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CHXII01:THE SOLID STATE

318951 In the lattice of $NaCl$ structure, if the diameter of ${Na}^{+}$ ions is $x$ and the radius of ${Cl}^{-}$ ions is $y$ , then edge length of $NaCl$ in the crystal is

1

x + y

2

x + 2 y

3

2 x + 2 y

4

2 x + y

Explanation:

Edge length of $NaCl = 2 (r_{{Na}^{+}} + r_{Cl})$
$= 2 (\frac{x}{2} + y) = x + 2 y$

CHXII01:THE SOLID STATE

318952 Volume occupied by single $CsCl$ ion pair in a crystal is $7.014 \times 10^{- 23} {cm}^{3}$ . The smallest Cs Cs internuclear distance is equal to length of the side of the cube corresponding to volume of one $CsCl$ ion pair. The smallest $Cs$ to $Cs$ internuclear distance is nearly

1

4 .4 \overset{^{\circ}}{A}

2

4 .3 \overset{^{\circ}}{A}

3

4 \overset{^{\circ}}{A}

4

4 .5 \overset{^{\circ}}{A}

Explanation:

Volume of $CsCl = a^{3}$
$\begin{array}{r} 7.014 \times 10^{- 23} {cm}^{3} = a^{3} (a = edge length) \\ a = \sqrt[3]{7.014 \times 10^{- 23}} \\ a = 4.12 \times 10^{- 8} cm = 4.12 \overset{\circ}{A} = 4 \overset{\circ}{A} \end{array}$

KCET - 2014

CHXII01:THE SOLID STATE

318953 Which of the following is the incorrect statement?

1

NaCl

has

6 : 6

coordination and

CsCl

has

8 : 8

coordination

2 In

{Na}_{2} O

each oxide ion is coordinated by

8 {Na}^{+}

ions and each

{Na}^{+}

ion by 4 oxide ions

3

NaCl

structure transform to

CsCl

structure on heating

4

NaCl

is subjected to high pressure, it transforms into

CsCl

CHXII01:THE SOLID STATE

318954 The melting point of $RbBr$ is $682^{\circ} C$ while that of $NaF$ is $988^{\circ} C$ . The principal reason that melting point of $NaF$ is much higher than that of $RbBr$ is that

1 The bond in

RbBr

has more covalent character than the bond in

NaF

2 The two crystals are not isomorphous

3 The internuclear distance

r_{c} + r_{a}

is greater for

RbBr

than for

NaF

4 The molar mass of NaF is smaller than that of

RbBr

Explanation:

$r_{c} + r_{a}$ is greater for $RbBr$ than for $NaF$ . Hence, bond in $NaF$ is stronger.

CHXII01:THE SOLID STATE

318955 In the crystals of which of the following ionic compounds would you except maximum distance between the centres of the cations and anions?

1 LiI

2

LiF

3 CsI

4

CsF

Explanation:

${Cs}^{+}$ and $I^{-}$ are largest ions.

CHXII01:THE SOLID STATE

318951 In the lattice of $NaCl$ structure, if the diameter of ${Na}^{+}$ ions is $x$ and the radius of ${Cl}^{-}$ ions is $y$ , then edge length of $NaCl$ in the crystal is

1

x + y

2

x + 2 y

3

2 x + 2 y

4

2 x + y

Explanation:

Edge length of $NaCl = 2 (r_{{Na}^{+}} + r_{Cl})$
$= 2 (\frac{x}{2} + y) = x + 2 y$

CHXII01:THE SOLID STATE

318952 Volume occupied by single $CsCl$ ion pair in a crystal is $7.014 \times 10^{- 23} {cm}^{3}$ . The smallest Cs Cs internuclear distance is equal to length of the side of the cube corresponding to volume of one $CsCl$ ion pair. The smallest $Cs$ to $Cs$ internuclear distance is nearly

1

4 .4 \overset{^{\circ}}{A}

2

4 .3 \overset{^{\circ}}{A}

3

4 \overset{^{\circ}}{A}

4

4 .5 \overset{^{\circ}}{A}

Explanation:

Volume of $CsCl = a^{3}$
$\begin{array}{r} 7.014 \times 10^{- 23} {cm}^{3} = a^{3} (a = edge length) \\ a = \sqrt[3]{7.014 \times 10^{- 23}} \\ a = 4.12 \times 10^{- 8} cm = 4.12 \overset{\circ}{A} = 4 \overset{\circ}{A} \end{array}$

KCET - 2014

CHXII01:THE SOLID STATE

318953 Which of the following is the incorrect statement?

1

NaCl

has

6 : 6

coordination and

CsCl

has

8 : 8

coordination

2 In

{Na}_{2} O

each oxide ion is coordinated by

8 {Na}^{+}

ions and each

{Na}^{+}

ion by 4 oxide ions

3

NaCl

structure transform to

CsCl

structure on heating

4

NaCl

is subjected to high pressure, it transforms into

CsCl

CHXII01:THE SOLID STATE

318954 The melting point of $RbBr$ is $682^{\circ} C$ while that of $NaF$ is $988^{\circ} C$ . The principal reason that melting point of $NaF$ is much higher than that of $RbBr$ is that

1 The bond in

RbBr

has more covalent character than the bond in

NaF

2 The two crystals are not isomorphous

3 The internuclear distance

r_{c} + r_{a}

is greater for

RbBr

than for

NaF

4 The molar mass of NaF is smaller than that of

RbBr

Explanation:

$r_{c} + r_{a}$ is greater for $RbBr$ than for $NaF$ . Hence, bond in $NaF$ is stronger.

