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CHXI11:THE P-BLOCK ELEMENTS

316481 Match the Column I with Column II
Column I
Column II
A
Melting point[K]
P
Tl>In>Ga>Al>B
B
Ionic radius $[M^{+ 3} / p m]$
Q
B>Tl>Al $\approx G a > I n$
C
$Δ_{i} H_{i} [k J m o l^{- 1}]$
R
Tl>In>Al>Ga>B
D
Atomic radius[pm]
S
B>Al>Tl>In>Ga

1 A - R,B - S,

C - P, D - Q

2 A - S,B - P,

C - Q

,

D - R

3 A - Q,B - R,

C - S

,D - P

4

A - P

,

B - Q

,

C - R

,D - S

Explanation:

Melting point ( K ):
$\underset{(2453)}{B} > \underset{\underset{}{(933)}}{A l} > \underset{(576)}{T l} > \underset{(430)}{In} > \underset{(303)}{G a} (A - S)$
$I o n i c r a d i u s (M^{3 +} / p m) :$
$\underset{(88.5)}{T l} > \underset{(80)}{I n} > \underset{(62)}{G a} > \underset{(53.5)}{A l} > \underset{(27)}{B} (B - P)$
$Δ_{i} H_{1} (k J / m o l) : \underset{(801)}{B} > \underset{(589)}{T l} > \underset{(579)}{G a} = \underset{(577)}{A l} > \underset{(558)}{I n}$
$(C - Q)$
$A t o m i c r a d i u s (p m) :$
$\underset{(107)}{T I} > \underset{(167)}{I n} > \underset{(143)}{A l} > \underset{(135)}{G a} > \underset{(88)}{B} (D - R)$
So, the correct option is (2)

JEE Main - 2024

CHXI11:THE P-BLOCK ELEMENTS

316482 For the properties mentioned, the correct trend for the different species is in

1 Strength as Lewis acids-

{BCl}_{3} > {AlCl}_{3} > {GaCl}_{3}

2 Inert pair effect

- Al > Ga >

In

3 Oxidising property

- {Al}^{3 +} > {In}^{3 +} > {Tl}^{3 +}

4 First ionization enthalpy

- B > Al > Tl

Explanation:

Strength of Lewis acids decreases in the order ${BCl}_{3} > {AlCl}_{3} > {GaCl}_{3}$ , as boron can accept electron pair easily.
$Al$ does not show inert pair effect.
${Al}^{3 +}$ has the highest oxidising power.
Ionization enthalpy of $Tl$ is higher than that of $Al$ .

CHXI11:THE P-BLOCK ELEMENTS

316483 Both boron and aluminium show difference in properties from the remaining members of group 13. This is because

1 Both B and Al have smaller size as compared to other members of the family

2 Both B and Al have high values of ionization enthalpy

3 Both B and Al have only the valence electrons

(n s^{2} n p^{1})

out side the noble gas core while the remaining elements have filled

d

and f-orbitals in between the noble gas core and the valence electrons

4 None of these

Explanation:

The difference in properties of $B$ and $Al$ from the remaining members of group 13 is due to the difference in their electronic configuration as stated.

CHXI11:THE P-BLOCK ELEMENTS

316484 Which member of group 13 does not exhibit the group valency in its compounds?

1 Boron

2 Aluminium

3 Gallium

4 Thallium

Explanation:

Due to inert pair effect, thallium amongst group 13 elements does not exhibit the group valency $(+ 3)$ in its compounds. It shows +1 oxidation state in its stable compounds.

CHXI11:THE P-BLOCK ELEMENTS

316481 Match the Column I with Column II
Column I
Column II
A
Melting point[K]
P
Tl>In>Ga>Al>B
B
Ionic radius $[M^{+ 3} / p m]$
Q
B>Tl>Al $\approx G a > I n$
C
$Δ_{i} H_{i} [k J m o l^{- 1}]$
R
Tl>In>Al>Ga>B
D
Atomic radius[pm]
S
B>Al>Tl>In>Ga

1 A - R,B - S,

C - P, D - Q

2 A - S,B - P,

C - Q

,

D - R

3 A - Q,B - R,

C - S

,D - P

4

A - P

,

B - Q

,

C - R

,D - S

Explanation:

