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An element crystallizes both in fcc and bcc lattice. If the density of the element in the two forms is the same, the ratio of unit cell length of fcc to that of bcc lattice is

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Important Questions on Solid State

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Chemistry>Physical Chemistry>Solid State>Calculation of Density of Unit Cell

If same type of atoms are packed in hexagonal close packing and cubic close packing separately, then

HARD

Chemistry>Physical Chemistry>Solid State>Calculation of Density of Unit Cell

How many number of unit cells are present in

100 g

of an element with FCC crystal having density

10 g / {cm}^{3}

and edge length

100 pm

MEDIUM

Chemistry>Physical Chemistry>Solid State>Calculation of Density of Unit Cell

A metal crystallizes in two phases, one as

fcc

and another as

bcc

with unit cell edge lengths of

3.5 \overset{°}{A}

and

3.0 \overset{°}{A}

, respectively. The ratio of density of

fcc

and

bcc

phases approximately is

MEDIUM

Chemistry>Physical Chemistry>Solid State>Calculation of Density of Unit Cell

Calcium metal crystallizes in an f.c.c. lattice with edge length

0.556 nm

. If it contains

0.5 %

Frenkel defects, the density of the metal is

MEDIUM

Chemistry>Physical Chemistry>Solid State>Calculation of Density of Unit Cell

A diatomic molecule

X_{2}

has a body-centred cubic

(bcc)

structure with a cell edge of

300 pm .

The density of the molecule is

6.17 {gcm}^{- 3} .

The number of molecules present in

200 g

X_{2}

is :
(Avogadro constant

(N_{A}) = 6 \times 10^{23} {mol}^{- 1}

)

EASY

Chemistry>Physical Chemistry>Solid State>Calculation of Density of Unit Cell

An element crystallises in fcc lattice. If edge length of the unit cell is

4.07 \times 10^{- 8} cm

and density is

10.5 g {cm}^{- 3} .

Calculate the atomic mass of element.

MEDIUM

Chemistry>Physical Chemistry>Solid State>Calculation of Density of Unit Cell

Calculate the number of unit cells in

38.6 g

of noble metal having density

19.3 g {cm}^{- 3}

and volume of one unit cell is

6.18 \times 10^{- 23} {cm}^{3}

HARD

Chemistry>Physical Chemistry>Solid State>Calculation of Density of Unit Cell

Iron exhibits BCC structure at room temperature. Above

900^{°} C

, it transforms to FCC structure. The ratio of the density of iron at room temperature to that at

900^{°} C

is (assuming molar mass and atomic radii of iron remains constant with temperature)

HARD

Chemistry>Physical Chemistry>Solid State>Calculation of Density of Unit Cell

Lithium has a bcc structure. Its density is

530 k g m^{- 3}

and its atomic mass is

6.94 g m o l^{- 1}

. Calculated the edge length of a unit cell of Lithium metal.

(N_{A} = 6.02 \times 10^{23} m o l^{- 1})

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Chemistry>Physical Chemistry>Solid State>Calculation of Density of Unit Cell

A metallic element has a cubic lattice. Each edge of the unit cell is

2 \dot{A}

and the density of metal is

25 g {cm}^{3}

. The unit cell in

200 g

of metal are

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Chemistry>Physical Chemistry>Solid State>Calculation of Density of Unit Cell

The edge length of a solid possessing cubic unit cell is $2 \sqrt{2} r$ (structure I), based on hard sphere model, which upon subjecting to a phase transition, a new cubic structure (structure II) having an edge length of $\frac{4 r}{\sqrt{3}}$ is obtained, where $r$ is the radius of the hard sphere. Which of the following statements is true ?

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Chemistry>Physical Chemistry>Solid State>Calculation of Density of Unit Cell

100^{o} C,

copper

(C u)

has

F C C

unit cell structure with cell edge length of

x Å

. What is the approximate density of

C u

(in

g c m^{- 3}

) at this temperature?

[A t o m i c M a s s o f C u = 63.55 u]

EASY

Chemistry>Physical Chemistry>Solid State>Calculation of Density of Unit Cell

A metal crystallises in BCC lattice with unit cell edge length of

300 pm

and density

6.15 {gcm}^{- 3} .

The molar mass of the metal is

EASY

Chemistry>Physical Chemistry>Solid State>Calculation of Density of Unit Cell

Copper crystallises with fcc unit cell. If the radius of copper atom is

127.8 pm,

calculate the density of copper? (at. Mass,

Cu = 63.55 g {mole}^{- 1}

)

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Chemistry>Physical Chemistry>Solid State>Calculation of Density of Unit Cell

Copper crystallizes in an FCC unit cell with cell edge of

3 .608 \times 10^{- 8} cm .

The density of copper is

8.92 g / {cm}^{3}

, Calculate the atomic mass of copper.

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Chemistry>Physical Chemistry>Solid State>Calculation of Density of Unit Cell

Sodium metal crystallizes in a body centred cubic lattice with a unit cell edge of

4.29 Å

. The radius of sodium atom is approximately:

EASY

Chemistry>Physical Chemistry>Solid State>Calculation of Density of Unit Cell

Iron crystallizes in several modifications. At about

911^{o} C

, the bcc

' α'

form undergoes a transition to fcc

' γ'

form. If the distance between two nearest neighbours is the same in the two forms at the transition temperature, what is the ratio of the density of iron in fcc form

(ρ_{2})

to the iron in bcc form

(ρ_{1})

at the transition temperature?

MEDIUM

Chemistry>Physical Chemistry>Solid State>Calculation of Density of Unit Cell

The density of a solid

X

1.5 g / {cm}^{3}

250^{o} C

. If the atoms are assumed sphere of radius

2.0 A

, the percentage of solid having empty space is
(Given atomic weight of

X = 60 g {mol}^{- 1})

MEDIUM

Chemistry>Physical Chemistry>Solid State>Calculation of Density of Unit Cell

The number of atoms in

2.4 g

of body centred cubic crystal with edge length

200 pm

is (density

= 10 g {cm}^{- 3}, N_{A} = 6 \times 10^{23} atoms {mol}^{- 1}

)

EASY

Chemistry>Physical Chemistry>Solid State>Calculation of Density of Unit Cell

Copper

(A t o m i c m a s s = 63.5)

crystallizes in a FCC lattice and has density

8 .93 g . {cm}^{- 3} .

The radius of copper atom is closest to

An element crystallizes both in fcc and bcc lattice. If the density of the element in the two forms is the same, the ratio of unit cell length of fcc to that of bcc lattice is

Important Questions on Solid State

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