Assertion $A$ : The first ionization enthalpy for oxygen is lower than that of nitrogen.
Reason $R$ : The four electrons in $2 p$ orbitals of oxygen experience more electron-electron repulsion.
In the light of the above statements, choose the correct answer from the options given below.
In oxygen atom, $2$ of the $42 p$ electrons must occupy the same $2 p$ orbital resulting in an increased electron electron-repulsion.
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$Xe{F_6}\xrightarrow{{ + {H_2}O}}A\xrightarrow{{ + {H_2}O}}B\xrightarrow{{ + {H_2}O}}C$
$4B(s) + 3O_2\,(g) \rightarrow 2B_2O_3\,(g)$ ; $E^o_{cell} = 1.433$ $volt$ What is molar entropy (in $J/K$) of oxygen gas
Given ${\left( {{\Delta _f}{H^o}} \right)_{{B_2}{O_3}}}\left( g \right) = - 840\,\frac{{KJ}}{{mol}}$
${\left( {S_m^o} \right)_{{B_2}{O_3}}} \left( g \right) = 280J/K - mol$
${{(S_{m}^{o})}_{B}}\,\,\left( s \right)=10\,J/K-mol$