CHXII01:THE SOLID STATE

318955 In the crystals of which of the following ionic compounds would you except maximum distance between the centres of the cations and anions?

1 LiI

2

LiF

3 CsI

4

CsF

Explanation:

${Cs}^{+}$ and $I^{-}$ are largest ions.

CHXII01:THE SOLID STATE

318951 In the lattice of $NaCl$ structure, if the diameter of ${Na}^{+}$ ions is $x$ and the radius of ${Cl}^{-}$ ions is $y$ , then edge length of $NaCl$ in the crystal is

1

x + y

2

x + 2 y

3

2 x + 2 y

4

2 x + y

Explanation:

Edge length of $NaCl = 2 (r_{{Na}^{+}} + r_{Cl})$
$= 2 (\frac{x}{2} + y) = x + 2 y$

CHXII01:THE SOLID STATE

318952 Volume occupied by single $CsCl$ ion pair in a crystal is $7.014 \times 10^{- 23} {cm}^{3}$ . The smallest Cs Cs internuclear distance is equal to length of the side of the cube corresponding to volume of one $CsCl$ ion pair. The smallest $Cs$ to $Cs$ internuclear distance is nearly

1

4 .4 \overset{^{\circ}}{A}

2

4 .3 \overset{^{\circ}}{A}

3

4 \overset{^{\circ}}{A}

4

4 .5 \overset{^{\circ}}{A}

Explanation:

Volume of $CsCl = a^{3}$
$\begin{array}{r} 7.014 \times 10^{- 23} {cm}^{3} = a^{3} (a = edge length) \\ a = \sqrt[3]{7.014 \times 10^{- 23}} \\ a = 4.12 \times 10^{- 8} cm = 4.12 \overset{\circ}{A} = 4 \overset{\circ}{A} \end{array}$

KCET - 2014

CHXII01:THE SOLID STATE

318953 Which of the following is the incorrect statement?

1

NaCl

has

6 : 6

coordination and

CsCl

has

8 : 8

coordination

2 In

{Na}_{2} O

each oxide ion is coordinated by

8 {Na}^{+}

ions and each

{Na}^{+}

ion by 4 oxide ions

3

NaCl

structure transform to

CsCl

structure on heating

4

NaCl

is subjected to high pressure, it transforms into

CsCl

CHXII01:THE SOLID STATE

318954 The melting point of $RbBr$ is $682^{\circ} C$ while that of $NaF$ is $988^{\circ} C$ . The principal reason that melting point of $NaF$ is much higher than that of $RbBr$ is that

1 The bond in

RbBr

has more covalent character than the bond in

NaF

2 The two crystals are not isomorphous

3 The internuclear distance

r_{c} + r_{a}

is greater for

RbBr

than for

NaF

4 The molar mass of NaF is smaller than that of

RbBr

Explanation:

$r_{c} + r_{a}$ is greater for $RbBr$ than for $NaF$ . Hence, bond in $NaF$ is stronger.

CHXII01:THE SOLID STATE

318955 In the crystals of which of the following ionic compounds would you except maximum distance between the centres of the cations and anions?

1 LiI

2

LiF

3 CsI

4

CsF

Explanation:

${Cs}^{+}$ and $I^{-}$ are largest ions.

CHXII01:THE SOLID STATE

318951 In the lattice of $NaCl$ structure, if the diameter of ${Na}^{+}$ ions is $x$ and the radius of ${Cl}^{-}$ ions is $y$ , then edge length of $NaCl$ in the crystal is

1

x + y

2

x + 2 y

3

2 x + 2 y

4

2 x + y

Explanation:

Edge length of $NaCl = 2 (r_{{Na}^{+}} + r_{Cl})$
$= 2 (\frac{x}{2} + y) = x + 2 y$

CHXII01:THE SOLID STATE

318952 Volume occupied by single $CsCl$ ion pair in a crystal is $7.014 \times 10^{- 23} {cm}^{3}$ . The smallest Cs Cs internuclear distance is equal to length of the side of the cube corresponding to volume of one $CsCl$ ion pair. The smallest $Cs$ to $Cs$ internuclear distance is nearly

