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The density of iridium is $22.4 g / {cm}^{3}$ . The unit cell of iridium is fcc. Calculate the radius of iridium atom. Molar mass of iridium is $192.2 g / mol . (136 pm)$ .

Important Questions on Solid State

MEDIUM

Chemistry>Physical Chemistry>Solid State>Density of Unit Cells

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})

HARD

Chemistry>Physical Chemistry>Solid State>Density of Unit Cells

An element with molar mass

2 .7 \times 10^{- 2} kg {mol}^{- 1}

forms a cubic unit cell with edge length

405 pm .

If its density is

2.7 \times 10^{3} kg m^{- 3}

, the radius of the element is approximately

\dots \dots \dots . \times 10^{- 12} m

(to the nearest integer)

MEDIUM

Chemistry>Physical Chemistry>Solid State>Density of Unit Cells

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

MEDIUM

Chemistry>Physical Chemistry>Solid State>Density of Unit Cells

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]

HARD

Chemistry>Physical Chemistry>Solid State>Density of Unit Cells

Consider the bcc unit cells of the solids $1$ and $2$ with the position of atoms as shown below. The radius of atom $B$ is twice that of atom $A .$ The unit cell edge length is $50 %$ more in solid $2$ than in $1$ . What is the approximate packing efficiency in solid $2$ ?

Question Image

EASY

Chemistry>Physical Chemistry>Solid State>Density of Unit Cells

The ratio of packing efficiency in

FCC, BCC

and simple cubic structure respectively, with respect to that of

FCC

structures is

MEDIUM

Chemistry>Physical Chemistry>Solid State>Density of Unit Cells

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}

)

HARD

Chemistry>Physical Chemistry>Solid State>Density of Unit Cells

An element has a body centered cubic bcc structure with a cell edge of

288 pm

. The density of the element is

7.2 g / {cm}^{3}

. How many atoms are present in

208 g

of the element?

MEDIUM

Chemistry>Physical Chemistry>Solid State>Density of Unit Cells

The percentage of unoccupied volume in simple cubic cell is

MEDIUM

Chemistry>Physical Chemistry>Solid State>Density of Unit Cells

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}

)

HARD

Chemistry>Physical Chemistry>Solid State>Density of Unit Cells

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

EASY

Chemistry>Physical Chemistry>Solid State>Density of Unit Cells

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

MEDIUM

Chemistry>Physical Chemistry>Solid State>Density of Unit Cells

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}

EASY

Chemistry>Physical Chemistry>Solid State>Density of Unit Cells

The vacant space in bcc lattice unit cell is:

MEDIUM

Chemistry>Physical Chemistry>Solid State>Density of Unit Cells

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>Density of Unit Cells

The unit cell of copper corresponds to a face centered cube of edge length

3.596 Å

with one copper atom at each lattice point. The calculated density of copper in

kg / m^{3}

is ___ . [Molar mass of

Cu : 63.54 g;

Avogadro Number

= 6.022 \times 10^{23} J

]

MEDIUM

Chemistry>Physical Chemistry>Solid State>Density of Unit Cells

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

MEDIUM

Chemistry>Physical Chemistry>Solid State>Density of Unit Cells

The correct order of the packing efficiency in different types of unit cells is

EASY

Chemistry>Physical Chemistry>Solid State>Density of Unit Cells

The packing efficiency of the face centered cubic (FCC), body centered cubic (BCC) and simple/primitive cubic (PC) lattices follows the order

HARD

Chemistry>Physical Chemistry>Solid State>Density of Unit Cells

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})

The density of iridium is 22.4g/cm3. The unit cell of iridium is fcc. Calculate the radius of iridium atom. Molar mass of iridium is 192.2g/mol.(136pm).

Important Questions on Solid State

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The density of iridium is $22.4 g / {cm}^{3}$ . The unit cell of iridium is fcc. Calculate the radius of iridium atom. Molar mass of iridium is $192.2 g / mol . (136 pm)$ .