Which of the following options are incorrect in accordance with the mentioned properties?

$I) | I P_{1} of ion M^{2 +} | > | E A_{1} o f M^{3 +} |$
$(IP = ionization potential, and EA = electron affinity)$

$I I) S > S e > T e > O (order of EA)$

$I I I) L i < B e < B < C (order of electronegativity)$

$I V) A l^{3 +} < M g^{2 +} < N a^{+} < F^{-} (order of ionic size)$

$V) L i^{+} > N a^{+} < K^{+} (order of hydrated size)$

$V I) N a C l > M g C l_{2} > A l C l_{3} (order of lattice energy)$

(i) and (v)

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(i), (v) and (ii)

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(i), (v), and (vi)

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(i) and (iii)

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Solution

The correct option is C (i), (v), and (vi)
$I) I P_{1} o f i o n M^{2 +} = E A_{1} o f M^{3 +}$
$(IP = ionization potential, and EA = electron affinity)$
$I) I P_{1} o f i o n M^{2 +}$ is the reverse of $E A_{1} o f M^{3 +}$

$I I) S > S e > T e > O (order of EA)$
Due to the small size oxygen has the poorest EA in the group

$I I I) L i < B e < B < C (order of electronegativity)$
As we move from left to rigth electronegativity increases due to increase in effective nuclear charge.

$I V) A l^{3 +} < M g^{2 +} < N a^{+} < F^{-} (order of ionic size)$
Greater the positive charge, greater the effective nuclear charge and hence smaller the radius.

$V) L i^{+} > N a^{+} > K^{+} (order of hydrated size)$
Smaller the size of the cation greater the hydrated size

$V I) N a C l < M g C l_{2} < A l C l_{3} (order of lattice energy)$
greater the charge, greater the lattice energy

Suggest Corrections

Similar questions

Q. Which of the following options are incorrect in accordance with the mentioned properties?

I) | I P_{1} of ion M^{2 +} | > | E A_{1} o f M^{3 +} |

(IP = ionization potential, and EA = electron affinity)

I I) S > S e > T e > O (order of EA)

I I I) L i < B e < B < C (order of electronegativity)

I V) A l^{3 +} < M g^{2 +} < N a^{+} < F^{-} (order of ionic size)

V) L i^{+} > N a^{+} < K^{+} (order of hydrated size)

V I) N a C l > M g C l_{2} > A l C l_{3} (order of lattice energy)

Q. In which of the following arrangements, the order is according to the property indicated against it.

(I) I < B r < F < C l increasing electron gain enthalpy

(I I) L i < N a < K < R b increasing metallic radius

(I I I) B < C < N < O increasing first ionization energy

(I V) A l^{3 +} < M g^{2 +} < N a^{+} < F^{-} increasing ionic size

In which of te following options order of arrangement does not agree with the variation of property indicated against it?
(a) $A l^{3 +} < M g^{2 +} < N a^{+} < F -$ (Increasing ionic size)
(b) B < C < N < O (Increasing first ionlsation enthalpy)
(c) I < Br < Cl< F (increasing electron gain enthalpy)
(d) Li < Na< K < Rb (Increasing metallic radius)

Q. Which of the following species are isoelectronic?

i) N e i i) O^{2 -} i i i) M g^{2 +} i v) F

v) A l^{3 +} v i) C l^{-} v i i) K v i i i) N a

In which of the following option the order of arrangement does not agree with the variation of property indicated against it

a) Li<Na<K<Rb(increasing metallic radius)

b) B<C<N<O(increasing 1st ionisation enthalpy)

c)I<Br<Cl<F(increasing electron gain enthalpy)

d) Al³⁺<Mg²⁺<Na⁺<F^-(increasing ionic size)

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