Consider the following ionization enthalpies of two elements 'A' and 'B'.
\begin{array}{lcll}
\hline & Element & Ionization & enthalpy (\mathrm{kJ} / \mathrm{mol}) \\
& 1 \mathrm{st} & 2 \mathrm{nd} & 3rd \\
\mathrm{A} & 899 & 1757 & 14847 \\
\mathrm{~B} & 737 & 1450 & 7731 \\
\hline
\end{array}
Which of the following statements is correct?

Question

Aicharya · Accepted Answer

Generally, the ionization enthalpies or energy increases from left to right in a period and decreases from top to bottom in a group. Several factor such as atomic radius, nuclear charge, shielding effect are responsible for change of ionization enthalpies.

Here, Ist ionization enthalpy of $A$ and $B$ is greater than group I $\left(\mathrm{Li}=520 \mathrm{kJmol}^{-1}ight.$ to $\mathrm{Cs}$ $=374 \mathrm{kJmol}^{-1}$ ), which means element $A$ and $B$ belong to group $-2$ and all three given ionization enthalpy values are less for element $B$ means $B$ will come below

Consider the following ionization enthalpies of two elements 'A' and 'B'. \begin{array}{lcll} \hline &…

Solution