Melting point ( K ):
$\underset{(2453)}{B} > \underset{\underset{}{(933)}}{A l} > \underset{(576)}{T l} > \underset{(430)}{In} > \underset{(303)}{G a} (A - S)$
$I o n i c r a d i u s (M^{3 +} / p m) :$
$\underset{(88.5)}{T l} > \underset{(80)}{I n} > \underset{(62)}{G a} > \underset{(53.5)}{A l} > \underset{(27)}{B} (B - P)$
$Δ_{i} H_{1} (k J / m o l) : \underset{(801)}{B} > \underset{(589)}{T l} > \underset{(579)}{G a} = \underset{(577)}{A l} > \underset{(558)}{I n}$
$(C - Q)$
$A t o m i c r a d i u s (p m) :$
$\underset{(107)}{T I} > \underset{(167)}{I n} > \underset{(143)}{A l} > \underset{(135)}{G a} > \underset{(88)}{B} (D - R)$
So, the correct option is (2)

JEE Main - 2024

CHXI11:THE P-BLOCK ELEMENTS

316482 For the properties mentioned, the correct trend for the different species is in

1 Strength as Lewis acids-

{BCl}_{3} > {AlCl}_{3} > {GaCl}_{3}

2 Inert pair effect

- Al > Ga >

In

3 Oxidising property

- {Al}^{3 +} > {In}^{3 +} > {Tl}^{3 +}

4 First ionization enthalpy

- B > Al > Tl

Explanation:

Strength of Lewis acids decreases in the order ${BCl}_{3} > {AlCl}_{3} > {GaCl}_{3}$ , as boron can accept electron pair easily.
$Al$ does not show inert pair effect.
${Al}^{3 +}$ has the highest oxidising power.
Ionization enthalpy of $Tl$ is higher than that of $Al$ .

CHXI11:THE P-BLOCK ELEMENTS

316483 Both boron and aluminium show difference in properties from the remaining members of group 13. This is because

1 Both B and Al have smaller size as compared to other members of the family

2 Both B and Al have high values of ionization enthalpy

3 Both B and Al have only the valence electrons

(n s^{2} n p^{1})

out side the noble gas core while the remaining elements have filled

d

and f-orbitals in between the noble gas core and the valence electrons

4 None of these

Explanation:

The difference in properties of $B$ and $Al$ from the remaining members of group 13 is due to the difference in their electronic configuration as stated.

CHXI11:THE P-BLOCK ELEMENTS

316484 Which member of group 13 does not exhibit the group valency in its compounds?

1 Boron

2 Aluminium

3 Gallium

4 Thallium

Explanation:

Due to inert pair effect, thallium amongst group 13 elements does not exhibit the group valency $(+ 3)$ in its compounds. It shows +1 oxidation state in its stable compounds.

CHXI11:THE P-BLOCK ELEMENTS

316481 Match the Column I with Column II
Column I
Column II
A
Melting point[K]
P
Tl>In>Ga>Al>B
B
Ionic radius $[M^{+ 3} / p m]$
Q
B>Tl>Al $\approx G a > I n$
C
$Δ_{i} H_{i} [k J m o l^{- 1}]$
R
Tl>In>Al>Ga>B
D
Atomic radius[pm]
S
B>Al>Tl>In>Ga

1 A - R,B - S,

C - P, D - Q

2 A - S,B - P,

C - Q

,

D - R

3 A - Q,B - R,

C - S

,D - P

4

A - P

,

B - Q

,

C - R

,D - S

Explanation:

Melting point ( K ):
$\underset{(2453)}{B} > \underset{\underset{}{(933)}}{A l} > \underset{(576)}{T l} > \underset{(430)}{In} > \underset{(303)}{G a} (A - S)$
$I o n i c r a d i u s (M^{3 +} / p m) :$
$\underset{(88.5)}{T l} > \underset{(80)}{I n} > \underset{(62)}{G a} > \underset{(53.5)}{A l} > \underset{(27)}{B} (B - P)$
$Δ_{i} H_{1} (k J / m o l) : \underset{(801)}{B} > \underset{(589)}{T l} > \underset{(579)}{G a} = \underset{(577)}{A l} > \underset{(558)}{I n}$
$(C - Q)$
$A t o m i c r a d i u s (p m) :$
$\underset{(107)}{T I} > \underset{(167)}{I n} > \underset{(143)}{A l} > \underset{(135)}{G a} > \underset{(88)}{B} (D - R)$
So, the correct option is (2)

JEE Main - 2024

CHXI11:THE P-BLOCK ELEMENTS

316482 For the properties mentioned, the correct trend for the different species is in

1 Strength as Lewis acids-

{BCl}_{3} > {AlCl}_{3} > {GaCl}_{3}

2 Inert pair effect

- Al > Ga >

In

3 Oxidising property

- {Al}^{3 +} > {In}^{3 +} > {Tl}^{3 +}

4 First ionization enthalpy

- B > Al > Tl

Explanation:

Strength of Lewis acids decreases in the order ${BCl}_{3} > {AlCl}_{3} > {GaCl}_{3}$ , as boron can accept electron pair easily.
$Al$ does not show inert pair effect.
${Al}^{3 +}$ has the highest oxidising power.
Ionization enthalpy of $Tl$ is higher than that of $Al$ .

