The increasing order of the first ionization | vedclass

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Question

(A) The first ionization enthalpy generally increases across a period from left to right due to an increase in effective nuclear charge. $B$ (Boron,gr

Vedclass · Accepted Answer

$B < S < P < F$

Vedclass · Answer

(A) The first ionization enthalpy generally increases across a period from left to right due to an increase in effective nuclear charge. $B$ (Boron,group $13$) has the lowest ionization enthalpy among the given elements. Comparing $P$ (Phosphorus,group $15$) and $S$ (Sulfur,group $16$),$P$ has a higher ionization enthalpy than $S$ because $P$ has a stable half-filled $p$-orbital configuration $(3s^2 3p^3)$. $F$ (Fluorine,group $17$) has the highest ionization enthalpy due to its small size and high effective nuclear charge. Thus,the order is $B < S < P < F$.

The increasing order of the first ionization enthalpies of the elements $B$,$P$,$S$ and $F$ (lowest first) is:

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