The first ionization enthalpy of the followin | vedclass

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

Question

(A) The first ionization enthalpy $(\Delta H_{IE})$ generally increases across a period from left to right and decreases down a group.
Comparing the

Vedclass · Accepted Answer

$Si < P < C < N$

Vedclass · Answer

(A) The first ionization enthalpy $(\Delta H_{IE})$ generally increases across a period from left to right and decreases down a group.
Comparing the elements $C$ (Group $14$,Period $2$),$N$ (Group $15$,Period $2$),$Si$ (Group $14$,Period $3$),and $P$ (Group $15$,Period $3$):
$1$. Elements in Period $2$ $(C, N)$ have higher ionization enthalpy than those in Period $3$ $(Si, P)$ due to smaller atomic size.
$2$. Within the same period,Group $15$ elements have higher ionization enthalpy than Group $14$ elements due to the stable half-filled $p$-orbital configuration $(ns^2 np^3)$.
$3$. Combining these trends,the order is $Si < P < C < N$.

The first ionization enthalpy of the following elements are in the order:

Similar Questions

Which of the following has the least ionization potential?

Which of the following is the correct order of the first ionization energy for $B$,$C$,and $N$?

The elements of Group $13$ with highest and lowest first ionisation enthalpies are respectively$:$

Which of the following groups of elements loses an electron most easily?

What factors should be considered to understand the trends in ionization enthalpy values? Explain.

Vedclass Test Series

Exam Paper Generator

Online Exam Module