Question

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Answer 1

Question:

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

(a) B < C < N < O (increasing first ionization enthalpy)

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

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

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

Answer:

Correct answer is Option (a)

We know that,

Correct order of increasing Electron gain enthalpy

I < Br < Cl < F

(In the Halogens Family Flourine has highest Electron gain enthalpy)

Correct order of increasing metallic radius

Li < Na < K < Rb

(From top to bottom in modern periodic table Metallic radius increases)

Correct order of increasing ionic size

Al³⁺ < Mg²⁺ < Na⁺ < F⁻

(The number of protons in the nucleus increases but the electrons are donated and hence lost.)

(So it pulls the outer electrons more)

Hence Option(b), Option(c), Option(d) have correct arrangement with respect to the property given.

But,

According to the question,

We are asked to find the incorrect arrangement

The Incorrect arrangement is in Option(a)

It is because,

The correct increasing order of first ionization enthalpy

$\rm{\boxed{\boxed{B < C < N > O}}}$

But the given order in question is

B < C < N < O (Hence, it is incorrect)

Additional Information:

Variation of Ionization enthalpy

• In periods from left to right Ionization enthalpy increases.
• It is due to decrease in atomic size and increased nuclear charge.
• In groups from top to bottom Ionization enthalpy decreases.
• It is due to increasing atomic size and increased screening effect.
• Element with lowest Ionization enthalpy is Caesium (Cs)
• Element with highest Ionization potential is Helium (He)

Answer 2

Answer:

A option is the correct answer.

Explanation:

In Nitrogen, due to stability of half filled 2p orbital it requires more energy than oxygen so nitrogen has more ionisation potential than oxygen