac{10 . g {cm}^{- 3} \times (3.14)^{3} \times 10^{- 30} {cm}^{3} \times 6.023 \times 10^{23} {mol}^{- 1}}{96 g {mol}^{- 1}} = 2$

The structure of the crystal lattice is B.C.C.

Some More Questions From The Solid State Chapter

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The Solid State

The unit cell of an element of atomic mass 96, and density 10.3 g cm^–3 is a cube with edge length of 314 pm. Find the structure of crystal lattice (simple cubic, F.C.C. or B.C.C.) Avogadro’s constant. N_A = 6.023 x 10²³ mol^–1?

Some More Questions From The Solid State Chapter

Classify the following as amorphous or crystalline solids: Polyurethane, naphthalene, benzoic acid, teflon, potassium nitrate, cellophane, polyvinyl chloride, fibre glass, copper.

Why is glass considred a super-cooled liquid?

Refractive index of a solid is observed to have the same value along all directions. Comment on the nature of this solid. Would it show clevage property?

Classify the following solids in different categories based on the nature of intermolecular forces operating in them:
Potassium sulphate, tin, benzene, urea, ammonia, water, zinc
sulphate, graphite, rubidium, argon, silicon carbide.

Solid A is a very hard, electrical insulator in solid as well as in molten state and melts at extremely high temperature. What type of solid is it?

Ionic solids conduct electricity in liquid state but not in solid state. Explain.

What type of solids are electrical conductors, malleable and ductile?

Give the significance of a 'lattice point'.

Name the parameters that characterize a unit cell.

Distinguish between Hexagonal and monoclinic unit cells.

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For Daily Free Study Material Join wiredfaculty

The Solid State

The unit cell of an element of atomic mass 96, and density 10.3 g cm–3 is a cube with edge length of 314 pm. Find the structure of crystal lattice (simple cubic, F.C.C. or B.C.C.) Avogadro’s constant. NA = 6.023 x 1023 mol–1?

Some More Questions From The Solid State Chapter

Classify the following as amorphous or crystalline solids: Polyurethane, naphthalene, benzoic acid, teflon, potassium nitrate, cellophane, polyvinyl chloride, fibre glass, copper.

Why is glass considred a super-cooled liquid?

Refractive index of a solid is observed to have the same value along all directions. Comment on the nature of this solid. Would it show clevage property?

Classify the following solids in different categories based on the nature of intermolecular forces operating in them: Potassium sulphate, tin, benzene, urea, ammonia, water, zinc sulphate, graphite, rubidium, argon, silicon carbide.

Solid A is a very hard, electrical insulator in solid as well as in molten state and melts at extremely high temperature. What type of solid is it?

Ionic solids conduct electricity in liquid state but not in solid state. Explain.

What type of solids are electrical conductors, malleable and ductile?

Give the significance of a 'lattice point'.

Name the parameters that characterize a unit cell.

Distinguish between Hexagonal and monoclinic unit cells.

Mock Test Series

NCERT Sample Papers

Entrance Exams Preparation

The unit cell of an element of atomic mass 96, and density 10.3 g cm^–3 is a cube with edge length of 314 pm. Find the structure of crystal lattice (simple cubic, F.C.C. or B.C.C.) Avogadro’s constant. N_A = 6.023 x 10²³ mol^–1?

Classify the following solids in different categories based on the nature of intermolecular forces operating in them:
Potassium sulphate, tin, benzene, urea, ammonia, water, zinc
sulphate, graphite, rubidium, argon, silicon carbide.