1

4 .4 \overset{^{\circ}}{A}

2

4 .3 \overset{^{\circ}}{A}

3

4 \overset{^{\circ}}{A}

4

4 .5 \overset{^{\circ}}{A}

Explanation:

Volume of $CsCl = a^{3}$
$\begin{array}{r} 7.014 \times 10^{- 23} {cm}^{3} = a^{3} (a = edge length) \\ a = \sqrt[3]{7.014 \times 10^{- 23}} \\ a = 4.12 \times 10^{- 8} cm = 4.12 \overset{\circ}{A} = 4 \overset{\circ}{A} \end{array}$

KCET - 2014

CHXII01:THE SOLID STATE

318953 Which of the following is the incorrect statement?

1

NaCl

has

6 : 6

coordination and

CsCl

has

8 : 8

coordination

2 In

{Na}_{2} O

each oxide ion is coordinated by

8 {Na}^{+}

ions and each

{Na}^{+}

ion by 4 oxide ions

3

NaCl

structure transform to

CsCl

structure on heating

4

NaCl

is subjected to high pressure, it transforms into

CsCl

CHXII01:THE SOLID STATE

318954 The melting point of $RbBr$ is $682^{\circ} C$ while that of $NaF$ is $988^{\circ} C$ . The principal reason that melting point of $NaF$ is much higher than that of $RbBr$ is that

1 The bond in

RbBr

has more covalent character than the bond in

NaF

2 The two crystals are not isomorphous

3 The internuclear distance

r_{c} + r_{a}

is greater for

RbBr

than for

NaF

4 The molar mass of NaF is smaller than that of

RbBr

Explanation:

$r_{c} + r_{a}$ is greater for $RbBr$ than for $NaF$ . Hence, bond in $NaF$ is stronger.

CHXII01:THE SOLID STATE

318955 In the crystals of which of the following ionic compounds would you except maximum distance between the centres of the cations and anions?

1 LiI

2

LiF

3 CsI

4

CsF

Explanation:

${Cs}^{+}$ and $I^{-}$ are largest ions.

CHXII01:THE SOLID STATE

318951 In the lattice of $NaCl$ structure, if the diameter of ${Na}^{+}$ ions is $x$ and the radius of ${Cl}^{-}$ ions is $y$ , then edge length of $NaCl$ in the crystal is

1

x + y

2

x + 2 y

3

2 x + 2 y

4

2 x + y

Explanation:

Edge length of $NaCl = 2 (r_{{Na}^{+}} + r_{Cl})$
$= 2 (\frac{x}{2} + y) = x + 2 y$

CHXII01:THE SOLID STATE

318952 Volume occupied by single $CsCl$ ion pair in a crystal is $7.014 \times 10^{- 23} {cm}^{3}$ . The smallest Cs Cs internuclear distance is equal to length of the side of the cube corresponding to volume of one $CsCl$ ion pair. The smallest $Cs$ to $Cs$ internuclear distance is nearly

1

4 .4 \overset{^{\circ}}{A}

2

4 .3 \overset{^{\circ}}{A}

3

4 \overset{^{\circ}}{A}

4

4 .5 \overset{^{\circ}}{A}

Explanation:

Volume of $CsCl = a^{3}$
$\begin{array}{r} 7.014 \times 10^{- 23} {cm}^{3} = a^{3} (a = edge length) \\ a = \sqrt[3]{7.014 \times 10^{- 23}} \\ a = 4.12 \times 10^{- 8} cm = 4.12 \overset{\circ}{A} = 4 \overset{\circ}{A} \end{array}$

KCET - 2014

CHXII01:THE SOLID STATE

318953 Which of the following is the incorrect statement?

1

NaCl

has

6 : 6

coordination and

CsCl

has

8 : 8

coordination

2 In

{Na}_{2} O

each oxide ion is coordinated by

8 {Na}^{+}

ions and each

{Na}^{+}

ion by 4 oxide ions

3

NaCl

structure transform to

CsCl

structure on heating

4

NaCl

is subjected to high pressure, it transforms into

CsCl

CHXII01:THE SOLID STATE

318954 The melting point of $RbBr$ is $682^{\circ} C$ while that of $NaF$ is $988^{\circ} C$ . The principal reason that melting point of $NaF$ is much higher than that of $RbBr$ is that

1 The bond in

RbBr

has more covalent character than the bond in

NaF

2 The two crystals are not isomorphous

3 The internuclear distance

r_{c} + r_{a}

is greater for

RbBr

than for

NaF

4 The molar mass of NaF is smaller than that of

RbBr

Explanation:

$r_{c} + r_{a}$ is greater for $RbBr$ than for $NaF$ . Hence, bond in $NaF$ is stronger.

CHXII01:THE SOLID STATE

318955 In the crystals of which of the following ionic compounds would you except maximum distance between the centres of the cations and anions?

1 LiI

2

LiF

3 CsI

4

CsF

Explanation:

${Cs}^{+}$ and $I^{-}$ are largest ions.