CHXI11:THE P-BLOCK ELEMENTS

316483 Both boron and aluminium show difference in properties from the remaining members of group 13. This is because

1 Both B and Al have smaller size as compared to other members of the family

2 Both B and Al have high values of ionization enthalpy

3 Both B and Al have only the valence electrons

(n s^{2} n p^{1})

out side the noble gas core while the remaining elements have filled

d

and f-orbitals in between the noble gas core and the valence electrons

4 None of these

Explanation:

The difference in properties of $B$ and $Al$ from the remaining members of group 13 is due to the difference in their electronic configuration as stated.

CHXI11:THE P-BLOCK ELEMENTS

316484 Which member of group 13 does not exhibit the group valency in its compounds?

1 Boron

2 Aluminium

3 Gallium

4 Thallium

Explanation:

Due to inert pair effect, thallium amongst group 13 elements does not exhibit the group valency $(+ 3)$ in its compounds. It shows +1 oxidation state in its stable compounds.

CHXI11:THE P-BLOCK ELEMENTS

316481 Match the Column I with Column II
Column I
Column II
A
Melting point[K]
P
Tl>In>Ga>Al>B
B
Ionic radius $[M^{+ 3} / p m]$
Q
B>Tl>Al $\approx G a > I n$
C
$Δ_{i} H_{i} [k J m o l^{- 1}]$
R
Tl>In>Al>Ga>B
D
Atomic radius[pm]
S
B>Al>Tl>In>Ga

1 A - R,B - S,

C - P, D - Q

2 A - S,B - P,

C - Q

,

D - R

3 A - Q,B - R,

C - S

,D - P

4

A - P

,

B - Q

,

C - R

,D - S

Explanation:

Melting point ( K ):
$\underset{(2453)}{B} > \underset{\underset{}{(933)}}{A l} > \underset{(576)}{T l} > \underset{(430)}{In} > \underset{(303)}{G a} (A - S)$
$I o n i c r a d i u s (M^{3 +} / p m) :$
$\underset{(88.5)}{T l} > \underset{(80)}{I n} > \underset{(62)}{G a} > \underset{(53.5)}{A l} > \underset{(27)}{B} (B - P)$
$Δ_{i} H_{1} (k J / m o l) : \underset{(801)}{B} > \underset{(589)}{T l} > \underset{(579)}{G a} = \underset{(577)}{A l} > \underset{(558)}{I n}$
$(C - Q)$
$A t o m i c r a d i u s (p m) :$
$\underset{(107)}{T I} > \underset{(167)}{I n} > \underset{(143)}{A l} > \underset{(135)}{G a} > \underset{(88)}{B} (D - R)$
So, the correct option is (2)

JEE Main - 2024

CHXI11:THE P-BLOCK ELEMENTS

316482 For the properties mentioned, the correct trend for the different species is in

1 Strength as Lewis acids-

{BCl}_{3} > {AlCl}_{3} > {GaCl}_{3}

2 Inert pair effect

- Al > Ga >

In

3 Oxidising property

- {Al}^{3 +} > {In}^{3 +} > {Tl}^{3 +}

4 First ionization enthalpy

- B > Al > Tl

Explanation:

Strength of Lewis acids decreases in the order ${BCl}_{3} > {AlCl}_{3} > {GaCl}_{3}$ , as boron can accept electron pair easily.
$Al$ does not show inert pair effect.
${Al}^{3 +}$ has the highest oxidising power.
Ionization enthalpy of $Tl$ is higher than that of $Al$ .

CHXI11:THE P-BLOCK ELEMENTS

316483 Both boron and aluminium show difference in properties from the remaining members of group 13. This is because

1 Both B and Al have smaller size as compared to other members of the family

2 Both B and Al have high values of ionization enthalpy

3 Both B and Al have only the valence electrons

(n s^{2} n p^{1})

out side the noble gas core while the remaining elements have filled

d

and f-orbitals in between the noble gas core and the valence electrons

4 None of these

Explanation:

The difference in properties of $B$ and $Al$ from the remaining members of group 13 is due to the difference in their electronic configuration as stated.

CHXI11:THE P-BLOCK ELEMENTS

316484 Which member of group 13 does not exhibit the group valency in its compounds?

1 Boron

2 Aluminium

3 Gallium

4 Thallium

Explanation:

Due to inert pair effect, thallium amongst group 13 elements does not exhibit the group valency $(+ 3)$ in its compounds. It shows +1 oxidation state in its stable compounds.