In which of the following arrangements, the order is according to the property indicated against it.
$(I) I < B r < F < C l increasing electron gain enthalpy$
$(I I) L i < N a < K < R b increasing metallic radius$
$(I I I) B < C < N < O increasing first ionization energy$
$(I V) A l^{3 +} < M g^{2 +} < N a^{+} < F^{-} increasing ionic size$

I, I I and I I I

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I and I I I only

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I, I I and I V

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I and I I only

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Solution

The correct option is C $I, I I and I V$
$(I)$ Electron gain enthalpy of halogen:
$I < B r < F < C l$
Halogens have maximum electron gain enthalpy in the corresponding period and it becomes less negative down the group.
However, the electron gain enthalpy of fluorine is less than that of chlorine. It is due to small size of fluorine, there is a strong electronic repulsion for incoming eletron.
$(I I)$ On going down the group, size of atom increases, metallic radii also increase.
$(I I I)$ On moving left to right in a period, ionisation energy increases but ionisation energy of nitrogen is more than oxygen due to half filled stable configuration. Hence, order of ionization energy is $B < C < O < N$
$(I V)$ Ionic radii order : $Anionic > Neutral > Cationic$
Therefore, increasing order of ionic size for isoelectronic species:
$A l^{3 +} < M g^{2 +} < N a^{+} < F^{-}$

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Similar questions

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)

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)

Arrange the following as per instructions given in the brackets.

(a) Mg. Cl, Na, S, Si (decreasing order of atomic size)

(b) Cs, Na, Li, K, Rb (increasing metallic character)

(d) Cl, F, Br, I (increasing electron affinity)

(e) Cs, Na, Li, K, Rb (decreasing electronegativity)

Q. Match the increasing orders given in column I with the property(ies) given in column II.

Column I	Column II
(A) $N a^{+} < F^{-} < O^{2 -} < N^{3 -}$	(p) electronegativity
(B) $L i^{+}$ < $N a^{+}$ < $K^{+}$ < $R b^{+}$ < $C s^{+}$	(q) Ionisation energy
(C) $O < S < F < C l$	(r) Size
(D) $C l^{-} < K^{+} < C a^{2 +} < S c^{3 +}$	(s) Electron affinity

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In which of the following arrangements, the order is according to the property indicated against it. (I) I<Br<F<Cl increasing electron gain enthalpy (II) Li<Na<K<Rb increasing metallic radius (III) B<C<N<O increasing first ionization energy (IV) Al3+<Mg2+<Na+<F− increasing ionic size