What is the increasing order of the first ion | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(D) The general trend for ionization enthalpy across a period from left to right is that it increases due to an increase in effective nuclear charge.T

Vedclass · Accepted Answer

$B < S < P < F$

Vedclass · Answer

(D) The general trend for ionization enthalpy across a period from left to right is that it increases due to an increase in effective nuclear charge.The elements $B, P, S, F$ belong to the second and third periods.The electronic configurations are: $B (Z=5): 1s^2 2s^2 2p^1$,$P (Z=15): [Ne] 3s^2 3p^3$,$S (Z=16): [Ne] 3s^2 3p^4$,$F (Z=9): 1s^2 2s^2 2p^5$.Phosphorus $(P)$ has a stable half-filled $p$-orbital $(3p^3)$,which makes its ionization enthalpy higher than that of Sulfur $(S)$.Comparing the values: $B$ has the lowest,followed by $S$,then $P$,and $F$ has the highest.Therefore,the increasing order is $B < S < P < F$.

What is the increasing order of the first ionization enthalpy of $B, P, S$ and $F$ (lowest first)?

Similar Questions

The electronic configurations of elements $A, B$ and $C$ are $[He] 2s^1$,$[Ne] 3s^1$ and $[Ar] 4s^1$ respectively. Which one of the following orders is correct for the first ionization potentials (in $kJ \ mol^{-1}$) of $A, B$ and $C$?

The correct order of ionisation energy of $C$,$N$,$O$,and $F$ is

Which of the following statements is incorrect?

The first ionization enthalpies of four consecutive elements present in the second period of the periodic table are $8.3, 11.3, 14.5$ and $13.6 \ eV,$ respectively. Which one of the following is the first ionization enthalpy of nitrogen?

The incorrect statement among the following is:

Vedclass Test Series

Exam Paper Generator

Online Exam Module