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Which of the following statements are correct –

1. CCP structure has three different type of layers.
2. In CCP structure, first and fourth layers are repeated.
3. In an HCP structure, first and fourth layers are repeated.
4. In FCC packing, the neighbouring face centred atoms touch each other.

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Important Questions on Solid State

MEDIUM

Chemistry>Physical Chemistry>Solid State>Calculations for Standard Cubical Unit Lattice

A crystalline solid has

A

-ions at the corners and face centres where as

B^{+}

ions are at the body centre and edge centres of the unit cell. The sim ple formula of the compound will be

MEDIUM

Chemistry>Physical Chemistry>Solid State>Calculations for Standard Cubical Unit Lattice

A compound is formed by atoms

{}^{'}A^{'}

and

{}^{'}B^{'}

B

atoms form

ccp

arrangement. If

A

occupy

\frac{1}{3}

of tetrahedral voids, what is the formula of the compound?

EASY

Chemistry>Physical Chemistry>Solid State>Calculations for Standard Cubical Unit Lattice

In the face centred cubic lattice structure of gold the closest distance between gold atoms is (

{}^{'}a^{'}

being the edge length of the cubic unit cell)

EASY

Chemistry>Physical Chemistry>Solid State>Calculations for Standard Cubical Unit Lattice

A compound made up of atoms of

Y

(anions) forming a CCP arrangement, where the element

X

(cation) occupies octahedral voids. The formula of the compound is

EASY

Chemistry>Physical Chemistry>Solid State>Calculations for Standard Cubical Unit Lattice

Element

B

forms ccp structure and

A

occupies half of the octahedral voids, while oxygen atoms occupy all the tetrahedral voids. The structure of bimetallic oxide is:

HARD

Chemistry>Physical Chemistry>Solid State>Calculations for Standard Cubical Unit Lattice

In a cubic-close packed structure containing

X, Y

and

Z

atoms, if

Z

occupies all the face centres, $\mathrm{X}$ occupies all the corners and

Y

occupies the body centre of the cube, what is the formula of this compound?

MEDIUM

Chemistry>Physical Chemistry>Solid State>Calculations for Standard Cubical Unit Lattice

A compound is formed from elements

X

and

Y

. The atoms of

Y

(anions) form a

ccp

lattice. The atoms of

X

(cations) occupy half of the octahedral voids and half of tetrahedral voids. What is the formula of the compound?

MEDIUM

Chemistry>Physical Chemistry>Solid State>Calculations for Standard Cubical Unit Lattice

The number of atoms in a body centred cubic unit cell of an element is

MEDIUM

Chemistry>Physical Chemistry>Solid State>Calculations for Standard Cubical Unit Lattice

The ratio of number of atoms present in a simple cubic, body centered cubic and face centered cubic structure are, respectively :

MEDIUM

Chemistry>Physical Chemistry>Solid State>Calculations for Standard Cubical Unit Lattice

How many total constituent particles are present in simple cubic unit cell?

EASY

Chemistry>Physical Chemistry>Solid State>Calculations for Standard Cubical Unit Lattice

The cubic unit cell of a metal (molar mass

= 63.55 g {mol}^{- 1}

) has an edge length of

362 pm

. Its density is

8.92 {gcm}^{- 3}

. The type of unit cell is

EASY

Chemistry>Physical Chemistry>Solid State>Calculations for Standard Cubical Unit Lattice

In a cubic close packed structure, fractional contributions of an atom at the corner and at the face in the unit cell are, respectively -

EASY

Chemistry>Physical Chemistry>Solid State>Calculations for Standard Cubical Unit Lattice

The number of atoms per unit cell of body centred cube is:

MEDIUM

Chemistry>Physical Chemistry>Solid State>Calculations for Standard Cubical Unit Lattice

In chrysoberyl, a compound containing Beryllium, Aluminium and oxygen, oxide ions form cubic close packed structure. Aluminium ions occupy

\frac{1}{4} th

of tetrahedral voids and beryllium ions occupy

\frac{1}{4} th

of octahedral voids. The formula of the compound is

EASY

Chemistry>Physical Chemistry>Solid State>Calculations for Standard Cubical Unit Lattice

The total number of atoms per unit cell in BCC is:

MEDIUM

Chemistry>Physical Chemistry>Solid State>Calculations for Standard Cubical Unit Lattice

A compound is formed of two elements 'A' and 'B'. The atoms of element 'A' forms face centered cubic close packing and atoms of 'B' occupies all the tetrahedral voids. What will be the formula of the compound?

MEDIUM

Chemistry>Physical Chemistry>Solid State>Calculations for Standard Cubical Unit Lattice

The total number of particles in a body centred cubic unit cell is

MEDIUM

Chemistry>Physical Chemistry>Solid State>Calculations for Standard Cubical Unit Lattice

A compound is formed by elements of

X, Y

and

Z

. Atoms of

Z

(anions) make

FCC

lattice. Atoms of

X

(cations) occupy all the octahedral voids. Atoms of

Y

(cations) occupy

\frac{1}{3} rd

of the tetrahedral voids. The formula of the compound is:

MEDIUM

Chemistry>Physical Chemistry>Solid State>Calculations for Standard Cubical Unit Lattice

In a face centered cubic lattice atoms A are at the corner points and atoms B at the face centered points. If atom B is missing from one of the face centered points, the formula of the ionic compound is :

MEDIUM

Chemistry>Physical Chemistry>Solid State>Calculations for Standard Cubical Unit Lattice

A mineral consists of a cubic close-packed structure formed by

O^{2 -}

ions where half the octahedral voids are occupied by

A l^{3 +}

and one-eighth of the tetrahedral voids are occupied by

M n^{2 +}

. The chemical formula of the mineral is

Which of the following statements are correct – 1. CCP structure has three different type of layers. 2. In CCP structure, first and fourth layers are repeated. 3. In an HCP structure, first and fourth layers are repeated. 4. In FCC packing, the neighbouring face centred atoms touch each other.

Important Questions on Solid State

Learn and Prepare for any exam you want !

Which of the following statements are correct –

1. CCP structure has three different type of layers.
2. In CCP structure, first and fourth layers are repeated.
3. In an HCP structure, first and fourth layers are repeated.
4. In FCC packing, the neighbouring face centred atoms touch each other.