Question

The correct order of first ionization enthalpy values of the following elements is :
(A) O (B) N (C) Be (D) F (E) B
Choose the correct answer from the options given below :

• A. B < D < C < E < A
• B. E < C < A < B < D
• C. C < E < A < B < D
• D. A < B < D < C < E

Answer 1

Answer: (B)

E < C < A < B < D

Answer 2

The correct order of first ionization enthalpies among the given elements can be deduced based on periodic trends. In general, ionization enthalpy increases across a period from left to right due to increasing nuclear charge and decreases down a group due to an increase in atomic size. Additionally, elements with stable electronic configurations, such as half-filled or fully-filled orbitals, tend to have higher ionization enthalpies.

The general trend for ionization enthalpy in the periodic table is:

$\text{Li} < \text{B} < \text{Be} < \text{C} < \text{O} < \text{N} < \text{F} < \text{Ne}$

Among the given elements:

$\text{E (B)} < \text{C (Be)} < \text{A (O)} < \text{B (N)} < \text{D (F)}$

Hence, the correct order of first ionization enthalpy values is:

$\text{E (B)} < \text{C (Be)} < \text{A (O)} < \text{B (N)} < \text{D (F)}$